Silberberg 4/e Chapter 3 Preview

 Silber4 3.001a.EOCP. The atomic mass of Cl is 35.45 amu. What is the mass in grams of 3 mol of Cl atoms? (_) 106.35 g Cl (o) 106.4 g Cl (_) 1.81 1024 g Cl (_) 1.807 1024 g Cl

 Silber4 3.001b.EOCP. The atomic mass of Al is 26.98 amu. What is the mass in grams of 2 mol of Al atoms? (_) 54.0 g Al (o) 53.96 g Al (_) 1.204 1024 g Al (_) 1.20 1024 g Al

 Silber4 3.002a.EOCP. How many moles of C atoms are in 1 mol of sucrose (C12H22O11)? (_) 7.226 1024 mol C (o) 12 mol C (_) 6.022 1023 mol C (_) 1 mol C

 Silber4 3.002b.EOCP. How many C atoms are in 1 mol of sucrose (C12H22O11)? (_) 12 C atoms (o) 7.228 1024 C atoms (_) 6.022 1023 C atoms (_) 1 C atom

Silber4 3.003.AP. ,
Why might the expression "1 mole of nitrogen" be confusing?
 Key: "1 mole of nitrogen" could be interpreted as a mole of nitrogen atoms or a mole of nitrogen molecules.

What change would remove any uncertainty?
 Key: Specify a mole of nitrogen atoms or a mole of nitrogen molecules to avoid confusion.

For what other elements might a similar confusion exist? (Select all that apply.)

Why?
 Key: The same problem is possible with other diatomic or polyatomic molecules, e.g., Cl2, Br2, S8, P4.

 Silber4 3.003.EOCP. "One mole of nitrogen" can be interpreted as one mole of nitrogen atoms or one mole of nitrogen molecules. (o) true (_) false

 Silber4 3.004.EOCP. Which is true for molecular mass and/or molar mass? (_) Both represent the SI unit for the amount of a substance. (o) Both will have the same numeric value for a given chemical substance. (_) Molar mass will have units in amu. (_) Molecular mass will have units in g/mol.

 Silber4 3.005.EOCP. Which is not true about the mole? (_) It maintains the same mass relationship between macroscopic samples as exist between individual chemical entities. (o) It represents a mass unit. (_) It relates the number of chemical entities to the mass. (_) It is the amount of a substance that contains the same number of entities as there are atoms in exactly 12 g of carbon-12.

 Silber4 3.007.AP. Each of the following balances weighs the indicated numbers of atoms of two elements. Each part (a), (b), etc below refers to the corresponding balance. (a) Which element has the lower molar mass? (_) left (o) right (_) neither (b) Which element has fewer atoms per gram? (_) left (o) right (_) neither (c) Which element has fewer atoms per gram? (o) left (_) right (_) neither (d) Which element has more atoms per mole? (_) left (_) right (o) neither

 Silber4 3.007a.EOCP. Each of the balances below weighs the indicated numbers of atoms of two elements. On Scale (a) which element has the higher molar mass? (_) the element on the right (o) the element on the left (_) neither element (_) not enough information to decide

 Silber4 3.007b.EOCP. Each of the balances below weighs the indicated numbers of atoms of two elements. On Scale (b) which element has more atoms per gram? (_) the element on the right (o) the element on the left (_) neither element (_) not enough information to decide

 Silber4 3.007c.EOCP. Each of the balances below weighs the indicated numbers of atoms of two elements. On Scale (c) which element has fewer atoms per gram? (_) the element on the right (o) the element on the left (_) neither element (_) not enough information to decide

 Silber4 3.007d.EOCP. Each of the balances below weighs the indicated numbers of atoms of two elements. On Scale (d) which element has fewer atoms per gram? (_) the element on the left (o) neither element (_) the element on the right (_) not enough information to decide

 Silber4 3.008.AP. Calculate the molar mass of each of the following. (a) SO2 [64.1] g/mol (b) N2O [44] g/mol (c) K2S [110] g/mol (d) C6H12O6 [180] g/mol

 Silber4 3.008a.EOCP. Calculate the molar mass of the compound: Sr(OH)2 (_) 121.636 g/mol (o) 121.64 g/mol (_) 105.636 g/mol (_) 105.64 g/mol

 Silber4 3.008b.EOCP. Calculate the molar mass of the compound: N2O (_) 44 g/mol (_) 44.0 g/mol (o) 44.02 g/mol (_) 44.1 g/mol

 Silber4 3.008c.EOCP. Calculate the molar mass of the compound: NaClO3 (_) 177.34 g/mol (_) 177 g/mol (o) 106.44 g/mol (_) 106 g/mol

 Silber4 3.008d.EOCP. Calculate the molar mass of the compound: Cr2O3 (_) 152 g/mol (_) 100 g/mol (o) 152.00 g/mol (_) 100.0 g/mol

 Silber4 3.009.AP. Calculate the molar mass of the following substances. (a) K2C4H4O5 [210] g/mol(b) P4O6 [220] g/mol(c) CuSO4 · 5 H2O [250] g/mol(d) Na2HPO4 [142] g/mol

 Silber4 3.009a.EOCP. Calculate the molar mass of the compound: (NH4)3PO4 (_) 149.100 g/mol (_) 121.08 g/mol (o) 149.10 g/mol (_) 121.1 g/mol

 Silber4 3.009b.EOCP. Calculate the molar mass of the compound: CH2Cl2 (_) 84.9 g/mol (_) 96.94 g/mol (o) 84.93 g/mol (_) 96.9 g/mol

 Silber4 3.009c.EOCP. Calculate the molar mass of the compound: CuSO4 · 5 H2 (_) 249.720 g/mol (_) 185.7 g/mol (o) 249.70 g/mol (_) 185.70 g/mol

 Silber4 3.009d.EOCP. Calculate the molar mass of the compound: BrF5 (_) 174.900 g/mol (_) 174.9 g/mol (o) 174.90 g/mol (_) 175 g/mol

 Silber4 3.010a.EOCP. Calculate the molar mass of the compound: SnO2 (_) 150 g/mol (_) 151 g/mol (o) 150.7 g/mol (_) 150.70 g/mol

 Silber4 3.010b.EOCP. Calculate the molar mass of the compound: BaF2 (_) 180 g/mol (_) 175 g/mol (o) 175.3 g/mol (_) 175.30 g/mol

 Silber4 3.010c.EOCP. Calculate the molar mass of the compound: Al2(SO4)3 (_) 278 g/mol (_) 278.03 g/mol (o) 342.17 g/mol (_) 342 g/mol

 Silber4 3.010d.EOCP. Calculate the molar mass of the compound: MnCl2 (_) 126 g/mol (_) 125.8 g/mol (o) 125.84 g/mol (_) 125.840 g/mol

 Silber4 3.011.AP. Calculate the molar mass of each of the following. (a) SrH2 [89.6] g/mol(b) Fe(ClO4)3 [354] g/mol(c) C7H8 [106] g/mol(d) CuCl2 · 2 H2O [170] g/mol

 Silber4 3.011a.EOCP. Calculate the molar mass of the compound: N2O4 (_) 92.020 g/mol (_) 92 g/mol (_) 92.0 g/mol (o) 92.02 g/mol

 Silber4 3.011b.EOCP. Calculate the molar mass of the compound: C8H10 (_) 106 g/mol (_) 106.2 g/mol (_) 106.160 g/mol (o) 106.16 g/mol

 Silber4 3.011c.EOCP. Calculate the molar mass of the compound: MgSO4 · 7 H2O (_) 150.49 g/mol (_) 150.492 g/mol (_) 246.492 g/mol (o) 246.49 g/mol

 Silber4 3.011d.EOCP. Calculate the molar mass of the compound: Ca(C2H3O2)2 (_) 131.12 g/mol (_) 131.124 g/mol (_) 158.168 g/mol (o) 158.17 g/mol

 Silber4 3.012.AP. Calculate each of the following quantities. (a) mass in grams of 0.67 mol KMnO4 [110] g(b) moles of O atoms in 7.56 g Mg(NO3)2 [0.306] mol(c) number of O atoms in 6.0 10-3 g CuSO4 · 5 H2O [1.3e+20] atoms

 Silber4 3.012a.EOCP. Calculate the mass in grams of 0.57 mol of KMnO4. (_) 2.77 102 g KMnO4 (_) 2.8 102 g KMnO4 (o) 9.0 101 g KMnO4 (_) 9.01 101 g KMnO4

 Silber4 3.012b.EOCP. Calculate the moles of O atoms in 8.18 g of Mg(NO3)2. (_) 0.110 mol O atoms (_) 0.16 mol O atoms (o) 0.331 mol O atoms (_) 0.0551 mol O atoms

 Silber4 3.012c.EOCP. Calculate the number of O atoms in 8.1 10-3 g of CuSO4 · 5 H2O. (_) 2.9 10-4 O atoms (_) 1.95 1019 O atoms (o) 1.8 1020 O atoms (_) 3.24 10-5 O atoms

 Silber4 3.013.AP. Calculate each of the following quantities. (a) mass in kilograms of 3.4 1020 molecules of NO2 [2.6e-05] kg (b) moles of Cl atoms in 0.0535 g C2H4Cl2 [0.00108] mol (c) number of H - ions in 5.39 g SrH2 [7.24e+22] ions

 Silber4 3.013a.EOCP. Calculate the mass in kilograms of 3.8 1020 molecules of NO2. (_) 2.90 10–2 kg NO2 (_) 1.7 1019 kg NO2 (_) 1.75 1022 kg NO2 (o) 2.9 10–5 kg NO2

 Silber4 3.013b.EOCP. Calculate the moles of Cl atoms in 0.0425 g of C2H4Cl2. (_) 4.2951 10-4 mol Cl atoms (_) 2.10 mol Cl atoms (_) 8.5 10-2 mol Cl atoms (o) 8.59 10-4 mol Cl atoms

 Silber4 3.013c.EOCP. Calculate the number of H- ions in 4.92 g of SrH2. (_) 1.098 10-1 H- ions (_) 3.30 1022 H- ions (_) 5.5 10-2 H- ions (o) 6.61 1022 H- ions

 Silber4 3.014.AP. Calculate each of the following quantities. (a) mass in grams of 0.55 mol MnSO4 [83] g (b) moles of compound in 13.4 g Fe(ClO4)3 [0.0378] mol (c) number of N atoms in 80.5 g NH4NO2 [1.52e+24] atoms

 Silber4 3.014a.EOCP. Calculate the mass in grams of 0.64 mol of MnSO4. (_) 96.6 g MnSO4 (o) 97 g MnSO4 (_) 4.24 10-3 g MnSO4 (_) 4.2 10-3 g MnSO4

 Silber4 3.014b.EOCP. Calculate the moles of compound in 15.8 g of Fe(ClO4)3. (_) 5.6 10-2 mol Fe(ClO4)3 (o) 4.46 10-2 mol Fe(ClO4)3 (_) 1.338 10-1 mol Fe(ClO4)3 (_) 3.36 1022 mol Fe(ClO4)3

 Silber4 3.014c.EOCP. Calculate the number of N atoms in 92.6 g of NH4NO2. (_) 1.446 N atoms (o) 1.74 1024 N atoms (_) 8.7 1023 N atoms (_) 2.89 N atoms

 Silber4 3.015.AP. Calculate each of the following quantities. (a) total number of ions in 28.7 g CaF2 [6.64e+23] ions (b) mass in milligrams of 2.18 mol CuCl2 · 2 H2O [3.72e+05] mg (c) mass in kilograms of 3.44 1022 formula units of Bi(NO3)3 · 5 H2O [0.0277] kg

 Silber4 3.015a.EOCP. Calculate the total number of ions in 38.1 g of CaF2. (o) 8.82 1023 ions (_) 0.976 ions (_) 5.9 1023 ions (_) 6.88 1025 ions

 Silber4 3.015b.EOCP. Calculate the mass in milligrams of 3.58 mol of CuCl2 · 2 H2O. (o) 6.10 105 mg CuCl2 · 2 H2O (_) 5.5304 105 mg CuCl2 · 2 H2O (_) 5.5 104 mg CuCl2 · 2 H2O (_) 6.1 102 mg CuCl2· 2 H2O

 Silber4 3.015c.EOCP. Calculate the mass in kilograms of 2.88 1022 formula units of Bi(NO3)3 · 5 H2O. (o) 2.32 10-2 kg Bi(NO3)3 · 5 H2O (_) 1.4 1022 kg Bi(NO3)3 · 5 H2O (_) 1.880 10-2 kg Bi(NO3)3 · 5 H2 O (_) 1.12 1022 kg Bi(NO3)3 · 5 H2O

 Silber4 3.016a.EOCP. Calculate the mass in grams of 8.41 mol of copper(I) carbonate. (o) 1.57 103 g Cu2CO3 (_) 1.04 103 g CuCO3 (_) 9.0 102 g CuCO2 (_) 1.439 103 g Cu2CO2

 Silber4 3.016b.EOCP. Calculate the mass in grams of 2.04 1021 molecules of dinitrogen pentaoxide. (o) 0.366 g N2O5 (_) 0.64 g (NO5)2 (_) 2 1023 g N2O5 (_) 3.836 1023 g (NO5)2

 Silber4 3.016c.EOCP. Calculate the number of moles in 57.9 g of sodium perchlorate. (o) 0.473 mol NaClO4 (_) 0.54 mol NaClO3 (_) 0.6 mol NaClO2 (_) 0.778 mol NaClO

 Silber4 3.016d.EOCP. Calculate the number of formula units in 57.9 g of sodium perchlorate. (o) 2.85 1023 formula units NaClO4 (_) 3.3 1023 formula units NaClO3 (_) 4 1023 formula units NaClO2 (_) 4.685 1023 formula units NaClO

 Silber4 3.016f.EOCP. Calculate the number of perchlorate ions in 57.9 g of sodium perchlorate. (o) 2.85 1023 ClO4- (_) 3.3 1023 ClO3- (_) 4 1023 ClO2- (_) 4.685 1023 ClO-

 Silber4 3.016g.EOCP. Calculate the number of Cl atoms in 57.9 g of sodium perchlorate. (o) 2.85 1023 Cl atoms (_) 3.3 1023 Cl atoms (_) 4 1023 Cl atoms (_) 4.685 1023 Cl atoms

 Silber4 3.016h.EOCP. Calculate the number of O atoms in 57.9 g of sodium perchlorate. (o) 1.14 1024 O atoms (_) 9.8 1023 O atoms (_) 7 1023 O atoms (_) 4.685 1023 O atoms

 Silber4 3.017.AP. Calculate each of the following quantities. (a) mass in grams of 2.05 mol chromium(III) sulfate decahydrate [1170] g (b) mass in grams of 9.46 1024 molecules of dichlorine heptaoxide [2870] g (c) number of moles and formula units in 59.2 g lithium sulfate moles [0.539] molformula units [3.24e+23] formula units (d) number of lithium ions, sulfate ions, S atoms, and O atoms in the mass in part (c)Li+ ions [6.49e+23] ionsSO42- ions [3.24e+23] ionsS atoms [3.24e+23] atomsO atoms [1.30e+24] atoms

 Silber4 3.017a.EOCP. Calculate the mass in grams of 3.52 mol of chromium(III) sulfate decahydrate. (_) 1.5 103 g Cr2(SO4)3 · 10 H2O (_) 1.32 103 g Cr3(SO4)2 · 10 H2O (_) 1.860 103 g Cr3(SO4)2 · 10 H2O (o) 2.02 103 g Cr2(SO4)3 · 10 H2O

 Silber4 3.017b.EOCP. Calculate the mass in grams of 9.64 1024 molecules of dichlorine heptaoxide. (_) 2.7 103 g Cl2O6 (_) 5.78 1022 g Cl2O6 (_) 5 1022 g Cl2O7 (o) 2.93 103 g Cl2O7

 Silber4 3.017c.EOCP. Calculate the number of moles in 56.2 g of lithium sulfate. (_) 0.6 mol Li2SO3 (_) 0.65 mol LiSO3 (_) 0.54 mol LiSO4 (o) 0.511 mol Li2SO4

 Silber4 3.017d.EOCP. Calculate the number of formula units in 56.2 g of lithium sulfate. (_) 4 1023 formula units Li2SO3 (_) 3.9 1023 formula units LiSO3 (_) 3.25 1023 formula units LiSO4 (o) 3.08 1023 formula units Li2SO4

 Silber4 3.017e.EOCP. Calculate the number of lithium ions in 56.2 g of lithium sulfate. (_) 7.2 1023 Li+ (_) 4 1023 Li+ (_) 3.25 1023 Li+ (o) 6.15 1023 Li+

 Silber4 3.017f.EOCP. Calculate the number of sulfate ions in 56.2 g of lithium sulfate. (_) 3.25 1023 SO42- (_) 3.6 1023 SO32- (_) 3.91 1023 SO32- (o) 3.08 1023 SO42-

 Silber4 3.017g.EOCP. Calculate the number of S atoms in 56.2 g of lithium sulfate. (_) 3.6 1023 S atoms (_) 3.91 1023 S atoms (_) 3.25 1023 S atoms (o) 3.08 1023 S atoms

 Silber4 3.017h.EOCP. Calculate the number of O atoms in 56.2 g of lithium sulfate. (_) 1.1 1024 O atoms (_) 1.174 1024 O atoms (_) 1.3 1024 O atoms (o) 1.23 1024 O atoms

 Silber4 3.018.AP. Calculate each of the following. (a) mass % of N in ammonium bicarbonate [17.7]% (b) mass % of H in sodium dihydrogen phosphate heptahydrate [6.55]%

 Silber4 3.018a.EOCP. Calculate the mass % of H in ammonium bicarbonate. (_) 6.50 mass % H (o) 6.375 mass % H (_) 10.710 mass % H (_) 5.2 mass % H

 Silber4 3.018b.EOCP. Calculate the mass % of O in sodium dihydrogen phosphate heptahydrate. (_) 70.15 mass % O (o) 71.52 mass % O (_) 69.8 mass % O (_) 57.895 mass % O

 Silber4 3.019a.EOCP. Calculate the mass % of I in strontium periodate. (_) 74.34 mass % I (o) 54.07 mass % I (_) 45.6 mass % I (_) 34.659 mass % I

 Silber4 3.019b.EOCP. Calculate the mass % of Mn in potassium permanganate. (_) 27.9 mass % Mn (o) 34.76 mass % Mn (_) 38.679 mass % Mn (_) 30 mass % Mn

 Silber4 3.020a.EOCP. Calculate the mass fraction of C in cesium acetate. (_) 0.07 mass fraction C (o) 0.1251 mass fraction C (_) 0.0742 mass fraction C (_) 0.13 mass fraction C

 Silber4 3.020b.EOCP. Calculate the mass fraction of O in uranyl sulfate trihydrate (the formula for the uranyl ion is UO22+). (_) 0.2601 mass fraction O (o) 0.3428 mass fraction O (_) 0.32 mass fraction O (_) 0.226 mass fraction O

 Silber4 3.021.AP. Calculate each of the following. (a) mass fraction of O in calcium perchlorate [0.464](b) mass fraction of P in tetraphosphorus hexaoxide [0.563]

 Silber4 3.021a.EOCP. Calculate the mass fraction of Cl in calcium chlorate. (_) 0.240 mass fraction Cl (_) 0.29 mass fraction Cl (_) 0.3297 mass fraction Cl (o) 0.3425 mass fraction Cl

 Silber4 3.021b.EOCP. Calculate the mass fraction of P in tetraphosphorus hexaoxide. (_) 0.453 mass fraction P (_) 0.52 mass fraction P (_) 0.4918 mass fraction P (o) 0.5634 mass fraction P

 Silber4 3.022.AP. , Oxygen is required for metabolic combustion of foods. Calculate the number of atoms in 38.0 g oxygen gas, the amount absorbed from the lungs at rest in about 15 minutes. [1.43e+24] atoms

 Silber4 3.022.EOCP. Oxygen is required for the metabolic combustion of foods. Calculate the number of atoms in 38.0 g of oxygen gas, the amount absorbed from the lungs at rest in about 15 minutes. (_) 2.86 1024 O atoms (_) 2.288 1025 O atoms (_) 7.2 1023 O atoms (o) 1.43 1024 O atoms

 Silber4 3.023.AP. Cisplatin (below) is a powerful drug used in the treatment of certain cancers.(a) Calculate the moles of compound in 275.1 g cisplatin. [0.9167] mol(b) Calculate the number of hydrogen atoms in 0.96 mol cisplatin. [3.5e+24] atoms

 Silber4 3.023a.EOCP. Cisplatin (below), or Platinol, is a powerful drug used in the treatment of certain cancers. Calculate the moles of compound in 285.3 g of cisplatin. (_) 0.95 mol Pt(NH3)2Cl2 (_) 0.95068 mol Pt(NH3)2Cl2 (_) 0.951 mol Pt(NH3)2Cl2 (o) 0.9507 mol Pt(NH3)2Cl2

 Silber4 3.023b.EOCP. Cisplatin (below), or Platinol, is a powerful drug used in the treatment of certain cancers. Calculate the number of hydrogen atoms in 0.98 mol of cisplatin. (_) 3.54 1024 H atoms (_) 3.541 1024 H atoms (_) 4 1024 H atoms (o) 3.5 1024 H atoms

 Silber4 3.024.AP. Allyl sulfide gives garlic its characteristic odor. (a) Calculate the mass in grams of 1.63 mol allyl sulfide. [186] g (b) Calculate the number of carbon atoms in 4.67 g allyl sulfide. [1.48e+23] atoms

 Silber4 3.024a.EOCP. Allyl sulfide (below) gives garlic its characteristic odor. Calculate the mass in grams of 1.63 mol of allyl sulfide. (_) 1.427 10-2 g S(C3H5)2 (_) 1.43 10-2 g S(C3H5)2 (_) 186.2 g S(C3H5)2 (o) 186 g S(C3H5)2

 Silber4 3.025.AP. Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3 · 4 H2O). (a) For 62.6 kg rust, calculate the moles of compound. [2.70e+02] mol(b) Find the moles of Fe2O3. [2.70e+02] mol(c) Determine the grams of iron. [30200] g

 Silber4 3.025a.EOCP. Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3 · 4 H2O). Calculate the moles of Fe2O3 · 4 H2O in 65.2 kg of rust. (_) 2.81 mol Fe2O3 · 4 H2O (_) 28.1 mol Fe2O3 · 4 H2O (_) 0.281 mol Fe2O3 · 4 H2O (o) 281 mol Fe2O3 · 4 H2O

 Silber4 3.025b.EOCP. Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3 · 4 H2O). Calculate the moles of Fe2O3 in 65.2 kg of rust. (_) 70.25 mol Fe2O3 (_) 7.02 mol Fe2O3 (_) 28.1 mol Fe2O3 (o) 281 mol Fe2O3

 Silber4 3.025c.EOCP. Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3 · 4 H2O). Calculate the grams of iron in 65.2 kg of rust. (_) 2.81 102 g Fe (_) 15.71 g Fe (_) 31.42 g Fe (o) 3.14 104 g Fe

 Silber4 3.026.AP. Propane (C3H8) is widely used in liquid form as a fuel for barbecue grills and camp stoves. For 67.7 g of propane, determine the following. (a) Calculate the moles for of compound. [1.54] mol (b) Calculate the grams of carbon. [55.3] g

 Silber4 3.026a.EOCP. Propane is widely used in liquid form as a fuel for barbecue grills and camp stoves. Calculate the moles of compound in 75.3 g of propane. (_) 2.264 103 mol C2H6 (_) 3.32 103 mol C3H8 (o) 1.71 mol C3H8 (_) 2.504 mol C2H6

 Silber4 3.026b.EOCP. Propane is widely used in liquid form as a fuel for barbecue grills and camp stoves. Calculate the grams of carbon in 75.3 g of propane. (_) 20.54 g C (_) 74.00 g C (o) 61.5 g C (_) 30.1 g C

 Silber4 3.027.EOCP. The effectiveness of a nitrogen fertilizer is determined mainly by its mass % N. Which of the following fertilizers is most effective? (_) potassium nitrate (_) ammonium nitrate (o) urea, CO(NH2)2 (_) ammonium sulfate

 Silber4 3.028a.EOCP. The mineral galena is composed of lead(II) sulfide and has an average density of 7.46 g/cm3. How many moles of lead(II) sulfide are in 1.00 ft3 of galena? (_) 0.950 mol (_) 1.12 10-3 mol (o) 883 mol (_) 15.9 mol

 Silber4 3.028b.EOCP. The mineral galena is composed of lead(II) sulfide and has an average density of 7.46 g/cm3. How many lead atoms are in 1.00 dm3 of galena? (_) 1.88 1018 atoms (_) 1.88 1023 atoms (o) 1.88 1025 atoms (_) 5.18 1023 atoms

 Silber4 3.029.AP. , Hemoglobin, a protein found in red blood cells, carries O2 from the lungs to the body's cells. Iron (as ferrous ion, Fe2+) makes up 0.33 mass % of hemoglobin. If the molar mass of hemoglobin is 6.8 104 g/mol, how many Fe2+ ions are present in one molecule? [4]

 Silber4 3.029.EOCP. Hemoglobin, a protein found in red blood cells, carries O2 from the lungs to the body's cells. Iron (as ferrous ion, Fe2+) makes up 0.33 mass % of hemoglobin. If the molar mass of hemoglobin is 6.8 104 g/mol, how many Fe2+ ions are present in one molecule? (_) 224 Fe2+ ions/molecule hemoglobin (_) 120 Fe2+ ions/molecule hemoglobin (o) 4 Fe2+ ions/molecule hemoglobin (_) 1218 Fe2+ ions/molecule hemoglobin

 Silber4 3.030.AP. , Select three ways compositional data may be given in a problem that involves finding an empirical formula. [x] elemental composition [x] combustion analysis [x] mass % of electrons [_] reaction states

 Silber4 3.030.EOCP. Which is not a way in which compositional data may be given in a problem to find an empirical formula? (_) Determine the empirical formula from mass % of elements. (_) Determine the empirical formula from elemental analysis. (o) Determine the empirical formula from the number of elements in a compound. (_) Determine the empirical formula from combustion analysis.

 Silber4 3.031.EOCP. Which of the following sets of information does not allow you to obtain the molecular formula of a covalent compound? (_) mass % of each element and the total number of atoms in a molecule of the compound (_) mass % of each element and the number of atoms of one element in a molecule of the compound (o) number of moles of each type of atom in a given sample of the compound (_) structural formula of the compound

 Silber4 3.032.EOCP. MgCl2 is a molecular formula for magnesium chloride. (_) True (o) False

 Silber4 3.033a.EOCP. Give the empirical formula for the compound below. C2H4 (_) C2H4 (_) CH (o) CH2 (_) C2H2

 Silber4 3.033b.EOCP. Give the empirical formula for the compound below. C2H6O2 (_) CHO (_) C2H2O2 (o) CH3O (_) C2H6O2

 Silber4 3.033c.EOCP. Give the empirical formula for the compound below. N2O5 (_) NO2 (_) N2O3 (o) N2O5 (_) NO

 Silber4 3.033d.EOCP. Give the empirical formula for the compound below. Ba3(PO4)2 (_) BaPO (_) Ba2P2O3 (o) Ba3(PO4)2 (_) Ba(PO)2

 Silber4 3.033e.EOCP. Give the empirical formula for the compound below. Te4I16 (_) Te4I8 (_) Te2I8 (o) TeI4 (_) TeI

Silber4 3.034.AP.
What is the empirical formula and empirical formula mass for each of the following compounds? (Type your answer using the format CH4 for CH4.)
 empirical formula empirical formula mass (a) P4O10 [P2O5] [141.96] g/mol (b) C4H8 [CH2] [14.03] g/mol (c) C3H6O3 [CH2O] [30.03] g/mol (d) S4N4 [SN] [46.08] g/mol

 Silber4 3.034a.EOCP. Give the empirical formula for the compound below. C4H8 (_) CH (_) C2H4 (o) CH2 (_) C4H8

 Silber4 3.034b.EOCP. Give the empirical formula for the compound below. C3H6O3 (_) C2H3O2 (_) C3H6O3 (o) CH2O (_) CHO

 Silber4 3.034c.EOCP. Give the empirical formula for the compound below. P4O10 (_) PO (_) P4O10 (o) P2O5 (_) PO5

 Silber4 3.034d.EOCP. Give the empirical formula for the compound below. Ga2(SO4)3 (_) Ga2(SO4)2 (_) GaSO2 (o) Ga2(SO4)3 (_) GaSO

 Silber4 3.034e.EOCP. Give the empirical formula for the compound below. Al2Br6 (_) AlBr (_) Al2Br3 (_) Al2Br6 (o) AlBr3

 Silber4 3.035.AP. , What is the molecular formula of each compound? (Type your answer using the format CO2 for CO2.)(a) CH2 ( = 42.08 g/mol) [C3H6] (b) NH2 ( = 32.05 g/mol) [N2H4] (c) NO2 ( = 92.02 g/mol) [N2O4] (d) CHN ( = 135.14 g/mol) [C5H5N5]

 Silber4 3.035a.EOCP. Give the molecular formula for the compound below. empirical formula CH2 (molar mass = 42.08 g/mol) (_) CH2 (_) C2H4 (_) CH (o) C3H6

 Silber4 3.035b.EOCP. Give the molecular formula for the compound below. empirical formula NH2 (molar mass = 32.05 g/mol) (_) NH (_) NH2 (_) N4H8 (o) N2H4

 Silber4 3.035c.EOCP. Give the molecular formula for the compound below. empirical formula NO2 (molar mass = 92.02 g/mol) (_) NO2 (_) NO (_) N3O6 (o) N2O4

 Silber4 3.035d.EOCP. Give the molecular formula for the compound below. empirical formula CHN (molar mass = 135.14 g/mol) (_) CHN (_) C3H3N3 (_) C2H2N2 (o) C5H5N5

 Silber4 3.036.AP. What is the molecular formula of each compound? (Type your answer using the format C6H12O6 for C6H12O6.) (a) empirical formula CHCl ( = 84.93 g/mol) [CH2Cl2] (b) empirical formula CH2Cl ( = 98.95 g/mol) [C2H4Cl2] (c) empirical formula CH ( = 78.11 g/mol) [C6H6] (d) empirical formula C3H6O2 ( = 74.08 g/mol) [C3H6O2]

 Silber4 3.036a.EOCP. Give the molecular formula for the compound below. empirical formula CH (molar mass = 78.11 g/mol) (_) C2H2 (o) C6H6 (_) CH4 (_) CH

 Silber4 3.036b.EOCP. Give the molecular formula for the compound below. empirical formula C3H6O2 (molar mass = 74.08 g/mol) (_) CH3O (o) C3H6O2 (_) CHO (_) C6H12O4

 Silber4 3.036c.EOCP. Give the molecular formula for the compound below. empirical formula HgCl (molar mass = 472.1 g/mol) (_) Hg3Cl3 (o) Hg2Cl2 (_) Hg4Cl4 (_) HgCl

 Silber4 3.036d.EOCP. Give the molecular formula for the compound below. empirical formula C7H4O2 (molar mass = 240.20 g/mol) (_) C7H4O2 (o) C14H8O4 (_) CHO (_) C3H2

 Silber4 3.037.AP. Determine the empirical formula of each of the following compounds. (Type your answer using the format CH4 for CH4.) (a) 0.088 mol chlorine atoms combined with 0.22 mol oxygen atoms [Cl2O5] (b) 3.37 g silicon combined with 12.4 g chlorine [SiCl3] (c) 27.3 mass % carbon and 72.7 mass % oxygen [CO2]

 Silber4 3.037a.EOCP. Give the empirical formula for the compound formed by: 0.063 mol of chlorine atoms combined with 0.22 mol of oxygen atoms (_) Cl2O5 (_) ClO (_) ClO2 (o) Cl2O7

 Silber4 3.037b.EOCP. Give the empirical formula for the compound formed by: 2.45 g of silicon combined with 12.4 g of chlorine (_) Si2Cl8 (_) Si4Cl (_) SiCl (o) SiCl4

 Silber4 3.037c.EOCP. Give the empirical formula for the compound formed by: 27.3 mass % carbon and 72.7 mass % oxygen (_) CO (_) C2O4 (_) C2O (o) CO2

 Silber4 3.038.AP. Determine the empirical formula of each of the following compounds. (Type your answer using the format CH4 for CH4.) (a) 0.039 mol iron atoms combined with 0.052 mol oxygen atoms [Fe3O4](b) 0.903 g phosphorus combined with 6.99 g of bromine [PBr3](c) a hydrocarbon with 79.9 mass % carbon [CH3]

 Silber4 3.038a.EOCP. Give the empirical formula for the compound formed by: 0.039 mol of iron atoms combined with 0.052 mol of oxygen atoms (_) Fe2O2 (_) Fe4O3 (_) FeO (o) Fe3O4

 Silber4 3.038b.EOCP. Give the empirical formula for the compound formed by: 0.903 g of phosphorus combined with 6.99 g of bromine (_) P2Br6 (_) P3Br (_) PBr (o) PBr3

 Silber4 3.038b.EOCP. Give the empirical formula for the compound formed: A hydrocarbon with 79.9 mass % carbon (_) C2H6 (_) CH (_) CH4 (o) CH3

 Silber4 3.039a.EOCP. An oxide of nitrogen contains 30.45 mass % N. What is the empirical formula of the oxide? (_) N2O4 (_) NO (_) NO3 (o) NO2

 Silber4 3.039b.EOCP. An oxide of nitrogen contains 30.45 mass % N. If the molar mass is 90 5 g/mol, what is the molecular formula? (_) NO2 (_) NO (_) NO3 (o) N2O4

 Silber4 3.040.AP. , A chloride of silicon contains 79.1 mass % Cl. (Type your answer using the format CO2 for CO2.) (a) What is the empirical formula of the chloride? [SiCl3] (b) If the molar mass is 269 g/mol, what is the molecular formula? [Si2Cl6]

 Silber4 3.040a.EOCP. A chloride of silicon contains 79.1 mass % Cl. What is the empirical formula of the chloride? (_) Si2Cl4 (_) Si2Cl6 (_) SiCl (o) SiCl3

 Silber4 3.040b.EOCP. A chloride of silicon contains 79.1 mass % Cl. If the molar mass is 269 g/mol, what is the molecular formula? (_) SiCl3 (_) SiCl (_) Si2Cl4 (o) Si2Cl6

 Silber4 3.041a.EOCP. A sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g of MF2. How many moles of F are in the sample of MF2 that forms? (_) 2.0 mol F (_) 0.600 mol F (_) 1.0 mol F (o) 1.20 mol F

 Silber4 3.041b.EOCP. A sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g of MF2. How many grams of M are in this sample of MF2 (_) 23 g M (_) 8.80 g M (_) 27.80 g M (o) 24.0 g M

 Silber4 3.041c.EOCP. A sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g of MF2. What element is represented by the symbol M? (_) vanadium (_) sodium (_) titanium (o) calcium

 Silber4 3.042.AP. , A sample of 0.370 mol of a metal oxide (M2O3) weighs 55.4 g. (a) How many moles of O are in the sample? [1.11] mol (b) How many grams of M are in the sample? [37.6] g (c) What element is represented by the symbol M? [vanadium -or- V]

 Silber4 3.042a.EOCP. A sample of 0.370 mol of a metal oxide (M2O3) weighs 55.4 g How many moles of O are in the sample? (_) 3.0 mol O (o) 1.11 mol O (_) 0.370 mol O (_) 1.0 mol O

 Silber4 3.042b.EOCP. A sample of 0.370 mol of a metal oxide (M2O3) weighs 55.4 g How many grams of M are in the sample? (_) 7.4 g M (o) 37.6 g M (_) 39 g M (_) 17.80 g M

 Silber4 3.042c.EOCP. A sample of 0.370 mol of a metal oxide (M2O3) weighs 55.4 g What element is represented by the symbol M? (_) sodium (o) vanadium (_) titanium (_) calcium

 Silber4 3.043.AP. , Nicotine is a poisonous, addictive compound found in tobacco. A sample of nicotine contains 6.16 mmol C, 8.56 mmol H, and 1.23 mmol N [1 mmol (one millimole) = 10-3 mol]. What is the empirical formula? (Type your answer using the format CH4 for CH4.) [C5H7N]

 Silber4 3.043.EOCP. Nicotine is a poisonous, addictive compound found in tobacco. A sample of nicotine contains 6.16 mmol of C, 8.56 mmol of H, and 1.23 mmol of N [1 mmol (1 millimole) = 10-3 mol]. What is the empirical formula for nicotine? (_) C2H5N (o) C5H7N (_) CHN (_) CH3N2

 Silber4 3.044.AP. , Cortisol ( = 362.47 g/mol), one of the major steroid hormones, is a key factor in the synthesis of protein. Its profound effect on the reduction of inflammation explains its use in the treatment of rheumatoid arthritis. Cortisol is 69.6% C, 8.34% H, and 22.1% O by mass. What is its molecular formula? (Type your answer using the format CO2 for CO2.) [C21H30O5]

 Silber4 3.044.EOCP. Cortisol (molar mass = 362.47 g/mol), one of the major steroid hormones, is a key factor in the synthesis of protein. Its profound effect on the reduction of inflammation explains its use in the treatment of rheumatoid arthritis. Cortisol is 69.6% C, 8.34% H, and 22.1% O by mass. What is its molecular formula? (_) C10H15O3 (o) C21H30O5 (_) CHO (_) C6H10O2

 Silber4 3.045.AP. , Acetaminophen is one of the most popular nonaspirin, "over-the-counter" pain relievers. What is the mass % of each element in acetaminophen? C [63.6]% H [6.01]% N [9.27]% O [21.2]%

 Silber4 3.045a.EOCP. Acetaminophen (below) is one of the most popular nonaspirin, "over-the-counter" pain relievers. What is the mass % of oxygen in acetaminophen? (_) 10.585 mass % O (o) 21.17 mass % O (_) 10.58 mass % O (_) 16.00 mass % O

 Silber4 3.045b.EOCP. Acetaminophen (below) is one of the most popular nonaspirin, "over-the-counter" pain relievers. What is the mass % of nitrogen in acetaminophen? (_) 14.00 mass % N (o) 9.268 mass % N (_) 0.324 mass % N (_) 18.54 mass % N

 Silber4 3.045c.EOCP. Acetaminophen (below) is one of the most popular nonaspirin, "over-the-counter" pain relievers. What is the mass % of carbon in acetaminophen? (_) 7.94 mass % C (o) 63.56 mass % C (_) 8 mass % C (_) 12.01 mass % C

 Silber4 3.045d.EOCP. Acetaminophen (below) is one of the most popular nonaspirin, "over-the-counter" pain relievers. What is the mass % of hydrogen in acetaminophen? (_) 0.667 % H (o) 6.002 % H (_) 12.00 % H (_) 0.7 % H

 Silber4 3.046.AP. , Menthol ( = 156.3 g/mol), a strong-smelling substance used in cough drops, is a compound of carbon, hydrogen, and oxygen. When 0.1595 g menthol was subjected to combustion analysis, it produced 0.449 g CO2 and 0.184 g H2O. What is its molecular formula? (Type your answer using the format CO2 for CO2.) [C10H20O]

 Silber4 3.046.EOCP. Menthol (molar mass = 156.3 g/mol), a strong-smelling substance used in cough drops, is a compound of carbon, hydrogen, and oxygen. When 0.1595 g of menthol was subjected to combustion analysis, it produced 0.449 g of CO2 and 0.184 g of H2O. What is its molecular formula? (_) CHO (o) C10H20O (_) C16H18O8 (_) C5H8O2

Silber4 3.047.AP.
What three types of information does a balanced chemical equation provide?
 Key: The balanced reaction provides information on the amount and type of reactants and products.

How?
 Key: The balanced reaction provides information in terms of molecules, mass and mass in grams.

 Silber4 3.047.EOCP. Which is not true about the types of information a balanced chemical equation provides? (_) the identity of the reactant and products (o) the empirical formulas of the reactants and products (_) the physical states of the reactants and products (_) the molar ratios of reactants and products expressed as coefficients

 Silber4 3.048.EOCP. In a balanced chemical equation, the total mass of the reactants is equal to the total mass of the products formed in the reaction. (o) True (_) False

 Silber4 3.049.EOCP. The following boxes represent a chemical reaction between elements A (red) and B (green). Which of the following best represents the balanced equation for the reaction? (_) 2A + 2B A2 + B2 (o) A2 + B2 2AB (_) 4A2 + 4B2 8AB (_) B2 + 2A B 2B2 + A2

 Silber4 3.049.EOCP. In the process of balancing the equation: Al + Cl2 AlCl3 Student I writes: Al + Cl2 AlCl2 Student II writes: Al + Cl2 + Cl AlCl3 Student III writes: 2 Al + 3 Cl2 2 AlCl3 Which student has written the correct balanced chemical equation for the reaction? (_) Student I (_) Student II (o) Student III (_) all three students

 Silber4 3.050.AP. , The following boxes represent a chemical reaction between elements A (red) and B (green): Which of the following best represents the balanced equation for the reaction? (_) 2 A + 2 B A2 + B2 (_) B2 + 2 AB 2 B2 + A2 (o) A2 + B2 2 AB (_) 4 A2 + 4 B2 8 AB

 Silber4 3.051.AP. , Write balanced equations for each of the following by inserting the correct coefficients in the blanks. (Use the lowest possible coefficients.) (a) [16]Cu(s) + [1]S8(s) [8]Cu2S(s) (b) [1]P4O10(s) + [6]H2O(l) [4]H3PO4(l) (c) [1]B2O3(s) + [6]NaOH(aq) [2]Na3BO3(aq) + [3]H2O(l) (d) [4]CH3NH2(g) + [9]O2(g) [4]CO2(g) + [10]H2O(g) + [2]N2(g)

 Silber4 3.051a.EOCP. Give the correct balanced equation for the reaction below. Cu(s) + S8(s) Cu2S(s) (_) 8 Cu(s) + S8(s) 8 Cu2S(s) (_) 16 Cu(s) + 2 S8(s) 16 Cu2S(s) (o) 16 Cu(s) + S8(s) 8 Cu2S(s) (_) Cu(s) + S8(s) Cu2S(s)

 Silber4 3.051b.EOCP. Give the correct balanced equation for the reaction below. P4O10(s) + H2O(l) H3PO4(l) (_) P4O10(s) + 3H2O(l) 2 H3PO4(l) (_) P4O10(s) + H2O(l) H3PO4(l) (o) P4O10(s) + 6 H2O(l) 4 H3PO4(l) (_) 2 P4O10(s) + 3 H2O(l) 2 H3PO4(l)

 Silber4 3.051c.EOCP. Give the correct balanced equation for the reaction below. B2O3(s) + NaOH(aq) Na3BO3(aq) + H2O(l) (_) B2O3(s) + NaOH(aq) Na3BO3(aq) + H2O(l) (_) B2O3(s) + 2 NaOH(aq) 2 Na3BO3(aq) + H2O(l) (o) B2O3(s) + 6 NaOH(aq) 2 Na3BO3(aq) + 3 H2O(l) (_) 2 B2O3(s) + 3 NaOH(aq) 4 Na3BO3(aq) + H2O(l)

 Silber4 3.051d.EOCP. Give the correct balanced equation for the reaction below. CH3NH2(g) + O2(g) CO2(g) + H2O(g) + N2(g) (_) 2 CH3NH2(g) + 2 O2(g) 2 CO2(g) + 5 H2O(g) + N2(g) (_) 3 CH3NH2(g) + O2(g) 3 CO2(g) + 2 H2O(g) + 2 N2(g) (o) 4 CH3NH2(g) + 9 O2(g) 4 CO2(g) + 10H2O(g) + 2 N2(g) (_) CH3NH2(g) + O2(g) CO2(g) + H2O(g) + N2(g)

 Silber4 3.052.AP. , Write (reduced) balanced equations for each of the following by inserting the correct coefficients in the blanks. (a) [1]Cu(NO3)2(aq) + [2]KOH(aq) [1]Cu(OH)2(s) + [2]KNO3(aq) (b) [1]BCl3(g) + [3]H2O(l) [1]H3BO3(s) + [3]HCl(g) (c) [1]CaSiO3(s) + [6]HF(g) [1]SiF4(g) + [1]CaF2(s) + [3]H2O(l) (d) [1](CN)2(g) + [4]H2O(l) [1]H2C2O4(aq) + [2]NH3(g)

 Silber4 3.052a.EOCP. Give the correct balanced equation for the reaction below. Cu(NO3)2(aq) + KOH(aq) Cu(OH)2(s) + KNO3(aq) (_) Cu(NO3)2(aq) + KOH(aq) Cu(OH)2(s) + KNO3(aq) (_) 2 Cu(NO3)2(aq) + 4 KOH(aq) 2 Cu(OH)2(s) + 4 KNO3(aq) (o) Cu(NO3)2(aq) + 2 KOH(aq) Cu(OH)2(s) + 2 KNO3(aq) (_) 2 Cu(NO3)2(aq) + KOH(aq) 2 Cu(OH)2(s) + 2 KNO3(aq)

 Silber4 3.052b.EOCP. Give the correct balanced equation for the reaction below. BCl3(g) + H2O(l) H3BO3(s) + HCl(g) (_) 3 BCl3(g) + 5 H2O(l) 3 H3BO3(s) + HCl(g) (_) 2 BCl3(g) + 3 H2O(l) 2 H3BO3(s) + 3 HCl(g) (o) BCl3(g) + 3 H2O(l) H3BO3(s) + 3 HCl(g) (_) BCl3(g) + H2O(l) H3BO3(s) + HCl(g)

 Silber4 3.052c.EOCP. Give the correct balanced equation for the reaction below. CaSiO3(s) + HF(g) SiF4(g) + CaF2(s) + H2O(l) (_) CaSiO3(s) + HF(g) SiF4(g) + CaF2(s) + H2O(l) (_) CaSiO3(s) + 6 HF(g) 2 SiF4(g) + CaF2(s) + 3 H2O(l) (o) CaSiO3(s) + 6 HF(g) SiF4(g) + CaF2(s) + 3 H2O(l) (_) 2 CaSiO3(s) + 2 HF(g) 2 SiF4(g) + 2 CaF2(s) + H2O(l)

 Silber4 3.052d.EOCP. Give the correct balanced equation for the reaction below. (CN)2(g) + H2O(l) H2C2O4(aq) + NH3(g) (_) (CN)2(g) + 2 H2O(l) H2C2O4(aq) + 2 NH3(g) (_) (CN)2(g) + H2O(l) H2C2O4(aq) + NH3(g) (o) (CN)2(g) + 4 H2O(l) H2C2O4(aq) + 2 NH3(g) (_) 2(CN)2(g) + 2 H2O(l) 2 H2C2O4(aq) + NH3(g)

 Silber4 3.053.AP. , Write balanced equations for each of the following by inserting the correct coefficients in the blanks. (Use the lowest possible coefficients.) (a) [2]SO2(g) + [1]O2(g) [2]SO3(g) (b) [1]Sc2O3(s) + [3]H2O(l) [2]Sc(OH)3(s) (c) [1]H3PO4(aq) + [2]NaOH(aq) [1]Na2HPO4(aq) + [2]H2O(l) (d) [1]C6H10O5(s) + [6]O2(g) [6]CO2(g) + [5]H2O(g)

 Silber4 3.053a.EOCP. Give the correct balanced equation for the reaction below. SO2(g) + O2(g) SO3(g) (_) 4 SO2(g) + 2 O2(g) 4 SO3(g) (_) SO2(g) + 3 O2(g) 2 SO3(g) (o) 2 SO2(g) + O2(g) 2 SO3(g) (_) SO2(g) + O2(g) SO3(g)

 Silber4 3.053b.EOCP. Give the correct balanced equation for the reaction below. Sc2O3(s) + H2O(l) Sc(OH)3(s) (_) Sc2O3(s) + H2O(l) Sc(OH)3(s) (_) Sc2O3(s) + H2O(l) 2 Sc(OH)3(s) (o) Sc2O3(s) + 3 H2O(l) 2 Sc(OH)3(s) (_) 2 Sc2O3(s) + 6 H2O(l) 4 Sc(OH)3(s)

 Silber4 3.053c.EOCP. Give the correct balanced equation for the reaction below. H3PO4(aq) + NaOH(aq) Na2HPO4(aq) + H2O(l) (_) 2 H3PO4(aq) + 4 NaOH(aq) 2 Na2HPO4(aq) + 4 H2O(l) (_) H3PO4(aq) + NaOH(aq) Na2HPO4(aq) + H2O(l) (o) H3PO4(aq) + 2 NaOH(aq) Na2HPO4(aq) + 2 H2O(l) (_) 2 H3PO4(aq) + 2 NaOH(aq) Na2HPO4(aq) + 3 H2O(l)

 Silber4 3.053d.EOCP. Give the correct balanced equation for the reaction below. C6H10O5(s) + O2(g) CO2(g) + H2O(g) (_) C6H10O5(s) + O2(g) CO2(g) + H2O(g) (_) 2 C6H10O5(s) + 12 O2(g) 12 CO2(g) + 10 H2O(g) (o) C6H10O5(s) + 6 O2(g) 6 CO2(g) + 5H2O(g) (_) C6H10O5(s) + 3 O2(g) 6 CO2(g) + 3 H2O(g)

 Silber4 3.054.AP. , Write (reduced) balanced equations for each of the following by inserting the correct coefficients in the blanks. (a) [1]As4S6(s) + [9]O2(g) [1]As4O6(s) + [6]SO2(g) (b) [2]Ca3(PO4)2(s) + [6]SiO2(s) + [10]C(s) [1]P4(g) + [6]CaSiO3(l) + [10]CO(g) (c) [3]Fe(s) + [4]H2O(g) [1]Fe3O4(s) + [4]H2(g) (d) [6]S2Cl2(l) + [16]NH3(g) [1]S4N4(s) + [1]S8(s) + [12]NH4Cl(s)

 Silber4 3.054a.EOCP. Give the correct balanced equation for the reaction below. As4S6(s) + O2(g) As4O6(g) + SO2(g) (o) As4S6(s) + 9 O2(g) As4O6(g) + 6 SO2(g) (_) As4S6(s) + 4 O2(g) As4O6(g) + 6 SO2(g) (_) 2 As4S6(s) + 15 O2(g) 2 As4O6(g) + 12 SO2(g) (_) As4S6(s) + O2(g) As4O6(g) + SO2(g)

 Silber4 3.054b.EOCP. Give the correct balanced equation for the reaction below. Ca3(PO4)2(s) + SiO2(s) + C(s) P4(g) + CaSiO3(l) + CO(g) (o) 2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s) P4(g) + 6 CaSiO3(l) + 10 CO(g) (_) Ca3(PO4)2(s) + SiO2(s) + C(s) P4(g) + CaSiO3(l) + CO(g) (_) 3 Ca3(PO4)2(s) + 4 SiO2(s) + 32 C(s) 2 P4(g) + 9 CaSiO3(l) + 32 CO(g) (_) Ca3(PO4)2(s) + 3 SiO2(s) + C(s) P4(g) + 3 CaSiO3(l) + 2 CO(g)

 Silber4 3.054c.EOCP. Give the correct balanced equation for the reaction below. Fe(s) + H2O(g) Fe3O4(s) + H2(g) (o) 3 Fe(s) + 4 H2O(g) Fe3O4(s) + 4 H2(g) (_) 2 Fe(s) + 4 H2O(g) Fe3O4(s) + H2(g) (_) Fe(s) + H2O(g) Fe3O4(s) + H2(g) (_) 6 Fe(s) + 8 H2O(g) 2 Fe3O4(s) + 8 H2(g)

 Silber4 3.054d.EOCP. Give the correct balanced equation for the reaction below. S2Cl2(l) + NH3(g) S4N4(s) + S8(s) + NH4Cl(s) (o) 6 S2Cl2(l) + 16 NH3(g) S4N4(s) + S8(s) + 12 NH4Cl(s) (_) 2 S2Cl2(l) + 4 NH3(g) S4N4(s) + S8(s) + 4 NH4Cl(s) (_) 2 S2Cl2(l) + NH3(g) S4N4(s) + S8(s) + 2 NH4Cl(s) (_) S2Cl2(l) + NH3(g) S4N4(s) + S8(s) + NH4Cl(s)

 Silber4 3.055.AP. , Convert the following into balanced equations. (Type your answer using the format CO2 for CO2. Use the lowest possible coefficients.) (a) When gallium metal is heated in oxygen gas, it melts and forms solid gallium(III) oxide. [4] [Ga](s) + [3] [O2](g) [2] [Ga2O3](s) (b) Liquid hexane burns in oxygen gas to form carbon dioxide gas and water vapor. [2] [C6H14](l) + [19] [O2](g) [12] [CO2](g) + [14] H2O(g) (c) When solutions of calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms and sodium chloride remains in solution. [3] [CaCl2](g) + [2] [Na3PO4](aq) [1] [Ca3(PO4)2](s) + [6] [NaCl](aq)

 Silber4 3.055a.EOCP. Convert the following description into a balanced equation: When gallium metal is heated in oxygen gas, it melts and forms solid gallium(III) oxide. (o) 4 Ga(s) + 3 O2(g) 2 Ga2O3(s) (_) 3 Ga(s) + O2(g) Ga3O2(s) (_) 2 Ga(s) + 3 O2(g) 2 Ga2O3(s) (_) Ga(s) + O(g) GaO(s)

 Silber4 3.055b.EOCP. Convert the following description into a balanced equation: Liquid hexane burns in oxygen gas to form carbon dioxide gas and water vapor. (o) 2 C6H14(l) + 19 O2(g) 12 CO2(g) + 14 H2O(g) (_) C7H14(l) + 21 O2(g) 7 CO2(g) + 7 H2O(g) (_) C7H16(l) + 11 O2(g) 7 CO2(g) + 8 H2O(g) (_) C6H14(l) + 19 O2(g) 6 CO2(g) + 7 H2O(g)

 Silber4 3.055c.EOCP. Convert the following description into a balanced equation: When solutions of calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms and sodium chloride remains in solution. (o) 3 CaCl2(aq) + 2 Na3PO4(aq) Ca3(PO4)2(s) + 6 NaCl(aq) (_) 2 CaCl2(aq) + 2 NaPO3(aq) 2 CaPO3(s) + 2 NaCl(s) (_) 2 CaCl(aq) + Na2PO3(aq) Ca2PO3 (s) + 2 NaCl(aq) (_) 3 CaCl2(aq) + Na3PO4(aq) Ca3(PO4)2(s) + 3 NaCl(s)

 Silber4 3.056.AP. , Convert the following into balanced equations. (Type your answer using the format CO2 for CO2. Use the lowest possible coefficients.) (a) When lead(II) nitrate solution is added to potassium iodide solution, solid lead(II) iodide forms and potassium nitrate solution remains. [1] [Pb(NO3)2](aq) + [2]KI(aq) [1] [PbI2](s) + [2] [KNO3](aq) (b) Liquid disilicon hexachloride reacts with water to form solid silicon dioxide, hydrogen chloride gas, and hydrogen gas. [1] [Si2Cl6](l) + [4]H2O(l) [2] [SiO2](s) + [6]HCl(g) + [1] [H2](g) (c) When nitrogen dioxide is bubbled into water, a solution of nitric acid forms and gaseous nitrogen monoxide is released. [3] [NO2](g) + [1] [H2O](l) [2] [HNO3](aq) + [1] [NO](g)

 Silber4 3.056a.EOCP. Convert the following description into a balanced equation: When lead(II) nitrate solution is added to potassium iodide solution, solid lead(II) iodide forms and potassium nitrate solution remains. (_) PbNO3(aq) + KI(aq) PbI(s) + KNO3(aq) (_) 2 Pb(NO3)2(aq) + 4 KI(aq) 2 PbI2(s) + 4 KNO3(aq) (_) Pb3NO2(aq) + 2 KI(aq) Pb3I2(s) + 2 KNO2(aq) (o) Pb(NO3)2(aq) + 2 KI(aq) PbI2(s) + 2 KNO3(aq)

 Silber4 3.056b.EOCP. Convert the following description into a balanced equation: Liquid disilicon hexachloride reacts with water to form solid silicon dioxide, hydrogen chloride gas, and hydrogen gas. (_) Si2Cl6(l) + 2 H2O(l) 2 SiO2(s) + 2 HCl(g) + H2(g) (_) Si2Cl7(l) + 4 H2O(l) 2 SiO2(s) + 2 HCl(g) + 2 H(g) (_) SiCl6(l) + 3 H2O(l) SiO2(s) + 6 HCl(g) + H(g) (o) Si2Cl6(l) + 4 H2O(l) 2 SiO2(s) + 6 HCl(g) + H2(g)

 Silber4 3.056c.EOCP. Convert the following description into a balanced equation: When nitrogen dioxide is bubbled into water, a solution of nitric acid forms and gaseous nitrogen monoxide is released. (_) 2 NO2(aq) + H2O(l) 2 HNO3(aq) + NO(g) (_) 3 NO2(g) + 6 H2O(l) 6 H2NO(aq) + N2O(g) (_) 2 NO2(g) + H2O(l) 2 HNO2(aq) + 2 NO(g) (o) 3 NO2(g) + H2O(l) 2 HNO3(aq) + NO(g)

 Silber4 3.057.EOCP. The phrase stoichiometrically equivalent molar ratio is the ratio of the subscripts in a balanced equation. (_) True (o) False

 Silber4 3.058.EOCP. The percent yield for a reaction will be the same whether it is calculated from mass quantities or from mole quantities. (o) True (_) False

 Silber4 3.060.AP. , Percent yields are generally calculated from mass quantities. Would the result be the same if mole quantities were used instead? (o) yes (_) no Why? (Select all that apply.) [_] The % yield will not be the same since mass and moles are not directly proportional. [_] The yields (%) are sums of actual and theoretical value. [x] The % yield will be same since mass and moles are directly proportional. [x] The yields (%) are ratios of actual to theoretical value. [x] Both can be expressed in mass or mole comparison.

 Silber4 3.061.AP. Chlorine gas can be made in the laboratory by the reaction of hydrochloric acid and manganese (IV) oxide.4 HCl(aq) + MnO2(s) MnCl2(aq) + 2 H2O(g) + Cl2(g) Consider the reaction of 2.44 mol HCl with excess MnO2. (a) How many moles of Cl2 form? [0.610] mol(b) How many grams of Cl2 form? [43.2] g

 Silber4 3.061a.EOCP. Chlorine gas can be made in the laboratory by combining hydrochloric acid and manganese(IV) oxide according to the following reaction: 4 HCl(aq) + MnO2(s) MnCl2(aq) + 2 H2O(g) + Cl2(g) When 1.82 mol of HCl reacts with excess MnO2, how many moles of Cl2 form? (_) 7.28 mol Cl2 (_) 1.82 mol Cl2 (_) 0.9 mol Cl2 (o) 0.455 mol Cl2

 Silber4 3.061b.EOCP. Chlorine gas can be made in the laboratory by combining hydrochloric acid and manganese(IV) oxide according to the following reaction: 4 HCl(aq) + MnO2(s) MnCl2(aq) + 2 H2O(g) + Cl2(g) When 1.82 mol of HCl reacts with excess MnO2, how many grams of Cl2 form? (_) 516 g Cl2 (_) 130 g Cl2 (_) 63.81 g Cl2 (o) 32.3 g Cl2

 Silber4 3.062.AP. Bismuth oxide reacts with carbon to form bismuth metal. Bi2O3(s) + 3 C(s) 2 Bi(s) + 3 CO(g) (a) When 439 g Bi2O3 reacts with excess carbon, how many moles of Bi2O3 react? [0.942] mol (b) How many moles of Bi form? [1.88] mol

 Silber4 3.062a.EOCP. Bismuth oxide reacts with carbon to form bismuth metal according to the following reaction: Bi2O3(s) + 3 C(s) Bi(s) + 3 CO(g) When 352 g of Bi2O3 reacts with excess carbon, how many moles of Bi2O3 react? (_) 1.51 mol Bi2O3 (_) 0.7554 mol Bi2O3 (_) 2 mol Bi2O3 (o) 0.755 mol Bi2O3

 Silber4 3.062b.EOCP. 0.755 mole of bismuth oxide reacts with an excess of carbon to form bismuth metal according to the following reaction: Bi2O3(s) + 3 C(s) 2 Bi(s) + 3 CO(g) How many moles of Bi form? (_) 2 mol Bi (_) 0.755 mol Bi (_) 0.7554 mol Bi (o) 1.51 mol Bi

 Silber4 3.063.AP. Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen. 4 KNO3(s) 2 K2O(s) + 2 N2(g) + 5 O2(g) (a) How many moles of KNO3 must be heated to produce 93.0 kg oxygen? [2330] mol(b) How many grams of KNO3 is this? [2.35e+05] g

 Silber4 3.063a.EOCP. Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen according to the following reaction: 4 KNO3(s) 2 K2O(s) + 2 N2(g) + 5 O2(g) To produce 88.6 kg of oxygen, how many moles of KNO3 must be heated? (_) 2.215 mol KNO3 (_) 1.1 104 mol KNO3 (_) 2.77 103 mol KNO3 (o) 2.22 103 mol KNO3

 Silber4 3.063b.EOCP. Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen according to the following reaction: 4 KNO3(s) 2 K2O(s) + 2 N2(g) + 5 O2(g) How many grams of KNO3 must be heated to produce 88.6 kg of oxygen? (_) 2.196 101 g KNO3 (o) 2.24 105 g KNO3 (_) 1.11 106 g KNO3 (_) 2.2 102 g KNO3

 Silber4 3.064.AP. Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water. Cr2O3(s) + 3 H2S(g) Cr2S3(s) + 3 H2O(l) (a) How many moles of Cr2O3 are required to produce 465 g of Cr2S3? [2.32] mol (b) How many grams of Cr2O3 are required? [353] g

 Silber4 3.064a.EOCP. Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water according to the following reaction: Cr2O3(s) + 3 H2S(g) Cr2S3(s) + 3 H2O(l) To produce 421 g of Cr2S3, how many moles of Cr2O3 are required? (_) 2 mol Cr2O3 (o) 2.10 mol Cr2O3 (_) 2.81 104 mol Cr2O3 (_) 6.3 mol Cr2O3

 Silber4 3.064b.EOCP. Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water according to the following reaction: Cr2O3(s) + 3 H2S(g) Cr2S3(s) + 3 H2O(l) How many grams of Cr2O3 are required to produce 421 g of Cr2S3? (_) 4.3 106 g Cr2O3 (o) 320. g Cr2O3 (_) 957.6 g Cr2O3 (_) 1.85 102 g Cr2O3

 Silber4 3.065.AP. Calculate the mass of each product formed when 37.38 g diborane (B2H6) reacts with excess water.B2H6(g) + H2O(l) H3BO3(s) + H2(g) [unbalanced]H3BO3 [167.1] gH2 [16.34] g

 Silber4 3.065a.EOCP. 33.61 g of diborane (B2H6) reacts with excess water according to the following unbalanced equation: B2H6(g) + H2O(l) H3BO3(s) + H2(g) Calculate the mass of H3BO3 formed. (_) 225.3 g H3BO3 (o) 150.2 g H3BO3 (_) 75 g H3BO3 (_) 1.21 g H3BO3

 Silber4 3.065b.EOCP. 33.61 g of diborane (B2H6) reacts with excess water according to the following unbalanced equation: B2H6(g) + H2O(l) H3BO3(s) + H2(g) Calculate the mass of H2 formed. (_) 7 g H2 (o) 14.69 g H2 (_) 7.347 g H2 (_) 2.452 g H2

 Silber4 3.066.AP. Calculate the mass of each product formed when 224 g of silver sulfide reacts with excess hydrochloric acid. Ag2S(s) + HCl(aq) AgCl(s) + H2S(g) [unbalanced] AgCl [259] gH2S [30.8] g

 Silber4 3.066a.EOCP. 174 g of silver sulfide reacts with excess hydrochloric acid according to the following unbalanced equation: Ag2S(s) + HCl(aq) AgCl(s) + H2S(g) Calculate the mass of AgCl formed. (_) 302 g AgCl (o) 201 g AgCl (_) 2 g AgCl (_) 100.6 g AgCl

 Silber4 3.066b.EOCP. 174 g of silver sulfide reacts with excess hydrochloric acid according to the following unbalanced equation: Ag2S(s) + HCl(aq) AgCl(s) + H2S(g) Calculate the mass of H2S formed. (_) 48 g H2 (o) 23.9 g H2 (_) 1.40 g H2 (_) 1265 g H2

 Silber4 3.067.AP. Elemental phosphorus occurs as tetratomic molecules, P4. What mass of chlorine gas is needed for complete reaction with 396 g phosphorus to form phosphorus pentachloride? [2270] g

 Silber4 3.067.EOCP. Elemental phosphorus occurs as tetratomic molecules, P4. What mass of chlorine gas is needed for complete reaction with 355 g of phosphorus to form phosphorus pentachloride? (_) 406.3 g Cl (o) 2.03 103 g Cl2 (_) 102 g Cl (_) 203.1 g Cl2

 Silber4 3.068.AP. Elemental sulfur occurs as octatomic molecules, S8. What mass of fluorine gas is needed for complete reaction with 26.5 g sulfur to form sulfur hexafluoride? [94.2] g

 Silber4 3.068.EOCP. Elemental sulfur occurs as octatomic molecules, S8. What mass of fluorine gas is needed for complete reaction with 17.8 g of sulfur to form sulfur hexafluoride? (_) 21.09 g F2 (o) 63.3 g F2 (_) 240.4 g F (_) 1.32 g F

 Silber4 3.069a.EOCP. Solid iodine trichloride is prepared by reaction between solid iodine and gaseous chlorine to form iodine monochloride crystals, followed by treatment with additional chlorine. Give the overall balanced equation for the formation of iodine trichloride. (_) I2(s) + Cl2(g) ICl3(s) (o) I2(s) + 3 Cl2(g) 2 ICl3(s) (_) I2(s) + Cl2(g) 2 ICl(s) (_) ICl(s) + Cl2(g) ICl3(s)

 Silber4 3.069b.EOCP. Solid iodine trichloride is prepared by reaction between solid iodine and gaseous chlorine to form iodine monochloride crystals, followed by treatment with additional chlorine. The overall balanced equation is shown below: I2(s) + 3 Cl2(g) 2 ICl3(s) How many grams of iodine are needed to prepare 31.4 kg of final product? (_) 2.885 101 g I2 (o) 1.71 104 g I2 (_) 3.4 104 g I2 (_) 7.97 103 g I2

 Silber4 3.070.AP. Lead can be prepared from galena [lead(II) sulfide] by first roasting in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide. (Type your answer using the format CO2 for CO2. Use the lowest possible coefficients.) (a) Write a balanced equation for each step. [2] [PbS](s) + [3] [O2](g) [2] [PbO](s) + [2] [SO2](g) [2] [PbO](s) + [1]PbS(s) [3] [Pb](l) + [1] [SO2](g) (b) Write an overall balanced equation for the process. [1] [PbS](s) + [1] [O2](g) [1] [Pb](l) + [1] [SO2](g) (c) How many metric tons of sulfur dioxide form for every metric ton of lead obtained? [0.309] metric tons

 Silber4 3.070a.EOCP. Lead can be prepared from galena [lead(II) sulfide] by first roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide. Give an overall balanced equation for the process. (_) 2 PbO(s) + PbS(s) 3 Pb(l) + SO2(g) (_) 2 PbS(s) + 3O2(g) 2 PbO(s) + 2SO2(g) (_) Pb2S(s) + O2(g) 2 Pb(l) + SO2(g) (o) PbS(s) + O2(g) Pb(l) + SO2(g)

 Silber4 3.070b.EOCP. Lead can be prepared from galena [lead(II) sulfide] by first roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide. How many metric tons of sulfur dioxide form for every metric ton of lead obtained? (_) 1.3 104 metric tons SO2 (_) 64.1 metric tons SO2 (_) 3.233 metric ton SO2 (o) 0.309 metric ton SO2

 Silber4 3.071a.EOCP. Many metals react with oxygen gas to form the metal oxide. For example, calcium reacts as follows: 2 Ca(s) + O2(g) 2 CaO(s) You wish to calculate the mass of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2. How many moles of CaO can be produced from the given mass of Ca? (_) 0.1 mol CaO (_) 0.1746 mol CaO (_) 0.210 mol CaO (o) 0.105 mol CaO

 Silber4 3.071b.EOCP. Many metals react with oxygen gas to form the metal oxide. For example, calcium reacts as follows: 2 Ca(s) + O2(g) 2 CaO(s) You wish to calculate the mass of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2. How many moles of CaO can be produced in this experiment from the given mass of O2? (_) 0.09 mol CaO (_) 0.438 mol CaO (_) 0.044 mol CaO (o) 0.175 mol CaO

 Silber4 3.071c.EOCP. Many metals react with oxygen gas to form the metal oxide. For example, calcium reacts as follows: 2 Ca(s) + O2(g) 2 CaO(s) You wish to calculate the mass of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2. Which is the limiting reactant? (_) calcium oxide (_) oxygen (_) not enough information to decide (o) calcium

 Silber4 3.071d.EOCP. Many metals react with oxygen gas to form the metal oxide. For example, calcium reacts as follows: 2 Ca(s) + O2(g) 2 CaO(s) You wish to calculate the mass of calcium oxide that can be prepared from 4.20 g of Ca and 2.80 g of O2. How many grams of CaO can be produced? (_) 267 g CaO (_) 9.791 g CaO (_) 534.1 g CaO (o) 5.89 g CaO

 Silber4 3.072.AP. Metal hydrides react with water to form hydrogen gas and the metal hydroxide. SrH2(s) + 2 H2O(l) Sr(OH)2(s) + 2 H2(g)You wish to calculate the mass of hydrogen gas that can be prepared from 5.89 g of SrH2 and 4.67 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2? [0.131] mol (b) How many moles of H2 can be produced from the given mass of H2O? [0.259] mol (c) Which is the limiting reactant? (Type your answer using the format CO2 for CO2.) [SrH2] (d) How many grams of H2 can be produced? [0.265] g

 Silber4 3.072a.EOCP. Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, SrH2(s) + 2 H2O(l) Sr(OH)2(s) + 2 H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 5.63 g of SrH2 and 4.80 g of H2O. How many moles of H2 can be produced from the given mass of SrH2? (_) 0.0535 mol H2 (_) 0.062 mol H2 (_) 0.11 mol H2 (o) 0.126 mol H2

 Silber4 3.072b.EOCP. Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, SrH2(s) + 2 H2O(l) Sr(OH)2(s) + 2 H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 5.63 g of SrH2 and 4.80 g of H2O. How many moles of H2 can be produced in this experiment from the given mass of H2O? (_) 0.53 mol H2 (_) 0.312 mol H2 (_) 2.556 mol H2 (o) 0.266 mol H2

 Silber4 3.072c.EOCP. Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, SrH2(s) + 2 H2O(l) Sr(OH)2(s) + 2 H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 5.63 g of SrH2 and 4.80 g of H2O. Which is the limiting reactant? (_) Sr(OH)2 (_) H2O (_) H2 (o) SrH2

 Silber4 3.072c.EOCP. Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, SrH2(s) + 2 H2O(l) Sr(OH)2(s) + 2 H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 5.63 g of SrH2 and 4.80 g of H2O. How many grams of H2 can be produced? (_) 0.536 g H2 (_) 0.13 g H2 (_) 0.27 g H2 (o) 0.253 g H2

 Silber4 3.073a.EOCP. 685 g of iodine trichloride reacts with 117.4 g of water to form iodic acid (HIO3), according to the following unbalanced reaction: ICl3 + H2O ICl + HIO3 + HCl Calculate the maximum number of moles of HIO3 that can be produced from this reaction. (_) 2.9 mol HIO3 (_) 2.17 mol HIO3 (_) 6.5 mol HIO3 (o) 1.47 mol HIO3

 Silber4 3.073b.EOCP. 685 g of iodine trichloride reacts with 117.4 g of water to form iodic acid (HIO3), according to the following unbalanced reaction: ICl3 + H2O ICl + HIO3 + HCl Calculate the maximum number of grams of HIO3 that can be produced from this reaction. (_) 510 g HIO3 (_) 381.7 g HIO3 (_) 1140 g HIO3 (o) 258 g HIO3

 Silber4 3.073c.EOCP. 685 g of iodine trichloride reacts with 117.4 g of water to form iodic acid (HIO3), according to the following unbalanced reaction: ICl3 + H2O ICl + HIO3 + HCl What mass of the excess reactant remains? (_) 568 g excess ICl3 (_) 80 g excess H2O (_) 79.5 g excess ICl3 (o) 37.9 g excess H2O

 Silber4 3.074.AP. Calculate the maximum number of moles and grams of H2S that can form when 176 g aluminum sulfide reacts with 122 g water.Al2S3 + H2O Al(OH)3 + H2S [unbalanced] [3.39] mol [115] g What mass of the excess reactant remains? [7] g

 Silber4 3.074a.EOCP. 158 g of aluminum sulfide reacts with 131 g of water according to the following unbalanced reaction: Al2S3 + H2O Al(OH)3 + H2S Calculate the maximum number of moles of H2S that can be produced from this reaction. (_) 3.6 mol H2S (_) 2.104 mol H2S (o) 3.16 mol H2S (_) 1.05 mol H2S

 Silber4 3.074b.EOCP. 158 g of aluminum sulfide reacts with 131 g of water according to the following unbalanced reaction: Al2S3 + H2O Al(OH)3 + H2S Calculate the maximum number of grams of H2S that can be produced from this reaction. (_) 122.7 g H2S (_) 72 g H2S (o) 108 g H2S (_) 35.79 g H2S

 Silber4 3.074c.EOCP. 158 g of aluminum sulfide reacts with 131 g of water according to the following unbalanced reaction: Al2S3 + H2O Al(OH)3 + H2S What mass of the excess reactant remains? (_) 27 g excess Al2S3 (_) 100 g excess Al2S3 (o) 17 g excess H2O (_) 114 g excess H2O

 Silber4 3.075a.EOCP. 0.100 mol of carbon is burned in a closed vessel with 8.00 g of oxygen. How many grams of carbon dioxide can be produced from this reaction? (_) 8.81 g CO2 (_) 0.004 g CO2 (o) 4.40 g CO2 (_) 2.2 g CO2

 Silber4 3.075b.EOCP. 0.100 mol of carbon is burned in a closed vessel with 8.00 g of oxygen. Which reactant is in excess? (_) carbon (_) not enough information to decide (o) oxygen (_) carbon dioxide

 Silber4 3.075c.EOCP. 0.100 mol of carbon is burned in a closed vessel with 8.00 g of oxygen. How many grams of excess reactant remain after the reaction? (_) 2.2 g excess CO2 (_) not enough information to decide (o) 4.80 g excess O2 (_) 6.8 g excess C

 Silber4 3.076a.EOCP. A mixture of 0.0359 g of hydrogen and 0.0175 mol of oxygen in a closed container is sparked to initiate a reaction. How many grams of water can form? (_) 0.0178 g H2O (_) 0.6 g H2O (o) 0.321 g H2O (_) 0.28 g H2O

 Silber4 3.076b.EOCP. A mixture of 0.0359 g of hydrogen and 0.0175 mol of oxygen in a closed container is sparked to initiate a reaction. Which reactant is in excess? (_) H2 (_) not enough information to decide (o) O2 (_) H2O

 Silber4 3.076c.EOCP. A mixture of 0.0359 g of hydrogen and 0.0175 mol of oxygen in a closed container is sparked to initiate a reaction. How many grams of the excess reactant remain after the reaction? (_) 0.018 g excess H2 (_) not enough information to decide (o) 0.275 g excess O2 (_) 0.3 g excess H2O

 Silber4 3.077a.EOCP. 62.5 g of aluminum nitrite and 54.6 g of ammonium chloride react completely to form aluminum chloride, nitrogen, and water. Calculate the mass of aluminum nitrite present after the reaction is complete. (_) 62.5 g (_) all reacted, none left (o) 6.4 g (_) 56 g

 Silber4 3.077b.EOCP. 62.5 g of aluminum nitrite and 54.6 g of ammonium chloride react completely to form aluminum chloride, nitrogen, and water. Calculate the mass of ammonium chloride present after the reaction is complete. (_) 54.6 g (_) 27.3 g (o) all reacted, none left (_) 14 g

 Silber4 3.077c.EOCP. 62.5 g of aluminum nitrite and 54.6 g of ammonium chloride react completely to form aluminum chloride, nitrogen, and water. Calculate the mass of aluminum chloride present after the reaction is complete. (_) 136.0 g (_) 15.1 g (o) 45.3 g (_) 271.9 g

 Silber4 3.077d.EOCP. 62.5 g of aluminum nitrite and 54.6 g of ammonium chloride react completely to form aluminum chloride, nitrogen, and water. Calculate the mass of nitrogen present after the reaction is complete. (_) 9.5 g (_) 1.62 g (o) 28.6 g (_) 57.16 g

 Silber4 3.077e.EOCP. 62.5 g of aluminum nitrite and 54.6 g of ammonium chloride react completely to form aluminum chloride, nitrogen, and water. Calculate the mass of water present after the reaction is complete. (_) 18.4 g (_) 3.1 g (o) 36.8 g (_) 6.127 g

 Silber4 3.078.AP. Calcium nitrate and ammonium fluoride react to form calcium fluoride, dinitrogen monoxide, and water vapor. What mass of each substance is present after 16.8 g of calcium nitrate and 16.52 g of ammonium fluoride react completely? Ca(NO3)2 [0.00e+00] g NH4F [8.94] g CaF2 [7.99] g N2O [9.01] g H2O [7.38] g

 Silber4 3.078a.EOCP. 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely to form calcium fluoride, dinitrogen monoxide, and water vapor. Calculate the mass of calcium nitrate present after the reaction is complete. (_) 16.8 g (_) 8 g (o) all reacted, none left (_) 0.10 g

 Silber4 3.078b.EOCP. 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely to form calcium fluoride, dinitrogen monoxide, and water vapor. Calculate the mass of ammonium fluoride present after the reaction is complete. (_) 7.6 g (_) all reacted, none left (o) 9.95 g (_) 18 g

 Silber4 3.078c.EOCP. 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely to form calcium fluoride, dinitrogen monoxide, and water vapor. Calculate the mass of calcium fluoride present after the reaction is complete. (_) 15.93 g (_) 3.98 g (o) 7.96 g (_) 32 g

 Silber4 3.078d.EOCP. 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely to form calcium fluoride, dinitrogen monoxide, and water vapor. Calculate the mass of dinitrogen monoxide present after the reaction is complete. (_) 4.5 g (_) 2.24 g (o) 8.98 g (_) 17.96 g

 Silber4 3.078e.EOCP. 16.8 g of calcium nitrate and 17.50 g of ammonium fluoride react completely to form calcium fluoride, dinitrogen monoxide, and water vapor. Calculate the mass of water vapor present after the reaction is complete. (_) 1.8 g (_) 0.9 g (o) 7.35 g (_) 3.68 g

 Silber4 3.079.AP. Two successive reactions, A B and B C, have yields of 77% and 53%, respectively. What is the overall percent yield for conversion of A to C? [41]%

 Silber4 3.079.EOCP. Two successive reactions, A B and B C, have yields of 82% and 65%, respectively. What is the overall percent yield for conversion of A to C? (_) 82% overall yield (_) 65% overall yield (o) 53% overall yield (_) 17% overall yield

 Silber4 3.080.EOCP. Two successive reactions, D E and E F, have yields of 48% and 73%, respectively. What is the overall percent yield for conversion of D to F? (_) 48% overall yield (_) 25% overall yield (o) 35% overall yield (_) 73% overall yield

 Silber4 3.081.AP. What is the percent yield of a reaction in which 41.6 g of tungsten (VI) oxide (WO3) reacts with excess hydrogen gas to produce metallic tungsten and 9.70 mL of water (d = 1.00 g/mL)? [1.00e+02]%

 Silber4 3.081.EOCP. What is the percent yield of a reaction in which 41.5 g of tungsten(VI) oxide (WO3) reacts with excess hydrogen gas to produce metallic tungsten and 9.50 mL of water (d = 1.00 g/mL)? (_) 50% yield (_) 53.7% yield (o) 98.2% yield (_) 18% yield

 Silber4 3.082.EOCP. What is the percent yield of a reaction in which 200. g of phosphorus trichloride reacts with excess water to form 128 g of HCl and aqueous phosphorous acid (H3PO3)? (_) 12.8% yield (_) 16% yield (o) 80.5% yield (_) 53% yield

 Silber4 3.083.AP. When 23.0 g methane and 47.2 g chlorine gas undergo a reaction that has an 80.0% yield, what mass of chloromethane (CH3Cl) forms? Hydrogen chloride also forms. [26.9] g

 Silber4 3.083.EOCP. When 18.5 g of methane and 43.0 g of chlorine gas undergo a reaction that has an 80.0% yield, what mass of chloromethane (CH3Cl) forms? (Note: Hydrogen chloride also forms.) (_) 30.59 g CH3Cl (_) 49 g CH3Cl (o) 24.5 g CH3Cl (_) 15.3 g CH3Cl

 Silber4 3.084.EOCP. When 56.6 g of calcium and 30.5 g of nitrogen gas undergo a reaction that has a 93.0% yield, what mass of calcium nitride forms? (_) 70.93 g CaN (_) 44.6 g CaN2 (o) 64.8 g Ca3N2 (_) 62 g Ca2N3

 Silber4 3.085.AP. Cyanogen, (CN)2, has been observed in the atmosphere of Titan, Saturn's largest moon, and in the gases of interstellar nebulas. On Earth, it is used as a welding gas and a fumigant. In its reaction with fluorine gas, carbon tetrafluoride and nitrogen trifluoride gases are produced. What mass of carbon tetrafluoride forms when 70.9 g of each reactant is used? [46.9] g

 Silber4 3.085.EOCP. Cyanogen, (CN)2, has been observed in the atmosphere of Titan, Saturn's largest moon, and in the gases of interstellar nebulas. On Earth, it is used as a welding gas and a fumigant. In its reaction with fluorine gas, carbon tetrafluoride and nitrogen trifluoride gases are produced. What mass of carbon tetrafluoride forms when 80.0 g of each reactant is used? (_) 185 g CF4 (_) 175.9 g CF4 (o) 52.9 g CF4 (_) 648 g CF4

 Silber4 3.086.EOCP. An intermediate step in the industrial production of nitric acid involves the reaction of ammonia with oxygen gas to form nitrogen monoxide and water. How many grams of nitrogen monoxide can form by the reaction of 466 g of ammonia with 812 g of oxygen? (_) 761.5 g NO (_) 950 g NO (o) 609 g NO (_) 101.5 g NO

 Silber4 3.087a.EOCP. Gaseous butane is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 6.50 mL of butane (d = 0.579 g/mL). How many grams of oxygen are needed to burn the butane completely? (_) 2.07 g O2 (_) 3.6 g O2 (o) 13.5 g O2 (_) 12.43 g O2

 Silber4 3.087b.EOCP. Gaseous butane is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 6.50 mL of butane (d = 0.579 g/mL). How many moles of CO2 form when all the butane burns? (_) 3.8 mol CO2 (_) 0.004 mol CO2 (_) 26 mol CO2 (o) 0.259 mol CO2

 Silber4 3.087c.EOCP. Gaseous butane is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 6.50 mL of butane (d = 0.579 g/mL). How many total molecules of gas form when the butane burns completely? (_) 3.9 1022 gas molecules (_) 1.95 1023 gas molecules (_) 1.6 1023 gas molecules (o) 3.51 1023 gas molecules

 Silber4 3.088.EOCP. Sodium borohydride (NaBH4) can be prepared by reacting sodium hydride with gaseous diborane (B2H6). Assuming a 95.5% yield, how many grams of NaBH4 can be prepared by reacting 7.88 g of sodium hydride and 8.12 g of diborane? (_) 34.6 g (_) 22.2 g (_) 12.4 g (o) 11.9 g

 Silber4 3.089.AP. Box A represents a unit volume of a solution. Choose from boxes B or C the one representing the same unit volume of solution that has each of the following. (a) more solute added (_) A (_) B (o) C (b) more solvent added (_) A (o) B (_) C (c) lower molarity (_) A (o) B (_) C (d) higher concentration (_) A (_) B (o) C

 Silber4 3.089a.EOCP. Box A represents a unit volume of a solution. Box B represents the same unit volume of solution that has: (_) more solute added and lower concentration. (_) more solute added and higher molarity. (_) more solute added and lower concentration. (o) more solvent added and lower concentration.

 Silber4 3.089b.EOCP. Box A represents a unit volume of a solution. Box C represents the same unit volume of solution that has: (_) more solute added and lower concentration. (_) more solvent added and lower concentration. (_) more solute added and lower concentration. (o) more solute added and higher molarity.

Silber4 3.091.AP.
Are the following instructions for diluting a 10.0 M solution to a 1.00 M solution correct: "Take 100.0 mL of the 10.0 M solution and add 900.0 mL water"?

Explain.
 Key: Volumes are not additive. Take 100.00 mL of the 10.0 M solution and add sufficient water to make 1.00 L of solution.

 Silber4 3.091.EOCP. To dilute a 10.0 M solution to a 1.00 M solution, take 100.0 mL of the 10.0 M solution and add 900.0 mL water. (_) True (o) False

 Silber4 3.092.AP. Calculate each of the following quantities. (a) grams of solute in 167.7 mL of 0.207 M calcium acetate [5.49] g(b) molarity of 512 mL solution containing 21.1 g of potassium iodide [0.248] M(c) moles of solute in 145.6 L of 0.743 M sodium cyanide [108] mol

 Silber4 3.092a.EOCP. Calculate the grams of solute in 175.8 mL of 0.207 M calcium acetate. (o) 5.76 g Ca(CH3COO)2 (_) 0.04 g Ca(CH3COO)2 (_) 32.7 g Ca(CH3COO)2 (_) 186.2 g Ca(CH3COO)2

 Silber4 3.092b.EOCP. Calculate the molarity of 500. mL of solution containing 21.1 g of potassium iodide. (o) 0.254 M (_) 4.22 M (_) 7.0 M (_) 2.5 10-4 M

 Silber4 3.092c.EOCP. Calculate the moles of solute in 145.6 L of 0.850 M sodium cyanide. (o) 124 mol NaCN (_) 0.17 mol NaCN (_) 12.4 mol NaCN (_) 17 mol NaCN

 Silber4 3.093.AP. Calculate each of the following quantities. (a) volume in liters of 1.71 M potassium hydroxide that contains 7.90 g of solute [0.0823] L(b) number of Cu2+ ions in 65 L of 3.0 M copper(II) chloride [1.2e+26] ions(c) molarity of a 296 mL of solution containing 100. mmol of glucose [0.338] M

 Silber4 3.093a.EOCP. Calculate the volume in liters of 2.26 M potassium hydroxide that contains 8.42 g of solute. (o) 0.0664 L KOH (_) 3.72 L KOH (_) 209 L KOH (_) 15 L KOH

 Silber4 3.093b.EOCP. Calculate the number of Cu2+ ions in 52 L of 2.3 M copper(II) chloride. (o) 7.2 1025 Cu2+ ions (_) 1.36 1025 Cu2+ ions (_) 3.6 1025 Cu2+ ions (_) 1.44 1026 Cu2+ ions

 Silber4 3.093c.EOCP. Calculate the molarity of 275 mL of solution containing 135 mmol of glucose. (o) 0.491 M glucose (_) 2.0 M glucose (_) 4.9 M glucose (_) 37.1 M glucose

 Silber4 3.094.AP. Calculate each of the following quantities. (a) grams of solute needed to make 427 mL of 5.62 10-2 M potassium sulfate [4.18] g (b) molarity of a solution that contains 6.26 mg of calcium chloride in each milliliter [0.0564] M(c) number of Mg2+ ions in each milliliter of 0.246 M magnesium bromide [1.48e+20] ions

 Silber4 3.094a.EOCP. Calculate the grams of solute needed to make 475 mL of 5.62 10-2 M potassium sulfate. (o) 4.65 g K2SO4 (_) 4.7 103 g K2SO4 (_) 26.70 g K2SO4 (_) 0.48 g K2SO4

 Silber4 3.094b.EOCP. Calculate the molarity of a solution that contains 6.55 mg of calcium chloride in each milliliter. (o) 5.90 10-2 M CaCl2 (_) 5.9 M CaCl2 (_) 7.269 10-1 M CaCl2 (_) 1.7 10-2 M CaCl2

 Silber4 3.094c.EOCP. Calculate the number of Mg2+ ions in each milliliter of 0.184 M magnesium bromide. (o) 1.11 1020 Mg2+ ions (_) 1.1 1023 Mg2+ ions (_) 1.84 10-4 Mg2+ ions (_) 2 1026 Mg2+ ions

 Silber4 3.095.AP. Calculate each of the following quantities. (a) molarity of the solution resulting from dissolving 34.4 g of silver nitrate in enough water to give a final volume of 326 mL [0.621] M(b) volume in liters of 0.489 M manganese(II) sulfate that contains 55.0 g of solute [0.745] L(c) volume in milliliters of 6.58 10-2 M adenosine triphosphate (ATP) that contains 1.41 mmol ATP [21.4] mL

 Silber4 3.095a.EOCP. Calculate the molarity of the solution resulting from dissolving 46.0 g of silver nitrate in enough water to give a final volume of 335 mL. (_) 15.41 M AgNO3 (_) 1.237 M AgNO3 (_) 11 M AgNO3 (o) 0.808 M AgNO3

 Silber4 3.095b.EOCP. Calculate the volume in liters of 0.385 M manganese(II) sulfate that contains 57.0 g of solute. (_) 148 L MnSO4 (_) 1.020 L MnSO4 (_) 0.007 L MnSO4 (o) 0.980 L MnSO4

 Silber4 3.095c.EOCP. Calculate the volume in milliliters of 6.44 10-2 M adenosine triphosphate (ATP) that contains 1.68 mmol of ATP. (_) 108 mL ATP (_) 38.33 mL ATP (_) 2.6 10-2 mL ATP (o) 26.1 mL ATP

 Silber4 3.096.AP. Calculate each of the following quantities. (a) molarity of a solution prepared by diluting 30.44 mL of 0.288 M potassium chloride to 150.00 mL [0.0584] M(b) molarity of a solution prepared by diluting 26.46 mL of 0.0626 M ammonium sulfate to 500.00 mL [0.00331] M(c) molarity of sodium ion in a solution made by mixing 4.42 mL of 0.265 M sodium chloride with 500. mL of 6.51 10-3 M sodium sulfate (assume volumes are additive) [0.0152] M

 Silber4 3.096a.EOCP. Calculate the molarity of a solution prepared by diluting 37.00 mL of 0.250 M potassium chloride to 150.00 mL. (_) 1.37 M KCl (_) 1.82 M KCl (_) 0.05142 M KCl (o) 0.0617 M KCl

 Silber4 3.096b.EOCP. Calculate the molarity of a solution prepared by diluting 25.71 mL of 0.0706 M ammonium sulfate to 500.00 mL. (_) 1.373 M (NH4)2SO4 (_) 0.0514 M (NH4)2SO4 (_) 0.73 M (NH4)2SO4 (o) 0.00363 M (NH4)2SO4

 Silber4 3.096c.EOCP. Calculate the molarity of sodium ion in a solution made by mixing 3.58 mL of 0.288 M sodium chloride with 500. mL of 6.51 10-3 M sodium sulfate (assume volumes are additive). (_) 1.5 10-5 M Na+ (_) 6.51 M Na+ (_) 1.031 M Na+ (o) 0.0150 M Na+

 Silber4 3.097.AP. Calculate each of the following quantities. (a) volume of 1.549 M copper(II) nitrate that must be diluted with water to prepare 776.3 mL of a 0.8543 M solution [428.1] mL(b) volume of 1.35 M calcium chloride that must be diluted with water to prepare 269 mL of a 2.78 10-2 M chloride ion solution [2.77] mL(c) final volume of a 0.0633 M solution prepared by diluting 21.0 mL of 0.155 M lithium carbonate with water [51.4] mL

 Silber4 3.097a.EOCP. Calculate the volume of 2.050 M copper(II) nitrate that must be diluted with water to prepare 750.0 mL of a 0.8543 M solution. (_) 2.400 mL Cu(NO3)2 (_) 366 mL Cu(NO3)2 (o) 312.5 mL Cu(NO3)2 (_) 640.7 mL Cu(NO3)2

 Silber4 3.097b.EOCP. Calculate the volume of 1.03 M calcium chloride that must be diluted with water to prepare 350. mL of a 2.66 10-2 M chloride ion solution. (_) 0.2213 mL CaCl2 (_) 9.039 mL CaCl2 (o) 4.52 mL CaCl2 (_) 18.1 mL CaCl2

 Silber4 3.097c.EOCP. Calculate the final volume of a 0.0700 M solution prepared by diluting 18.0 mL of 0.155 M lithium carbonate with water. (_) 116.1 mL Li2CO3 (_) 257 mL Li2CO3 (o) 39.9 mL Li2CO3 (_) 20.21 mL Li2CO3

 Silber4 3.098.AP. , A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass. (a) What mass of HNO3 is present per liter of solution? [2.77] g(b) What is the molarity of the solution? [15.7] M

 Silber4 3.098a.EOCP. A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass. What mass of HNO3 is present per liter of solution? (_) 496.4 g HNO3 (_) 0.987 g HNO3 (o) 987 g HNO3 (_) 2014 g HNO3

 Silber4 3.098b.EOCP. A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass. What is the molarity of the HNO3 solution? (_) 7.9 M HNO3 (_) 0.016 M HNO3 (o) 15.7 M HNO3 (_) 31.96 M HNO3

 Silber4 3.099a.EOCP. Concentrated sulfuric acid (18.3 M) has a density of 1.84 g/mL. How many moles of sulfuric acid are present per milliliter of solution? (_) 3.4 10-2 mol H2SO4/mL (_) 33.7 mol H2SO4/mL (o) 1.83 10-2 mol H2SO4/mL (_) 1.005 10-1 mol H2SO4/mL

 Silber4 3.099b.EOCP. Concentrated sulfuric acid (18.3 M) has a density of 1.84 g/mL. What is the mass % of H2SO4 in the solution? (_) 1.025 mass % H2SO4 (_) 17.95 mass % H2SO4 (o) 97.6 mass % H2SO4 (_) 0.98 mass % H2SO4

 Silber4 3.100.AP. How many milliliters of 0.55 M HCl are needed to react with 6.9 g of CaCO3?2 HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) [250] mL

 Silber4 3.100.EOCP. How many milliliters of 0.383 M HCl are needed to react with 16.2 g of CaCO3 according to the following reaction? 2 HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) (_) 4 104 mL HCl (_) 0.1240 mL HCl (o) 8.45 102 mL HCl (_) 42.3 mL HCl

 Silber4 3.101.AP. How many grams of NaH2PO4 are needed to react with 43.81 mL of 0.285 M NaOH? NaH2PO4(s) + 2 NaOH(aq) Na3PO4(aq) + 2 H2O(l) [0.749] g

 Silber4 3.101.EOCP. How many grams of NaH2PO4 are needed to react with 38.74 mL of 0.275 M NaOH according to the following reaction? NaH2PO4(s) + 2 NaOH(aq) Na3PO4(aq) + 2 H2O(l) (_) 1.28 g NaH2PO4 (_) 1278 g NaH2PO4 (o) 0.639 g NaH2PO4 (_) 25.6 g NaH2PO4

 Silber4 3.102.AP. How many grams of solid barium sulfate form when 28.5 mL of 0.160 M barium chloride reacts with 63.5 mL of 0.055 M sodium sulfate? Aqueous sodium chloride is the other product. [0.82] g

 Silber4 3.102.EOCP. How many grams of solid barium sulfate form when 25.0 mL of 0.160 M barium chloride reacts with 68.0 mL of 0.055 M sodium sulfate? (Aqueous sodium chloride is the other product). (_) 2.5 g BaSO4 (_) 0.934 g BaSO4 (o) 0.87 g BaSO4 (_) 0.321 g BaSO4

 Silber4 3.103.EOCP. How many moles of which reactant are in excess when 350.0 mL of 0.210 M sulfuric acid reacts with 0.500 L of 0.196 M sodium hydroxide to form water and aqueous sodium sulfate? (_) 4.9 10-2 mol H2SO4 (_) 7.35 10-2 mol H2SO4 (o) 2.45 10-2 mol H2SO4 (_) 9.8 10-2 mol H2SO4

 Silber4 3.104.EOCP. Ordinary household bleach is an aqueous solution of sodium hypochlorite. What is the molarity of a bleach solution that contains 20.5 g of sodium hypochlorite in a total volume of 375 mL? (_) 0.5722 M NaClO (_) 0.27 M NaClO (o) 0.734 M NaClO (_) 7.7 M NaClO

 Silber4 3.105a.EOCP. Muriatic acid, an industrial grade of concentrated HCl, is used to clean masonry and etch cement for painting. Its concentration is 11.7 M. Calculate the volume in milliliters of muriatic acid needed to make 5.0 gallons of 3.5 M acid for routine use (1 gal = 4 qt; 1 qt = 0.946 L). (_) 41 mL muriatic acid (_) 1.50 mL muriatic acid (o) 5.7 103 mL muriatic acid (_) 1.89 104 mL muriatic acid

 Silber4 3.105b.EOCP. Muriatic acid, an industrial grade of concentrated HCl, is used to clean masonry and etch cement for painting. Its concentration is 11.7 M. How many milliliters of the muriatic acid solution contain 9.55 g of HCl? (_) 816 mL muriatic acid (_) 3.1 mL muriatic acid (o) 22.4 mL muriatic acid (_) 4.074 mL muriatic acid

 Silber4 3.106.AP. A sample of impure magnesium was analyzed by allowing it to react with excess HCl solution, as shown below. Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)After 1.69 g of the impure metal was treated with 0.100 L of 0.768 M HCl, 0.0125 mol HCl remained. Assuming the impurities do not react with the acid, what is the mass % Mg in the sample? [46.3]%

 Silber4 3.106.EOCP. A sample of impure magnesium was analyzed by allowing it to react with excess HCl solution according to the following reaction: Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g) After 1.32 g of the impure metal was treated with 0.100 L of 0.750 M HCl, 0.0125 mol of HCl remained. Assuming the impurities do not react with the acid, what is the mass % Mg in the sample? (o) 57.5 mass % Mg (_) 6.25 mass % Mg (_) 1.51 mass % Mg (_) 76.0 mass % Mg

 Silber4 3.108.AP. , The study of sulfur-nitrogen compounds is an active area of chemical research, made more so by the discovery in the early 1980s of one such compound that conducts electricity like a metal. The first sulfur-nitrogen compound was prepared in 1835 and serves today as a reactant for preparing many of the others. Mass spectrometry of the compound shows a molar mass of 184.27 g/mol, and analysis shows it to contain 2.288 g of S for every 1.000 g of N. What is its molecular formula? (Type your answer using the format CO2 for CO2.) [S4N4]

 Silber4 3.108.EOCP. The study of sulfur-nitrogen compounds is an active area of chemical research, made more so by the discovery in the early 1980s of one such compound that conducts electricity like a metal. The first sulfur-nitrogen compound was prepared in 1835 and serves today as a reactant for preparing many of the others. Mass spectrometry of the compound shows a molar mass of 184.27 g/mol, and analysis shows it to contain 2.288 g of S for every 1.000 g of N. What is its molecular formula? (o) S4N4 (_) S3N2 (_) S2N3 (_) S6N6

 Silber4 3.109.EOCP. Narceine is a narcotic in opium. It crystallizes from water solution as a hydrate that contains 10.8 mass % water. If the molar mass of narceine hydrate is 499.52 g/mol, determine x in narceine · xH2O. (o) 3 (_) 2 (_) 5 (_) 6

Silber4 3.110.AP. ,
Hydrogen-containing fuels have a "fuel value" based on their mass % H. Rank the following compounds from highest mass % H to lowest: ethane, propane, benzene, ethanol, cetyl palmitate (whale oil, C32H64O2).

 ethane ---Select---1 (lowest mass)2345 (highest mass)[ 1 (lowest mass) ] propane ---Select---1 (lowest mass)2345 (highest mass)[ 2 ] benzene ---Select---1 (lowest mass)2345 (highest mass)[ 5 (highest mass) ] ethanol ---Select---1 (lowest mass)2345 (highest mass)[ 4 ] cetyl palmitate ---Select---1 (lowest mass)2345 (highest mass)[ 3 ]

 Silber4 3.110.EOCP. Hydrogen-containing fuels have a "fuel value" based on their mass % H. Which of the following compounds contains the highest mass % H? (o) ethane (_) propane (_) benzene (_) ethanol

 Silber4 3.111.AP. , Serotonin ( = 176 g/mol) is a compound that conducts nerve impulses in brain and muscle. It contains 68.2 mass % C, 6.86 mass % H, 15.9 mass % N, and 9.08 mass % O. What is its molecular formula? (Type your answer using the format CH4 for CH4.) [C10H12N2O]

 Silber4 3.111.EOCP. Serotonin (molar mass = 176 g/mol) is a compound that conducts nerve impulses in brain and muscle. It contains 68.2 mass % C, 6.86 mass % H, 15.9 mass % N, and 9.08 mass % O. What is its molecular formula? (o) C10H12N2O (_) C20H30N3O3 (_) C12H10NO2 (_) C5H6NO2

 Silber4 3.112.AP. , Convert the following descriptions of reactions into balanced equations. (Type your answer using the format CO2 for CO2. Use the lowest possible coefficients.) (a) In a gaseous reaction, hydrogen sulfide burns in oxygen to form sulfur dioxide and water vapor. [2] [H2S](g) + [3]O2(g) [2] [SO2](g) + [2]H2O(g)(b) When crystalline potassium chlorate is heated to just above its melting point, it reacts to form two different crystalline compounds, potassium chloride and potassium perchlorate. [4] [KClO3](s) [1]KCl(s) + [3] [KClO4](s) (c) When hydrogen gas is passed over powdered iron(III) oxide, iron metal and water vapor form. [3] [H2](g) + [1] [Fe2O3](s) [2] [Fe](s) + [3] [H2O](g) (d) The combustion of gaseous ethane in air forms carbon dioxide and water vapor. [2] [C2H6](g) + [7]O2(g) [4] [CO2](g) + [6]H2O(g) (e) Iron(II) chloride can be converted to iron(III) fluoride by treatment with chlorine trifluoride gas. Chlorine gas is also formed. [2] [FeCl2](s) + [2] [ClF3](g) [2] [FeF3](s) + [3] [Cl2](g)

 Silber4 3.112a.EOCP. Convert the following description of the reaction into a balanced equation. In a gaseous reaction, hydrogen sulfide burns in oxygen to form sulfur dioxide and water vapor. (_) 2 H2S(s) + O2(g) 2 SO2(g) + 2 H2O(g) (_) 2 HS(s) + O2(g) S2O(g) + H2O(g) (o) 2 H2S(s) + 3 O2(g) 2 SO2(g) + 2 H2O(g) (_) 4 HS(s) + 5 O2(g) 4 SO2(g) + 2 H2O(g)

 Silber4 3.112b.EOCP. Convert the following description of the reaction into a balanced equation. When crystalline potassium chlorate is heated to just above its melting point, it reacts to form two different crystalline compounds, potassium chloride and potassium perchlorate. (_) 2 KClO(s) KCl(s) + KClO2(s) (_) 6 KClO4(s) 3 KCl(s) + 3 KClO3(s) (o) 4 KClO3(s) KCl(s) + 3 KClO4(s) (_) 2 KClO3(s) KCl(s) + KClO4(s)

 Silber4 3.112c.EOCP. Convert the following description of the reaction into a balanced equation. When hydrogen gas is passed over powdered iron(III) oxide, iron metal and water vapor form. (_) 3 H2(g) + Fe2O3(s) Fe2(s) + 3 H2O(g) (_) 3 H2(g) + 2 Fe2O3(s) 2 Fe(s) + 3 H2O(g) (o) 3 H2(g) + Fe2O3(s) 2 Fe(s) + 3 H2O(g) (_) 6 H(g) + Fe3O2(s) 3 Fe(s) + 3 H2O(g)

 Silber4 3.112d.EOCP. Convert the following description of the reaction into a balanced equation. The combustion of gaseous ethane in air forms carbon dioxide and water vapor. (_) C3H8(g) + 2 O2(g) 3 CO2(g) + 4 H2O(g) (_) 2 C2H6(g) + 4 O2(g) 4 CO2(g) + 2 H2O(g) (o) 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) (_) CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

 Silber4 3.112e.EOCP. Convert the following description of the reaction into a balanced equation. Iron(II) chloride can be converted to iron(III) fluoride by treatment with chlorine trifluoride gas. Chlorine gas is also formed. (_) FeCl2(s) + ClF3(g) FeF3(s) + 3 Cl (g) (_) Fe3Cl2(s) + 4 ClF3(g) Fe3F3(s) + 3 Cl2(g) (o) 2 FeCl2(s) + 2 ClF3(g) 2 FeF3(s) + 3 Cl2(g) (_) FeCl2(s) + ClF3(g) FeF3(s) + Cl2(g)

 Silber4 3.113.AP. , Isobutylene is a hydrocarbon used in the manufacture of synthetic rubber. When 0.847 g of isobutylene was analyzed by combustion (using an apparatus similar to that of Figure 3.5), the gain in mass of the CO2 absorber was 2.657 g and that of the H2O absorber was 1.089 g. What is the empirical formula of isobutylene? (Type your answer using format CH4 for CH4.) [CH2] Figure 3.5

 Silber4 3.113.EOCP. Isobutylene is a hydrocarbon used in the manufacture of synthetic rubber. When 0.847 g of isobutylene was analyzed by combustion (using an apparatus similar to that of Figure 3.4 in the text), the gain in mass of the CO2 absorber was 2.657 g and that of the H2O absorber was 1.089 g. What is the empirical formula of isobutylene? (_) C4H8 (_) C4H10 (o) CH2 (_) CH

 Silber4 3.114.AP. One of the compounds used to increase the octane rating of gasoline is toluene (below). Suppose 19.9 mL toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air.(a) How many grams of oxygen are needed for complete combustion of the toluene? [53.9] g(b) How many total moles of gaseous products form? [2.06] mol(c) How many molecules of water vapor form? [4.51e+23] molecules

 Silber4 3.114a.EOCP. One of the compounds used to increase the octane rating of gasoline is toluene (below). Suppose 15.0 mL of toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air. How many grams of oxygen are needed for complete combustion of the toluene? (_) 5.21 g O2 (_) 4.5 g O2 (o) 40.6 g O2 (_) 49.81 g O2

 Silber4 3.114b.EOCP. One of the compounds used to increase the octane rating of gasoline is toluene (below). Suppose 15.0 mL of toluene (d = 0.867 g/mL) is consumed when a sample of gasoline burns in air. How many total moles of gaseous products form? (_) 11 mol gaseous products (_) 0.141 mol gaseous products (o) 1.55 mol gaseous products (_) 0.987 mol gaseous products

 Silber4 3.115.EOCP. The smelting of ferric oxide to form elemental iron occurs at high temperatures in a blast furnace through a reaction sequence with carbon monoxide. In the first step, ferric oxide reacts with carbon monoxide to form Fe3O4. This substance reacts with more carbon monoxide to form iron(II) oxide, which reacts with still more carbon monoxide to form molten iron. Carbon dioxide is also produced in each step. Write an overall balanced equation for the iron-smelting process. (_) 3 Fe2O3 + CO 2 Fe3O4 + CO2 (_) 2 Fe3O4 + 2CO 6 FeO + 2 CO2 (o) Fe2O3 + 3 CO 2 Fe + 3 CO2 (_) 6 FeO + 6 CO 6 Fe + 9 CO2

Silber4 3.116.AP.
During studies of the following reaction (i), a chemical engineer measured a less-than-expected yield of N2 and discovered that the following side reaction (ii) occurs.
 (i) N2O4(l) + 2 N2H4(l) 3 N2(g) + 4 H2O(g) (ii) 2 N2O4(l) + N2H4(l) 6 NO(g) + 2 H2O(g)
In one experiment 13.3 g of NO formed when 101.7 g of each reactant was used. What is the highest percent yield of N2 that can be expected?
[86.6]%

 Silber4 3.116.EOCP. During studies of the reaction shown below: N2O4(l) + 2 N2H4(l) 3 N2(g) + 4 H2O(g) a chemical engineer measured a less-than-expected yield of N2 and discovered that the following side reaction occurs: 2 N2O4(l) + N2H4(l) 6 NO(g) + 2 H2O(g) In one experiment, 10.0 g of NO formed when 100.0 g of each reactant was used. What is the highest percent yield of N2 that can be expected? (_) 97.6% N2 (_) 32.61% N2 (o) 89.8% N2 (_) 29.28% N2

 Silber4 3.117.EOCP. A mathematical equation useful for dilution calculations is Mdil Vdil = Mconc Vconc. This equation works because the quantity of the solution remains the same. (_) True (o) False

 Silber4 3.118.AP. The following boxes represent a chemical reaction between AB2 and B2. (a) Write a balanced equation for the reaction. (Type your answer using the format CO2 for CO2. Use the lowest possible coefficients.) [2]AB2 + [1]B2 [2] [AB3] (b) What is the limiting reactant in this reaction? [AB2] (c) How many moles of product can be made from 2.8 mol B2 and 5.6 mol AB2? [5.6] mol (d) How many moles of excess reactant remain after the reaction in part (c)? [0] mol

 Silber4 3.118a.EOCP. The boxes below represent a chemical reaction between AB2 and B2. Give the balanced equation for the reaction. (_) AB2 + B2 AB3 (_) AB2 + B2 AB3 + 2 B (o) 2 AB2 + B2 2 AB3 (_) 6 AB2 + 5 B2 6 AB3 + 2 B2

 Silber4 3.118b.EOCP. The boxes below represent a chemical reaction between AB2 and B2. What is the limiting reactant in this reaction? (_) AB3 (_) B (o) AB2 (_) B2

 Silber4 3.118c.EOCP. The boxes below represent a chemical reaction between AB2 and B2. How many moles of AB3 can be made from 3.0 mol of B2 and 5.0 mol of AB2? (_) 3.0 mol AB3 (_) 2.0 mol AB3 (o) 5.0 mol AB3 (_) 6.0 mol AB3

 Silber4 3.119.AP. Calculate each of the following quantities. (a) volume of 16.4 M sulfuric acid that must be added to water to prepare 2.00 L f a 0.329 M solution [0.0401] L (b) molarity of the solution obtained by diluting 81.5 mL of 0.250 M ammonium chloride to 0.250 L [0.0815] M (c) volume of water added to 0.150 L of 0.0284 M sodium hydroxide to obtain a 0.0100 M solution (assume the volumes are additive at these low concentrations) [0.276] L (d) mass of calcium nitrate in each milliliter of a solution prepared by diluting 52.6 mL of 0.772 M calcium nitrate to a final volume of 0.100 L [0.0666] g

 Silber4 3.119a.EOCP. Calculate the volume of 18.0 M sulfuric acid that must be added to water to prepare 2.00 L of a 0.309 M solution. (_) 0.29 L (_) 1.16 L (o) 0.0343 L (_) 2.781 L

 Silber4 3.119b.EOCP. Calculate the molarity of the solution obtained by diluting 80.6 mL of 0.225 M ammonium chloride to 0.250 L. (_) 0.70 M (_) 1.433 M (o) 0.0725 M (_) 13.8 M

 Silber4 3.119c.EOCP. Calculate the volume of water added to 0.150 L of 0.0262 M sodium hydroxide to obtain a 0.0100 M solution (assume the volumes are additive at these low concentrations). (_) 0.543 L water (_) 0.336 L water (o) 0.243 L water (_) 0.393 L water

 Silber4 3.119d.EOCP. Calculate the mass of calcium nitrate in each milliliter of a solution prepared by diluting 64.0 mL of 0.745 M calcium nitrate to a final volume of 0.100 L (_) 78.28 g Ca(NO3)2 (_) 1.164 g Ca(NO3)2 (o) 0.0783 g Ca(NO3)2 (_) 0.477 g Ca(NO3)2

 Silber4 3.120.EOCP. Agricultural biochemists use 6-benzylaminopurine (C12H11N5) in trace amounts as a plant growth regulator. In a typical application, 150. mL of a solution contains 0.030 mg of the compound. What is the molarity of the solution? (_) 4.5 10-2 M C12H11N5 (_) 8.9 10-4 M C12H11N5 (o) 8.9 10-7 M C12H11N5 (_) 2.0 10-8 M C12H11N5

 Silber4 3.121.AP. One of Germany's largest chemical manufacturers is building a new plant to produce 3.60 108 lb vinyl acetate per year. This compound (below) is used to make some of the polymers in adhesives, paints, fabric coatings, floppy disks, plastic films, and so on. Assuming production goals are met, how many moles of vinyl acetate will the plant produce each month? [1.58e+08] mol

 Silber4 3.121.EOCP. One of Germany's largest chemical manufacturers has built a plant to produce 3.74 108 lb of vinyl acetate per year. This compound (below) is used to make some of the polymers in adhesives, paints, fabric coatings, floppy disks, plastic films, and so on. Assuming production goals are met, how many moles of vinyl acetate will the plant produce each month? (_) 3.630 105 mol vinyl acetate each month (_) 4.34 106 mol vinyl acetate each month (o) 1.64 108 mol vinyl acetate each month (_) 1.970 109 mol vinyl acetate each month

 Silber4 3.122a.EOCP. Seawater is approximately 4.0% by mass dissolved ions. About 85% of the mass of the dissolved ions is from NaCl. Calculate the percent by mass of NaCl in seawater. (_) 0.047% NaCl (_) 21.2% NaCl (o) 3.4% NaCl (_) 0.034% NaCl

 Silber4 3.122b.EOCP. Seawater is approximately 4.0% by mass dissolved ions. About 85% of the mass of the dissolved ions is from NaCl. Calculate the percent by mass of Na+ ions in seawater. (_) 0.078% (_) 0.00086% (o) 1.3% (_) 0.034%

 Silber4 3.122c.EOCP. Seawater is approximately 4.0% by mass dissolved ions. About 85% of the mass of the dissolved ions is from NaCl. Calculate the percent by mass of Cl- ions in seawater. (_) 5.6% (_) 0.00021% (o) 2.1% (_) 0.034%

 Silber4 3.122d.EOCP. Seawater is approximately 4.0% by mass dissolved ions. About 85% of the mass of the dissolved ions is from NaCl. Calculate the molarity of NaCl in seawater at 15°C. (d of seawater at 15°C = 1.025g/mL) (_) 0.00060 M (_) 0.0019 M (o) 0.60 M (_) 0.70 M

 Silber4 3.123a.EOCP. A mole of one substance has the same number of atoms as a mole of any other substance. (_) True (o) False

 Silber4 3.123b.EOCP. The theoretical yield for a reaction is based on the balanced chemical equation. (o) True (_) False

 Silber4 3.123c.EOCP. To prepare 1.00 L of 3.00 M NaCl, weigh 175.5 g of NaCl and dissolve it in 1.00 L of distilled water. (_) True (o) False

 Silber4 3.123d.EOCP. The concentration of a solution is an intensive property, but the amount of solute in a solution is an extensive property. (o) True (_) False

 Silber4 3.124a.EOCP. Box A represents one unit volume of solution A. Which box represents one unit volume after adding enough solvent to solution A to triple its volume? (_) Box B (_) not enough information (o) Box C (_) Box D

 Silber4 3.124b.EOCP. Box A represents one unit volume of solution A. Which box represents one unit volume after adding enough solvent to solution A to double its volume? (_) Box C (_) not enough information (o) Box B (_) Box D

 Silber4 3.124c.EOCP. Box A represents one unit volume of solution A. Which box represents one unit volume after adding enough solvent to solution A to quadruple its volume? (_) Box B (_) not enough information (o) Box D (_) Box C

 Silber4 3.125a.EOCP. Choose the larger of the following quantities. Number of entities: 0.4 mol of O3 molecules or 0.4 mol of O atoms (_) 0.4 mol of O3 molecules (_) not enough information to decide to decide (o) both quantities are equal (_) 0.4 mol of O atoms

 Silber4 3.125b.EOCP. Choose the larger of the following quantities. mass: 0.4 mol of O3 molecules or 0.4 mol of O atoms (_) 0.4 mol of O atoms (_) not enough information (o) 0.4 mol of O3 molecules (_) both quantities are equal

 Silber4 3.125c.EOCP. Choose the larger of the following quantities. number of moles: 4.0 g of N2O4 or 3.3 g of SO2 (_) 4.0 g of N2O4 (_) not enough information to decide (o) 3.3 g of SO2 (_) both quantities are equal

 Silber4 3.125d.EOCP. Choose the larger of the following quantities. mass: 0.6 mol of C2H4 or 0.6 mol of F2 (_) 0.6 mol of C2H4 (_) not enough information to decide (o) 0.6 mol of F2 (_) both quantities are equal

 Silber4 3.125e.EOCP. Choose the larger of the following quantities. total number of ions: 2.3 mol of sodium chlorate or 2.2 mol of magnesium chloride (_) 2.3 mol of sodium chlorate (_) not enough information (o) 2.2 mol of magnesium chloride (_) both quantities are equal

 Silber4 3.125f.EOCP. Choose the larger of the following quantities. number of molecules: 1.0 g of H2O or 1.0 g of H2O2 (_) 1.0 g of H2O2 (_) not enough information (o) 1.0 g of H2O (_) both quantities are equal

 Silber4 3.125g.EOCP. Choose the larger of the following quantities. number of Na+ ions: 0.500 L of 0.500 M NaBr or 0.0146 kg of NaCl (_) 0.500 L of 0.500 M NaBr (_) not enough information to decide (o) both quantities are equal (_) 0.0146 kg of NaCl

 Silber4 3.125h.EOCP. Choose the larger of the following quantities. mass: 6.02 1023 atoms of 235U or 6.02 1023 atoms of 238U (_) 6.02 1023 atoms of 235U (_) not enough information (o) 6.02 1023 atoms of 238U (_) both quantities are equal

 Silber4 3.126.EOCP. Balance the equation for the reaction between solid tetraphosphorus trisulfide and oxygen gas to form solid tetraphosphorus decaoxide and gaseous sulfur dioxide. (_) 2 P3S3(s) + 16 O2(g) 2 P3O10(s) + 6 SO2(g) (_) P3S3(s) + 5 O2(g) P3O10(s) + 3 SO2(g) (o) P4S3(s) + 8 O2(g) P4O10(s) + 3 SO2(g) (_) P4S3(s) + 5 O2(g) P4O10(s) + 3 SO2(g)

 Silber4 3.127.AP. Hydrogen gas has been suggested as a clean fuel because it produces only water vapor when it burns. If the reaction has a 98.8% yield, what mass of hydrogen forms 77.1 kg of water? [8.73] kg

 Silber4 3.127.EOCP. Hydrogen gas has been suggested as a clean fuel because it produces only water vapor when it burns. If the reaction has a 98.8% yield, what mass of hydrogen forms 85.0 kg of water? (_) 170. kg H2 (_) 4.77 kg H2 (o) 9.62 kg H2 (_) 9.509 kg H2

 Silber4 3.128.EOCP. Assuming that the volumes are additive, what is the concentration of KBr in a solution prepared by mixing 0.200 L of 0.053 M KBr with 0.550 L of 0.078 M KBr? (_) 0.0405 M KBr (_) 0.054 M KBr (o) 0.071 M KBr (_) 0.0320 M KBr

 Silber4 3.129a.EOCP. Solar winds composed of free protons, electrons, and particles, bombard Earth constantly, knocking gas molecules out of the atmosphere. In this way, Earth loses 3.0 kg of matter per second. It is estimated that the atmosphere will be gone in about 50 billion years. Use this estimate to calculate the mass (kg) of Earth's atmosphere. (_) 1.5 1012 kg (_) 1.6 103 kg (o) 4.7 1018 kg (_) 7.9 107 kg

 Silber4 3.129b.EOCP. Solar winds composed of free protons, electrons, and particles, bombard Earth constantly, knocking gas molecules out of the atmosphere. In this way, Earth loses 3.0 kg of matter per second. It is estimated that the atmosphere will be gone in about 50 billion years. Use this estimate to calculate the amount (mol) of nitrogen, which makes up 75.5% of the atmosphere. (_) 4.5 1020 mol (_) 2.5 1018 mol (o) 2.5 1020 mol (_) 3.6 1019 mol

 Silber4 3.130.AP. Calculate each of the following quantities. (a) moles of compound in 0.580 g ammonium bromide [0.00592] mol (b) number of potassium ions in 59.9 g potassium nitrate [3.57e+23] ions (c) mass in grams of 5.77 mol glycerol (C3H8O3) [531] g (d) volume of 2.35 mol of glycerol (CHCl3; d=1.48 g/mL) [1.90e+02] mL (e) number of sodium ions in 3.65 mol sodium carbonate [4.40e+24] ions (f) number of atoms in 10.0 µg of cadmium [5.36e+15] atoms (g) number of atoms in 0.0015 mol fluorine gas [1.8e+21] atoms

 Silber4 3.130a.EOCP. Calculate the moles of compound in 0.588 g of ammonium bromide. (_) 57.6 mol NH4Br (_) 6.07 10-3 mol NH3Br (o) 6.00 10-3 mol NH4Br (_) 57.0 mol NH3Br

 Silber4 3.130b.EOCP. Calculate the number of potassium ions in 68.5 g of potassium nitrate. (_) 4.8 1023 K+ ions (_) 4.12 1023 K+ ions (o) 4.08 1023 K+ ions (_) 4.2 1027 K+ ions

 Silber4 3.130c.EOCP. Calculate the mass in grams of 5.85 mol of glycerol (C3H8O3). (_) 15.7 g C3H8O3 (_) 0.0635 g C3H8O3 (o) 539 g C3H8O3 (_) 92.09 g C3H8O3

 Silber4 3.130d.EOCP. Calculate the volume of 2.55 mol of chloroform (CHCl3; d = 1.48 g/mL). (_) 8.1 101 mL CHCl3 (_) 3.045 102 mL CHCl3 (o) 2.06 102 mL CHCl3 (_) 4.51 102 mL CHCl3

 Silber4 3.130e.EOCP. Calculate the number of sodium ions in 2.11 mol of sodium carbonate. (_) 6.4 1023 Na+ ions (_) 1.27 1024 Na+ ions (o) 2.54 1024 Na+ ions (_) 1.20 1024 Na+ ions

 Silber4 3.130f.EOCP. Calculate the number of atoms in 10.0 µg of cadmium. (_) 5.36 1019 Cd atoms (_) 5.36 1022 Cd atoms (o) 5.36 1016 Cd atoms (_) 5.36 1020 Cd atoms

 Silber4 3.130g.EOCP. Calculate the number of atoms in 0.0015 mol of fluorine gas. (_) 4.52 1020 F atoms (_) 9.03 1020 F atoms (o) 1.8 1021 F atoms (_) 1.81 1024 F atoms

 Silber4 3.131.AP. Elements X (green) and Y (purple) react according to the following equation. X2 + 3 Y2 2 XY3 Which molecular scene represents the product of the reaction? ---Select---ABCD[ C ]

 Silber4 3.131.EOCP. Elements X (green) and Y (purple) react according to the following equation: X2 + 3 Y2 2 XY3. Which molecular scene represents the product of the reaction? (_) Scene A (_) Scene B (o) Scene C (_) Scene D

 Silber4 3.132.EOCP. Hydrocarbon mixtures are used as fuels. How many grams of CO2(g) are produced by the combustion of 200. g of a mixture that is 25.0% CH4 and 75.0% C3H8 by mass? (o) 586 g CO2 (_) 102 g CO2 (_) 312 g CO2 (_) 414 g CO2

 Silber4 3.134.AP. , Nitrogen (N), phosphorus (P), and potassium (K) are the main nutrients in fertilizers. According to an industry convention, the numbers on the label refer to the mass percents of N, P2O5, and K2O, in that order. Calculate the N : P : K ratio of a 30 : 10 : 10 fertilizer in terms of moles of each element, and express it as x : y : 1.0. [10] : [0.67] : 1.0

 Silber4 3.134.EOCP. Nitrogen (N), phosphorus (P), and potassium (K) are the main nutrients in plant fertilizers. According to an industry convention, the numbers on the label refer to the mass percents of N, P2O5, and K2O, in that order. Calculate the N:P:K ratio of a 30:10:10 fertilizer in terms of moles of each element, and express it as x:y:1.0. (o) 10 : 0.67 : 1.0 (_) 2.1 : 0.14 : 1.0 (_) 3.0 : 1.0 : 1.0 (_) 0.14 : 0.21 : 1.0

 Silber4 3.135.EOCP. A 0.652 g sample of a pure strontium halide reacts with excess sulfuric acid, and the solid strontium sulfate formed is separated, dried, and found to weigh 0.755 g. What is the formula of the original halide? (o) SrCl2 (_) SrBr2 (_) SrF2 (_) SrI2

 Silber4 3.136.EOCP. Methane and ethane are the two simplest hydrocarbons. What is the mass % C in a mixture that is 40.0% methane and 60.0% ethane by mass? (_) 17.9 mass % C (o) 77.9 mass % C (_) 30.0 mass % C (_) 47.9 mass % C

 Silber4 3.137.EOCP. When carbon-containing compounds are burned in a limited amount of air, some CO(g) as well as CO2(g) is produced. A gaseous product mixture is 35.0 mass % CO and 65.0 mass % CO2. What is the mass % C in the mixture? (_) 15.0 mass % C (o) 32.7 mass % C (_) 17.7 mass % C (_) 2.7 mass % C

 Silber4 3.138.EOCP. Ferrocene, first synthesized in 1951, was the first organic iron compound with direct Fe-C bonds. An understanding of ferrocene's structure gave rise to new ideas about chemical bonding and led to the preparation of many useful compounds. In the combustion analysis of ferrocene, which contains only Fe, C, and H, a 0.9437 g sample produced 2.233 g of CO2 and 0.457 g of H2O. What is the empirical formula of ferrocene? (_) CHFe (o) C10H10Fe (_) C5H10Fe (_) CHFe2

 Silber4 3.139.AP. Citric acid (below) is concentrated in citrus fruits and plays a central metabolic role in nearly every animal and plant cell. (a) What are the molar mass and formula of citric acid? molar mass [192] g/mol formula (Type your answer using the format C6H11O6 for C6H11O6.) [C6H8O7](b) How many moles of citric acid are in 2.35 qt of lemon juice (d = 1.09 g/mL) that is 5.78% citric acid by mass? [0.729] mol

 Silber4 3.139b.EOCP. Citric acid (below) is concentrated in citrus fruits and plays a central metabolic role in nearly every animal and plant cell. How many moles of citric acid are in 1.50 qt of lemon juice (d = 1.09 g/mL) that is 6.82% citric acid by mass? (_) 105 mol citric acid (o) 0.549 mol citric acid (_) 0.05 mol citric acid (_) 54.9 mol citric acid

 Silber4 3.140a.EOCP. Various nitrogen oxides, as well as oxides of sulfur, contribute to acidic rainfall through complex reaction sequences. Atmospheric nitrogen and oxygen combine to form nitrogen monoxide gas, which reacts with more oxygen to form nitrogen dioxide gas. In contact with water vapor, nitrogen dioxide forms aqueous nitric acid and more nitrogen monoxide. Give the overall balanced equation that does not include nitrogen monoxide and nitrogen dioxide. (_) 4 N2(g) + O2(g) + 4 H2O(l) 8 HNO3(aq) + NO3(g) (o) 2 N2(g) + 5 O2(g) + 2 H2O(l) 4 HNO3(aq) (_) N2(g) + 3 O2(g) 2 HNO3(aq) + H2O(l) (_) 2 N(g) + 3 O2(g) + H2O(l) 2 HNO3(aq)

 Silber4 3.140b.EOCP. Various nitrogen oxides, as well as oxides of sulfur, contribute to acidic rainfall through complex reaction sequences. Atmospheric nitrogen and oxygen combine to form nitrogen monoxide gas, which reacts with more oxygen to form nitrogen dioxide gas. In contact with water vapor, nitrogen dioxide forms aqueous nitric acid and more nitrogen monoxide. How many metric tons (t) of nitric acid form when 1.25 103 t of atmospheric nitrogen is consumed (1 t = 1000 kg)? (_) 5.62 1010 t HNO3 (_) 2.811 103 t HNO3 (_) 5.62 10-4 t HNO3 (o) 5.62 103 t HNO3

 Silber4 3.141a.EOCP. Alum [KAl(SO4)2 · xH2O] is used in food preparation, dye fixation and water purification. A 0.5404 g sample of alum is heated to drive off the waters of hydration. The resulting KAl(SO4)2 weighs 0.2941 g. The value of x in the formula of alum is: (_) 17 (_) 80 (_) 7 (o) 12

 Silber4 3.141b.EOCP. Alum [KAl(SO4)2 · 12H2O] is used in food preparation, dye fixation and water purification. To prepare alum, aluminum is reacted with potassium hydroxide and the product with sulfuric acid. Upon cooling, alum crystallizes from the solution. When 0.7500 g of aluminum is used, 8.500 g of alum forms. The percent yield of this reaction is: (_) 0.5485% (_) 84.38% (_) 13.19% (o) 64.44%

 Silber4 3.142.AP. , When 1.5173 of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.838 g of CO2 and 0.8122 g of H2O were produced. In a separate experiment to determine the mass % of iron, 0.3355 g of the compound yielded 0.0758 g of Fe2O3. What is the empirical formula of the compound? (Type your answer using the format CH4 for CH4.) [C15H21O6Fe]

 Silber4 3.142.EOCP. When 1.5173 g of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.838 g of CO2 and 0.8122 g of H2O were produced. In a separate experiment to determine the mass % of iron, 0.3355 g of the compound yielded 0.0758 g of Fe2O3. What is the empirical formula of the compound? (_) C10HO3Fe5 (_) C5H7O2Fe (_) CHOFe (o) C15H21O6Fe

 Silber4 3.143a.EOCP. Fluorine is so reactive that it forms compounds with materials inert to other treatments. When 0.327 g of platinum is heated in fluorine, 0.519 g of a dark red, volatile solid forms. The empirical formula of this compound is: (_) Pt2F6 (_) Pt6F2 (_) PtF (o) PtF6

 Silber4 3.143b.EOCP. Fluorine is so reactive that it forms compounds with materials inert to other treatments. When 0.265 g of the compound PtF6 reacts with excess xenon gas, 0.378 g of an orange-yellow solid forms. What is the empirical formula of this compound, the first noble gas compound formed? (_) Xe2PtF (_) XePtF12 (_) XePtF (o) XePtF6

 Silber4 3.143b.EOCP. Fluorides of the relatively unreactive noble gas xenon can be formed by direct reaction of the elements at high pressure and temperature. Depending on the temperature and the reactant amounts, the product mixture may include XeF2, XeF4, and XeF6. Under conditions that produce only XeF4 and XeF6, 1.85 10-4 mol of Xe reacted with 5.00 10-4 mol of F2, and 9.00 10-6 mol of Xe was found to be in excess. What is the mass percent of XeF4 in the product? (_) 2.46% XeF4 (_) 84.8% XeF4 (_) 58% XeF4 (o) 14% XeF4

 Silber4 3.143c.EOCP. Fluorides of the relatively unreactive noble gas xenon can be formed by direct reaction of the elements at high pressure and temperature. Depending on the temperature and the reactant amounts, the product mixture may include XeF2, XeF4, and XeF6. Under conditions that produce only XeF4 and XeF6, 1.85 10-4 mol of Xe reacted with 5.00 10-4 mol of F2, and 9.00 10-6 mol of Xe was found to be in excess. What is the mass percent of XeF6 in the product? (_) 97.5% XeF6 (_) 42% XeF6 (_) 15.2% XeF6 (o) 86.2% XeF6

 Silber4 3.144.AP. Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.52 g of hemoglobin. (a) How many grams of heme are in the sample? [0.031] g (b) How many moles of heme? [5.1e-05] mol (c) How many grams of Fe? [0.0028] g (d) How many grams of hemin could be formed for a forensic chemist to measure? [0.033] g

 Silber4 3.144a.EOCP. Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove the heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.45 g of hemoglobin. How many grams of heme are in the sample? (_) 0.0027 g heme (_) 0.00027 g heme (_) 0.27 g heme (o) 0.027 g heme

 Silber4 3.144b.EOCP. Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove the heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.45 g of hemoglobin. How many moles of heme are in the sample? (_) 4.4 10-6 mol heme (_) 4.4 10-7 mol heme (_) 4.4 10-4 mol heme (o) 4.4 10-5 mol heme

 Silber4 3.144c.EOCP. Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove the heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.45 g of hemoglobin. How many grams of Fe are in the sample? (_) 2.4 10-4 g Fe (_) 2.4 10-6 g Fe (_) 2.4 10-5 g Fe (o) 2.4 10-3 g Fe

 Silber4 3.144c.EOCP. Hemoglobin is 6.0% heme (C34H32FeN4O4) by mass. To remove the heme, hemoglobin is treated with acetic acid and NaCl to form hemin (C34H32N4O4FeCl). At a crime scene, a blood sample contains 0.45 g of hemoglobin. How many grams of hemin could be formed for a forensic chemist to measure? (_) 2.9 10-5 g hemin (_) 2.9 10-3 g hemin (_) 2.9 10-4 g hemin (o) 2.9 10-2 g hemin

 Silber4 3.145a.EOCP. Manganese is a key component of extremely hard steel. The element occurs naturally in many oxides. A 542.3 g sample of a manganese oxide mixture has an Mn:O molar ratio of 1.00:1.42 and consists of braunite (Mn2O3) and manganosite (MnO). What is the mass percent of braunite in the ore? (_) 5.31% braunite (_) 21.3% braunite (_) 14.0% braunite (o) 85.4% braunite

 Silber4 3.145b.EOCP. Manganese is a key component of extremely hard steel. The element occurs naturally in many oxides. A 542.3 g sample of a manganese oxide mixture has an Mn:O molar ratio of 1.00:1.42 and consists of braunite (Mn2O3) and manganosite (MnO). What is the mass percent of manganosite in the ore? (_) 78.7% manganosite (_) 86.0% manganosite (_) 94.7% manganosite (o) 14.6% manganosite

 Silber4 3.145c.EOCP. Manganese is a key component of extremely hard steel. The element occurs naturally in many oxides. A 542.3 g sample of a manganese oxide mixture has an Mn:O molar ratio of 1.00:1.42 and consists of braunite (Mn2O3) and manganosite (MnO). What is the molar ratio of Mn3+ to Mn2+ in the ore? (_) 4.00 (_) 17.8 (_) 8.01 (o) 5.25

 Silber4 3.146a.EOCP. Sulfur dioxide gas can be produced by roasting iron pyrite (iron disulfide, FeS2) in oxygen, which yields the gas and solid iron(III) oxide. What mass of iron pyrite is used in the formation of 1.00 kg of sulfur dioxide? (_) 3750 g (_) 7.80 g (_) 870 g (o) 936 g

 Silber4 3.146b.EOCP. Sulfur dioxide gas can be produced by roasting iron pyrite (iron disulfide, FeS2) in oxygen, which yields the gas and solid iron(III) oxide. What mass of oxygen is used in the formation of 1.00 kg of sulfur dioxide? (_) 363 g (_) 21.5 g (_) 499 g (o) 687 g

 Silber4 3.146c.EOCP. Sulfur dioxide gas can be produced by roasting iron pyrite (iron disulfide, FeS2) in oxygen, which yields the gas and solid iron(III) oxide. What mass of iron(III) oxide is produced in the formation of 1.00 kg of sulfur dioxide? (_) 2490 g (_) 62.4 g (_) 3.90 g (o) 623 g

 Silber4 3.147a.EOCP. The human body excretes nitrogen in the form of urea, NH2CONH2. The key biochemical step in urea formation is the reaction of water with arginine to produce urea and ornithine: What is the mass percent of nitrogen in urea? (_) 21.43 mass % N (_) 2.1 mass % N (_) 23.3 mass % N (o) 46.65 mass % N

 Silber4 3.147b.EOCP. The human body excretes nitrogen in the form of urea, NH2CONH2. The key biochemical step in urea formation is the reaction of water with arginine to produce urea and ornithine: What is the mass percent of nitrogen in arginine? (_) 16.1 mass % N (_) 31.09 mass % N (_) 8.04 mass % N (o) 32.17 mass % N

 Silber4 3.147c.EOCP. The human body excretes nitrogen in the form of urea, NH2CONH2. The key biochemical step in urea formation is the reaction of water with arginine to produce urea and ornithine: What is the mass percent of nitrogen in ornithine? (_) 4.71 mass % N (_) 47.17 mass % N (_) 10.6 mass % N (o) 21.20 mass % N

 Silber4 3.147d.EOCP. The human body excretes nitrogen in the form of urea, NH2CONH2. The key biochemical step in urea formation is the reaction of water with arginine to produce urea and ornithine: How many grams of nitrogen can be excreted as urea when 143.2 g of ornithine is produced? (_) 111 g N (_) 50.54 g N (_) 65.1 g N (o) 30.36 g N

 Silber4 3.148a.EOCP. Aspirin (acetylsalicylic acid, C9H8O4) can be made by reacting salicylic acid (C7H6O3) with acetic anhydride [(CH3CO)2O]: C7H6O3(s) + (CH3CO)2O(l) C9H8O4(s) + CH3COOH(l) In one reaction, 3.027 g of salicylic acid and 6.00 mL of acetic anhydride react to form 3.261 g of aspirin. Which is the limiting reactant? (d of acetic anhydride = 1.080 g/mL.) (_) C9H8O4 (_) CH3COOH (_) (CH3CO)2O (o) C7H6O3

 Silber4 3.148b.EOCP. Aspirin (acetylsalicylic acid, C9H8O4) can be made by reacting salicylic acid (C7H6O3) with acetic anhydride [(CH3CO)2O]: C7H6O3(s) + (CH3CO)2O(l) C9H8O4(s) + CH3COOH(l) In one reaction, 3.027 g of salicylic acid and 6.00 mL of acetic anhydride react to form 3.261 g of aspirin. What is the percent yield of aspirin of this reaction? (_) 28.51% (_) 76.67% (_) 26.46% (o) 82.60%

 Silber4 3.148c.EOCP. Aspirin (acetylsalicylic acid, C9H8O4) can be made by reacting salicylic acid (C7H6O3) with acetic anhydride [(CH3CO)2O]: C7H6O3(s) + (CH3CO)2O(l) C9H8O4(s) + CH3COOH(l) What is the percent atom economy of this reaction? (_) 60.05% (_) 25.00% (_) 42.50% (o) 75.00%

 Silber4 3.149.EOCP. The rocket fuel hydrazine (N2H4) is manufactured by the Raschig process, a three-step reaction with the following overall equation: NaOCl(aq) + 2 NH3(aq) N2H4(aq) + NaCl(aq) + H2O(l) What is the percent atom economy of this process? (_) 53.86% (_) 16.60% (_) 18.59% (o) 29.54%

 Silber4 3.150.EOCP. Lead(II) chromate (PbCrO4) is used as a yellow pigment to designate traffic lanes, but has been banned from house paint because of the potential for lead poisoning. The compound is produced from chromite (FeCr2O4), an ore of chromium, by the following reaction. 4 FeCr2O4(s) + 8 K2CO3(aq) + 7 O2(g) 2 Fe2O3(s) + 8 K2CrO4(aq) + 8 CO2(g) Lead(II) ion then replaces K+ ions in a subsequent step. If a yellow paint is 0.511% PbCrO4 by mass, how many grams of chromite are needed per kilogram of paint? (_) 3.5 g FeCr2O4 (_) 1.8 g FeCr2O4 (_) 7.9 g FeCr2O4 (o) 2 g FeCr2O4

 Silber4 3.151a.EOCP. Ethanol (CH3CH2OH), the intoxicant in alcoholic beverages, is also used as a precursor of many other organic compounds. In concentrated sulfuric acid, ethanol forms diethyl ether: 2 CH3CH2OH(l) CH3CH2OCH2CH3(l) + H2O(g) In a side reaction, some ethanol forms ethylene: CH3CH2OH(l) CH2=CH2(g) + H2O(g) If 50.0 g of ethanol yields 33.9 g of diethyl ether, what is the percent yield of diethyl ether? (_) 42.16% diethyl ether (_) 67.8% diethyl ether (_) 54.26% diethyl ether (o) 84.3% diethyl ether

 Silber4 3.151b.EOCP. Ethanol (CH3CH2OH), the intoxicant in alcoholic beverages, is also used as a precursor of many other organic compounds. In concentrated sulfuric acid, ethanol forms diethyl ether: 2 CH3CH2OH(l) CH3CH2OCH2CH3(l) + H2O(g) In a side reaction, some ethanol forms ethylene: CH3CH2OH(l) CH2=CH2(g) + H2O(g) 50.0 g of ethanol yields 33.9 g of diethyl ether. During the process, 50.0% of the ethanol that did not produce diethyl ether reacts by the side reaction. What mass of ethylene is produced? (_) 15.2 g C2H4 (_) 30.4 g C2H4 (_) 4.90 g C2H4 (o) 2.39 g C2H4

 Silber4 3.152a.EOCP. When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms according to the unbalanced reaction: Zn(s) + S8(s) ZnS(s) Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 85.2 g of Zn reacts with 52.4 g of S8, 105.4 g of ZnS forms. What is the percent yield of ZnS? (_) 76.74% ZnS (_) 12.7% ZnS (_) 19.9% ZnS (o) 83.0% ZnS

 Silber4 3.152b.EOCP. When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms according to the unbalanced reaction: Zn(s) + S8(s) ZnS(s) Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 85.2 g of Zn reacts with 52.4 g of S8, 105.4 g of ZnS forms. If all the remaining reactants combine with oxygen, how many grams of zinc oxide form? (_) 24.6 g ZnO (_) 92.37 g ZnO (_) 84.75 g ZnO (o) 18.0 g ZnO

 Silber4 3.152c.EOCP. When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms according to the unbalanced reaction: Zn(s) + S8(s) ZnS(s) Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 85.2 g of Zn reacts with 52.4 g of S8, 105.4 g of ZnS forms. If all the remaining reactants combine with oxygen, how many grams of sulfur dioxide form? (_) 40.84 g SO2 (_) 94.0 g SO2 (_) 88.0 g SO2 (o) 35.6 g SO2

 Silber4 3.153.EOCP. Cocaine (C17H21O4N) is a natural substance found in coca leaves, which have been used for centuries as a local anesthetic and stimulant. Illegal cocaine arrives in the United States either as the pure compound or as the hydrochloride salt (C17H21O4NHCl). At 25°C, the salt is very soluble in water (2.50 kg/L), but cocaine is much less so (1.70 g/L). What is the maximum amount (in g) of the salt that can dissolve in 50.0 mL of water? (_) 12.5 g salt (_) 1250 g salt (_) 1.25 g salt (o) 125 g salt

 Silber4 3.154a.EOCP. High temperature superconducting oxides hold great promise in the utility, transportation, and computer industries. One superconductor is La2-xSrxCuO4. Calculate the molar mass of this oxide when x = 0. (_) 127.55 amu (_) 266.45 amu (_) 492.97 amu (o) 405.35 amu

 Silber4 3.154b.EOCP. High temperature superconducting oxides hold great promise in the utility, transportation, and computer industries. One superconductor is La2-xSrxCuO4. Calculate the molar mass of this oxide when x = 1. (_) 306.07 amu (_) 441.69 amu (_) 492.97 amu (o) 354.07 amu

 Silber4 3.154c.EOCP. High temperature superconducting oxides hold great promise in the utility, transportation, and computer industries. One superconductor is La2-xSrxCuO4. Calculate the molar mass of this oxide when x = 0.163 (this value characterizes the compound with optimum superconducting properties). (_) 405.35 amu (_) 354.07 amu (_) 492.97 amu (o) 396.99 amu

 Silber4 3.154d.EOCP. A common superconducting oxide is made by heating a mixture of barium carbonate, copper(II) oxide, and yttrium(III) oxide, followed by further heating in O2: 4 BaCO3(s) + 6 CuO(s) + Y2O3(s) 2 YBa2Cu3O6.5(s) + 4 CO2(g) 2 YBa2Cu3O6.5(s) + 1/2 O2(g) 2 YBa2Cu3O7(s) When equal masses of the three reactants are heated, which reactant is limiting? (_) Y2O3 (_) CuO (_) YBa2Cu3O7 (o) BaCO3

 Silber4 3.155.EOCP. The zirconium oxalate K2Zr(C2O4)3(H2C2O4) · H2O, was synthesized by mixing 1.60 g of ZrOCl2 · 8 H2O with 5.20 g of H2C2O4 · 2 H2O and an excess of aqueous KOH. After 2 months, 1.20 g of crystalline product was obtained, as well as aqueous KCl and water. The percent yield of this reaction is: (_) 5.37% (_) 21.5% (_) 14.5% (o) 44.6%

 Silber4 3.156.EOCP. How many atoms are in 0.001 g of C? (_) 6 1023 atoms (_) 1 1028 atoms (_) 4 1019 atoms (o) 5 1019 atoms

Silber4 3.FP.01.
 FOLLOW-UP PROBLEM 3.1 Calculating the Mass and Number of Atoms in a Given Number of Moles of an Element
(a) Graphite is the crystalline form of carbon used in lead pencils. How many moles of carbon are there in 335 mg of graphite?
[0.0279] mol

(b) Manganese (Mn) is a transition element essential for the growth of bones. What is the mass in grams of 1.29 1021 Mn atoms, the number found in 4.00 kg of bone.
[0.118] g
 HINTS Getting Started I'm Stuck

 Silber4 3.TB.001. Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass. (_) 99.15 g/mol (o) 78.07 g/mol (_) 118.15 g/mol (_) 50.01 g/mol (_) 59.08 g/mol

 Silber4 3.TB.002. Calculate the molar mass of tetraphosphorus decaoxide, P4O10, a corrosive substance which can be used as a drying agent. (_) 190.97 g/mol (o) 283.89 g/mol (_) 469.73 g/mol (_) 94.97 g/mol (_) 139.88 g/mol

 Silber4 3.TB.003. Calculate the molar mass of rubidium carbonate, Rb2CO3. (_) 255.00 g/mol (o) 230.94 g/mol (_) 340.43 g/mol (_) 113.48 g/mol (_) 145.47 g/mol

 Silber4 3.TB.004. Calculate the molar mass of (NH4)3AsO4. (_) 165.02 g/mol (o) 193.03 g/mol (_) 417.80 g/mol (_) 108.96 g/mol (_) 156.96 g/mol

 Silber4 3.TB.005. Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass. (_) 315.15 g/mol (o) 342.15 g/mol (_) 450.06 g/mol (_) 74.98 g/mol (_) 278.02 g/mol

 Silber4 3.TB.006. Which of the following chemical equations is NOT balanced? (_) H3PO4(aq) + Al(OH)3(s) 3 H2O(l) + AlPO4(s) (o) 3 H2SO4(aq) + 2 Al(OH)3(s) 3 H2O(l) + Al2(SO4)3(aq) (_) 2 NaOH(aq) + H2SO4(aq) Na2SO4(aq) + 2 H2O(l) (_) 2 C6H14O4(s) + 15 O2(g) 14 H2O(g) + 12 CO2(g)

 Silber4 3.TB.006. Calculate the molar mass of Ca(BO2)2 · 6 H2O. (_) 183.79 g/mol (o) 233.79 g/mol (_) 273.87 g/mol (_) 143.71 g/mol (_) 174.89 g/mol

 Silber4 3.TB.007. Magnesium fluoride is used in the ceramics and glass industry. What is the mass of 1.72 mol of magnesium fluoride? (_) 62.3 g (o) 107 g (_) 43.3 g (_) 92.9 g (_) 74.5 g

 Silber4 3.TB.008. Sodium bromate is used in a mixture which dissolves gold from its ores. Calculate the mass in grams of 4.68 mol of sodium bromate. (_) 383 g (o) 706 g (_) 482 g (_) 0.0310 g (_) 32.2 g

 Silber4 3.TB.009. What is the mass in grams of 0.250 mol of the common antacid calcium carbonate? (_) 17.0 g (o) 25.0 g (_) 4.00 102 g (_) 2.50 10-3 g (_) 4.00 10-2 g

 Silber4 3.TB.010. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. (_) 2.32 mol (o) 0.305 mol (_) 3.28 mol (_) 0.200 mol (_) 0.431 mol

 Silber4 3.TB.011. Phosphorus pentachloride, PCl5, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl5. (_) 3.55 mol (o) 0.186 mol (_) 5.38 mol (_) 0.282 mol (_) 0.583 mol

 Silber4 3.TB.012. Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3. (_) 2.146 mol (o) 0.4660 mol (_) 2.377 mol (_) 0.4207 mol (_) 1.105 mol

 Silber4 3.TB.013. Calculate the number of oxygen atoms in 29.34 g of sodium sulfate, Na2SO4. (_) 2.409 1024 O atoms (o) 4.976 1023 O atoms (_) 1.244 1023 O atoms (_) 1.166 1025 O atoms (_) 2.915 1024 O atoms

 Silber4 3.TB.014. Potassium dichromate, K2Cr2O7, is used in tanning leather, decorating porcelain and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K2Cr2O7. (_) 2.248 1024 Cr atoms (o) 3.227 1023 Cr atoms (_) 9.490 1025 Cr atoms (_) 1.613 1023 Cr atoms (_) 1.124 1024 Cr atoms

 Silber4 3.TB.015. Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 1020 molecules of SO3. (_) 2.91 10-2 g (o) 4.85 10-2 g (_) 6.06 10-4 g (_) 1650 g (_) 20.6 g

 Silber4 3.TB.016. Calculate the mass in grams of 8.35 1022 molecules of CBr4. (_) 0.139 g (o) 46.0 g (_) 0.0217 g (_) 12.7 g (_) 7.21 g

 Silber4 3.TB.017. What is the number of hydrogen atoms in 0.050 mol of C3H8O3? (_) 1.2 1023 H atoms (o) 2.4 1023 H atoms (_) 3.0 1022 H atoms (_) none of these (_) 4.8 1023 H atoms

 Silber4 3.TB.018. Copper(II) sulfate pentahydrate, CuSO4 · 5 H2O, is used as a fungicide and algicide. Calculate the mass of oxygen in 1.000 mol of CuSO4 · 5 H2O. (_) 96.00 g (o) 144.0 g (_) 249.7 g (_) 64.00 g (_) 80.00 g

 Silber4 3.TB.019. Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO3)2. (_) 90.8 g (o) 87.0 g (_) 107 g (_) 62.6 g (_) 83.4 g

 Silber4 3.TB.020. Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass? (_) 33.3% (o) 42.1% (_) 26.7% (_) 52.8% (_) 41.4%

 Silber4 3.TB.021. Gadolinium oxide, a colorless powder which absorbs carbon dioxide from the air, contains 86.76 mass % Gd. Determine its empirical formula. (_) Gd3O4 (o) Gd2O3 (_) Gd3O2 (_) GdO (_) Gd4O3

 Silber4 3.TB.022. Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. Determine its empirical formula. (_) HN6O16 (o) H2NO2 (_) HNO (_) H2NO3 (_) HN16O7

 Silber4 3.TB.023. Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula? (_) N3H3O3 (o) N2H4O4 (_) NH2O5 (_) N2H2O4 (_) N4H8O2

 Silber4 3.TB.024. A compound of bromine and fluorine is used to make UF6, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula. (_) BrF2 (o) BrF3 (_) BrF (_) Br3F (_) Br2F3

 Silber4 3.TB.025. A compound containing chromium and silicon contains 73.52 mass percent chromium. Determine its empirical formula. (_) Cr3Si (_) Cr2Si3 (_) CrSi3 (_) Cr2S (o) Cr3Si2

 Silber4 3.TB.026. Alkanes are compounds of carbon and hydrogen with the general formula CnH2n + 2. An alkane component of gasoline has a molar mass of between 125 and 130 g/mol. What is the value of n for this alkane? (_) 13 (_) 10 (_) 4 (_) 14 (o) 9

 Silber4 3.TB.027. Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. What is its empirical formula? (_) C5H12O4 (_) C3H4O2 (_) C2H3O4 (_) C2H2O (o) C4H3O2

 Silber4 3.TB.028. Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. If its molar mass is between 158 and 167 g/mol, what is its molecular formula? (_) C7H12O4 (_) C6H8O5 (_) C4H6O7 (_) C4H3O2 (o) C8H6O4

 Silber4 3.TB.029. Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula? (_) HN3O4Cl9 (_) H2N2O2Cl (_) H2N7O8Cl18 (_) H4NOCl2 (o) H4NOCl

 Silber4 3.TB.030. In the combustion analysis of 0.1127 g of glucose (C6H12O6), what mass, in grams, of CO2 would be produced? (_) 0.4132 g (_) 0.0825 g (_) 0.0451 g (_) 1.466 g (o) 0.1652 g

 Silber4 3.TB.031. Balance the following equation: B2O3(s) + HF(l) BF3(g) + H2O(l). (_) B2O3(s) + 3 HF(l) 2 BF3(g) + 3 H2O(l) (_) B2O3(s) + 2 HF(l) 2 BF3(g) + H2O(l) (_) B2O3(s) + H6F6(l) B2F6(g) + H6O3(l) (_) B2O3(s) + 6 HF(l) 2 BF3(g) + 6 H2O(l) (o) B2O3(s) + 6 HF(l) 2 BF3(g) + 3 H2O(l)

 Silber4 3.TB.032. Balance the following equation: UO2(s) + HF(l) UF4(s) + H2O(l). (_) UO2(s) + 4 HF(l) UF4(s) + 4 H2O(l) (_) UO2 (s) + H4F4(l) UF4 (s) + H4O2(l) (_) UO2(s) + 2 HF(l) UF4(s) + H2O(l) (_) UO2(s) + 8 HF(l) 2 UF4(s) + 4 H2O(l) (o) UO2(s) + 4 HF(l) UF4(s) + 2 H2O(l)

 Silber4 3.TB.033. Balance the following equation for the combustion of benzene: C6H6(l) + O2(g) H2O(g) + CO2(g). (_) C6H6(l) + 15 O2(g) 3 H2O(g) + 6 CO2(g) (_) C6H6(l) + 9 O2(g) 6 H2O(g) + 6 CO2(g) (_) C6H6(l) + 9 O2(g) 3 H2O(g) + 6 CO2(g) (_) 2 C6H6(l) + 9 O2(g) 6 H2O(g) + 12 CO2(g) (o) 2 C6H6(l) + 15 O2(g) 6 H2O(g) + 12 CO2(g)

 Silber4 3.TB.034. Balance the following equation: C8H18O3(l) + O2(g) H2O(g) + CO2(g). (_) C8H18O3(l) + 13 O2(g) 18 H2O(g) + 8 CO2(g) (_) 2 C8H18O3(l) + 22 O2(g) 9 H2O(g) + 16 CO2(g) (_) C8H18O3(l) + 8 O2(g) 9 H2O(g) + 8 CO2(g) (_) 2 C8H18O3(l) + 17 O2(g) 18 H2O(g) + 16 CO2(g) (o) C8H18O3(l) + 11 O2(g) 9 H2O(g) + 8 CO2(g)

 Silber4 3.TB.035. Balance the following equation: Ca3(PO4)2(s) + SiO2(s) + C(s) CaSiO3(s) + CO(g) + P4(s). (_) Ca3(PO4)2(s) + 3 SiO2(s) + 8 C(s) 3 CaSiO3(s) + 8 CO(g) + 2 P4(s) (_) Ca3(PO4)2(s) + 3 SiO2(s) + 14 C(s) 3 CaSiO3(s) + 14 CO(g) + P4(s) (_) Ca3(PO4)2(s) + 3 SiO2(s) + 8 C(s) 3 CaSiO3(s) + 8 CO(g) + P4(s) (_) 2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s) 6 CaSiO3(s) + 10 CO(g) + 4 P4(s) (o) 2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s) 6 CaSiO3(s) + 10 CO(g) + P4(s)

 Silber4 3.TB.036. Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles). SO2(g) + 2 Cl2(g) SOCl2(g) + Cl2O(g) If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed? (_) 0.100 mol (_) 0.400 mol (_) 0.800 mol (_) 0.0500 mol (o) 0.200 mol

 Silber4 3.TB.037. Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis).Al(s) + Br2(l) Al2Br6(s) [unbalanced]How many moles of Al are needed to form 2.43 mol of Al2Br6? (_) 1.62 mol (_) 2.43 mol (_) 7.29 mol (_) 1.22 mol (o) 4.86 mol

 Silber4 3.TB.038. Ammonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in production of aluminum, in uranium processing, and in frosting of light bulbs).2 NH3(g) + 5 F2(g) N2F4(g) + 6 HF(g)How many moles of NH3 are needed to react completely with 13.6 mol of F2? (_) 6.80 mol (_) 27.2 mol (_) 34.0 mol (_) 2.27 mol (o) 5.44 mol

 Silber4 3.TB.039. Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine.N2(g) + 3 H2(g) 2 NH3(g)How many grams of nitrogen are needed to produce 325 grams of ammonia? (_) 178 g (_) 535 g (_) 1070 g (_) 108 g (o) 267 g

 Silber4 3.TB.040. How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are needed to form 485 g of sulfur tetrafluoride?3 SCl2(l) + 4 NaF(s) SF4(g) + S2Cl2(l) + 4 NaCl(s) (_) 205 g (_) 1510 g (_) 1940 g (_) 51.3 g (o) 754 g

 Silber4 3.TB.041. How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH3?4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) (_) 3.406 g (_) 250.0 g (_) 300.6 g (_) 2.180 g (o) 469.7 g

 Silber4 3.TB.042. Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water.PH3(g) + O2(g) P4O10(s) + H2O(g) [unbalanced]Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen. (_) 900. g (_) 940. g (_) 1880 g (_) 56.3 g (o) 470 g

 Silber4 3.TB.043. Potassium chlorate (used in fireworks, flares and safety matches) forms oxygen and potassium chloride when heated.KClO3(s) KCl(s) + O2(g) [unbalanced]How many grams of oxygen are formed when 26.4 g of potassium chlorate is heated? (_) 6.86 g (_) 99.1 g (_) 223 g (_) 4.60 g (o) 10.3 g

 Silber4 3.TB.044. Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl3. What mass of chlorine gas is needed to react completely with 163 g of aluminum? (_) 321 g (_) 245 g (_) 214 g (_) 489 g (o) 643 g

 Silber4 3.TB.045. Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide? (_) 37.7 g (_) 50.3 g (_) 123 g (_) 9.41 g (o) 151 g

 Silber4 3.TB.046. An important reaction sequence in the industrial production of nitric acid is the following.N2(g) + 3 H2(g) 2 NH3(g)4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(l)Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one? (_) 25.0 mol O2 (_) 20.0 mol O2 (_) 12.5 mol O2 (_) 100. mol O2 (o) 50.0 mol O2

 Silber4 3.TB.047. In a blast furnace, elemental iron is produced from a mixture of coke (C), iron ore (Fe3O4) and other reactants. An important reaction sequence is given below.2 C(s) + O2(g) 2 CO(g)Fe3O4(s) + 4 CO(g) 3 Fe(l) + 4 CO2(g)How many moles of iron can be formed in this sequence when 1.00 mol of carbon, as coke, is consumed? (_) 1.33 mol Fe (_) 3.00 mol Fe (_) 6.00 mol Fe (_) 1.25 mol Fe (o) 0.750 mol Fe

 Silber4 3.TB.048. Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen.4 Al(s) + 3 O2(g) 2 Al2O3(s)A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00 g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed? (_) 311.7 g (_) 249.9 g (_) 200.2 g (_) 374.9 g (o) 155.8 g

 Silber4 3.TB.049. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions.4 Al(s) + 3 O2(g) 2 Al2O3(s)A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. (_) Aluminum is the limiting reactant; 16.70 g of oxygen remain. (_) Oxygen is the limiting reactant; 35.16 g of aluminum remain. (_) Oxygen is the limiting reactant; 19.81 g of aluminum remain. (_) Aluminum is the limiting reactant; 35.16 g of oxygen remain. (o) Aluminum is the limiting reactant; 44.24 g of oxygen remain.

 Silber4 3.TB.050. Magnesium reacts with iron(III) chloride to form magnesium chloride (which can be used in fireproofing wood and in disinfectants) and iron.3 Mg(s) + 2 FeCl3(s) 3 MgCl2(s) + 2 Fe(s)A mixture of 41.0 g of magnesium ( = 24.31 g/mol) and 175 g of iron(III) chloride ( = 162.2 g/mol) is allowed to react. What mass of magnesium chloride ( = 95.21 g/mol) is formed? (_) 71.4 g MgCl2 (_) 77.0 g MgCl2 (_) 68.5 g MgCl2 (_) 107 g MgCl2 (o) 154 g MgCl2

 Silber4 3.TB.051. Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron.3 Mg(s) + 2 FeCl3(s) 3 MgCl2(s) + 2 Fe(s)A mixture of 41.0 g of magnesium ( = 24.31 g/mol) and 175 g of iron(III) chloride ( = 162.2 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. (_) Limiting reactant is Mg; 104 g of FeCl3 remain. (_) Limiting reactant is Mg; 134 g of FeCl3 remain. (_) Limiting reactant is Mg; 67 g of FeCl3 remain. (_) Limiting reactant is FeCl3; 87 g of Mg remain. (o) Limiting reactant is FeCl3; 2 g of Mg remain.

 Silber4 3.TB.052. Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride. (_) Chlorine is the limiting reactant; 2.70 g of potassium remain. (_) Chlorine is the limiting reactant; 4.64 g of potassium remain. (_) Potassium is the limiting reactant; 7.23 g of chlorine remain. (_) No limiting reagent: the reactants are present in the correct stoichiometric ratio. (o) Potassium is the limiting reactant; 2.47 g of chlorine remain.

 Silber4 3.TB.053. Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas.P4(s) + 3 O2(g) P4O6(s)If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction? (_) 32.4% (_) 38.0% (_) 57.5% (_) 16.3% (o) 48.8%

 Silber4 3.TB.054. What is the percent yield for the following reaction if 119.3 g of PCl5 ( = 208.2 g/mol) are formed when 61.3 g of Cl2 ( = 70.91 g/mol) react with excess PCl3?PCl3(g) + Cl2(g) PCl5(g) (_) 51.4% (_) 85.0% (_) 195% (_) 43.7% (o) 66.3%

 Silber4 3.TB.055. Methanol (CH4O) is converted to bromomethane (CH3Br) as follows.CH4O + HBr CH3Br + H2OIf 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield? (_) 100.% (_) 245% (_) 40.9% (o) 82.6% (_) 121%

 Silber4 3.TB.056. A 0.150 M sodium chloride solution is referred to as a physiological saline solution because it has the same concentration of salts as normal human blood. Calculate the mass of solute needed to prepare 275.0 mL of a physiological saline solution. (_) 31.9 g (_) 8.77 g (_) 41.3 g (o) 2.41 g (_) 16.1 g

 Silber4 3.TB.057. Sodium chlorate is used as an oxidizer in the manufacture of dyes, explosives and matches. Calculate the mass of solute needed to prepare 1.575 L of 0.00250 M NaClO3 ( = 106.45 g/mol). (_) 169 g (_) 0.00394 g (_) 419 g (o) 0.419 g (_) 0.169 g

 Silber4 3.TB.058. Lithium hydroxide is used in alkaline batteries. Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give a final volume of 750. mL. (_) 1.12 M (_) 0.00199 M (_) 1.50 M (o) 1.99 M (_) 0.502 M

 Silber4 3.TB.059. Hydrochloric acid is widely used as a laboratory reagent, in refining ore for the production of tin and tantalum, and as a catalyst in organic reactions. Calculate the number of moles of HCl in 62.85 mL of 0.453 M hydrochloric acid. (_) 1.04 mol (_) 0.00721 mol (_) 28.5 mol (o) 0.0285 mol (_) 0.139 mol

 Silber4 3.TB.060. Sodium hydroxide, also known as caustic soda, is used to neutralize acids and to treat cellulose in making of cellophane. Calculate the number of moles of solute in 1.875 L of 1.356 M NaOH solution. (_) 0.7232 mol (_) 0.001383 mol (_) 1.383 mol (o) 2.543 mol (_) 0.3932 mol

 Silber4 3.TB.061. Calculate the molarity of a 23.55 mL solution which contains 28.24 mg of sodium sulfate (used in dyeing and printing textiles, = 139.04 g/mol). (_) 1.199 M (_) 0.2031 M (_) 8.625 M (o) 0.008625 M (_) 0.8339 M

 Silber4 3.TB.062. When 2.61 g of solid Na2CO3 is dissolved in sufficient water to make 250 mL of solution, what is the concentration of Na2CO3? (_) 10.4 M (_) 0.141 M (_) 0.0246 M (o) 0.0985 M2 (_) 0.205 M

 Silber4 3.TB.063. Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL. (_) 0.743 M (_) 0.114 M (_) 3.86 M (o) 0.123 M (_) 0.222 M

 Silber4 3.TB.064. What will be the final volume of a solution prepared by diluting 25 mL of 8.25 M sodium hydroxide to a concentration of 2.40 M? (_) 210 mL (_) 7.3 mL (_) 330 mL (o) 86 mL (_) 60 mL

 Silber4 3.TB.065. What volume, in L, of 10.0 M HCl is needed to make 2.00 L of 2.00 M HCl solution by dilution with water? (_) 0.200 L (_) none of these (_) 0.800 L (o) 0.400 L (_) 0.100 L

 Silber4 3.TB.066. How many mL of concentrated nitric acid (HNO3, 16.0 M) should be diluted with water in order to make 2.00 L of 2.00 M solution? (_) 62.5 mL (_) 500. mL (_) 32.0 mL (o) 250. mL (_) 125 mL

 Silber4 3.TB.067. How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO3 ( = 84.02 g/mol)?HCl(aq) + NaHCO3(s) NaCl(s) + H2O(l) + CO2(g) (_) 572 mL (_) 276 mL (_) 638 mL (o) 175 mL (_) 536 mL

 Silber4 3.TB.068. Copper(II) sulfide, CuS, is used in the development of aniline black dye in textile printing. What is the maximum mass of CuS which can be formed when 38.0 mL of 0.500 M CuCl2 are mixed with 42.0 mL of 0.600 M (NH4)2S? Aqueous ammonium chloride is the other product. (_) 1.21 g (_) 0.044 g (_) 2.41 g (o) 1.82 g (_) 0.909 g

 Silber4 3.TB.069. What mass of carbon is needed to react with 10.00 g of SnO2(s) according to the following chemical equation: SnO2(s) + 2 C(s) Sn(s) + 2 CO(g)? (_) 7.94 g (_) 23.8 g (_) 3.97 g (o) 1.59 g

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