Chemistry & Chemical Reactions Kotz9e TB CH 04 PDF

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Chemistry & Chemical Reactions Chapter 4...

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Chapter 4—Stoichiometry: Quantitative Information about Chemical Reactions MULTIPLE CHOICE 1. Potassium hydrogen carbonate decomposes with heat as follows: 2KHCO3(s)  K2CO3(s) + CO2(g) + H2O(l) How many moles of potassium carbonate will be produced if 201 g of potassium hydrogen carbonate are heated? a. 1.00 mol b. 1.45 mol c. 10.8 mol d. 101 mol e. 2.01 mol ANS: A 2. Calculate the number of moles of O2 required to react with phosphorus to produce 4.76 g of P4O6. (Molar mass P4O6 = 219.9 g/mol) a. 0.0216 mol b. 0.149 mol c. 0.0649 mol d. 0.0433 mol e. 0.130 mol ANS: C 3. The complete combustion of 0.32 moles of propane, C3H8, will a. consume 0.32 mol O2 and produce 0.32 mol CO2. b. consume 0.32 mol O2 and produce 0.64 mol CO2. c. consume 1.6 mol O2 and produce 0.96 mol CO2. d. consume 1.6 mol O2 and produce 4.8 mol CO2. e. consume 1.6 mol O2 and produce 1.3 mol CO2. ANS: C 4. 2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2(g) According to the equation above, how many grams of aluminum are needed to completely react with 3.83 mol of hydrochloric acid? a. 310 g b. 46.6 g c. 34.4 g d. 3.83 g e. 103.3 g ANS: C 5. Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g) + H2O(l)  H2SO3(l) What mass of sulfur dioxide is needed to prepare 21.06 g of H2SO3(l)? a. 16.44 g b. 26.98 g c. 0.3287 g d. 0.2566 g

e.

21.06 g

ANS: A 6. When strongly heated, boric acid breaks down to boric oxide and water. What mass of boric oxide is formed from the decomposition of 15.0 g B(OH) 3? 2 B(OH)3(s)  B2O3(s) + 3 H2O(g) a. 7.50 g b. 15.0 g c. 8.44 g d. 16.9 g e. 33.8 g ANS: C

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

7. If the complete combustion of an unknown mass of ethylene produces 16.0 g CO2, what mass of ethylene is combusted? C2H4(g) + 3 O2(g)  2 CO2(g) + 2 H2O(g) a. 0.182 g b. 0.364 g c. 5.10 g d. 8.00 g e. 12.6 g ANS: C

8. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu2S(s) + O2(g)  2Cu(s) + SO2(g) What mass of copper(I) sulfide is required in order to prepare 0.610 kg of copper metal? a. 0.610 kg b. 0.305 kg c. 0.459 kg d. 1.53 kg e. 0.764 kg ANS: E 9. The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below. P4S3(s) + O2(g)  P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.401 g P4S3? a. 0.134 g b. 1.20 g c. 0.0389 g d. 0.117 g e. 0.350 g ANS: E

10. How many grams of dioxygen are required to completely burn 4.3 g of C2H5OH? a. 19 g b. 15 g c. 3.0 g d. 42 g e. 58 g ANS: A 11. Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of H2O2? a. 58.8 g b. 66.4 g c. 107 g d. 118 g e. 125 g ANS: A

12. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following balanced chemical equation: Rh2(SO4)3(aq) + 6NaOH(aq)



2Rh(OH)3(s) + 3Na2SO4(aq)

If 6.20 g of rhodium(III) sulfate reacts with excess sodium hydroxide, what mass of rhodium(III) hydroxide may be produced? a. 3.86 g b. 12.4 g c. 6.20 g d. 0.966 g e. 7.73 g ANS: A

Chapter 4

Kotz 9e

Stoichiometry: Quantitative Information about Chemical Reactions

13. The commercial production of phosphoric acid, H3PO4, can be represented by the equation 1500 g Ca3(PO4)2 + 310 g/mol

300 g 3SiO2 + 60.1 g/mol

307 g 1180 g 300 g 5C + 5O2 + 3H2O  3CaSiO3 + 5CO2 + 2H3PO4 12.0 g/mol 32.0 g/mol 18.0 g/mol

The molar mass for each reactant is shown below the reactant, and the mass of each reactant for this problem is given above. Which substance is the limiting reactant? a. H2O b. C c. O2 d. Ca3(PO4)2 e. SiO2 ANS: E 14. How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s) + Br2(g)  2 NaBr(s) a. 0.650 mol b. 1.03 mol c. 1.30 mol d. 2.06 mol e. 0.515 mol ANS: B 15. How many moles of Mg3P2(s) can be produced from the reaction of 0.14 mol Mg(s) with 0.020 mol P4(s)? 6 Mg(s) + P4(s)  2 Mg3P2(s) a. 0.047 mol b. 0.14 mol c. 0.42 mol d. 0.020 mol e. 0.040 mol ANS: E 16. Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2? 4 NH3(g) + 5 O2(g)  4 NO(g) + 6 H2O(g) a. 4.54 g b. 12.8 g c. 14.1 g d. 15.9 g e. 25.0 g ANS: B 17. If 5.00 g Br2 and 1.10 g NH3 react according to the equation below, what is the maximum mass of ammonium bromide produced? 3 Br2( ) + 8 NH3(g)  6 NH4Br(s) + N2(g) a. 3.06 g b. 6.13 g c. 12.9 g d. 4.74 g e. 8.43 g ANS: D 18. What mass of iron can be produced from the reaction of 175 kg Fe 2O3 with 385 kg CO? Fe2O3(s) + 3 CO(g)  2 Fe(s) + 3 CO2(g) a. 2.19 kg b. 30.6 kg c. 61.2 kg d. 122 kg e. 512 kg ANS: D 19. Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of MgI 2 can be produced from the reaction of 5.15 g Mg and 50.0 g I 2? a. 29.5 g b. 44.9 g c. 54.8 g d. 55.2 g e. 58.9 g ANS: C

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

20. If 48.8 g of O2 is mixed with 48.8 g of H2 and the mixture is ignited, what is the maximum mass of water that may be produced? a. 439 g b. 54.9 g c. 48.8 g d. 98 g e. 86.8 g ANS: B 21. Aspirin (C9H8O4) is produced by the reaction of salicylic acid ( M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol). C7H6O3(s) + C4H6O3( )  C9H8O4(s) + C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3, what mass of aspirin (M = 180.2 g/mol) can theoretically be obtained? a. 0.40 g b. 2.61 g c. 2.82 g d. 1.53 g e. 3.60 g ANS: B 22. A 5.95-g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3(aq) + BaCl2(aq)  2AgCl(s) + Ba(NO3)2(aq) to give 3.75 g of AgCl. What is the percent yield of AgCl? a. 49.8 % b. 37.4 % c. 74.7 % d. 63.0 % ANS: C

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e. 100 %

4.3 Percent Yield

23. The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.3 g of CCl4, carbon tetrachloride: 2CHCl3 + 2Cl2  2CCl4 + 2HCl What is the percent yield? a. 86.6 % b. 100 % ANS: C

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c. 67.2 %

d. 33.6 %

e. 44.8 %

4.3 Percent Yield

24. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu2S(s) + O2(g)  2Cu(s) + SO2(g) If the reaction of 0.630 kg of copper(I) sulfide with excess oxygen produces 0.190 kg of copper metal, what is the percent yield? a. 75.5 % b. 39.9 % c. 30.2 % d. 151 % e. 37.8 % ANS: E

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4.3 Percent Yield

25. Sulfur trioxide, SO3, is made from the oxidation of SO2as follows: 2SO2 + O2  2SO3 A 21-g sample of SO2 gives 18 g of SO3. The percent yield of SO3 is . a. 11 % b. 69 % c. 17 % d. 26 % e. 100 % ANS: B

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4.3 Percent Yield

26. Nitric oxide, NO, is made from the oxidation of NH3 as follows: 4NH3 + 5O2  4NO + 6H2O If 9.4-g of NH3 gives 12.0 g of NO, what is the percent yield of NO? a. 91 % b. 44 % c. 17 % d. 72 % e. 22 % ANS: D

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4.3 Percent Yield

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

27. Consider the fermentation reaction of glucose: C6H12O6  2C2H5OH + 2CO2 A 1.00-mol sample of C6H12O6 was placed in a vat with 100 g of yeast. If 67.8 g of C2H5OH was obtained, what was the percent yield of C2H5OH? a. 73.6 % b. 36.8 % c. 67.8 % d. 100 % e. none of these ANS: A

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4.3 Percent Yield

28. Aspirin is produced by the reaction of salicylic acid ( M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol). C7H6O3(s) + C4H6O3( )  C9H8O4(s) + C2H4O2( ) If 2.04 g of C9H8O4 (M = 180.2 g/mol) is produced from the reaction of 3.03 g C7H6O3 and 4.01 g C4H6O3, what is the percent yield? a. 28.8% b. 29.0% c. 50.9% d. 51.6% e. 67.3% ANS: D

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4.3 Percent Yield

29. Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH3 must react with excess oxygen to yield 157 g NO? 4 NH3(g) + 5 O2(g)  4 NO(g) + 6 H2O(g) a. 89.1 g b. 302 g c. 263 g d. 26.3 g e. 938 g ANS: B

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4.3 Percent Yield

30. If 15.0 g N2 and 2.00 g H2 react to produce 1.38 g NH3, what is the percent yield of the reaction? N2(g) + 3 H2(g)  2 NH3(g) a. 7.57% b. 12.2% c. 8.12% d. 15.1% e. 8.17% ANS: B

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4.3 Percent Yield

31. Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S8(s) + 24 F2(g)  8 SF6(g) What is the percent yield if 18.3 g SF6 is isolated from the reaction of 10.0 g S8 and 30.0 g F2? a. 40.2% b. 45.8% c. 47.6% d. 54.6% e. 61.0% ANS: C

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4.3 Percent Yield

32. Of the following, the only empirical formula is a. C6H12. b. C2H8. c. C3H8.

d. H2O2.

e. O3.

ANS: C 33. A certain compound has a molar mass of 150 g/mol. Which is a possible empirical formula for this compound? a. CH2O b. CHO c. C2H2O2 d. C2HO e. C2H2O ANS: A

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

34. The empirical formula of ethylene is CH2. An experimental determination of the molar mass of ethylene yields the value of 28 g/mol. What is the molecular formula of ethylene? a. C5H10 b. CH2 c. C2H4 d. C3H8 e. C6H9 ANS: C 35. A compound consists of only C and F. It contains 38.71% C by mass. What is the empirical formula of the compound? a. CF b. CF2 c. CF3 d. C2F e. CF4 ANS: A 36. The amount of calcium in a 15.0-g sample was determined by converting the calcium to calcium oxalate, CaC2O4. The CaC2O4 weighed 11.5 g. What is the percent of calcium in the original sample? a. 9.8 % b. 24.0 % c. 13.5 % d. 30.7 % e. 76.7 % ANS: B 37. A mass of 2.213 g of a metal carbonate, MCO3, is heated to drive off carbon dioxide. The remaining metal oxide has a mass of 1.061 g. MCO3(s)  MO(s) + CO2(g) What is the identity of the metal? a. Mg b. Ca c. Cu d. Sr e. Ba ANS: A 38. A mixture of MnSO4 and MnSO44H2O has a mass of 2.005 g. After heating to drive off all the water the mass is 1.780 g. What is the mass percent of MnSO44H2O in the mixture? a. 11.2% b. 34.7% c. 65.3% d. 69.6% e. 88.8% ANS: B 39. A 1.850 g mixture of SrCO3 and SrO is heated. The SrCO3 decomposes to SrO and CO2. What was the mass percentage of SrCO3 in the mixture if the mass after heating is 1.445 g? a. 26.6% b. 21.9% c. 13.7% d. 73.4% e. 78.1% ANS: D 40. Chlorine was passed over 2.02 g of heated titanium, and 6.50 g of a chloride-containing compound of Ti was obtained. What is the empirical formula of the chloride-containing compound? a. TiCl2 b. TiCl4 c. TiCl d. TiCl3 e. Ti2Cl3 ANS: D 41. The reaction of 0.779 g K with O2 forms 1.417 g potassium superoxide, a substance used in selfcontained breathing devices. Determine the formula for potassium superoxide. a. KO2 b. KO c. K2O3 d. K2O e. KO4 ANS: A

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

42. A 2.841 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 7.794 g CO2 and water. What mass of hydrogen is contained in the original sample? a. 0.7140 g b. 4.953 g c. 10.64 g d. 2.826 g e. 1.421 g ANS: A 43. A 3.361 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 6.295 g CO2 and 3.866 g H2O. What is the empirical formula of the hydrocarbon? a. CH3 b. CH2 c. C2H3 d. CH4 e. CH ANS: A 44. Complete combustion of a 0.30-mol sample of a hydrocarbon, CxHy, gives 1.80 mol of CO2 and 1.20 mol of H2O. The molecular formula of the original hydrocarbon is a. C3H8. b. C6H8. c. C7H18. d. C5H5. e. C5H6. ANS: B 45. The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H2O and 3.5927 g CO2. What is the molar mass of the hydrocarbon? a. 16.0 g/mol b. 30.1 g/mol c. 44.1 g/mol d. 72.2 g/mol e. 92.1 g/mol ANS: C 46. Polyethylene is a polymer consisting of only carbon and hydrogen. If 2.300 g of the polymer is burned in oxygen it produces 2.955 g H2O and 7.217 g CO2. What is the empirical formula of polyethylene? a. CH b. CH2 c. C2H3 d. C5H8 e. C7H8 ANS: B 47. Soft drink bottles are made of polyethylene terephthalate (PET), a polymer composed of carbon, hydrogen, and oxygen. If 1.9022 g PET is burned in oxygen it produces 0.6585 g H2O and 4.0216 g CO2. What is the empirical formula of PET? a. CHO b. CH7O5 c. C5H7O d. C8H10O e. C10H8O5 ANS: E 48. A 1.185 g sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 2.264 g CO2 and 1.390 g H2O. What mass of oxygen is contained in the original sample? a. 0.4117 g b. 0.5673 g c. 1.079 g d. 0.8733 g e. 0.2053 g ANS: A 49. A 4.541 g sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 8.674 g CO2 and 5.328 g H2O. What is the empirical formula of the compound? a. CHO b. C2H6O c. C3H6O d. C3H4O e. C3H8O3 ANS: B

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

50. Naphthalene, a hydrocarbon, has an approximate molar mass of 128 g/mole. If the combustion of 0.6400 g naphthalene produces 0.3599 g H2O and 2.1977 g CO2, what is the molecular formula of this compound? a. C8H32 b. C9H18 c. C9H20 d. C10H8 e. C11H7 ANS: D 51. What is the molarity of an NaI solution that contains 5.3 g of NaI in 41.0 mL of solution? a. 0.86 M b. 0.035 M c. 0.0077 M d. 0.00027 M e. 0.13 M ANS: A 52. What volume of 0.464 M Na2CO3 solution contains 74.7 g of Na2CO3? a. 0.327 L b. 1.71  104 L c. 1.52 L d. 3.67  103 L e. 0.658 L ANS: C 53. How many moles of sulfate ions are there in a 0.387-L solution of 0.927 M Al2(SO4)3? a. 0.359 mol b. 1.08 mol c. 1.25 mol d. 0.120 mol e. 7.19 mol ANS: B 54. What mass of Na2CO3 is present in 0.250 L of a 0.852 M Na2CO3 solution? a. 22.6 g b. 26.5 g c. 90.3 g d. 31.1 g e. 361 g ANS: A 55. In order to dilute 35.5 mL of 0.533 M HCl to 0.100 M, the volume of water that must be added is a. 28.8 mL. b. 6.66 mL. c. 1.89  102 mL. d. 1.50  10–3 mL. e. 1.54  102 mL. ANS: E 56. A dilute solution is prepared by transferring 45.00 mL of a 0.5616 M stock solution to a 400.0 mL volumetric flask and diluting to mark. What is the molarity of this dilute solution? a. 0.06318 M b. 0.1264 M c. 0.04992 M d. 0.01580 M e. 0.2808 M ANS: A 57. What volume of 2.52 M HCl is required to prepare 176.5 mL of 0.449 M HCl? a. 9.91  102 mL b. 1.56  102 mL c. 31.4 mL d. 0.0318 mL e. 2.00  102 mL ANS: C

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

58. What is the pH of 5.3  103 M HCl(aq)? a. –1.01 b. 2.28 c. 3.50

d. 1.01

e. 5.65

ANS: B 59. The pH of an aqueous NaOH solution is 12.83. What is the hydrogen ion concentration of this solution? a. 1.5  10–13 M b. 6.7  10–2 M c. 1.2 M d. 6.7  1012 M e. 2.7  10–6 M ANS: A 60. The pH of a vinegar solution is 4.15. What is the H3O+ concentration of the solution? a. 7.1  10–5 M b. 1.6  10–2 M c. 0.62 M d. 1.4 M e. 1.4  104 M ANS: A 61. The concentration of sulfate in a sample of wastewater is to be determined by using gravimetric analysis. To a 100.0-mL sample of the wastewater is added an excess of calcium nitrate, forming the insoluble calcium sulfate (136.1 g/mol) according to the balanced equation given below. The solid calcium sulfate is dried, and its mass is measured to be 0.7272 g. What was the concentration of sulfate in the original wastewater sample? SO42–(aq) + Ca(NO3)2(aq)  CaSO4(s) + 2NO3–(aq) a. 0.05343 M

b. 0.9897 M

c. 18.72 M

d. 1.872 M

e. 9.897 M

ANS: A 62. An aqueous nitric acid solution has a pH of 2.15. What mass of HNO3 is present in 20.0 L of this solution? a. 0.11 g b. 0.022 g c. 3.7 g d. 6.8 g e. 8.9 g ANS: E

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

63. Zn reacts with hydrochloric acid. Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g) What volume of 3.05 M HCl(aq) will react with 25.0 g Zn(s)? a. 0.251 L b. 4.01 L c. 0.125 L d. 0.0627 L e. 2.33 L ANS: A 64. What minimum mass of copper (II) nitrate must be added to 30.0 mL of a 0.0387 M phosphate solution in order to completely precipitate all of the phosphate as solid copper (II) phosphate? 2PO43–(aq) + 3Cu(NO3)2(aq)  Cu3(PO4)2(s) + 6NO3–(aq) a. 0.218 g ANS: E NOT:

b. 0.653 g

c. 0.145 g

d. 0.0726 g

e. 0.327 g

Dynamic Question

65. A mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq), what is the molar mass of the acid? a. 2.965  10–3 g/mol b. 9.128 g/mol c. 138.7 g/mol d. 337.3 g/mol e. 820.7 g/mol ANS: C 66. An unknown diprotic acid (H2A) requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580 g sample. Calculate the approximate molar mass of the acid. a. 406 g/mol

b. 235 g/mol

c. 118 g/mol

d. 59 g/mol

e. 203 g/mol

ANS: B 67. The reaction of HCl with NaOH is represented by the equation HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l) What volume of 0.686 M HCl is required to titrate 42.8 mL of 0.334 M NaOH? a. 9.81 mL b. 1.46 mL c. 20.8 mL d. 42.8 mL e. 87.9 mL ANS: C

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

68. If 0.1800 g of impure soda ash (Na2CO3) is titrated with 15.66 mL of 0.1082 M HCl, what is the percent purity of the soda ash? Na2CO3(aq) + 2 HCl(aq)  2 NaCl(aq) + H2O( ) + CO2(g) a. 17.96% b. 49.89% c. 50.11% d. 94.13% e. 99.77% ANS: B 69. An impure sample of benzoic acid (C6H5COOH, 122.12 g/mol) is titrated with 0.8067 M NaOH. A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint. What is the percent by mass of benzoic acid in the sample? C6H5COOH(aq) + NaOH(aq)  NaC6H5COO(aq) + H2O(l) a. 0.02442 %

b. 2.982 %

c. 100.0 %

d. 24.42 %

e. 71.29 %

ANS: E 70. A 50.00-mL sample of a weak monoprotic acid is titrated with 0.0955 M NaOH. At the endpoint, it is found that 32.56 mL of titrant was used. What was the concentration of the weak acid? a. 0.0622 M b. 3.11 M c. 0.0955 M d. 5.87  10–5 M e. 0.147 M ANS: A 71. A solution of sodium oxalate (Na2C2O4) in acidic solution is titrated with a solution of potassium permanganate (KMnO4) according to the following balanced chemical equation: 2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq)  2MnSO4(aq) + 8H2O(l) + 10CO2(g) + 5Na2SO4(aq) + K2SO4(aq) What volume of 0.0388 M KMnO4 is required to titrate 0.134 g of Na2C2O4 dissolved in 20.0 mL of solution? a. 1.38 mL b. 3.45 mL c. 10.3 mL d. 25.8 mL e. 20.0 mL ANS: C 72. Transmittance, T, is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample. The absorbance, A, is defined as a. A = –log T b. A = log (–T) c. A = 10T d. A = 10–T e. A = 10–1/T ANS: A

Kotz 9e

Chapter 4

Stoichiometry: Quantitative Information about Chemical Reactions

73. Which of the following statements is/are CORRECT? 1. Absorbance is directly proportional to the intensity of the incident light. 2. Absorbance is inversely proportional to the analyte concentration. 3. Absorbance is directly proportional to the path length of the light. a. 1 only

b. 2 only

c. 3 only

d. 2 and 3

e. 1,2, and 3

ANS: C 74. Calibration of a spectrophotmeter using a se...