Chapter 10 - An Introduction to Chemistry: Chemical Calculations ...

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402 Chapter 10 Chemical Calculations and Chemical Equations Objective 6 Objective 7 42. Aniline, C 6 H 5 NH 2 , which is used to make antioxidants, can be formed from nitrobenzene, C 6 H 5 NO 2 , in the following reaction. FeCl 4C 6 H 5 NO 2 + 9Fe + 4H 2 O 2 4C 6 H 5 NH 2 + 3Fe 3 O 4 Objective 6 Objective 7 Objective 6 Objective 6 Objective 8 a. What is the maximum mass of aniline, C 6 H 5 NH 2 , formed in the reaction of 810.5 g of nitrobenzene, C 6 H 5 NO 2 , with 985.0 g of Fe and 250 g of H 2 O? b. Explain why two of these substances are in excess and one is limiting. 43. Uranium is distributed in a form called yellow cake, which is made from uranium ore. In the second step of the reactions that form yellow cake from uranium ore, uranyl sulfate, UO 2 SO 4 , is converted to (NH 4 ) 2 U 2 O 7 . 2UO 2 SO 4 + 6NH 3 + 3H 2 O → (NH 4 ) 2 U 2 O 7 + 2(NH 4 ) 2 SO 4 a. What is the maximum mass, in kilograms, of (NH 4 ) 2 U 2 O 7 that can be formed from the reaction of 100 kg of water and 100 kg of ammonia with 481 kg of UO 2 SO 4 ? b. Explain why two of these substances are in excess and one is limiting. 44. Calcium carbide, CaC 2 , is formed in the reaction between calcium oxide and carbon. The other product is carbon monoxide. a. Write a balanced equation for this reaction. (You do not need to write the states.) b. If you were designing the procedure for producing calcium carbide from calcium oxide and carbon, which of the reactants would you have as the limiting reactant? Why? c. Assuming 100% yield from the limiting reactant, what are the approximate amounts of CaO and carbon that you would combine to form 860.5 g of CaC 2 ? 45. Calcium carbide, CaC 2 , reacts with water to form acetylene, C 2 H 2 , and calcium hydroxide. a. Write a balanced equation for this reaction. (You do not need to write the states.) b. If you were designing the procedure for producing acetylene from calcium carbide and water, which of the reactants would you have as the limiting reactant? Why? c. Assuming 100% yield from the limiting reactant, what are the approximate amounts of CaC 2 and water that you would combine to form 127 g of C 2 H 2 ? 46. Give four reasons why the actual yield in a chemical reaction is less than the theoretical yield. 47. When determining the theoretical yield for a reaction, why must we first determine which reactant is the limiting reactant? 48. Does the reactant in excess affect the actual yield for a reaction? If it does, explain how. 49. Can the calculated percent yield ever be above 100%. If it can, explain how.
Chapter Problems 403 Section 10.3 Molarity and Equation Stoichiometry 50. What is the molarity of a solution made by dissolving 37.452 g of aluminum sulfate, Al 2 (SO 4 ) 3 , in water and diluting with water to 250.0 mL total? 51. What is the molarity of a solution made by dissolving 18.476 g of potassium carbonate, K 2 CO 3 , in water and diluting with water to 100.0 mL total? 52. The following equation represents the first step in the conversion of UO 3 , found in uranium ore, into the uranium compounds called “yellow cake.” UO 3 + H 2 SO 4 → UO 2 SO 4 + H 2 O a. How many milliliters of 18.0 M H 2 SO 4 are necessary to react completely with 249.6 g of UO 3 ? b. What is the maximum mass, in grams, of UO 2 SO 4 that forms from the complete reaction of 125 mL of 18.0 M H 2 SO 4 ? 53. Most of the sodium chlorate, NaClO 3 , produced in the United States is converted into chlorine dioxide, which is then used for bleaching wood pulp. NaClO 3 (aq) + 2HCl(aq) → ClO 2 (g) + ½Cl 2 (g) + NaCl(aq) + H 2 O(l ) a. How many milliliters of 12.1 M HCl are necessary to react completely with 35.09 g of sodium chlorate, NaClO 3 ? b. What is the maximum mass, in grams, of ClO 2 that can be formed from the complete reaction of 65 mL of 12.1 M HCl? 54. When a water solution of sodium sulfite, Na 2 SO 3 , is added to a water solution of iron(II) chloride, FeCl 2 , iron(II) sulfite, FeSO 3 , precipitates from the solution. a. Write a balanced equation for this reaction. b. What is the maximum mass of iron(II) sulfite that will precipitate from a solution prepared by adding an excess of a Na 2 SO 3 solution to 25.00 mL of 1.009 M FeCl 2 ? 55. Consider the precipitation reaction that takes place when a water solution of aluminum nitrate, Al(NO 3 ) 3 , is added to a water solution of potassium phosphate, K 3 PO 4 . a. Write a balanced equation for this reaction. b. What is the maximum mass of aluminum phosphate that will precipitate from a solution prepared by adding an excess of an Al(NO 3 ) 3 solution to 50.00 mL of 1.525 M K 3 PO 4 ? 56. Consider the neutralization reaction that takes place when nitric acid reacts with aqueous potassium hydroxide. a. Write a conversion factor that relates moles of HNO 3 to moles of KOH for this reaction. b. What is the minimum volume of 1.50 M HNO 3 necessary to neutralize completely the hydroxide in 125.0 mL of 0.501 M KOH? 57. Consider the neutralization reaction that takes place when hydrochloric acid reacts with aqueous sodium hydroxide. a. Write a conversion factor that relates moles of HCl to moles of NaOH for this reaction. b. What is the minimum volume of 6.00 M HCl necessary to neutralize completely the hydroxide in 750.0 mL of 0.107 M NaOH? Objective 10 Objective 10 Objective 11 Objective 12 Objective 13 Objective 11 Objective 12 Objective 13 Objective 11 Objective 12 Objective 13 Objective 11 Objective 12 Objective 13 Objective 11 Objective 12 Objective 13 Objective 11 Objective 12 Objective 13
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Chapter 10 - An Introduction to Chemistry: Chemical Calculations ...

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