Moles, Mass, and Limiting Reactants

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Moles, Mass, and Limiting Reactants Interpreting a Chemical Equation 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol H 2 (g) + Cl 2 (g) 2 HCl(g) 2. Assuming similar conditions, how many liters of chlorine gas react to produce 2 L of hydrogen chloride gas? (a) 1 L (b) 2 L (c) 3 L (d) 4 L H 2 (g) + Cl 2 (g) 2 HCl(g) 3. How many moles of carbon monoxide react with 1 mol of oxygen gas according to the balanced chemical equation? 2 CO(g) + O 2 (g) 2 CO 2 (g) (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol

4. Assuming similar conditions, how many liters of carbon monoxide gas react to produce 2 L of carbon dioxide gas? 2 CO(g) + O 2 (g) 2 CO 2 (g) (a) 1 L (b) 2 L (c) 3 L (d) 4 L 5. How many moles of water vapor, H 2 O, react with 1 mol of charcoal, C, according to the balanced chemical equation? C(s) + H 2 O(g) CO(g) + H 2 (g) (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol 6. Assuming similar conditions, how many liters of water vapor, H 2 O, react to produce 1 L of hydrogen gas? C(s) + H 2 O(g) CO(g) + H 2 (g) (a) 1 L (b) 2 L (c) 3 L (d) 4 L 7. In an experiment, 5.585 g of iron metal reacts with 3.207 g of yellow sulfur. Using the conservation of mass law, predict the mass of product. Fe(s) + S(s) FeS(s) (a) 2.198 g (b) 2.378 g (c) 4.396 g (d) 8.792 g (e) 17.584 g

8. In an experiment, 1.201 g of charcoal reacts with 6.414 g of powdered sulfur. Using the conservation of mass law, predict the mass of product. C(s) + 2 S(s) CS 2 (g) (a) 4.408 g (b) 5.213 g (c) 7.615 g (d) 8.816 g (e) 14.029 g 9. In an experiment, 0.520 g of chromium metal reacts with 3.807 g of iodine. Using the conservation of mass law, predict the mass of product. 2 Cr(s) + 3 I 2 (s) 2 CrI 3 (s) (a) 1.529 g (b) 3.287 g (c) 4.327 g (d) 8.654 g (e) 12.461 g 10. In an experiment, 0.243 g of magnesium reacts to give 0.403 g magnesium oxide. Using the conservation of mass law, predict the mass of reacting oxygen gas. 2 Mg(s) + O 2 (g) 2 MgO(s) (a) 0.080 g (b) 0.160 g (c) 0.320 g (d) 0.646 g (e) 1.292 g 11. In an experiment, 0.327 g of zinc metal reacts to produce 0.407 g of zinc oxide. Using the conservation of mass law, predict the mass of reacting oxygen gas. 2 Zn(s) + O 2 (g) 2 ZnO(s) (a) 0.040 g (b) 0.080 g (c) 0.160 g (d) 0.734 g (e) 1.468 g

12. In an experiment, 0.197 g of gold metal reacts to yield 0.303 g of gold(iii) chloride. Using the conservation of mass law, predict the mass of reacting chlorine gas. 2 Au(s) + 3 Cl 2 (g) 2 AuCl 3 (s) (a) 0.035 g (b) 0.106 g (c) 0.318 g (d) 0.167 g (e) 0.500 g Mole Mole Relationships 13. How many moles of iodine vapor react with 1.00 mol of hydrogen gas? H 2 (g) + I 2 (g) HI(g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 14. How many moles of hydrogen iodide are produced from 1.00 mol of iodine? H 2 (g) + I 2 (g) HI(g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 15. How many moles of hydrogen gas react to yield 1.00 mol of hydrogen iodide? H 2 (g) + I 2 (g) HI(g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol

16. How many moles of water are produced from 1.00 mol of hydrogen peroxide? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 17. How many moles of oxygen are produced from 1.00 mol of hydrogen peroxide? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 18. How many moles of hydrogen peroxide decompose to give 1.00 mol of oxygen? H 2 O 2 (l) H 2 O(l) + O 2 (g) (a) 0.500 mol (b) 1.00 mol (c) 2.00 mol (d) 4.00 mol 19. How many moles of oxygen gas react with 1.00 mol NO? UV NO(g) + O 2 (g) NO 2 (g) (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol

20. How many moles of nitrogen dioxide gas are produced from 1.00 mol NO? UV NO(g) + O 2 (g) NO 2 (g) (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol 21. How many moles of oxygen gas react to yield 1.00 mol NO 2? UV NO(g) + O 2 (g) NO 2 (g) (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol 22. How many moles of water react with 5.00 mol of lithium metal? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g) 23. How many moles of hydrogen gas are produced from 5.00 mol of water? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g)

24. How many moles of lithium metal react to yield 5.00 mol of hydrogen gas? (a) 2.50 mol (b) 5.00 mol (c) 10.0 mol (d) 20.0 mol Li(s) + H 2 O(l) LiOH(aq) + H 2 (g) 25. How many moles of water react with 0.500 mol of calcium metal? (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g) 26. How many moles of hydrogen gas are produced from 0.500 mol of water? (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g) 27. How many moles of calcium metal react to yield 0.500 mol of hydrogen gas? (a) 0.250 mol (b) 0.500 mol (c) 1.00 mol (d) 2.00 mol Ca(s) + H 2 O(l) Ca(OH) 2 (aq) + H 2 (g)

28. How many moles of oxygen gas react with 0.100 mol of pentane, C 5 H 12? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) 0.100 mol (b) 0.500 mol (c) 0.600 mol (d) 0.800 mol 29. How many moles of water are produced from 0.100 mol pentane, C 5 H 12? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) 0.100 mol (b) 0.500 mol (c) 0.600 mol (d) 0.800 mol 30. How many moles of oxygen gas react to yield 0.100 mol water? spark C 5 H 12 (g) + O 2 (g) CO 2 (g) + H 2 O(g) (a) 0.100 mol (b) 0.500 mol (c) 0.600 mol (d) 0.800 mol Mass Mole Mole Mass Problems 31. What is the mass of silver metal produced from 6.35 g of copper? (a) 0.187 g (b) 0.540 g (c) 0.747 g (d) 1.08 g (e) 21.6 g Cu(s) + AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + Ag(s)

32. What is the mass of copper metal that yields 0.500 g of silver? (a) 0.147 g (b) 0.294 g (c) 0.425 g (d) 0.589 g (e) 1.70 g Cu(s) + AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + Ag(s) 33. What is the mass of silver bromide (187.77 g/mol) precipitated from 2.96 g of iron(iii) bromide (295.55 g/mol)? (a) 0.940 g (b) 0.627 g (c) 1.88 g (d) 5.64 g (e) 3.76 g FeBr 3 (s) + AgNO 3 (aq) AgBr(s) + Fe(NO 3 ) 3 (aq) 34. What is the mass of iron(iii) bromide (295.55 g/mol) that yields 0.188 g of silver bromide (187.77 g/mol) precipitate? (a) 0.0986 g (b) 0.148 g (c) 0.296 g (d) 0.592 g (e) 0.888 g FeBr 3 (s) + AgNO 3 (aq) AgBr(s) + Fe(NO 3 ) 3 (aq) 35. What is the mass of lead(ii) iodide (461.0 g/mol) precipitated from 0.830 g of potassium iodide (166.00 g/mol)? (a) 0.149 g (b) 0.598 g (c) 1.15 g (d) 2.31 g (e) 4.61 g Pb(NO 3 ) 2 (aq) + KI(s) PbI 2 (s) + KNO 3 (aq)

36. What is the mass of potassium iodide (166.00 g/mol) that yields 0.500 g of lead(ii) iodide (461.0 g/mol) precipitate? (a) 0.0900 g (b) 0.180 g (c) 0.360 g (d) 0.694 g (e) 2.78 g Pb(NO 3 ) 2 (aq) + KI(s) PbI 2 (s) + KNO 3 (aq) 37. What is the mass of insoluble calcium phosphate (310.18 g/mol) produced from 0.555 g of calcium chloride (110.98 g/mol)? (a) 0.0662 g (b) 0.517 g (c) 0.596 g (d) 1.55 g (e) 4.65 g CaCl 2 (s) + Na 3 PO 4 (aq) Ca 3 (PO 4 ) 2 (s) + NaCl(aq) 38. What is the mass of sodium phosphate (163.94 g/mol) that yields 1.00 g of calcium phosphate (310.18 g/mol) precipitate? (a) 0.264 g (b) 0.358 g (c) 0.931 g (d) 1.06 g (e) 8.38 g CaCl 2 (s) + Na 3 PO 4 (aq) Ca 3 (PO 4 ) 2 (s) + NaCl(aq) 39. What is the mass of aluminum oxide (101.96 g/mol) produced from 3.59 g of iron(ii) oxide (71.85 g/mol)? FeO(l) + Al(l) Fe(l) + Al 2 O 3 (l) (a) 0.842 g (b) 1.70 g (c) 5.10 g (d) 7.58 g (e) 15.3 g

40. What is the mass of aluminum metal that reacts to give 1.00 g of iron? FeO(l) + Al(l) Fe(l) + Al 2 O 3 (l) (a) 0.322 g (b) 0.483 g (c) 0.725 g (d) 0.966 g (e) 1.449 g 41. What is the mass of aluminum oxide (101.96 g/mol) produced from 1.74 g of manganese(iv) oxide (86.94 g/mol)? MnO 2 (l) + Al(l) Mn(l) + Al 2 O 3 (l) (a) 0.988 g (b) 1.36 g (c) 2.04 g (d) 2.22 g (e) 3.06 g 42. What is the mass of aluminum metal that reacts to give 11.1 g of manganese metal? MnO 2 (l) + Al(l) Mn(l) + Al 2 O 3 (l) (a) 3.64 g (b) 4.09 g (c) 5.45 g (d) 7.27 g (e) 8.18 g 43. What is the mass of hydrogen gas released from 2.70 g of aluminum metal and hydrochloric acid? (a) 0.101 g (b) 0.135 g (c) 0.202 g (d) 0.303 g (e) 0.606 g Al(s) + HCl(aq) AlCl 3 (aq) + H 2 (g)

44. What is the mass of aluminum metal that reacts to give 1.00 g of hydrogen gas? (a) 4.46 g (b) 8.90 g (c) 13.4 g (d) 20.0 g (e) 26.7 g Al(s) + HCl(aq) AlCl 3 (aq) + H 2 (g) Limiting Reactant Problems 45. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 1.00 mol A and 1.00 mol B? (a) 1.00 mol (b) 1.50 mol (c) 2.00 mol (d) 3.00 mol A(g) + 2 B(g) 3 C(g) 46. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 1.50 mol A and 3.50 mol B? (a) 1.50 mol (b) 3.50 mol (c) 4.50 mol (d) 5.25 mol A(g) + 2 B(g) 3 C(g) 47. Considering the limiting reactant concept, how many moles of C are produced from the reaction of 2.00 mol A and 4.50 mol B? (a) 2.00 mol (b) 3.00 mol (c) 4.00 mol (d) 4.50 mol A(g) + 3 B(g) 2 C(g)

48. Considering the limiting reactant concept, how many moles of copper(i) sulfide are produced from the reaction of 1.00 mol of copper and 1.00 mol of sulfur? 2 Cu(s) + S(s) Cu 2 S(s) (a) 0.500 mol (b) 1.00 mol (c) 1.50 mol (d) 2.00 mol 49. Considering the limiting reactant concept, how many moles of copper(i) sulfide are produced from the reaction of 3.00 mol of copper and 1.00 mol of sulfur? 2 Cu(s) + S(s) Cu 2 S(s) (a) 1.00 mol (b) 1.50 mol (c) 4.00 mol (d) 6.00 mol 50. Considering the limiting reactant concept, how many moles of cobalt(iii) oxide are produced from the reaction of 1.00 mol of cobalt and 1.00 mol of oxygen gas? 4 Co(s) + 3 O 2 (g) 2 Co 2 O 3 (s) (a) 0.500 mol (b) 0.667 mol (c) 1.50 mol (d) 2.00 mol 51. Considering the limiting reactant, what is the mass of zinc sulfide (97.46 g/mol) produced from 0.750 g of zinc and 0.750 g of sulfur? Zn(s) + S(s) ZnS(s) (a) 0.560 g (b) 1.12 g (c) 1.50 g (d) 2.24 g (e) 2.28 g

52. Considering the limiting reactant, what is the mass of zinc sulfide (97.46 g/mol) produced from 0.750 g of zinc and 0.350 g of sulfur? Zn(s) + S(s) ZnS(s) (a) 0.530 g (b) 1.06 g (c) 1.10 g (d) 1.12 g (e) 2.28 g 53. Considering the limiting reactant, what mass of cobalt(iii) sulfide (214.07 g/mol) is produced from 0.750 g of cobalt and 0.350 g of sulfur? 2 Co(s) + 3 S(s) Co 2 S 3 (s) (a) 0.779 g (b) 1.36 g (c) 2.34 g (d) 2.72 g (e) 5.45 g 54. Considering the limiting reactant, what is the mass of iron produced from 75.0 g of ferrous oxide (71.85 g/mol) and 25.0 g of magnesium metal? FeO(s) + Mg(s) Fe(l) + MgO(s) (a) 28.7 g (b) 29.1 g (c) 57.4 g (d) 58.3 g (e) 100.0 g 55. Considering the limiting reactant, what is the mass of iron produced from 80.0 g of ferrous oxide (71.85 g/mol) and 20.0 g of magnesium metal? FeO(s) + Mg(s) Fe(l) + MgO(s) (a) 23.0 g (b) 31.1 g (c) 45.9 g (d) 62.2 g (e) 100.0 g

56. Considering the limiting reactant, what is the mass of manganese produced from 25.0 g of manganese(iv) oxide (86.94 g/mol) and 25.0 g of aluminum metal? 3 MnO 2 (s) + 4 Al(s) 3 Mn(l) + 2 Al 2 O 3 (s) (a) 15.8 g (b) 38.2 g (c) 47.4 g (d) 50.9 g (e) 67.8 g 57. Considering the limiting reactant, what is the volume of NO gas produced from 30.0 L of nitrogen gas and 40.0 L of oxygen gas? (Assume constant conditions.) N 2 (g) + O 2 (g) 2 NO(g) (a) 30.0 L (b) 40.0 L (c) 60.0 L (d) 80.0 L 58. Considering the limiting reactant, what is the volume of NO gas produced from 30.0 L of nitrogen gas and 20.0 L of oxygen gas? (Assume constant conditions.) N 2 (g) + O 2 (g) 2 NO(g) (a) 20.0 L (b) 30.0 L (c) 40.0 L (d) 60.0 L 59. Considering the limiting reactant, what is the volume of NO 2 gas produced from 3.00 L of NO gas and 2.00 L of oxygen gas? (Assume constant conditions.) 2 NO(g) + O 2 (g) 2 NO 2 (g) (a) 1.00 L (b) 2.00 L (c) 3.00 L (d) 4.00 L

60. Considering the limiting reactant, what is the volume of NO gas produced from 40.0 L of ammonia gas and 40.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 32.0 L (b) 40.0 L (c) 50.0 L (d) 80.0 L 61. Considering the limiting reactant, what is the volume of NO gas produced from 50.0 L of ammonia gas and 60.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 48.0 L (b) 50.0 L (c) 60.0 L (d) 75.0 L 62. Considering the limiting reactant, what is the volume of NO gas produced from 60.0 L of ammonia gas and 50.0 L of oxygen gas? (Assume constant conditions.) 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g) (a) 40.0 L (b) 50.0 L (c) 60.0 L (d) 62.5 L

Percent Yield 63. Starting with 1.550 g of potassium chlorate, a student releases 0.617 g of oxygen gas. If the calculated mass of oxygen gas is 0.607 g, what is the percent yield? (a) 39.2% (b) 39.8% (c) 98.4% (d) 102% (e) 255% 64. Starting with 0.657 g of lead(ii) nitrate, a student collects 0.925 g of precipitate. If the calculated mass of precipitate is 0.914 g, what is the percent yield? (a) 71.0% (b) 71.9% (c) 98.8% (d) 101% (e) 139% 65. Starting with 1.56 g of salicylic acid, a student prepares 1.75 g of aspirin. If the calculated mass of aspirin is 1.88 g, what is the percent yield? (a) 83.0% (b) 89.1% (c) 93.1% (d) 107% (e) 121% 66. The decomposition of 1.500 g of baking soda gave 0.200 L of carbon dioxide gas. If the calculated volume of carbon dioxide gas is 0.210 L, what is the percent yield? (a) 63.5% (b) 70.0% (c) 95.2% (d) 105% (e) 158% 67. The decomposition of 1.500 g of potassium chlorate evolved 405 ml of oxygen gas. If the calculated volume of oxygen gas is 411 ml, what is the percent yield? (a) 65.7% (b) 67.3% (c) 98.5% (d) 101% (e) 148%

68. The decomposition of 1.500 g of sodium nitrate produced 195 ml of oxygen gas. If the calculated volume of oxygen gas is 198 ml, what is the percent yield? (a) 65.7% (b) 68.0% (c) 98.5% (d) 102% (e) 152%

Answer Key 1. A 2. A 3. B 4. B 5. A 6. A 7. D 8. C 9. B 10. B 11. B 12. B 13. B 14. C 15. A 16. B 17. A 18. C 19. B 20. C 21. B 22. B 23. A 24. C 25. C 26. A 27. B 28. D 29. C 30. E 31. E 32. A 33. D 34. A 35. C 36. C 37. B 38. D 39. B 40. A 41. B 42. D 43. D 44. B 45. B 46. C 47. B 48. A 49. A 50. A 51. B 52. B 53. A 54. C 55. C 56. A 57. C 58. C 59. C 60. A 61. A 62. A

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