Chemical Equation Calculations

Mole Relationships Chemical Equation Calculations 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 1

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 2

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 3

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 4

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 5

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) 6

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) 7

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 Types of Stoichiometry Problems Mass Mass Problems 47. 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) 8

48. 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) 49. 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) 50. 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) 51. 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) 9

52. 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) 53. 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) 54. 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) 55. 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 10

56. 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 57. 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 58. 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 59. 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) 11

60. 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) The Limiting Reactant Concept 85. 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) 86. 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) 87. 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) 12

88. 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 89. 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 90. 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 Limiting Reactant Problems 91. 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 13

92. 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 93. 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 94. 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 95. 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 14

96. 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 Note: When working with gases you can use volumes instead of moles. 97. 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 98. 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 99. 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 15

100. 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 101. 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 102. 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 Empirical Formula 85. If 0.500 mol of copper combines with 0.250 mol of sulfur, what is the empirical formula of the copper sulfide product? (a) CuS (b) Cu 2 S (c) CuS 2 (d) Cu 5 S 5 16

86. If 0.300 mol of lead combines with 0.300 mol of sulfur, what is the empirical formula of the lead sulfide product? (a) PbS (b) Pb 2 S (c) PbS 2 (d) Pb 3 S 3 87. If 0.225 mol of tin combines with 0.450 mol of sulfur, what is the empirical formula of the tin sulfide product? (a) SnS (b) Sn 2 S (c) SnS 2 (d) Sn 3 S 3 88. If 6.00 mol of cobalt combines with 9.00 mol of sulfur, what is the empirical formula of the cobalt sulfide product? (a) Co 2 S 3 (b) Co 3 S 2 (c) Co 6 S 9 (d) Co 9 S 6 89. If 0.250 mol of red phosphorus reacts with 0.375 mol of yellow sulfur, what is the empirical formula of the product? (a) P 2 S 3 (b) P 2 S 5 (c) P 3 S 2 (d) P 5 S 2 90. If 0.250 mol of red phosphorus reacts with 0.625 mol of yellow sulfur, what is the empirical formula of the product? (a) P 2 S 3 (b) P 2 S 5 (c) P 3 S 2 (d) P 5 S 2 17

91. If 0.587 g of nickel metal reacts with 1.065 g of chlorine gas, what is the empirical formula of the nickel chloride product? (a) NiCl (b) NiCl 2 (c) NiCl 3 (d) Ni 2 Cl 3 (e) Ni 3 Cl 2 92. If 1.823 g of cobalt metal react with 0.495 g of oxygen gas, what is the empirical formula of the cobalt oxide product? (a) CoO (b) CoO 2 (c) CoO 3 (d) Co 2 O 3 (e) Co 3 O 2 93. If 1.216 g of cobalt metal react with 0.495 g of oxygen gas, what is the empirical formula of the cobalt oxide product? (a) CoO (b) CoO 2 (c) CoO 3 (d) Co 2 O 3 (e) Co 3 O 2 94. If 1.000 g of tin metal reacts with 0.640 g of fluorine gas, what is the empirical formula of the product? (a) SnF (b) SnF 2 (c) SnF 4 (d) SnF 10 (e) Sn 2 F 3 95. If 1.888 g of bismuth metal react with sulfur to give 2.323 g of bismuth sulfide, what is the empirical formula of the product? (a) BiS (b) BiS 2 (c) BiS 3 (d) Bi 2 S 3 (e) Bi 3 S 2 18

96. If 1.500 g of vanadium metal react with oxygen gas to give 2.679 g of vanadium oxide, what is the empirical formula of the product? (a) VO (b) V 2 O 3 (c) V 2 O 5 (d) V 3 O 2 (e) V 5 O 2 97. Acetylene is used in oxyacetylene gas welding. Calculate the empirical formula for acetylene given its percent composition: 92.25% C and 7.75% H. (a) CH (b) CH 2 (c) CH 8 (d) C 8 H 8 (e) C 12 H 98. Fructose is a sugar found in fruit and honey. Calculate the empirical formula for fructose given its percent composition: 40.00% C, 6.72% H, and 53.29% O. (a) CHO (b) CH 2 O (c) CHO 2 (d) C 3 H 6 O 3 (e) C 6 HO 8 99. Butyric acid is the odor of rancid cheese. Calculate the empirical formula for butyric acid given its percent composition: 54.53% C, 9.15% H, and 36.32% O. (a) CHO (b) C 2 H 4 O (c) C 2 H 3 O (d) C 5 H 9 O 2 (e) C 6 H 9 O 3 19

Mole Relationships 1. A 2. A 3. B 4. B 5. A 6. A 7. D 8. C 9. C 10. B 11. B 12. B Mol-Mol Relationship 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 Mass-Mass Problems 47. E 48. A 49. D 50. A 51. C 52. C 53. B 54. D 55. B 56. A 57. B 58. D 59. D 60. B 61. A 62. E 63. A 64. E 65. D 66. B 67. A 68. E 69. E 70. C 71. D 72. B 73. C 74. E Lim. React. Concept 85. B 86. C 87. B 88. A 89. A 90. A Lim. React Problems 91. B 92. B 93. A 94. C 95. C 96. A 97. C 98. C 99. C 100. A 101. A 102. A Empirical Formulas 85. B 86. A 87. C 88. A 89. A 90. B 91. C 92. A 93. D 94. C 95. D 96. C 97. A 98. B 99. B 20