Chapter 10napavalley.edu/people/sfawl/Documents/Chem 120/Mole... · Web view3.How many moles of carbon monoxide react with 1 mol of oxygen gas according to the ... (III) chloride

Chemical Equation CalculationsMole Relationships

1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation?

H2(g) + Cl2(g) 2 HCl(g)

(a) 1 mol(b) 2 mol(c) 3 mol(d) 4 mol(e) none of the above

2. Assuming similar conditions, how many liters of chlorine gas react to produce 2 L of hydrogen chloride gas?

H2(g) + Cl2(g) 2 HCl(g)

(a) 1 L(b) 2 L(c) 3 L(d) 4 L(e) none of the above

3. How many moles of carbon monoxide react with 1 mol of oxygen gas according to the balanced chemical equation?

2 CO(g) + O2(g) 2 CO2(g)


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4. Assuming similar conditions, how many liters of carbon monoxide gas react to produce 2 L of carbon dioxide gas?

2 CO(g) + O2(g) 2 CO2(g)


5. How many moles of water vapor, H2O, react with 1 mol of charcoal, C, according to the balanced chemical equation?

C(s) + H2O(g) CO(g) + H2(g)


6. Assuming similar conditions, how many liters of water vapor, H2O, react to produce 1 L of hydrogen gas?

C(s) + H2O(g) CO(g) + H2(g)


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) CS2(g)

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(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 I2(s) 2 CrI3(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) + O2(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) + O2(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 Cl2(g) 2 AuCl3(s)

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(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?

__H2(g) + __I2(g) __HI(g)

(a) 0.500 mol(b) 1.00 mol(c) 2.00 mol(d) 4.00 mol(e) none of the above

14. How many moles of hydrogen iodide are produced from 1.00 mol of iodine?

__H2(g) + __I2(g) __HI(g)


15. How many moles of hydrogen gas react to yield 1.00 mol of hydrogen iodide?

__H2(g) + __I2(g) __HI(g)


16. How many moles of water are produced from 1.00 mol of hydrogen peroxide?

__H2O2(l) __H2O(l) + __O2(g)

(a) 0.500 mol

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(b) 1.00 mol(c) 2.00 mol(d) 4.00 mol(e) none of the above

17. How many moles of oxygen are produced from 1.00 mol of hydrogen peroxide?

__H2O2(l) __H2O(l) + __O2(g)


18. How many moles of hydrogen peroxide decompose to give 1.00 mol of oxygen?

__H2O2(l) __H2O(l) + __O2(g)


19. How many moles of oxygen gas react with 1.00 mol NO?UV

__NO(g) + __O2(g) __NO2(g)


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20. How many moles of nitrogen dioxide gas are produced from 1.00 mol NO?

UV__NO(g) + __O2(g) __NO2(g)


21. How many moles of oxygen gas react to yield 1.00 mol NO2?UV

__NO(g) + __O2(g) __NO2(g)


22. How many moles of water react with 5.00 mol of lithium metal?__Li(s) + __H2O(l) __LiOH(aq) + __H2(g)


23. How many moles of hydrogen gas are produced from 5.00 mol of water?__Li(s) + __H2O(l) __LiOH(aq) + __H2(g)


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24. How many moles of lithium metal react to yield 5.00 mol of hydrogen gas?

__Li(s) + __H2O(l) __LiOH(aq) + __H2(g)


25. How many moles of water react with 0.500 mol of calcium metal?__Ca(s) + __H2O(l) __Ca(OH)2(aq) + __H2(g)


26. How many moles of hydrogen gas are produced from 0.500 mol of water?

__Ca(s) + __H2O(l) __Ca(OH)2(aq) + __H2(g)


27. How many moles of calcium metal react to yield 0.500 mol of hydrogen gas?

__Ca(s) + __H2O(l) __Ca(OH)2(aq) + __H2(g)


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28. How many moles of oxygen gas react with 0.100 mol of pentane, C5H12?spark

__C5H12 (g) + __O2(g) __CO2(g) + __H2O(g)


29. How many moles of water are produced from 0.100 mol pentane, C5H12?spark

__C5H12 (g) + __O2(g) __CO2(g) + __H2O(g)


30. How many moles of oxygen gas react to yield 0.100 mol water?spark

__C5H12 (g) + __O2(g) __CO2(g) + __H2O(g)


Types of Stoichiometry Problems

Mass–Mass Problems

47. What is the mass of silver metal produced from 6.35 g of copper?__Cu(s) + __AgNO3(aq) __Cu(NO3)2(aq) + __Ag(s)

(a) 0.187 g(b) 0.540 g(c) 0.747 g(d) 1.08 g(e) 21.6 g

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48. What is the mass of copper metal that yields 0.500 g of silver?__Cu(s) + __AgNO3(aq) __Cu(NO3)2(aq) + __Ag(s)

(a) 0.147 g(b) 0.294 g(c) 0.425 g(d) 0.589 g(e) 1.70 g

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)?

__FeBr3(s) + __AgNO3(aq) __AgBr(s) + __Fe(NO3)3(aq)

(a) 0.940 g(b) 0.627 g(c) 1.88 g(d) 5.64 g(e) 3.76 g

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?

__FeBr3(s) + __AgNO3(aq) __AgBr(s) + __Fe(NO3)3(aq)

(a) 0.0986 g(b) 0.148 g(c) 0.296 g(d) 0.592 g(e) 0.888 g

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)?

__Pb(NO3)2(aq) + __KI(s) __PbI2(s) + __KNO3(aq)

(a) 0.149 g(b) 0.598 g(c) 1.15 g(d) 2.31 g(e) 4.61 g

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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?

__Pb(NO3)2(aq) + __KI(s) __PbI2(s) + __KNO3(aq)

(a) 0.0900 g(b) 0.180 g(c) 0.360 g(d) 0.694 g(e) 2.78 g

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)?

__CaCl2(s) + __Na3PO4(aq) __Ca3(PO4)2(s) + __NaCl(aq)

(a) 0.0662 g(b) 0.517 g(c) 0.596 g(d) 1.55 g(e) 4.65 g

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?

__CaCl2(s) + __Na3PO4(aq) __Ca3(PO4)2(s) + __NaCl(aq)

(a) 0.264 g(b) 0.358 g(c) 0.931 g(d) 1.06 g(e) 8.38 g

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) + __Al2O3(l)

(a) 0.842 g(b) 1.70 g(c) 5.10 g(d) 7.58 g(e) 15.3 g

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56. What is the mass of aluminum metal that reacts to give 1.00 g of iron?

__FeO(l) + __Al(l) __Fe(l) + __Al2O3(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)?

__MnO2(l) + __Al(l) __Mn(l) + __Al2O3(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?

__MnO2(l) + __Al(l) __Mn(l) + __Al2O3(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?

__Al(s) + __HCl(aq) __AlCl3(aq) + __H2(g)

(a) 0.101 g(b) 0.135 g(c) 0.202 g(d) 0.303 g(e) 0.606 g

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60. What is the mass of aluminum metal that reacts to give 1.00 g of hydrogen gas?

__Al(s) + __HCl(aq) __AlCl3(aq) + __H2(g)

(a) 4.46 g(b) 8.90 g(c) 13.4 g(d) 20.0 g(e) 26.7 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(g) + 2 B(g) 3 C(g)(a) 1.00 mol(b) 1.50 mol(c) 2.00 mol(d) 3.00 mol(e) none of the above





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?

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2 Cu(s) + S(s) Cu2S(s)


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) Cu2S(s)

(a) 1.00 mol(b) 1.50 mol (c) 4.00 mol(d) 6.00 mol(e) none of the above

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 O2(g) 2 Co2O3(s)


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

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)

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(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) Co2S3(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

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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 MnO2(s) + 4 Al(s) 3 Mn(l) + 2

Al2O3(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.)

N2(g) + O2(g) 2 NO(g)

(a) 30.0 L(b) 40.0 L(c) 60.0 L(d) 80.0 L(e) none of the above

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.)

N2(g) + O2(g) 2 NO(g)


99. Considering the limiting reactant, what is the volume of NO2 gas produced from 3.00 L of NO gas and 2.00 L of oxygen gas? (Assume constant conditions.)

2 NO(g) + O2(g) 2 NO2(g)

(a) 1.00 L(b) 2.00 L

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(c) 3.00 L(d) 4.00 L(e) none of the above

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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 NH3(g) + 5 O2(g) 4 NO(g) + 6

H2O(g)



4 NH3(g) + 5 O2(g) 4 NO(g) + 6

H2O(g)



4 NH3(g) + 5 O2(g) 4 NO(g) + 6

H2O(g)


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) Cu2S(c) CuS2(d) Cu5S5

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(e) none of the above

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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) Pb2S(c) PbS2(d) Pb3S3(e) none of the above

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) Sn2S(c) SnS2(d) Sn3S3(e) none of the above

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) Co2S3(b) Co3S2(c) Co6S9(d) Co9S6(e) none of the above

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) P2S3(b) P2S5(c) P3S2(d) P5S2(e) none of the above

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) P2S3(b) P2S5(c) P3S2(d) P5S2(e) none of the above

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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) NiCl2(c) NiCl3(d) Ni2Cl3(e) Ni3Cl2

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) CoO2(c) CoO3(d) Co2O3(e) Co3O2

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) CoO2(c) CoO3(d) Co2O3(e) Co3O2

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) SnF2(c) SnF4(d) SnF10(e) Sn2F3

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) BiS2(c) BiS3(d) Bi2S3(e) Bi3S2

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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) V2O3(c) V2O5(d) V3O2(e) V5O2

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) CH2(c) CH8(d) C8H8(e) C12H

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) CH2O(c) CHO2(d) C3H6O3(e) C6HO8

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) C2H4O(c) C2H3O(d) C5H9O2(e) C6H9O3

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Mole Relationships1. A2. A3. B4. B5. A6. A7. D8. C9. C10. B11. B12. B

Mol-Mol Relationship

13. B14. C15. A16. B17. A18. C19. B20. C21. B22. B23. A24. C25. C26. A27. B28. D29. C30. E

Mass-Mass Problems

47. E48. A49. D50. A51. C52. C53. B54. D55. B56. A57. B

58. D59. D60. B61. A62. E63. A64. E65. D66. B67. A68. E69. E70. C71. D72. B73. C74. E

Lim. React. Concept

85. B86. C87. B88. A89. A90. A

Lim. React Problems

91. B92. B93. A94. C95. C96. A97. C98. C99. C100.A101.A102.A

Empirical Formulas

85. B86. A87. C88. A89. A

90. B91. C92. A93. D94. C95. D96. C97. A98. B99. B

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