Stoichiometry
Name:
Mole-Mole Problems
Problems: Solve each of the following problems as directed. Show all your work.
1. How many moles of magnesium are required to react 2.0 mol of hydrochloric acid in a single
replacement reaction? Write the balanced equation and solve the problem.
2.. Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. Write the
balanced equation for this reaction and calculate the number of moles of hydrochloric acid required to
react with 0.87 mol of Al.
3. Glucose (C6H12O6) combines with oxygen gas in the body in a combustion reaction to produce
carbon dioxide gas and water. Write the balanced equation for this reaction. How many moles of
oxygen gas are required to combine with 0.25 mol of glucose? How many moles of carbon dioxide
gas and water would be produced by this reaction?
4. Calcium carbonate combines with hydrochloric acid to produce calcium chloride, water and carbon
dioxide gas. Write the balanced equation for this reaction. How many moles of hydrochloric acid are
required to react with 2.5 mol of calcium carbonate? How many moles of carbon dioxide would
be produced?
5. Zinc reacts with sulfuric acid in a single replacement reaction. How many moles of hydrogen gas will
be produced if 0.36 mol of zinc reacts completely?
Mass-Mass
Solve each of the following as directed. Show all your work.
6. Lead reacts with hydrochloric acid in a single replacement reaction. How many moles of hydrochloric
acid are needed to completely react with 0.36 mol of lead? Assume that the lead forms a +2 cation.
7. Determine the mass of lithium hydroxide produced when 0.38 g of lithium nitride reacts with water
according to the following unbalanced equation:
Li3N +
H2O →
NH3 +
LiOH
8. How many moles of HNO3 will be produced when 0.51 mol of N2O5 reacts according to the following
unbalanced equation?
N2O5 +
H2O →
HNO3
9. What mass of sodium chloride is produced when chlorine gas reacts with 0.29 g of sodium iodide?
(HINT: This is a single replacement reaction)
10. Carbon will react with zinc oxide to produce zinc and carbon dioxide. How many moles of carbon
dioxide will be produced if 0.38 mol of zinc oxide is completely reacted?
11. Determine the mass of carbon dioxide produced when 0.85 g of butane (C4H10) burns.
12. How many moles of sodium bromide will be produced when 0.69 mol of bromine gas reacts with
sodium iodide in a single replacement reaction
13. Determine the mass of antimony produced when 0.46 g of antimony (III) oxide reacts with carbon
according to the following equation:
antimony (III) oxide +
carbon
→
antimony
+
carbon monoxide
14. Phosphorus will react with bromine to produce phosphorus tribromide in a synthesis reaction. How
many grams of phosphorus tribromide will be produced if 0.78 mol of bromine is reacted?
15. What mass of hydrogen peroxide (H2O2) must decompose to produce 0.77 g of water? (HINT: Refer
to your Predicting Products Lab to review this reaction.)
Mass-Volume
Solve each of the following as directed. Show all your work.
16. What mass of carbon monoxide must react with oxygen to produce 0.69 g of carbon dioxide in a
synthesis reaction?
17. Find the mass of sugar (C6H12O6) required to produce 1.82 L of carbon dioxide at STP from the
unbalanced reaction below:
C6H12O6
→
C2H6O +
CO2
18. How many moles of hydrogen will be produced if 0.44 mol of calcium hydride reacts according to the
following equation?
calcium hydride
+
water
→
calcium hydroxide
+
hydrogen
19. How many liters of oxygen are necessary for the combustion of 425 g of sulfur, assuming that the
reaction occurs at STP?
S
+
O2 → SO2
20. Determine the mass of sodium nitrate produced when 0.73 g of Nickel (II) nitrate reacts with sodium
hydroxide in a double replacement reaction? (Nickel is also a +2 cation as a product)
21. How many moles of oxygen will be needed to completely burn 0.38 mol of propane (C3H8)?
22. How many grams of ozone (O3) must decompose to produce 0.87 g of oxygen? Assume only one
product is formed.
23. Find the mass of aluminum required to produce 4.72 L of hydrogen gas at STP from the reaction of
aluminum and sulfuric acid?
24. The compound TNT (trinitrotoluene) decomposes explosively into carbon, carbon monoxide,
hydrogen, and nitrogen. What volumes of hydrogen and nitrogen are produced if 5.8 L of carbon
monoxide is produced? The balanced equation is:
2C7H5(NO2)3
→
2C
+
12CO +
5H2 +
3N2
25. How many moles of water will be produced if 2.35 mol of oxygen reacts to burn benzene (C6H6)?
26. When 9.8 g of aluminum oxide decomposes, how many grams of aluminum metal are produced?
27. How many grams of iodine are produced when 0.72 mol of fluorine react with potassium iodide?
28. How many grams of sodium are required to react with water to produce 5.0 g of sodium hydroxide?
How many grams of hydrogen gas are produced? What volume would this gas occupy at STP?
29. 20.0 g of potassium react with water to produce potassium hydroxide and hydrogen gas. How many
liters would the hydrogen gas occupy at STP?
30. If 30.2 g of aluminum react with hydrochloric acid to produce aluminum chloride and hydrogen gas,
how many liters of hydrogen are produced at STP?
31. How many liters of hydrochloric acid are produced by the reaction of 5.7 L of hydrogen gas with an
equal amount of chlorine gas.
32. How many liters of hydrogen gas are required to react with 0.45 mol of oxygen gas to produce water?
33. How many liters of sulfur dioxide gas are produced from the reaction of sulfur with 26.9 L of oxygen?
34. How many grams of zinc chloride will be produced if zinc is allowed to react with 16.8 L of chlorine
gas at STP?
% Yield
Solve each of the following as directed. Show all your work.
35. Determine the percent yield for the reaction between 6.92 g of potassium and excess oxygen if 7.36 g
of potassium oxide is produced in this direct combination (synthesis) reaction.
36. Determine the percent yield for the reaction between 82.4 g of rubidium and excess oxygen if 39.7 g
of rubidium oxide is formed in this direct combination (synthesis) reaction.
37. Determine the percent yield for the reaction between 28.1 g of Sb4O6 and excess carbon if 17.3 g of
antimony is recovered along with an unknown quantity of carbon monoxide.
38. Determine the percent yield for the reaction between 45.9 g of sodium bromide and excess chlorine
gas if to produce 12.8 g of sodium chloride and an unknown quantity of bromine gas.
39. Determine the percent yield for the reaction between 46.1 g of cesium and excess oxygen if only 28.3
g of cesium oxide is produced.
40. Determine the percent yield for the reaction between 15.8 g of ammonia and excess oxygen to
produce 21.8 g of nitrogen monoxide and some amount of water.
41. Determine the percent yield for the reaction between 98.7 g of Sb2S3 and excess oxygen if 72.4 g of
Sb4O6 is recovered along with an unknown amount of sulfur dioxide.
42. Determine the percent yield for the reaction between 46.5 g of zinc sulfide and excess oxygen if 18.4
g of zinc oxide is recovered along with an unknown quantity of sulfur dioxide.
Mixed Practice Problems
Solve each of the following problems as directed. Show all your work.
43. How many molecules of aluminum bromide can be produced by the reaction of aluminum sulfate with
8.75 g of potassium bromide?
44. How many formula units of calcium hydroxide are produced from the single replacement reaction
of calcium and 0.533 moles of water?
45. How many formula units of iron (III) oxide will be produced from the oxidation of 7.02 x 1025 atoms
of Fe?
46. How many grams of sodium sulfate must be reacted in a double replacement reaction with 82.0 g of
barium phosphate?
47. How many moles of aluminum are produced from the decomposition of 9.8 g of aluminum oxide?
48. How many liters of hydrogen are produced from the single replacement reaction of magnesium with
4.03 x 1024 molecules of hydrochloric acid?
49. What volume of oxygen will be used to burn 91.6 g of cyclohexane (C6H12) in a combustion reaction.
50. Acetylene (C2H2) burns in oxygen in a combustion reaction. What volume of carbon dioxide is
produced when 1.60 L of oxygen is consumed?
51. How many moles of iron (III) oxide are produced in a synthesis reaction from 8.6 L of oxygen?
52. If 25.6 g of sodium iodide reacts with lead (II) nitrate, how many particles of lead (II) iodide are
produced?
Stoichiometry Review
Chapter 9 Practice Test
53. How many moles of aluminum sulfate will be produced from 2.65 mol of copper (II) sulfate
reacted with aluminum metal in a single replacement reaction?
54. If you react 6.0 mol of sodium iodide with lead (II) nitrate, how many grams of lead (II) iodide
will be produced in this double replacement reaction?
55. If 87.0 g of lithium and excess oxygen combine in a synthesis reaction, how many particles of
lithium oxide will be produced?
56. If excess aluminum bromide and 92.0 g of chlorine gas react in a single replacement reaction, how
many grams of aluminum chloride will be produced?
57. 2.76 g of magnesium completely reacts with excess hydrochloric acid in a single replacement
reaction, how many liters of hydrogen gas will be produced?
58. If 3.00 moles of sucrose (C12H22O11) reacts in a combustion reaction, how many liters of
carbon dioxide gas will be produced?
59. How many liters of oxygen are required to completely combust 1.27 x 1024 molecules of
pentane (C5H12) in a complete combustion reaction?
60. What volume of nitrogen gas is needed to react with 175 Liters of hydrogen gas in order
to produce ammonia, NH3?
61. A 5.00 gram piece of copper is placed in a solution of silver nitrate in a single
replacement reaction. If 5.20 grams of silver metal is recovered, determine the percent
yield.
62. When 2.32 g of iron is reacted with excess copper (II) sulfate, 2.51 g of copper is
recovered. Determine the percent yield for copper in this reaction.