1. The balanced equation of 4Al + 3O2 → 2Al2O3 can be interpreted by saying that 1 mol of Al:
8.1
Reacts with 3 mol of O2
Produces 1 mol of Al2O3
Produces 0.5 mol Al2O3
Reacts with 2 mol of O2
Cannot react with O2

2. The balanced equation of 4Al + 3O2 → 2Al2O3 can be interpreted by saying that 1 mol of Al:
8.1
Reacts with 3 mol of O2
Produces 1 mol of Al2O3
Produces 0.5 mol Al2O3
Reacts with 2 mol of O2
Cannot react with O2

3. How many moles of oxygen are needed to produce 6 mol of Fe2O3 in the following equation: Fe + 3O2 → 2Fe2O3?
8.2 3 1 6 9 18

4. How many moles of oxygen are needed to produce 6 mol of Fe2O3 in the following equation: 4Fe + 3O2 → 2Fe2O3?
8.2 3 1 6 9 18

5. How many moles of gaseous oxygen are required for the complete combustion of 4.0 mol of butane (C4H10)?
8.3
4.0
8.0 13 26 52

6. How many moles of gaseous oxygen are required for the complete combustion of 4.0 mol of butane (C4H10)?
8.3
4.0
8.0 13 26 52

7. How many grams of oxygen are required to completely burn 5
How many grams of oxygen are required to completely burn 5.90 g of C3H8 in the following unbalanced equation: C3H8(g) + O2(g) → CO2(g) + H2O(g)?
8.4
5.90 g
21.4 g
4.28 g
10.7 g
29.5 g

8. How many grams of oxygen are required to completely burn 5
How many grams of oxygen are required to completely burn 5.90 g of C3H8 in the following unbalanced equation: C3H8(g) + O2(g) → CO2(g) + H2O(g)?
8.4
5.90 g
21.4 g
4.28 g
10.7 g
29.5 g

9. How many grams of aluminum sulfate are produced from 2
How many grams of aluminum sulfate are produced from 2.67 mol sulfuric acid in the following unbalanced equation: Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)?
8.5
305 g
457 g
272 g
914 g
342 g

10. How many grams of aluminum sulfate are produced from 2
How many grams of aluminum sulfate are produced from 2.67 mol sulfuric acid in the following unbalanced equation: Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)?
8.5
305 g
457 g
272 g
914 g
342 g

11. How many moles of phosphorus are required to produce 15
How many moles of phosphorus are required to produce 15.5 g P4O6 in the following equation: 4P(s) + 3O2(g) → P4O6(s)?
8.6
mol
mol
mol
mol
mol

12. How many moles of phosphorus are required to produce 15
How many moles of phosphorus are required to produce 15.5 g P4O6 in the following equation: 4P(s) + 3O2(g) → P4O6(s)?
8.6
mol
mol
mol
mol
mol

13. How many moles of oxygen gas are produced from the following decomposition of 3.0 mol of Al2O3, assuming a 85% yield: 2Al2O3 → 4Al + 3O2?
8.7
4.5 mol
3.8 mol
5.3 mol
3.0 mol
4.2 mol

14. How many moles of oxygen gas are produced from the following decomposition of 3.0 mol of Al2O3, assuming a 85% yield: 2Al2O3 → 4Al + 3O2 ?
8.7
4.5 mol
3.8 mol
5.3 mol
3.0 mol
4.2 mol

15. How many kg of methane (CH4) are produced from 25
How many kg of methane (CH4) are produced from 25.0 kg of hydrogen in the following catalytic methanation: 3H2 + CO → CH4 + H2O?
8.8
115 kg
74.3 kg
134 kg
25.0 kg
66.2 kg

16. How many kg of methane (CH4) are produced from 25
How many kg of methane (CH4) are produced from 25.0 kg of hydrogen in the following catalytic methanation: 3H2 + CO → CH4 + H2O?
8.8
115 kg
74.3 kg
134 kg
25.0 kg
66.2 kg

17. How many moles of water are produced from the combustion of 3
How many moles of water are produced from the combustion of 3.5 mol of hydrogen and 5.2 mol of oxygen?
8.9
7.0 mol
5.2 mol
3.5 mol
10. mol
1.8 mol

18. How many moles of water are produced from the combustion of 3
How many moles of water are produced from the combustion of 3.5 mol of hydrogen and 5.2 mol of oxygen?
8.9
7.0 mol
5.2 mol
3.5 mol
10. mol
1.8 mol

19. How many grams of NO are produced from the oxidation of 14
How many grams of NO are produced from the oxidation of 14.5 g of NH3 by 12.2 g of O2 in the following equation: 4NH3 + 5O2 → 4NO + 6H2O?
8.10
0.305 g g g g
0.851 g

20. How many grams of NO are produced from the oxidation of 14
How many grams of NO are produced from the oxidation of 14.5 g of NH3 by 12.2 g of O2 in the following equation: 4NH3 + 5O2 → 4NO + 6H2O?
8.10
0.305 g g g g
0.851 g

21. How many grams of the excess reagent are left over after the reaction of 4.36 g of Al and 8.50 g HCl in the following unbalanced equation: Al + HCl → AlCl3 + H2?
8.11
2.26 g
4.14 g
2.3 g
21.5 g
10.4 g

22. How many grams of the excess reagent are left over after the reaction of 4.36 g of Al and 8.50 g HCl in the following unbalanced equation: Al + HCl → AlCl3 + H2?
8.11
2.26 g
4.14 g
2.3 g
21.5 g
10.4 g

23. How many molecules of water are produced from the combustion of 2
How many molecules of water are produced from the combustion of 2.56 mol of octane in the following equation: 2C8H O2 → 16CO2 + 18H2O?
8.12
1.08 x 1025
2.77 x 1025
2.56 x 1025
1.39 x 1025
6.02 x 1023

24. How many molecules of water are produced from the combustion of 2
How many molecules of water are produced from the combustion of 2.56 mol of octane in the following equation: 2C8H O2 → 16CO2 + 18H2O?
8.12
1.08 x 1025
2.77 x 1025
2.56 x 1025
1.39 x 1025
6.02 x 1023

25. How many molecules of oxygen are produced from the decomposition of 8
How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation: 2H2O2 → 2H2 + O2?
8.13
8.75 x 1024
7.74 x 1022
1.55 x 1022
5.27 x 1024
6.02 x 1023

26. How many molecules of oxygen are produced from the decomposition of 8
How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation: 2H2O2 → 2H2 + O2?
8.13
8.75 x 1024
7.74 x 1022
1.55 x 1022
5.27 x 1024
6.02 x 1023

27. How many molecules of ammonia are produced from 7
How many molecules of ammonia are produced from 7.54 x 1025 molecules of hydrogen in the following equation: 3H2 + N2 → 2NH3?
8.14
molecules
7.54 x molecules
5.03 x molecules
1.51 x molecules
6.02 x molecules

28. How many molecules of ammonia are produced from 7
How many molecules of ammonia are produced from 7.54 x 1025 molecules of hydrogen in the following equation: 3H2 + N2 → 2NH3?
8.14
molecules
7.54 x molecules
5.03 x molecules
1.51 x molecules
6.02 x molecules

29. How many molecules of CO2 are produced from the combustion of 2 molecules of C8H18 and 5 molecules of O2? (Hint: This is a tricky question.)
8.15
1.93 x 1024 molecules
molecules
9.63 x 1024 molecules
molecules
3.2 x molecules

30. How many molecules of CO2 are produced from the combustion of 2 molecules of C8H18 and 5 molecules of O2? (Hint: This is a tricky question.)
8.15
1.93 x 1024 molecules
molecules
9.63 x 1024 molecules
molecules
3.2 x molecules

31. What is the theoretical yield of acetic acid when 22
What is the theoretical yield of acetic acid when 22.5 g of methanol reacts with 32.0 g of carbon monoxide in the following equation: CH3OH + CO → HC2H3O2?
8.16
24.2 g
32.0 g
42.2 g
68.6 g
84.4 g

32. What is the theoretical yield of acetic acid when 22
What is the theoretical yield of acetic acid when 22.5 g of methanol reacts with 32.0 g of carbon monoxide in the following equation: CH3OH + CO → HC2H3O2?
8.16
24.2 g
32.0 g
42.2 g
68.6 g
84.4 g

33. What is the theoretical yield of SO3 from the combustion of 3
What is the theoretical yield of SO3 from the combustion of 3.00 mol of S and 6.00 mol of O2?
8.17
3.00 g
320. g
2.00 g
4.00 g
240. g

34. What is the theoretical yield of SO3 from the combustion of 3
What is the theoretical yield of SO3 from the combustion of 3.00 mol of S and 6.00 mol of O2?
8.17
3.00 g
320. g
2.00 g
4.00 g
240. g

35. What is the theoretical yield of MgO from the combustion of 5
What is the theoretical yield of MgO from the combustion of 5.25 x 1023 atoms of Mg and x 1023 molecules of O2?
8.18 g
2.17 x g g
3.78 x g g

36. What is the theoretical yield of MgO from the combustion of 5
What is the theoretical yield of MgO from the combustion of 5.25 x 1023 atoms of Mg and x 1023 molecules of O2?
8.18 g
2.17 x g g
3.78 x g g

37. Which reactant is in excess from the reaction of 35
Which reactant is in excess from the reaction of 35.0 g of hydrogen with 276 g of oxygen to form water?
8.19 H O O2 H2
H2O

38. Which reactant is in excess from the reaction of 35
Which reactant is in excess from the reaction of 35.0 g of hydrogen with 276 g of oxygen to form water?
8.19 H O O2 H2
H2O

39. Its coefficient in the balanced equation is the smallest one.
Which of the following statements is NOT correct about the limiting reactant in a reaction?
8.20
It has the lowest mass.
Its coefficient in the balanced equation is the smallest one.
It has the highest mass.
It doesn’t react completely.
All of the above

40. Its coefficient in the balanced equation is the smallest one.
Which of the following statements is NOT correct about the limiting reactant in a reaction?
8.20
It has the lowest mass.
Its coefficient in the balanced equation is the smallest one.
It has the highest mass.
It doesn’t react completely.
All of the above

41. In the combustion of a sample of methane, the theoretical yield is 28
In the combustion of a sample of methane, the theoretical yield is 28.9 g CO2. When a chemistry student performed the experiment, the yield was g CO2. What is the percent yield of their reaction by the student?
8.21
100. %
91.3 %
109 %
85.2 %
55.9 %

42. In the combustion of a sample of methane, the theoretical yield is 28
In the combustion of a sample of methane, the theoretical yield is 28.9 g CO2. When a chemistry student performed the experiment, the yield was g CO2. What is the percent yield of their reaction by the student?
8.21
100. %
91.3 %
109 %
85.2 %
55.9 %

43. An experiment had a percent yield of 91
An experiment had a percent yield of 91.8% and a calculated theoretical yield of 28.2 g. How many grams were actually produced?
8.22
25.9 g
2.50 g
92.0 g
28.5 g
30.7 g

44. An experiment had a percent yield of 91
An experiment had a percent yield of 91.8% and a calculated theoretical yield of 28.2 g. How many grams were actually produced?
8.22
25.9 g
2.50 g
92.0 g
28.5 g
30.7 g

45. Both are used up at the same time.
What is the limiting reactant for the reaction between 18.2 g of K and 8.38 g of water in the following unbalanced reaction: K + H2O → KOH + H2?
8.23 K
H2O
KOH H2
Both are used up at the same time.

46. Both are used up at the same time.
What is the limiting reactant for the reaction between 18.2 g of K and 8.38 g of water in the following unbalanced reaction: K + H2O → KOH + H2?
8.23 K
H2O
KOH H2
Both are used up at the same time.

47. 5. 0 kg of hydrogen is reacted with 31 kg of oxygen
5.0 kg of hydrogen is reacted with 31 kg of oxygen. The experiment yields 28 kg of water. Calculate the percent yield of the reaction.
8.24
40. %
63 %
80. %
90. %
161%

48. 5. 0 kg of hydrogen is reacted with 31 kg of oxygen
5.0 kg of hydrogen is reacted with 31 kg of oxygen. The experiment yields 28 kg of water. Calculate the percent yield of the reaction.
8.24
40. %
63 %
80. %
90. %
161%

49. 4. 25 mol of Cl2 are reacted with 1. 49 mol NaOH. 12
4.25 mol of Cl2 are reacted with 1.49 mol NaOH g of NaClO3 are produced. Calculate the percent yield of the following reaction: Cl2 + 6 NaOH → 5 NaCl + NaClO3 + 3H2O.
8.25
28.1%
47.3%
79.9%
82.8%
91.2%

50. 4. 25 mol of Cl2 are reacted with 1. 49 mol NaOH. 12
4.25 mol of Cl2 are reacted with 1.49 mol NaOH g of NaClO3 are produced. Calculate the percent yield of the following reaction: Cl2 + 6 NaOH → 5 NaCl + NaClO3 + 3H2O.
8.25
28.1%
47.3%
79.9%
82.8%
91.2%