Chapter 03
Stoichiometry: Ratios of Combination
1. Calculate the molecular mass of tetraphosphorus decaoxide, P 4O10, a corrosive substance which can be used as a drying
agent.
A. 469.73 amu
B. 283.88 amu
C. 190.97 amu
D. 139.88 amu
E. 94.97 amu
Blooms: 3. Apply
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mas
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
2. Calculate the formula mass of rubidium carbonate, Rb2CO3.
A. 340.43 amu
B. 255.00 amu
C. 230.95 amu
D. 145.47 amu
E. 113.48 amu
Blooms: 3. Apply
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3. Calculate the formula mass of (NH4)3AsO4.
A. 417.80 amu
B. 193.05 amu
C. 165.02 amu
D. 156.96 amu
E. 108.96 amu
Blooms: 3. Apply
Difficulty: Hard
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
4. Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and the manufacture of antiperspirants. Calculate
its molecular or formula mass.
A. 450.06 amu
B. 342.17 amu
C. 315.15 amu
D. 278.02 amu
E. 74.98 amu
Blooms: 3. Apply
Difficulty: Hard
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
5. Calculate the molar mass of Ca(BO2)2·6H2O.
A. 273.87 g/mol
B. 233.80 g/mol
C. 183.79 g/mol
D. 174.89 g/mol
E. 143.71 g/mol
Blooms: 3. Apply
Difficulty: Hard
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-1
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McGraw-Hill Education.
6. Calculate the formula mass of potassium permanganate, KMnO4.
A. 149.91 amu
B. 79.41 amu
C. 127.41 amu
D. 158.04 amu
E. 174.04 amu
Blooms: 3. Apply
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
7. Calculate the molecular mass of menthol, C10H20O.
A. 156 amu
B. 140 amu
C. 29 amu
D. 146 amu
E. 136 amu
Blooms: 3. Apply
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
8. What is the molecular mass of acetaminophen, C8H9NO2?
A. 43 amu
B. 76 amu
C. 151 amu
D. 162 amu
E. 125 amu
Blooms: 3. Apply
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
9. What is the molar mass of nicotine, C10H14N2?
A. 134 g/mol
B. 148 g/mol
C. 158 g/mol
D. 210 g/mol
E. 162 g/mol
Blooms: 3. Apply
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
10. Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass?
A. 26.7%
B. 33.3%
C. 41.4%
D. 42.1%
E. 51.4%
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-2
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McGraw-Hill Education.
11. What is the percent carbon in CH3CH2OH?
A. 13%
B. 26%
C. 35%
D. 46%
E. 52%
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
12. What is the percent sodium in sodium carbonate?
A. 43.4%
B. 11.3%
C. 45.3%
D. 27.7%
E. 21.7%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
13. What is the mass percent of oxygen in barium perchlorate?
A. 4.7%
B. 8.5%
C. 23.4%
D. 38.1%
E. 19.0%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
14. What is the percent sulfur in iron(III) sulfate?
A. 28%
B. 32%
C. 24%
D. 48%
E. 42%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-3
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15. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) 2.
A. 3.28 mol
B. 2.32 mol
C. 0.431 mol
D. 0.305 mol
E. 0.200 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
16. How many moles are present in 17.4 g of lead?
A. 0.0994 moles
B. 1.05 × 1025 moles
C. 0.0840 moles
D. 10.06 moles
E. 11.9 moles
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
17. How many grams are present in 0.885 moles of manganese?
A. 62.1 g
B. 48.6 g
C. 21.5 g
D. 27.5 g
E. 0.016 g
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
18. How many moles of aspirin, C9H8O4, are in a tablet that contains 325 mg of aspirin?
A. 0.00180 moles
B. 0.555 moles
C. 0.467 moles
D. 0.357 moles
E. 2.80 moles
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
19. How many grams are contained in a 0.893 mol sample of methane, CH4?
A. 1.48 × 10–24 g
B. 5.38 × 1023 g
C. 8.64 × 1024 g
D. 14.3 g
E. 18.0 g
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-4
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20. How many moles of ammonia, NH3, are in 13.81 g of NH3?
A. 1.234 moles
B. 0.8107 moles
C. 8.316 × 1024 moles
D. 4.881 × 1023 moles
E. 235.3 moles
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
21. How many grams are contained in a 0.183 mol sample of ammonium phosphate?
A. 1.23 × 10–3 g
B. 617 g
C. 20.7 g
D. 27.3 g
E. 815.1 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
22. Phosphorus pentachloride, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic
reactions. Calculate the number of moles in 38.7 g of phosphorus pentachloride.
A. 5.38 mol
B. 3.55 mol
C. 0.583 mol
D. 0.282 mol
E. 0.186 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
23. Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators.
Calculate the number of moles in 47.51 g of Al2O3.
A. 2.377 mol
B. 2.146 mol
C. 1.105 mol
D. 0.4660 mol
E. 0.4207 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-5
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24. What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?
A. 4.00 × 102 g
B. 25.0 g
C. 17.0 g
D. 4.00 × 10–2 g
E. 2.50 × 10–3 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
25. What is the mass of 0.0250 mol of P 2O5?
A. 35.5 g
B. 5676 g
C. 0.0250 g
D. 1.51 × 1022 g
E. 3.55 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
26. Calculate the mass of 3.00 moles of CF2Cl2.
A. 3.00 g
B. 174 g
C. 363 g
D. 1.81 × 1024 g
E. 40.3
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
27. Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol–1)
A. 2.92 × 1023 molecules
B. 4.73 × 10–25 molecules
C. 1.24 × 1023 molecules
D. 5.83 × 10–24 molecules
E. 1.71 × 1023 molecules
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-6
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McGraw-Hill Education.
28. What is the average mass, in grams, of one atom of iron? (NA = 6.022 × 1023 mol–1)
A. 6.02 × 1023 g
B. 1.66 × 10–24 g
C. 9.27 × 10–23 g
D. 55.85 g
E. 55.85 × 10–23 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
29. What is the mass, in grams, of one arsenic atom? (NA = 6.022 × 1023 mol–1)
A. 5.48 × 10–23 g
B. 33.0 g
C. 74.9 g
D. 1.24 × 10–22 g
E. 8.04 × 1021 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
30. What is the mass of one copper atom? (NA = 6.022 × 1023 mol–1)
A. 1.055 × 10–22 g
B. 63.55 g
C. 1 amu
D. 1.66 × 10–24 g
E. 9.476 × 1021 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
31. What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol–1)
A. 3.88 × 1021 g
B. 2.00 mg
C. 32.06 g
D. 6.44 mg
E. 2.00 × 10–4 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-7
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McGraw-Hill Education.
32. What is the mass of 1.63 × 1021 atoms of silicon? (NA = 6.022 × 1023 mol–1)
A. 2.71 × 10–23 g
B. 4.58 × 1022 g
C. 28.08 g
D. 1.04 × 104 g
E. 7.60 × 10–2 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
33. What is the mass of 7.80 × 1018 carbon atoms? (NA = 6.022 × 1023 mol–1)
A. 1.30 × 10–5 g
B. 6.43 × 103 g
C. 7.80 × 1018 g
D. 1.56 × 10–4 g
E. 12.01 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
34. The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 6.25 mL of water at this
temperature? (NA = 6.022 × 1023 mol–1)
A. 6.27 × 1023 molecules
B. 3.76 × 1024 molecules
C. 2.09 × 1023 molecules
D. 6.02 × 1023 molecules
E. 0.347 molecules
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Stoichiometry and Chemical Reactions
35. Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in
grams of 3.65 × 1020 molecules of sulfur trioxide.
A. 6.06 × 10–4 g
B. 2.91 × 10–2 g
C. 4.85 × 10–2 g
D. 20.6 g
E. 1650 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-8
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McGraw-Hill Education.
36. Calculate the mass in grams of 8.35 × 1022 molecules of CBr4.
A. 0.0217 g
B. 0.139 g
C. 7.21 g
D. 12.7 g
E. 46.0 g
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: The Mole (Definition and Avogadro's Number)
Topic: Stoichiometry and Chemical Reactions
37. Which of the following substances contains the greatest mass of carbon?
A. 100 g CH4
B. 100 g C2H4
C. 100 g CCl4
D. 100 g CH2Cl2
E. 100 g CO2
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
38. Proteins found in humans are polymers that consist of different combinations of 20 amino acids. Proline, one of the 20
amino acids, has the molecular formula, C5H9NO2. If a human protein has 25 proline monomers, how many carbon atoms
from proline are present in the protein?
A. 4 C atoms
B. 25 C atoms
C. 40 C atoms
D. 100 C atoms
E. 125 C atoms
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
39. Smooth muscle myosin is a motor protein that plays a crucial role in the contraction of smooth muscle. If this protein has
a molar mass of 480,000 grams/mol, what is the mass, in grams, of 27 moles of smooth muscle myosin?
A. 1.8 × 104 g
B. 1.3 × 107 g
C. 1.8 × 102 g
D. 2.8 × 1029 g
E. None of the answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
40. As a research assistant, you are asked to prepare a 3.00 liter solution of magnesium sulfate at 45.0 micromoles per liter.
How many moles of magnesium sulfate are required to make this solution?
A. 0.000135 moles
B. 0.0000150 moles
C. 1.35 × 108 moles
D. 1.50 × 107 moles
E. None of the answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Measurement (SI Units)
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
Topic: Study of Chemistry
3-9
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McGraw-Hill Education.
41. Calculate the molar mass of sulfuric acid.
A. 98.086 g/mol
B. 81.078 g/mol
C. 49 g/mol
D. 41 g/mol
E. None of the answers are correct.
Blooms: 3. Apply
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
42. What is the name given to the quantitative relationship between the substances that are consumed and produced in a
chemical reaction?
A. Law of definite proportions
B. Law of molecular balance
C. Percent composition
D. Stoichiometry
E. Percent equivalency
Blooms: Remember
Difficulty: Easy
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Topic: Stoichiometry and Chemical Reactions
43. Balance the following equation:
B2O3(s) + HF(l) → BF3(g) + H2O(l)
A. B2O3(s) + 6HF(l) → 2BF3(g) + 3H2O(l)
B. B2O3(s) + H6F6 (l) → B2F6(g) + H6O3(l)
C. B2O3(s) + 2HF(l) → 2BF3(g) + H2O(l)
D. B2O3(s) + 3HF(l) → 2BF3(g) + 3H2O(l)
E. B2O3(s) + 6HF(l) → 2BF3(g) + 6H2O(l)
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
44. Balance the following equation:
UO2(s) + HF(l) → UF4(s) + H2O(l)
A. UO2(s) + 2HF(l) → UF4(s) + H2O(l)
B. UO2(s) + 4HF(l) → UF4(s) + 2H2O(l)
C. UO2(s) + H4F4(l) → UF4(s) + H4O2(l)
D. UO2(s) + 4HF(l) → UF4(s) + 4H2O(l)
E. UO2(s) + 8HF(l) → 2UF4(s) + 4H2O(l)
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
45. Balance the following equation for the combustion of benzene:
C6H6(l) + O2(g) → H2O(g) + CO2(g)
A. C6H6(l) + 9O2(g) → 3H2O(g) + 6CO2(g)
B. C6H6(l) + 9O2(g) → 6H2O(g) + 6CO2(g)
C. 2C6H6(l) + 15O2(g) → 6H2O(g) + 12CO2(g)
D. C6H6(l) + 15O2(g) → 3H2O(g) + 6CO2(g)
E. 2C6H6(l) + 9O2(g) → 6H2O(g) + 12CO2(g)
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-10
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McGraw-Hill Education.
46. Balance the following equation:
C8H18O3(l) + O2(g) → H2O(g) + CO2(g)
A. C8H18O3(l) + 8O2(g) → 9H2O(g) + 8CO2(g)
B. C8H18O3(l) + 11O2(g) → 9H2O(g) + 8CO2(g)
C. 2C8H18O3(l) + 22O2(g) → 9H2O(g) + 16CO2(g)
D. C8H18O3(l) + 13O2(g) → 18H2O(g) + 8CO2(g)
E. 2C8H18O3(l) + 17O2(g) → 18H2O(g) + 16CO2(g)
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
47. Balance the following equation:
Ca3(PO4)2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)
A. Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + P4(s)
B. Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) → 3CaSiO3(s) + 14CO(g) + P4(s)
C. Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + 2P4(s)
D. 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + P4(s)
E. 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + 4P4(s)
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
48. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole
numbers?
___ Na + ___ H2O → ___ NaOH + ___ H2
A. 1
B. 2
C. 3
D. 4
E. 5
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
49. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole
numbers?
___ Al4C3 + ___ H2O → ___ Al(OH)3 + ___ CH4
A. 3
B. 4
C. 6
D. 12
E. 24
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
50. What is the coefficient of O2 when the following equation is properly balanced with the smallest set of whole numbers?
__ C2H4 + __ O2 → __ CO2 + __ H2O
A. 1
B. 2
C. 3
D. 4
E. 6
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-11
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McGraw-Hill Education.
51. When a chemical equation is balanced, it will have a set of whole number coefficients that cannot be reduced to smaller
whole numbers. What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced?
___ C7H14 + ___ O2 → ___ CO2 + ___ H2O
A. 42
B. 21
C. 11
D. 10
E. None of these answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
52. What is the coefficient preceding O2 when the following combustion reaction of a fatty acid is properly balanced using
the smallest set of whole numbers?
__ C18H36O2 + __ O2 → __ CO2 + __ H2O
A. 1
B. 8
C. 9
D. 26
E. 27
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
53. What is the coefficient of H2SO4 when the following equation is properly balanced with the smallest set of whole
numbers?
___ Ca3(PO4)2 + ___ H2SO4 → ___ CaSO4 + ___ H3PO4
A. 3
B. 8
C. 10
D. 11
E. None of these answers is correct.
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
54. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers?
___ PCl3(l) + ___ H2O(l) → ___ H3PO3(aq) + ___ HCl(aq)
A. 1
B. 2
C. 3
D. 5
E. None of these answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
55. What is the coefficient of O2 when the following equation is properly balanced with the smallest set of whole numbers?
___ CH3OH + ___ O2 → ___ CO2 + ___ H2O
A. 1
B. 2
C. 3
D. 7
E. None of these answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-12
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
56. Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the
coefficients? (Don't forget to include coefficients of one.)
__ SF4 + __ H2O → __ H2SO3 + __ HF
A. 4
B. 6
C. 7
D. 9
E. None of these answers is correct.
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
57. Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the
coefficients? (Don't forget to include coefficients of one.)
___ Cr + ___ H2SO4 → ___ Cr2(SO4)3 + ___H2
A. 4
B. 9
C. 11
D. 13
E. 15
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
58. Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the
coefficients? (Don't forget to include coefficients of one.)
___ Al + ___ H2SO4 → ___ Al2(SO4)3 + ___ H2
A. 3
B. 5
C. 6
D. 9
E. 12
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
59. Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the
coefficients? (Don't forget to include coefficients of one.)
___ CH4 + ___ Cl2 → ___ CCl4 + ___ HCl
A. 4
B. 6
C. 8
D. 10
E. 12
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-13
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
60. What is the empirical formula for a 100-g sample containing 87.42 g of nitrogen and 12.58 g of hydrogen?
A. NH
B. N2H
C. NH2
D. NH3
E. N7H
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
61. What is the empirical formula for a sample containing 81.70% carbon and 18.29% hydrogen?
A. CH
B. CH3
C. C2H6
D. CH4
E. C3H8
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
62. An oxide of gadolinium contains 86.76 mass % Gd. What is its empirical formula?
A. Gd2O3
B. Gd3O2
C. Gd3O4
D. Gd13O2
E. GdO
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
63. Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its empirical
formula?
A. HNO
B. H2NO2
C. HN6O16
D. HN16O7
E. H2NO3
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-14
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
64. A certain compound of bromine and fluorine is used to make UF 6, which is an important chemical in the processing and
reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. What is its empirical formula?
A. BrF
B. BrF2
C. Br2F3
D. Br3F
E. BrF3
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
65. A compound containing chromium and silicon contains 73.52 mass percent chromium. Determine its empirical formula.
A. CrSi3
B. Cr2Si3
C. Cr3Si
D. Cr3Si2
E. Cr4Si3
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
66. What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4%
fluorine by mass?
A. U2F
B. U3F4
C. UF4
D. UF6
E. UF8
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
67. Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen.
When 0.6943 g of terephthalic acid was subjected to combustion analysis, it produced 1.471 g CO2 and 0.226 g H2O. What
is its empirical formula?
A. C2H3O4
B. C3H4O2
C. C4H3O2
D. C5H12O4
E. C2H2O
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-15
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
68. Hydroxyl ammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. If its molar mass is
between 94 and 98 g/mol, what is its molecular formula?
A. NH2O5
B. N2H4O4
C. N3H3O3
D. N4H8O2
E. N2H2O4
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
69. The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound
is 284.5 g/mol. What is the molecular formula of the compound?
A. C10H6O
B. C9H18O
C. C16H28O4
D. C20H12O2
E. C18H36O2
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
70. A compound was discovered whose composition by mass is 85.6% C and 14.4% H. Which of these formulas could be
the molecular formula of this compound?
A. CH4
B. C2H4
C. C3H4
D. C2H6
E. C3H8
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
71. Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and
dichlorine oxide (used as a bleach for wood, pulp and textiles).
SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g)
If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?
A. 0.800 mol
B. 0.400 mol
C. 0.200 mol
D. 0.100 mol
E. 0.0500 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-16
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
72. Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis).
Al(s) + Br2(l) → Al2Br6(s) [unbalanced]
How many moles of Al are needed to form 2.43 mol of Al 2Br6?
A. 7.29 mol
B. 4.86 mol
C. 2.43 mol
D. 1.62 mol
E. 1.22 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
73. Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of
aluminum, in uranium processing, and in the frosting of light bulbs).
2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g)
How many moles of NH3 are needed to react completely with 13.6 mol of F 2?
A. 34.0 mol
B. 27.2 mol
C. 6.80 mol
D. 5.44 mol
E. 2.27 mol
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
74. What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?
A. 3.26 g
B. 0.629 g
C. 13.04 g
D. 17.63 g
E. 6.52 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
75. What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?
A. 25.8 g
B. 12.9 g
C. 78.2 g
D. 38.7 g
E. 77.4 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
76. What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia?
A. 11.2 g
B. 0.06 g
C. 22.4 g
D. 16.5 g
E. 44.8 g
Difficulty: Hard
Gradable: automatic
3-17
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McGraw-Hill Education.
77. What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate,
carbon dioxide, and water?
A. 28.1 g
B. 14.04 g
C. 4.96 g
D. 7.02 g
E. 400.0 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
78. How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to
produce lead(II) chloride and nitric acid?
A. 5.82 g
B. 14.33 g
C. 0.086 g
D. 11.64 g
E. 16.52 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
79. How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen
gas?
A. 8.62 g
B. 34.5 g
C. 4.31 g
D. 40.1 g
E. 17.2 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
80. What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?
A. 12.8 g
B. 25.6 g
C. 6.39 g
D. 0.399 g
E. 51.1 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-18
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
81. What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g
of sulfur tetrafluoride?
3SCl2(l) + 4NaF(s) → SF4(g) + S2Cl2(l) + 4NaCl(s)
A. 1.94 kg
B. 1.51 kg
C. 754 g
D. 205 g
E. 51.3 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
82. Phosphine, an extremely poisonous and highly reactive gas, reacts with oxygen gas to form tetraphosphorus decaoxide
and water.
PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced]
Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.
A. 1880 g
B. 940. g
C. 900. g
D. 470. g
E. 56.3 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
83. Potassium chlorate (used in fireworks, flares, and safety matches) forms oxygen and potassium chloride when heated.
KClO3(s) → KCl(s) + O2(g) [unbalanced]
What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?
A. 223 g
B. 99.1 g
C. 10.3 g
D. 6.86 g
E. 4.60 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
84. Aluminum metal reacts with chlorine gas to form solid aluminum trichloride. What mass of chlorine gas is required to
react completely with 163 g of aluminum?
A. 214 g
B. 286 g
C. 321 g
D. 428 g
E. 643 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-19
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
85. Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate
and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?
A. 151 g
B. 123 g
C. 50.3 g
D. 37.7 g
E. 9.41 g
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
86. How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO 2 and 30.0 g of HCl according to the
following balanced chemical equation?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
A. 6.52 g
B. 7.29 g
C. 13.0 g
D. 14.6 g
E. 58.4 g
Difficulty: Hard
Gradable: automatic
87. Hydrochloric acid can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq) → 2HCl(g) + Na2SO4(s)
What mass of HCl can be prepared from 2.00 mol H2SO4 and 150. g NaCl?
A. 2.57 g
B. 46.8 g
C. 93.6 g
D. 146 g
E. 167g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
88. What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S 8?
8Fe(s) + S8(s) → 8FeS(s)
A. 186 g
B. 142 g
C. 119 g
D. 14.8 g
E. 0.169 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-20
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
89. What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2?
2SO2 + O2 → 2SO3
A. 10.0 g
B. 12.5 g
C. 22.5 g
D. 55.0 g
E. 77.5 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
90. What is the maximum number of grams of ammonia, NH3, which can be obtained from the reaction of 10.0 g of H2 and
80.0 g of N2?
N2 + 3H2 → 2NH3
A. 34.1 g
B. 48.6 g
C. 56.3 g
D. 90.0 g
E. 97.3 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
91. How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?
A. 90. g
B. 36 g
C. 42 g
D. 45 g
E. 108 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
92. What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following
chemical equation?
2Al + Cr2O3 → Al2O3 + 2Cr
A. 15.1 g
B. 30.2 g
C. 67.4 g
D. 99.9 g
E. 104 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-21
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McGraw-Hill Education.
93. If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia, what is the limiting reactant and what mass of
ammonia is produced?
A. Hydrogen is the limiting reactant and 0.22 g of ammonia are produced.
B. Nitrogen is the limiting reactant and 2.07 g of ammonia are produced.
C. Nitrogen is the limiting reactant and 4.15 g of ammonia are produced.
D. Hydrogen is the limiting reactant and 23.5 g of ammonia are produced.
E. Hydrogen is the limiting reactant and 15.8 g of ammonia are produced.
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
94. If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of
calcium oxide is produced?
A. Calcium is the limiting reactant and 47.2 g of calcium oxide are produced
B. Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced
C. Calcium is the limiting reactant and 47.2 g of calcium oxide are produced
D. Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced
E. Calcium is the limiting reactant and 23.6 g of calcium oxide are produced
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
95. If 31.3 g of manganese(II) chloride, 48.3 g of chlorine gas, and 25.7 g of water react to produce manganese(IV) oxide
and hydrochloric acid, what is the limiting reactant and what mass of hydrochloric acid is produced?
A. manganese(II) chloride is the limiting reactant and 9.07 g of hydrochloric acid is produced
B. chlorine is the limiting reactant and 99.3 g of hydrochloric acid is produced
C. chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced
D. manganese(II) chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced
E. water is the limiting reactant and 52.0 g of hydrochloric acid is produced
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-22
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McGraw-Hill Education.
96. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for
organic reactions. A mixture of 82.49 g of aluminum and 117.65 g of oxygen is allowed to react. Identify the limiting
reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.
A. Oxygen is the limiting reactant; 19.81 g of aluminum remain.
B. Oxygen is the limiting reactant; 35.16 g of aluminum remain.
C. Aluminum is the limiting reactant; 16.70 g of oxygen remain.
D. Aluminum is the limiting reactant; 35.16 g of oxygen remain.
E. Aluminum is the limiting reactant; 44.27 g of oxygen remain.
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
97. Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron.
A mixture of 41.0 g of magnesium and 175.0 g of iron(III) chloride is allowed to react. Identify the limiting reactant and
determine the mass of the excess reactant present in the vessel when the reaction is complete.
A. Limiting reactant is Mg; 7.4 g of FeCl3 remain.
B. Limiting reactant is Mg; 46.5 g of FeCl3 remain.
C. Limiting reactant is FeCl3; 1.7 g of Mg remain.
D. Limiting reactant is FeCl3; 37.8 g of Mg remain.
E. Limiting reactant is Mg; 134.0 g of FeCl3 remain.
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
98. Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the
limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of
potassium to form potassium chloride.
A. Chlorine is the limiting reactant; 1.14 g of potassium remain.
B. Potassium is the limiting reactant; 2.00 g of chlorine remain.
C. Potassium is the limiting reactant; 2.47 g of chlorine remain.
D. Chlorine is the limiting reactant; 3.07 g of potassium remain.
E. Potassium is the limiting reactant; 4.50 g of chlorine remain.
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Nomenclature
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
3-23
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McGraw-Hill Education.
99. Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of
phosphorus and 38.7 g of oxygen produce 43.3 g of P 4O6, what is the percent yield for the reaction?
A. 57.5%
B. 48.8%
C. 38.0%
D. 89.4%
E. 16.3%
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
100. If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent yield?
PCl3(g) + Cl2(g) → PCl5(g)
A. 94.6%
B. 66.3%
C. 57.3%
D. 51.3%
E. 48.6%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
101. Methanol (CH3OH) is converted to bromomethane (CH3Br) as follows:
CH3OH + HBr → CH3Br + H2O
If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield?
A. 12.9%
B. 33.8%
C. 40.9%
D. 59.1%
E. 82.6%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
102. The first step in the Ostwald process for producing nitric acid is as follows:
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g).
If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this
reaction?
A. 29.0%
B. 32.9%
C. 49.5%
D. 61.8%
E. 77.3%
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
3-24
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McGraw-Hill Education.
103. One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona,
Na3(CO3)(HCO3)·2H2O.
2Na3(CO3)(HCO3)·2H2O(s) → 3Na2CO3(s) + CO2(g) + 5H2O(g)
When 1.00 metric ton (1.00 × 103 kg) of trona is decomposed, 0.650 metric ton of Na2CO3 is recovered. What is the percent
yield of this reaction?
A. 92.4%
B. 72.1%
C. 65.0%
D. 48.1%
E. 35.0%
Blooms: 4. Analyze
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
104. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr 2O3 with 8.00 g of
aluminum according to the chemical equation below?
2Al + Cr2O3 → Al2O3 + 2Cr
A. 7.7 g
B. 15.4 g
C. 27.4 g
D. 30.8 g
E. 49.9 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
105. Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows:
4NH3 + 5O2 → __________4NO + 6H2O
What is the maximum amount of water that may be produced if 40.0 g NH 3 and 50.0 g O2 are mixed and allowed to react?
A. 1.56mol
B. 1.88 mol
C. 3.52 mol
D. 3.91 mol
E. 2.35 mol
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
106. What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole of V2O5 with 6.0
mole of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A. 1.0 mol
B. 1.6 mol
C. 2.0 mol
D. 2.4 mol
E. 4.0 mol
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-25
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McGraw-Hill Education.
107. What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0
moles of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A. 1.0 mol
B. 1.6 mol
C. 2.0 mol
D. 0.80 mol
E. 3.2 mol
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
108. What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium
based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A. 11.2 g
B. 5.6 g
C. 22.4 g
D. 40.0 g
E. 20.3 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
109. What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g
of carbon according to the following chemical equation?
Al2O3 + 3C → 2Al + 3CO
A. 15.9 g
B. 31.8 g
C. 44.9 g
D. 63.6 g
E. 67.4 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
110. When octane (C8H18) is burned in a particular internal combustion engine, the yield of products (carbon dioxide and
water) is 93%. What mass of carbon dioxide will be produced in this engine when 15.0 g of octane is burned with 15.0 g of
oxygen gas?
A. 13 g
B. 12 g
C. 21 g
D. 54 g
E. 43 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-26
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
111. Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form
nitrogen trichloride?
A.
B.
C.
D.
E.
Blooms: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-27
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McGraw-Hill Education.
112. Which could represent the reaction mixture after the complete combustion of acetaldehyde, CH3CHO?
A.
B.
C.
D.
E.
Blooms: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Mole Conversions
Subtopic: Types of Chemical Reactions (Acid-Base, REDOX, Displacement, etc.)
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-28
Copyright © 2016 McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of
McGraw-Hill Education.
113. Suppose white atoms (W) and black atoms (B) react according to the following balanced chemical equation.
2W + B → BW2
If the initial reaction mixture is prepared as follows, what will the final reaction mixture be once the reaction is complete?
A.
B.
C.
D.
E.
Blooms: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Mole Conversions
Topic: Stoichiometry and Chemical Reactions
3-29
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McGraw-Hill Education.
114.Which of the following is least helpful in balancing an equation?
A. Use a balance sheet to keep track of the number of elements.
B. Try different coefficients and subscripts to balance the number of atoms.
C. Begin with elements that appear only once on each side of the equation.
D. Change only the coefficients to balance the number of atoms.
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
115. The empirical formula of C6H6 is CH.
TRUE
Blooms: 4. Analyze
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
116. The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
117. Many compounds can be represented with the same empirical formula.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
118. There is only one distinct empirical formula for each compound that exists.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
119. The molecular formula is a whole number multiple of the empirical formula.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
120. In a correctly balanced equation, the number of reactant molecules must equal the number of product molecules.
FALSE
Blooms: 3. Apply
Difficulty: Easy
Gradable: automatic
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
121. The limiting reactant is the reactant with the smallest initial mass.
FALSE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-30
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McGraw-Hill Education.
122. The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
123. Many compounds can be represented with the same empirical formula.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
124. There is only one distinct empirical formula for each compound that exists.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
125. The molecular formula is a whole number multiple of the empirical formula.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Topic: Stoichiometry and Chemical Reactions
126. The percent yield can be determined by dividing the actual yield by the theoretical yield and multiplying this value by
100%.
TRUE
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
127. ______________ is defined by the following equation
# of atoms × atomic mass of element
× 100%
molecular or formula mass of compound
Percent by mass of an element
Blooms: 2. Understand
Difficulty: Medium
Gradable: automatic
Subtopic: Mass Percent Composition
Subtopic: Molar Mass
Topic: Stoichiometry and Chemical Reactions
128. What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole
numbers?
___ Na + ___ H2O → ___ NaOH + ___ H2
2
Blooms: 4. Analyze
Difficulty: Medium
Gradable: automatic
Subtopic: Mole Conversions
Subtopic: Types of Chemical Reactions (Acid-Base, REDOX, Displacement, etc.)
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-31
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McGraw-Hill Education.
129. What is the coefficient of O2 when the following combustion reaction of a fatty acid is properly balanced using the
smallest set of whole numbers?
___ C18H36O2 + ___ O2 → ___ CO2 + ___ H2O
26
Blooms: 2. Understand
Difficulty: Medium
Gradable: automatic
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
130. The ______________ is defined by the following equation
percent yield
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Topic: Stoichiometry and Chemical Reactions
131. The ______________ is the one component that is completely consumed during a chemical reaction.
limiting reactant
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Topic: Stoichiometry and Chemical Reactions
132. The ______________ is the amount of product that forms when all the limiting reactant reacts to form the desired
product.
theoretical yield
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
133. The ____ is the amount of product physically collected from a chemical reaction and is typically less than the
theoretical yield.
actual yield
Blooms: 2. Understand
Difficulty: Easy
Gradable: automatic
Subtopic: Reaction Yield
Topic: Stoichiometry and Chemical Reactions
134. What is the theoretical yield of calcium oxide, in grams, that can be produced by the reaction of 5.61 g of V2O5 with
7.44 g of calcium to produce vanadium and calcium oxide? (Show all your work)
8.65 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: manual
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-32
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McGraw-Hill Education.
135. Ammonia reacts with oxygen to form nitrogen monoxide and water. What is the theoretical yield and the percent yield
if 17.25 g of nitrogen monoxide is produced when 21.50 g of ammonia and 26.85 g of oxygen react? (Show all your work)
Theoretical yield = 20.14 g of NO and the percent yield = 85.63%
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: manual
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
136. How many grams of magnesium oxide remain after 18.50 g of magnesium oxide reacts with 30.30 g hydrochloric acid
to produce magnesium chloride and water?
1.75 g
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: manual
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
137. The insecticide DDT was formerly in widespread use, but now it is severely restricted owing to its adverse
environmental effects. It is prepared as follows:
C2HCl3O
C6H5Cl →
C14H9Cl5 + H2O [unbalanced]
+
chloral chlorobenzene DDT
Suppose 10.00 g of chloral was put in a container with 10.00 g of chlorobenzene and allowed to react.
a. What is the maximum amount, in mol, of DDT which could be formed?
b. What is the limiting reactant?
c. What is the percent yield, if 12.15 g of DDT is produced?
a. 0.0444 mol DDT b. Chlorobenzene is the limiting reactant. c. 77.16%
Blooms: 5. Evaluate
Difficulty: Hard
Gradable: manual
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Limiting Reactant
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Reaction Yield
Subtopic: Writing and Balancing Chemical Equations
Topic: Stoichiometry and Chemical Reactions
3-33
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McGraw-Hill Education.
Category
Blooms: 2. Understand
Blooms: 3. Apply
Blooms: 4. Analyze
Blooms: 5. Evaluate
Blooms: Remember
Difficulty: Easy
Difficulty: Hard
Difficulty: Medium
Gradable: automatic
Gradable: manual
Subtopic: Calculating Amounts of Reactant and Product (including solutions)
Subtopic: Chemical Formulas
Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)
Subtopic: Limiting Reactant
Subtopic: Mass Percent Composition
Subtopic: Measurement (SI Units)
Subtopic: Molar Mass
Subtopic: Mole Conversions
Subtopic: Molecules and Ions
Subtopic: Nomenclature
Subtopic: Reaction Yield
Subtopic: Structure of the Atom
Subtopic: The Mole (Definition and Avogadro's Number)
Subtopic: Types of Chemical Reactions (Acid-Base, REDOX, Displacement, etc.)
Subtopic: Writing and Balancing Chemical Equations
Topic: Components of Matter
Topic: Stoichiometry and Chemical Reactions
Topic: Study of Chemistry
# of Questions
17
11
78
28
1
32
53
52
133
4
52
20
20
29
14
1
88
98
8
15
14
6
10
2
47
32
135
1
3-34
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McGraw-Hill Education.