Chemistry 4th Edition by Julia Burdge – Test Bank

 

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Sample Test

Chapter 03

Stoichiometry: Ratios of Combination

 

1.Calculate the molecular mass of tetraphosphorusdecaoxide, P4O10, a corrosive substance whichcan be used as a drying agent.

469.             469.73 amu

470.             283.88 amu

471.             190.97 amu

472.             139.88 amu

473.             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.

3.   340.43 amu

4.   255.00 amu

5.   230.95 amu

6.   145.47 amu

7.   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.

4.   417.80 amu

B.193.05 amu

165.             165.02 amu

166.             156.96 amu

167.             108.96 amu

Blooms: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Molar Mass

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

4.   Aluminumsulfate, Al2(SO4)3, is used in tanning leather, purifying water, and the manufacture ofantiperspirants. Calculate its molecular or formula mass.

5.   450.06 amu

B.342.17 amu

315.             315.15 amu

316.             278.02 amu

317.             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.

6.   273.87 g/mol

B.233.80 g/mol

183.             183.79 g/mol

184.             174.89 g/mol

185.             143.71 g/mol

Blooms: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Molar Mass

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

6.   Calculate the formula mass of potassium permanganate, KMnO4.

7.   149.91 amu

8.   79.41 amu

9.   127.41 amu

10.                158.04 amu

11.                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.

8.   156 amu

9.   140 amu

10.                29 amu

11.                146 amu

12.                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?

9.   43 amu

10.                76 amu

11.                151 amu

12.                162 amu

13.                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?

10.                134 g/mol

11.                148 g/mol

12.                158 g/mol

13.                210 g/mol

14.                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 insucrose, by mass?

11.                26.7%

12.                33.3%

13.                41.4%

D.42.1%

51.                51.4%

Blooms: 4. Analyze

Difficulty: Medium

Gradable: automatic

Subtopic: Mass Percent Composition

Subtopic: Molar Mass

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

 

 

11.                What is the percent carbon in CH3CH2OH?

12.                13%

13.                26%

14.                35%

15.                46%

16.                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?

13.                43.4%

14.                11.3%

15.                45.3%

16.                27.7%

17.                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?

14.                4.7%

15.                8.5%

16.                23.4%

17.                38.1%

18.                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?

15.                28%

16.                32%

17.                24%

18.                48%

19.                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

 

 

 

 

 

 

15.                Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2.

16.                3.28 mol

17.                2.32 mol

18.                0.431 mol

19.                0.305 mol

20.                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?

17.                0.0994 moles

18.                1.05 × 1025 moles

19.                0.0840 moles

20.                10.06 moles

21.                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?

18.                62.1 g

19.                48.6 g

20.                21.5 g

21.                27.5 g

22.                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?

19.                0.00180 moles

20.                0.555 moles

21.                0.467 moles

22.                0.357 moles

23.                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?

20.                1.48 × 10–24 g

21.                5.38 × 1023 g

22.                8.64 × 1024 g

23.                14.3 g

24.                18.0 g

Blooms: 4. Analyze

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

 

 

 

20.                How many moles of ammonia, NH3, are in 13.81 g of NH3?

21.                1.234 moles

22.                0.8107 moles

23.                8.316 × 1024 moles

24.                4.881 × 1023 moles

25.                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?

22.                1.23 × 10–3 g

23.                617 g

24.                20.7 g

25.                27.3 g

26.                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 catalystfor certain organic reactions. Calculate the number of moles in 38.7 g of phosphoruspentachloride.

23.                5.38 mol

24.                3.55 mol

25.                0.583 mol

26.                0.282 mol

27.                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 ofelectrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

24.                2.377 mol

25.                2.146 mol

26.                1.105 mol

27.                0.4660 mol

28.                0.4207 mol

Blooms: 4. Analyze

Difficulty: Medium

Gradable: automatic

Subtopic: Molar Mass

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

 

 

 

 

 

 

 

24.                What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

25.                4.00 × 102 g

26.                25.0 g

27.                17.0 g

28.                4.00 × 10–2 g

29.                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 P2O5?

26.                35.5 g

27.                5676 g

28.                0.0250 g

29.                1.51 × 1022 g

30.                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.

27.                3.00 g

28.                174 g

29.                363 g

30.                1.81 × 1024 g

31.                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)

28.                2.92 × 1023 molecules

29.                4.73 × 10–25 molecules

30.                1.24 × 1023 molecules

31.                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

 

 

 

 

 

 

 

 

 

 

 

28.                What is the average mass, in grams, of one atom of iron? (NA = 6.022 × 1023 mol–1)

29.                6.02 × 1023 g

30.                1.66 × 10–24 g

C.9.27 × 10–23 g

55.                55.85 g

56.                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)

30.                5.48 × 10–23 g

31.                33.0 g

32.                74.9 g

D.1.24 × 10–22 g

8.   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

63.                63.55 g

64.                1 amu

65.                1.66 × 10–24 g

66.                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)

32.                3.88 × 1021 g

33.                2.00 mg

34.                32.06 g

D.6.44 mg

2.   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

 

 

 

 

 

 

 

 

 

32.                What is the mass of 1.63 × 1021 atoms of silicon? (NA = 6.022 × 1023 mol–1)

33.                2.71 × 10–23 g

34.                4.58 × 1022 g

35.                28.08 g

36.                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)

34.                1.30 × 10–5 g

35.                6.43 × 103 g

36.                7.80 × 1018 g

D.1.56 × 10–4 g

12.                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 ofwater at this temperature? (NA = 6.022 × 1023 mol–1)

35.                6.27 × 1023 molecules

36.                3.76 × 1024 molecules

C.2.09 × 1023 molecules

6.   6.02 × 1023 molecules

7.   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.

36.                6.06 × 10–4 g

37.                2.91 × 10–2 g

C.4.85 × 10–2 g

20.                20.6 g

21.                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

 

 

 

 

 

 

 

36.                Calculate the mass in grams of 8.35 × 1022 molecules of CBr4.

37.                0.0217 g

38.                0.139 g

39.                7.21 g

40.                12.7 g

41.                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?

38.                100 g CH4

B.100 g C2H4

1.   100 g CCl4

2.   100 g CH2Cl2

3.   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 has25 proline monomers, how many carbon atoms from proline are present in the protein?

39.                4 C atoms

40.                25 C atoms

41.                40 C atoms

42.                100 C atoms

43.                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 smoothmuscle. If this protein has a molar mass of 480,000 grams/mol, what is the mass, in grams, of 27moles of smooth muscle myosin?

40.                1.8 × 104 g

B.1.3 × 107 g

1.   1.8 × 102 g

2.   2.8 × 1029 g

3.   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 at45.0 micromoles per liter. How many moles of magnesium sulfate are required to make thissolution?

41.                0.000135 moles

42.                0.0000150 moles

43.                1.35 × 108 moles

44.                1.50 × 107 moles

45.                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

 

41.                Calculate the molar mass of sulfuric acid.

A.98.086 g/mol

81.                81.078 g/mol

82.                49 g/mol

83.                41 g/mol

84.                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 consumedand produced in a chemical reaction?

43.                Law of definite proportions

44.                Law of molecular balance

45.                Percent composition

46.                Stoichiometry

47.                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)

1.   B2O3(s) + H6F6 (l) → B2F6(g) + H6O3(l)

2.   B2O3(s) + 2HF(l) → 2BF3(g) + H2O(l)

3.   B2O3(s) + 3HF(l) → 2BF3(g) + 3H2O(l)

4.   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)

1.   UO2(s) + 2HF(l) → UF4(s) + H2O(l)

B.UO2(s) + 4HF(l) → UF4(s) + 2H2O(l)

1.   UO2(s) + H4F4(l) → UF4(s) + H4O2(l)

2.   UO2(s) + 4HF(l) → UF4(s) + 4H2O(l)

3.   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)

1.   C6H6(l) + 9O2(g) → 3H2O(g) + 6CO2(g)

2.   C6H6(l) + 9O2(g) → 6H2O(g) + 6CO2(g)

C.2C6H6(l) + 15O2(g) → 6H2O(g) + 12CO2(g)

1.   C6H6(l) + 15O2(g) → 3H2O(g) + 6CO2(g)

2.   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

 

 

 

46.                Balance the following equation:

C8H18O3(l) + O2(g) → H2O(g) + CO2(g)

1.   C8H18O3(l) + 8O2(g) → 9H2O(g) + 8CO2(g)

B.C8H18O3(l) + 11O2(g) → 9H2O(g) + 8CO2(g)

1.   2C8H18O3(l) + 22O2(g) → 9H2O(g) + 16CO2(g)

2.   C8H18O3(l) + 13O2(g) → 18H2O(g) + 8CO2(g)

3.   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)

1.   Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + P4(s)

2.   Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) → 3CaSiO3(s) + 14CO(g) + P4(s)

3.   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)

1.   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 smallestset of whole numbers?

___ Na + ___ H2O → ___ NaOH + ___ H2

1.   1

2.   2

3.   3

4.   4

5.   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 smallestset of whole numbers?

___ Al4C3 + ___ H2O → ___ Al(OH)3 + ___ CH4

1.   3

2.   4

3.   6

4.   12

5.   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 setof whole numbers?

__ C2H4 + __ O2 → __ CO2 + __ H2O

1.   1

2.   2

3.   3

4.   4

5.   6

Blooms: 4. Analyze

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

 

 

 

51.                When a chemical equation is balanced, it will have a set of whole number coefficients that cannotbe reduced to smaller whole numbers. What is the coefficient for O2 when the followingcombustion reaction of a hydrocarbon is balanced?

___ C7H14 + ___ O2 → ___ CO2 + ___ H2O

1.   42

2.   21

3.   11

4.   10

5.   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 isproperly balanced using the smallest set of whole numbers?

__ C18H36O2 + __ O2 → __ CO2 + __ H2O

1.   1

2.   8

3.   9

4.   26

5.   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 smallestset of whole numbers?

___ Ca3(PO4)2 + ___ H2SO4 → ___ CaSO4 + ___ H3PO4

1.   3

2.   8

3.   10

4.   11

5.   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 smallestset of whole numbers?

___ PCl3(l) + ___ H2O(l) → ___ H3PO3(aq) + ___ HCl(aq)

1.   1

2.   2

3.   3

4.   5

5.   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 setof whole numbers?

___ CH3OH + ___ O2 → ___ CO2 + ___ H2O

1.   1

2.   2

3.   3

4.   7

5.   None of these answers is correct.

Blooms: 4. Analyze

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

 

 

56.                Once the following equation is balanced with the smallest set of whole number coefficients, what isthe sum of the coefficients? (Don’t forget to include coefficients of one.)

__ SF4 + __ H2O → __ H2SO3 + __ HF

1.   4

2.   6

3.   7

4.   9

5.   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 isthe sum of the coefficients? (Don’t forget to include coefficients of one.)

___ Cr + ___ H2SO4 → ___ Cr2(SO4)3 + ___H2

1.   4

2.   9

3.   11

4.   13

5.   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 isthe sum of the coefficients? (Don’t forget to include coefficients of one.)

___ Al + ___ H2SO4 → ___ Al2(SO4)3 + ___ H2

1.   3

2.   5

3.   6

4.   9

5.   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 isthe sum of the coefficients? (Don’t forget to include coefficients of one.)

___ CH4 + ___ Cl2 → ___ CCl4 + ___ HCl

1.   4

2.   6

3.   8

4.   10

5.   12

Blooms: 4. Analyze

Difficulty: Easy

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

 

 

 

 

 

 

 

 

 

 

 

 

 

60.                What is the empirical formula for a 100-g sample containing 87.42 g of nitrogen and 12.58 g ofhydrogen?

61.                NH

62.                N2H

63.                NH2

64.                NH3

65.                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?

62.                CH

63.                CH3

64.                C2H6

65.                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

1.   Gd3O2

2.   Gd3O4

3.   Gd13O2

4.   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. Whatis its empirical formula?

64.                HNO

B.H2NO2

1.   HN6O16

2.   HN16O7

3.   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