Test Bank For Chemistry The Molecular Nature of Matter and Change 8th Edition by Martin Silberberg

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INSTANT DOWNLOAD COMPLETE TEST BANK WITH ANSWERS

Chemistry The Molecular Nature of Matter and Change 8th Edition by Martin SilberbergLUTGENS – TEST BANK

 

Sample  Questions

 

 

Chapter 3 Test Bank

Stoichiometry of Formulas and Equations

 

1. Calcium fluoride, CaF₂, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass.
2. 118.15 g/mol
3. 99.15 g/mol
4. C.07 g/mol
5. 59.08 g/mol
6. 50.01 g/mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

2. Calculate the molar mass of tetraphosphorus decaoxide, P₄O₁₀, a corrosive substance which can be used as a drying agent.
3. 469.73 g/mol
4. B.89 g/mol
5. 190.97 g/mol
6. 139.88 g/mol
7. 94.97 g/mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

3. Calculate the molar mass of rubidium carbonate, Rb₂CO₃.
4. 340.43 g/mol
5. 255.00 g/mol
6. C.94 g/mol
7. 145.47 g/mol
8. 113.48 g/mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

4. Calculate the molar mass of (NH₄)₃AsO₄.
5. 417.80 g/mol
6. B.03 g/mol
7. 165.02 g/mol
8. 156.96 g/mol
9. 108.96 g/mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

5. Aluminum sulfate, Al₂(SO₄)₃, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.
6. 450.06 g/mol
7. B.15 g/mol
8. 315.15 g/mol
9. 278.02 g/mol
10. 74.98 g/mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

6. Calculate the molar mass of Ca(BO₂)₂·6H₂O.
7. 273.87 g/mol
8. B.79 g/mol
9. 183.79 g/mol
10. 174.89 g/mol
11. 143.71 g/mol

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

7. Magnesium fluoride is used in the ceramics and glass industry. What is the mass of 1.72 mol of magnesium fluoride?
8. 43.3 g
9. 62.3 g
10. 74.5 g
11. 92.9 g
12. E. 107 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

8. Sodium bromate is used in a mixture which dissolves gold from its ores. Calculate the mass in grams of 4.68 mol of sodium bromate.
9. A. 706 g
10. 482 g
11. 383 g
12. 32.2 g
13. 0.0310 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

9. What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?
10. 4.00 × 10² g
11. B.0 g
12. 17.0 g
13. 4.00 × 10^–2 g
14. 2.50 × 10^–3 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

10. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)₂.
11. 3.28 mol
12. 2.32 mol
13. 0.431 mol
14. D.305 mol
15. 0.200 mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

11. Phosphorus pentachloride, PCl₅, 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 PCl₅.
12. 5.38 mol
13. 3.55 mol
14. 0.583 mol
15. 0.282 mol
16. E.186 mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

12. 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.
13. 2.377 mol
14. 2.146 mol
15. 1.105 mol
16. D.4660 mol
17. 0.4207 mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

13. Which of the following samples has the most moles of the compound?
14. A.0 g of Li₂O
15. 75.0 g of CaO
16. 200.0 g of Fe₂O₃
17. 50.0 g of CO₂
18. 100.0 g of SO₃

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

14. Calculate the number of oxygen atoms in 29.34 g of sodium sulfate, Na₂SO₄.
15. 1.244 × 10²³ O atoms
16. B.976 × 10²³ O atoms
17. 2.409 × 10²⁴ O atoms
18. 2.915 × 10²⁴ O atoms
19. 1.166 × 10²⁵ O atoms

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

15. A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8 g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?
16. A.0 × 10²²
17. 2.2 × 10²²
18. 5.8 × 10²³
19. 1.7 × 10²⁵
20. 1.8 × 10²⁵

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

16. Which of the following samples contains the greatest total number atoms?
17. 50.0 g of Li₂O
18. 75.0 g of CaO
19. C.0 g of Fe₂O₃
20. 50.0 g of CO₂
21. 100.0 g of SO₃

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

17. A single atom of hydrogen has a mass of 1.0 amu, while a mole of hydrogen atoms has a mass of 1.0 g. Select the correct conversion factor between atomic mass units and grams.
18. 1 amu = 1 g exactly
19. 1 amu = 6.0 × 10²³ g
20. C. 1 g = 6.0 × 10²³ amu
21. 1 g = 1.7 × 10^–24 amu
22. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

18. How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4πr³/3; density of mercury = 13.6 g/cm³)
19. A.1 × 10¹⁹
20. 1.7 × 10²⁰
21. 2.1 × 10²²
22. 1.7 × 10²³
23. None of these choices are correct.

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

19. Potassium dichromate, K₂Cr₂O₇, is used in tanning leather, decorating porcelain, and water proofing fabrics. Calculate the number of chromium atoms in 78.82 g of K₂Cr₂O₇.
20. 9.490 × 10²⁵ Cr atoms
21. 2.248 × 10²⁴ Cr atoms
22. 1.124 × 10²⁴ Cr atoms
23. D.227 × 10²³ Cr atoms
24. 1.613 × 10²³ Cr atoms

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Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

20. 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 SO₃.
21. 6.06 × 10^–4 g
22. 2.91 × 10^–2 g
23. C.85 × 10^–2 g
24. 20.6 g
25. 1650 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

21. Calculate the mass in grams of 8.35 × 10²² molecules of CBr₄.
22. 0.0217 g
23. 0.139 g
24. 7.21 g
25. 12.7 g
26. E.0 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

22. The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is
23. 3.0 × 10²² H atoms.
24. 1.2 × 10²³ H atoms.
25. C.4 × 10²³ H atoms.
26. 4.8 × 10²³ H atoms.
27. None of these choices are correct.

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

23. How many protons are there in a molecule of adrenaline (C₉H₁₃NO₃), a neurotransmitter and hormone?
24. 22
25. 26
26. 43
27. D. 98
28. 183

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

24. Copper(II) sulfate pentahydrate, CuSO₄·5H₂O, is used as a fungicide and algicide. Calculate the mass of oxygen in 1.000 mol of CuSO₄·5H₂O.
25. 249.7 g
26. B.0 g
27. 96.00 g
28. 80.00 g
29. 64.00 g

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

25. Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO₃)₂.
26. 107 g
27. 90.8 g
28. C.0 g
29. 83.4 g
30. 62.6 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

26. Household sugar, sucrose, has the molecular formula C₁₂H₂₂O₁₁. What is the percent of carbon in sucrose, by mass?
27. 26.7%
28. 33.3%
29. 41.4%
30. D.1%
31. 52.8%

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mass Percent Composition

Topic: Stoichiometry and Chemical Reactions

27. Determine the percent composition of potassium dichromate, K₂Cr₂O₇.
28. 17.5% K, 46.6% Cr, 35.9% O
29. 29.8% K, 39.7% Cr, 30.5% O
30. 36.5% K, 48.6% Cr, 14.9% O
31. 37.2% K, 24.7% Cr, 38.1% O
32. E. None of these choices are correct.

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Mass Percent Composition

Topic: Stoichiometry and Chemical Reactions

28. Gadolinium oxide, a colorless powder which absorbs carbon dioxide from the air, contains 86.76 mass % Gd. Determine its empirical formula.
29. A. Gd₂O₃
30. Gd₃O₂
31. Gd₃O₄
32. Gd₄O₃
33. GdO

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

29. Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. Determine its empirical formula.
30. HNO
31. B. H₂NO₂
32. HN₆O₁₆
33. HN₁₆O₇
34. H₂NO₃

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

30. Hydroxylamine 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?
31. NH₂O₅
32. B. N₂H₄O₄
33. N₃H₃O₃
34. N₄H₈O₂
35. N₂H₂O₄

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Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

31. Analysis of a carbohydrate showed that it consisted of 40.0 % C, 6.71 % H, and 53.3 % O by mass. Its molecular mass was found to be between 140 and 160 amu. What is the molecular formula of this compound?
32. C₄H₈O₆
33. B. C₅H₁₀O₅
34. C₅H₁₂O₅
35. C₆H₁₂O₄
36. None of these choices are correct.

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Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

32. A compound of bromine and fluorine is used to make UF₆, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.
33. BrF
34. BrF₂
35. Br₂F₃
36. Br₃F
37. E. BrF₃

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

33. A compound containing chromium and silicon contains 73.52 mass percent chromium. Determine its empirical formula.
34. CrSi₃
35. Cr₂Si₃
36. Cr₃Si
37. D. Cr₃Si₂
38. Cr₂S

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

34. Alkanes are compounds of carbon and hydrogen with the general formula C_nH_2n+2. An alkane component of gasoline has a molar mass of between 125 and 130 g/mol. What is the value of n for this alkane?
35. 4
36. B. 9
37. 10
38. 13
39. 14

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Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

35. 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?
36. C₂H₃O₄
37. C₃H₄O₂
38. C. C₄H₃O₂
39. C₅H₁₂O₄
40. C₂H₂O

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Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

36. 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. If its molar mass is between 158 and 167 g/mol, what is its molecular formula?
37. C₄H₆O₇
38. C₆H₈O₅
39. C₇H₁₂O₄
40. C₄H₃O₂
41. E. C₈H₆O₄

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Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

37. Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?
38. H₂N₇O₈Cl₁₈
39. H₂N₂O₂Cl
40. HN₃O₄Cl₉
41. D. H₄NOCl
42. H₄NOCl₂

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

38. In the combustion analysis of 0.1127 g of glucose (C₆H₁₂O₆), what mass, in grams, of CO₂ would be produced?
39. 0.0451 g
40. 0.0825 g
41. C.1652 g
42. 0.4132 g
43. 1.466 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

39. Balance the following equation:

B₂O₃(s) + HF(l) → BF₃(g) + H₂O(l)

1. A. B₂O₃(s) + 6HF(l) → 2BF₃(g) + 3H₂O(l)
2. B₂O₃(s) + H₆F₆(l) → B₂F₆(g) + H₆O₃(l)
3. B₂O₃(s) + 2HF(l) → 2BF₃(g) + H₂O(l)
4. B₂O₃(s) + 3HF(l) → 2BF₃(g) + 3H₂O(l)
5. B₂O₃(s) + 6HF(l) → 2BF₃(g) + 6H₂O(l)

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

40. Balance the following equation:

UO₂(s) + HF(l) → UF₄(s) + H₂O(l)

1. UO₂(s) + 2HF(l) → UF₄(s) + H₂O(l)
2. B. UO₂(s) + 4HF(l) → UF₄(s) + 2H₂O(l)
3. UO₂ (s) + H₄F₄(l) → UF₄ (s) + H₄O₂(l)
4. UO₂(s) + 4HF(l) → UF₄(s) + 4H₂O(l)
5. UO₂(s) + 8HF(l) → 2UF₄(s) + 4H₂O(l)

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

41. 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)
3. C. 2C₆H₆(l) + 15O₂(g) → 6H₂O(g) + 12CO₂(g)
4. C₆H₆(l) + 15O₂(g) → 3H₂O(g) + 6CO₂(g)
5. 2C₆H₆(l) + 9O₂(g) → 6H₂O(g) + 12CO₂(g)

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

42. Balance the following equation:

C₈H₁₈O₃(l) + O₂(g) → H₂O(g) + CO₂(g)

1. C₈H₁₈O₃(l) + 😯₂(g) → 9H₂O(g) + 8CO₂(g)
2. B. C₈H₁₈O₃(l) + 11O₂(g) → 9H₂O(g) + 8CO₂(g)
3. 2C₈H₁₈O₃(l) + 22O₂(g) → 9H₂O(g) + 16CO₂(g)
4. C₈H₁₈O₃(l) + 13O₂(g) → 18H₂O(g) + 8CO₂(g)
5. 2C₈H₁₈O₃(l) + 17O₂(g) → 18H₂O(g) + 16CO₂(g)

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

43. 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)
4. D. 2Ca₃(PO₄)₂(s) + 6SiO₂(s) + 10C(s) → 6CaSiO₃(s) + 10CO(g) + P₄(s)
5. 2Ca₃(PO₄)₂(s) + 6SiO₂(s) + 10C(s) → 6CaSiO₃(s) + 10CO(g) + 4P₄(s)

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

44. How many molecules of molecular oxygen react with four molecules of NH₃ to form four molecules of nitrogen monoxide and six molecules of water?
45. 2
46. 10
47. 3
48. 4
49. E. 5

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

45. 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?

1. 0.800 mol
2. 0.400 mol
3. C.200 mol
4. 0.100 mol
5. 0.0500 mol

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

46. Aluminum will react 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 Al₂Br₆?

7. 7.29 mol
8. B.86 mol
9. 2.43 mol
10. 1.62 mol
11. 1.22 mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

47. Ammonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in production of aluminum, in uranium processing, and in 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 F₂?

34. 34.0 mol
35. 27.2 mol
36. 6.80 mol
37. D.44 mol
38. 2.27 mol

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Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

48. Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine.

N₂(g) + 3H₂(g) → 2NH₃(g)

How many grams of nitrogen are needed to produce 325 grams of ammonia?

1. 1070 g
2. 535 g
3. C. 267 g
4. 178 g
5. 108 g

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Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

49. How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are needed to form 485 g of sulfur tetrafluoride?

3SCl₂(l) + 4NaF(s) → SF₄(g) + S₂Cl₂(l) + 4NaCl(s)

1. 1940 g
2. 1510 g
3. C. 754 g
4. 205 g
5. 51.3 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

50. How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH₃?

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)

469. A.7 g
470. 300.6 g
471. 250.0 g
472. 3.406 g
473. 2.180 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

51. Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen 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.

1. 1880 g
2. 940. g
3. 900. g
4. D. 470 g
5. 56.3 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

52. Potassium chlorate (used in fireworks, flares, and safety matches) forms oxygen and potassium chloride when heated.

KClO₃(s) → KCl(s) + O₂(g) [unbalanced]

How many grams of oxygen are formed when 26.4 g of potassium chlorate is heated?

1. 223 g
2. 99.1 g
3. C.3 g
4. 6.86 g
5. 4.60 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

53. Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl₃. What mass of chlorine gas is needed to react completely with 163 g of aluminum?
54. 214 g
55. 245 g
56. 321 g
57. 489 g
58. E. 643 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

54. 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?
55. A. 151 g
56. 123 g
57. 50.3 g
58. 37.7 g
59. 9.41 g

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

55. An important reaction sequence in the industrial production of nitric acid is the following:

N₂(g) + 3H₂(g) → 2NH₃(g)

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(l)

Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

12. 12.5 mol O₂
13. 20.0 mol O₂
14. 25.0 mol O₂
15. D.0 mol O₂
16. 100. mol O₂

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

56. In a blast furnace, elemental iron is produced from a mixture of coke (C), iron ore (Fe₃O₄), and other reactants. An important reaction sequence is

2C(s) + O₂(g) → 2CO(g)

Fe₃O₄(s) + 4CO(g) → 3Fe(l) + 4CO₂(g)

How many moles of iron can be formed in this sequence when 1.00 mol of carbon, as coke, is consumed?

6. 6.00 mol Fe
7. 3.00 mol Fe
8. 1.33 mol Fe
9. 1.25 mol Fe
10. E.750 mol Fe

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

57. The iodine “clock reaction” involves the following sequence of reactions occurring in a reaction mixture in a single beaker.
58. IO₃(aq) + 5I^–(aq) + 6H⁺(aq) → 3I₂(aq) + 3H₂O(l)
59. I₂(aq) + 2S₂O₃^2–(aq) → 2I^–(aq) + S₄O₆^2–(aq)

 

The molecular iodine (I₂) formed in reaction 1 is immediately used up in reaction 2, so that no iodine accumulates. What is the overall reaction occurring in this experiment?

1. IO₃^–(aq) + 3I^–(aq) + 2S₂O₃^2–(aq) + 6H⁺(aq) → 2I₂(aq) + S₄O₆^2–(aq) + 3H₂O(l)
2. IO₃(aq) + 4S₂O₃^2–(aq) + 6H⁺(aq) → I^–(aq) + 2S₄O₆^2–(aq) + 3H₂O(l)
3. C. IO₃^–(aq) + 6S₂O₃^2–(aq) + 6H⁺(aq) → I^–(aq) + 3S₄O₆^2–(aq) + 3H₂O(l)
4. IO₃^–(aq) + I₂(aq) + 8S₂O₃^2–(aq) + 6H⁺(aq) → 3I^–(aq) + 4S₄O₆^2–(aq) + 3H₂O(l)
5. IO₃(aq) + 2I₂(aq) + 6S₂O₃^2–(aq) + 6H⁺(aq) → 5I^–(aq) + 3S₄O₆^2–(aq) + 3H₂O(l)

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Writing and Balancing Chemical Equations

Topic: Stoichiometry and Chemical Reactions

58. The iodine “clock reaction” involves the following sequence of reactions occurring in a reaction mixture in a single beaker.
59. IO₃(aq) + 5I^–(aq) + 6H⁺(aq) → 3I₂(aq) + 3H₂O(l)
60. I₂(aq) + 2S₂O₃^2–(aq) → 2I^–(aq) + S₄O₆^2–(aq)

 

The molecular iodine (I₂) formed in reaction 1 is immediately used up in reaction 2, so that no iodine accumulates. In one experiment, a student made up a reaction mixture which initially contained 0.0020 mol of iodate ions (IO₃^–). If the iodate ions reacted completely, how many moles of thiosulfate ions (S₂O₃^2–) were needed in reaction 2, in order to react completely with the iodine (I₂) produced in reaction 1?

1. 0.0020 mol
2. B.012 mol
3. 0.0040 mol
4. 0.0010 mol
5. 0.0060 mol

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

59. Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen.

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00 g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

155. A.8 g
156. 200.2 g
157. 249.9 g
158. 311.7 g
159. 374.9 g

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

60. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant, or catalyst for organic reactions.

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00 g/mol) 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.

19. Oxygen is the limiting reactant; 19.81 g of aluminum remain.
20. Oxygen is the limiting reactant; 35.16 g of aluminum remain.
21. Aluminum is the limiting reactant; 16.70 g of oxygen remain.
22. Aluminum is the limiting reactant; 35.16 g of oxygen remain.
23. E. Aluminum is the limiting reactant; 44.24 g of oxygen remain.

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

61. Magnesium reacts with iron(III) chloride to form magnesium chloride (which can be used in fireproofing wood and in disinfectants) and iron.

3Mg(s) + 2FeCl₃(s) → 3MgCl₂(s) + 2Fe(s)

A mixture of 41.0 g of magnesium ( = 24.31 g/mol) and 175 g of iron(III) chloride ( = 162.2 g/mol) is allowed to react. What mass of magnesium chloride = 95.21 g/mol) is formed?

68. 68.5 g MgCl₂
69. 77.0 g MgCl₂
70. 71.4 g MgCl₂
71. 107 g MgCl₂
72. E. 154 g MgCl₂

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

62. Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron.

3Mg(s) + 2FeCl₃(s) → 3MgCl₂(s) + 2Fe(s)

A mixture of 41.0 g of magnesium ( = 24.31 g/mol) and 175 g of iron(III) chloride ( = 162.2 g/mol) 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.

1. Limiting reactant is Mg; 67 g of FeCl₃ remain.
2. Limiting reactant is Mg; 134 g of FeCl₃ remain.
3. Limiting reactant is Mg; 104 g of FeCl₃ remain.
4. D. Limiting reactant is FeCl₃; 2 g of Mg
5. Limiting reactant is FeCl₃; 87 g of Mg remain.

 

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

63. 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.
64. A. Potassium is the limiting reactant; 2.47 g of chlorine remain.
65. Potassium is the limiting reactant; 7.23 g of chlorine remain.
66. Chlorine is the limiting reactant; 4.64 g of potassium remain.
67. Chlorine is the limiting reactant; 2.70 g of potassium remain.
68. No limiting reagent: the reactants are present in the correct stoichiometric ratio.

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

64. Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas.

P₄(s) + 3O₂(g) → P₄O₆(s)

If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

57. 57.5%
58. B.8%
59. 38.0%
60. 32.4%
61. 16.3%

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Reaction Yield

Topic: Stoichiometry and Chemical Reactions

65. What is the percent yield for the reaction

PCl₃(g) + Cl₂(g) → PCl₅(g)

If 119.3 g of PCl₅ (M = 208.2 g/mol) are formed when 61.3 g of Cl₂ ( = 70.91 g/mol) react with excess PCl₃?

1. 195%
2. 85.0%
3. C.3%
4. 51.4%
5. 43.7%

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Reaction Yield

Topic: Stoichiometry and Chemical Reactions

66. Methanol (CH₄O) is converted to bromomethane (CH₃Br) as follows:

CH₄O + 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?

40. 40.9%
41. B.6%
42. 100%
43. 121%
44. 245%

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Reaction Yield

Topic: Stoichiometry and Chemical Reactions

67. One mole of O₂ has a mass of 16.0 g.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

68. One mole of methane (CH₄) contains a total of 3 × 10²⁴ atoms.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

69. The formula CH₃O_0.5 is an example of an empirical formula.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Chemical Formulas

Topic: Components of Matter

70. In combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO₂ and H₂O, respectively, which are collected in the absorbers.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

71. In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO₂ and H₂O collected in the absorbers.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

72. Constitutional (structural) isomers have the same empirical formula but different molecular formulas.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Chemical Formulas

Topic: Components of Matter

73. Constitutional (structural) isomers have the same molecular formula but different structural formulas.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Chemical Formulas

Topic: Components of Matter

74. In a correctly balanced equation, the number of reactant molecules must equal the number of product molecules.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Stoichiometry and Chemical Reactions

Subtopic: Writing and Balancing Chemical Equations

Topic: Components of Matter

 

Category                                                                                                                                        # of Questions

Accessibility: Keyboard Navigation                                                                                                                        68

Bloom’s: 1. Remember                                                                                                                                            5

Bloom’s: 2. Understand                                                                                                                                           5

Bloom’s: 3. Apply                                                                                                                                                   64

Difficulty: Easy                                                                                                                                                       23

Difficulty: Hard                                                                                                                                                       12

Difficulty: Medium                                                                                                                                                  39

Gradable: automatic                                                                                                                                                 74

Subtopic: Calculating Amounts of Reactant and Product (including solutions)                                                       13

Subtopic: Chemical Formulas                                                                                                                                  3

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)                        13

Subtopic: Limiting Reactant                                                                                                                                     5

Subtopic: Mass Percent Composition                                                                                                                      2

Subtopic: Molar Mass                                                                                                                                             7

Subtopic: Mole Conversions                                                                                                                                   20

Subtopic: Reaction Yield                                                                                                                                         3

Subtopic: Stoichiometry and Chemical Reactions                                                                                                    1

Subtopic: Writing and Balancing Chemical Equations                                                                                             8

Topic: Components of Matter                                                                                                                                  4

Topic: Stoichiometry and Chemical Reactions                                                                                                         70

 

Chapter 5 Test Bank

Gases and the Kinetic-Molecular Theory

 

1. A ballerina weighs 103 lbs and is up on her toes with only 10.0 cm² of her slippers in contact with the floor. What pressure is she exerting on the floor?
2. A.59 × 10⁵ Pa
3. 4.59 × 10³ Pa
4. 4.59 × 10¹ Pa
5. 4.59 × 10^–1 Pa
6. 4.59 × 10^–3 Pa

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

2. Given that pressure has dimensions of force ÷ area; that force has dimensions of mass × acceleration; and that the S.I. unit of pressure is the pascal, what is 1 pascal in terms of S.I. base units?
3. A. 1 Pa = 1000 g/cm·s²
4. 1 Pa = 1 g/m·s²
5. 1 Pa = 10^–3 kg·m/s²
6. 1 Pa = 1 kg·m/s²
7. 1 Pa = 1 kg/m·s²

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

3. Mineral oil can be used in place of mercury in manometers when small pressure changes are to be measured. What is the pressure of an oxygen sample in mm of mineral oil if its pressure is 28.5 mm Hg?

(d of mineral oil = 0.88 g/mL; d of Hg = 13.5 g/mL)

1. 1.9 mm mineral oil
2. 15 mm mineral oil
3. 32 mm mineral oil
4. 380 mm mineral oil
5. E. 440 mm mineral oil

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

4. Mercury is 13.6 times as dense as liquid water. What would be the reading of a water-filled barometer at normal atmospheric pressure, 760. mmHg?
5. 1.03 × 10³ torr
6. 1.03 × 10³ Pa
7. 1.03 × 10³ mm height of water column
8. D.03 × 10³ cm height of water column
9. 13.6 atm

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

5. A flask containing helium gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 752 torr. The mercury level in the open arm is 26 mm above that in the arm connected to the flask of helium. What is the helium pressure, in torr?
6. –26 torr
7. 26 torr
8. 726 torr
9. D. 778 torr
10. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

6. A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 50. mm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?
7. –50. torr
8. 50. torr
9. C. 695 torr
10. 795 torr
11. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

7. A flask containing argon gas is connected to a closed-ended mercury manometer. The closed end is under vacuum. If the mercury level in the closed arm is 230. mm above that in the arm connected to the flask, what is the argon pressure, in torr?
8. –230.
9. B.
10. 530.
11. 790.
12. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

8. Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmospheres?
9. 0.217 atm
10. 0.466 atm
11. C.613 atm
12. 1.63 atm
13. 4.60 atm

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

9. The pressure of hydrogen sulfide gas in a container is 35,650 Pa. What is this pressure in torr?
10. 46.91 torr
11. B.4 torr
12. 351.8 torr
13. 3612 torr
14. 27090 torr

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

10. The pressure of sulfur dioxide in a container is 159 kPa. What is this pressure in atmospheres?
11. 0.209 atm
12. 0.637 atm
13. C.57 atm
14. 21.2 atm
15. 15900 atm

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

11. The air pressure in a volleyball is 75 psi. What is this pressure in torr?
12. 520 torr
13. 562 torr
14. C. 3900 torr
15. 7600 torr
16. 75000 torr

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

12. “The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure” is a statement of __________________ Law.
13. Charles’s
14. Boyle’s
15. Amontons’s
16. D. Avogadro’s
17. Dalton’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

13. “The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles” is a statement of __________________ Law.
14. Charles’s
15. B. Boyle’s
16. Amontons’s
17. Avogadro’s
18. Gay-Lussac’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

14. “The pressure of an ideal gas is directly proportional to its absolute temperature at constant volume and number of moles” is a statement of ________________ Law.
15. Charles’s
16. Boyle’s
17. Amontons’s
18. D. Avogadro’s
19. Gay-Lussac’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

15. “The volume of an ideal gas is directly proportional to its absolute temperature at constant pressure and number of moles” is a statement of ________________ Law.
16. A. Charles’s
17. Boyle’s
18. Amontons’s
19. Avogadro’s
20. Dalton’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

16. “The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gases” is a statement of __________________ Law.
17. Charles’s
18. Graham’s
19. Boyle’s
20. Avogadro’s
21. E. Dalton’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Dalton’s Law of Partial Pressures

Topic: Gases

17. “The rate of effusion of a gas is inversely proportional to the square root of its molar mass” is a statement of ______________________ Law.
18. Charles’s
19. B. Graham’s
20. Dalton’s
21. Avogadro’s
22. Boyle’s

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Effusion and Diffusion (Graham’s Law)

Topic: Gases

18. Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant?

 

1. a
2. b
3. c
4. d
5. E. e

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

19. Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its absolute temperature, other factors remaining constant?
20. a
21. b
22. C. c
23. d
24. e

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

20. Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its Celsius temperature, other factors remaining constant?

 

1. a
2. B. b
3. c
4. d
5. e

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

21. Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

 

1. a
2. b
3. C. c
4. d
5. e

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

22. A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?
23. 10 torr
24. B. 50 torr
25. 100 torr
26. 200 torr
27. 1000 torr

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

23. A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume?
24. A.0 L
25. 6.0 L
26. 9 L
27. 36 L
28. 48 L

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

24. A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?
25. increased by 44.3 L
26. B. increased by 9.3 L
27. increased by 7.4 L
28. decreased by 27.6 L
29. decreased by 7.4 L

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Topic: Gases

25. A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?
26. 22.3 L
27. B.2 L
28. 44.9 L
29. 112 L
30. 380 L

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Topic: Gases

26. A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?
27. A. 212 torr
28. 289 torr
29. 356 torr
30. 441 torr
31. 359 torr

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Topic: Gases

27. A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?
28. 20 mL
29. 133 mL
30. C. 200 mL
31. 400 mL
32. 800 mL

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28. A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr?
29. A. 182 K
30. 298 K
31. 387 K
32. 489 K
33. 538 K

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Topic: Gases

29. A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and 1.35 atm?
30. 5.38 L
31. 10.9 L
32. 19.0 L
33. D.3 L
34. 77.9 L

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Topic: Gases

30. A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is –15.8°C and its pressure is 524 torr?
31. 3.69 L
32. B.6 L
33. 20.2 L
34. 63.5 L
35. not possible, since the volume would have to be negative

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31. A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?
32. 200 torr
33. 400 torr
34. 800 torr
35. 2400 torr
36. E. 3200 torr

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32. A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume?
33. 188 torr
34. 562 torr
35. 1.11 × 10³ torr
36. D.20 × 10³ torr
37. 1.90 × 10³ torr

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Topic: Gases

33. A sample of methane gas, CH₄(g), occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3°C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?
34. A. –116.5°C
35. 15.2°C
36. 15.5°C
37. 57.7°C
38. 310.6°C

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Topic: Gases

34. What are the conditions of STP?
35. 0 K and l atm
36. B.15 K and 760 torr
37. 0°C and 760 atm
38. 273.15°C and 760 torr
39. None of these choices are correct.

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Subtopic: Units of Pressure and STP

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35. A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP?
36. 25.2 L
37. 30.6 L
38. 33.6 L
39. D.1 L
40. 49.2 L

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Topic: Gases

36. Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3°C and 89.9 kPa. What is its volume at STP?
37. A.8 L
38. 27.6 L
39. 29.6 L
40. 37.6 L
41. 153 L

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37. Calculate the pressure of a helium sample at –207.3°C and 768 mL if it exerts a pressure of 175 kPa at 25.0°C and 925 mL.
38. 32.1 kPa
39. B.6 kPa
40. 657 kPa
41. 953 kPa
42. not possible, since the pressure would have to be negative

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38. Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0°C and 41.1 kPa.
39. 95.0°C
40. 85.1°C
41. 77.2°C
42. 72.9°C
43. E.2°C

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39. A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65°C and 645 torr. What is its volume at STP?
40. A.4 L
41. 31.1 L
42. 34.3 L
43. 35.2 L
44. 47.7 L

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40. A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container?
41. A.271 mol
42. 2.27 mol
43. 3.69 mol
44. 206 mol
45. 227 mol

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41. A compressed gas cylinder containing 1.50 mol methane has a volume of 3.30 L. What pressure does the methane exert on the walls of the cylinder if its temperature is 25°C?
42. 9.00 × 10^–2 atm
43. 0.933 atm
44. 1.11 atm
45. 1.70 atm
46. E.1 atm

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Topic: Gases

42. Assuming ideal behavior, what is the density of argon gas at STP, in g/L?
43. 0.0176 g/L
44. 0.0250 g/L
45. 0.0561 g/L
46. D.78 g/L
47. 181. g/L

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Subtopic: Density of a Gas

Topic: Gases

43. What is the density of carbon dioxide gas at –25.2°C and 98.0 kPa?
44. 0.232 g/L
45. 0.279 g/L
46. 0.994 g/L
47. 1.74 g/L
48. E.09 g/L

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44. Ima Chemist found the density of Freon-11 (CFCl₃) to be 5.58 g/L under her experimental conditions. Her measurements showed that the density of an unknown gas was 4.38 g/L under the same conditions. What is the molar mass of the unknown?
45. 96.7 g/mol
46. B. 108 g/mol
47. 127 g/mol
48. 165 g/mol
49. 175 g/mol

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Subtopic: Molar Mass of a Gas

Topic: Gases

45. A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas?
46. 7.76 g/mol
47. 66.1 g/mol
48. C.0 g/mol
49. 81.4 g/mol
50. 144 g/mol

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Subtopic: Molar Mass of a Gas

Topic: Gases

46. Dr. I. M. A. Brightguy adds 0.1727 g of an unknown gas to a 125-mL flask. If Dr. B finds the pressure to be 736 torr at 20.0°C, is the gas likely to be methane, CH₄, nitrogen, N₂, oxygen, O₂, neon, Ne, or argon, Ar?
47. CH₄
48. N₂
49. Ne
50. Ar
51. E. O₂

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47. A 250.0-mL sample of ammonia, NH₃(g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia is in the container?
48. 0.0787 g
49. B.180 g
50. 8.04 g
51. 17.0 g
52. 59.8 g

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48. What is the pressure in a 7.50-L flask if 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen? The temperature of the mixture is 48.0°C.
49. 0.252 atm
50. 0.592 atm
51. C.69 atm
52. 3.96 atm
53. 4.80 atm

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Subtopic: Dalton’s Law of Partial Pressures

Topic: Gases

49. If 0.750 L of argon at 1.50 atm and 177°C and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0°C are added to a 1.00-L flask and the flask’s temperature is adjusted to 25.0°C, what is the resulting pressure in the flask?
50. 0.0851 atm
51. 0.244 atm
52. C.946 atm
53. 1.74 atm
54. 1.86 atm

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Subtopic: Dalton’s Law of Partial Pressures

Topic: Gases

50. A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr?
51. 80.0 torr
52. 200. torr
53. 256 torr
54. D. torr
55. 556 torr

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Subtopic: Dalton’s Law of Partial Pressures

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51. A gas mixture, with a total pressure of 300. torr, consists of equal masses of Ne (atomic weight 20.) and Ar (atomic weight 40.). What is the partial pressure of Ar, in torr?
52. 75 torr
53. B. torr
54. 150. torr
55. 200. torr
56. None of these choices are correct.

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Subtopic: Dalton’s Law of Partial Pressures

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52. An unknown liquid is vaporized in a 273-mL flask by immersion in a water bath at 99°C. The barometric pressure is 753 torr. If the mass of the vapor retained in the flask is 1.362 g, what is its molar mass?
53. 20.4 g/mol
54. 40.9 g/mol
55. 112 g/mol
56. D. 154 g/mol
57. 184 g/mol

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Subtopic: Molar Mass of a Gas

Topic: Gases

53. A gas consists of 85.7 percent carbon and 14.3 percent hydrogen, by weight. A sample of this gas weighing 0.673 g occupies 729 mL at a pressure of 720.0 mmHg and a temperature of 77°C. Calculate its empirical and molecular formulas.
54. CH, C₂H₂
55. B. CH₂, C₂H₄
56. CH₂, C₃H₆
57. CH₃, C₂H₆
58. CH₄, CH₄

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54. Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of HCl are combined and react to completion. How many liters of hydrogen gas, measured at STP, are produced?

Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

2. A.24 L of H₂
3. 4.48 L of H₂
4. 5.60 L of H₂
5. 11.2 L of H₂
6. 22.4 L of H₂

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Subtopic: Limiting Reactant

Topic: Stoichiometry and Chemical Reactions

55. Linolenic acid (C₁₈H₃₀O₂) can be hydrogenated to stearic acid by reacting it with hydrogen gas according to the equation:

C₁₈H₃₀O₂ + 3H₂ → C₁₈H₃₆O₂

What volume of hydrogen gas, measured at STP, is required to react with 10.5 g of linolenic acid in this reaction?

2. A.53 L
3. 1.69 L
4. 1.27 L
5. 845 mL
6. 422 mL

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Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

56. Hydrogen peroxide was catalytically decomposed and 75.3 mL of oxygen gas was collected over water at 25°C and 742 torr. What mass of oxygen was collected? (P_water = 24 torr at 25°C)
57. 0.00291 g
58. B.0931 g
59. 0.0962 g
60. 0.0993 g
61. 0.962 g

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57. Small quantities of hydrogen can be prepared by the addition of hydrochloric acid to zinc. A sample of 195 mL of hydrogen was collected over water at 25°C and 753 torr. What mass of hydrogen was collected? (P_water = 24 torr at 25°C)
58. 0.00765 g
59. B.0154 g
60. 0.0159 g
61. 0.0164 g
62. 0.159 g

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Subtopic: Molar Mass of a Gas

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58. Lithium oxide is an effective absorber of carbon dioxide and can be used to purify air in confined areas such as space vehicles. What volume of carbon dioxide can be absorbed by 1.00 kg of lithium oxide at 25°C and 1.00 atm?

Li₂O(aq) + CO₂(g) → Li₂CO₃(s)

1. 687 mL
2. 819 mL
3. 687 L
4. D. 819 L
5. 22.4 L

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Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

59. Methane, CH₄(g), reacts with steam to give synthesis gas, a mixture of carbon monoxide and hydrogen, which is used as starting material for the synthesis of a number of organic and inorganic compounds.

CH₄(g) + H₂O(g) → CO(g) + H₂(g) [unbalanced]

What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas?

12. 12.3 g
13. 24.7 g
14. 37.1 g
15. 49.4 g
16. E.2 g

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Subtopic: Calculating Amounts of Reactant and Product (including solutions)

Topic: Stoichiometry and Chemical Reactions

60. Hydrochloric acid is prepared by bubbling hydrogen chloride gas through water. What is the concentration of a solution prepared by dissolving 225 L of HCl(g) at 37°C and 89.6 kPa in 5.25 L of water?
61. A.49 M
62. 1.66 M
63. 7.82 M
64. 12.5 M
65. 16.6 M

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Subtopic: The Ideal Gas Law

Topic: Gases

61. Which of the following gases effuses most rapidly?
62. Nitrogen
63. Oxygen
64. Hydrogen chloride
65. D. Ammonia
66. Carbon monoxide

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Subtopic: Effusion and Diffusion (Graham’s Law)

Topic: Gases

62. Which of the following gases will be the slowest to diffuse through a room?
63. methane, CH₄
64. hydrogen sulfide, H₂S
65. C. carbon dioxide, CO₂
66. water, H₂O
67. neon, Ne

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Subtopic: Effusion and Diffusion (Graham’s Law)

Topic: Gases

63. Arrange the following gases in order of increasing rate of effusion.

C₂H₆            Ar            HCl         PH₃

1. A. Ar < HCl < PH₃ < C₂H₆
2. C₂H₆ < PH₃ < HCl < Ar
3. Ar < PH₃ < C₂H₆ < HCl
4. C₂H₆ < HCl < PH₃ < Ar
5. Ar < PH₃< HCl < C₂H₆

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Subtopic: Effusion and Diffusion (Graham’s Law)

Topic: Gases

64. A 3.0-L sample of helium was placed in a container fitted with a porous membrane. Half of the helium effused through the membrane in 24 hours. A 3.0-L sample of oxygen was placed in an identical container. How many hours will it take for half of the oxygen to effuse through the membrane?
65. 8.5 h
66. 12 h
67. 48 h
68. 60. h
69. E. 68 h

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Subtopic: Effusion and Diffusion (Graham’s Law)

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65. A compound composed of carbon, hydrogen, and chlorine effuses through a pinhole 0.411 times as fast as neon. Select the correct molecular formula for the compound.
66. A. CHCl₃
67. CH₂Cl₂
68. C₂H₂Cl₂
69. C₂H₃Cl
70. CCl₄

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Subtopic: Effusion and Diffusion (Graham’s Law)

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66. The volume of a single molecule of water is 2.99 × 10^–23 mL. For a sample of gaseous water at 1.00 atm and 150°C, what fraction of the container’s volume is occupied by the molecules themselves?
67. 5.2 × 10^–7
68. 4.5 × 10^–5
69. C.2 × 10^–4
70. 5.2 × 10^–1
71. None of these choices are correct.

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Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

67. Helium gas is being pumped into a rigid container at a constant temperature. As a result, the pressure of helium in the container is increasing. Select the one correct statement below.
68. As the pressure increases, helium atoms move faster, on average.
69. As the pressure increases, helium atoms move more slowly, on average.
70. As the pressure increases, the volume of the container must decrease.
71. As the pressure increases, helium atoms stay closer to the wall of the container, on average.
72. E. As the pressure increases, there are more collisions of helium atoms with the container wall.

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Subtopic: Kinetic-Molecular Theory

Topic: Gases

68. Which of the following changes will not affect the total pressure of gas in a container, assuming all other factors remain constant?
69. The frequency of collisions of molecules with the walls is increased.
70. The average velocity of the molecules is lowered.
71. The temperature of the sample is altered.
72. D. Half of the molecules are replaced by an equal number of molecules of a gas with a different molecular weight.
73. The total number of molecules is altered.

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Subtopic: Kinetic-Molecular Theory

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69. Select the statement that does not apply to an ideal gas.
70. There are no attractive forces between the gas molecules.
71. B. There are strong repulsive forces between the gas molecules.
72. The volume occupied by the molecules is negligible compared to the container volume.
73. The gas behaves according to the ideal gas equation.
74. The average kinetic energy of the molecules is proportional to the absolute temperature.

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Subtopic: Kinetic-Molecular Theory

Topic: Gases

70. At what temperature in kelvin is the root mean square speed of helium atoms (atomic weight = 4.00) equal to that of oxygen molecules (molecular weight = 32.00) at 300. K?
71. A.5 K
72. 75 K
73. 106 K
74. 292 K
75. 2400. K

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

71. Select the gas with the highest average kinetic energy per mole at 298 K.
72. O₂
73. CO₂
74. H₂O
75. H₂
76. E. All have the same average kinetic energy.

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

72. The most probable speed of an oxygen molecule in the gas phase at room temperature is 450 m/s. The root-mean-square speed (u_rms) is therefore
73. equal to 450 m/s.
74. slightly less than 450 m/s.
75. much less than 450 m/s.
76. D. slightly greater than 450 m/s.
77. much greater than 450 m/s.

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

73. Select the gas with the largest root-mean-square molecular speed at 25°C.
74. NH₃
75. CO
76. C. H₂
77. SF₆
78. All the gases have the same root-mean-square molecular speed at 25°C.

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

74. Calculate the root-mean-square speed of methane, CH₄ (g), at 78°C.
75. 23 m/s
76. 350 m/s
77. 550 m/s
78. 667 m/s
79. E. 740 m/s

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

75. Freon-12, CF₂Cl₂, which has been widely used in air conditioning systems, is considered a threat to the ozone layer in the stratosphere. Calculate the root-mean-square velocity of Freon-12 molecules in the lower stratosphere where the temperature is –65°C.
76. 20 m/s
77. 120 m/s
78. C. 210 m/s
79. 260 m/s
80. 4.4 × 10⁴ m/s

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

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76. Calculate the rms speed of carbon dioxide molecules at STP.
77. 12.4 m/s
78. 155 m/s
79. C. 393 m/s
80. 1.55 × 10⁵ m/s
81. The answer can’t be calculated without more data.

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

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77. If the molecular mass of a gas increases by a factor of 4 at constant temperature, its rms speed will
78. decrease by a factor of 4.
79. increase by a factor of 4.
80. decrease by a factor of 16.
81. increase by a factor of 16.
82. E. decrease by a factor of 2.

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78. The temperature of the carbon dioxide atmosphere near the surface of Venus is 475°C. Calculate the average kinetic energy per mole of carbon dioxide molecules on Venus.
79. 2520 J/mol
80. 4150 J/mol
81. 5920 J/mol
82. D. 9330 J/mol
83. 5920 kJ/mol

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Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

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79. The ozone layer is important because
80. ozone absorbs low energy radiation which warms the troposphere.
81. ozone purifies the atmosphere by reacting with excess fluorocarbons.
82. C. ozone absorbs ultraviolet radiation.
83. ozone reflects high energy radiation such as X-rays and gamma rays.
84. humans need to breathe air containing some ozone.

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Atmospheric Chemistry

Topic: Environmental Chemistry

80. Nitrogen will behave most like an ideal gas
81. at high temperature and high pressure.
82. B. at high temperature and low pressure.
83. at low temperature and high pressure.
84. at low temperature and low pressure.
85. at intermediate (moderate) temperature and pressure.

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

81. The ideal gas law tends to become inaccurate when
82. the pressure is lowered and molecular interactions become significant.
83. B. the pressure is raised and the temperature is lowered.
84. the temperature is raised above the temperature of STP.
85. large gas samples are involved.
86. the volume expands beyond the standard molar volume.

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

82. Use the van der Waals equation for real gases to calculate the pressure exerted by 1.00 mole of ammonia at 27°C in a 750-mL container. (a = 4.17 L²·atm/mol², b = 0.0371 L/mol)
83. 23.2 atm
84. B.1 atm
85. 32.8 atm
86. 42.0 atm
87. 32.8 torr

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

83. At moderate pressures (~ 200 atm), the measured pressure exerted by CO₂ gas is less than that predicted by the ideal gas equation. This is mainly because
84. such high pressures cannot be accurately measured.
85. CO₂ will condense to a liquid at 200 atm pressure.
86. gas phase collisions prevent CO₂ molecules from colliding with the walls of the container.
87. D. of attractive intermolecular forces between CO₂
88. the volume occupied by the CO₂ molecules themselves becomes significant.

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

84. At very high pressures (~ 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because
85. such high pressures cannot be accurately measured.
86. real gases will condense to form liquids at 1000 atm pressure.
87. gas phase collisions prevent molecules from colliding with the walls of the container.
88. of attractive intermolecular forces between gas molecules.
89. E. the volume occupied by the gas molecules themselves becomes significant.

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

85. When a closed-ended manometer is used for pressure measurements, and the closed end is under vacuum, the level of manometer liquid in the closed arm can never be lower than that in the other arm.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Gases

86. For a gas obeying Boyle’s Law, a plot of V versus 1/P will give a straight line passing through the origin.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

87. For a gas obeying Charles’s Law, a plot of V versus 1/T will give a straight line passing through the origin.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

88. At a temperature of absolute zero, the volume of an ideal gas is zero.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)

Topic: Gases

89. According to the postulates of kinetic-molecular theory, the molecules of all gases at a given temperature have the same average speed.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

90. According to the postulates of kinetic-molecular theory, the molecules of all gases at a given temperature have the same average kinetic energy.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

91. According to the kinetic theory of gases, in a collision between two molecules the kinetic energy of one molecule will decrease by the same amount that the kinetic energy of the other one increases.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Kinetic-Molecular Theory

Topic: Gases

92. According to the postulates of kinetic-molecular theory, the average kinetic energy of gas molecules is proportional to the absolute temperature.

TRUE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

93. For a pure gas sample, the average kinetic energy is also the most probable kinetic energy.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)

Topic: Gases

94. The rate of diffusion of a gas is inversely proportional to its molar mass.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Effusion and Diffusion (Graham’s Law)

Topic: Gases

95. For an ideal gas, a plot of PV/nRT versus P gives a straight line with a positive slope.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: The Ideal Gas Law

Topic: Gases

96. For real gases, PV > nRT, always.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

97. For real gases, PV < nRT, always.

FALSE

Accessibility: Keyboard Navigation

Bloom’s: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)

Topic: Gases

98. Convert a gas pressure of 485 cmHg to atmospheres.
99. 0.64 atm
100. 33.0 atm
101. C.38 atm
102. 5.50 atm
103. 6.46 atm

Accessibility: Keyboard Navigation

Bloom’s: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Units of Pressure and STP

Topic: Stoichiometry and Chemical Reactions

 

Category                                                                                                                                        # of Questions

Accessibility: Keyboard Navigation                                                                                                                        94

Bloom’s: 1. Remember                                                                                                                                            23

Bloom’s: 2. Understand                                                                                                                                           15

Bloom’s: 3. Apply                                                                                                                                                   60

Difficulty: Easy                                                                                                                                                       33

Difficulty: Hard                                                                                                                                                       5

Difficulty: Medium                                                                                                                                                  60

Gradable: automatic                                                                                                                                                 98

Subtopic: Atmospheric Chemistry                                                                                                                           1

Subtopic: Calculating Amounts of Reactant and Product (including solutions)                                                       3

Subtopic: Dalton’s Law of Partial Pressures                                                                                                           5

Subtopic: Density of a Gas                                                                                                                                      2

Subtopic: Deviation From Ideal Behavior (van der Waals Equation)                                                                      8

Subtopic: Effusion and Diffusion (Graham’s Law)                                                                                                7

Subtopic: Kinetic Energy and Temperature (Root-Mean-Square Speed)                                                                 13

Subtopic: Kinetic-Molecular Theory                                                                                                                        4

Subtopic: Limiting Reactant                                                                                                                                     1

Subtopic: Molar Mass of a Gas                                                                                                                               7

Subtopic: The Gas Laws (Boyle, Avogadro, and Charles)                                                                                      23

Subtopic: The Ideal Gas Law                                                                                                                                  10

Subtopic: Units of Pressure and STP                                                                                                                      14

Topic: Environmental Chemistry                                                                                                                             1

Topic: Gases                                                                                                                                                            92

Topic: Stoichiometry and Chemical Reactions                                                                                                         5