LT 8.1-8.4 Practice Test

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1 point

1. Which of the following statements about gases is false?

1 point

Gases are highly compressible.

Distances between molecules of gas are very large compared to bond distances within molecules.

Non-reacting gas mixtures are homogeneous.

Gases expand spontaneously to fill the container they are placed in.

All gases are colorless and odorless at room temperature.

Clear selection

2. One significant difference between gases and liquids is that __________.

1 point

a gas is made up of molecules

a gas assumes the volume of its container

a gas may consist of both elements and compounds

gases are always mixtures

All of the above answers are correct.

Clear selection

3. Gaseous mixtures __________.

1 point

can only contain molecules

are all heterogeneous

can only contain isolated atoms

are all homogeneous

must contain both isolated atoms and molecules

Clear selection

4. A pressure of 1.00 atm is the same as a pressure of __________ of mm Hg.

1 point

193

101

760.

29.9

33.0

Clear selection

5. Which of the following equations shows an incorrect relationship between pressures given in terms of different units?

1 point

1.20 atm = 122 kPa

152 mm Hg = 2.03 × 10⁴ Pa

0.760 atm = 578 mm Hg

1.0 torr = 2.00 mm Hg

1.00 atm = 760 torr

Clear selection

6. Which statement about atmospheric pressure is false?

1 point

As air becomes thinner its density decreases.

Air actually has weight.

With an increase in altitude atmospheric pressure increases as well.

The warmer the air the lower the atmospheric pressure.

Atmospheric pressure prevents water in lakes, rivers and oceans from boiling away.

Clear selection

7. A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was __________ atm.

1 point

4.00

2.00

1.00

8.00

16.0

Clear selection

8. A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is __________ atm.

1 point

1.5

7.5

0.67

3.3

Clear selection

9. A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to __________°C to reduce its volume to 3.78 L (at constant pressure).

1 point

72.9

273

546

Clear selection

10. If 3.21 mol of a gas occupies 56.2 L at 44°C and 793 torr, 5.29 mol of this gas occupies __________ L under these conditions.

1 point

14.7

61.7

30.9

92.6

478

Clear selection

11. A gas originally at 27°C and 1.00 atm pressure in a 3.9 L flask is cooled at constant pressure until the temperature is 11°C. The new volume of the gas is __________ L.

1 point

0.27

3.7

3.9

4.1

0.24

Clear selection

12. If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy __________ L at STP.

1 point

3.92

50.8

12.9

25.5

5.08

Clear selection

13. A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is __________ L at 423 K and 1.00 atm.

1 point

0.709

41.1

81.6

1.41

57.9

Clear selection

14. A sample of H₂ gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies __________ L at 353 K and 2.00 atm.

1 point

109

68.2

54.7

147

77.3

Clear selection

15. A sample of an ideal gas (3.00 L) in a closed container at 25.0°C and 76.0 torr is heated to 300 °C. The pressure of the gas at this temperature is __________ torr.

1 point

912

146

76.5

39.5

2.53 × 10-2

Clear selection

16. A sample of a gas originally at 25°C and 1.00 atm pressure in a 2.5 L container is allowed to expand until the pressure is 0.85 atm and the temperature is 15°C. The final volume of the gas is __________ L.

1 point

3.0

2.8

2.6

2.1

0.38

Clear selection

17. The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation shown below will produce a total of __________ mL of products if pressure and temperature are kept constant.

Cl₂(g) + CH₄(g) → HCl (g) + CH₃Cl (g)

1 point

100

200

150

250

Clear selection

18. The reaction of 50 mL of N₂ gas with 150 mL of H₂ gas to form ammonia via the equation shown below will produce __________ mL of ammonia if pressure and temperature are kept constant.

N₂(g) + 3H₂(g) → 2NH₃(g)

1 point

250

200

150

100

Clear selection

19. The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation shown below will produce a total of __________ mL of products if pressure and temperature are kept constant.

Cl₂(g) + CH₄(g) → HCl (g) + CH₃Cl (g)

1 point

100

125

150

Clear selection

20. The first person to investigate the relationship between the pressure of a gas and its volume was __________.

1 point

Amadeo Avogadro

Lord Kelvin

Jacques Charles

Robert Boyle

Joseph Louis Gay-Lussac

Clear selection

21. Of the following, __________ is a correct statement of Boyle's law.

1 point

PV = constant

P/V= constant

V/P= constant

V/T= constant

VT= constant

Clear selection

22. Of the following, __________ is a valid statement of Charles' law.

1 point

T/V= constant

TV = constant

PV = constant

V = constant × n

V = constant × P

Clear selection

23. Which one of the following is a valid statement of Avogadro's law?

1 point

V/P= constant

V/n= constant

PV = constant

V = constant × n

V = constant × P

Clear selection

24. A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

1 point

846

0.118

5.26 × 10⁴

526

1.11

Clear selection

25. A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

1 point

10.9

13.2

2.07

7.56

48.4

Clear selection

26. The amount of gas that occupies 60.82 L at 31°C and 367 mm Hg is __________ mol.

1 point

1.18

0.850

894

11.6

0.120

Clear selection

27. The pressure of a sample of CH₄ gas (6.022 g) in a 30.0 L vessel at 402 K is __________ atm.

1 point

2.42

6.62

0.413

12.4

22.4

Clear selection

28. At a temperature of __________ °C, 0.444 mol of CO gas occupies 11.8 L at 889 torr.

1 point

379

106

Clear selection

29. The pressure exerted by 1.3 mol of gas in a 13 L flask at 22°C is __________ kPa.

1 point

560

250

2.4

1.0

Clear selection

30. A 0.325 L flask filled with gas at 0.914 atm and 19°C contains __________ mol of gas.

1 point

1.24 × 10⁻²

1.48 × 10⁻²

9.42

12.4

80.7

Clear selection

31. A gas in a 325 mL container has a pressure of 695 torr at 19°C. There are __________ mol of gas in the flask.

1 point

1.24 × 10⁻²

1.48 × 10⁻²

9.42

12.4

80.6

Clear selection

32. A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mm Hg. The flask is opened and more gas is added to the flask. The new pressure is 795 mm Hg and the temperature is now 26°C. There are now __________ mol of gas in the flask.

1 point

1.6

2.1

2.9

3.5

0.28

Clear selection

33. A sample of gas (1.3 mol) occupies __________ L at 22°C and 2.5 atm.

1 point

0.079

0.94

3.2 × 10⁻²

Clear selection

34. The volume of 0.65 mol of an ideal gas at 365 torr and 97°C is __________ L.

1 point

0.054

9.5

2.4 × 10⁻²

Clear selection

35. The volume occupied by 1.5 mol of gas at 35°C and 2.0 atm pressure is __________ L.

1 point

2.2

0.053

0.026

Clear selection

36. The mass of nitrogen dioxide contained in a 4.32 L vessel at 48°C and 141600 Pa is __________ g.

1 point

5.35 × 10⁴

53.5

10.5

70.5

9.46 × 10⁻²

Clear selection

37. The molar volume of a gas at STP is __________ L.

1 point

0.08206

62.36

1.00

22.4

14.7

Clear selection

38. How many moles of gas are there in a 45.0 L container at 25.0°C and 500.0 mm Hg?

1 point

0.630

6.11

18.4

1.21

207

Clear selection

39. Standard temperature and pressure (STP), in the context of gases, refers to __________.

1 point

298.15 K and 1 atm

273.15 K and 1 atm

298.15 K and 1 torr

273.15 K and 1 pascal

273.15 K and 1 torr

Clear selection

40. The volume of 1.20 mol of gas at 61.3 kPa and 25.0°C is __________ L.

1 point

135

48.5

52.4

108

55.7

Clear selection

41. Sodium bicarbonate is reacted (in a single replacement reaction) with concentrated hydrochloric acid at 37.0°C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO₂.

1 point

1.09 × 10²

2.85 × 10⁴

1.82 × 10⁴

8.70 × 10²

1.82 × 10³

Clear selection

42. The density of ammonia gas in a 4.32 L container at 837 torr and 45.0°C is __________ g/L.

1 point

3.86

0.719

0.432

0.194

4.22 × 10⁻²

Clear selection

43. The density of N₂O at 1.53 atm and 45.2°C is __________ g/L.

1 point

18.2

1.76

0.388

9.99

2.58

Clear selection

44. The molecular weight of a gas is __________ g/mol if 3.5 g of the gas occupies 2.1 L at STP.

1 point

5.5 × 10³

4.6 × 10²

2.7 × 10⁻²

Clear selection

45. The molecular weight of a gas that has a density of 6.70 g/L at STP is __________ g/mol.

1 point

4.96 x 10²

1.50 x 10²

7.30 x 10¹

3.35

2.98 x 10⁻¹

Clear selection

46. The molecular weight of a gas that has a density of 7.10 g/L at 25.0°C and 1.00 atm pressure is __________ g/mol.

1 point

174

14.6

28.0

5.75 × 10⁻³

6.85 × 10⁻²

Clear selection

47. The molecular weight of a gas that has a density of 5.75 g/L at STP is __________ g/mol.

1 point

3.90

129

141

578

1.73 × 10⁻³

Clear selection

48. The density of chlorine (Cl₂) gas at 25°C and 60. kPa is __________ g/L.

1 point

4.9

1.7

0.86

0.58

Clear selection

49. The volume of hydrogen gas at 38.0°C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is __________ L.

1 point

1.68

2.71 × 10⁻⁴

3.69 × 10⁴

2.84

0.592

Clear selection

50. The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is __________ L.

1 point

6.82

2.19

13.6

4.38

3.41

Clear selection

51. The volume of fluorine gas required to react with 2.67 g of calcium bromide to form calcium fluoride and bromine at 41.0°C and 4.31 atm is __________ mL.

1 point

10.4

210

420

79.9

104

Clear selection

52. What volume (mL) of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl (aq), when the final SO₂ pressure is 827 torr at 44.0°C?

1 point

7.60 x 10²

1.39 × 10⁻⁴

1.00 × 10⁻³

0.106

5.78 x 10²

Clear selection

53. Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation (shown below). What mass (g) of NaN₃ is required to provide 40.0 L of N₂ at 25.0°C and 763 torr?

2NaN₃ (s) → 2Na (s) + 3N₂ (g).

1 point

1.64

1.09

160

71.1

107

Clear selection

54. The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl (shown below). What volume (L) of CO is formed from the complete decomposition of 444 g of Ni(CO)₄ at 752 torr and 22.0°C?

Ni(CO)₄ (l) → Ni (s) + 4CO (g).

1 point

0.356

63.7

255

20.2

11.0

Clear selection

55. What volume (L) of NH₃ gas at STP is produced by the complete reaction of 7.5 g of H₂O according to the following reaction?

Mg₃N₂ (s) + 6H₂O (l) → 3Mg(OH)₂ (aq) + 2NH₃ (g)

1 point

3.1

9.3

0.32

Clear selection

56. Ammonium nitrite undergoes thermal decomposition to produce only gases (see below). What volume (L) of gas is produced by the decomposition of 35.0 g of NH₄NO₂ (s) at 525°C and 1.5 atm?

NH₄NO₂ (s) → N₂ (g) + 2H₂O (g)

1 point

160

Clear selection

57. The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory (see below). What volume (L) of O₂ gas at 25°C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO₃ (s)?

2KClO₃ (s) → 2KCl (s) + 3O₂ (g)

1 point

4.5

7.5

2.2

3.7

Clear selection

58. The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62°C. The gas is __________.

1 point

SO₂

SO₃

NH₃

NO₂

Clear selection

59. The density of __________ is 0.900 g/L at STP.

1 point

CH₄

N₂

Clear selection

60. The density of NO₂ in a 3.50 L tank at 780.0 torr and 37.0°C is _________ g/L.

1 point

1.64

9.30

1.86

2.92

3.27

Clear selection

61. The density (in g/L) of CO₂ at 1140 torr and 60.0°C is __________.

1 point

2.42

16.2

5.70

44.0

10.9

Clear selection

62. Of the following gases, __________ has density of 2.104 g/L at 303 K and 1.31 atm.

1 point

Clear selection

63. A 255 mL round-bottom flask is weighed and found to have a mass of 114.85 g. A few milliliters of an easily vaporized liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vaporizes at the boiling temperature of water, filling the flask with vapor. When all of the liquid has vaporized, the flask is removed from the bath, cooled, dried, and reweighed. The new mass of the flask and the condensed vapor is 115.23 g. Which of the following compounds could the liquid be? (Assume the ambient pressure is 1 atm.)

1 point

C₄H₁₀

C₃H₇OH

C₂H₆

C₂H₅OH

C₄H₉OH

Clear selection

64. A sample of an unknown volatile liquid was injected into a Dumas flask and heated until no visible traces of the liquid could be found. The flask and its contents were then rapidly cooled and reweighed The atmospheric pressure and temperature during the experiment were 0.976 atm and 18.0°C, respectively. The unknown volatile liquid was __________.

1 point

C₆H₁₂

C₆H₁₄

C₇H₁₄

C₇H₁₆

C₆H₆

Clear selection

65. The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP?

1 point

CH₄

NH₃

Clear selection

66. The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is __________ g/L.

1 point

0.0451

0.740

1.35

0.273

8.2

Clear selection

67. The density of krypton gas at 1.21 atm and 50.0°C is __________ g/L.

1 point

0.0456

0.262

0.295

3.82

7.65

Clear selection

68. The density of chlorine gas at 1.21 atm and 34.9°C is __________ g/L.

1 point

0.0479

0.295

0.423

1.70

3.39

Clear selection

69. A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is __________.

1 point

argon

helium

krypton

neon

xenon

Clear selection

70. Calcium hydride (CaH₂) reacts with water to form hydrogen gas (see belwo). How many grams of CaH₂ are needed to generate 48.0 L of H₂ gas at a pressure of 0.888 atm and a temperature of 32°C?

CaH₂ (s) + 2H₂O (l) → Ca(OH)₂ (aq) + 2H₂ (g)

1 point

50.7

0.851

143

35.8

71.7

Clear selection

71. A vessel contained N₂, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was __________ torr.

1 point

42.4

521

19.4

239

760

Clear selection

72. The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42°C is __________ mm Hg.

1 point

263

134

395

116

0.347

Clear selection

73. A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6 atm and 25°C at constant temperature in a 9.0 L flask. The total pressure in the flask was __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

1 point

2.6

9.2

1.0

3.7

Clear selection

74. A sample of H₂ gas (2.0 L) at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25°C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

1 point

0.56

2.8

1.0

1.6

Clear selection

75. In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is __________ if the partial pressures of He and Ne are 1.50 and 2.00 atm, respectively.

1 point

0.179

0.238

0.357

0.583

0.417

Clear selection

76. A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of gas. If the partial pressure of Ne is 2.75 atm, how many moles of Ar are in the mixture?

1 point

11.0

5.00

6.75

9.25

12.0

Clear selection

77. A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm.

1 point

1.7

1.5

0.60

0.35

1.0

Clear selection

78. A flask contains a mixture of He and Ne at a total pressure of 2.6 atm. There are 2.0 mol of He and 5.0 mol of Ne in the flask. The partial pressure of He is __________ atm.

1 point

9.1

6.5

1.04

0.74

1.86

Clear selection

79. Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas (see below). A sample of NaH weighing __________ g will produce 982 mL of gas at 28.0°C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr.

NaH (s) + H₂O (l) → NaOH (aq) + H₂ (g)

1 point

2.93

0.960

0.925

0.0388

925

Clear selection

80. SO₂ (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 mL container at 50.0°C. The total pressure in the container was __________ atm.

1 point

0.192

4.02

2.76

6.78

1.60

Clear selection

81. SO₂ (5.00 g) and CO₂ (5.00 g) are placed in a 750.0 mL container at 50.0°C. The partial pressure of SO₂ in the container was __________ atm.

1 point

2.76

4.02

6.78

0.192

1.60

Clear selection

82. SO₂ (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO₂ in the container was __________ atm.

1 point

6.78

2.76

1.60

0.192

4.02

Clear selection

83. CO (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 mL container at 50.0°C. The total pressure in the container was __________ atm.

1 point

10.3

4.02

6.31

0.292

1.60

Clear selection

84. CO (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO in the container was __________ atm.

1 point

6.31

4.02

10.3

0.292

1.60

Clear selection

85. CO (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO₂ in the container was __________ atm.

1 point

4.02

10.3

1.60

0.292

6.31

Clear selection

86. 10.0 grams of argon and 20.0 grams of neon are placed in a 1200.0 ml container at 25.0°C. The partial pressure of neon is __________ atm.

1 point

20.2

8.70

0.700

3.40

5.60

Clear selection

87. A mixture of Xe, Kr, and Ar has a total pressure of 6.70 atm. What is the mole fraction of Kr if the partial pressures of Xe and Ar are 1.60 atm and 2.80 atm, respectively.

1 point

0.174

0.256

0.343

0.481

0.570

Clear selection

88. Zinc reacts with aqueous sulfuric acid to form hydrogen gas (see below). In an experiment, 225 mL of wet H₂ is collected over water at 27 °C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr.

Zn (s) + H₂SO₄ (aq) → ZnSO₄ (aq) + H₂ (g)

1 point

4.79 × 10⁶

0.567

567

431

4.31 × 10⁵

Clear selection

89. Zinc reacts with aqueous sulfuric acid to form hydrogen gas (see below). In an experiment, 201 mL of wet H⁶ is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is __________ atm.

Zn (s) + H₂SO₄ (aq) → ZnSO₄ (aq) + H₂ (g)

1 point

0.929

706

0.964

760

1.00

Clear selection

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