Ch12 Gaseous State – Test Bank | Chemistry Review 15e

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Package Title: Hein Test Bank

Course Title: Hein 15e

Chapter Number: 12

Question type: Multiple Choice

1. Which of the following gases would have the greatest kinetic energy at 300 K?

A. N₂

B. NH₃

C. Ar

D. All of them would have the same kinetic energy.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

2. Which gas would have the lowest velocity at 280 K?

A. Ar

B. Ne

C. H₂

D. CO

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

3. In the ideal gas equation PV=nRT, the value of R depends upon

1. nature of gas
2. temperature of gas
3. pressure of gas
4. unit of measurement

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

4. The following figure shows 1 mol of an ideal gas inside a container with a movable piston.

If we add two additional moles of gas at constant temperature and pressure, select the image that represents what change, if any, that will take place.

A.

B.

C.

D.

Difficulty: hard

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

5. A hot air balloon is filled to a volume of 44.5 L at 758 torr. What will be the volume of the balloon if the pressure decreases to 748 torr under constant temperature?

A. 45.1 L

B. 43.9 L

C. 44.5 L

D. 49.0 L

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Reference: 12.2

6. Under which set of conditions will a real gas be least likely to act as an ideal gas?

A. High temperature and high pressure

B. High temperature and low pressure

C. Low temperature and high pressure

D. Low temperature and low pressure

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

7. Under which set of conditions will a real gas be most likely to act as an ideal gas?

A. High temperature and high pressure

B. High temperature and low pressure

C. Low temperature and high pressure

D. Low temperature and low pressure

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

8. Which of the gases below is least likely to behave as an ideal gas at STP?

1. Hydrogen
2. Helium
3. Neon
4. Chlorine

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

9. Different molecular forms of an element are called

A. Isotopes

B. Allotropes

C. Isomers

D. Isoelements

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature and number of moles.

Section Reference: 12.6

10. The following figure represents one mole of an ideal gas in a container fit with a movable piston.

Which image shows what change, if any, that would take place if the Kelvin temperature is doubled under constant pressure?

A.

B.

C.

D.

Difficulty: hard

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

11. A pressure of 3.00 atm is equal to

A. 819 mm Hg

B. 3000 mm Hg

C. 2280 mm Hg

D. 253 mm Hg

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

12. A sample of a gas is held at constant temperature. If the number of moles of gas in the sample is doubled while the pressure is halved, what will happen to the volume of the gas sample?

A. It will increase.

B. It will decrease.

C. It will not change.

Difficulty: hard

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

13. A pressure of 0.414 mm Hg is equal to

A. 0.0545 atm

B. 0.0659 atm

C. 0.152 atm

D. 0.184 atm

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

14. A pressure of 1030 torr is equal to

A. 0.738 atm

B. 0.265 atm

C. 1.36 atm

D. 3.77 atm

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

15. A pressure of 340. mm Hg is equal to

A. 2.24 torr

B. 0.448 torr

C. 340. torr

D. 1.25 torr

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

16. If the pressure of an ideal gas is doubled from 1.0 atm to 2.0 atm and its temperature is halved from 80.0 ^oC to 40.0 ^oC, the volume of the gas

1. will double its original value.
2. will be half its original value.
3. will increase by a factor of 0.56.
4. will decrease by a factor of 0.56

Difficulty: hard

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

17. As the number of molecules in a gas sample increases, temperature and volume remaining constant, the pressure exerted by the gas

A. increases.

B. decreases.

C. remains the same.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

18. Which is/are not true in case of an ideal gas? Select all that apply.

1. Ideal gas can not be converted into a liquid
2. There is no interaction between the molecules
3. All molecules of the gas moves with the same speed
4. At the given temperature, PV is proportional to the amount of gas.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

19. As the temperature of a gas sample increases, the number of molecules and volume remaining constant, the pressure exerted by the gas

A. increases.

B. decreases.

C. remains the same.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

20. As the pressure of a sample of gas is increased at constant temperature, the volume of the gas

A. increases.

B. decreases.

C. remains the same.

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

21. A 3.00 L sample of a gas at a pressure of 4.00 atm is compressed to 2.00 L at a constant temperature. What is the pressure of the gas?

A. 2.00 atm

B. 6.00 atm

C. 12.0 atm

D. 24.0 atm

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

22. 500.0 mL sample of a gas at 760.0 mm Hg were compressed to 200.0 mL. Find the new pressure if the temperature remains constant.

A. 1900 mmHg

B. 304.0 mmHg

C. 131.6 mmHg

D. 0.0005263 mmHg

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

23. A mole of gas at 0.0^oC and 760. torr occupies 22.4 L. What is the volume of this gas at 25.^oC and 760. torr?

1. 24.5 L
2. 0.0 L
3. 20.5 L
4. 19.8 L

Difficulty: medium

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

24. At constant pressure, 500. mL of oxygen gas at 27.0 ^oC is cooled to -5.0 ^oC . Calculate the new volume in liters.

1. 560 L
2. 2700 L
3. 450 L
4. .45 L

Difficulty: medium

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

25. A 4.00 L sample of a gas is at a pressure of 2.00 atm. If the temperature remains constant, what will be its volume at 0.500 atm of pressure?

A. 1.00 L

B. 16.0 L

C. 0.250 L

D. 4.00 L

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

26. At 1 atm pressure, a gas is compressed to 1/4^th of its initial volume at constant temperature. Find the new pressure.

1. 1atm
2. 2 atm
3. 4 atm
4. 0.25 atm

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

27. What should be the pressure of helium gas at 25^oC in order to have the same density as oxygen gas at STP?

A. 5.7 atm

B. 8.7 atm

C. 3.2 atm

D. 4.4 atm

Difficulty: medium

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

28. A sample of gas has a volume of 200. mL at 20.0 ^° C. What will be its volume at 40.0 ^°C,

pressure remaining constant?

A. 18.8 mL

B. 214 mL

C. 100. mL

D. 400. mL

Difficulty: medium

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

29. A sample of gas has a volume of 3.40 L at 10.0 ^°C. What will be its volume at 100.0^°C,

pressure remaining constant?

A. 0.340 L

B. 4.48 L

C. 34.0 L

D. 2.58 L

Difficulty: medium

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

30. A sample of gas has a volume of 1380 mL at a temperature of 20.0 ^° C. What will be its volume at 0.0^°C, pressure remaining constant?

A. 0.00 mL

B. 1290 mL

C. 1380 mL

D. 1480 mL

Difficulty: medium

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

31. A sample of gas in a 3.0 L container has a pressure of 4.0 atm. If this container is connected to a 5.0 L container and the gas is allowed to enter this container as well, what will be the final pressure of this gas if the temperature remains constant?

1. 1.5 atm
2. 2.4 atm
3. 6.6 atm
4. 1.8 atm

Difficulty: medium

Learning Objective: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

32. According to Boyles’s law,

1. Pressure and temperature of a gas are directly proportional at fixed volume and amount.
2. Pressure and volume of a gas are directly proportional at a fixed temperature and amount.
3. Volume and temperature of a gas are directly proportional at fixed pressure and amount.
4. Pressure and volume of a gas are inversely proportional at a fixed temperature and amount.

Difficulty: Easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

33. The volume of a gas must always decrease when

A. temperature increases and pressure increases.

B. temperature increases and pressure decreases.

C. temperature decreases and pressure increases.

D. temperature decreases and pressure decreases.

Difficulty: easy

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

34. A sample of gas has a volume of 8.00 L at 20.0 ^° C and 700. torr. What will be its volume at STP?

A. 1.20 L

B. 9.32 L

C. 53.2 L

D. 6.87 L

Difficulty: medium

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

35. A sample of gas has a volume of 400. mL at STP. What will be its volume at 20.0 ^° C and 700. torr?

A. 466 mL

B. 343 mL

C. 60.1 mL

D. 2660 mL

Difficulty: medium

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

36. A sample of gas has a volume of 850. mL at 23.0 ^° C and 1.10 atm. The temperature is increased to 33.0 ^° C, at what pressure will its volume be 900. mL?

A. 1.20 atm

B. 1.49 atm

C. 1.07 atm

D. 0.812 atm

Difficulty: medium

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5

37. A sample of oxygen is collected over water at 22 ^° C and 762 torr. What is the partial pressure of the dry oxygen? The vapor pressure of water at 22^°C is 19.8 torr.

A. 742 torr

B. 782 torr

C. 784 torr

D. 750. torr

Difficulty: hard

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

38. A mixture of gases consists of helium at a partial pressure of 400. torr, neon at a partial pressure of 300. torr, and argon at a partial pressure of 200. torr. What is the total pressure of this mixture of gases?

A. 300. torr

B. 760. torr

C. 900. torr

D. 1000 torr

Difficulty: easy

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

39. A 400. mL sample of hydrogen is collected over water at 23.0 ^° C and 758.4 torr. What is the volume of the dry hydrogen gas at 23.0 ^° C and 758.4 torr? The vapor pressure of water at 23.0 ^° C is 21.1 torr.

A. 144 mL

B. 389 mL

C. 411 mL

D. 14400 mL

Difficulty: medium

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

40. At STP, 3.00 L of nitrogen gas contains the same number of molecules as

A. 1.00 L of nitrogen gas

B. 2.00 L of oxygen gas

C. 3.00 L of chlorine gas

D. 4.00 L of hydrogen gas

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

41. 3.70 g of an unknown gas at 25.0 ^° C occupied the same volume as 0.184 g of hydrogen gas at 17.0 ^° C and at the same pressure. What is the molar mass of the gas?

A. 41.3 g/mol

B. 59.1 g/mol

C. 39.1 g/mol

D. 20.7 g/mol

Difficulty: hard

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

42. At STP, which sample contains twice the number of molecules found in 4.00 L of hydrogen gas?

A. 1.00 L of He

B. 2.00 L of He

C. 4.00 L of He

D. 8.00 L of He

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

43. What is the volume of 3.00 mol of neon gas at STP?

A. 6.73 L

B. 7.47 L

C. 60.6 L

D. 67.2 L

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

44. What is the volume of 0.132 mol of carbon dioxide gas at STP?

A. 2.96 L

B. 5.81 L

C. 170. L

D. 333 L

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

45. How many moles are present in 10.0 L of nitrogen gas at STP?

A. 2.24 mol

B. 2.80 mol

C. 0.446 mol

D. 224 mol

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

46. How many moles are present in 30.0 L of helium gas at STP?

A. 0.179 mol

B. 0.747 mol

C. 1.34 mol

D. 7.47 mol

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

47. What is the volume of 1.40 mol of chlorine gas at STP?

A. 31.4 L

B. 16.0 L

C. 0.316 L

D. 3.17 L

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

48. The mass of 5.6 liters of a gas at STP is 11 g. Find the identity of the gas.

1. PH₃
2. COCl₂
3. NO
4. N₂O

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

49. How many moles are present in 300. L of ammonia gas at STP?

A. 0.0568 mol

B. 13.4 mol

C. 0.0747 mol

D. 17.6 mol

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

50. What is the molar mass of a gas if 12.0 L of the gas at STP has a mass of 16.0 grams?

A. 8.57 g

B. 22.4 g

C. 16.8 g

D. 29.9 g

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

51. Find the volume of 6.00 g of hydrogen at 1.50 atm and 273 ^°C?

A. 89.6 L

B. 44.8 L

C. 179 L

D. 6.77 L

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

52. What is the molar mass of a gas if 18.0 L of the gas at STP has a mass of 41.6 grams?

A. 51.8 g

B. 9.69 g

C. 33.4 g

D. 1.86 g

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

53. What is the molar mass of a gas if 30.0 L of the gas at STP has a mass of 16.0 grams?

A. 2.05 g

B. 11.9 g

C. 21.4 g

D. 42.0 g

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

54. Find the volume in mL occupied by 7.000 g of nitrogen gas at 27.0 ^°C and 750. torr.

A. 6240 mL

B. 1120 mL

C. 562 mL

D. 1.94 mL

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

55. What is the molar mass of a gas if 16.0 L of the gas has a mass of 19.0 g at 765 torr and 20.0 ^°C?

A. 0.0352 g

B. 28.4 g

C. 26.8 g

D. 1.94 g

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

56. The total number of molecules contained in 22.4 L of nitrogen gas at STP is ___

1. 1 molecule
2. 22.4 molecules
3. 6.023 10^-23 molecules
4. 6.023 10²³ molecules

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

57. With each breath of air, you inhale 4.50 × 10²³ molecules of nitrogen gas. What is the mass of the inhaled nitrogen gas?

1. 10.5 g
2. 20.9 g
3. 18.7 g
4. 37.5 g

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

58. What is the molar mass of a gas if 40.0 L of the gas has a mass of 36.0 g at 740. torr and

30.0 ^° C?

A. 333 g

B. 33.1 g

C. 23.0 g

D. 56.0 g

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

59. 1.0 g sample of a diatomic gas occupies a volume of 350 mL at 0.0 ^° C and 2.0 atm. Find the mass of one atom of the gas.

A. 2.7 X 10^-23 g

B. 2.7 X 10^-20 g

C. 1.4 X 10^-23 g

D. 1.4 X 10^-20 g

Difficulty: hard

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

60. What is the density of carbon dioxide gas at STP?

A. 1.96 g/L

B. 0.509 g/L

C. 2.40 g/L

D. 1.00 g/L

Difficulty: easy

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

61. What is the volume occupied by 5.00 g of acetylene gas (C₂H₂) at 50.0 ^° C and 740. mmHg pressure?

A. 5.24 L

B. 136 L

C. .810 L

D. 145 L

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

62. Which of the following is not an assumption under KMT?

A. Gas particles have no attraction for one another.

B. During a collision, energy is lost by the gas particles and later is regained.

C. Gases at the same temperature have the same average kinetic energy.

D. Gas particles move in straight lines in all directions.

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

63. The value of R in L atm/K mol is

1. 0.082
2. 8.314
3. 1.987
4. 8.314 X 10⁷

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

64. What is the volume of 1.40 mol of nitrogen gas at 20.0 ^° C and 770. torr?

A. 33.2 L

B. 2.27 L

C. 0.0437 L

D. 405 L

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

65. At which pressure would a 2.60 mol sample of gas at 20.0 ^° C have a volume of 25.0 L?

A. 0.171 atm

B. 15.8 atm

C. 2.08 atm

D. 2.50 atm

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

66. Find the pressure applied by two moles of an ideal gas at 273 ^° C and occupies a volume of 44.8 L.

1. 2.00 atm
2. 3.00 atm
3. 4.00 atm
4. 1.00 atm

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

67. At what temperature would 0.600 mol of a gas at 700. torr have a volume of 22.6 L?

A. 150. ^° C

B. 225 ^° C

C. 423 ^° C

D. 498 ^° C

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

68. Calculate the temperature in Kelvin of 2.0 moles of oxygen gas occupying a volume of 5.0 L at 2.46 atm.

A. 75K

B. .013 K

C. 2.0 K

D. 50. K

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

69. What volume of oxygen is consumed when 3.00 mol of carbon monoxide is produced in the following equation at STP?

2 C(s) + O₂(g) → 2 CO(g)

A. 1.50 L

B. 33.6 L

C. 67.2 L

D. 22.4 L

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

70. What volume of ammonia is produced when 0.500 mol of nitrogen reacts completely in the

following equation at STP?

N₂(g) + 3 H₂(g) → 2NH₃(g)

A. 1.00 L

B. 22.4 L

C. 44.8 L

D. 11.2 L

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

71. How many grams of oxygen are consumed when 18.0 L of CH₄ gas react completely in the following equation at STP?

CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g)

A. 51.4 grams

B. 79.7 grams

C. 576 grams

D. 1.1510³ grams

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

72. How many moles of hydrogen gas are required to completely react with chlorine gas in the following reaction that has a pressure of 735 torr at 34 ^oC in a 450. mL container according to the reaction

H₂ (g) + Cl₂ (g) 🡪 2 HCl (g)

1. 2.4 mol
2. 0.017 mol
3. 0.61 mol
4. 1.8 mol

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Learning Objective 2: Solve stoichiometric problems involving gases.

Section References: 12.6 and 12.9

73. How many moles of nitrogen are consumed when 100. L of dinitrogen pentoxide are produced in the following equation at STP?

2 N₂(g) + 5 O₂(g) → 2 N₂O₅(g)

A. 4.46 mol

B. 1.79 mol

C. 0.0896 mol

D. 11.2 mol

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

74. What mass of water is produced when 10.0 L of hydrogen react completely in the following equation at STP?

2 H₂(g) + O₂(g) → 2 H₂O(l)

A. 14.2 g

B. 8.03 g

C. 16.1 g

D. 40.3 g

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

75. A gas mixture containing N₂ and O₂ was kept inside a 2.00 L container at a temperature of 23.0°C and a total pressure of 1.00 atm. The partial pressure of oxygen was 0.722 atm. How many grams of nitrogen were present in the gas mixture?

A. 2.31 g

B. 0.577 g

C. 0.641 g

D. 1.90 g

Difficulty: hard

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

76. What mass of water is produced when 10.0 L of oxygen react completely in the following equation at STP?

2 C₂H₆(g) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(g)

A. 6.90 g

B. 21.0 g

C. 9.39 g

D. 34.6 g

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

77. Look at the apparatus shown below. Inside each chamber there is a sample of a gas at the specified volume and pressure. Once the stopcock is opened, what will be the total pressure inside the system? The whole process is done under constant temperature.

A. 890 torr

B. 445 torr

C. 190 torr

D. 223 torr

Difficulty: hard

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

78. What volume of chlorine is consumed when it reacts with 12.0 g of hydrogen gas in the following equation at STP?

H₂(g) + Cl₂(g) → 2 HCl(g)

A. 1.07 L

B. 134 L

C. 268 L

D. 1.86 L

Difficulty: medium

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

79. A mixture of 10.0 g of Ne and 10.0 g of Ar was kept in a 1.00 L container at 765 torr. Calculate the partial pressure of Ar inside the container.

A. 508 torr

B. 257 torr

C. 614 torr

D. 125 torr

Difficulty: medium

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

80. What volume of sulfur dioxide gas will be consumed when 12.0 L of oxygen is consumed in the following equation at STP?

2 SO₂(g) + O₂(g) → 2 SO₃(g)

A. 6.00 L

B. 12.0 L

C. 24.0 L

D. 60.0 L

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

81. What volume of dinitrogen pentoxide gas is produced when 500. mL of oxygen react completely in the following equation at STP?

2 N₂(g) + 5 O₂(g) → 2 N₂O₅(g)

A. 500. mL

B. 400. mL

C. 1250 mL

D. 200. mL

Difficulty: easy

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

82. At the same temperature and pressure an 11.2-L sample of nitrogen contains the same number of molecules as

A. 8.00 g of oxygen

B. 16.0 g of oxygen

C. 22.4 L of oxygen

D. 5.60 L of oxygen

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

83. At the same temperature and pressure a 64.0-g sample of oxygen contains the same number of molecules as

A. 44.8 L of nitrogen

B. 14.01 g of nitrogen

C. 24.8 L of nitrogen

D. 28.02 g of nitrogen

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

84. Which gas is most dense at STP?

A. Helium

B. Nitrogen

C. Oxygen

D. Hydrogen

Difficulty: medium

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

85. Which gas has approximately the same density as carbon dioxide gas at STP?

A. CH₄

B. C₂H₆

C. C₃H₈

D. C₄H₁₀

Difficulty: medium

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

86. What mass of helium would be contained within a 1.8 L balloon at a pressure of 766 torr and a temperature of 24.5°C?

• 1. 3.61 g
  2. 0.297 g
  3. 226 g
  4. 0.594 g

Difficulty: easy

Learning Objective: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

87. When the following reaction took place at 23.8 °C and a pressure of 758 torr, 3.90 L of O₂(g) were collected. What mass of KClO₃ decomposed?

2KClO₃(s) 2KCl(s) + 3O₂(g)

1. 163 g
2. 19.6 g
3. 13.0 g
4. 39.1 g

Difficulty: hard

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles

Learning Objective 2: Solve stoichiometric problems involving gases.

Section References: 12.6 and 12.9

88. A mixture containing 5.00 g of H₂(g) and 10.0 g of O₂(g) is allowed to react in a 15.0 L rigid container at a constant temperature of 25.0°C.

2H₂(g) + O₂(g) 2H₂O(l)

Once the reaction is complete, what will be the pressure of the excess gas inside the container?

1. 1.51 atm
2. 4.04 atm
3. 3.53 atm
4. 3.02 atm

Difficulty: hard

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Learning Objective 2: Solve stoichiometric problems involving gases.

Section References: 12.7 and 12.9

Question type: True/False

89. A real gas most closely resembles an ideal gas at high temperature and low pressure.

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

90. The pressure of a gas is directly proportional to the number of gas molecules present.

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

91. When the temperature of a gas in a cylinder of fixed volume is increased, the internal pressure of the gas increases.

Difficulty: easy

Learning Objective 1: Explain atmospheric pressure and how it is measured. Be able to convert among the various units of pressure.

Section Reference: 12.1

92. The ideal gas law is obeyed by gases under the assumption that the size of their particles is negligible compared to the distance between them.

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

93. Strong intermolecular forces are present between the molecules of an ideal gas.

Difficulty: easy

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

94. The volume of a gas, at constant pressure, is inversely proportional to its absolute temperature.

Difficulty: easy

Learning Objective 1: Use Charles’ law to calculate changes in temperature or volume of a sample of gas at constant pressure.

Section Reference: 12.3

95. The volume of a gas, at constant temperature, is inversely proportional to its pressure.

Difficulty: easy

Learning Objective 1: Use Boyle’s law to calculate changes in pressure or volume of a sample of gas at a constant temperature.

Section Reference: 12.2

96. The volume of one mole of any ideal gas at STP is 22.4 L.

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

97. Equal volume of oxygen and nitrogen gas contains equal number of atoms.

Difficulty: easy

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

98. Ideal gas molecules do not occupy any space and have intermolecular attractions.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles.

Section Reference: 12.6

99. According to Dalton’s law of partial pressures; in a mixture of gases each gas behaves as if it were alone.

Difficulty: medium

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

100. Ideal gas obeys gas laws under all conditions of temperature and pressure.

Difficulty: medium

Learning Objective 1: Use the ideal gas law to solve problems involving pressure, volume, temperature, and number of moles

Section Reference: 12.6

Question type: Free Response

101. A 400. mL sample of hydrogen gas is collected over water at 20.0 ^° C and 760.0 torr.

The vapor pressure of water at 20.0^°C is 17.5 torr. What volume will the dry hydrogen gas occupy at 20.0 ^° C and 760. torr?

Difficulty: medium

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

102. A 250. mL sample of methane gas is collected over water at 21.0 ^° C and 768.0 torr.

The vapor pressure of water at 21.0 ^° C is 18.7 torr. What volume will the dry methane gas occupy at STP?

Difficulty: medium

Learning Objective 1: Use Dalton’s law of partial pressures to calculate the total pressure from a mixture of gases or the pressure of a single gas in a mixture of gases.

Section Reference: 12.7

103. A 28.0 L sample of a gas has a mass of 14.6 g at 23.0 ^° C and 1.05 atm. What is the density of the gas at STP?

Difficulty: easy

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

104. A 15.0 L sample of a gas has a mass of 18.0 g at 25.0 ^° C and 740. torr. What is the density of the gas at STP?

Difficulty: easy

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

105. Ammonia gas is produced from nitrogen gas and hydrogen gas.

A. Write a balanced chemical equation for this reaction.

B. What mass of ammonia is produced from the complete reaction of 20.0 L of nitrogen in this reaction at STP?

C. What volume of ammonia is produced from the complete reaction of 20.0 L of hydrogen in this reaction at STP?

Difficulty: medium

Learning Objective 1: Solve stoichiometric problems involving gases.

Section Reference: 12.9

106. What is the molar mass of a gas if 36.4 g of the gas occupies 100.0 L at 32.0 ^° C and 0.800 atm?

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

107. What is the molar mass of a gas if 10.00 g of the gas occupies 13.60 L at 20.00 ^° C and

1.050 atm?

Difficulty: medium

Learning Objective 1: Solve problems using the relationship among moles, mass, and volume of gases.

Section Reference: 12.4

108. The density of an unknown gas at STP is 1.63 g/L. Is the gas H₂(g), N₂(g), HCl(g), or CO₂(g)?

Difficulty: easy

Learning Objective 1: Calculate the density of a gas.

Section Reference: 12.8

109. A small, 0.500 mL, bubble forms at the bottom of a lake where the temperature is 2.0 ^°C and the pressure is 2.40 atm. What volume will the bubble occupy near the surface where the temperature is 32.0 ^° C and the pressure is 1.10 atm?

Difficulty: medium

Learning Objective 1: Use the Combined gas law to calculate changes in pressure temperature, or volume of a sample of gas.

Section Reference: 12.5