Test Bank Bauer The Gaseous State Chapter 9

Introduction to Chemistry, 5e (Bauer)

Chapter 9 The Gaseous State

1) Which of the following is not a property of gases?

A) Gases are compressible.

B) Gases expand to fill their containers.

C) The density of a gas is similar to that of a liquid.

D) Gas particles move about rapidly.

E) If one property, such as pressure or volume, or a gas changes, one or more other properties must change as well.

2) Which of the following is not a property of gases?

A) Gases consist of particles that are relatively far apart.

B) Gases can be compressed in a container.

C) Gas particles collide with one another.

D) When gas particles collide, attractive forces keep them attached to one another.

E) When gases are stored under pressure, their densities increase.

3) Which physical characteristic does not apply to a gas?

A) It can be compressed.

B) Its molecules are separated by large distances.

C) It occupies the total volume of its container.

D) It has a high density.

E) It can be formed by the evaporation of its liquid state.

4) Which of the following statements is incorrect?

A) Warm air is less dense than cold air.

B) Warm air rises above cold air.

C) When gases are heated, they expand.

D) The properties of gases are very similar to the properties of liquids.

E) Many properties of gases are the same, regardless of the chemical makeup of the gases.

5) The "Before" image in the figure shows the initial condition of a gas at a certain temperature in a container with a movable piston. Which of the images represents the condition of the gas when the temperature of the gas is increased, and the external pressure is held constant?

A) image I

B) image II

C) image III

D) image IV

E) None of the images

6) Which of the following statements regarding gas pressure is correct?

A) Gas pressure is commonly measured in units of pounds per square foot.

B) The pressure of air on the outside of a metal can with a low internal pressure is sufficient to crush the can.

C) If the volume of a container filled with a gas increases at constant temperature, the pressure will also increase.

D) If the temperature of a gas sample increases while the gas is held at a constant volume, the pressure will decrease.

E) When the volume of a container of a gas increases, the gas particles will stay together in the bottom of the container.

7) The figure shows a "Before" image of gas atoms at a certain temperature. If the volume of the container increases, and the temperature remains constant, which of the images represents the final condition of the gas?

A) image I

B) image II

C) image III

D) image IV

E) None of the images

8) Convert 689 torr to atm.

A) 0.689 atm

B) 0.760 atm   

C) 0.906 atm

D) 1.10 atm

E) 9.98 x 107 atm

9) Convert 723 torr to atm.

A) 7.32 x 107 atm

B) 0.723 atm

C) 0.760 atm

D) 0.951 atm

E) 1.05 atm

10) Convert 705 torr to atm.

A) 7.01 x 107 atm

B) 0.705 atm

C) 0.928 atm

D) 1.08 atm

E) 5.36 x 105 atm

11) Convert 1.13 atm to torr.

A) 1.13 x 103 torr

B) 1.14 x 105 torr

C) 859 torr

D) 1.16 x 10-3 torr

E) 1.49 x 10-3 torr

12) Convert 1.28 atm to mm Hg.

A) 1.28 x 103 mm Hg

B) 1.30 x 105 mm Hg

C) 1.68 x 10-3 mm Hg

D) 972.8 mm Hg

E) 1.03 x 10-3 mm Hg

13) According to kinetic-molecular theory, in which of the following gases will the average speed of the molecules be the highest at 400°C?

A) HF

B) Cl2

C) H2O

D) SF6

E) SO2

14) Convert 0.157 atm to mm Hg.

A) 119 mm Hg

B) 8.38 x 10-3 mm Hg

C) 2.07 x 10-4 mm Hg

D) 0.157 mm Hg

E) 1.59 x 104 mm Hg

15) Convert 6.25 x 104 Pa to mm Hg.

A) 0.617 mm Hg

B) 469 mm Hg

C) 4.75 x 107 mm Hg

D) 82.2 mm Hg

E) 625 mm Hg

16) Convert 986 mm Hg to Pa.

A) 1.30 Pa

B) 1.01 x 103 Pa

C) 1.31 x 105 Pa

D) 9.99 x 107 Pa

E) 7.49 x 105 Pa

17) Which of the following statements is incorrect? (Assume a fixed amount of gas under constant temperature conditions.)

A) Boyle's law says that the volume occupied by a gas is inversely proportional to its pressure.

B) If the volume of a container of gas is halved, the pressure will be doubled.

C) If the volume of a container of gas is tripled, the pressure will decrease by a factor of three.

D) When the volume of a container is increased, the distance between the gas particles decreases.

E) If the pressure on a gas sample is quadrupled, the volume will decrease by a factor of four.

18) If the initial pressure of a 2.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 3.00 L at constant temperature?

A) 1.50 atm

B) 1.67 atm

C) 15.0 atm

D) 2.40 atm

E) 0.600 atm

19) If a 1.50 L gas sample is held at a constant temperature, and its pressure is changed from 2.30 atm to 3.60 atm, what will the final volume be?

A) 1.50 L

B) 3.45 L

C) 0.958 L

D) 8.28 L

E) 0.828 L

20) If a 2.75 L gas sample is held at a constant temperature, and its pressure is changed from 750.0 torr to 360.0 torr, what will the final volume be?

A) 2.75 L

B) 5.73 L

C) 1.32 L

D) 1.41 L

E) 2.92 L

21) If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?

A) 5.50 atm

B) 2.50 atm

C) 7.50 atm

D) 1.88 atm

E) 0.533 atm

22) Which of the following statements is incorrect? (Assume that pressure and amount of gas are constant.)

A) Charles's law says that volume is directly proportional to temperature.

B) If the absolute temperature of a gas doubles, then the volume of the gas will double.

C) If the volume of a gas is halved, then the absolute temperature of the gas will be halved also.

D) If the temperature of a gas sample decreases from 50oC to 25oC, the pressure will be halved.

E) When a gas is cooled, the particles move more slowly.

23) If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

A) become higher because of fewer collisions with the container.

B) become lower because of fewer collisions with the container.

C) become lower because of more collisions with the container.

D) become higher because of more collisions with the container.

E) stay the same because temperature has no effect on pressure.

24) If the temperature of a gas at a constant pressure is increased, the volume will

A) become smaller because of fewer collisions with the sides of the container.

B) become larger because of fewer collisions with the sides of the container.

C) become smaller because of more collisions with the sides of the container.

D) become larger because of more collisions with the sides of the container.

E) stay the same because temperature has no effect on pressure.

25) Charles's Law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature. Which of the following is a consequence of Charles's Law?

A) Oxygen cylinders are often used by climbers on Mt. Everest.

B) Underwater divers often use air cylinders.

C) Gases can be condensed to liquids at certain temperatures and pressures.

D) A sealed balloon will rise if the air in it is heated.

E) Application of sufficient pressure to carbon dioxide gas produces solid dry ice.

26) The pressure-volume relationship expressed by Boyle's law can be explained by the kinetic molecular theory as follows:

A) When a gas is subjected to more pressure, more of the gas dissolves in a liquid.

B) When the volume of a gas is decreased, its molecules become closer together, causing more frequent collisions with the walls of the container.

C) The volume of a gas decreases as the pressure applied to the gas increases.

D) When the volume is decreased, the increased temperature causes the molecules to move faster and to hit the walls of the container more frequently.

E) The pressure of a gas results from its molecules being so close to one another that they cause the container walls to bulge.

27) Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0oC to 30.0oC.

A) 1.00 L   

B) 4.00 L

C) 2.20 L    

D) 0.455 L

E) 1.82 L

28) Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0oC to 30.0oC.

A) 1.17 L

B) 10.5 L

C) 4.19 L

D) 2.92 L

E) 1.75 L

29) A gas in a closed container with constant volume is heated from room temperature to 100°C. According to the kinetic molecular theory, the

A) average velocity of the molecules will increase.

B) gas will increase in weight.

C) individual molecules of the gas will increase their size.

D) average distance between molecules will increase.

E) pressure on the sides of the container will decrease.

30) Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0°C were to have a final volume of 1.50 L.

A) 2.0°C

B) 127°C

C) −146°C

D) 9.8°C

E) 43.2°C

31) Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0°C were to have a final volume of 3.50 L.

A) 46.0°C

B) 89.5°C

C) 169°C

D) 319°C

E) 592°C

32) A given mass of gas in a rigid container is heated from 100°C to 500°C.  Which of the following best describes what will happen to the pressure of the gas?

A) The pressure will remain the same.

B) The pressure will decrease by a factor of five.

C) The pressure will increase by a factor of five.

D) The pressure will increase by a factor less than five.

E) The pressure will increase by a factor greater than five.

33) Given a fixed amount of gas in a rigid container (no change in volume), what pressure will the gas exert if the pressure is initially 2.50 atm at 22.0°C, and the temperature is changed to 66.0°C?

A) 7.50 atm

B) 2.87 atm

C) 0.833 atm

D) 2.50 atm

E) 3.75 atm

34) Given a fixed amount of gas in a rigid container (no change in volume), what pressure will the gas exert if the pressure is initially 1.50 atm at 22.0°C, and the temperature is changed to 11.0°C?

A) 0.750 atm

B) 3.00 atm

C) 1.56 atm

D) 1.44 atm    

E) 301 atm

35) Given a fixed amount of gas in a rigid container (no change in volume), what temperature will the gas have to be changed to if the pressure is initially 3.50 atm at 22.0°C, and the desired final pressure is 1.75 atm?

A) −126°C

B) 11.0°C

C) 44.0°C

D) 148°C

E) −148°C

36) Given a fixed amount of gas in a rigid container (no change in volume), what temperature will the gas have to be changed to if the pressure is initially 1.50 atm at 42.0°C, and the desired final pressure is 3.00 atm?

A) 84.0°C

B) 21.0°C

C) 630°C

D) 357°C

E) 273°C

37) For which of the following changes is it not clear whether the volume of a particular sample of an ideal gas will increase or decrease?

A) increase the temperature and increase the pressure

B) decrease the temperature and increase the pressure

C) increase the temperature and decrease the pressure

D) increase the temperature and keep the pressure constant

E) keep temperature constant and decrease the pressure

38) A sample of gas initially occupies 3.35 L at a pressure of 0.950 atm at 13.0°C. What will the volume be if the temperature is changed to 22.5°C, and the pressure is changed to 1.05 atm?

A) 5.13 L

B) 3.13 L

C) 1.79 L

D) 2.93 L

E) 3.58 L

39) A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0°C. What will the volume be if the temperature is changed to 11.5°C, and the pressure is changed to 1.50 atm?

A) 2.31 L

B) 1.20 L

C) 4.82 L

D) 2.50 L

E) 7.21 L

40) A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0°C. What will the pressure be if the temperature is changed to 22.5°C, and the volume is changed to 1.50 L?

A) 6.39 atm

B) 11.4 atm

C) 0.211 atm

D) 2.84 atm

E) 1.59 atm

41) A sample of gas initially occupies 2.50 L at a pressure of 0.900 atm at 22.0°C. What will the pressure be if the temperature is changed to 56.5°C, and the volume is changed to 1.50 L?

A) 0.584 atm

B) 3.85 atm

C) 1.68 atm

D) 1.34 atm

E) 3.77 atm

42) A sample of gas initially occupies 2.50 L at a pressure of 905 torr at 22.0°C. What will the temperature be if the pressure is changed to 2.00 atm, and the volume is changed to 1.50 L?

A) 22.2°C

B) 554°C

C) 1.09°C

D) 271°C

E) 24.5°C

43) A sample of gas initially occupies 3.50 L at a pressure of 795 torr at 32.0°C. What will the temperature be if the pressure is changed to 4.00 atm, and the volume is changed to 1.50 L?

A) 0.658°C

B) 225°C

C) 244°C

D) 52.2°C

E) 3.60°C

44) Calculate the number of moles and the mass of gas in 3.40 L of He at STP.

A) 0.152 mol, 0.608 g

B) 76.2 mol, 305 g

C) 0.152 mol, 0.0379 g

D) 76.2 mol, 19.0 g

E) 1.00 mol, 4.00 g

45) Calculate the number of moles and the mass of gas in 10.2 L of O2 at STP.

A) 0.455 mol, 7.28 g

B) 0.455 mol, 14.6 g

C) 228 mol, 7.14 g

D) 228 mol, 3648 g

E) 1.00 mol, 32.0 g

46) Calculate the number of moles and the mass of gas in 5.25 L of N2 at STP.

A) 0.234 mol, 0.00836 g

B) 0.234 mol, 3.28 g    

C) 0.234 mol, 6.56 g

D) 118 mol, 4.20 g

E) 118 mol, 1652 g

47) Calculate the number of moles and the mass of gas in 2.50 L of Ar at STP.

A) 56.0 mol, 784 g

B) 56.0 mol, 2.00 g

C) 0.112 mol, 0.00279 g

D) 0.112 mol, 4.47 g

E) 1.00 mol, 40.0 g

48) In January a balloon is taken inside where the temperature is 25°C.  If the balloon is filled to 2.0 L at –20°C outside, what will happen to the balloon when taken inside?

A) The balloon expands because the higher temperature will increase the speed of the molecules.

B) Nothing happens to the balloon because temperature has no affect on the behavior of gases.

C) The balloon compresses because the higher temperature will cause the molecules get bigger.

D) The balloon expands because the higher temperature will cause the molecules to slow down.

E) The balloon compresses because the higher temperature will increase the speed of the molecules.

49) A balloon is filled with helium at sea level, and then taken into the mountains to an elevation of 7500 feet. Assuming the temperatures are the same, what will happen to the balloon?

A) The balloon will compress because the lower pressure will increase the speed of the molecules.

B) Nothing happens to the balloon because pressure has no affect on the behavior of gases.

C) The balloon expands because the molecules get bigger.

D) The balloon expands because the molecules move faster.

E) The balloon will expand because the external pressure in the mountains is lower.

50) The two balloons shown in the figure each have the same volume, temperature, and pressure. Which of the following statements regarding the two balloons is correct?

A) The CO2 balloon has fewer molecules than the O2 balloon.

B) The density of the O2 balloon is greater than the density of the CO2 balloon.

C) The mass of the O2 balloon is greater than the mass of the CO2 balloon.

D) The CO2 balloon is more buoyant than the O2 balloon.

E) None of these statements is correct.

51) The two balloons shown in the figure have the same volume, and are at the same temperature and pressure. Which balloon has the greater number of gas particles, and why?

A) The Ar balloon has fewer molecules than the He balloon.

B) The density of the Ar balloon is greater than the density of the He balloon.

C) The mass of the He balloon is greater than the mass of the Ar balloon.

D) The CO2 balloon is more buoyant than the O2 balloon.

E) The He balloon has fewer moles than the He balloon.

52) A liter container of CO2 and a liter container of H2 are both at 25°C and 1 atm pressure. Which of the following statements about these gas samples is true?

A) The CO2 and H2 molecules have the same average velocity.

B) There are more H2 molecules than CO2 molecules.

C) The average kinetic energy of the CO2 molecules is greater than that of the H2 molecules.

D) The CO2 molecules on average are moving more slowly than the H2 molecules.

E) The masses of the two gas samples are equal.

53) The number of molecules in equal volumes of two different gases under the same conditions of temperature and pressure are

A) widely different.

B) extremely numerous.

C) impossible to compare without specific data.

D) equal.

E) greater for the molecule with the greater molar mass.

54) Calculate the number of moles in 7.5 g of Ar, and the volume that it would occupy at STP.

A) 0.19 mol, 0.0085 L

B) 0.19 mol, 4.2 L

C) 3.0 x 102 mol, 13 L

D) 3.0 x 102 mol, 6.7 x 103 L

E) 1.0 mol, 22 L

55) Calculate the number of moles in 75 g of O2, and the volume that it would occupy at STP.

A) 2.3 mol, 52 L

B) 2.3 mol, 0.10 L

C) 2.4 x 103 mol, 107 L

D) 2.4 x 103 mol, 5.4 x 104 L

E) 4.7 mol, 52 L

56) Calculate the number of moles in 55 g of N2, and the volume that it would occupy at STP.

A) 2.0 mol, 45 L

B) 2.0 mol, 0.089 L

C) 1.5 x 103 mol, 67 L

D) 1.5 x 103 mol, 3.4 x 104 L

E) 3.9 mol, 88 L

57) Calculate the number of moles in 55 g of an unknown gas, and the volume that it would occupy at STP.

A) 2.0 mol, 45 L

B) 2.0 mol, 0.089 L

C) 1.5 x 103 mol, 67 L

D) 1.5 x 103 mol, 3.4 x 104 L

E) not enough information

58) Assuming that all of the gas in the tank in the figure is used to fill balloons with an average volume of 2.0 L of helium, approximately how many balloons could be filled at STP?

A) about 45 balloons

B) about 106 balloons

C) about 210 balloons

D) about 850 balloons

E) about 1200 balloons

59) Calculate the number of moles in 75.0 g of N2, and the volume that it would occupy at 50.0°C and 1.50 atm.

A) 2.68 mol, 60.0 L

B) 2.68 mol, 47.4 L

C) 2.10 x 103 mol, 93.7 L

D) 2.10 x 103 mol, 4.71 x 104 L

E) 5.36 mol, 121 L

60) Calculate the number of moles in 95.0 g of O2, and the volume that it would occupy at 80.0°C and 3.50 atm.

A) 11.9 mol, 266 L

B) 5.94 mol, 11.1 L

C) 5.94 mol, 49.2 L

D) 2.97 mol, 24.6 L

E) 2.97 mol, 5.57 L

61) Calculate the number of moles in 75.0 g of O2, and the pressure that it would exert at 80.0°C in a 5.00 L steel tank.

A) 4.69 mol, 6.18 atm

B) 4.69 mol, 27.2 atm

C) 2.34 mol, 13.6 atm

D) 2.34 mol, 3.09 atm

E) 9.38 mol, 27.2 atm

62) Calculate the number of moles in 45.0 g of N2, and the pressure that it would exert at 20.0°C in a 5.00 L steel tank.

A) 1.61 mol, 0.525 atm

B) 1.61 mol, 7.74 atm

C) 3.21 mol, 15.48 atm

D) 3.21 mol, 1.05 atm

E) 6.43 mol, 31.0 atm

63) Calculate the number of moles and the mass of Ar gas present in a 3.00 L steel container if the pressure is 5.75 atm, and the temperature is 22.0°C.

A) 1.00 mol, 40.0 g

B) 0.712 mol, 28.4 g

C) 9.56 mol, 382 g

D) 6.20 x 104 mol, 1.55 x 103 g

E) 4.59 x 103 mol, 1.84 x 105 g

64) Calculate the number of moles and the mass of He gas present in a 2.00 L steel container if the pressure is 6.50 atm, and the temperature is 42.0°C.

A) 1.00 mol, 4.00 g

B) 0.503 mol, 2.01 g

C) 3.77 mol, 15.1 g

D) 4.99 x 104 mol, 1.25 x 104 g

E) 6.65 x 103 mol, 2.66 x 105 g

65) Two balloons are at the same temperature and pressure, and contain equal volumes of gas, but one is floating, and the other is not. The reason for this behavior is that:

A) the balloon that is not floating has the molecules more closely spaced than the other.

B) the balloon that is not floating has a gas with a higher molar mass than that of air.

C) the balloon that is floating has molecules with more kinetic energy.

D) the balloon that is not floating has molecules that have slowed down, since it was filled before the floating balloon.

E) the balloon that is floating has a more dense gas than the one that is not floating, so it holds up the balloon better.

66) Two balloons are at the same temperature and pressure, and contain equal volumes of gas, but one is floating, and the other is not. Suggest a possible composition for the contents of the balloons.

A) The floating balloon contains CO2, while the other contains SO2.

B) The floating balloon contains SO2, while the other contains CO2.

C) The floating balloon contains Ne, while the other contains CO2.

D) The floating balloon contains Ar, while the other contains He.

E) None of these answers could be correct.

67) Equal volumes of methane (CH4) and hydrogen (H2) gases under the same conditions of temperature and pressure have equal

A) numbers of molecules.

B) masses.

C) numbers of atoms.

D) numbers of covalent bonds.

E) average velocities.

68) Calculate the density of NO2 in g/L at STP.

A) 22.41 g/L

B) 2.053 g/L

C) 1.031 x 103 g/L

D) 0.04462 g/L

E) 0.4871 g/L

69) Calculate the density of CO2 in g/L at STP

A) 22.41 g/L

B) 1.964 g/L

C) 9.864 x 102 g/L

D) 0.02272 g/L

E) 0.5092 g/L

70) Calculate the density of Ar in g/L at 20.0°C and 695 torr.

A) 22.41 g/L

B) 1.71 x 104 g/L

C) 1.18 x 103 g/L

D) 1.52 g/L

E) 8.86 g/L

71) Calculate the density of Ne in g/L at 22.0°C and 735 torr.

A) 22.41 g/L

B) 8.22 x 103 g/L

C) 6.12 x 102 g/L

D) 0.806 g/L

E) 1.24 g/L

72) Which of the following gases will have a density of 2.104 g/L at 303 K and 1.31 atm?

A) He

B) Ne

C) Ar

D) Kr

E) Xe

73) If a 5.00 L container is filled with H2 to a pressure of 975 torr at 23.0°C, calculate the mass of the hydrogen in the container.

A) 0.263 g   

B) 0.530 g

C) 201 g

D) 404 g

E) 258 g

74) If a 4.00 L container is filled with N2 to a pressure of 895 torr at 53.0°C, calculate the mass of the nitrogen in the container.

A) 0.176 g

B) 4.93 g

C) 134 g

D) 5.68 g

E) 0.202 g

75) If a 7.00 L container is filled with O2 to a pressure of 995 torr at 33.0°C, calculate the mass of the oxygen in the container.

A) 11.7 g

B) 0.365 g

C) 277 g

D) 2.57 x 103 g

E) 0.0854 g

76) The total pressure of a mixture of gases

A) is always constant.

B) increases as the temperature is lowered.

C) equals the sum of the partial pressures of the individual gases.

D) equals the difference between the partial pressures of the individual gases.

E) is proportional to the average of the boiling points of the gases.

77) A sample of CO2 is collected over water at 23°C. If the total pressure of the sample is 734 torr, what is the partial pressure of the CO2? The vapor pressure of water at 23°C is 21.2 torr.

A) 734 torr

B) 755 torr

C) 713 torr

D) 34.6 torr

E) not enough information

78) A sample of O2 is collected over water at 21°C. If the total pressure of the sample is 712 torr, what is the partial pressure of the O2?  The vapor pressure of water at 21°C is 18.6 torr.

A) 712 torr

B) 731 torr

C) 693 torr

D) 38.3 torr

E) not enough information

79) A sample of N2 is collected over water at 24°C. If the total pressure of the sample is 694 torr, what is the partial pressure of the N2? The vapor pressure of water at 24°C is 22.4 torr.

A) 672 torr

B) 694 torr

C) 0.913 atm

D) 716 torr

E) 31.0 torr

80) A sample of H2 is collected over water at 22°C. If the total pressure of the sample is 744 torr, what is the partial pressure of the H2? The vapor pressure of water at 22°C is 19.8 torr.

A) 37.6 torr

B) 0.979 atm

C) 764 torr

D) 724 torr

E) 744 torr

81) Calculate the molar mass of a gas that has a density of 1.963 g/L at STP.

A) 11.42 g/mol

B) 19.63 g/mol

C) 44.00 g/mol

D) 0.08758 g/mol

E) 0.5094 g/mol

82) Calculate the molar mass of a gas that has a density of 1.250 g/L at STP.

A) 11.42 g/mol

B) 12.50 g/mol

C) 28.02 g/mol

D) 0.05577 g/mol

E) 0.8000 g/mol

83) Calculate the molar mass of a gas that has a density of 1.428 g/L at STP.

A) 15.70 g/mol

B) 14.28 g/mol

C) 0.4460 g/mol

D) 32.01 g/mol

E) 0.7002 g/mol

84) Which characteristic does not describe an ideal gas?

A) negligible volume occupied by ideal gas molecules

B) no attractive forces between ideal gas molecules

C) obeys the equation PV = nRT

D) PV/RT = a constant

E) strong repulsions between molecules

85) Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?

A) Gases are composed of small particles with a small amount of space between them.

B) Gas particles move in a zigzag pattern until they collide with something.

C) When gas particles collide, they lose some of their kinetic energy, and will slow down over time.

D) In a mixture of gases, attractive forces between particles cause the measured pressure to be lower than that expected for a pure gas.

E) The pressure of a gas arises from the sum of the collisions of the particles with the walls of the container.

86) Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?

A) There are no attractive or repulsive forces between and among gas particles.

B) Gas particles move slowly in a chaotic pattern until they collide with something.

C) For a given amount of gas, the smaller the volume of the container, the fewer the collisions that occur with the container walls, since there is less surface area.

D) The density of a gas is somewhat lower than that of a liquid.

E) The more gas particles there are in a container, the more frequently they collide with one another, so the particles stick together, resulting in a lower pressure.

87) Which of the following statements related to kinetic-molecular theory of gases is correct for an ideal gas?

A) There is a very small range of measured velocities for the particles in a given gas sample.

B) When the temperature of a gas sample increases, the velocity of some of the particles increases, while others slow down, so that the average velocity stays the same.

C) Larger particles move faster than smaller gas particles because they have more momentum.

D) The average kinetic energy of gas particles depends only on the absolute temperature.

E) Larger gas particles strike the walls of the container harder, so a given amount of argon in a container will have a higher pressure than the same amount of helium under similar conditions.

88) It can be observed experimentally that the volume of a gas will be decreased by applying pressure. This observation is best explained by the assumption that

A) the average kinetic energy of gas molecules is directly proportional to the absolute temperature.

B) gas molecules collide without loss of kinetic energy.

C) gas molecules are small compared to the distance between them.

D) gas molecules exert almost no attractive forces on one another.

E) gas molecules become smaller.

89) A weather balloon filled with helium gas gets larger as it ascends to high altitudes. The expansion of the balloon is primarily due to

A) a decrease in the average kinetic energy of the helium atoms inside the balloon.

B) an increase in the average kinetic energy of the helium atoms inside the balloon.

C) a decrease in the average kinetic energy of the air molecules outside the balloon.

D) an increase in the rate of collision of the helium atoms against the inside walls of the balloon.

E) a decrease in the rate of collision of the air molecules on the outside walls of the balloon.

90) According to kinetic-molecular theory, molecules of different gases at the same temperature always have the same

A) molar mass.

B) pressure.

C) average kinetic energy.

D) volume.

E) number of moles.

91) Under which conditions does sulfur trioxide (SO3) have the greatest molar volume?

A) high temperature and low pressure

B) low temperature and high pressure

C) high temperature and high pressure

D) low temperature and low pressure

E) The molar volume is always 22.414 L.

92) Rank the following substances in order of increasing average velocity, assuming they are all at the same temperature:  O2, CO2, Ar, He

A) O2 < CO2 < Ar < He

B) CO2 < Ar < O2 < He

C) Ar < O2 < CO2 < He

D) CO2 < O2 < Ar < He

E) He < O2 < Ar < CO2

93) Rank the following substances in order of increasing average velocity, assuming they are all at the same temperature:  N2, CH4, Ne, Kr

A) N2 < CH4 < Ne < Kr

B) CH4 < Ne < N2 < Kr

C) Kr < N2 < Ne < CH4

D) Ne < CH4 < N2 < Kr

E) Ne < Kr < N2 < CH4

94) Rank the following substances in order of increasing average kinetic energy, assuming they are all at the same temperature:  N2, CH4, Ne, Kr

A) N2 < CH4 < Ne < Kr

B) CH4 < Ne < N2 < Kr

C) Kr < N2 < CH4 < Ne

D) Ne < CH4 < N2 < Kr

E) none of these choices is correct

95) Rank the following substances in order of increasing average kinetic energy, assuming they are all at the same temperature:   N2, CH4, Ne, Kr

A) N2 < CH4 < Ne < Kr

B) CH4 < Ne < N2 < Kr

C) Kr < N2 < CH4 < Ne

D) Ne < CH4 < N2 < Kr

E) none of these choices is correct

96) Under which conditions would the density of helium be the smallest?

A) high pressure and high temperature

B) low pressure and high temperature

C) high pressure and low temperature

D) low pressure and low temperature

E) The density of helium is independent of pressure and temperature.

97) Which gas diffuses more rapidly than the other gases under similar conditions?

A) oxygen, O2

B) hydrogen, H2

C) nitrogen, N2

D) fluorine, F2

E) sulfur dioxide, SO2

98) Which of these gases would leak fastest from a balloon with a small hole?    

A) H2

B) Ar

C) NH3

D) O2

E) Ne

99) Which of the following gases would have the highest average molecular speed at 25oC?

A) O2

B) N2

C) CO2

D) CH4

E) SO2

100) Propane burns in air according to the equation:

                         C3H8(g) + 5O2(g) → 3CO2(g)  + 4H2O(g)

What volume of CO2 would be formed if 5.00 L of propane burns, assuming that all of the gases are under the same conditions?

A) 5.00 L

B) 15.0 L

C) 3.00 L   

D) 4.00 L

E) 1.67 L

101) Propane burns in air according to the equation:

                             C3H8(g) + 5O2(g) → 3CO2(g)  + 4H2O(g)

What volume of CO2 would be formed if 8.00 L of propane burns, assuming that all of the gases are under the same conditions?

A) 8.00 L

B) 12.0 L

C) 24.0 L

D) 3.00 L

E) 2.67 L

102) Propane burns in air according to the equation:

            C3H8(g) + 5O2(g) → 3CO2(g)  + 4H2O(g)

What volume of O2 would be required if 8.00 L of propane burns, assuming that all of the gases are under the same conditions?

A) 8.00 L   

B) 40.0 L

C) 20.0 L

D) 15.0 L

E) 1.60 L

103) Propane burns in air according to the equation:

                    C3H8(g) + 5O2(g) → 3CO2(g)  + 4H2O(g)

What volume of O2 would be required if 5.00 L of propane burns, assuming that all of the gases are under the same conditions?

A) 25.0 L

B) 15.0 L

C) 5.00 L

D) 20.0 L

E) 1.00 L

104) What volume of H2 would be collected at 22.0oC and a pressure of 713 torr if 2.65 g of zinc react according to the equation:

                                            Zn(s) + 2HCl(aq) → ZnCl2(aq)  + H2(g)

A) 0.908 L

B) 0.0405 L

C) 1.04 L

D) 2.08 L

E) 0.523 L

105) What volume of H2 would be collected at 21.5oC and a pressure of 695 torr if 5.25 g of zinc react according to the equation:

                                               Zn(s) + 2HCl(aq) → ZnCl2(aq)  + H2(g)

A) 1.06 L

B) 4.25 L

C) 1.80 L

D) 2.12 L

E) 5.49 L

106) Oxygen gas can be prepared in the laboratory by heating potassium chlorate, so that it decomposes according to the equation:

                                       2KClO3(s) → 2KCl(s) + 3O2(g)

What would the pressure of O2 be in a 2.00 L glass container at 23.5oC if 5.75 g of KClO3 is decomposed?

A) 0.0704 atm

B) 0.571 atm

C) 0.857 atm

D) 0.381 atm

E) 0.0651 atm

107) Oxygen gas can be prepared in the laboratory by heating potassium chlorate, so that it decomposes according to the equation:

                                                2KClO3(s) → 2KCl(s) + 3O2(g)

What would the pressure of O2 be in a 2.50 L glass container at 22.0oC if 6.50 g of KClO3 is decomposed? 

A) 0.0796 atm

B) 1.78 atm

C) 6.62 atm

D) 0.771 atm

E) 0.0575 atm

108) When the pressure on a sample of a gas is increased, the particles move closer together.

109) When the temperature of a gas sample is decreased, the particles move more slowly.

110) When the temperature of a gas sample is increased, the pressure of the gas decreases.

111) The molar volume of argon gas at standard temperature and pressure (STP) is larger than the molar volume of helium at STP, since the atoms are larger.

112) When working with gaseous products and reactants at constant temperature and pressure, it is possible to use volumes to calculate stoichiometric quantities.

113) If equal amounts of helium and argon are placed in a porous balloon, the argon will escape faster.

114) The reason that you can smell the lighter fluid from your neighbor's barbeque is that gases diffuse through the air.

115) The ideal gas law is a combination of several other gas laws which deal with fewer variables.

116) The kinetic-molecular theory of gases explains the behavior of gases.

117) If 60.0 L of nitrogen gas at 22.0oC is compressed to 30.0 L at constant pressure, what is the new temperature (in degrees Celsius) of the gas?

118) A steel tank contains gas at a pressure of 6.50 atm at 30.0oC. At what temperature (in degrees Celsius) will the pressure decrease to 5.00 atm?

119) If a steel tank is filled with acetylene to a pressure of 7.50 atm in the morning, when the temperature is 18.0oC, what will the pressure (in atm) be in the afternoon, when the temperature rises to 33.5oC?

120) What volume (in liters) of N2 at STP can be pumped into a 2.50 L tank at 22.4oC to give a pressure of 5.50 atm?

121) Propane burns in air according to the equation:

                C3H8(g) + 5O2(g) → 3CO2(g)  + 4H2O(g)

What volume of O2 in liters would be required if 15.0 L of propane burns, assuming that all of the gases are under the same conditions?