WOLPA/AP CHEMISTRY
CHAPTER TWELVE: GASES
Review Problems II
1. Kirsten is in her lab, and reacts two unknown gases (A(g) and B(g)) to get
nitrogen dioxide (NO2). Using her data, she is able to write the following balanced
equation:
2A(g) + B(g) --> 2NO2(g)
If she started with 8 L of A(g) and 3 L of B(g), how many liters of NO2(g) would
she get? [Assume everything is at STP.]
a.
b.
c.
d.
e.
2
3
4
6
8
L
L
L
L
L
2. Calculate the number of kilograms of O2(g) that can be stored in a compressed
gas chamber with a volume of 40 L when the cylinder is filled at 150 atm and
21oC.
a. 4.0 kg
b. 8.0 kg
c. 4000 kg
d. 8000 kg
e. Not enough information
3. Yesterday, Jason had a sample of helium indoors (T = 23oC) in a sealed
container, with a pressure of 760 mm Hg. He got bored and took the container
outside, where the temperature was a blistering 35oC. He calculated the new
pressure to be 750 mm Hg. Jason knew that this answer was not correct
because:
a. TK = ToC + 273.15
b. Equal volumes of gas have the same number of moles.
c. P is proportional to n
d. P is proportional to T
e. He forgot to convert his temperature to K and the pressure should have
decreased even more.
4. Suppose that Quebec had managed to succeed from Canada and became an
independent country. Just to be difficult, they decreed that they will only
measure pressure in mm Hg and volume in cm3. What value for R, the ideal gas
constant, would students in Quebec use when solving the ideal gas solution?
a. 7.6 x 105
b. 6.23 x 104
c. 8.14
d. 2.78
e. 0.082
5. Consider two 1 L flasks, one containing O2, the other containing He, each at STP.
Which of the following statements is NOT true regarding these gases?
a. Each flask contains the same number of atoms or molecules
b. The gases in each flask have the same average kinetic energy
c. The gases in each flask have the same density
d. The pressure in each flask is the same
e. The temperature of the gases in each flask is 273.15 K.
6. The density of N2 at STP is:
a. 1.25 g/L
b. 1.04 g/L
c. 0.625 g/L
d. 0.0625 g/L
e. 5.43 mg/L
7. A 1.00 L flask containing 450 torr of H2 is connected to and mixed with a second
flask with a volume of 0.500 L containing 250 torr N2. What is the final pressure
of the resulting mixed gas system?
a. 250 torr
b. 383 torr
c. 450 torr
d. 575 torr
e. it cannot be determined
8. A piston is used to compress a gas from 1.0 atm to 3.5 atm. If the volume
changes from 1.5 L to 0.75 L, what is the final temperature, if it started at 300
K?
a. 1050 K
b. 700 K
c. 525 K
d. 300 K
e. 150K
9. 2.00 g of sucrose is combusted in excess oxygen. What is the volume of dry CO2
that is formed at 1 atm pressure and 37oC? (MW sucrose = 342.3 g/mol)
C12H22O11 + 12O2 --> 12CO2 + 11H2O
a.
b.
c.
d.
e.
22.4 L
10.4 L
1.78 L
0.545 L
0.148 L
10. Which of the following statements regarding the kinetic-molecular theory of ideal
gases is incorrect?
a. gas molecules collide elastically
b. gases molecules are in random motion
c. the average kinetic energy is constant if T is constant
d. the kinetic energy of all the molecules is the same
e. attractive and repulsive forces can be neglected
11. Which of the following graphs does NOT correctly illustrate the ideal gas law?
12. The ideal gas law asserts that when two other variables are held constant:
a. n and V are inversely proportional.
b. n and T are directly proportional.
c. P and V are directly proportional.
d. n and T are inversely proportional.
e. P and T are inversely proportional.
13. What volume would a weather balloon containing 105 liters of helium at STP
occupy if the temperature fell to -90.0oC and the pressure fell to 8.45 torr (as it
must in the upper atmosphere)?
a. 0.783 L
b. 8.33 L
c. 6330 L
d. 9450 L
e. 14100 L
14. A balloon is filled with He to a pressure of 1.06 atm. The volume of the balloon
at 25oC is 1.30 x 104 L. How many cylinders of He gas are needed to fill the
balloon if the pressure in the cylinder at 20oC is 98.5 atm and the volume of the
cylinder is 40.0 L. [You may have some He left in one of the cylinders.]
a. 1
b. 2
c. 3
d. 4
e. 5
15. A sample of nitrogen dioxide gas occupies 76.3 mL at 35oC and 765 mm Hg. The
density of the nitrogen dioxide is:
a. 0.546 g/L
b. 1.39 g/L
c. 1.83 g/L
d. 18.2 g/L
e. 24.0 g/L
16. The density of CH4 gas at 0oC and P = 1 atm is four times that of gas X at the
same T, P. X could be:
a. H2
b. He
c. O2
d. C4H16
e. The identity of X cannot be determined from the given information.
17. Nitrogen gas escapes through a pinhole in 68.4 seconds. Under the same
conditions, a gaseous compound with the empirical formula CH2 escapes in 83.8
seconds. What is its molecular formula?
a. CH2
b. C2H4
c. C3H6
d. C4H8
e. C5H10
18. You have 3 identical balloons at room temperature. You inflate each one to the
same size, filling them with different gases. You put helium in balloon 1, nitrogen
in balloon 2, and xenon in balloon 3. You realize that the pressure inside each
balloon is equal to atmospheric pressure. You notice that balloon 1 floats to the
ceiling, balloon 2 feels light, and balloon 3 feels heavy. Which balloon contains
the most gas particles?
a. Balloon 1
b. Balloon 2
c. Balloon 3
d. Balloons 1 and 3 have equal numbers and more than Balloon 2 since
nitrogen atoms are bonded to each other.
e. All 3 balloons have the same number of gas particles.
19. A quantity of 73.0 g of NH3(g) is mixed with an equal mass of HCl(g). What is
the volume of the gas remaining (i.e., NH3 or HCl) measured at 14oC and 752
mm Hg after the reaction has gone to completion?
NH3(g) + HCl(g) --> NH4Cl(s)
a.
b.
c.
d.
e.
47.7 L HCl
51.0 L HCl
54.3 L NH3
102 L NH3
No gas remains since equal masses react.
20. A gas mixture at 25oC and a total pressure at 1.00 atm contains 1.03 g of each
of the following gases: H2, He, N2, CO2. Which has the highest molecular speed?
a. H2
b. He
c. N2
d. CO2
e. All have the same speed since all are at the same temperature in the
same container.
21. 16 g of O2 are mixed with 16 g of He in a container. The total gas pressure is 1.0
atm. The partial pressure of O2 is:
a. 0.11 atm
b. 0.13 atm
c. 0.5 atm
d. 0.89 atm
e. The partial pressure cannot be determined because the temperature and
volume of the container are not given.
22. At 20oC the rms speed of methane, CH4, produced by Indiana cows is
approximately:
a. 300 m/s
b. 700 m/s
c. 5 x 105 m/s
d. 10 m/s
e. 20 m/s
23. Van der Waals constant, a, that appears in the relationship
corrects for:
a.
b.
c.
d.
the density of gas molecules.
variation in the gas constant, R.
the volume occupied by the gas molecules.
the attractive forces between gas molecules.
24. A balloon contains 14.0 L of air at a pressure of 760 torr. What will the volume of
the air be when the balloon is taken to a depth of 10 ft in a swimming pool,
where the pressure is 981 torr? The temperature of the air in the balloon does
not change.
a. 8.8 L
b. 17.7 L
c. 15.4 L
d. 5.4 L
e. 10.8 L
25. A sample of freon gas used in an air conditioner has a volume of 325 L and a
pressure of 96.3 kPa at 20oC. What will be the pressure of the gas when its
volume is 975 L at 20oC?
a. 289 kPa
b. 32.1 kPa
c. 105 kPa
d. 96.3 kPa
e. 75.4 kPa
26. A particular hydrogen gas thermometer has a volume of 150.0 cm3 when
immersed in a mixture of ice and water (0.00oC). When immersed in boiling
liquid ammonia, the volume of the hydrogen, at the same pressure, is 131.7 cm3.
What is the temperature of the boiling ammonia?
a. -33oC
b. 38oC
c. 0.00oC
d. 235oC
e. -77oC
27. Methane, CH4, can be used as a fuel for an automobile; however, it is a gas at
normal temperatures and pressures, which causes a problem with storage. One
gallon of gasoline could be replaced by 655 g of CH4. What is the volume of this
much methane at 25oC and 745 torr? [At. Wts: C = 12.01 amu; H = 1.008 amu;
3.79 L = 1.00 gallon]
a. 9.55 gal
b. 175 gal
c. 269 gal
d. 1002 gal
e. 2515 gal
28. A hydrocarbon (containing the elements carbon and hydrogen) is commonly
used as an anesthetic. If a 2.00 L flask contains 3.11 g of the hydrocarbon gas at
684 torr and 23oC, what is the molecular formula of the hydrocarbon? [At. Wts:
C = 12.01 amu; H = 1.008 amu]
a. C5H10
b. C2H6
c. C2H4
d. C4H10
e. C3H6
29. What is the total pressure in atmospheres in a 10.0 L vessel containing 2.50 x
10-3 mol of H2, 1.00 x 10-3 mol of He, and 3 x 10-4 mol of Ne at 35oC?
a. 1.10 atm
b. 2.75 x 10-2 atm
c. 8.76 x 10-4 atm
d. 3.80 x 10-3 atm
e. 9.61 x 10-3 atm
30. A balloon contains 4.70 x 10-2 mol O2 and 8.87 x 10-2 mol N2 at a total pressure
of 1.00 atm. What is the partial pressure of O2 in the balloon?
a. 0.65 atm
b. 0.35 atm
c. 0.95 atm
d. 2.86 atm
e. 0.23 atm
31. A gas of unknown identity diffuses at the rate of 83.3 mL/s in a diffusion
apparatus in which a second gas, whose molecular weight is 44.0 amu, diffuses
at the rate of 102 mL/s. What is the molecular weight of the first gas?
a. 66.0 amu
b. 40.4 amu
c. 34.2 amu
d. 22.4 amu
e. 10.2 amu
32. Which of the following statements is not true?
a. The pressure of a real gas is greater than or equal to the pressure
calculated for an ideal gas.
b. The volume of a real gas is greater than or equal to the volume
calculated for an ideal gas.
c. The van der Waals equation helps to calculate the pressure and volume
of real gases.
d. Real gas molecules do occupy a finite, but small, volume.
e. Real gas molecules experience intermolecular forces.
33. The "a" term in the van der Waals equation arises because:
a. real gas molecules occupy a finite volume.
b. at high pressures the observed pressure is greater than the ideal
pressure.
c. the average kinetic energy of gas molecules is proportional to
temperature in Kelvin.
d. real gas molecules experience intermolecular forces.
e. the volume of real gas depends on root-mean-square velocity.
34. An atmospheric chemist isolates a gaseous pollutant. At STP she determines that
the density of the gas is 2.14 g/L. What is the identity of the pollutant?
a. NO
b. NO2
c. O3
d. SO2
e. SO3
35. In lecture, the composition of air was given to be by volume 78% N2, 21% O2,
and 1% other. If the total pressure of air inside a sealed container is 2.0 atm,
what is the partial pressure of the O2?
a. 0.10 atm
b. 0.21 atm
c. 0.42 atm
d. 1.0 atm
e. 2.0 atm
Consider these identical flasks filled with three different gases:
Flask A
CO at 760 torr and 0.0oC
Flask B
N2 at 250 torr and 0.0oC
Flask C
H2 at 100 torr and 0.0oC
36. In which flask will the molecules have the greatest average kinetic energy?
a. Flask A
b. Flask B
c. Flask C
d. All three have the same average kinetic energy.
e. Not enough information.
37. Which of the following assumptions of the kinetic molecular theory of gases is
not valid for real gases at high pressure?
a. The volume of the gas particles is much smaller than the distance
between the gas particles.
b. The gas particles behave like hard, spherical objects in a state of
constant, random motion.
c. The average kinetic energy of the gas particles depends upon
temperature of the gas only.
d. Collisions between gas particles are perfectly elastic. No energy of a gas
particle is lost when it collides.
e. The gas particles move in a straight line until they collide with another
particle or the walls of the container.
38. A gas sample occupies 400 mL at a pressure of 2.00 atm. What is the volume if
the pressure is changed to 20 atm at constant temperature?
a. 4000 mL
b. 20 mL
c. 40 mL
d. 800 mL
e. 8000 mL
39. What is the volume (L) occupied by 2.19 moles of methane gas (CH4) at 298 K
and 1 atm?
a. 0.0186
b. 4.5
c. 11.2
d. 49.2
e. 53.6
40. Which
a.
b.
c.
d.
e.
of the following is not a postulate of kinetic-molecular theory of gases?
Gases consist of large numbers of molecules in constant random motion.
Attractive and repulsive forces between gas molecules are negligible.
The volume of all the molecules of the gas is negligible.
Gas molecules collide frequently, and collisions are perfectly elastic.
At a given temperature, a gas with low molar mass has less kinetic
energy than a gas with high molar mass.
41. 2.00 moles of Cl2 gas at 20oC is heated to 350oC while the volume is kept
constant. The density of the gas
a. increases.
b. decreases.
c. remains the same.
d. cannot be determined.
42. Calculate the ratio of effusion rates of O2 and H2:
a. rate O2/rate H2 = 1/16
b. rate O2/rate H2 = 32/1
c. rate O2/rate H2 = 1/4
d. rate O2/rate H2 = 16/1
e. rate O2/rate H2 = 4/1
43. A mixture of three gases has a total pressure of 1388 torr at 298 K. If the
mixture contains 1.27 mol Cl2, 3.04 mol CO, and 1.50 mol Ar, what is the partial
pressure (torr) of Ar?
a. 196
b. 301
c. 358
d. 5345
e. 8020
44. Deviation from the ideal gas law is greatest at:
a. low temperature and low pressure.
b. low temperature and high pressure.
c. high temperature and high pressure.
d. high temperature and low pressure.
45. Molecules of different gases have the same average kinetic energies at the same
a. pressure.
b. temperature.
c. volume.
d. density.
46. A gas has a volume of 175 L at 760 torr and 288 K. What is the temperature if
the gas volume and pressure are changed to 198 L and 640 torr?
a. 547 K
b. 487 K
c. 387 K
d. 274 K
e. 214 K
47. The SI
a.
b.
c.
d.
e.
unit of pressure is
pascal
torr
atm
mm Hg
joule
48. What is the molar mass of Freon gas if its density is 6.13 g/L at STP?
a. 0.274 g/mol
b. 3.64 g/mol
c. 78.2 g/mol
d. 137 g/mol
e. 365 g/mol
49. Which
a.
b.
c.
d.
e.
gas has molecules with the greatest average molecular speed at 25oC?
CH4
Kr
N2
CO2
Ar
50. A 5.0 L volume of a certain gas weighs 289 mg. If the mass was measured at a
pressure of 540 torr and a temperature of 27oC, what is the identity of the gas?
a. H2
b. He
c. N2
d. Ar
e. CO2
51. What is the density of Xe gas (MW=131.3 g/mol) in a 1.0 L flask at 100oC and
2.0 atm pressure?
a. 0.065 g/L
b. 0.65 g/L
c. 8.6 g/L
d. 15.4 g/L
e. 131 g/L
52. Molecular speed distributions for a gas at two different temperatures are shown
below. Which of the following graphs correctly describes the distributions at the
two temperatures, where T2 > T1? [Note: the small vertical lines indicate average
speed]
53. Which of the following graphs is inconsistent with ideal gas behavior?
54. Two separate glass bulbs, bulb A and bulb B, are both filled with helium. The
pressure in bulb A is twice that of bulb B. The volume of bulb B is twice that of
bulb A. What can be said about these two systems if they are held at the same
temperature?
a. Bulb A has more atoms of helium in it than bulb B.
b. Bulb B has more atoms of helium in it than bulb A.
c. Bulb B and bulb A contain the same number of atoms of helium.
d. The densities of the gases in both bulbs are the same since they are filled
with the same gas.
e. More information is needed to make any of these conclusions.
55. The system below is a two dimensional representation of a gas. What happens to
the gas if it is placed into the container on the right (assuming both containers
are at the same temperature)?
a.
b.
c.
d.
The density of gas would increase.
The density of gas would decrease.
The number of gas molecules would increase.
The mean or average molecular speed of the gas molecules would
decrease.
e. None of the above describe what would happen.
56. An inflated balloon has a volume of 6.0 L at sea level (1.0 atm). It is allowed to
ascend in altitude until the pressure is 0.45 atm. During ascent the temperature
of the gas falls from 22oC to -21oC. Calculate the volume of the balloon at its
final altitude.
a. 0.6 L
b. 1.1 L
c. 6.0 L
d. 11 L
e. 12 L
57. The volume of a 1 mole sample of propane gas at 50 atm pressure and 100oC is
measured, and the quantity PV/RT is found to be significantly smaller than 1.00.
The explanation for this is:
a. the propane must be above its critical temperature.
b. the propane molecules attract one another.
c. the volume of the propane molecules cannot be neglected.
d. propane is an incompressible gas.
e. hydrogen bonding influences the properties of propane.
58. Which graph best represents the distribution of molecular speeds for the gases
argon and methane, CH4, when both are in the same flask with a total pressure
of 600 mm Hg and a partial pressure of 450 mm Hg for the argon? [Note: The
vertical lines on each curve represents the root mean square velocity.]
59. A gas phase reaction takes place in a syringe at a constant temperature and
pressure. If the initial volume is 40 cm3and the final volume is 60 cm3, which
general reaction took place?
a. A(g) + B(g) --> AB(g)
b. 2A(g) + B(g) --> A2B(g)
c. 2AB2(g) --> A2(g) + 2B2(g)
d. 2AB(g) --> A2(g) + B2(g)
e. 2A2(g) + 4B(g) --> 4AB(g)
60. Air (assume 100% N2) effuses out of a tire in 2.5 minutes. How long would it
take for the same volume of xenon (at the same T,P) to effuse out of the tire?
a. 61 min
b. 12 min
c. 5.4 min
d. 1.2 min
e. 0.53 min
61. Chemical analysis of a gaseous compound showed that it contained 33.0% Si
and 67.0% F by mass. At 35oC, 0.210 L of the compound exerted a pressure of
1.70 atm. If the mass of 0.210 L of the compound was 2.40 g, determine its
molecular formula.
a. SiF4
b. SiF3
c. Si2F8
d. Si2F6
e. Si3F9
62. Which
a.
b.
c.
d.
e.
of the following gases has a density of 0.714 g/L at STP?
He
CH4
CO
CO2
Cl2
63. What is the partial pressure of H2 in a mixture of 10.0 g H2 and 10.0 g N2 for
which the total pressure is 5.00 x 102 torr? [AW: H = 1.01; N = 14.01]
a. 34 torr
b. 2.50 x 102 torr
c. 4.66 x 102 torr
d. 5.00 x 102 torr
e. the question cannot be answered because the temperature is not given.
64. Under conditions of standard temperature and pressure, what volume of O2(g) is
necessary to react with 2.0 L of NO(g) to give 3.0 L of a product mixture
containing only NO2(g) and O2(g)?
a. 1.0 L
b. 1.5 L
c. 2.0 L
d. 2.5 L
e. 3.0 L
65. A balloon is to be filled with helium until the volume at a presure of 1.00 atm is
2.00 x 104 L. The temperature is 300 K. The helium is stored in pressurized
cylinders each with a volume of 50.00 L and a He pressure of 150 atm at 300 K.
How many cylinders are needed to fill the balloon (the He in the last cylinder
may not be used up completely)?
a. 2
b. 3
c. 4
d. 400
e. 812
66. If a 2.0-L vessel contains 0.5 mol Ar at 298 K, the gas pressure in atm is:
a. 6.1 atm
b. 0.51 atm
c. 240 atm
d. 1.0 atm
e. 75 atm
67. A sample of an unknown gas is placed in a 1.50-L bulb at a pressure of 356 torr,
a temperature of 22.5oC, and is found to weigh 0.9847 g. What is the molecular
weight of the gas?
a. 34.0
b. 64.0
c. 17.0
d. 38.0
e. 76.0
68. If all else is constant, which of the following steps will double the volume of an
ideal gas?
a. halve the pressure
b. double the absolute temperature
c. remove half the molecules
d. a and b only
e. a, b and c
69. Which of the following statements concerning the kinetic theory of gases is(are)
correct?
I.
Molecules make elastic collisions with each other and with the walls of
their container.
II.
The average kinetic energy of a large number of molecules of mass, M, is
proportional to M1/2 at a given temperature.
III.
The molecules of a gas are in constant random motion.
IV.
All the molecules of a gas have the same kinetic energy at a given
temperature.
a. I, II, III, IV
b. I, II, III
c. I, III, IV
d. I, III
e. only III
70. The average temperature at an altitude of 20 km is 220 K. What is the rms
speed (in meters per second) of N2 molecules at this altitude?
.
5 m/s
a.
55 m/s
b.
111 m/s
c.
221 m/s
d.
443 m/s
71. The rms speed of O2 molecules is 5.0 x 102 m/s at a certain temperature. The
rms speed of H2 molecules at the same temperature is:
.
8.0 x 103 m/s
a.
2.0 x 103 m/s
b.
5.0 x 102 m/s
c.
1.3 x 102 m/s
d.
3.1 x 101 m/s
72. O2 gas escapes through a pinhole in 37.5 seconds. Under the same conditions,
the same volume of another gas escapes in 44.0 seconds. This gas could be:
.
He
a.
CO
b.
Cl2
c.
F2
d.
CO2
73. 20 g of H2 gas are mixed with 20 g of He gas in a container. The total gas
pressure is 1.0 atm. The partial pressure of H2 is:
.
1.0 atm
a.
0.67 atm
b.
0.50 atm
c.
0.33 atm
d.
The partial pressure cannot be determined because the temperature and
volume of the container are not given.
74. The following volume-temperature plots were made at different values of
constant pressure and constant number of moles of gas. Which plot represents
measurements at the highest pressure?
.
a.
b.
c.
d.
A
B
C
D
none of the above
75. Compare the root mean square speed of a O2 molecule with that of a CH4
molecule at the same temperature and pressure.
.
O2 is 2.5 times faster since it has 2 atoms per molecule while CH4 has 5.
a.
The speeds are the same since the weights of O2 and of CH4 are both 16
g/mol.
b.
The speeds are the same because at the same temperature all gas
molecules have the same root mean square speed.
c.
CH4 is 2.00 times faster because the M.W. of O2 is 2.00 times greater
than the molecular weight of CH4.
d.
CH4 is 1.41 times faster since at equal temperature all gas molecules
have the same kinetic energy. The root mean square speed then is
inversely proportional to the square root of the molecular weight.
76. What is the volume of a scuba tank if it takes 2000 L of air collected at 1 atm to
fill the tank to a pressure of 150 atm?
.
500 L
a.
2.07 L
b.
8.80 L
c.
13.3 L
d.
3.00 x 105 L
77. Calculate the partial pressure of propane in a mixture that contains equal
weights of propane (C3H8) and butane (C4H10) at 20oC and 746 mm Hg. [At Wts:
C = 12.01 amu; H = 1.008 amu]
.
424 mm Hg
a.
212 mm Hg
b.
646 mm Hg
c.
322 mm Hg
d.
196 mm Hg
78. If it takes 6.5 seconds for 25.0 cm3 of helium gas to effuse through a pinhole
into a vaccum, how long would it take 25.0 cm3 of CH4 to escape under the same
conditions? [At Wts: He = 4.003 amu; C = 12.00 amu; H = 1.008 amu]
.
13.0 s
a.
3.25 s
b.
26.2 s
c.
1.82 s
d.
10.1 s
79. Calculate the density of helium which is at 0.00oC and 1.00 atm. Report your
answer in units of g/L.
.
0.00 g/L
a.
0.0146 g/L
b.
0.0446 g/L
c.
0.178 g/L
d.
not enough information
80. A gas initially at 4.00 atm has a volume of 8.00 L. What is the pressure required
to compress the gas to a volume of 2.00 L?
.
4.00 atm
a.
2.00 atm
b.
1.00 atm
c.
8.00 atm
d.
16.0 atm
81. How many moles of gas occupy 60.82 L at 31oC and 0.483 atm?
.
1.18
a.
0.850
b.
894
c.
11.6
d.
0.120
82. A mixture of two gases, A and B, has a total pressure of 0.95 atm and contains
0.32 moles of gas A and 0.56 moles of gas B. What is the partial pressure (in
atm) of gas B?
.
1.7
a.
1.5
b.
0.60
c.
0.35
d.
0.56
83. The kinetic molecular theory of gases predicts pressure to rise as the
temperature of a gas increases because
.
the average kinetic energy of the gas molecules decreases
a.
gas molecules collide more frequently with the container walls
b.
gas molecules collide less frequently with the container walls
c.
gas molecules collide less energetically with the container walls
d.
both (b) and (d)
Answers
1. D
2. B
3. D
4. B
5. C
6. A
7. B
8. C
9. C
10. D
11. D
12. D
13. C
14. D
15. C
16. B
17. C
18. E
19. C
20. A
21. A
22. B
23. E
24. E
25. B
26. A
27. C
28. E
29. E
30. B
31. A
32. A
33. D
34. C
35. C
36. D
37. A
38. C
39. E
40. E
41. C
42. C
43. C
44. B
45. B
46. D
47. A
48. D
49. A
50. A
51. C
52. A
53. A
54. C
55. B
56. D
57. B
58. C
59. C
60. C
61. D
62. B
63. C
64. C
65. B
66. A
67. A
68. D
69. D
70. E
71. B
72. E
73. B
74. A
75. E
76. D
77. A
78. A
79. D
80. E
81. A
82. C
83. B