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Review of Gases
Chemistry
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Gases Review Test
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Further Study
Gases Review Test
Further Study
Gases Review Test
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1. Which of the following is a correct interpretation of the ideal gas law?
nPV
=
nPV
=
=
PT
=
2. What is the correct relationship between
v
_{rms}
,
, and
v
_{p}
?
v
_{rms}
=
=
v
_{p}
<
v
_{p}
≤
v
_{rms}
v
_{p}
<
<
v
_{rms}
v
_{rms}
<
<
v
_{p}
3. An isolated container of gas doubles in pressure and triples in volume. By what factor does T change?
2
3
6
6
4. If the volume of a gas is doubled at constant temperature, the factor by which the pressure increases is:
2
1
5. A barometer filled with an unknown liquid has a height of 1 m at 1 atm. During stormy weather, the height of the column is observed to rise to 1.3 m. What is the atmospheric pressure?
atm
1.3 atm
1 atm
Cannot be determined
6. Which of the following are possible units of R?
7.
You take a reading of 760 mm of Hg at 0 degrees Celsius. However, you realize that the volume at the top of the barometer is
not
a complete vacuum. There is some Hg vapor above the Hg column! If the pressure of Hg is 10 mm Hg, what is the actual atmospheric pressure?
770 mm Hg
760 mm Hg
750 mm Hg
Cannot be determined
8. What are the conditions of STP?
1 bar, 273 K
1 bar, 298 K
1.013×10
^{5}
Pa
, 298 K
1.013×10
^{5}
Pa
, 273 K
9. A container contains 32 grams of
O
_{2}
gas and 2 grams of
H
_{2}
gas. If the total pressure of the vessel is 16 atm, what is the partial pressure of the
H
_{2}
gas?
1 atm
2 atm
8 atm
10 atm
10. As the average radius of a population of gas molecules increases, how does the factor b of van der Waals equation change?
Increase
Stay the same
Decrease
Depends on identity of the gas
11. All of the following are properties of an ideal gas except:
Easily compressible
Individual molecules are assumed to have no volume.
Individual molecules exert attractive forces on one another.
Fills any container in which it is placed
12. The ideal gas law is most valid under these conditions:
High temperature, high pressure
High temperature, low pressure
Low temperature, low pressure
Low temperature, high pressure
13. The reaction
N
_{2}
+2
O
_{2}
→2
NO
_{2}
1 mol of
N
_{2}
and 2 mol
O
_{2}
react completely in an isolated, rigid container with initial pressure 1 atm. The temperature does not change. What is the pressure inside the container after the reaction has gone to completion?
1 atm
3/2 atm
2/3 atm
5/2 atm
14.
There are 4.0 mol of gas a in container A at 1.0 atm and 273 K. There are 2.0 mol of gas b in container B at 2.0 atm and 273 K. What is the total volume of containers A and B?
130 L
90 L
110 L
22.4 L
15.
Is the equation for:
v
_{p}
v
_{rms}
None of the above
16. For the van der Waals equation:
(
P
+
)(
V

nb
) =
nRT
The value "b" corrects for:
The volume occupied by the gas molecules
Inelastic collisions between gas molecules
Intermolecular attractions
The Boltzmann constant
17. For the equation
PV
=
nRT
, the value of T must be expressed in:
Degrees Celsius
Degrees Fahrenheit
Only positive values of degrees Fahrenheit
An absolute temperature scale
18. Which of the following is not a SI unit
Kilograms
Atmospheres
Newtons
Kelvin
19. A sample of gas has a volume of 22.4 L at a temperature of 273 K. How many moles are in the sample?
2.0
1.0
0.50
Cannot be determined from the information given.
20. The volume of a sample of gas expands five times at constant pressure. By what factor has the absolute temperature changed?
1/5
1
5
Cannot be determined from the information given
21. The following reaction produces
H
_{2}
O
gas:
2
H
_{2}
+
O
_{2}
→2
H
_{2}
O
64.0 g of O_2 are used and an excess of
H
_{2}
, and the reaction goes to completion. How many liters of
H
_{2}
O
gas will be generated if the pressure is 2.0 atm and the temperature is 273 K?
64 L
22 L
45 L
11 L
22. A sample of gas occupies 100 L at STP. If the absolute temperature is halved while all other conditions are constant, what will be the final volume?
50 L
100 L
150 L
200 L
23. Calculate the
v
_{rms}
of a sample of
O
_{2}
at 300 K.
484 m/s
242 m/s
141 m/s
9.8 m/s
24. A closed jar contains 2 moles of
O
_{2}
and 3 moles of
N
_{2}
. What is the ratio of the partial pressure of the
O
_{2}
over the total pressure in the jar?
0.1
0.2
0.4
0.6
25. The rate of effusion of gas A is four times that of gas B. What is
?
1/16
1/2
2
16
26.
The Hg containing dish of the barometer is replaced with one four times its diameter. By what factor does
H
change?
1/2
2
4
H
does not change.
27. The density of a certain gas at STP is 1.43 g/L. What is the identity of the gas?
H
_{2}
O
_{2}
CO
_{2}
Cl
_{2}
28. One end of a mercury manometer is open to the atmosphere (
P
_{a}
tm
= 760
mmHg
). The other end is connected to a 1 mol sample of
CH
_{4}
that is at 273 K and occupies 22.4 L. What is the height of the mercury column?
760 mm
560 mm
120 mm
0 mm Hg
29. The MaxwellBoltzmann distribution graph plots:
Pressure vs. Volume
Mean free path vs. time
Mean free path vs. velocity
The velocity distribution of a population of gas molecules.
30. James the giant has big shoes to fill. His shoes have a total area of
20
m
^{2}
in contact with the ground. Unfortunately, James' feet are not so big. Barefoot, his weight is spread over
1
m
^{2}
. What is the ratio of the pressure he exerts on the ground barefoot over the pressure he exerts with his shoes on?
40
20
10
1/20
31. The "air" in airbags is generated via the decomposition of solid
NaN
_{3}
:
2
NaN
_{3}
→2
Na
+ 3
N
_{2}
2/3 mole of solid
NaN
_{3}
are completely decomposed at a temperature of 300 K. In order for the final pressure in the airbag to be 1.2 atm, what must the final volume of the bag be in L? Assume that the Na takes up no appreciable volume.
R
= 0.0821
.
11 L
15 L
21 L
34 L
32. A sample of an
ideal
gas is compressed at constant temperature. What happens to the average kinetic energy of the molecules?
The molecules bounce into the walls more often. Thus average kinetic energy decreases.
When in a confined space, molecules move slower. Average kinetic energy decreases.
Average kinetic energy is solely dependent on pressure. As pressure rises, so does the average kinetic energy.
Average kinetic energy is solely dependent on temperature. The temperature does not change, so the average kinetic energy stays constant.
33. A piston compresses a gas at constant temperature. Initially the gas occupied 1 L and was at a pressure of 1 atm. After compression, the gas occupies 0.1 atm. What is the pressure of the compressed gas?
0.1 atm
1 atm
10 atm
100 atm
34. A collaborator from a foreign country reports that the value of
R
as
8
. He has probably used units of "woozle" for which of the following variables:
Pressure
Volume
Temperature
Mole fraction
35. Avogadro's number is:
8.314
0.0821
1.38×10
^{23}
6.02×10
^{23}
36. What is
if both samples of gas are at the same temperature?
2
1/2
37. The following MaxwellBoltzmann distribution plot was measured for two gases A and B at the same temperature:
Which gas has the greater molecular mass?
Gas A
Gas B
Their molecular masses are equal
Cannot be determined
38. A rigid container holds a mixture of gases. Within this mixture, the partial pressure of
O
_{2}
is 400 torr. If an additional quantity of
N
_{2}
gas is injected into the container such that the total pressure of the container rises by 760 torr, what is the change in the partial pressure of
O
_{2}
? Assume that the temperature of the container's contents stays constant.
 100 torr
0 torr
+ 100 torr
+ 760/400 torr
39. If the pressure of a gas doubles and the temperature quadruples, by what factor does the volume change?
1/2
1
2
4
40. Which of the following are possible units for pressure?
41. The following MaxwellBoltzmann distribution plot was measured for a gas at two temperatures A and B:
What is the relationship between A and B?
A
>
B
A
<
B
A
=
B
Cannot be determined
42. For the following calculation of
v
_{rms}
, the molar mass (MM) should be expressed in what units?
v
_{rms}
=
=
sqrt
lb/mol
g/mol
kg/mol
slugs/mol
43. By what significant numerical value are Boltzmann's constant (k) and the gas constant (R) related?
The acceleration due to gravity g
The speed of light, c
Avogadro's number,
N
_{A}
The mass of a single C12 atom
44. The pressure of a gas is tripled while the volume is halved. By what factor does the temperature increase?
1/2
2/3
3/2
2
45. The gas constant R:
Is unitless
Varies with varying temperature, pressure, and volume.
Is the foundation of Charle's law
Has units of (pressure * volume) over (mol * absolute temperature)
46. One end of a manometer is sealed off to a vacuum. The other end of the manometer is connected to a pressurized gas. The height of the liquid column is indicative of:
The atmospheric pressure
The pressure of the gas
The difference between the atmospheric pressure and the pressure of the gas
The dimensions of this particular manometer
47. A sample of
O
_{2}
and a sample of
N
_{2}
both have a temperature of 330 K. What is the ratio of the average kinetic energy of the
O
_{2}
over that of the
N
_{2}
?
28/32
1
32/28
Cannot be determined
48. The density of a gas at STP is 0.089 g/L. What is the molar mass of the gas?
4.0 g/mol
2.0 g/mol
1.0 g/mol
Cannot be determined from the given data
49. The following MaxwellBoltzmann distribution plot was measured for two gases A and B at temperatures
T
_{A}
and
T
_{B}
:
Which gas has the greater molar mass?
Gas A
Gas B
MM Gas A = MM Gas B
Cannot be determined from the given data
50. Gaseous methane (
CH
_{4}
) burns completely in gaseous oxygen to produce carbon dioxide gas and water vapor.
CH
_{4}
+2
O
_{2}
→
CO
_{2}
+ 2
HOH
2 mole of
CH
_{4}
and 4 moles of
O
_{2}
completely react in a closed vessel. If temperature and volume are constant, by what factor will pressure increase?
1/2
1
2
Cannot be determined from the given data.
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