Chemistry -- Gas Laws ACT Questions [USE TO STUDY FOR YOUR TEST]
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1. At 22°C, the air pressure in a car tire is 1293 torr.
c. 755
Convert this pressure to atmospheres (atm).
d. 877
a. 12.76
5. At 1.00 atm, a sealed weather balloon contains 20.0
b. 5.262
L of helium (He) gas at 25.0°C. Assume that none
c. 1.701
of the He escapes and the pressure is constant.
d. 1.293
What is the volume, in liters, of He in the weather
2. This diagram shows a closed-end mercury (Hg)
balloon at 35.0°C?
a. 40.0
b. 28.0
c. 20.7
d. 14.3
barometer.
When atmospheric pressure is 1.30 atm, what is
the height (h), in millimeters, of the Hg in the
barometer?
a. 132
b. 585
c. 760
d. 988
3. A chemist compresses a 1.5 L sample of carbon
dioxide (CO2) gas at 1.2 atm to a final volume of
0.75 L. Assuming the temperature is constant, what
is the final pressure, in atm, exerted by the CO2
gas?
a. 0.60
b. 0.94
c. 1.7
d. 2.4
6. At 1254 m above sea level, the city of Helena,
Montana, has an average atmospheric pressure of
0.859 atm. A chemistry student in Helena finds that
pure distilled water boils at 95.9°C. Which
statement explains the student’s results at this high
elevation?
a. The boiling point of water increases due to
lower atmospheric pressure.
b. The boiling point of water increases due to
higher atmospheric pressure.
c. The boiling point of water decreases due to
lower atmospheric pressure.
d. The boiling point of water decreases due to
higher atmospheric pressure.
4. A vessel connected to an open-end mercury (Hg)
manometer contains nitrogen (N2) gas. The
atmospheric pressure is 0.993 atm. The height
difference between the two arms of the manometer
7. For a chemistry homework assignment, Beth must
consider the effusion rates of methane (CH4) gas
and nitrogen trifluoride (NF3) gas at 25°C. Effusion
occurs as gas particles escape from a container
through a small hole. Which statement accurately
compares the effusion rates of CH4 and NF3 at
25°C?
a. CH4 effuses 2 times faster than NF3.
b. CH4 effuses 4 times faster than NF3.
c. NF3 effuses 2 times faster than CH4.
d. NF3 effuses 4 times faster than CH4.
is 122 mm.
What is the pressure, in mm Hg, of the N2 gas?
a. 355
b. 633
8. At standard temperature and pessure, a chemist
burns 3.50 L of pentane (C5H12) in excess oxygen
(O2) gas.
C5H12(l) + 8 O2(g) -> 5 CO2(g)
+ 6 H2O(l)
What is the maximum
number of liters of carbon dioxide (CO2) that the
reaction can produce?
a. 17.5
b. 8.50
c. 5.60
d. 0.700
9. At high temperatures, chlorine (Cl2) reacts wiht
flourine (F2) to produce chlorine triflouride (ClF3)
Cl2 (g) + 3 F2 (g) --> 2 ClF3 (g)
A chemist carries out the reaction of 0.250 mol of
F_2 wit excess Cl2. At 250.0°c and 1.00 atm, what
is the maximum volume of ClF3 in liters, that the
reaction can produce?
a.
b.
c.
d.
3.42
3.73
7.16
10.7
10. Real gases best imitate the behavior of ideal gases
under what conditions?
a. Low temperatures and low pressure
b. low temperature and high pressure
c. high temperatures and low pressure
d. high temperatures and high pressure
11. A chemist purchases a 43.7 L cylinder of methane
(
) gas. At 295 K, the pressure inside the
cylinder is 1.88 atm. How many grams of
are
in the cylinder?
a. 3.39
b. 12.2
c. 23.2
d. 54.4
12. At 83.7 kPa and 35.0°C, what is the density, in g/L,
of phosphorous hydride (
)?
a. 0.528
b. 1.11
c. 1.52
d. 2.39
13. At 15°C, 0.252 mol of argon (Ar) gas occupies 174
ml. What is the pressure, in atm, of the Ar gas?
a. 1.78
b. 2.92
c. 12.6
d. 34.2
14. Sylvia heats 2.28g of a liquid until it completely
vaporizes. The boiling point of the liquid is 56.3°C.
She collects all of the gas in a 750.0 ml vessel. The
pressure of the gas is 1.41 atm at 56.3°C. What is
the molar mass, in g/mol, of the liquid?
a. 9.97
b. 22.3
c. 58.3
d. 121
15. The boiling point of chlorine (
) is -34.6°C.
What is this temperature in Kelvin?
a. 307.6 K
b. 238.4 K
c. -238.4
d. -307.6 K
16. Which statement correctly describes the melting
point of a solid?
a. The particles in the solid lose enough kinetic
energy to overcome the interactions preventing
them from approaching one another.
b. The particles in the solid lose enough kinetic
enrgy to overcome the interactions holding
them in an organized pattern.
c. The particles in the solid gain enough kinetic
enrgy to overcome the interactions preventing
them from approaching one another.
d. The particles in the solid gain enough kinetic
energy to overcome the interactiong holding
them in an organized pattern.
17. At constant temperature, Kelly increases the
volume of a fixed amount of gas. Use the kineticmolecular theory to explain how increasing the
volume affects the pressure of a gas.
a. The pressure decreases because there are fewer
collisions between gas molecules and the
container walls.
b. The pressure decreses because there are more
collisions between gas molecuyles and the
container walls.
c. The pressure increases becuase there are fewer
collisions between gas molecules and the
container walls.
d. The pressure increses because there are more
collisions between gas molecuyles and the
container walls.