Unit
4 Quiz--Empirical Gas Laws--Thurston High Chemistry
Multiple Choice (Choose the best
answer.)
Standard temperature and pressure (STP) refers to which conditions?
0 oC and 1 KPa
0 oC and 1 mm Hg
0 K and 1 KPa
0 K and 1 atm
273 K and 1 atm
If 4 moles of a gas are added to
a container that already holds 1 mole of gas, how will the pressure change within
the container? (Assume volume and temperature are constant.)
The pressure will be 5 times as great.
The pressure will be 2 times as great.
The pressure will be 4 times as great.
The pressure will not change.
None of the above are correct.
The next 3 questions
ask you about the relationship known as Boyle's Law. Refer to your notes or the
book if you have trouble.
A 4.0 L sample of hydrogen
gas at 700 mm Hg would occupy what volume at 250 mm Hg? (Assume temperature and
number of particles stays constant.)
1.4 x 10 -7 L
1.4 L
11.2 L
2.4 L
7.0 x 10 5 L
A 25 L tank of oxygen under
a pressure of 80. atm would require what pressure to decrease the volume to 1.0
L? (Assume temperature and number of particles stays constant.)
0.31 atm
3.2 atm
2000
atm
There is not enough information to answer the question.
None of these is correct.
A balloon containing
2.50 L of gas at 1 atm would be what volume at a pressure of 300 KPa? (Assume
temperature and number of particles stays constant.)
6.33 L
8.11 L
0.844
L
120. L
000833 L
The next two questions ask you about Charles'
Law. Refer to your notes or the text if you have problems.
A syringe containing 75.0 mL of air is at 298 K. What will the volume of the
syringe be if it is placed in a boiling water bath (373 K). Assume pressure and
the number of particles are held constant.
59.9 mL
188 mL
300. mL
8.34 x 106 mL
None of the above are correct.
A gas occupies
40.0 mL at 127 oC. What volume will it occupy at -73 oC?
(Assume pressure and number of particles is constant.)
182 mL
8.80 mL
80.0 mL
20.0
mL
None of these
is correct.
Which of the following equations correctly
combines Boyle's and Charles' Laws?
Use the combined gas law to
answer the next two questions. Refer to your notes or the text if you need to.
A 50.0 mL sample of a gas is at 3.00 atm of pressure
and a temperature of 298 K . What volume would the gas occup at STP?
0.00728 mL
15.3 mL
18.2 mL
137
mL
None of these
is correct.
A syringe contains 60.0 mL of air at
740 mm Hg pressure and 20 oC. What would be the temperature at which
the syringe would contain 30.0 mL at a pressure of 370 mm Hg? (Assume no gas could
leak in or out of the syringe.)
-200 oC
0.0137 oC
5 oC
73.3 oC
None of these is correct.
The next three questions
ask you about Dalton's Law of Partial Pressures. Refer to your notes or the text
if you need to refresh your memory.
A sealed container
contains 1.0 mol of hydrogen and 2.0 moles of nitrogen gas. If the total pressure
in the container is 1.5 atm, what is the amount of pressure exerted by each gas?
H2 = 1.0 atm and N2 = .50 atm
H2 = 0.50 atm and N2 = 1.0 atm
H2 = 1.0 atm and N2 = 2.0 atm
H2 = 2.0 atm and N2 = 1.0 atm
There is not enough information given to answer the question.
A sample of gas is collected by water displacement. The atmospheric pressure
in the room is 757 mm Hg and the vapor pressure of water is 17 mm Hg. What is
the partial pressure of hydrogen under these conditions?
17 mm Hg
740 mm Hg
757 mm Hg
774 mm Hg
You cannot
answer this question because you do not know the temperature.
The volume of a gas collected over water is 15.0 mL when the atmospheric pressure
is 101.3 KPa. What will be the volume of the gas if the atmospheric pressure increases
to 120.0 KPa. Assume that the vapor pressure of water is 2.7 KPa and that the
temperature is constant.
