Chapter 14:
Gases
Practice Test
1.
When will the molecules of all samples of ideal gases have the same average kinetic energies?
a.
at constant volume
b.
at constant temperature
c.
at constant amount
d.
at constant pressure
Hint
2.
How can the relationship between a gas at two sets of conditions be expressed mathematically by Boyle’s law?
a.
P
1
/
V
1
=
P
2
/
V
2
b.
P
1
V
1
=
P
2
V
2
c.
V
1
/
T
1
=
V
2
/
T
2
d.
V
1
T
1
=
V
2
T
2
Hint
3.
What relationship is demonstrated by the expansion of a gas-filled balloon when it is heated?
a.
Boyle’s law
b.
Gay-Lussac’s law
c.
Charles’s law
d.
Avogadro’s number
Hint
4.
If the pressure exerted by a gas at 100°C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a.
1.0 mol
b.
100 mol
c.
5.5 × 10
-3
mol
d.
1.8 × 10
2
mol
Hint
5.
What is the molar mass of a gas if 0.104 g of the gas occupies 48.7 mL at STP?
a.
28.2 g/mol
b.
47.9 g/mol
c.
34.5 g/mol
d.
40.0 g/mol
Hint
6.
What is the volume of 2.0 moles of a gas at STP?
a.
0.0223 L
b.
44.8 L
c.
0.0446 L
d.
22.4 L
Hint
7.
Which of the following states that equal volumes of gases at the same temperature and pressure contain the same number of particles?
a.
Avogadro’s principle
b.
Gay-Lussac’s law
c.
Boyle’s law
d.
Charles’s law
Hint
8.
Determine the Celsius temperature of 1.50 moles of ammonia contained in a 10.0-L vessel under a pressure of 2.0 atm.
a.
162°C
b.
-50°C
c.
-111°C
d.
0.0°C
Hint
9.
A gaseous compound is 30.6% nitrogen and 69.4% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at –4.0°C. What is the molecular formula for the gas?
a.
NO
2
b.
NO
c.
N
3
O
6
d.
N
2
O
2
Hint
10.
How many grams of ammonia (NH
3
) are present in a sample that occupies 2.0 L at a pressure at 2.0 atm and 25°C?
a.
0.16 grams
b.
0.36 grams
c.
6.3 grams
d.
2.7 grams
Hint
11.
A gas occupies a volume of 1.0 L at 1.0 atm pressure. What is the pressure when the gas expands to fill 2.0 L?
a.
0.50 atm
b.
2.0 atm
c.
1.0 atm
d.
10 atm
Hint
12.
How many moles of an ideal gas are contained in 8.21 L at 73°C and 380 torr?
a.
1.5 × 10
23
b.
0.14
c.
7.5 × 10
23
d.
0.25
Hint
13.
What is the name given to the relationship that shows that an increase in pressure leads to a decrease in the volume of a gas?
a.
Gay-Lussac’s law
b.
Charles’s law
c.
Boyle’s law
d.
Avogadro’s number
Hint
14.
A 10.0-L vessel contains gas A at a pressure of 300.0 torr. A 3.00-L vessel contains gas B at a pressure of 400.0 torr. Gas A is forced into the second vessel. Calculate the resulting pressure in torr. Assume the temperature remains constant.
a.
2000 torr
b.
1800 torr
c.
1400 torr
d.
1000 torr
Hint
15.
How can gases be defined?
a.
A chemical state of matter.
b.
A physical state of matter that does not have a fixed shape but has a fixed volume.
c.
A physical state of matter that has a fixed volume and a fixed shape.
d.
A physical state of matter that does not have a fixed shape or a fixed volume.
Hint
16.
How can the molar volume of a gas be defined?
a.
the volume that one mole occupies at 100
C and 1 atm pressure
b.
the volume that one mole occupies at STP
c.
the volume that one gram occupies at STP
d.
the volume that one gram occupies at 100
C and 1 atm pressure
Hint
17.
Particles of matter that are in constant, random motion and that have a size that is much smaller than the distance between them are _____________.
a.
liquids
b.
gases
c.
solids
d.
solutions
Hint
18.
A gas occupies 2.0 L at STP. What volume will the gas occupy if the pressure is increased to 2.0 atm, and the temperature is kept constant?
a.
1.0 L
b.
4.0 L
c.
2.0 L
d.
0.50 L
Hint
19.
A sample of helium occupies 2.20 L at 1.0 atm. What is the volume at 1.5 atm?
a.
0.68 L
b.
1.0 L
c.
1.5 L
d.
2.20 L
Hint
20.
What is the name given to the conditions in which the temperature is the freezing point of water and the pressure is one atmosphere?
a.
standard state
b.
ideal gas
c.
combined gas law
d.
standard temperature and pressure
Hint
