Section 14.3
The Ideal Gas Law
Practice Test
1.
Determine the Celsius temperature of 1.50 moles of ammonia contained in a 10.0-L vessel under a pressure of 2.0 atm.
SC.A.1.4.3
a.
-50°C
b.
-111°C
c.
0.0°C
d.
162°C
Hint
2.
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.
40.0 g/mol
c.
47.9 g/mol
d.
34.5 g/mol
Hint
3.
What will happen to a real gas when the temperature is lowered and the pressure is raised?
SC.A.1.4.3
a.
The gas eventually condenses to become a liquid.
b.
The gas does not change.
c.
The gas expands.
d.
The number of gas particles doubles.
Hint
4.
How many moles of an ideal gas are contained in 8.21 L at 73°C and 380 torr?
a.
7.5 x 10
23
b.
0.14
c.
0.25
d.
1.5 x 10
23
Hint
5.
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?
SC.A.1.4.3
a.
2.7 grams
b.
6.3 grams
c.
0.16 grams
d.
0.36 grams
Hint
6.
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.
1.8 x 10
2
mol
d.
5.5 x 10
-3
mol
Hint
7.
What is the name given to a gas whose particles do not take up space, do not have intermolecular attractive forces, and follow the gas laws under all conditions of temperature and pressure?
a.
real gas
b.
ideal gas
c.
diatomic gas
d.
noble gas
Hint
