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Gas Laws Practice Problems
I. Dalton's Law of Partial Pressure
1.) One liter of hydrogen gas with a pressure of 1.2 atm is added to a one liter container of oxygen gas with a
pressure of 0.7 atm, what is the final pressure of these two gases?
2.) A mixture of nitrogen and oxygen gases has a pressure of 740 mm Hg. If the partial pressure of nitrogen
is 310 mm Hg, calculate the partial pressure of the oxygen.
3.) A 44.1 L sample of nitrogen gas at a pressure of 88.3 kPa is placed into a container of equal volume that
already holds hydrogen gas at a pressure of 125.6 kPa.
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What is the partial pressure of the nitrogen in the new container?
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What is the total pressure in the new container?
II.Boyle's Law (temperature and moles held constant)
4.) If 250.0 mL of oxygen gas at 750 mm Hg are compressed to a pressure of 450 mm Hg, what will the new
volume be?
5.) What will the pressure be when the a volume of a gas with a pressure of 630. mm Hg is compressed from
2.50 L to 1.65 L?
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6.) A sample of hydrogen gas occupies 40.0 L at 1.00 atm pressure. What volume will it occupy at 5.00 atm?
7.) A gas occupies a volume of 200.0 mL at 400.0 mm Hg pressure. To what pressure must the gas be
subjected in order to change its volume to 75.0 mL?
III. Charles's Law (pressure and moles held constant)
8.) 3.00 liters of hydrogen gas at 253 K is allowed to warm to a room temperature of 298 K. What is the
new volume?
9.) If 20.0 L of nitrogen gas is cooled from 100°C to 0°C, what is the new volume?
10.) If an unknown gas occupies a volume of 5.00 L is cooled from a starting temperature of 27°C, at what
temperature (in degrees Celsius) will the volume be 1.25 L?
IV. Gay-Lussac's Law (volume and moles held constant)
11.) A 10.0 L container of helium has a pressure of 640. mm Hg at 22°C. What will the pressure be at 44°C?
12.) A 5.00 L container holds oxygen at 285 K and 3.00 atm. If the volume remains held constant, what will
be the pressure at 344 K?
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13.) A sealed, rigid container holds an unknown gas at 12°C and 233 kPa. What temperature is needed to
raise the pressure to 291 kPa?
V. Combined Gas Law (only moles held held constant)
14.) 645 mL of carbon dioxide has a pressure of 720.0 mm Hg at 35 °C. If the volume expands to 745 mL at
125 °C, what will the pressure be?
15.) Given 20.0 L of ammonia gas at 5°C and 730 mm Hg pressure, calculate the volume at 50. °C and 800.0
mm Hg.
16.) The volume of a gas filled balloon is 50.0 L at 20.0°C and 742 mm Hg. What volume will it occupy at STP?
17.) At the temperature of -15.0°C and a pressure of 87.2 kPa, the volume of a gas has been determined to
be 43.5 mL. What would the volume of the gas become if it were placed at STP?
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VI. Ideal Gas Law (all gas variables held constant)
18) How many moles of nitrogen monoxide are in a flask with a volume of 500.0 mL at a pressure of 2.10
atm and a temperature of 15.3° C?
19.) Calculate the pressure in atmospheres exerted by 5.6 grams of carbon dioxide in a 1.0 liter container at
25° C.
20.) How may grams of oxygen gas are in a 5.00 liter container at 25° C and 750. mm Hg?
21.) What volume will 8.00 grams of ammonia gas (NH3) occupy if its temperature is measured to be 48.5 °C
and its pressure 208.3 kPa?
22. Assuming all other variables are held constant, give the corresponding relationship if....
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Example: If the temperature of a gas doubles, what happens to its volume? it doubles
a. If the pressure of a gas is reduced by 1/2, what happens to its temperature?
b. If the volume of a gas is tripled, what happens to its temperature?
c. If the mass of a gas is reduced by 1/4, what happens to its pressure?
d. If the temperature of a gas is reduced by 1/5, what happens to its pressure?
e If the volume of a gas is increases 2-fold, what happens to it's Kelvin temperature?
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