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Gas Laws Practice Problems
(Part II)
V. 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. What is the partial pressure of the nitrogen in the new
container? What is the total pressure in the new container?
VI. Ideal Gas Law (all gas variables held constant)
1) 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?
2.) Calculate the pressure in atmospheres exerted by 5.6 grams of carbon dioxide in a 1.0 liter container at
25° C.
3.) How may grams of oxygen gas are in a 5.00 liter container at 25° C and 750. mm Hg?
4.) 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?
(over)
Review
Assuming all other variables are held constant, give the corresponding relationship if....
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 reduced by 1/2, what happens to it's temperature?