Gas Laws Unit Worksheet
All problems that involve calculations must be done on your own paper and stapled to this
sheet. Label with the section name.
Temperature and Pressure Conversions
1. 2.00 atm to mmHg
7. -25oC to Kelvin
13.Standard
o
2. 115kPa to atm
8. -227 C to Kelvin
temperature in
3. 500. mmHg to atm
9. 1800. mmHg to kPa
kelvin and Celsius
4. 3.5x104 torr to
10.93500 Pa to atm
14.298 K to oC
mmHg
11.950. Torr to atm
15.100.K to oC
5. 35oC to Kelvin
12.0.490 atm to kPa
16.5.0K to oC
6. 120oC to kelvin
Ideal Gas Equation Worksheet
1. 1. What is the pressure exerted by 2.0moles of an ideal gas when it occupies a volume
of 12.0L at 373K?
2. A flashbulb of volume 2.6cm3 contains O2 gas at a pressure of 2.3atm and a
temperature of 26oC. How many moles of oxygen gas does the flashbulb contain?
3. If 0.20 moles of helium occupies a volume of 64.0L at a pressure of 0.15atm, what is the
temperature of the gas?
4. What is the volume of 0.35 moles of gas at 1.7 atm of pressure and a temperature of
100.K?
5. What is the pressure of 1.5 moles of an ideal gas at a temperature of 150K that occupies
of a volume of 20.0L?
6. How many moles of gas occupy 16.2L at a pressure of 1.05 atm and a temperature of
37oC?
7. Calculate the volume of exactly 1.00 mole of a gas at STP.
8. How many moles of nitrogen are present in 17.8L at 27oC and 1.3 atm pressure?
9. What is the pressure of 2.3 moles of carbon dioxide at 235K occupying 23.7L of space?
10.How many moles of argon are in 30.6L at 28K and 658mmHg?
Combined Gas Law Problems
1. The gas pressure in an aerosol can is 1.5atm at 25oC. Assuming that the gas inside obeys
the ideal gas equation, what would the pressure be if the can were heated to 450oC?
Assume constant volume due to the rigid metal of the can.
2. A pocket of gas is discovered in a deep drilling operation. The gas has a temperature of
480oC and is at a pressure of 12.8atm. Assuming ideal behavior, what volume of the gas
is required to provide 18.0L at the surface at 1.00atm and 22oC?
3. A fixed quantity of gas is compressed at constant temperature from a volume of 368mL
to 108mL. If the initial pressure was 5.22 atm, what is the final pressure?
4. A gas originally at 15oC and having a volume of 182 mL is reduced in volume to 82.0mL
while its pressure is held constant. What is its final temperature?
5. At 36oC and 1.00atm pressure, a gas occupies a volume of 0.600L. How many liters will
it occupy at 0.0oC and 0.205 atm?
6. Chlorine is widely used to purify municipal water supplies and to treat swimming pool
waters. Suppose that the volume of a particular sample of Cl2 is 6.18L at 0.90atm and
33oC. What volume will the Cl2 occupy at 107oC and 0.75 atm?
7. A gas exerts a pressure of 1.5 atm at 27oC. The temperature is increased to 108oC with
no volume change. What is the gas pressure at the higher temperature?
8. The pressure of a gas at 35.6oC is 114.3kPa. What is the pressure when the
temperature drops to 17.3oC? Assume constant volume.
9. A 21.5L sample of gas at 107kPa has a temperature of 27.2oC. What is the pressure of
the gas if it is transferred to a 32.6L container at 44.1oC?
10.A gas at 19oC occupies 4.0L. What will be the new volume if the temperature increases
to 70.0oC? Assume a flexible container that allows constant pressure.
Avogadro’s Law
1. A balloon has 0.256 moles of helium gas and occupies a volume of 1320 ml.. What will
be the new volume if the moles of gas is reduced to 0.2moles?
2. What will be the new volume is 0.57moles of gas occupying 4430L is increased to 1.1
moles?
3. A gas system has initial volume and moles of 6200mL and 0.191moles. If the volume
changes to 9.19L, under conditions of constant P and T, what will the resultant number
of moles be?
4. A gas system has an initial volume of 4700mL with the number of moles unknown.
When the volume changes to 7.70L, under conditions of constant P and T, the number
of moles is found to be 0.424moles. What was the initial number of moles?
5. A gas system has an initial number of moles of 0.0832moles with the volume unknown.
When the number of moles changes to 0.0601moles, under conditions of constant P and
T, the volume is found to be 5.13L. What was the initial volume in mL?
Dalton’s Law of Partial Pressure
1. A mixture of oxygen, carbon dioxide and nitrogen has a total pressure of 0.97atm. What
is the partial pressure of oxygen, if the partial pressure of CO2 is 0.70atm and the partial
pressure of nitrogen is 0.12atm.
2. What is the partial pressure of hydrogen gas in a mixture of hydrogen and helium if the
total pressure is 600mmHg and the partial pressure of helium is 439mmHg?
3. Find the total pressure for a mixture that contains four gases with partial pressures of
5.00kPa, 4.56kPa, 3.02kPa, and 1.20kPa.
4. Find the partial pressure of carbon dioxide in a gas mixture with a total pressure of
30.4kPa if the partial pressures of the other two gases in the mixture are 16.5kPa and
3.7kPa.
5. What is the total gas pressure in a sealed flask that contains oxygen at a partial pressure
of 0.41 atm and water vapor at a partial pressure of 0.58 atm?
Vapor Pressure and Boiling
1. Given an atmospheric pressure of 400 torr, at what temperature would each liquid boil?
A.
B.
C.
2. How low must the atmospheric pressure be for each liquid to boil at 35oC?
A.
B.
C.
3. What is the normal boiling point of each liquid?
A.
B.
C.
4. Define normal boiling point
5. Under what conditions do liquids boil?
6. If you were at the top of Mt. Everest, would water boil at the same temperature as it
does in Lincolnton? Explain.
Phase Diagram of Water
For each of the numbered arrows, (a) state the initial state of matter and final state of
matter; (b) what is increasing or decreasing (pressure or temperature); and (c) the phase
change that is occurring.