Boyle’s Law, Charles’s Law, and Gay-Lussac’s Law
Chemistry I
1. If a sample of methane gas is kept in a piston with an volume of 250mL at STP, what
would the new volume be if the temperature of the piston was increased to 300 oC?
2. If methane gas was kept in a 3.00 L container at STP, what would the pressure be at
3.2 L?
3. If a container of gas has a pressure of 4.5 atm at 451 K, what would the temperature
have to be for the pressure to reduce to .6 atm?
4. If a sample of gas has a volume of 1.1L of gas and a pressure of 721 mmHg, what
would the volume be at STP?
5. If a sample of gas has a volume of 350 mL at 100 K, what would the volume be at
500K?
Charles’s Law and Boyle’s Law
Chemistry I
1. What is 3.4 atm of pressure in kPa and mm Hg?
2. A gas has a volume of 250mL at 25oC. If the gas is warmed to 305 oC, what is the
new volume?
3. Methane, a highly flammable gas, is placed in a piston that has a volume of 2.1 L at
STP. The piston then compresses the gas to 125 mL. What is the pressure inside the
piston?
4. A 129 mL balloon is filled with helium at room temperature, 25 oC. The balloon is
then taken out on a warm day and it expands to 155mL. What was the temperature
outside?
5. A 2.2 L sample of gas is kept at STP. The temperature is raised 21 degrees Celsius.
What would the new volume of the gas be?
Boyle’s Law
Chem. I
Gas Law Problems
1. What are the three units of pressure?
2. What is standard pressure in all three units?
3. What is STP? What do the letters stand for?
4. A sample of oxygen is found to have a volume of 251 mL at 216 kPa. The volume is
then increased to 364 mL while the temperature is held constant. What is the new
pressure?
5. A 1.00 L piston contains a gas at standard atmospheric pressure. The piston is then
compressed to half of its original volume while the temperature is held constant.
What is the pressure inside the piston?
6. A container holds 6.34 cm3 of gas at a pressure of 1033 mm Hg. While the
temperature is held constant, the container expands to 103 cm3. What is the new
pressure in atm?
7. A 250 mL sample of methane gas at STP is compressed into a 212 mL bottle. What
is the pressure inside the bottle?
8. A balloonist fills up his balloon with 200 liters of air at standard pressure. As he and
his balloon rise, the atmospheric pressure drops from standard pressure to .782 atm.
What is the new volume of his balloon?
9. A box has the following measurements: 15 cm long, 19 cm deep, and 10 cm wide.
The lid of the box is closed and sealed at standard atmospheric pressure. The box is
then place in a room where the atmospheric pressure is 175.2 kPa. To what volume
will the box crumple?
Worksheet for Boyle’s, Charles’s, and Gay-Lussac’s Law
P1V1 = P2V2
V1 V 2

T1 T 2
P1V 1 P 2V 2

T1
T2
P1 P 2

T1 T 2
STP
T = 273 K
P = 1atm
= 760 mm Hg
= 101.325 kPa
1. Convert the following pressures:
a. 79.1 kPa
 mm Hg
b. 1011 mm Hg  atm
c. 2.15 atm
 kPa
2. If a gas at STP raises its temperature to 1000 K, what is its pressure assuming that
volume is constant?
3. A gas is placed in a 5.21 L balloon at 21 oC. The temperature is then dropped to 3 oC.
What is the new volume?
4. The pressure in a 1250 mL piston is 2500 mm Hg. What is the pressure if the volume
is decreased to 750 mL?
5. The pressure in a sealed container is 300 kPa at 303 K. If the pressure is increased to
413 kPa, what is the temperature?
6. A balloon has a volume of 21.3 mL at 21 oC. The balloon is taken outside on a warm
and expands to 23.1 mL. What is the temperature?
7. A 6.19 L piston has its pressure decreased from 3 atm to 2.76 atm. What is the new
volume?
8. If 23.9 L of a gas at STP has its temperature increased to 30 oC and the pressure
increased to 2.3 atm, what is the new volume?
Ideal Gas Law
1. What is the number of moles in a sample of gas that has a volume of 3.5 L, a
pressure of 200 kPa, and a temperature of 300 K?
2. What is the volume of 2.5 moles of oxygen gas at STP?
3. What is the temperature of a sample of gas that has 4.5 moles in 40,550 mL at a
pressure of 500 mm Hg?
4. A gas’s container has a volume of 450 mL. What would be the number of moles
that would fit in the container if the gas had a temperature of 56oC and a pressure
of 3.5 atm.
5. What is the pressure of a 9045 mL of .0059 moles of gas that has a temperature of
1oC.
6. There is a sample of gas in a box that is 3.5 cm of length, 6.9 cm of width, and
19.1 cm of depth. The pressure is 1705 mm Hg. What is the temperature?
Ideal Gas Law, Molar Volume, and Dalton’s Law
PV = nRT
R = 8.31 kPa*L/mol*K
PT = P1 + P2 + P3...
1 mole = 22.4 L @ STP
STP is 273 K and 1 atm = 760 mm Hg = 101.325 kPa
1. A gas is collected over water at 29oC. The atmospheric pressure that day
is 745 mm Hg. What is the partial pressure of the water vapor? What is
the partial pressure of the gas.
2. A gas is 46.8 L at STP. How many moles does the gas contain? What
would the volume be at 34oC and 550 mm Hg?
3. .56 grams of zinc react with sulfuric acid to produce hydrogen gas and
zinc (II) sulfate. How many moles of hydrogen gas are formed? How
many liters of hydrogen gas are formed at STP?
4. A 46.7 mL sample of gas contains 45.9 moles at 300 mm Hg. What is
the temperature?
5. 9.12 moles of N2 gas is mixed with 6.7 moles of O2 gas in a 4.0 L
container at 25oC. What is the partial pressure of N2? What is the partial
pressure of O2? What is the total pressure?
6. 273 mL of a gas is collected over water at 21oC. The atmospheric
pressure is 100.7 kPa. What is the partial pressure of the gas? What
would the volume if the ‘dry gas’ be at atmospheric pressure?
7. How many moles of air are container in a 2-liter coke bottle at 21oC and
1.05 atm? What would the volume be at STP?