Name:_______________________________ Date: _______________________ Period: _________________
MR. HOLT’S COLLEGE BOUND CHEMISTRY HOMEWORK #3
Boyles Law: P1*V1 = P2*V2
Gay-Lussac’s Law: P1*T2 = P2*T1
Charles’ Law: V1*T2 = V2*T1
Combined Gas Law: P1*V1 = P2*V2
T1
T2
Ideal Gas Law: P*V = n*R*T
R = 0.0821 L*atm
mol*K
1) Match the following descriptions to the correct Gas Law
_______ Can be used when Temperature is constant
_______ Can be used when Pressure is constant
_______ The constant for this Gas Law is always 0.0821 L*atm
mol*K
_______ Can be used when Pressure, Volume, and Temperature
are changing
_______ Can be used when Volume is constant
a) Gay-Lussac’s Law
b) Boyle’s Law
c) Ideal Gas Law
d) Charles’ Law
e)Combined Gas Law
2) A sample of oxygen gas has a volume of 150.0 mL at a pressure of 0.947 atm. The
pressure is then increased to 1.000 atm with a constant temperature.
What Gas Law do you need to use to solve this problem? ________________________________
What is the new volume?
3) Helium gas in a balloon occupies 2.5 L at 300.0 K. The balloon is dipped into
liquid nitrogen that is at a temperature of 80.0K.
What Gas Law do you need to use to solve this problem? ________________________________
What is the new volume of the balloon at this lower temperature?
4) At 395.15 K the pressure of a sample of nitrogen is 1.07 atm. The temperature is
then raised to 478.15 K at constant volume.
What Gas Law do you need to use to solve this problem? ________________________________
What is the new pressure of the sample?
5) Calculate the pressure exerted by 43 moles of nitrogen in a 65 L cylinder at
278.15 K.
What Gas Law do you need to use to solve this problem? ________________________________
6) What will be the volume of 111 moles of nitrogen in the stratosphere where the
temperature is -57 degrees Celsius and the pressure is 4.00 atm. (Hint: don’t forget
to change Celsius to Kelvin)
What Gas Law do you need to use to solve this problem? ________________________________
7) A 15 L cylinder of gas at 4.8 atm pressure at 298.15K is heated to 348.15K and
compressed to 17 atm. What is the new volume?
What Gas Law do you need to use to solve this problem? ________________________________