Gas Law Classwork
IMPORTANT!!!
All gas law calculations involving temperature MUST be done in Kelvin.
To convert remember two things:
 To go back and forth you either add or subtract 273°
 Kelvin can never be negative
1. A balloon full of air has a volume of 2.75 L at a temp of 18°C. What is the
balloons volume at 45°C?
2. A cylinder of compressed gas has a pressure of 4.882 atm on one day. The
next day, the same cylinder of gas has a pressure of 4.690 atm, and its
temperature is 8°C. What was the temperature in °C on the previous day?
3. A sample of neon gas occupies a volume of 2.8 L at 1.8 atm. What will its
volume be at 1.2 atm?
4. Determine the moles of gas present in a 15.0 L container at STP.
5. A sample of argon has a volume of 0.43 mL at 24°C. At what temperature
in °C will it have a volume of 0.57 mL?
6. To what pressure would you have to compress 48.0 L of oxygen gas at 99.3
kPa in order to reduce its volume to 16.0 L?
7. Calculate the volume of a balloon containing 2.35 moles of Cl2 gas at 25°C
under 285 kPa.
8. A mylar balloon is filled with helium gas to a pressure of 107 kPa when the
temperature is 22°C. If the temperature changes to 45°C, what will be the
pressure of the balloon?
9. A chemist collects 59.0 mL of sulfur dioxide gas on a day when the
atmospheric pressure is 0.989 atm. On the next day, the pressure has
changed to 0.967 atm. What will the volume of the gas be on the second day?
10. Calculate the pressure in kPa of a 15.0 mole, 300.0 L sample of gas at room
temperature.
Gas Law Classwork
1. A balloon full of air has a volume of 2.75 L at a temp of 18°C. What is the
balloons volume at 45°C?
V1 V2
2.75 V2
V2 = 3.01 L
=
=
T1 T2
291 318
2. A cylinder of compressed gas has a pressure of 4.882 atm on one day. The
next day, the same cylinder of gas has a pressure of 4.690 atm, and its
temperature is 8°C. What was the temperature in °C on the previous day?
P1 P2
4.882 4.690
T1 = 293 K  20°C
=
=
T1 T2
T1
281
3. A sample of neon gas occupies a volume of 2.8 L at 1.8 atm. What will its
volume be at 1.2 atm?
P1V1 = P2V2
1.8 (2.8) = 1.2 V2
V2 = 4.2 L
4. Determine the moles of gas present in a 15.0 L container at STP.
(1.00) (15.0) = n (0.0821) (273) n = 0.669 moles
5. A sample of argon has a volume of 0.43 mL at 24°C. At what temperature
in °C will it have a volume of 0.57 mL?
V1 V2
0.43 0.57
T2 = 394 K  121 K
=
=
T1 T2
297
T2
6. To what pressure would you have to compress 48.0 L of oxygen gas at 99.3
kPa in order to reduce its volume to 16.0 L?
P1V1 = P2V2
(99.3) (48.0) = P2 (16.0)
P2 = 298 kPa
7. Calculate the volume of a balloon containing 2.35 moles of Cl2 gas at 25°C
under 285 kPa.
(285) V = 2.35 (8.314) (298)
V = 20.4 L
8. A mylar balloon is filled with helium gas to a pressure of 107 kPa when the
temperature is 22°C. If the temperature changes to 45°C, what will be the
pressure of the balloon?
P1 P2
107
P
P2 = 115 kPa
=
= 2
T1 T2
295 318
9. A chemist collects 59.0 mL of sulfur dioxide gas on a day when the
atmospheric pressure is 0.989 atm. On the next day, the pressure has
changed to 0.967 atm. What will the volume of the gas be on the second day?
P1V1 = P2V2
(0.989) (59.0) = (0.967) V2
V2 = 60.3 L
10. Calculate the pressure in kPa of a 15.0 mole, 300.0 L sample of gas at room
temperature.
300.0 P = 15.0 (8.314) (296)
P = 123 kPa