Charles' Law Problems
Conversions:

K  =  C  +  273             1.00 atm  =  760.0 mm Hg  =  101.325 kPa  =  101,325 Pa

Note: temperature using Charles’ Law is always in Kelvin!

1. Calculate the decrease in temperature when 2.00 L at 20.0 C is compressed to 1.00 L.
 
 
 
 

2. 600.0 mL of air is at 20.0 C. What is the volume at 60.0 .C?
 
 
 
 
 
 

3. A gas occupies 900.0 mL at a temperature of 27.0 C. What is the volume at 132.0 C?
 
 
 
 
 

4. What change in volume results if 60.0 mL of gas is cooled from 33.0 C to 5.
00 C?
 
 
 
 
 

5. A gas occupies 1.00 L at standard temperature. What is the volume at 333.0 C?
 
 
 
 
 

6. At 210.0 C a gas has a volume of 8.00 L. What is the volume of this gas at -23.0 C?
 
 
 
 
 
 

7. The temperature of a 4.00 L sample of gas is changed from 10.0 C to 20.0 C. What will the volume of this gas be at the new temperature if the pressure is held constant?
 
 
 
 

8. Carbon dioxide is usually formed when gasoline is burned. If 30.0 L of CO2 is produced at a temperature of 1.00 x 103 C and allowed to reach room temperature (25.0 C) without any pressure changes, what is the new volume of the carbon dioxide?
 
 
 
 
 

9. A gas syringe contains 56.05 milliliters of a gas at 315.1 K. Determine the volume that the gas will occupy if the temperature is increased to 380.5 K
 
 
 
 
 
 

10. When the temperature of a gas decreases, does the volume increase or decrease?
 
 
 
 

11. If the Kelvin temperature of a gas is doubled, the volume of the gas will increase by  how much?
 
 
 
 
 

12. How would a graph of pressure vs. volume (Boyle’s law) look different from a graph of temperature vs. volume?
 
 
 
 
 

13. How can Charles’ Law be used to theoretically estimate absolute zero?
 
 
 


Copyright Alexplorer. Some items taken from or adapted from other materials. This page is free for use in a classroom setting.
Back to the Chemistry index