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?

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