Gay-Lussac's Law is: P1 / T1 = P2 / T2 or P1T2 = P2T1 Temperature must be in Kelvin units!
Abbreviations: atm = atmosphere, mm Hg = millimeters of mercury, torr = another name for mm Hg
Pa = Pascal (kPa = kilo Pascal), K = Kelvin, °C = degrees Celsius

Conversions: 1 torr = 1 mm Hg, K = °C + 273, °F = 1.8(°C) + 32, °C = F - 32
1.8
1 dm3 (cubic decimeter)= 1 L (liter) = 1000 mL (milliliter)

Under Standard Conditions, STP(Standard Temperature & Pressure):
Temperature = 0.00 °C = 273 K = 32ºF
Pressure = 1.00 atm = 760.0 mm Hg = 760 torr = 101.325 kPa = 101,325 Pa = 14.7 psi

1. Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 °C to 30.0 °C.

2. A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure at standard temperature?

3. A gas has a pressure of 699.0 mm Hg at 40.0 °C. What is the temperature at standard pressure?

4. If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant what final pressure would result if
the original pressure was 750.0 mm Hg?

5. If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original
temperature was 25.0 °C, what would the final temperature of the gas be?

6. A 30.0 L sample of nitrogen inside a rigid, metal container at 20.0 °C is placed inside an oven whose
temperature is 50.0 °C. The pressure inside the container at 20.0 °C was at 3.00 atm. What is the pressure of the
nitrogen after its temperature is increased?

7. A sample of gas at 3.00 x 103 mm Hg inside a steel tank is cooled from 500.0 °C to 0.00 °C. What is the final
pressure of the gas in the steel tank?

8. The temperature of a sample of gas in a steel container at 30.0 kPa is increased from -100.0 °C to 1.00 x 103
°C. What is the final pressure inside the tank?