Gas Laws

State Boyle's Law.

At constant temperature, the pressure and volume of a gas are inversely related: P1V1 = P2V2

State Charles's Law.

At constant pressure, the volume and temperature (in Kelvin) of a gas are directly related: V1/T1 = V2/T2

What does the Ideal Gas Law equation PV = nRT relate?

Pressure, volume, number of moles, and temperature of a gas, using the universal gas constant R

Why must temperature be in Kelvin, not Celsius, when using the gas laws?

The gas law relationships are proportional to absolute temperature, and Kelvin has no negative values, so ratios like V1/T1 only make physical sense in Kelvin

If a gas is compressed to half its volume at constant temperature, what happens to its pressure?

It doubles (Boyle's Law: P and V are inversely proportional)