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Five gas laws are commonly used in the General Chemistry courses at Eastfield College. They are Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, The Combined Gas Law, and the Ideal Gas Law. This handout is a guide to help you understand how they are defined and also how they work. Each Law will be defined and you will be given an example for each.
Charles’ Law (Temperature–Volume Law) – The Volume of a gas is directly proportional to the Kelvin temperature at a constant pressure.
In layman terms this means that when the temperature goes up the volume goes up and when the temperature goes down the volume goes down.
Mathematically the problem would be:
V1 = V2
T1 T2
Example: A gas occupies a 100ml at a temperature of 293K(20°C). What will the volume be at 283K (10° C) at a constant pressure?
V1 = 100ml
T1 = 293K
V2 = ?
T 2= 283K
100ml = V2
293K 283K
(100ml)(283K) = V2
293K
96.58 or 96.6ml = V2
Mnemonic: Charles is Very Tall