A sample of xenon gas occupies a volume of 5.82 L 5.82 L at 475 K. 475 K. If the pressure remains constant, at what temperature will this same xenon gas sample have a volume of 2.64 L?

Answer: 215.5K

Explanation:

Charles' law states that, at constant pressure the volume of a given mass of gas is directly proportional to its temperature in Kelvin (or absolute temperature).

This means that for an increase in gas volume there is a corresponding increase in the Kelvin temperature and a decrease in gas volume will also result in a decrease in the Kelvin temperature.

During calculations, the temperature must be converted to Kelvin temperature if otherwise given.

Mathematically, V * T (at constant pressure)

Introducing a constant,

V = KT where V = volume in litres, T = temperature in Kelvin, K = mathematical constant.

Also, for initial and final states of the gas,

V1/T1=V2/T2 where V1 = volume at temperature T1 and V2 = volume at temperature T2.

Using V1/T1=V2/T2 where V1 = 5.82L, V2=2.64L, T1 = 475K, T2=?

T2=V2T1/V1 = 2.64 x 475/5.82 = 1254/5.82 = 215.5K