500 ml of nitrogen at 27°C is cooled to –5°C at the same pressure. The new volume becomes

Given initial volume (V₁) = 500 ml ; Initial temperature (T₁) = 27ºC = 300 K and final temperature (T₂) = –5ºC = 268 K.

From Charle’s law :

      $\frac{{\mathrm{V}}_1}{{\mathrm{T}}_1}=\frac{{\mathrm{V}}_2}{{\mathrm{T}}_2}\text{ or }\frac{500}{300}=\frac{{\mathrm{V}}_2}{268}$

Where V₂ = New volume of gas

${\mathrm{V}}_2=\frac{500}{300}\times 268=446.66\mathrm{ml}$