Calculate the temperature to which a gas must be heated, so that the volume triples without any change in pressure. The gas is originally at 57°C and having a volume 150 cc.

V₁ = Initial volume of the gas = 150 cc
T₁ = Initial temperature of the gas = 57°C = 57 + 273 = 330 K

V₂ = Final volume of the gas = 3 x 150 = 450 cc
T₂ = Final temperature of the gas = ?

By Charles's Law:

$\dfrac{\text{V}$1}{\text{T}1} = \dfrac{\text{V}2}{\text{T}2}

Substituting the values :

$\dfrac{150}{330} = \dfrac{450}{\text{T}$2} \\[1em] \text{T}2 = \dfrac{450 \times 11}{5} = 990 \text{K}

T₂ °C = 990 - 273 = 717°C

Therefore, final temperature of the gas = 717°C