What is the volume of a balloon of gas at 842 mm Hg and - 23° C, if its volume is 915 mL at a pressure of 1,170 mm Hg and a temperature of 24°C?

V₂ = 1070 mL or 1.07 L

Solution:

Data Given;

P₁ = 1170 mmHg

V₁ = 915 mL

T₁ = 24 °C + 273 K = 297 K

P₂ = 842 mmHg

V₂ = ?

T₂ = - 23 °C + 273 K = 250 K

According to Ideal gas equation,

P₁ V₁ / T₁ = P₂ V₂ / T₂

Solving for V₂,

V₂ = P₁ V₁ T₂ / P₂ T₁

Putting Values,

V₂ = (1170 mmHg * 915 mL * 250 K) : (842 mmHg * 297 K)

V₂ = 1070 mL or 1.07 L