Question

Choose the correct option for the total pressure (in atm.) in a mixture of $4g$ $O_2$ and $2g$ $H_2$ confined in a total volume of one litre at $0°C$ is:
Given,
$R=0.082L.atmmo{l}^{–1}{K}^{–1}T=273K$

• A. 2.602
• B. 25.18
• C. 26.02
• D. 2.518

Answer 1

The correct option is B 25.18

Finding partial pressure of $O_2$:
Moles of oxygen:
$\frac{4}{32}=0.125mol$
$P_1=\frac{nRT}{V}=\frac{0.125\times 0.082\times 273}{1}=2.8atm$
Finding partial pressure of $H_2$:
$P_1=\frac{nRT}{V}=\frac{1\times 0.082\times 273}{1}=22.386atm$
Total pressure of the mixture $=2.8+22.38=25.18atm$