Question

Molar solubility of helium, nitrogen and oxygen are plotted against partial pressure of the gas at constant temperature as given below.
Which of the following is the correct sequence for the Henry's Law constant for the following gases?

• A. $O_2>N_2>He$
• B. $O_2<N_2<He$
• C. $O_2=N_2=He$
• D. $O_2>N_2<He$

Answer 1

The correct option is B $O_2<N_2<He$

From Henry's law, Partial pressure, $p=K_H\times$Solubility
So, higher the value of olubility of the gas in the liquid, the lower is the Henry's law constant.

$$\begin{array}{ccc}\text{Gas}& \text{Temperature}& {\text{K}}_H\text{(K-bar)}\\ \text{He}& 293& 144.97\\ {\text{N}}_2& 293& 76.48\\ {\text{O}}_2& 293& 34.86\end{array}$$
Hence, (b) is the correct option.