Henry’s constant (in K.bar) for four gases $\alpha ,\beta ,\gamma$ and  $\delta$ in water at 298K is given below:

gases	$\mathrm{\alpha }$	$\mathrm{\beta }$	$\mathrm{\gamma }$	$\mathrm{\delta }$
${\mathrm{K}}_{\mathrm{H}}$	50	2	$2\times {10}^{-5}$	0.5

(density of water $={10}^3\mathrm{kg}/{\mathrm{m}}^3$ at 298K)

This table implies that

A) From Henry’s law,  $p=K_{H}X\Rightarrow X=\frac{p}{K_H}\Rightarrow X\alpha \frac{1}{K_H}(p=\text{constant})$

Higher the value of $K_H$ smaller will be the solubility of the gas, so $\text{'}\gamma \text{'}$ is more soluble.

B)Though solubility of gases will decrease with increase in temp

C)$P_{\gamma }=K_H{X}_{\gamma }=2\times {10}^{-5}\left[\frac{55.5}{55.5+\frac{1000}{18}}\right]={10}^{-5}K.bar={10}^{-2}bar$

D)$P_{\delta }=K_H{X}_{\delta }=0.5\left[\frac{55.5}{55.5+\frac{1000}{18}}\right]=0.5\times 0.5=0.25Kbar=250bar$