The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas. This statement is known as ...

Solubility of $N_2$ gas in water at $25\,^{\circ}C$ and $0.78\, atm$ is $5.4 \times 10^{-4}\, M$. Calculate Henry's law constant for $N_2$ in water at $25\,^{\circ}C$.

Calculate the solubility of a gas in water at $0.8 \ atm$ and $25^{\circ} C$. [Henry's law constant is $6.85 \times 10^{-4} \ mol \ dm^{-3} \ atm^{-1}$]

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

Gas	$K_{H} \ (kbar)$
$\alpha$	$50$
$\beta$	$2$
$\gamma$	$2 \times 10^{-5}$
$\delta$	$0.5$

(Density of water $= 10^{3} \ kg \ m^{-3}$ at $298 \ K$). Which of the following statements is correct?

Assertion : The molecules of the dissolved gas present in a liquid gain kinetic energy as temperature is raised.
Reason : Gases tend to be more soluble in liquids as the temperature is raised.

Calculate the solubility of a gas having partial pressure $0.15 \ bar$ at $25^{\circ} C$.
$[K_{H} = 0.16 \ mol \ dm^{-3} \ bar^{-1}]$