The oxygen dissolved in water exerts a partial pressure of $20 \ kPa$ in the vapour above water. The molar solubility of oxygen in water is ............ $\times 10^{-5} \ mol \ dm^{-3}$ (Round off to the Nearest Integer). [Given: Henry's law constant $K_H = 8.0 \times 10^{4} \ kPa$ for $O_2$,Density of water $= 1.0 \ kg \ dm^{-3}$]

Henry's law constant for the molality of methane in benzene at $298 \, K$ is $4.27 \times 10^{5} \, mm \, Hg$. Calculate the solubility of methane in benzene at $298 \, K$ under $760 \, mm \, Hg$.

What is the solubility of oxygen gas in $100 \, cm^3$ of water at $293 \, K$ (in $, cm^3$)?

$A$ company dissolves '$X$' amount of $CO_{2}$ at $298 \ K$ in $1 \ L$ of water to prepare soda water. $X = ........ \ \times 10^{-3} \ g$ (nearest integer).
(Given: partial pressure of $CO_{2}$ at $298 \ K = 0.835 \ bar$.
Henry's law constant for $CO_{2}$ at $298 \ K = 1.67 \ kbar$.
Atomic mass of $H$,$C$ and $O$ is $1$,$12$ and $16 \ g \ mol^{-1}$,respectively.)

Solubility of a gas in a liquid increases with

The $K_{H}$ values for some gases at the same temperature '$T$' are given below:

Gas	$K_{H} / \text{kbar}$
$Ar$	$40.3$
$CO_{2}$	$1.67$
$HCHO$	$1.83 \times 10^{-5}$
$CH_{4}$	$0.413$

where $K_{H}$ is Henry's Law constant in water. The order of their solubility in water is: