Dry air contains $79 \% \,N_2$ and $21 \% \,O_2$. At $T \,K$, if Henry's law constants for $N_2$ and $O_2$ in water are $8.57 \times 10^4 \,atm$ and $4.56 \times 10^4 \,atm$ respectively, the ratio of mole fractions of $N_2$ and $O_2$ dissolved in water at $1 \,atm$ is

Calculate the solubility of gas in water at $1.2 \text{ atm}$ and $25^{\circ} C$ if Henry's law constant is $0.45 \text{ mol dm}^{-3} \text{ atm}^{-1}$ at $25^{\circ} C$.

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

$CO_2$ gas is bubbled through water during a soft drink manufacturing process at $298 \ K$. If $CO_2$ exerts a partial pressure of $0.835 \ bar$,then $x \ mmol$ of $CO_2$ would dissolve in $0.9 \ L$ of water. The value of $x$ is $.....$ (Nearest integer).
(Henry's law constant for $CO_2$ at $298 \ K$ is $1.67 \times 10^3 \ bar$)

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

Why are aquatic species more comfortable in cold water in comparison to warm water?