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

The relation between the solubility of a gas in a liquid at a constant temperature and external pressure is stated by which law?

According to Henry's law,the solubility of a gas in a given volume of liquid increases with increase in

$A$ gas '$X$' is dissolved in water at $2 \ bar$ pressure. Its mole fraction is $0.02$ in solution. The mole fraction of water when the pressure of gas is doubled at the same temperature is

If $N_2$ gas is bubbled through water at $293 \ K$,how many millimoles of $N_2$ gas would dissolve in $1 \ L$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. Given that Henry's law constant for $N_2$ at $293 \ K$ is $76.48 \ kbar$.

Calculate the pressure of the gas if the solubility of the gas in water at $25^{\circ} C$ is $6.85 \times 10^{-4} \ mol \ dm^{-3}$. (Henry's law constant $K_H$ is $6.85 \times 10^{-4} \ mol \ dm^{-3} \ bar^{-1}$) (in $bar$)