If four gases $A$,$B$,$C$ and $D$ have Henry's constant $(K_H)$ values $1.9 \times 10^1 \ bar$,$6.5 \times 10^{-4} \ bar$,$7.8 \times 10^{-4} \ bar$ and $6.0 \times 10^3 \ bar$ respectively,then which of the following gas has maximum solubility at the same partial pressure?

The solubility of $N_2$ in water at $300 \ K$ and $500 \ torr$ partial pressure is $0.01 \ g \ L^{-1}$. The solubility (in $g \ L^{-1}$) at $750 \ torr$ partial pressure is

In which solution,the solubility of the solute decreases with an increase in temperature?

Henry's law constants for $O_2$ and $N_2$ are $K_{O_2} = 3.3 \times 10^7 \ atm$ and $K_{N_2} = 6.51 \times 10^7 \ atm$. Calculate the ratio of $\frac{X_{O_2}}{X_{N_2}}$,i.e.,the ratio of mole fractions of $O_2$ and $N_2$ dissolved in water at $25 \ ^\circ C$ from air. (Assume air contains $20 \%$ $O_2$ and $80 \%$ $N_2$ by volume).

If $O_2$ gas is bubbled through water at $303 \; K$,the number of millimoles of $O_2$ gas that dissolve in $1 \; L$ of water is (Nearest Integer). (Given: Henry's Law constant for $O_2$ at $303 \; K$ is $46.82 \; kbar$ and partial pressure of $O_2 = 0.920 \; bar$). (Assume solubility of $O_2$ in water is too small,nearly negligible).

The solubility of a gas in a liquid is directly proportional to the pressure of the gas over the solution. Identify the law for this statement.