The Henry's law constant for the dissolution of a gas in an aqueous medium is $3 \times 10^2 \ atm$. At what partial pressure of the gas will the molality of the gas in the aqueous solution be $\frac{5}{9} \ m$?

Calculate the concentration of dissolved gas in water at $25^{\circ} C$ if the partial pressure of the gas at the same temperature is $0.15 \ atm$. $\left[K_H = 0.15 \ mol \ dm^{-3} \ atm^{-1}\right]$ (in $M$)

Consider a solution of $CO_{2(g)}$ dissolved in water in a closed container. Which one of the following plots correctly represents the variation of $log$ (partial pressure of $CO_2$ in vapour phase above water) [y-axis] with $log$ (mole fraction of $CO_2$ in water) [x-axis] at $25^{\circ}C$?

Calculate the solubility of a gas in water at $260 \ mm \ Hg$ and $25^{\circ} C$ if Henry's law constant of the gas is $0.159 \ mol \ dm^{-3} \ atm^{-1}$ at $25^{\circ} C$.

$5.5 \text{ mg}$ of nitrogen gas dissolves in $180 \text{ g}$ of water at $273 \text{ K}$ and $1 \text{ atm}$ pressure due to nitrogen gas. The mole fraction of nitrogen in $180 \text{ g}$ of water at $5 \text{ atm}$ nitrogen pressure is approximately:

Which one of the following statements regarding Henry's law is not correct?