The variation of solubility of four different gases $(G_1, G_2, G_3, G_4)$ in a given solvent with pressure at a constant temperature is shown in the plot. The gas with the highest value of Henry's law constant is

The partial pressure of a gas at $25 \text{ }^\circ\text{C}$ is $0.18 \text{ atm}$. Calculate the concentration of the gas dissolved at the same temperature, if $K_H$ is $0.15 \text{ mol dm}^{-3} \text{atm}^{-1}$. (in $\text{ M}$)

Calculate $K_H$ when $2 \ mmol$ of $O_2$ dissolve in $540 \ mL$ of water at $27 \ ^oC$ temperature. Given $P_{O_2} = 2 \times 10^{-8} \ bar$.

Give an example of a solution where both the solute and the solvent are in the gaseous state.

What is the significance of Henry's Law constant $K_H$?

The partial pressure of ethane over a solution containing $7.14 \times 10^{-3} \ g$ of ethane is $1 \ bar$. If the solution contains $5 \times 10^{-2} \ g$ of ethane,then what shall be the partial pressure of the gas (in $bar$)? (At equal temperature)