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.

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

For the solution of the gases $w$,$x$,$y$ and $z$ in water at $298 \ K$,the Henry's law constants $(K_H)$ are $0.5$,$2$,$35$ and $40 \ kbar$,respectively. The correct plot for the given data is

Assertion: $A$ mixture of $He$ and $O_2$ is used for respiration for deep sea divers.
Reason: $He$ is soluble in blood.

Which of the following laws represents the quantitative relationship between the solubility of gas in liquid and its pressure?

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?