Which of the following statement$(s)$ is/are correct regarding the solubility of solid $I_2$?

At $293 \ K$,methane gas was passed into $1 \ L$ of water. The partial pressure of methane is $1 \ bar$. The number of moles of methane dissolved in $1 \ L$ water is ($K_{H}$ of methane $= 0.4 \ kbar$)

Assertion : When a salt such as $NaCl$ dissolves,the $Na^{+}$ and $Cl^{-}$ ions leaving the crystal lattice acquire far greater freedom.
Reason : In thermodynamic terms,the formation of solution occurs with a favourable change in free energy,i.e.,$\Delta H$ has a high positive value and $T\Delta S$ a low negative value.

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).

In which of the following salts,the solubility increases appreciably with an increase in temperature?

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?