Henry's law constant for the solubility of $N_2$ gas in water at $298\, K$ is $1.0 \times 10^5\, atm$. The mole fraction of $N_2$ in air is $0.6$. The moles of $N_2$ from air dissolved in $10$ moles of water at $298\, K$ and $5\, atm$ pressure is

$5.5 \text{ mg}$ 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:

Identify a pair of gases from the following that does not obey Henry's law.

If $N_2$ gas is bubbled through water at $293 \ K$,how many millimoles of $N_2$ gas would dissolve in $1 \ L$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. The Henry's law constant for $N_2$ at $293 \ K$ is $76.48 \ kbar$.

Given below are two statements:
Statement $I$: The Henry's law constant $K_{H}$ is constant with respect to variations in solution's concentration over the range for which the solution is ideally dilute.
Statement $II$: $K_{H}$ does not differ for the same solute in different solvents.
In the light of the above statements, choose the correct answer from the options.

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.