In a mixture of camphor in nitrogen gas,the physical states of the solute and the solvent are,respectively:

$A$ liquid freezes at $7^{\circ} C$ and boils at $77^{\circ} C$. If $K_{f}$ and $K_{b}$ values for the liquid are $5.6$ and $2.5 \ ^{\circ} C \ kg \ mol^{-1}$ respectively,then the ratio of latent heat of vaporisation of the liquid to the latent heat of fusion is $:-$

The solution from the following with the highest depression in freezing point (lowest freezing point) is:

At $T(K)$,$2$ moles of liquid $A$ and $3$ moles of liquid $B$ are mixed. The vapour pressure of the ideal solution formed is $320 \ mm \ Hg$. At this stage,one mole of $A$ and one mole of $B$ are added to the solution. The vapour pressure is now measured as $328.6 \ mm \ Hg$. The vapour pressures of pure $A$ and pure $B$ (in $mm \ Hg$) are respectively:

Given: Molar mass of $C$,$H$,$O$,$Cl$ are $12$,$1$,$16$ and $35.5 \text{ g mol}^{-1}$,respectively. Statement $I$: In $30\%$ (w/w) solution of methanol in $CCl_4$ (at $T \text{ K}$),the mole fraction of $CCl_4$ is equal to $0.33$. Statement $II$: Mixture of methanol and $CCl_4$ shows positive deviation from Raoult's law.

An aqueous solution freezes at $-2.55 \ ^oC$. What is its boiling point in $^oC$?
[$K_b(H_2O) = 0.52 \ K \ kg \ mol^{-1}, K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1}$]