$x \ g$ of urea (molar mass $60 \ g \ mol^{-1}$) is completely dissolved in $y \ g$ of pure water and the solution boiled at $373.202 \ K$. If the boiling point of pure water at $1.013 \ bar$ is $373.15 \ K$, then $x:y$ is $(K_b(H_2O) = 0.52 \ K \ kg \ mol^{-1})$

The rise in the boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of a solvent is $0.1 \ ^\circ C$. The molal elevation constant of the liquid is .......... $K/m$.

The plot given below shows $P-T$ curves (where $P$ is the pressure and $T$ is the temperature) for two solvents $X$ and $Y$ and isomolal solutions of $NaCl$ in these solvents. $NaCl$ completely dissociates in both the solvents.
On addition of equal number of moles of a non-volatile solute $S$ in equal amount (in $kg$) of these solvents,the elevation of boiling point of solvent $X$ is three times that of solvent $Y$. Solute $S$ is known to undergo dimerization in these solvents. If the degree of dimerization is $0.7$ in solvent $Y$,the degree of dimerization in solvent $X$ is. . . . . . .

If the boiling point of a solution is $T_1$ and the boiling point of the pure solvent is $T_2$,then the elevation in boiling point is given by:

$A$ solution of non-volatile solute has a boiling point elevation of $1.75 \ K$. Calculate the molality of the solution $[K_{b} = 3.5 \ K \ kg \ mol^{-1}]$.

If an aqueous solution contains $9 \%$ and $1 \%$ $(w/w)$ of two non-volatile non-electrolytes $X$ (molecular weight $180$) and $Y$ (molecular weight $50$) respectively,the boiling point of the solution in ${ }^{\circ} C$ is approximately $(K_b = 0.52 \ K \ kg \ mol^{-1})$