If the boiling point of a urea solution is $100.18^{\circ}C$ and $K_b$ for water is $0.512 \ K \ kg \ mol^{-1}$,what is the molality of the solution? (Boiling point of water $= 100^{\circ}C$)

Calculate the boiling point elevation of a solution if $15 \ g$ of urea is dissolved in $1000 \ g$ of water. $\left[K_{b} \text{ for water} = 0.52 \ K \ kg \ mol^{-1}; \text{ molar mass of urea} = 60 \ g \ mol^{-1}\right]$ (in $K$)

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. . . . . . .

Which of the following solutions will exhibit the highest boiling point?

When $174.5 \ mg$ of octatomic sulfur $(S_8)$ is added to $78 \ g$ of bromine $(Br_2)$,the boiling point of bromine becomes ............. $K$. Given: $K_b$ for $Br_2 = 5.2 \ K \ kg \ mol^{-1}$ and the boiling point of pure $Br_2 = 332.15 \ K$.

$A$ solution of $50 \text{ g}$ of solute '$X$' is dissolved in $150 \text{ g}$ of '$Y$' solvent boils at $357.27 \text{ K}$. What is the molar mass of solute (in $\text{ g/mol}$)? (Given $K_b$ and boiling point of pure solvent are $2.77 \text{ K kg/mol}$ and $350.06 \text{ K}$ respectively.)