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:

Calculate the number of moles of nonvolatile solute dissolved in $0.3 \ kg$ solvent if $\Delta T_{b}=0.3 \ K$ and $K_{b}$ for solvent is $1.8 \ K \ kg \ mol^{-1}$.

For water,$K_b = 0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $200 \ mL$ of water,at what temperature will the resulting solution boil at $1 \ atm$ pressure (in $^oC$)?

Two different solutions were prepared by dissolving sucrose in water having concentrations of $1 \ m$ and $2 \ m$ respectively. The value of $(T_2 - T_1)$ will be ........... $K$. (Given: $K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$)

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 correct relation between the elevation in boiling point and the molar mass of a solute is: ($W_1$ and $W_2$ are respectively weight of solvent $\&$ solute)