The boiling point of benzene is $353.23 \, K$. When $1.80 \, g$ of a nonvolatile solute was dissolved in $90 \, g$ of benzene,the boiling point is raised to $354.11 \, K$. The molar mass of the solute is $........ \, g \, mol^{-1}$. $[K_b \text{ for benzene} = 2.53 \, K \, kg \, mol^{-1}]$

What is the boiling point of a solution of $0.1 \ m$ $KCl$ (in $K$)? $K_{b}$ of water is $0.52 \ K \ kg \ mol^{-1}$ and $\alpha = 100 \ \%$ (boiling point of pure water is $373 \ K$).

Vessel-$1$ contains $w_2 \ g$ of a non-volatile solute $X$ dissolved in $w_1 \ g$ of water. Vessel-$2$ contains $w_2 \ g$ of another non-volatile solute $Y$ dissolved in $w_1 \ g$ of water. Both the vessels are at the same temperature and pressure. The molar mass of $X$ is $80 \%$ of that of $Y$. The van't Hoff factor for $X$ is $1.2$ times that of $Y$ for their respective concentrations. The elevation of boiling point for the solution in Vessel-$1$ is . . . . . . $\%$ of the solution in Vessel-$2$.

The molal elevation constant is the ratio of the elevation in boiling point to the $......$.

$A$ solution containing $12.5 \ g$ of non-electrolyte substance in $250 \ g$ of water shows boiling point elevation of $0.52 \ K$. Calculate the molar mass of the substance. $(K_b = 0.52 \ K \ kg \ mol^{-1})$ ......... $g \ mol^{-1}$.

$A$ solution of $5.6 \ g$ nonvolatile solute in $50 \ g$ solvent has an elevation in boiling point of $1.75 \ K$. What is the molar mass of the solute $\left(K_{b} = 3 \ K \ kg \ mol^{-1}\right)$?