Calculate $\Delta T_b$ of a $0.45 \text{ m}$ solution of a nonvolatile solute in a solvent if the molal elevation constant of the solvent is $3.0 \text{ K kg mol}^{-1}$. (in $\text{ K}$)

$13.44 \ g$ of $CuCl_2$ is dissolved in $1 \ kg$ of water. Determine the elevation in boiling point of the solution. [$K_b = 0.52 \ K \ kg \ mol^{-1}$,$mol \ wt$ of $CuCl_2 = 134.4$]

When salt is dissolved in water,then.....

The elevation in boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of solvent is $0.1^{\circ}C$. The value of $K_b$ for the solvent is ........ $\frac{K}{m}$.

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 $1.8 \ K \ kg \ mol^{-1}$.

$2 \, g$ of a non-volatile non-electrolyte solute is dissolved in $200 \, g$ of two different solvents $A$ and $B$ whose ebullioscopic constants are in the ratio of $1: 8$. The elevation in boiling points of $A$ and $B$ are in the ratio $\frac{x}{y} (x: y)$. The value of $y$ is .... (Nearest integer)