When $3.00 \, g$ of a substance $'X'$ is dissolved in $100 \, g$ of $CCl_4$,it raises the boiling point by $0.60 \, K$. The molar mass of the substance $'X'$ is $..... \, g \, mol^{-1}$. (Nearest integer).
$[$ Given $K_b$ for $CCl_4$ is $5.0 \, K \, kg \, mol^{-1} ]$

$A$ solution of $6 \ g$ of solute in $100 \ g$ of water boils at $100.52^{\circ} C$. The molal elevation constant of water is $0.52 \ K \ kg \ mol^{-1}$. What is the molar mass of the solute?

What will be the boiling point of $1 \ m$ urea solution in $K$ unit? $(K_b = 0.52 \ K \ kg \ mol^{-1})$

When common salt is dissolved in water,

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-$2$.

When a solute is dissolved in a solvent,the vapor pressure of the solvent decreases. As a result,........