When $0.5143 \ g$ of anthracene is dissolved in $35 \ g$ of $CHCl_3$,the boiling point of $CHCl_3$ increases by $0.323 \ K$. Calculate the molar mass of anthracene. ($K_b$ for $CHCl_3 = 3.9 \ K \ kg \ mol^{-1}$)

$A$ 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.)

If the boiling point of water is $100 \,^{\circ}C$,how many grams of $NaCl$ must be added to $500 \,g$ of water to increase the boiling point by approximately $1 \,^{\circ}C$ (in $,g$)? Given $(K_{b})_{H_2O} = 0.52 \,K \cdot kg/mol$.

Calculate the molality of the solution containing a nonvolatile solute if the boiling point elevation of the solution is $0.39 \ K$.
[$K_{b}$ of water $= 0.52 \ K \ kg \ mol^{-1}$]

$2 \, g$ 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)

The boiling point of a $0.1 \ m$ aqueous solution of urea is $100.18 \ ^\circ C$ at $1 \ atm$. The molal elevation constant $(K_b)$ of water is: