Molal elevation constant is the elevation in boiling point produced by

If $0.15 \ g$ of a solute is dissolved in $15 \ g$ of solvent and the solution boils at a temperature $0.216 \ ^oC$ higher than that of the pure solvent, what is the molecular weight of the substance? (Given: molal elevation constant for the solvent is $2.16 \ ^oC \ kg \ mol^{-1}$)

The boiling point of chloroform was raised by $0.323 \ K$ when $0.5143 \ g$ of anthracene was dissolved in $35 \ g$ of chloroform. The molecular mass of anthracene is ....... $g/mol$. (${K_b}$ for $CHCl_3 = 3.9 \ K \ kg \ mol^{-1}$)

Calculate the molar mass of a non-volatile solute when $5 \ g$ of it is dissolved in $50 \ g$ of solvent,which boils at $119.6^{\circ} C$. $[K_{b} = 3.2 \ K \ kg \ mol^{-1}$,boiling point of pure solvent $= 118^{\circ} C]$.

What is the relation between the molar mass of a solute and the boiling point elevation?

The following graph shows the vapour pressure (in $atm$) on the $y$-axis versus temperature $T$ (in $K$) on the $x$-axis for pure water and an aqueous urea solution. What is the boiling point (in $K$) of the urea solution? (Atmospheric pressure $= 1 \ atm$)