$A$ solution containing $0.1050 \ g$ of a substance in $15.84 \ g$ of ether has a boiling point $1 \ ^\circ C$ higher than that of pure ether. What is the molar mass of the substance? [Given: Molar elevation constant for ether per $100 \ g = 21.6$]

$A$ 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?

When $1.8 \ g$ of glucose is dissolved in $100 \ g$ of solvent,the boiling point of the solution increases by $0.1 \ ^\circ C$. The molal elevation constant of the solvent is ............ $\frac{K}{m}$.

Calculate the boiling point of an aqueous solution containing $18 \text{ g}$ of glucose in $100 \text{ g}$ of water, given that the molal elevation constant $(K_b)$ of water is $0.5 \text{ K kg mol}^{-1}$. [Molar mass of glucose $= 180 \text{ g mol}^{-1}$ and boiling point of pure water $= 100^{\circ}\text{C}$] (in $^{\circ}\text{C}$)

Calculate the molar mass of a non-volatile solute when $4 \text{ g}$ of it is dissolved in $100 \text{ g}$ of a solvent that boils at $319.4 \text{ K}$. Given: $K_b = 2.4 \text{ K kg mol}^{-1}$ and the boiling point of the pure solvent is $319 \text{ K}$.

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 $= 1 \ atm$)