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 $CHCl_3 = 3.9 \ K \ kg \ mol^{-1}$)

If the enthalpy of vaporization is approximately the same,for which of the following will the value of the ebullioscopic constant $(K_b)$ be maximum?

The order of boiling point $(B.P.)$ of the solutions formed is:

$5 \text{ g}$ of urea is dissolved in $100 \text{ g}$ of water. Find the amount of glucose to be dissolved in $120 \text{ g}$ of water so that the boiling points of both solutions are the same. [Molar mass of urea $= 60 \text{ g mol}^{-1}$, Molar mass of glucose $= 180 \text{ g mol}^{-1}$] (in $\text{ g}$)

What is the molal elevation constant if one gram mole of a nonvolatile solute is dissolved in $1 \ kg$ of ethyl acetate? $(\Delta T_{b} = x \ K)$

Which of the following solutions will exhibit the highest boiling point?