Calculate the molality of a solution of a nonvolatile solute having a boiling point elevation of $1.89 \ K$,if the boiling point elevation constant of the solvent is $3.15 \ K \ kg \ mol^{-1}$. (in $m$)

$5 \text{ g}$ 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 $\text{ g}$)

$A$ solution of $5.6 \ g$ nonvolatile solute in $50 \ g$ solvent has an elevation in boiling point of $1.75 \ K$. What is the molar mass of the solute $\left(K_{b} = 3 \ K \ kg \ mol^{-1}\right)$?

$x \ g$ of urea (molar mass $60 \ g \ mol^{-1}$) is completely dissolved in $y \ g$ of pure water and the solution boiled at $373.202 \ K$. If the boiling point of pure water at $1.013 \ bar$ is $373.15 \ K$, then $x:y$ is $(K_b(H_2O) = 0.52 \ K \ kg \ mol^{-1})$

$Y \ g$ of non-volatile organic substance of molecular mass $M$ is dissolved in $250 \ g$ benzene. The molal elevation constant of benzene is $K_b$. The elevation in its boiling point is given by:

Molal elevation constant is the elevation in boiling point produced by