What is the molality of a solution of a nonvolatile solute having a boiling point elevation of $7.15 \ K$ and a molal elevation constant of $2.75 \ K \ kg \ mol^{-1}$ (in $m$)?

When $3 \ g$ of a non-volatile solute is dissolved in $200 \ mL$ of water, the boiling point of the solution becomes $100.52 \ ^oC$. If $K_b$ for water is $0.6 \ K \ kg \ mol^{-1}$, the molar mass of the solute is ......... $g \ mol^{-1}$.

Which of the following statements is correct for the boiling point of a liquid?

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

The boiling point of benzene is $353.23 \, K$. When $1.80 \, g$ of a non-volatile solute was dissolved in $90 \, g$ of benzene,the boiling point is raised to $354.11 \, K$. Calculate the molar mass of the solute. $K_{b}$ for benzene is $2.53 \, K \, kg \, mol^{-1}$.

$A$ solution is prepared by dissolving a $2.5 \ g$ sample of an unknown compound in $34 \ g$ of benzene,$C_6H_6$. The solution boils at $1.38 \ ^\circ C$ higher than pure benzene. Which expression gives the molar mass of the unknown compound? $K_b$ of $C_6H_6$ is $2.53 \ ^\circ C \ m^{-1}$.