Calculate the molality of a solution of a non-volatile solute if the boiling point elevation is $1.75 \ K$ and the $K_b$ for the solvent is $3 \ K \ kg \ mol^{-1}$. (in $m$)

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

$A$ solution of a nonvolatile solute is obtained by dissolving $1.5 \ g$ in $30 \ g$ of solvent. The boiling point elevation is $0.65 \ K$. Calculate the molal elevation constant if the molar mass of the solute is $150 \ g \ mol^{-1}$.

If the boiling point of a solution is $T_1$ and the boiling point of the pure solvent is $T_2$,then the elevation in boiling point is given by:

$0.15 \ g$ of a solute is dissolved in $15 \ g$ of a solvent. If the solution boils at a temperature $0.215 \ K$ higher than the boiling point of the pure solvent,what is the molar mass of the solute? $(K_b = 2.15 \ K \ kg \ mol^{-1})$

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