The vapour pressure vs. temperature curve for a solution-solvent system is shown below. The boiling point of the solvent is $........\,^{\circ} C$.

Calculate the number of moles of nonvolatile solute dissolved in $0.5 \ kg$ solvent if molal elevation constant for solvent is $2 \ K \ kg \ mol^{-1}$ and the elevation in boiling point is $\Delta T_{b} = 0.8 \ K$.

The solution containing $3 \ g$ urea (molar mass $60 \ g \ mol^{-1}$) per $dm^3$ of water and another solution containing $4.5 \ g$ of solute $A$ per $dm^3$ of water boil at the same temperature. What is the molar mass of $A$?

$2 \, g$ of a non-volatile non-electrolyte solute is dissolved in $200 \, g$ of two different solvents $A$ and $B$ whose ebullioscopic constants are in the ratio of $1: 8$. The elevation in boiling points of $A$ and $B$ are in the ratio $\frac{x}{y} (x: y)$. The value of $y$ is .... (Nearest integer)

$A$ solution of a nonvolatile solute is obtained by dissolving $3.5 \ g$ of solute in $100 \ g$ of solvent. The boiling point elevation is $0.35 \ K$. Calculate the molar mass of the solute. $(K_b = 2.5 \ K \ kg \ mol^{-1})$

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