Which among the following solutions has minimum boiling point elevation?

$2 \text{ g}$ of a non-electrolyte solute, when dissolved in $50 \text{ g}$ of water, increases its boiling point by $0.13 \text{ K}$. Calculate the molar mass of the solute if the molal elevation constant $(K_b)$ of water is $0.52 \text{ K kg mol}^{-1}$.

The correct relation between the elevation in boiling point and the molar mass of a solute is: ($W_1$ and $W_2$ are respectively weight of solvent $\&$ solute)

$18 \, g$ of glucose $(C_{6}H_{12}O_{6})$ dissolved in $1 \, kg$ of water is heated to boiling. The boiling point (in $K$) measured at $1 \, atm$ pressure is closest to: [Ebullioscopic constant,$K_{b}$ for water is $0.52 \, K \, kg \, mol^{-1}$. Consider the boiling point of pure water to be $373.15 \, K$]

$0.15 \ g$ 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? $(K_b = 2.15 \ K \ kg \ mol^{-1})$

$18 \ g$ of glucose,$C_6H_{12}O_6$,is dissolved in $1 \ kg$ of water in a saucepan. At what temperature will water boil at $1.013 \ bar$ (in $K$)? $K_b$ for water is $0.52 \ K \ kg \ mol^{-1}$.