What is the boiling point of a decimolal aqueous solution of glucose if the molal elevation constant for water is $0.52 \ ^{\circ}C \ kg \ mol^{-1}$ (in $^{\circ}C$)?

$A$ 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 $150 \ g \ mol^{-1}$.

$2 \, g$ 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)

Calculate the number of moles of nonvolatile solute dissolved in $0.3 \ kg$ solvent if $\Delta T_{b}=0.3 \ K$ and $K_{b}$ for solvent is $1.8 \ K \ kg \ mol^{-1}$.

If the boiling point of water is $100 \,^{\circ}C$,how many grams of $NaCl$ must be added to $500 \,g$ of water to increase the boiling point by approximately $1 \,^{\circ}C$ (in $,g$)? Given $(K_{b})_{H_2O} = 0.52 \,K \cdot kg/mol$.

$180 \ g$ of glucose,$C_6H_{12}O_6$,is dissolved in $1 \ kg$ of water in a vessel. The temperature at which water boils at $1.013 \ bar$ is $ . . . . . . $ (given,$K_b$ for water is $0.52 \ K \ kg \ mol^{-1}$. Boiling point for pure water is $373.15 \ K$) (in $K$)