The boiling point of $0.2 \ m$ aqueous urea solution is $....... \ ^oC$. ($K_b$ of water $= 0.52 \ K \ kg \ mol^{-1}$)

If $K_{b}$ denotes the molal elevation constant of water,then the boiling point of an aqueous solution containing $36 \ g$ of glucose (molar mass $= 180 \ g/mol$) per $1 \ kg$ of water is:

Two different solutions were prepared by dissolving sucrose in water having concentrations of $1 \ m$ and $2 \ m$ respectively. The value of $(T_2 - T_1)$ will be ........... $K$. (Given: $K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$)

The elevation in boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of solvent is $0.1^{\circ}C$. The value of $K_b$ for the solvent is ........ $\frac{K}{m}$.

The value of $K_b$ is given by $mRT_b^2 / 1000 \, X$. In this relation,$X$ is :-

Which of the following statements is correct for the boiling point of a solvent containing a dissolved solid substance?