To observe an elevation of boiling point of $0.05^{\circ} C$,the amount of a solute (mol. wt. $= 100$) to be added to $100 \ g$ of water $(K_{b} = 0.5)$ is (in $g$)

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:

The molal elevation constant is the ratio of the elevation in boiling point to the $......$.

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

Give the unit for the molal elevation constant in boiling point.

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 $1.8 \ K \ kg \ mol^{-1}$.