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 $\Delta T_{b} = 0.8 \ K$.

If the boiling point of a urea solution is $100.18^{\circ}C$ and $K_b$ for water is $0.512 \ K \ kg \ mol^{-1}$,what is the molality of the solution? (Boiling point of water $= 100^{\circ}C$)

Elevation in boiling point was $0.52 \, ^\circ C$ when $6 \, g$ of a compound $X$ was dissolved in $100 \, g$ of water. The molecular weight of $X$ is: ($K_b$ for water is $0.52 \, K \, kg \, mol^{-1}$)

When $0.5 \ g$ of anthracene is dissolved in $35 \ g$ of chloroform,the boiling point increases by $0.3 \ K$. If the $K_b$ value for $CHCl_3$ is $3.9 \ K \ kg \ mol^{-1}$,the experimental molar mass of anthracene is ......... $g \ mol^{-1}$.

Which of the following aqueous solutions containing $10 \ g$ of solute in each case has the highest boiling point $(B.P.)$?

Which of the following aqueous solutions will have a boiling point of $102.2^{\circ} C$? The molal elevation constant for water is $K_b = 0.512 \ K \ kg \ mol^{-1}$. (Note: The provided constant $2.2 \ K \ kg \ mol^{-1}$ in the prompt is incorrect for water; using standard $K_b = 0.512 \ K \ kg \ mol^{-1}$ for calculation).