The boiling point of a $0.1 \ m$ aqueous solution of urea is $100.18 \ ^\circ C$ at $1 \ atm$. The molal elevation constant $(K_b)$ of water is:

If $0.15 \ g$ of a solute dissolved in $15 \ g$ of solvent is boiled at a temperature higher by $0.216 \ ^oC$ than that of the pure solvent,what is the molecular weight of the substance? (Given: molal elevation constant for the solvent is $2.16 \ ^oC \ kg \ mol^{-1}$)

The rise in the boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of a solvent is $0.1 \ ^\circ C$. The molal elevation constant of the liquid is .......... $K/m$.

The elevation in boiling point of a $0.25 \ molal$ aqueous solution of a substance is $(K_b = 0.52 \ K \ kg \ mol^{-1})$. (in $K$)

Boiling point of a $2\%$ aqueous solution of a non-volatile solute $A$ is equal to the boiling point of an $8\%$ aqueous solution of a non-volatile solute $B$. The relation between molecular weights of $A$ and $B$ is:

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