Which of the following solutions exhibits the lowest value of boiling point elevation assuming complete dissociation?

The following graph shows the vapour pressure (in $atm$) on the $y$-axis versus temperature $T$ (in $K$) on the $x$-axis for pure water and an aqueous urea solution. What is the boiling point (in $K$) of the urea solution? (Atmospheric pressure $= 1 \ atm$)

Which among the following solutions has minimum boiling point elevation?

The order of boiling point $(B.P.)$ of the solutions formed is:

$A$ solution of a non-volatile solute has a boiling point elevation of $0.70 \text{ K}$. If $K_b$ for the solvent is $2.44 \text{ K kg mol}^{-1}$, what is the molality of the solution (in $\text{ m}$)?

An aqueous solution containing $1 \ g$ of urea boils at $100.25 \ ^oC$. The aqueous solution containing $3 \ g$ of glucose in the same volume will boil at ........ $^oC$. (Molecular weight of urea and glucose are $60$ and $180$ respectively)