The elevation in boiling point of 1 molal aqueous solution of urea is X K. The  elevation in boing point of 0.2 molal aqueous solution of Aluminium sulphate is (Assuming complete ionization).

For Urea solution, the elevation is boiling point, i.e;

$$\begin{gathered} ∆{\mathrm{T}}_{\mathrm{b}} = {\mathrm{k}}_{\mathrm{b}}\mathrm{m} \\ \mathrm{X}={\mathrm{k}}_{\mathrm{b}}\times 1..\left(1\right) \end{gathered}$$

For 1 molal solution, kb is X, then for 0.2 

For Al₂(SO₄)₃ solution, formula used:

$∆{\mathrm{T}}_{\mathrm{b}} =\mathrm{i} {\mathrm{k}}_{\mathrm{b}}\mathrm{m}$ 

Here, i = Van't Hoff Factor 

Assuming complete ionization:

 ${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3\to 2{\mathrm{Al}}^{3+}+2{\mathrm{SO}}_4^{2-}$

 $∆{\mathrm{T}}_{\mathrm{b}} =\mathrm{i} {\mathrm{k}}_{\mathrm{b}}\mathrm{m}=5\times 0.2\times {\mathrm{k}}_{\mathrm{b}}=1 {\mathrm{k}}_{\mathrm{b}}...\left(2\right)$

Equation (2) and equation (1) is same, hence option-4 is correct.