1. For spontaneity, we use the Gibbs free energy relation:

$\Delta G = \Delta H - T\Delta S$

A reaction is spontaneous when:

$\Delta G < 0$

and non-spontaneous when:

$\Delta G > 0$

2. The question states that the reaction is endothermic.

So,

$\Delta H > 0$

This already rules out options A and C.

3. The reaction is non-spontaneous at the freezing point of water ($0^\circ C = 273\,K$), but spontaneous at the boiling point of water ($100^\circ C = 373\,K$).

That means:

• At lower temperature: $\Delta G > 0$
• At higher temperature: $\Delta G < 0$

4. Since

$\Delta G = \Delta H - T\Delta S$

and increasing temperature makes the reaction become spontaneous, the term $-T\Delta S$ must become more negative as $T$ increases.

This is possible only if:

$\Delta S > 0$

Because if $\Delta S$ were negative, then $-T\Delta S$ would be positive and increasing temperature would make $\Delta G$ even more positive, not negative.

5. Therefore, we have:

$\Delta H > 0, \qquad \Delta S > 0$

6. Now evaluate the options:

• A: $\Delta H<0$, $\Delta S<0$ → incorrect
• B: $\Delta H>0$, $\Delta S<0$ → incorrect
• C: $\Delta H<0$, $\Delta S>0$ → incorrect
• D: $\Delta H>0$, $\Delta S>0$ → correct

Therefore, the correct option is:

$\boxed{D}$