On increasing the temperature, the equilibrium constant of an endothermic reaction increases. It is due to

Given An equilibrium constant of an endothermic reaction.

Formula
For an exothermic reaction, heat is a product. Increasing the temperature will shift the equilibrium to the left while decreasing the temperature will shift the equilibrium to the
right.

Step $\mathrm{l}$ 

Increasing the temperature decreases the value of the equilibrium constant.

Step $\mathrm{ll}$

The forward reaction is endothermic, increasing the temperature increase the value of the equilibrium constant.

Hence, a greater increase in the activation energy of forwarding reaction in comparison to that of backward reaction is correct.

Therefore, the correct option is 1.