For an endothermic reaction, where Δ H represent the enthalpy of...

We know that, $\Delta H = {E}_{f} - {E}_{b}$

where, ${E}_{b}$ and ${E}_{f} =$ activation energy for backward and forward respectively.

Thus,${E}_{f} = \Delta H + {E}_{b}$, means ${E}_{f} > \Delta H$.

$\Delta H =$ heat of reaction (endothermic)

${E}_{a} =$ energy of activation

Thus, ${E}_{a} > \Delta H$

Heat is absorbed in an endothermic reaction. Thus, for an endothermic reaction, where $\Delta H$ represent the enthalpy of reaction in $kJ{mol}^{- 1}$, the minimum value for energy of activation (for forward reaction) will be more than $\Delta H$.