Activation energy

$\Delta H = (E_a)_f - (E_a)_b$
Given $(E_a)_f = (E_a)_b$, so $\Delta H = 0$

In an endothermic reaction the products lie at a higher energy than the reactants by $\Delta H$.
The reactants must climb to the top of the energy barrier (the activated complex), which lies above the products.
From the energy profile: $E_a(\text{forward}) = \Delta H + E_a(\text{backward})$
$E_a(\text{backward})$ is always a positive quantity.
Therefore $E_a(\text{forward}) > \Delta H$; the activation energy must be more than $\Delta H$.