For an endothermic reaction, where ΔΗ represents the enthalpy of the reaction in kJ/mole, the minimum value for the energy of activation will be:

More than ΔΗ

For an endothermic reaction, the minimum value for the energy of activation will be greater than ΔH (the enthalpy change of the reaction).

The energy of activation (E_a) represents the minimum energy required for the reactant molecules to reach the transition state and form the products. In an endothermic reaction, energy is absorbed from the surroundings, and the products have higher energy than the reactants.

Since the reaction requires an input of energy, the energy of activation must be higher than the enthalpy change (ΔH) of the reaction. This ensures that the reactants have enough energy to overcome the energy barrier and proceed to the product state.

Therefore, the correct answer is (3) More than ΔH, indicating that the minimum value for the energy of activation will be greater than the enthalpy change of the reaction.