For an endothermic reaction, where \(\Delta Η\) represents the enthalpy of the reaction in kJ/mole, the minimum value for the energy of activation will be:

More than \(\Delta Η\)

The answer is (3) More than \(\Delta Η\).

The minimum value for the energy of activation for an endothermic reaction will be more than \(\Delta Η\).

An endothermic reaction is a reaction that absorbs heat from its surroundings. This means that the products of the reaction have a higher energy than the reactants. The energy of activation is the minimum amount of energy that a reactant molecule must have in order to react. In order for an endothermic reaction to occur, the reactant molecules must have enough energy to overcome the energy barrier of activation and reach the transition state. The transition state is the unstable intermediate state that forms when the reactant molecules collide and react.

The energy of activation is always greater than or equal to \(\Delta Η\). This is because the reactant molecules must have enough energy to overcome the energy barrier of activation and reach the transition state, and then they must also have enough energy to form the products of the reaction. The minimum value for the energy of activation will be equal to \(\Delta Η\) if the transition state is at the same energy level as the reactants. However, the transition state is usually at a higher energy level than the reactants, so the minimum value for the energy of activation will be more than \(\Delta Η\).

Option (1) is incorrect because the energy of activation cannot be less than \(\Delta Η\). Option (2) is incorrect because the energy of activation cannot be zero. Option (4) is incorrect because the energy of activation cannot be equal to \(\Delta Η\).