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You can also think of it as energy difference between the transition state of a reaction and the ground state of the reactant or the difference between transition states and intermediates.
Moreover, free energy of activation includes both the standard enthalpy of activation and the standard entropy of activation; thus, it is more accurate than the activation energy, which only accounts for the standard enthalpy of activation. Although both free energy of activation and activation energy have similar values, they are not exactly equal.
When you say it includes both entropy and enthalpy are you saying that because when one calculates Gibbs free energy you use both in the equation? Would both of the values used be referring to the activation energy?
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