The change in the activation energy barrier is the same: 27.6 kJ/mole.
By reducing the activation energy, a catalyst can speed up a process. In the case of this question, the activation energy is reduced by 27.6 kg per mole, which unquestionably speeds up the reaction.
However, a catalyst does not disrupt the equilibrium because it clearly affects both the forward and backward reaction rates as shown in the picture attached below.
As a result, the forward reaction's activation energy is reduced by 27.6 kJ/mole. Then perhaps the activation energy barrier, 27.6 KJ/mole for the reverse reaction, does not change. Consequently, the addition of a catalyst has no effect on the equilibrium.
Therefore, the activation energy barrier remains constant at 27.6 kJ/mole.
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