Which outcome results when a catalyst decreases the activation energy barrier in a reversible chemical reaction approaching equilibrium?

💡 Explanation

When a catalyst decreases the activation energy, both forward and reverse reaction rates are accelerated equally because the catalyst lowers the activation energy barrier for both pathways according to the Arrhenius equation, thus increasing the rate constants, kf and kr, to the same extent. Therefore, equally increasing constants occurs, rather than equilibrium shift or selectively improved action which alters the kinetics differentially.

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