Which outcome occurs when a solid catalyst is introduced to reactants already at equilibrium in a closed system?

💡 Explanation

When a catalyst is introduced to a system at equilibrium, the forward and reverse reaction rates both increase equally because the catalyst lowers the activation energy for both directions, maintaining the same equilibrium concentrations. Therefore, the equilibrium constant remains unchanged, rather than the shift favoring products, or a rate decrease, which violate Le Chatelier's principle.

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