How does adding a heterogeneous solid catalyst affect an equilibrium reaction such as the contact process for sulfuric acid production?

Answer and explanation

Correct answer: C. It increases the rates of both forward and reverse reactions equally without altering Kc

  1. Step 1: A catalyst lowers the activation energy by providing an alternative reaction pathway.
  2. Step 2: Because it lowers the barrier equally for both forward and reverse processes, both rates increase by the exact same factor.
  3. Step 3: A catalyst helps reach equilibrium faster, but does not alter the equilibrium constant Kc or final product yield.
Answer
It increases the rates of both forward and reverse reactions equally without altering Kc.
Why not the others: 'It shifts the position of equilibrium toward the products and increases yield' is a common misconception; catalysts do not affect thermodynamic equilibrium; 'It decreases the activation energy of the forward reaction only' violates microscopic reversibility; 'It increases the equilibrium constant Kc' is false because Kc depends exclusively on temperature.

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