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(A) For an exothermic reaction, the energy of the products is lower than the energy of the reactants. As shown in the energy profile diagram, the acti

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The backward reaction has higher activation energy than the forward reaction

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(A) For an exothermic reaction, the energy of the products is lower than the energy of the reactants. As shown in the energy profile diagram, the activation energy for the forward reaction $(E_{a,f})$ is the energy difference between the transition state and the reactants. The activation energy for the backward reaction $(E_{a,b})$ is the energy difference between the transition state and the products. Since the products are at a lower energy level than the reactants, the energy barrier to reach the transition state from the products $(E_{a,b})$ is greater than the energy barrier from the reactants $(E_{a,f})$. Therefore, $(E_{a,b}) > (E_{a,f})$.

For a reversible chemical reaction where the forward process is exothermic, which of the following statements is correct?

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