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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 activa

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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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