Why is the value of E_a for a spontaneous reaction less than the E_a value for t

Question

Why is the value of E_a for a spontaneous reaction less than the E_a value for the same reaction running in reverse? The delta H is negative for the forward reaction, so the activation energy for the reverse reaction is larger because it is starting from a lower energy position. The delta G is negative for the reverse reaction, requiring more energy to be put into the system. The delta H is positive for the forward reaction, so the activation energy for the reverse reaction must provide the enthalpy change as well as the activation energy. The delta G is negative for the forward reaction, which causes the reverse reaction to start from a lower energy position. The delta S is positive for the forward reaction, so the activation energy for the reverse reaction must be larger to compensate. The delta S is negative for the forward reaction, so the activation energy for the reverse reaction must include the entropy change as well as the activation energy.

Explanation / Answer

Delta H is negative for the forward reaction, so the activation energy for the reverse reaction is larger because it is starting from a lower energy position.

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