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The activation energy of reverse reaction will depend upon whether the forward reaction is exothermic or endothermic. For exothermic reaction, ΔH = Eₐ(forward reaction) − Eₐ(backward reaction). For endothermic reaction, ΔH = Eₐ(backward reaction) − Eₐ(forward reaction). Which of the following is correct?

1. ΔH = −ve, Eₐ(forward) > Eₐ(backward)
2. ΔH = +ve, Eₐ(forward) < Eₐ(backward)
3. ΔH = −ve, Eₐ(forward) < Eₐ(backward)
4. ΔH = +ve, Eₐ(forward) > Eₐ(backward)

Correct answer: ΔH = −ve, Eₐ(forward) > Eₐ(backward)

Solution

For an exothermic reaction, ΔH is negative, and the activation energy of the forward reaction is greater than that of the backward reaction. This is consistent with the relationship ΔH = Eₐ(forward) − Eₐ(backward).

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