Consider an endothermic reaction, X → Y with the activation energies E_b and E_f for the backward and forward reactions, respectively. In general: - Chemistry MCQ AIEEE 2026 | ExamTest.live

mediumMCQAIEEE2026Chemistry

2 attempts0% success rate1 mark

Consider an endothermic reaction, X \to Y with the activation energies E_{b} and E_{f} for the backward and forward reactions, respectively. In general:

Solution & Step-by-step Explanation

For any reaction, the enthalpy change (Δ H) is given by: Δ H = E_{f} - E_{b} For an endothermic reaction, Δ H is positive (Δ H > 0). E_{f} - E_{b} > 0 ⟹ E_{f} > E_{b} Therefore, the activation energy of the forward reaction is greater than that of the backward reaction.

Try it yourself before checking the explanation above.

Consider an endothermic reaction, X \to Y with the activation energies E_{b} and E_{f} for the backward and forward reactions, respectively. In general:

E_{b} < E_{f}

E_{b} > E_{f}

E_{b} = E_{f}

There is no definite relation between E_{b} and E_{f}

Practice with timed mock tests and track your performance across Chemistry.