Consider an endothermic reaction with activation energies and for the backward and forward reactions — Reaction Mechanism Chemistry Question

💡 Solution & Explanation

In an energy profile diagram, the enthalpy change of the reaction is given by $\Delta H = E_f - E_b$. For an endothermic reaction, the energy of the products is higher than the energy of the reactants, meaning $\Delta H$ is positive ($+ve$). Therefore, $E_f - E_b > 0$, which implies $E_b < E_f$.