For a reversible endothermic reaction , the overall enthalpy change is . If the activation energy of — Chemical Kinetics Chemistry Question
Question
For a reversible endothermic reaction $A \rightarrow B$, the overall enthalpy change is $\Delta H = +20 \text{ kJ/mol}$. If the activation energy of the forward reaction is $E_{a(f)} = 85 \text{ kJ/mol}$, calculate the backward activation energy $E_{a(b)}$.
Answer: B
💡 Solution & Explanation
The fundamental thermodynamic relationship is $\Delta H = E_{a(f)} - E_{a(b)}$. Substituting the known values yields $+20 = 85 - E_{a(b)}$. Rearranging immediately provides $E_{a(b)} = 85 - 20 = 65 \text{ kJ/mol}$.
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