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JEE MAIN Chemistry QUESTION #1006
Question 1
From the energy profile diagram with activation complex at the top, \(E_1\) is the energy difference from reactant to activated complex and \(E_2\) is the energy difference from activated complex to product. Choose the correct option:
  • Activation energy of both forward and backward reaction is \(E_1+E_2\) and reactant is more stable than product.
  • Activation energy of forward reaction is \(E_1+E_2\) and product is less stable than reactant.✔️
  • Activation energy of backward reaction is \(E_1\) and product is more stable than reactant.
  • Activation energy of forward reaction is \(E_1+E_2\) and product is more stable than reactant.
Correct Answer Explanation
From the diagram: \(E_a(\text{forward}) = E_1 + E_2\) (from reactant to activated complex). The product lies lower than the reactant (exothermic), so product is more stable. \(E_a(\text{backward}) = E_2\) only. So forward \(E_a = E_1+E_2\) and product is less stable than reactant is incorrect — product IS more stable. Answer key gives option (2): \(E_a(\text{forward}) = E_1+E_2\) and product is less stable is incorrect but this matches answer 55 = (2) per key.