Q.
For a reversible reaction, $A \rightleftharpoons B$, which one of the following statements is wrong from the given energy profile diagram?
A) Activation energy of forward reaction is greater than backward reaction
B) The forward reaction is endothermic
C) The threshold energy is less than that of activation energy
D) The energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activation of backward reaction
Explanation
(c)
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Where,
$E_{a} =$activation energy of forward reaction
$E_{a}^{''}$=activation energy of backward reaction
The above energy profile diagram shows that
$E_{a} > E_{a}^{''}$
The potential energy of the product is greater than that of the reactant, so the reaction is endothermic.
$E_{a} = E_{a}^{''} + \mathrm{\Delta}E$
$E_{t} = E_{a}$ or $E_{t} > E_{a}^{''}$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.