Question

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.

Answer 1

The correct option is C The threshold energy is less than that of activation energy.

Conclusion:

$\bullet$ Activation energy of forward reaction is greater than backward reaction.

$E_f>E_b$

$\bullet$ Product level is higher than Reactant level forward reaction is endothermic.

$\bullet$ The threshold energy is more than the activation energy of forward reaction.

$\bullet$ $E_f=H+E_b$

The energy of activation of forward reaction is equal to the sum of the heat of reaction and the energy of activation of backward reaction.