For a reversible& reaction, A ⇌ B ,& which one of the following...

For a reversible& reaction, $A ⇌ B$ ,& which one of the following statement is wrong from the given energy& profile diagram?

For a reversible& reaction, A ⇌ B ,& which one of the following statement is wrong from the given energy& profile

Options

AActivation energy of forward reaction is greater than backward reaction
BThe forward reaction is endothermic
CThe threshold energy is less than that of activation energy
DThe energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activation of backward reaction

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

For a reversible& reaction, A ⇌ B ,& which one of the following statement is wrong from the given energy& profile

where, ${E}_{a} =$ activation energy of forward reaction

${E}_a^{'} =$ activation energy of backward reaction

The above energy profile diagram shows that ${E}_{a} > {Ea}^{'}$

The potential energy of the product is greater than that of the reactant, so the reaction is endothermic.

${E}_{a} = {E}_a^{'} + \Delta E$

${E}_{t} = {E}_{a}$ or ${E}_{t} > {Ea}^{'}$