For a reversible reaction $\quad A \rightleftharpoons B$, which one of the following statements is wrong…

For a reversible reaction $\quad A \rightleftharpoons B$, which one of the following statements is wrong from the given energy profile diagram?

1. Activation energy of forward reaction is greater than backward reaction
2. The forward reaction is endothermic
3. The threshold energy is less than that of activation energy
4. The energy of activation of forward reaction is equal to the sum of heat of reaction and the energy of activation of backward reaction

Solution

where, $E_a=$ activation energy of forward reaction $E_a^{\prime}=$ activation energy of backward reaction The above energy profile diagram shows that $ E_a>E_a^{\prime} $ The potential energy of the product is greater than that of the reactant, so the reaction is endothermic. $ \begin{aligned} & E_a=E_a^{\prime}+\Delta E \\ & E_t=E_a \text { or } E_t>E_a^{\prime} \end{aligned} $

Asked in: AP EAMCET 2008

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