Consider an endothermic reaction X arrow Y with the activation energies Eb and Ef for the backward and forward reactions, respectively. In general

Question

Consider an endothermic reaction X arrow Y with the activation energies Eb and Ef for the backward and forward reactions, respectively. In general (A) Eb< Ef (B) Eb> Ef (C) Eb=Ef (D) there is no definite relation between Eb and Ef.

Tardigrade Admin · Accepted Answer

For endothermic reaction, Δ H=+ mathrmve Δ H=Ef-Eb, it means Eb< Ef

Q. Consider an endothermic reaction $X \to Y$ with the activation energies $E_{b}$ and $E_{f}$ for the backward and forward reactions, respectively. In general

$E_{b} < E_{f}$

$E_{b} > E_{f}$

$E_{b} = E_{f}$

there is no definite relation between $E_{b}$ and $E_{f}$ .

For endothermic reaction, $Δ H = + ve$
$Δ H = E_{f} - E_{b},$ it means $E_{b} < E_{f}$

Q. Consider an endothermic reaction X→Y with the activation energies Eb​ and Ef​ for the backward and forward reactions, respectively. In general

Eb​<Ef​

Eb​>Ef​

Eb​=Ef​

there is no definite relation between Eb​ and Ef​.