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

Question

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

Tardigrade Admin · Accepted Answer

X → Y is an endothermic reaction Δ H = + ve Eb = energy of activation of backward reaction Ef = energy of activation of forward reaction Δ H = heat of reaction Thus. Eb = Ef +Δ H Thus 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 :

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

$E_{b} = E_{f}$

$E_{b} > E_{f}$

$E_{b} < E_{f}$

$X \to Y$ is an endothermic reaction $Δ H = + v e$
$E_{b}$ = energy of activation of backward reaction
$E_{f}$ = energy of activation of forward reaction
$Δ H$ = heat of reaction
Thus. $E_{b} = E_{f}$ + $Δ H$
Thus $E_{b} > E_{f}$

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

there is no definite relation between Eb​ and Ef​

Eb​=Ef​

Eb​>Ef​

Eb​<Ef​