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 $E_{b} a n d E_{f}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$E_{b} = E_{f}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$E_{b} > E_{f}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$E_{b} < E_{f}$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D
$E_{b} < E_{f}$

Enthalpy of reaction $(Δ H) = E_{a_{(f)}} - E_{a_{(b)}}$ for an endothermic reaction $Δ H$ = + ve hence for $Δ H$ to be negative $E_{a_{(b)}}$ < $E_{a_{(f)}}$

Suggest Corrections

Similar questions

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

Q. Consider the endothermic reaction,

X ⟶ Y

, with the activation energies

E_{b}

and

E_{f}

for backward and forward reactions, respectively. In general:

Q. Consider an endothermic reaction

X \to Y

with the activation energies

E_{b}

and

E_{f}

for the backward and forward reactions respectively. Here

Q. Which one of the following is true for an exothermic reaction

A ⇌ B

. If

E_{f}

and

E_{b}

are the activation energies of forward and backward reactions respectively?

Q. For an endothermic reaction, the correct statement about the energy of activation for forward and backward reaction is:

Join BYJU'S Learning Program

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

The correct option is D Eb<Ef Enthalpy of reaction (ΔH)=Ea(f)−Ea(b) for an endothermic reaction ΔH = + ve hence for ΔH to be negative Ea(b) < Ea(f)

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

The correct option is D
$E_{b} < E_{f}$

Enthalpy of reaction $(Δ H) = E_{a_{(f)}} - E_{a_{(b)}}$ for an endothermic reaction $Δ H$ = + ve hence for $Δ H$ to be negative $E_{a_{(b)}}$ < $E_{a_{(f)}}$