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Activation Energy

The Δ H val...

Question

The $Δ H$ value of the reaction $H_{2} + C l_{2} ⇌ 2 H C l$ is $- 44.12 k c a l$ . If $E_{1}$ is the activation energy of the products, then for the above reaction

E_{1} > E_{2}

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E_{1} < E_{2}

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E_{1} = E_{2}

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Δ H

is not related to

E_{1}

and

E_{2}

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None is correct

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Solution

The correct option is A $E_{1} > E_{2}$
$Δ H = E_{2} - E_{1} = N e g a t i v e$
$E_{1}$ is the activation energy of the products
$E_{2}$ is the activation energy of the reactants.

Thus , $E_{1} > E_{2}$

Option (A) is correct.

Suggest Corrections

Similar questions

Consider figure and mark the correct option.

(a) Activation energy of forward reaction is $E_{1}$ + $E_{2}$ and product is less stable than reactant

(b) Activation energy of forward reaction is $E_{1}$ + $E_{2}$ and product is more stable than reactant

(c) Activation energy of both forward and backward reaction is $E_{1}$ + $E_{2}$ and reactant is more stable than product

(d) Activation energy of backward reaction is $E_{1}$ and product is more stable than reactant

E_{1}, E_{2}, E_{3} a n d E_{4}

1^{s t}, 2^{n d}, 3^{r d}

4^{t h}

N_{2} + 3 H_{2} ⟶ 2 N H_{3}

E_{1}

E_{2}

N H_{3}

N_{2}

E_{1} - E_{2}

E_{1}, E_{2}, E_{3} a n d E_{4}

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