In the equilibrium reaction, A + B $⇌$ C + D, the activation energy for the forward reaction is 25 kcal mole $^{- 1}$ and that of the backward reaction is 15 kcal mole $^{- 1}$ . Which one of the following statements is correct?

The reaction is exothermic

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The reaction is endothermic

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The reaction has

Δ H

of 20 kcal mol

^{- 1}

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Both

A

and

C

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Solution

The correct option is C The reaction is endothermic
Reaction is endothermic as activation energy required for forward reaction is more than the reverse reaction.

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In the equilibrium reaction, A + B ⇌ C + D, the activation energy for the forward reaction is 25 kcal mole−1 and that of the backward reaction is 15 kcal mole−1. Which one of the following statements is correct?

The correct option is C The reaction is endothermicReaction is endothermic as activation energy required for forward reaction is more than the reverse reaction.

In the equilibrium reaction, A + B $⇌$ C + D, the activation energy for the forward reaction is 25 kcal mole $^{- 1}$ and that of the backward reaction is 15 kcal mole $^{- 1}$ . Which one of the following statements is correct?

The correct option is C The reaction is endothermic
Reaction is endothermic as activation energy required for forward reaction is more than the reverse reaction.