JEE MAIN - Chemistry (2025 - 22nd January Evening Shift - No. 8)
Consider the given figure and choose the correct option :
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Activation energy of both forward and backward reaction is $E_1+E_2$ and reactant is more stable than product.
Activation energy of forward reaction is $E_1+E_2$ and product is more stable than reactant.
Activation energy of backward reaction is $\mathrm{E}_1$ and product is more stable than reactant.
Activation energy of forward reaction is $E_1+E_2$ and product is less stable than reactant.
Explanation
$E_1$ represents the activation energy for the backward reaction.
$E_1 + E_2$ is the activation energy for the forward reaction.
The product has more energy than the reactant, indicating that the product is less stable compared to the reactant.
This information is crucial in determining the relative stability of reactants and products and the required energy for the reactions to proceed in either direction.
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