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  • Consider Fig. 4.1 and mark the correct option. (i) The activation energy of forwarding reaction is E1 + E2 and the product is less stable than reactant.

Consider Fig. 4.1 and mark the correct option.

(i) The activation energy of forward reaction is E1 + E2 and the product is less stable than reactant.

(ii) The activation energy of forward reaction is E1 + E2 and product is more stable than reactant.

(iii) The activation energy of both forward and backward reaction is E1 + E2 and reactant is more stable than the product.

(iv) The activation energy of the backward reaction is E1 and the product is more stable than reactant.

 

Answers (1)

The answer is the option (i) E_{a}\; \text {forward}=E_{1}+E_{2}

As reactants have lower energy than the products, the products are less stable.

In the Arrhenius model of reaction rates, activation energy is the minimum amount of energy that must be available to reactants for a chemical reaction to occur. The activation energy of a reaction is measured in kilojoules per mole or kilocalories per mole. 

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