Ncert Exercises & Solutions

The correct statement based on the graph below is:

1.	The activation energy of the forward reaction is E₁ + E₂ and the product is less stable than reactant.
2.	The activation energy of the forward reaction is E₁ + E₂ and the product is more stable than the reactant.
3.	The activation energy of both forward and backward reaction is E₁+ E₂ and reactant is more stable than the product.
4.	The activation energy of the backward reaction is E₁ and the product is more stable than reactant.

HINT: Reactant is more stable than product.

Explanation:

Activation energy is the minimum energy required to convert reactant molecules to product molecules. Here, the energy gap between reactants and activated complex is the sum of $E_{1}$ $and$ $E_{2}$ .

Activation energy = $E_{1}$ $+ E_{2}$

The product is less stable than the reactant as the energy of the product is greater than the reactant.

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