JEE Main 2025 Jan 22 Shift 2, Chemistry Q4: Factors Affecting The Rate of a Chemical Reaction

JEE Main2025Jan 22, Shift 2Chemistry

Consider the given figure and choose the correct option :

A
Activation energy of backward reaction is $E_{1}$ and product is more 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 forward reaction is $E_{1} + E_{2}$ and product is less stable than reactant.
D
Activation energy of both forward and backward reaction is $E_{1} + E_{2}$ and reactant is more stable than product.

Solution

From the diagram, the activated complex sits at the top of the energy barrier. Starting from the reactant, the system must climb the full barrier to reach the transition state, so:

$E_{a, forward} = E_{1} + E_{2}$ .

The product energy level lies above the reactant level (closer to the peak by $E_{1}$ alone). Since lower energy corresponds to greater thermodynamic stability:

$E_{product} > E_{reactant} \Rightarrow$ product is less stable than reactant.

$∴$ The correct statement is option (3).

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JEE Main 2025 Jan 22 Shift 2, Chemistry Q4: Factors Affecting The Rate of a Chemical Reaction

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