NEET Chemistry Activation Energy Assertion Reason Question
Assertion (A): Activation energy is necessary for the formation of an unstable intermediate in a reaction. | Reason (R): The Arrhenius equation shows that a reaction can only occur when molecules collide with energy equal to or greater than the activation energy.
Both A and R are true, and R is the correct explanation of A.
Both A and R are true, but R is not the correct explanation of A.
A is true, but R is false.
A is false, but R is true.
Correct Answer
Detailed Explanation
The assertion and reason both are true as the activation energy is needed for the formation of an unstable intermediate, and the Arrhenius equation supports this by indicating that collisions must have energy greater than or equal to the activation energy for a reaction to occur.
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