Question

Assertion: All the collisions of the reactant molecules lead to product formation.

Reason: Only those collisions in which the molecules have the correct orientation and sufficient kinetic energy lead to compound formation.

• A. Both assertion and reason are incorrect.
• B. Assertion is incorrect but reason is correct.
• C. Both assertion and reason are correct and the reason is correct explanation of assertion.
• D. Assertion is correct but reason is incorrect.
• E. Both assertion and reason are correct but reason does not explain assertion.

Answer 1

The correct option is B

Assertion is incorrect but reason is correct.

Analysing the assertion:

For the formation of a compound, the molecules should have energy greater than $e^{-E_a/RT}$, and there should be a proper orientation of the collision for better energy transfer and compound formation.

So, the assertion is an incorrect statement.

Analysing the reason

Only effective collisions result in product formation i.e., collisions in which the reactant molecules collide with the proper orientation and sufficient kinetic energy to facilitate the breaking of bonds between the reacting species and forming new bonds lead to product formation.

Collision without proper orientation or sufficient kinetic energy does not lead to the formation of a compound.

Therefore, all the collisions of the reactant molecules do not lead to product formation.

So, the reason is a correct statement.

Assertion is incorrect but the reason is correct.

Hence, the correct answer is option $\left(E\right).$