Question

Assertion (A): Rate of reaction decreases with increase in temperature. Reason (R): Number of effective collisions increases with increase in temperature.

• A. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
• B. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
• C. Assertion (A) is true, but Reason (R) is false.
• D. Assertion (A) is false, but Reason (R) is true.

Hint:

Reaction rates usually increase with temperature due to an increase in the number of molecules with energy greater than the activation energy.

Answer 1

The Correct Option is D

Increasing temperature generally increases the rate of reaction because more molecules gain sufficient energy to overcome the activation barrier. The assertion is incorrect, but the reason is correct. \[ \text{Rate} \propto e^{-\frac{E_a}{RT}} \] where \( E_a \) is the activation energy, \( R \) is the gas constant, and \( T \) is temperature. A higher \( T \) leads to a higher reaction rate.