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Which of the following statements correctly describes the effect of increasing temperature on the rate constant of a chemical reaction?

medium MCQ 3 marks Class 12 · Chemistry · Chemical Kinetics
  1. A. The value of decreases because the activation energy becomes larger.
  2. B. The value of increases because more molecules possess energy equal to or greater than .
  3. C. The value of remains unchanged; only the equilibrium constant is affected.
  4. D. The value of increases, but only for reactions that are catalyzed.
Answer
B. The value of increases because more molecules possess energy equal to or greater than .

The correct answer is B. The value of increases because more molecules possess energy equal to or greater than . — Option B states exactly this; the other options contradict the Arrhenius relationship.

Step-by-step solution

  1. The Arrhenius equation shows depends exponentially on .
  2. When temperature rises, becomes smaller, making larger.
  3. Thus increases because a larger fraction of molecules have kinetic energy .
  4. Option B states exactly this; the other options contradict the Arrhenius relationship.
Common mistake: Assuming temperature changes the activation energy instead of the exponential factor.

Concept tested: Temperature effect on rate constant (Arrhenius)

Published · How this solution was prepared and checked

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