Question

In a reaction carried out at 400 K, 0.01% of the total collisions are effective. What is the energy of activation of the reaction?

• A. (A) 13.3 kJ/mol
• B. (B) 23.5 kJ/mol
• C. (C) 3.2 kJ/mol
• D. (D) 30.6 kJ/mol

Answer 1

Answer: (D)

(D) 30.6 kJ/mol

Answer 2

Explanation:
In the Arrhenius equation,k=Ae−knnT'A' is the pre-exponential factor which represents the number of collisions that are favourably oriented.e−EaRT represents the fraction of molecules that possess energy equal to or greater than the threshold energy.e−E2RT=0.01100⇒−E3RT=2.303log⁡10−4⇒E3=2.303×4×8.314×400=30.6kJ/mol