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Two reactions A 1 and A 2 have identical pre-exponential factors. The activation energy of A 1 is more than A 2 by 10 kJ mol - 1 . If k 1 and k 2 are the rate constants for reactions A 1 and A 2 , respectively at 300 K , then ln ⁡ k 2 k 1 is equal to R = 8 .314 J mol - 1 K - 1

Options

  1. A12
  2. B6
  3. C4
  4. D8

Correct answer

C. 4

Step-by-step solution

From Arrhenius equation k = Ae - Ea / RT k 1 = Ae - Ea 1 / RT k 2 = Ae - Ea 2 / RT ln k 2 k 1 = e Ea 1 - Ea 2 / RT ln ⁡ k 2 k 1 = Ea 1 - Ea 2 RT = 10 × 1000 8 .314 × 300 = 4

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