Two reactions A 1 and A 2 have identical pre-exponential factors. The activation energy of A 1 is more than…

Two reactions A1 and A2 have identical pre-exponential factors. The activation energy of A1 is more than A2 by 10 kJ mol-1 . If k1 and k2 are the rate constants for reactions A1 and A2, respectively at 300 K, then ln⁡k2k1 is equal to

R=8.314 J mol-1K-1
  1. 12
  2. 6
  3. 4
  4. 8

Solution

From Arrhenius equation

k=Ae-Ea/RT

k1=Ae-Ea1/RT

k2=Ae-Ea2/RT

lnk2k1=eEa1-Ea2/RT

ln⁡k2k1=Ea1-Ea2RT=10×10008.314×300=4

Asked in: JEE Main 2017 (02 Apr)

Practice more Chemical Kinetics questions on Aicharya