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

Step-by-step solution

K = A e - E a R T e E a R T = 0.01 100 ⇒ E a R T = 2.303 log ⁡ 10 - 4 ⇒ E a = 2.303 × 4 × 400 = 30.6 k J / m o l