A → B The rate constants of the above reaction at 200 K and 300 K are 0 . 03 min - 1 and 0 . 05 min - 1 respectively. The activation energy for the reaction is J (Nearest integer) (Given : In 10 = 2 . 3 R = 8 . 3 J K - 1 mol - 1 log 5 = 0 . 70 log 3 = 0 . 48 log 2 = 0 . 30

Step-by-step solution

If K is known at two different temperatures the activation energy can be calculated as: At temperature 1: ln   K 1   =   - E a RT 1   +   ln   A At temperature 2: ln   K 2   =   - E a RT 2   +   ln   A We can subtract one of these equations from the other: ln   K 1   -   ln   K 2   =   - E a RT 1   +   ln   A   -   - E a RT 2   +   ln   A This equation can further simplified to: ln K 1 K