The rate of a reaction quadruples when the temperature changes from 300   to 310   K . The activation energy of this reaction is: (Assume Activation energy and pre-exponential factor are independent of temperature; ln ( 2 ) = 0 . 693 ; R = 8 . 314 J mol - 1 K - 1 )

Step-by-step solution

The activation energy, rate constant and temperature can be related using Arrhenius equation. k = Ae - E a RT ln k 2 k 1 = E a R   1 T 1 - 1 T 2   ln 4 = E a R   1 300 - 1 310   2 × 0 . 693 = E a R   10 300 × 310   E a   =   2 × 0.693 × 300 × 310 × 8.314 10   =   107.2   kJ/mol