The activation energy of the reaction is 6.1 kJ/mol.
What is the Arrhenius equation?
The Arrhenius equation specifies the relationship between the activation energy and the temperature as follows;
ln(k2/k1) = Ea/R(1/T1 - 1/T2)
k1= 3.12x10^3 M^-1 s^-1
k2 = 2.70x10^4 M^-1 s^-1
T1= 275K
T2 = 300K
Hence;
ln(2.70x10^4/3.12x10^3) = Ea/8.314 ×(1/275 - 1/300)
2.2 = 0.0003Ea/8.314
Ea = 2.2 x 8.314/0.0003
Ea = 6.1 kJ/mol
Learn more about activation energy: https://brainly.com/question/11334504
