The rate of the chemical reaction doubles for an increase of 10K in absolute temperature from 298K. Calculate Ea.


Given-


Initial temperature, T1 = 298 K


Final temperature, T2 = 298 K + 10 K = 308 K


Knowing that the rate constant of a chemical reaction normally increases with increase in temperature, we assume that,


Initial value of rate constant, k1 = k


Final value of rate constant, k2 = 2k


Using Arrhenius equation,


Equation 1


where, R = 8.314 J K-1 mol-1 (gas constant).


Substituting all the values in equation 1, we get,



log 2 =


Ea =


Ea =


Ea = 52897 J mol-1


Ea = 52.897 kJ mol-1


The energy of activation, Ea is 52.897 kJ mol-1


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