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

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 =

E_a =

E_a =

E_a = 52897 J mol^-1

E_a = 52.897 kJ mol^-1

The energy of activation, E_a is 52.897 kJ mol^-1