Q. 84.2( 41 Votes )
The rate of the chemical reaction doubles for an increase of 10K in absolute temperature from 298K. Calculate Ea.
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 = 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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