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The rate constant of a reaction is 6 × 10-3 s-1 at 50° and 9 × 10-3 s-1 at 100° C. Calculate the energy of activation of the reaction.

The rate constant of a reaction is 6 × 10-3 s-1 at 50° and 9 × 10-3 s-1 at 100° C. Calculate the energy of activation of the reaction. Correct Answer 8.124 kJ mol-1

Given, k1=6 × 10-3s-1 T1=50 + 273=323 K k2=9 × 10-3s-1 T2=100 + 273=373 K Substituting these values in the equatiolog (k2 / k1 ) = (Ea / 2.303 R) × ((T2 – T1) / T1 T2), we get log (9 × 10-3 s-1 / 6 × 10-3 s-1 ) = ((Ea / (2.303 × 8.314)) × ((373 – 323) / (373 × 323)) log 9 / 6 = ((Ea / (2.303 × 8.314)) × (50 / (373 × 323)) Ea = 8.124 kJ mol-1.

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