Question

The rate constants of a reaction at 200 K and 500 K are 0.02 s^–1 and 0.20 s^–1 respectively. Calculate the value of Ea (Given 2.303 R = 19.15 JK^-1 mol^-1).

Answer 1

`log ("k"_2/"k"_1) = "Ea"/(2.303 " R") [1/"T"_1 - 1/"T"_2]`

`log 0.20/0.05 = "Ea"/(2.303 " R") [1/200 - 1/500]`

log 10 = `"Ea"/19.15 (300/(200 xx 600))`

Ea = `(19.15 xx 200 xx 500)/300`

Ea = 6383 J/mol