1.

A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are k1, k2, k3 and k5 respectively. The overall rate constant is is given by: k = k_(2)/k_(1) (k_(1)/k_(2))^(1/2) activation energy are 40,60, 50 and 10 kJ/mol respectively, find the overall energy of activation (kJ/mol).

Answer»


SOLUTION :`k = A.e^(-E_(a)//(RT))`
`therefore` Effective overall energy of activation
`E_(a) = E_(a)(2) -E_(a)(3) + 1/2 E_(a)(1) -1/2 E_(a)(5)`
`=60-50 + 1/2 xx 40 - 1/2 xx 10 = 25` kJ/mol


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