The activation energy for a reaction is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a catalyst. If the uncatalyzed reaction takes about 3900 years to occur, about how long will the catalyzed reaction take?

The catalyzed reaction will take time of .

Explanation:

According to the Arrhenius equation,

The expression used with catalyst and without catalyst is,

where,

= rate of reaction with catalyst

= rate of reaction without catalyst

= activation energy with catalyst  = 59.0 kJ/mol = 59000 J/mol

= activation energy without catalyst  = 184 kJ/mol = 184000 J/mol

R = gas constant

T = temperature =

Now put all the given values in this formula, we get:

The reaction enhances by  when catalyst is present.

Time taken by reaction without catalyzed = 3900 years

Time taken by reaction with catalyzed = x

The catalyzed reaction will take time of .

dynamic equilibrium is the answer.