The activation energy for a reaction is 84.0kJ/mol. Addition of a catalyst lowers the activation energy by 23.0 kJ/mol, while leaving the A-factor unchanged. By what factor ( uncatalyzed catalyzed k k ) does the rate increase at 25 °C?

Answer : The rate constant of the reaction is increased by factor,

Solution :

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  = 23.0 kJ/mol = 23000 J/mol

= activation energy without catalyst  = 84.0 kJ/mol = 84000 J/mol

R = gas constant = 8.314 J/mol.K

T = temperature =

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

Therefore, the rate constant of the reaction is increased by factor,

is there multiple choice answers?