The given question is incomplete.The complete question is:
The presence of a catalyst provides a reaction pathway in which the activation energy of a reaction is reduced by 51.00 kJ /mol Uncatalyzed: A ⟶ B A⟶B E a = 136.00 kJ/mol Catalyzed: A ⟶ B A⟶B E a = 85.00 k J/mol. determine the factor by which tha catalysed reaction is faster than the uncatalysed reaction at 289.0 K if all other factors are equal.
Answer: The factor by which the catalysed reaction is faster than the uncatalysed reaction at 289.0 K is 
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
= activation energy without catalyst
R = gas constant = 
T = temperature = 
Now put all the given values in this formula, we get



Therefore, the factor by which the catalysed reaction is faster than the uncatalysed reaction at 289.0 K is 