[xc630]

Hello,

I would appreciate if anyone could explain the following problem:

The activation energy of an uncatalyzed reaction is 95 kj/mol.  The addition of a catalyst lowers the Ea to 55 kj/mol.  Assuming the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25 degrees celsius and b) 125 degrees celsius.

The answer is a) the catalyzed rxn is 10,000,000 times faster at 25 degrees C and b)  the catalyzed rxn is 180,000 times faster at 125 degrees C.

I tried using the Arrhenius equation to compare but did not get anything close to the answers.

[enahs]

Can you show how you are doing it? As when I solve it using the Arrhenius equation I get the same general answers.

Make sure you are converting kJ to J.

[xc630]

I guess I'm confused on what I'm supposed to plug in and compare.

The Arrhenius equation is k= Ae^(-Ea/RT) 

I'm supposed to compare the rates but isn't k the rate constant?  Also, if I am to use this formula what would be the temperature for the uncatalyzed reaction? 

[xc630]

Never mind I got it. thanks