I am an organic chemist none of this shit makes sense to me.

Calculate the activation energy (in kJ mol-1) for a reaction where the rate constant at 301.0 K is tripled when the temperature is raised by 10.0 K.

I guess I am stumbling on how to go about solving this as the temperature is not given so if i tried to do a regular arrhenius equation I would have two variables (Eact and T)

It does not make sense to me that activation energy would be independent of temperature so I am wondering if I can somehow manipulate the equation to where the temperatures cancel out?

ty for help I can get fg to pay you if needed.

Plz don't just give answer I would rather solve myself just looking for tips

The temperatures are given, the actual rate constant is not but you can set it to some value or just call it x.

original: temperature = 301, k = x
raised by 10: temperature = 311, k = 3x

also, im pretty sure for this you can assume activation energy is considered temperature independent.

so then you should be able to use just the arrhenius

This post was edited by cialda on Mar 20 2014 04:45pm

ohhhhh SHIT i got confused with the rate constant being K and the kelvin wow thanks