A certain reaction has an activation energy of 72.51 kJ/mol. At what Kelvin temperature will the reaction proceed 5.00 times faster than it did at 325 K?

Question

I can't seem to solve this one, some help would be great.

Answer 1

Use the Arrhenius equation but use it to solve for T2 

Given:  

T1 = 325K

T2 = ?? 

R = 8.3145 J/mol K 

k1 = 1 

k2= 5

Ea = 72.51kJ/mol x 1000 = 72510 J/mol  

solve for T2

T2 = 1/(1/T1) - R/Ea)(ln k2/k1)

You do the math