At 35C, the rate constant for the reaction: C12H22O11 + H20 --> C6H12O6 + C6H12O6 is k=6.2 x 10^-5 s-1. The activation energy for the reaction is 108 kJ/mol. What is the rate constant for the reaction at 45C? Determine the impact on the rate.
The Attempt at a Solution
I don't know if I am even using the right equation, (Arrhenius equation) however I tried seperating the reaction into 35C and 45C stages and analyzed from there. At 35C, Ae is given so I plugged the Ae into the Arrhenius eq at 45C and cancel out the A base as it is the same at both 35C and 45C.
Ended up with :
r=e^(-108000/8.314*10). (change in temp of 10C)
Does this make any sense or even work? If so, what does the second part of impact on the rate mean?
Thanks a bunch.