[anger3]

For a parallel reaction A goes to B with rate constant k1 and A goes to C with rate constant k2, you determine that the activation energies are 45,052 for k1 and 69,372 for k2 in J.mol-1. If the rate constants are equal at a temperature of 322 K, at what temperature will k1/k2 =2?

I have tried using the equation [A]=[Ao] - kt to equate the rate constants at 322K to solve for the temperature when k1/k2 =2, but it's making no sense because there are 2 unknowns (A and k). So confused, if someone could shed some light on this that would be amazing.

Thank you!

[Schrödinger]

Hint :
Use the Arrhenius equation in order to solve this question.

k=Ae^(E/RT)

where k = rate constant
A = Arrhenius parameter (not the concentration of reactant A)
E = Activation energy in Jmol^-1
R = Gas constant in Jmol^-1K^-1
T = Temperature in K

[catgreat]

ln k1/k2= ln A-ΔE/R（1/T1-1/T2）