There is actually one method depending of the order of the reaction.
We will work with the reaction aA —> bB
We’ll start with the order 0:
rate=k[A]^0[B]^0=k=(1/a)(d[A]/dt)
d[A]=kadt
You integrate.
[A](t)-[A](0)=kat
Then you can access to k.
You do the same for an order 1 and 2 reaction.
The difference will be that you will have k[A]=(1/a)(d[A]/dt) and
k[A]^2=(1/a)(d[A]/dt)
You can also work with the Arrhenius law, it can be another method actually:
K(T)=Aexp((-Ea)/RT)
I hope I helped you :)
Alexis
