Consider the kinetic data given in the table below for the first order reaction:
What is the value of the activation energy?
A_2_--> 2A
Expt. Initial [A2] Temp. Initial Rate
mol/L (°C) [A2]·s–1
1 0.10 100 1.2 x 10–3
2 0.20 200 4.8 x 10–3
3 0.15 ? 4.5 x 10–3
2 answers
Can't you simply plug in k1 and k2 along with T1 and T2 and solve for activation energy with the Arrhenius equation?
I have calculated K1 and K2 by dividing initial rate to initial concentration [A2], and I solved for Ea but for some reason I don't get the right answer, (which is 10.2KJ)
1 answer