[serah1206]

The question is to calculate the activation energy. I'm given this table

Expt      Temp      Time (s)    [A]       [ B ]         [C]          [D]
1            25         0          0.250     0.500           0             0
                         1.0         0.238    0.482      0.0060     0.0240
2           25          0          0.350    0.500          0             0
                         1.0        0.333     0.475      0.0085     0.0340
3           77          0          0.350     0.250         0             0
                         1.0        0.334     0.226      0.0080     0.0320
4           77          0         0.300     0.200          0             0
                         1.0        0.289     0.183      0.0055.    0.0220

I've determined the reaction rate is Rate = k [A]² [ B ]³
I know I need to use the Arrhenius equation to find the activation energy, but I am confused as to what values to use to find my rate constant and what rates I should be using.

[mjc123]

I've determined the reaction rate is Rate = k [A]2 [ B ]3

How did you determine that? (Hint: it's wrong.)
Have you actually determined the stoichiometry of the reaction?
2A + 3B  C + 4D
The order of a reaction is not necessarily related to the stoichiometry. A very important principle of kinetics.
How do you determine the order of the reaction with respect to a reagent?