I was doing some research and I came across an experiment similar to mine (potassium iodate with sodium bisulfite) from the University of Massachusetts (http://www.chem.umass.edu/genchem/chem122/122_Experiment_4.htm), but with the reaction of potassium permanganate with oxalic acid.
The rate equation is given as: Rate = k[KMnO4][H2C2O4].
It was stated that the value of k could be determined by dividing the concentration of the potassium permanganate [KMnO4] by the reaction time to find the rate and then dividing the rate by [KMnO4] multiplied by the concentration of the oxalic acid [H2C2O4] to find the reaction rate constant.
They provide the following equations:
Rate = [KMnO4]/t
k = Rate/([KMnO4][H2C2O4])
Would this be applicable to my reaction (potassium iodate with sodium bisulfite), because this would allow me to find the activation energy without performing trials to find k experimentally?