What is the rate law for the reaction?

Question

The following set of data was obtained by the method of initial rates for the reaction: 

S2O82-(aq) + 3 I-(aq) → 2 SO42-(aq) + I3-(aq)

Answer 1

The rate law can be determined if there is experimental data to work with, such as what happens to the rate if one of the reactants' concentration doubles, or what happens when the concentration of the other reactant quadruples? The rate law consists of the following: RATE = [A]^a * [B]^b where 'a' and 'b' are the exponents to which the concentrations of 'A' and 'B' are held respectively. These values are heavily dependent on the experimental data I just mentioned. For example; if doubling the concentration of 'A' quadruples the overall rate, then the value of 'a' is 2. If the overall rate goes up five times after doubling the concentration then the value of 'a' is sqrt(5). (for quick math, 'a' and 'b' in this case are the Nth root of the change in rate, where N is how much the concentration of 'A' or 'B' are changed respectively. Such as, when doubling the concentration, N=2). This only works this way because of the way this specific equation is set up. Sorry if this was a little confusing!