Problem 1. Question 3. What will be the form of the experimental rate law? a. rate=k[S_(2)O_(3)^2-]^n[BrO_(3)^-]^m[H^+]^p b time=k[S_(2)O_(3)^2-]^n[BrO_(3)^-]^m[H^+]^p C rate=k[S_(2)O_(3)^2-]^n[BrO_(3)^-]^n[H^+]^n d. time=k[S_(2)O_(3)^2-][BrO_(3)^-][H^+] e. rate=k[S_(2)O_(3)^2-][BrO_(3)^-][H^+] a. b. C. d e.

The correct answer is option a.The form of the experimental rate law is given by: where:- is the rate of the reaction,- is the rate constant,- , , and are the concentrations of the reactants,- , , and are the orders of the reaction with respect to each reactant.The rate law expresses the relationship between the rate of a reaction and the concentration of the reactants. It is determined experimentally and provides information about the mechanism of the reaction.