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.<br /><br />The form of the experimental rate law is given by:<br /><br />$rate = k[S_{2}O_{3}^{2-}]^{n}[BrO_{3}^{-}]^{m}[H^{+}]^{p}$<br /><br />where:<br />- $rate$ is the rate of the reaction,<br />- $k$ is the rate constant,<br />- $[S_{2}O_{3}^{2-}]$, $[BrO_{3}^{-}]$, and $[H^{+}]$ are the concentrations of the reactants,<br />- $n$, $m$, and $p$ are the orders of the reaction with respect to each reactant.<br /><br />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.