How a reaction progresses over time is an indication of its reaction order. For a reaction,

$A+B$longrightarrow Products

the differential rate law is Rate $=k[A{]}^m[B{]}^n$ where $m$ and $n$ are the order of the reaction with respect to each reactant, and $k$ is rate constant. Knowing the order of the reaction with respect to each reactant allows you to predict how much the rate would change if the initial concentrations of the reactants were changed. The method of initial rates can be used to experimentally determine the order of reaction and subsequently the rate constant $k$ can be calculated.

A student carried out an experiment using the method of initial rates to determine the order of the reaction

$I{O}_3^{+}+3HS{O}_3^{+}$longrightarrow Products

and collected the following data

$\backslash$table$[[$Run$,\backslash$table$[[I{O}_3^2$