The reaction between potassium bromate KBrO3 and potassium bromide KBr is as follows:3Br aq + BrO aq + 6H aq 3HO l + 2Br aq To determine the reaction order with respect to bromide ions Br , we need to analyze the rate law for this reaction. The rate law is an expression that shows the relationship between the rate of the reaction and the concentrations of the reactants. It has the general form:Rate = k[A]^m[B]^nwhere Rate is the reaction rate, k is the rate constant, [A] and [B] are the concentrations of the reactants, and m and n are the reaction orders with respect to A and B, respectively.For the reaction between potassium bromate and potassium bromide, the rate law can be written as:Rate = k[Br]^m[BrO]^nTo find the reaction order m with respect to bromide ions, we need to perform experiments and analyze the data. Typically, this involves measuring the reaction rate at different initial concentrations of bromide ions while keeping the concentration of bromate ions constant.If the reaction rate doubles when the initial concentration of bromide ions doubles, then the reaction is first-order with respect to bromide ions m = 1 . If the reaction rate quadruples when the initial concentration of bromide ions doubles, then the reaction is second-order with respect to bromide ions m = 2 , and so on.Once the reaction order with respect to bromide ions is determined, we can understand how changing the initial concentration of bromide ions affects the reaction rate. If the reaction is first-order with respect to bromide ions, then doubling the initial concentration of bromide ions will double the reaction rate. If the reaction is second-order with respect to bromide ions, then doubling the initial concentration of bromide ions will quadruple the reaction rate, and so on.