Bromide ion is oxidized by bromate ion in acidic solution. 5Br-(aq) + BrO3-(aq) + 6H+(aq) = 3Br2(aq) + 3H2O(l) The experimentally determined rate law is Rate = k[Br-][BrO3-][H+]2 a) What is the order of reaction with respect to each reactant species? b) What is the overall order of the reaction? c) If the concentration of BrO3- was tripled, while Br- and H+ remained constant, what would happen to the rate of reaction?

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