Potassium bromate(V) reacts with potassium bromide and sulfuric acid to form potassium sulfate, bromine and water according to the following equation. KBrO3(aq) + 5KBr(aq) + 3H2SO4(aq) → 3K2SO4(aq) + 3Br₂(aq) + 3H2O(l) A student is investigating how the rate of this reaction is affected by changing the concentration of the reactants in turn. This is done by keeping the total volume of mixture constant and adding different, small volumes of each reagent. The reaction produces bromine which is orange in colour. The student times the reaction and then determines the rate as 1/time. The rate equation for the reaction is of the form: rate = k[KBrO3]ˣ[KBr]ʸ[H₂SO₄]ᶻ k is the rate constant for the reaction and x, y and z are the respective orders of the reaction for each reagent. The student carried out the experiment and obtained the following data. Table 3.1 mixture [KBrO3] /mol dm⁻³ [KBr] /mol dm⁻³ [H2SO4] /mol dm⁻³ rate of reaction /s⁻¹ A 0.025 0.125 0.075 0.059 B 0.050 0.125 0.075 0.117 C 0.025 0.250 0.075 0.118 D 0.025 0.125 0.150 0.235 E 0.050 0.250 0.150 0.941