+ 5 Br (aq) 0.00200M 1. Consider this reaction and the experimental quantities given in the table. BrO3 (aq) + 6 H+ (aq) 3 Br, 2 (aq) + 3 HO (1) Run 0.00200M 0.0200M HO Total KBr No. KBrO, (mL) HCl (mL) (mL) volume (mL) Initial Rate= A[Br] At (M/s) (mL) 1 10.0 10.0 10.0 70.0 100.0 1.44 X 10-12 2 20.0 10.0 10.0 60.0 100.0 2.88 X 10-12 3 10.0 20.0 10.0 60.0 100.0 2.88 X 10-12 to hol 4 10.0 10.0 20.0 60.0 100.0 5.76 X 10-12 a. Calculate the molarities in each of the reaction mixtures. Run No. KBr KBrO3 M HCl 1 0.0002 0.0002 0.002 2 0.0004 0.0002 0.0002 3 0.0002 0.0004 .002 0.0004.002 4 .0002 .0002 .004 b. Determine the order of each reactant. (Show work below.) order of [Br] order of [BrO3] order of [H+] C. Determine the value of the rate constant (including units) for the formation of Br. d. Write the complete rate law expression for the formation of Br.. e. What would be the initial rate of formation of Br, (in units of M/s) when the following initial concentrations were used? [Br] =3.00 x 10-2 M; [BrO,] = 8.00 x 10-2 M; [H+] = 2.00 x 10-2 M f. Under the conditions specified in part "e" (directly above), what would be the initial rate of disappearance of hydrogen ion (in units of M/s) for this reaction?