Kinetics of the Decomposition of Hydrogen Peroxide slow fast Hydrogen peroxide decomposes to form molecular iodine and water according to the following oxidation-reduction reaction: H2O2 +2 1 + 2 H+ 12 + 2 H20 This reaction can be carried out under catalysis or not. For the uncatalyzed reaction, a suitable mechanism would be: H2O2+1 HOI + OH kunca HI+I" 12 + OH 2 OH + 2H 2 H2O 2 H+H,02 +21 12 + 2H20 For the catalyzed reaction, a suitable mechanism would be: Mo0,2 + H2O2 Moog 2 + H20 large K Mo0,2 +1 Alle 10 + M0042 fast - a fast slow fast HOI 10+H' HOI+I fast fast 12 + OH HO OH + H 2H+ +H2O2 + 21 1. + 2H2O Goal The goal of this experiment is to determine (1) the order of the reaction a with respect to H2O2, the order of the reaction b with respect to I and the rate constant kuncat of the uncatalyzed reaction at room temperature; (2) the order of the reaction x with respect to Mo04% for the catalyzed reaction at room temperature; and (3) the activation energies for both the uncatalyzed and catalyzed pathways. Available Materials and Equipment Buffer-starch Na2S2O3 stock solution (pH 4.5)* 0.060 M KI solution 0.040 M H2O2 solution 1.0 x 10' M NazMo04 solution Ice bath * The buffer-starch Na S2O3 stock solution is made by combining 25 ml of 0.01 M Na S203, 25 ml of buffer (1 M HC,H,O2 and 1 M NaC H302), 25 ml of a 2% starch solution and 175 ml of deionised water uncal 7. The entire rate law for the catalyzed reaction is the following: rate = rate +kw Moo:][-] 6 What calculations or graphical analysis are required to determine x? Which parameters do you need to keep constant? To vary? 8. Do you need to do another experiment to determine the activation energies for the uncatalyzed and catalyzed pathways