Part 2: Several experiments have been completed to solve for the rate constants for the above steps in the proposed mechanism. (Assume a single, constant temperature) Step 1: kforward 232 M-1s1; kreverse = 0.987 M¯1s-1 Step 2: k2 = 7.52e-05 M-1s-1 Step 3: k3 = 0.0633 M-1s-1- Based on the experimental rate constants and the proposed mechanism, what would be the overall rate constant for the rate law? M-1s-1 Submit Answer Tries 0/99

S2O3:2 + H3O+ = SO2 + H2O + S what is the activation energy of this reaction which has to be taken from a literature and must show reference.

Q2: Nitramide decomposes in water according to the chemical equation, kobs N₂O + H₂O 0,N-NH, The observed rate law is the following, The proposed mechanism is: O,N-NH, = 1² +11 d[N₂0] dt = kobs [0,N – NH2] [H+] O,N-NH + H* N₂O O,N-NH H* + OH H₂O Fast Is the reaction mechanism consistent with the observed rate law? If so, what is the relationship between kobs and the rate constants of the individual steps? Fast Equilibrium + он Slow

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 3+ AsO3³ + 2Ce¹+ + H₂O → AsO4³ + 2Ce³+ + 2H+ Rate = k = [ASO3³] [Ce¹+] M M 0.0311 0.0622 0.0311 0.0622 M-2.s I Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. -1 0.145 0.145 0.290 0.290 Initial Rate, M.s-1 S 0.000345 0.000690 0.00138 0.00276