Chemical Kinetics Methods of Initial Rates/ Reaction Orders and Rate Laws I need

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Chemical Kinetics

Methods of Initial Rates/ Reaction Orders and Rate Laws

I need help with reaction order with respect to I-, BrO^3- and H+, I am assuming we us the rate of S2O3^2- INSTEAD OF BrO3^-

Santa Monica College Summary of Results for Use in the Method of (copy the appropriate values from the tables on the previods tho P Reaction Mixture [I1o Chemistry 12 Initial Rates: | [H+] () | Rate (M-s-1) [Br03-Jo () 10-3 | 0.02 | 2.13X 10-s 20 02 .053 x 10 2 3 4 0-02 - . 30 1 x 10- |5.43 x 10-r 2Xi03 2KIO 2 x10 8x10-3 | 001 Use the method of initial rates and the relevant data in the table above to determine the order of each reactant as given by Equation (2) and state the experimentally determined rate law below. Clearly show all your calculations, including which mixtures the data you used came from. The reaction order with respect to Reachan Me Rule o4 Bro3-] 3.55 x 1O MS q, 05 x 10 ms he reaction order with respect to BrOs The reaction order with respect to H The Rate Law

Explanation / Answer

order w.r.t I-

r1/r2 = (a1/a2)^x

(2.13*10^-5/(3.053*10^-5)) = ((2*10^-3)/(4*10^-3))^x

   x = 0.52

Order w.r.t BrO3-

r1/r3 = (a1/a3)^y

(2.13*10^-5/(4.301*10^-5)) = ((8*10^-3)/(0.016))^y

y = 1

Order w.r.t H+

r1/r4 = (a1/a4)^z

(2.13*10^-5/(5.43*10^-5)) = ((0.02)/(0.04))^z

z = 1.35

The rate law , Rate = K[I-]^0.52[BrO3-][H+]^1.35

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