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I have given this question a go but not too sure on the how to find the rate for each concentration, can you please go into further detail on this. Thank you

37. Bromate ions (BrO3-) react with bromide ions (Br-) in acid solution to form bromine (Br2)

BrO3-(aq)+ 5 Br -(aq)+ 6H+(aq)→ 3 Br2(aq)+ 3H2O

(l)The concentration of BrO3 –(aq) was monitored at 298K in four separate experiments, each withdifferent initial concentrations of the reactants as shown in the following table

Experiment [BrO3] [Br] [H] initial rate (mol/Ls) 0.10 0.10 0.10 1.2 x 10-3 0.100.10 0.10 12x103 0.20 0.100.1024x103 0.10 0.3

What is the overall rate equation for this reaction and the overall order of the reaction?

A.Rate = k [BrO3-]2[Br -]2[H+]4and the overall order is 8

B. Rate = k [BrO3-][Br -][H+]2and the overall order is 4

C.Rate = k [BrO3-][Br -][H+] and the overall order is 3

D.Rate = k [H+]2and the overall order is 2E. None of these

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Answer #1

Rate = k [ Booz-]? [ 80-7% [ +1² From experiment 1. and 2. 1.2 x 10-3 = K [0-100*10.103860-107 2.4 x 10-3 = x (0-20]. [0.1077- From experiment 4. 9:6710-3. * (0-20)*[040][0.20] equation 4 - 2 9.6 x 10-3 x/[0.20]? [0.1879 [0.207² 2.4 x 16-3 .Tk [0/0]

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