Rate Law

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Rate Law For the following reaction, use the experimental data to determine the rate law. 2 BrO3 – (aq) + 5 HSO3 – (aq) → Br2(g) + 5 SO42 – (aq) + H2O(l) + 3 H+(aq) Solution: Experiment Initial [BrO 3 ] (mmol•L −1 ) Initial [HSO 3 – ] (mmol•L −1 ) Initial Rate of Formation of Bromine (mmol•L −1 •s −1 ) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 The general equation for the rate law can be expressed as: Rate = k [BrO 3 ] x . [HSO 3 ⁻ ] y From the first experiment, we have: 1.6 = k [4] x . [6] y So k = 1.6 / [4] x . [6] y …………………………………………………………………………..1 Similarly from experiment 2 we have: 0.8 = k [2] x . [6] y So k = 0.8 / [2] x . [6] y …………………………………………………………………………..2 Comparing eq 1 and 2: 1.6/ 0.8 = [4] x / [2] x => 2 = [2] x => x = 1 ………………………………………………………………………………………3 Also from experiment 3 we have:
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