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Rate Law

An in-depth study of rate laws in chemical reactions, focusing on reaction rate determination and the underlying mechanisms.

Chloe Martinez
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Rate LawFor 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:ExperimentInitial[BrO3](mmol•L−1)Initial[HSO3–](mmol•L−1)Initial Rate ofFormation of Bromine(mmol•L−1•s−1)14.06.01.6022.06.00.8034.03.00.40The general equation for the rate law can be expressed as:Rate = k [BrO3]x. [HSO3⁻]yFrom the first experiment, we have:1.6 = k [4]x. [6]ySo k = 1.6 / [4]x. [6]y…………………………………………………………………………..1Similarly from experiment 2 we have:0.8 = k [2]x. [6]ySo k = 0.8 / [2]x. [6]y…………………………………………………………………………..2Comparing eq 1 and 2:1.6/ 0.8 = [4]x/ [2]x=> 2 = [2]x=>x = 1………………………………………………………………………………………3Also from experiment 3 we have:

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Chemistry

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