The mechanism proposed for the oxidation of iodide ion, I, by the hypochlorite ion, CIO, in aqueous solution is shown. 1. CIO (aq) + H₂O(1) =HCIO(aq) + OH¯(aq) fast in both directions 2. I¯(aq) + HCIO(aq) HIO(aq) + Cl(aq) slow 3. HIO(aq) + OH(aq) - IO (aq) + H₂O(1) fast Complete the rate law for the formation of IO implied by this mechanism. rate = k [CI] Answer Bank [HCIO] [CIO] [-]
The mechanism proposed for the oxidation of iodide ion, I, by the hypochlorite ion, CIO, in aqueous solution is shown. 1. CIO (aq) + H₂O(1) =HCIO(aq) + OH¯(aq) fast in both directions 2. I¯(aq) + HCIO(aq) HIO(aq) + Cl(aq) slow 3. HIO(aq) + OH(aq) - IO (aq) + H₂O(1) fast Complete the rate law for the formation of IO implied by this mechanism. rate = k [CI] Answer Bank [HCIO] [CIO] [-]
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 31E: The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what...
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