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Abstract
The reactions in sulphuric acid solutions between the tri-iodine cation and deactivated aromatic compounds follow second-order kinetics, first-order in each reagent. The rate of iodination varies with the concentration of water in the solvent and there is a moderately large kinetic isotope effect. The results are consistent with the occurrence of a two-stage reaction in which the loss of the proton is catalysed by the hydrogen sulphate ion.
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Schedule a callMore From: Journal of the Chemical Society B: Physical Organic
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