Redox and redox equilibria
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What is a reproportionation / disproportionation reaction?
Ulex says ...
A disproportionation reaction is a redox reaction in which the same element both increases and decreases in oxidation number. An example of this is the reaction between chlorine and cold sodium hydroxide solution:
Cl2 + 2NaOH -> NaCl + NaClO + H2O
The chlorine is initially in oxidation number 0. It changes to –1 in NaCl and to +1 in NaClO. No other element changes in oxidation number in this reaction.
The word ‘reproportionation’ is not an officially recognised description but I have heard it used to refer to the opposite of a disproportionation, i.e. where the same element in two oxidation states becomes part of a single species. An example would be the reaction between copper and copper(II) chloride to give copper(I) chloride:
Cu + CuCl2 -> 2CuCl
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updated: 07 January 2004
