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Equilibration of Redox Reactions

A vanadate ion can react with itself through the redox reaction [Pg.201]

The reaction evolving from left to right is called a disproportionation reaction and that evolving from right to left a retrodisproportionation reaction or an amphoter-ization reaction. They are particular cases of redox reactions, and all the general considerations developed so far can be applied to them. Another example of a disproportionation reaction is provided by the reaction of dichlorine with water in the interval 3.3 pH 7.5. Hypochlorous acid (HCIO) and chloride ions (Cl ) are formed  [Pg.201]

The oxidation numbers of oxygen and hydrogen do not change in the course of this reaction, whereas that of chlorine has changed from 0 to simultaneously -I and +1. The two involved half-redox couples are [Pg.201]

One example of retrodisproportionation is provided by the element iodine in the iodate/iodide reaction  [Pg.201]

The oxidation numbers of oxygen and hydrogen have not changed in the course of the reaction. However, that of iodine has changed. It went from +V (iodate ion) and -I (iodide ion) to 0 (iodine). The two redox couples are [Pg.201]


The equilibration of redox reactions can be done in several steps. Let s consider the oxidation reaction of iodide ions by dichromate ions. It must be written as... [Pg.201]


See other pages where Equilibration of Redox Reactions is mentioned: [Pg.201]    [Pg.201]    [Pg.204]   


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Equilibrator

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