Information AboutDisproportionation |
| CATEGORIES ABOUT DISPROPORTIONATION | |
| chemical reactions | |
| chemical processes | |
| organic reactions | |
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Disproportionation is a type of reaction in Redox Chemistry in which a Reactant is both oxidised and reduced in the same chemical reaction forming 2 separate compounds. Examples:
The ionic equation for this reaction is as follows: Cl2 + 6OH− → Cl− + ClO3− + 3H2O In the above equation, the initial oxidation number of chlorine is 0. In the products, Cl− has an oxidation number of −1, having been reduced, whereas the oxidation number of chlorine in the Chlorate ion is +5, indicating that it has been oxidised. It should be noted that there is no change of oxidation state for the sodium hydroxide.
2C4H4 → C6H6 + C2H2
Disproportionation is the opposite of Synproportionation . |
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