What is a disproportionation reaction?
Generally in redox chemical reactions one entity is oxidized and other is reduced. In a disproportionation reaction one entity under goes both oxidation as well as reduction and two different products are formed.
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A disproportionation reaction is when a multiatomic species whose pertinent element has a specific oxidation state gets oxidized and reduced in two separate half-reactions, yielding two other products containing the same pertinent element.
EXAMPLE: MANGANESE OXIDES
A convenient example is
From this Pourbaix diagram:
...we see that
In a Pourbaix diagram, this indicates a disproportionation reaction (which, by the way, is spontaneous below pH 4).
(Hence, You could also see it in a Frost diagram, albeit it's a bit harder to identify unless you remember how it works.
In this case, the disproportionation occurs from a "hill" point to the immediate left and right points (e.g. THE HALF-REACTIONS We can write the half-reactions like so. Reduction: This is a reduction from Add water to balance the oxygens. Add protons (since we are in acidic pH) to balance the hydrogens. Now adding the electrons balances the charge. Oxidation: This is an oxidation from Add water to balance the oxygens... and protons to balance the hydrogens... and electrons to balance the charge. Overall reaction: And the final result would be: Finally, cancel out the common multiples.
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A disproportionation reaction is a redox reaction in which one species undergoes BOTH oxidation and reduction.
Which is balanced with respect to mass and charge, as is always required. Clearly zerovalent chlorine gas has undergone reduction to chloride ion, and oxidation to chlorate ion; i.e. a disproportionation reaction.
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It is when a species reacts to simultaneously produce one oxidized and one reduced species.
For instance, consider the following Pourbaix diagram of manganese:
This diagram graphs the species present in aqueous solution at various A disproportionation reaction could occur starting from The skeletal half-reactions are (with only manganese oxidation states labeled): You can see that the same species got oxidized and reduced at the same time. As the reaction is at The resultant two balanced half-reactions are: So, we add them to get: Finally, we are in basic solution, so we add As a result, we cancel out some of the waters to get:
(reduction)
(oxidation)
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A reaction in which the same species is both oxidised and reduced.
A great example is chlorine mixing with water.
Therefore chlorine has been both oxidised and reduced in the same reaction. This is disproportionation.
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A disproportionation reaction is a chemical reaction in which a single substance is both oxidized and reduced, resulting in the formation of two different products with different oxidation states.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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- How does oxygen react with hydrogen?
- How does #"silver nitrate"# react with #"sodium oxalate"# in aqueous solution?
- How do compounds differ from their component elements?

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