Disproportionation
Disproportionation[edit | edit source]
Disproportionation is a chemical reaction in which a single substance is simultaneously oxidized and reduced, resulting in the formation of two different products. This reaction is often observed in redox reactions involving certain elements or compounds.
Mechanism[edit | edit source]
The mechanism of disproportionation involves the transfer of electrons from one species to another. In this reaction, the species being disproportionated acts as both the oxidizing agent and the reducing agent. The reaction proceeds through two half-reactions: one in which the species is oxidized and another in which it is reduced.
For example, consider the disproportionation of hydrogen peroxide (H2O2):
2H2O2 -> 2H2O + O2
In this reaction, hydrogen peroxide is both oxidized and reduced. One molecule of hydrogen peroxide is oxidized to form two molecules of water, while another molecule of hydrogen peroxide is reduced to form one molecule of oxygen gas.
Applications[edit | edit source]
Disproportionation reactions have various applications in different fields. One notable application is in the field of chemistry, where disproportionation reactions are used to synthesize certain compounds. For instance, the Wurtz reaction is a disproportionation reaction that is commonly used to prepare organometallic compounds.
In addition, disproportionation reactions play a crucial role in biological systems. One such example is the disproportionation of superoxide radicals (O2-) in living organisms. This reaction is catalyzed by the enzyme superoxide dismutase, which helps convert harmful superoxide radicals into less reactive species, such as hydrogen peroxide and molecular oxygen.
Examples[edit | edit source]
Apart from the hydrogen peroxide disproportionation mentioned earlier, there are several other examples of disproportionation reactions:
1. Disproportionation of chlorine gas (Cl2):
2Cl2 -> 2Cl- + ClO3-
2. Disproportionation of nitric acid (HNO3):
4HNO3 -> 2H2O + 4NO2 + O2
3. Disproportionation of sulfur dioxide (SO2):
2SO2 + O2 -> 2SO3
See Also[edit | edit source]
References[edit | edit source]
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