Hedwigeeeee
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what is the difference between redox reactions and dispropotionate reactions?
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aashan21
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Redox is when one molecule/atom is oxidised and another is reduced.
Disproportionately is when one atom is reduced and oxidised in the same reaction.
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David Getling
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(Original post by Wuxinyu)
what is the difference between redox reactions and dispropotionate reactions?
Disproportionation reactions are a form of redox reaction. The defining characteristic of a disproportionation reaction is that something in a particular oxidation state reacts in such a way that some of it ends up in a higher oxidation state and some in a lower one. Here's an example.

2H2O2 → 2H20 + O2

On the LHS all the oxygen is in the -1 state, whereas on the RHS some is in the -2 and some is in the 0 state.
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anosmianAcrimony
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(Original post by aashan21)
Redox is when one molecule/atom is oxidised and another is reduced.
Disproportionately is when one atom is reduced and oxidised in the same reaction.
Not quite. A disproportionation reaction is when the same element is reduced and oxidised in the same reaction - i.e. some atoms of it are oxidised and some reduced.
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aashan21
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(Original post by anosmianAcrimony)
Not quite. A disproportionation reaction is when the same element is reduced and oxidised in the same reaction - i.e. some atoms of it are oxidised and some reduced.
That’s what I meant. But you explained it a lot better
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