How does `Cu_(2)O` acts as both oxidant and reductant ? Explain with proper reaction showing the change of oxidation number in each example

Explanation

`Cu^(+)` undergoes disproportination to form `Cu^(2+)` and Cu

Here `Cu^(2+) to Cu^(2+) therefore Cu^(+)` acts an oxidant
Again `Cu^(+) "reduces" Cu^(+) "to" Cu therefore Cu^(+)` acts as a reductant
Thus `Cu^(+) or Cu_(2)O` acts both as an oxidatn as well as a reductant
(i)`Cu_(2)O` acts in air `Cu_(2)O` is oxidised to `CuO,Cu_(2)O + 1//2 O_(2) rarr 2CuO`
(ii) When heated with `Cu_(2)S` it oxidises `S^(2-)` to `SO_(2)` and hence `Cu_(2)O` acts as an oxidant
`2 Cu_(2)O+Cu_(2) rarr 6Cu+SO_(2)`