Justify that the reaction : `2Cu_(2)O(s)+Cu_(2)(s)rarr6Cu(s)+SO_(2)(g)`
is a redox rection identify the species oxidised / reduced which acts as an oxidant and which acts as a reductant

Explanation

Writing the oxidation number of each atom its symbol we have
`2Cu_(2)O(s)Cu_(2)rarr6Cu(s)+SO_(2)(g)`
here in this reaction the oxidatio number of copper decrease from +1 in `Cu_(2)S` to 0 in copper metal therefore `Cu^(+)` is reduced further the oxidation number of S increase from - 2 in `Cu_(2)S` to +4 in `SO_(2)` therefore `S^(2-)` is oxidised thus the above reaction is a redox reaction further oxygen in `Cu_(2)O` helps suphur in `Cu_(2)O` to increase its oxidation number from -2 to +4 therefore `Cu_(2)O` is an oxidant conversely suphur in `Cu_(2)` helps coper both in `Cu_(2)O` and `Cu_(2)S` to decrease its oxidation number from +1 to zero in copper metal therefore `Cu_(2)S` is the reductant