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$2 \mathrm{Cu}_2 \mathrm{O}(s)+\mathrm{Cu}_2 \mathrm{~S}(s) \longrightarrow 6 \mathrm{Cu}(s)+\mathrm{SO}_2(g)$
the oxidant and reductant respectively in the above reaction are
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the oxidant and reductant respectively in the above reaction are
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$\mathrm{Cu}(\mathrm{I})$ of $\mathrm{Cu}_2 \mathrm{O}, \mathrm{Cu}_2 \mathrm{~S}$ and sulphide of $\mathrm{Cu}_2 \mathrm{~S}$
$\mathrm{Cu}(\mathrm{I})$ of $\mathrm{Cu}_2 \mathrm{O}(s)$ and $\mathrm{Cu}_2 \mathrm{~S}(s)$ undergoes reduction to form $\mathrm{Cu}(s)$ while sulphide of $\mathrm{Cu}_2 \mathrm{~S}$ undergoes oxidation to form $\mathrm{SO}_2(\mathrm{~g})$. Thus, $\mathrm{Cu}(\mathrm{I})$ of $\mathrm{Cu}_2 \mathrm{O} \cdot \mathrm{Cu}_2 \mathrm{~S}$ acts as an oxidising agent (oxidant) and sulphide of $\mathrm{Cu}_2$ Sacts as a reducing agent (reductant).
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