Consider the following redox reaction: 2Cu₂O (s) + Cu₂S (s) → 6Cu (s) + SO₂ (g) Identify the species among the following acting as oxidant and reductant, respectively:

In the redox reaction 2Cu₂O + Cu₂S → 6Cu + SO₂, the oxidation states of the elements change significantly. In both Cu₂O and Cu₂S, copper (Cu) exists in the +1 oxidation state. In the product side, copper is in its elemental form with an oxidation state of 0. Since the oxidation number of Cu(I) decreases from +1 to 0, it undergoes reduction and acts as the oxidant (oxidizing agent). Conversely, the sulfur (S) in Cu₂S has an oxidation state of -2, which increases to +4 in the product SO₂. This increase in oxidation number indicates that sulfur undergoes oxidation, thereby acting as the reductant (reducing agent). Thus, Cu(I) is the oxidant and the sulfur of Cu₂S is the reductant, making option 1 the correct identification of the species involved.