Question

In the reaction n2(g) + 2O₂(g) → 2nO₂(g), which species is/are oxidized and which species is/are reduced?

1) N₂ is oxidized and O₂ is reduced
2) O₂ is oxidized and N₂ is reduced
3) NO₂ is oxidized and N₂ is reduced
4) N₂ is oxidized and NO₂ is reduced

Answer 1

In the reaction N2(g) + 2O2(g) → 2NO2(g), N2 is oxidized as its oxidation state increases from 0 to +4. Oxygen remains with an oxidation number of 0, so it is neither oxidized nor reduced.

Step-by-step explanation:

In the reaction N2(g) + 2O2(g) → 2NO2(g), to identify what species is oxidized and which is reduced, we need to assign oxidation numbers to each atom in the reaction. Nitrogen in N2 is initially at an oxidation state of 0, and in NO2, it has an oxidation state of +4. Oxygen in O2 is initially at an oxidation state of 0, and in NO2, it has an oxidation state of -2.

Since nitrogen's oxidation number increases from 0 to +4, N2 is being oxidized. On the other hand, oxygen's oxidation number does not change as it remains at 0 in both O2 and NO2, so it is neither oxidized nor reduced. Therefore, the correct answer is that N2 is oxidized while O2 is not involved in the redox process in this reaction.