Question

Determine the oxidation numbers of each of the elements in the following reaction, and identify which of them, if any, are oxidized or reduced.

3NO₂(g) H₂O--->2H (aq) 2NO₃⁻(aq) NO(g)

Answer 1

In the given reaction, 3NO₂(g) + H₂O → 2H⁺ (aq) + 2NO₃⁻(aq) + NO(g), the oxidation numbers of each element can be determined. Nitrogen (N) is being oxidized from +2 to +4, while hydrogen (H) is being reduced from +1 to 0.

Step-by-step explanation:

In the given reaction, 3NO₂(g) + H₂O → 2H⁺ (aq) + 2NO₃⁻(aq) + NO(g), we can determine the oxidation numbers of each element to identify which ones are being oxidized and reduced.

1. The oxidation number of oxygen (O) is -2, so in NO₂, the total oxidation number of oxygen is -4. Since there are two oxygen atoms, the oxidation number of nitrogen (N) in NO₂ is +4.
2. In H₂O, the oxidation number of hydrogen (H) is +1 and the oxidation number of oxygen (O) is -2.
3. In H⁺ (aq), the oxidation number of hydrogen (H) is +1.
4. In NO₃⁻(aq), the total oxidation number of oxygen is -6, so the oxidation number of nitrogen (N) is +5.
5. In NO(g), the oxidation number of oxygen (O) is -2, so the oxidation number of nitrogen (N) is +2.

From the above, we can see that in this reaction, nitrogen (N) is being oxidized from +2 to +4 and hydrogen (H) is being reduced from +1 to 0. Therefore, nitrogen is oxidized and hydrogen is reduced.