Justify that the following reactions are redox reactions:

$4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} (s)$

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Solution

The oxidation number of nitrogen( $N$ ) increases from $- 3$ to $+ 2$ . The oxidation number of oxygen( $O$ ) decreases from $0$ to $- 2$ .

Ammonia is oxidized and oxygen is reduced.

Thus, it is a redox reaction.

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Justify that the following reactions are redox reactions:

(a) CuO(s) + H₂(g) → Cu(s) + H₂O(g)

(b) Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

(d) 2K(s) + F₂(g) → 2K+F– (s)

(e) 4 NH₃(g) + 5 O₂(g) → 4NO(g) + 6H₂O(g)

4 N H_{3} (g)

5 O_{2} (g)

\to

4 N O (g)

6 H_{2} O (g)

4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (g)

4 {N H}_{3 (g)} + 5 O_{2 (g)} \Leftrightarrow 4 {N O}_{(g)} + 6 H_{2} O_{(g)}

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