**Question:** Which of the following statements are correct for the reaction:

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)?

(a) Nitrogen gets oxidized. (b) Oxygen gets oxidized. (c) Nitrogen gets reduced. (d) Oxygen gets reduced.

Question

**Question:** Which of the following statements are correct for the reaction:

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)?

(a) Nitrogen gets oxidized. (b) Oxygen gets oxidized. (c) Nitrogen gets reduced. (d) Oxygen gets reduced.

Accepted Answer

Step 1 — Balanced reaction:

The reaction is $4\mathrm{NH}_3 + 5\mathrm{O}_2 	o 4\mathrm{NO} + 6\mathrm{H}_2\mathrm{O}$.

Step 2 — Assign oxidation states:

- In $\mathrm{NH}_3$: H is $+1$, so N is $-3$.
- In $\mathrm{O}_2$: O is $0$ (elemental form).
- In $\mathrm{NO}$: O is typically $-2$, so N is $+2$ (since $+2 + (-2)=0$).
- In $\mathrm{H}_2\mathrm{O}$: O is $-2$.

Step 3 — Determine changes:

- Nitrogen: $-3 	o +2$ (increase in oxidation number) ⇒ N is oxidized ⇒ statement (a) is true, (c) is false.
- Oxygen: $0 	o -2$ (decrease in oxidation number) ⇒ O is reduced ⇒ statement (d) is true, (b) is false.

Therefore the true statements are (a) and (d), which corresponds to choice (1).

FINAL_ANSWER: a

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