Question
Explain the oxidation number method to balance the redox reaction with explain.
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$\text{O}_2,\text{O}_2^+,\text{O}^-_2$ (superoxide), $\text{O}^{2-}_2$ (peroxide)
| S. No | Column I (Reaction) | S. No | Column II (Equilibrium constant) |
| 1. | $2\text{N}_2(\text{g})+6\text{H}_2(\text{g})\rightleftharpoons4\text{NH}_3(\text{g})$ | (i) | $2\text{K}_{\text{c}}$ |
| 2. | $2\text{NH}_3(\text{g})\rightleftharpoons\text{N}_2(\text{g})+3\text{H}_2(\text{g})$ | (ii) | $\text{K}_{\text{c}}^{\frac{1}{2}}$ |
| 3. | $\frac{1}{2}\text{N}_2\text{(g)}+\frac{3}{2}(\text{g})\rightleftharpoons\text{NH}_3(\text{g})$ | (iii) | $\frac{1}{\text{K}}$ |
| 4. |
| (iv) | $\text{K}^2_{\text{c}}$ |