Question
Explain the oxidation number method to balance the redox reaction with explain.
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$\text{N}_2(\text{g})+3\text{H}_2(\text{g})\rightleftharpoons2\text{NH}_3(\text{g}),$
The value of Kp is 3.6 × 10-2 at 500K.
Colculate the value of Kc for the reaction at the same temperature R = 0.083L bar K-1mol-1.
$\text{PCl}_5(\text{g})\rightleftharpoons\text{PCl}_3(\text{g})+\text{Cl}_2\text{(g)}$
$\text{N}_2(\text{g})+\text{O}_2(\text{g})\rightleftharpoons2\text{NO(g)}$
| Prefix | Multiples | |
| (i) | micro | 106 |
| (ii) | deca | 109 |
| (iii) | mega | 10-6 |
| (iv) | giga | 10-15 |
| (v) | femto | 10 |
| Elements | | $\Delta\text{H}_1$ | $\Delta\text{H}_2$ | $\Delta_{\text{eg}}\text{H}$ | |
| i. | Most reactive non metal | A. | 419 | 3051 | -48 |
| ii. | Most reactive metal | B. | 1681 | 3374 | -328 |
| iii. | Least reactive element | C. | 738 | 1451 | -40 |
| iv. | Metal forming binary halide | D. | 2372 | 5251 | +8 |