Question
Explain relationship between $E _{\text {cell }}^{\circ}$ and equilibrium constant with the help of Nernst equation.
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| Column I | Column II | ||
| (i) | Mathematical expression for rate of reaction. | (a) | Rate constant. |
| (ii) | Rate of reaction for zero order reaction is equal to. | (b) | Rate law. |
| (iii) | Units of rate constant for zero order reaction is same as that of. | (c) | Oder of slowest step. |
| (iv) | Order of a complex reaction is determined by. | (d) | Rate of a reaction. |
| Column I | | Column II | |
| i. | F2 | a. | Metal is the strongest reducing agent. |
| ii. | Li | b. | Metal ion which is the weakest oxidising agent. |
| iii. | Au3+ | c. | Non metal which is the best oxidising agent. |
| iv. | Br- | d. | Unreactive metal. |
| v. | Au | e. | Anion that can be oxidised by Au3+ |
| vi. | Li+ | f. | Anion which is the weakest reducing agent. |
| vii. | F- | g. | Metal ion which is an oxidising agent. |
| t/s | 0 | 400 | 800 | 1200 | 1600 | 2000 | 2400 | 2800 | 3200 |
| 102 × [N2O5]/mol L-1 | 1.63 | 1.36 | 1.14 | 0.93 | 0.78 | 0.64 | 0.53 | 0.43 | 0.35 |