- 1(current)
Q. No.Consider the given cell:
\(\mathrm{Z n \left|\right. Z n S O_{4} \left(\right. 0 . 01 M \left.\right) \left|\right. \left|\right. C u S O_{4} \left(\right. 1 . 0 M \left.\right) \left|\right. C u}\)
In the electrochemical cell, the emf of this Daniel cell is E1. When the concentration of ZnSO4 is changed to 1.0 M and that of CuSO4 is changed to 0.01 M, the emf changes to E2. From the following, which one is the relationship between E1 and E2 ?
(Given: \(\frac{RT}{F}\) = 0.059)
| 1. | \(\mathrm{E_{1} < E_{2}}\) | 2. | \(\mathrm{E_{1} > E_{2}}\) |
| 3. | \(\mathrm{E_{2} = 0 \neq E_{1}}\) | 4. | \(\mathrm{E_{1} = E_{2}}\) |
Find the emf of the cell in which the following reaction takes place at 298 K:
\(\mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) \)
\(\small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=1.05 \mathrm{~V}; \dfrac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059} )\)
| 1. | 1.05 V | 2. | 1.0385 V |
| 3. | 1.385 V | 4. | 0.9615 V |
The pressure of H2 required to make the potential of H2 - electrode zero in pure water at 298 K is:
| 1. | 10–12 atm | 2. | 10–10 atm |
| 3. | 10–4 atm | 4. | 10–14 atm |
- 1(current)
Q. No.
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