Which is the correct representation for Nernst equation ?
1. \(E_{\mathrm{RP}}=E_{\mathrm{RP}}^{\circ}+\frac{0.059}{\mathrm{n}} \log \frac{[\text { oxidant }]}{[\text { reductant }]}\)
2. \(E_{\mathrm{OP}}=E_{\mathrm{OP}}^{\circ}-\frac{0.059}{\mathrm{n}} \log \frac{[\text { oxidant }]}{[\text { reductant }]}\)
3. \(E_{\mathrm{OP}}=E_{\mathrm{OP}}^{\circ}+\frac{0.059}{\mathrm{n}} \log \frac{[\text { reductant }]}{[\text { oxidant }]}\)
4. All of the above
The voltage of the cell given below increases with:
Cell: Sn(s) + 2Ag+(aq) → Sn2+(aq) + 2Ag(s)
1. Increase in size of the silver rod.
2. Increase in the concentration of Sn2+ ions.
3. Increase in the concentration of Ag+ ions.
4. None of the above.
Which graph correctly correlates Ecell as a function of concentrations for the cell (for different values of M and M') ?
1. 2.
3. 4.
The solution of CuSO4 in which copper rod is immersed is diluted to 10 times, the reduction electrode potential:
1. increases by 0.030 V
2. decreases by 0.030 V
3. increases by 0.059 V
4. decreases by 0.059 V
The change in reduction potential of a hydrogen electrode when its solution initialy at pH = 0 is neutralised to pH = 7, is a/an-
1. | Increase by 0.059 V | 2. | Decrease by 0.059 V |
3. | Increase by 0.41 V | 4. | Decrease by 0.41 V |
For the cell, Ti|Ti+(0.001M)||Cu2+(0.1M)|Cu,Ecell at 25C is 0.83 V. Ecell can be increased:
1. By increasing [Cu2+]
2. By increasing [Ti+]
3. By decreasing [Cu2+]
4. None of these
By how much will the potential of half cell Cu2+| Cu change if the solution is diluted to 100 times at 298 K. It will -
1. | Increase by 59 mV | 2. | Decrease by 59 mV |
3. | Increase by 29.5 mV | 4. | Decrease by 29.5 mV |
At 298 K the Emf
of the following cell is:-
\(\small{Pt|H_{2}(1 \ atm)|H^{+}(0.02 \ M) \ || \ H^{+}(0.01 \ M)|H_{2}(1 \ atm)|Pt}\)
1. - 0.017 V
2. 0.0295 V
3. 0.1 V
4. 0.059 V
At 25C temperature Zn electrode is placed in 0.1M solution of zinc salt then what will be the reduction potential ? If it is assumed that salt dissociates 25% at this dilution ()
(1) -0.713 V
(2) - 0.81 V
(3) + 0.778 V
(4) - 0.84 V
The reduction potential of Hydrogen electrode is -118mV then the concentration of ion in solution will be :-
(1) 10-4M
(2) 2M
(3) 0.01M
(4) 10-3M