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

Subtopic:  Nernst Equation |
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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.

Subtopic:  Nernst Equation |
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Which graph correctly correlates Ecell as a function of concentrations for the cell (for different values of M and M') ?

Zn(s) + Cu2+(M)           Zn2+(M') + Cu(s);
                Ecell = 1.10 V
X-axis : log10Zn2+Cu2+, Y-axis : Ecell 

1.                         2. 
3.                         4. 

Subtopic:  Nernst Equation |
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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

Subtopic:  Nernst Equation |
 50%
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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
Subtopic:  Electrode & Electrode Potential | Nernst Equation |
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For the cell, Ti|Ti+(0.001M)||Cu2+(0.1M)|Cu,Ecell at 25°C is 0.83 V. Ecell can be increased:

1. By increasing [Cu2+]

2. By increasing [Ti+]

3. By decreasing [Cu2+]

4. None of these

Subtopic:  Nernst Equation |
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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
Subtopic:  Nernst Equation |
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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

Subtopic:  Nernst Equation |
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At 25°C 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 (EZn2+Zn° = -0.76 V)

(1) -0.713 V

(2) - 0.81 V

(3) + 0.778 V

(4) - 0.84 V

Subtopic:  Nernst Equation |
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The reduction potential of Hydrogen electrode is -118mV then the concentration of Hion in solution will be :-

(1) 10-4M

(2) 2M

(3) 0.01M

(4) 10-3M

Subtopic:  Nernst Equation |
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