# A silver cup is plated with silver by passing 965 coulomb of electricity. The amount of Ag deposited is: 1. 1.08 g 2. 1.0002 g 3. 9.89 g 4. 107.89 g

Subtopic:  Faraday’s Law of Electrolysis |
80%
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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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When a copper wire is immersed in a solution of AgNO3, the colour of the solution becomes blue because copper:

1. Forms a soluble complex with $$AgNO_3$$
2. Is oxidised to $$Cu^{2+}$$
3. Is reduced to $$Cu^{2-}$$
4. Splits up into atomic form and dissolves

Subtopic:  Electrochemical Series |
79%
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The specific conductance of a 0.1 M KCl solution at 23 °C is 0.012  Ω–1 cm–1. The resistance of cells containing the solution at the same temperature was found to be 55 Ω. The cell constant will be:

 1 0.142 cm–1 2 0.66 cm–1 3 0.918 cm–1 4 1.12 cm–1
Subtopic:  Conductance & Conductivity |
85%
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Given below are two half-cell reactions:

Mn2+ + 2e → Mn;          E0 = -1.18V

2Mn3+ + 2e → 2Mn2+;  E0 = +1.51V

The E0 for 3Mn2+ → 2Mn+3  +  Mn  will be:

1. -2.69V; the reaction will not occur

2. -2.69V; the reaction will occur

3. -0.33V; the reaction will not occur

4. -0.33V; the reaction will occur

Subtopic:  Electrode & Electrode Potential |
50%
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E0 for Fe2+ + 2e → Fe is –0.44 volt and E0 for Zn2+ + 2e→ Zn is –0.76 volt, thus:

1. Zn is more electropositive than Fe.

2. Fe is more electropositive than Zn.

3. Zn is more electronegative.

4. None of the above.

Subtopic:  Electrode & Electrode Potential |
64%
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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 |
60%
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A 5A current is passed through a solution of copper sulphate for 40 min. The amount of copper deposited at the cathode is:

 1 40.65g 2 0.45g 3 3.94g 4 65.04g
Subtopic:  Faraday’s Law of Electrolysis |
67%
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, the standard emf of the reaction

will be

1. 0.111V

2. 0.330V

3. 1.653V

4. 1.212V

Subtopic:  Electrode & Electrode Potential |
66%
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The standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for the Cr3+/Cr couple is -0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be:

 1 +0.89 V 2 +0.18 V 3 +1.83 V 4 +1.199 V
Subtopic:  Electrode & Electrode Potential |
90%
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