# A current is passed through two voltameters connected in series. The first voltmeter connected in series. The first voltmeter contains XSO4(aq) while the second voltmeter contains Y2SO4(aq). The relative  atomic masses of X and Y are in the ratio of 2:1. The ration of the mass of X liberated to the mass of Y liberated is:  1. 1:1 2. 1:2 3. 2:1 4. none of these

Subtopic:  Faraday’s Law of Electrolysis |
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The mass of silver(eq. mass = 108) displaced by that quantity of current which displaced 5600 mL of hydrogen at STP is:

1. 54 g

2. 108 g

3. 5.4 g

4. none of these

Subtopic:  Faraday’s Law of Electrolysis |
53%
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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 |
79%
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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 |
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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 |
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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 |
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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 |
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