A button cell used in watches functions as following  Zn(s) + Ag2O(s) + H2O(l) $$\rightleftharpoons$$ 2Ag(s) + Zn2+(aq) + 2OH–(aq) If half-cell potentials are: Zn2+(aq) + 2e–→ Zn(s)  Eo = – 0.76 V  Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq) Eo = 0.34 V The cell potential will be: 1. 0.42 V 2. 0.84 V 3. 1.34 V 4. 1.10 V

Subtopic:  Electrode & Electrode Potential |
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Limiting molar conductivity of NH4OH (i.e., ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{OH}\right)}^{0}$ is equal to -

1. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}$

2. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}$

3. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{OH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(HCl\right)}^{0}$

4. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}$

Subtopic:   Kohlrausch Law & Cell Constant |
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Standard electrode potential of three metals X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be :

1.  Y > X > Z

2.  Z > X > Y

3.  X > Y > Z

4.  Y > Z > X

Subtopic:  Electrode & Electrode Potential |
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If the  for a given reaction has a negative value, then which of the following gives the correct relationship for the values of ?

1.

2.

3.

4.

Subtopic:  Electrolytic & Electrochemical Cell | Relation between Emf, G, Kc & pH |
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Based on electrode potentials in the table below:
 Cu2+(aq) + e- → Cu+(aq) 0.15 V Cu+(aq) + e- → Cu(s) 0.50 V

The value of $$E_{Cu^{2+}/Cu}^{o}$$ will be:
1. 0.325 V
2. 0650 V
3. 0.150 V
4. 0.500 V

Subtopic:  Electrode & Electrode Potential |
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Standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for Cr3+/Cr couple is -0.74. 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 |
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In producing chlorine by electrolysis, 100 kW power at 125 V is being consumed. How much chlorine per minute is liberated (ECE of chlorine is 0.367 X 10-6 kgC-1)

1.

2.

3.

4.

Subtopic:  Faraday’s Law of Electrolysis |
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For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25 °C. The value of standard Gibbs energy, ΔGo will be :

(F = 96500 C mol-1)

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

Subtopic:  Faraday’s Law of Electrolysis |
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An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

1. increase in ionic mobility of ions

2. 100% ionization of electrolyte at normal dilution

3. increase in both, i.e, number of ions and ionic mobility of ions

4. increase in the number of ions

Subtopic:  Conductance & Conductivity |
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Al2Ois reduced by electrolysis at low potentials and high currents. If 4.0 x 10A of current is passed through molten Al2O3 for 6 hours, what mass of aluminium is produced ?

(Assume 100 % current efficiency, atomic mass of Al = 27 g mol-1)

1. 9.0 x 103 g

2. 8.1 X 104 g

3. 2.4 x 105 g

4. 1.3 X 104 g

Subtopic:  Faraday’s Law of Electrolysis |
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