# 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 |
90%
From NCERT
AIPMT - 2011
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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:
(Given -ECE of chlorine is 0.367 X 10-6 kgC-1)

1. $kg$

2. $9.67×{10}^{-3}$ $kg$

3. $17.61×{10}^{-3}$ $kg$

4. $3.67×{10}^{-3}$ $kg$

Subtopic:  Faraday’s Law of Electrolysis |
52%
From NCERT
AIPMT - 2010
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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 |
69%
From NCERT
AIPMT - 2010
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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 |
AIPMT - 2010
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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, the mass of aluminum produced is:
(Assume 100 % current efficiency, the 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 |
65%
From NCERT
AIPMT - 2009
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The molar conductance of $\frac{\mathrm{M}}{32}$ solution of a weak monobasic acid is 8.0 ohm-1 cmand at infinite dilution is 400 ohm-1 cm2. The dissociation constant of this acid is:

 1 $$1.25 \times10^{-5}$$ 2 $$1.25 \times10^{-6}$$ 3 $$6.25 \times10^{-4}$$ 4 $$1.25 \times10^{-4}$$
Subtopic:   Kohlrausch Law & Cell Constant |
64%
From NCERT
AIPMT - 2009
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Given:
(i) ${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Cu}$    Eo = 0.337 V
(ii) ${\mathrm{Cu}}^{2+}+{\mathrm{e}}^{-}\to {\mathrm{Cu}}^{+}$  Eo = 0.153 V
Electrode potential, Eo for the reaction,
${\mathrm{Cu}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Cu}$, will be:

1. 0.52 V

2. 0.90 V

3. 0.30 V

4. 0.38 V

Subtopic:  Relation between Emf, G, Kc & pH |
75%
From NCERT
AIPMT - 2009
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Kohlrausch's law states that at:

 1 Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte. 2 Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte. 3 Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte. 4 Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.
Subtopic:   Kohlrausch Law & Cell Constant |
53%
From NCERT
AIPMT - 2008
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The correct order of ionic mobility of ions in an aqueous solution is:
1. K+> Na+> Rb+> Cs+
2. Cs+> Rb+> K+> Na+
3. Rb+> K+> Cs+> Na+
4. Na+> K+> Rb+> Cs+
Subtopic:  Relation between Emf, G, Kc & pH |
75%
From NCERT
AIPMT - 2008
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A steady current of 1.5 A flows through a copper voltmeter for 10 min. If the electrochemical equivalent of copper is 30 × 10-5 g C-1, the mass of copper deposited on the electrode will be:

1. 0.40 g

2. 0.50 g

3. 0.67 g

4. 0.27 g

Subtopic:  Faraday’s Law of Electrolysis |
75%
From NCERT
AIPMT - 2007
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