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 M32 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) Cu2++2e-Cu    Eo = 0.337 V 
(ii) Cu2++e-Cu+  Eo = 0.153 V 
Electrode potential, Eo for the reaction, 
Cu++e-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 |
 54%
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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For a given reaction, 
Cu(s) + 2Ag+ (aq) → Cu2+(aq)+2Ag(s); 
E0=0.46 V at 298 K . The equilibrium constant will be :

1. 2.4×1010

2. 2.0×1010

3. 4.0×1010

4. 4.0×1015

Subtopic:  Nernst Equation | Relation between Emf, G, Kc & pH |
 61%
From NCERT
AIPMT - 2007
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The efficiency of a fuel cell is given by:

1. HG

2. GS

3. GH

4. SG

Subtopic:  Batteries & Salt Bridge |
 65%
AIPMT - 2007
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In producing chlorine through electrolysis, 100 W power at 125 V is being consumed.
The liberation of chlorine per min is:
(ECE of chlorine is 0.367×10-6 kg/C)
1. 17.6 mg 2. 21.3 mg
3. 24.3 mg 4. 13.6 mg
Subtopic:  Faraday’s Law of Electrolysis |
 64%
From NCERT
AIPMT - 2006
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