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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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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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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If EFe2+/Feo = -0.441 V and  EFe3+/Fe2+o = 0.771 V, the standard emf of the reaction: 

Fe + 2Fe3+→ 3Fe2+ will be:

1. 0.330 V 2. 1.653 V
3. 1.212 V 4. 0.111 V
Subtopic:  Electrode & Electrode Potential |
 71%
From NCERT
AIPMT - 2006
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For the cell reaction \(2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)\)

\(E_{cell}^{o} \ = \ 0.24 \ V\) at 298 K. The standard Gibbs energy ∆rG of the cell reaction is:

[Given: 96500 C mol-1]

1. 23.16 kJ mol-1

2. -46.32 kJ mol-1

3. -23.16 kJ mol-1

4. 46.32 kJ mol-1

Subtopic:  Relation between Emf, G, Kc & pH |
 73%
From NCERT
NEET - 2019
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For a cell involving one electron Ecell=0.59 V at 298 K.
The equilibrium constant for the cell reaction is :
Given that 2.303 RTF=0.059 V at T=298 K)

1. 1.0×1030

2. 1.0×102

3. 1.0×105

4. 1.0×1010

Subtopic:  Relation between Emf, G, Kc & pH |
 69%
From NCERT
NEET - 2019
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The half cell reduction potential of a hydrogen electrode at pH = 10 will be :

1. 0.59 V                   

2. – 0.59 V

3. 0.059 V                 

4. – 0.059 V

Subtopic:  Nernst Equation |
 69%
From NCERT
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