# Al2O3 is reduced by electrolysis at low potentials and high currents. If 4.0 x 104 A 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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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. $2.4×{10}^{10}$

2. $2.0×{10}^{10}$

3. $4.0×{10}^{10}$

4. $4.0×{10}^{15}$

Subtopic:  Nernst Equation | Relation between Emf, G, Kc & pH |
62%
From NCERT
AIPMT - 2007
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The efficiency of a fuel cell is given by:

1. $\frac{∆H}{∆G}$

2. $\frac{∆G}{∆S}$

3. $\frac{∆G}{∆H}$

4. $\frac{∆S}{∆G}$

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 |
63%
From NCERT
AIPMT - 2006
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If ${\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{\mathrm{o}}$ = -0.441 V and  ${\mathrm{E}}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}^{\mathrm{o}}$ = 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 |
72%
From NCERT
AIPMT - 2006
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