When 0.1 mol MnO42– is oxidized, the quantity of electricity required to completely oxidise MnO42– to MnO4 is:

1. 96500 C

2. 2 × 96500 C

3. 9650 C

4. 96.50 C

Subtopic:  Faraday’s Law of Electrolysis |
77%
From NCERT
AIPMT - 2014
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The weight of silver (at.wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of Oat STP will be:

1. 5.4 g

2. 10.8 g

3. 54.0 g

4. 108.0 g

Subtopic:  Faraday’s Law of Electrolysis |
55%
From NCERT
AIPMT - 2014
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How many grams of cobalt metal will be deposited when a solution of cobalt (II) chloride is electrolyzed with a current of 10 amperes for 109 minutes?
(1 Faraday = 96,500 C; Atomic mass of Co = 59 u)

 1 4 2 20 3 40 4 0.66
Subtopic:  Faraday’s Law of Electrolysis |
71%
From NCERT
NEET - 2013
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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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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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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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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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