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

1. 96500 C

2. 2 x 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. 4.0 2. 20.0
3. 40.0 4. 0.66
Subtopic:  Faraday’s Law of Electrolysis |
 70%
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. 1.76×10-3 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 |
 64%
From NCERT
AIPMT - 2006
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