The three cells with their \(E^\circ_{\text{(cell)}}\) values are given below:

Cells \(E^\circ_{\text{(cell)}}/V\)
(a) Fe|Fe2+||Fe3+|Fe 0.404
(b) Fe|Fe2+||Fe3+, Fe2+|Pt 1.211
(c) Fe|Fe3+||Fe3+, Fe2+|Pt 0.807
The standard Gibbs free energy change values for three cells are, respectively
(F represents the charge on 1 mole of electrons.)
 
1. -1.212 F, -1.211 F, -0.807 F
2. +2.424 F, +2.422 F, +2.421 F
3. -0.808 F, -2.422 F, -2.421 F
4. -2.424 F, -2.422 F, -2.421 F
Subtopic:  Faraday’s Law of Electrolysis |
 55%
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NEET - 2022
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The number of Faradays (F) required to produce 20 g of calcium from molten CaCl2 (Atomic mass of Ca=40 g mol-1) is:

1. 2

2. 3

3. 4

4. 1

Subtopic:  Faraday’s Law of Electrolysis |
 67%
From NCERT
NEET - 2020
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During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is:

1. 55 minutes

2. 110 minutes

3. 220 minutes

4. 330 minutes

Subtopic:  Faraday’s Law of Electrolysis |
 56%
From NCERT
NEET - 2016
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The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Charge on electron = 1.60 × 10–19 C)

1.  6×1023

2.  6×1020

3.  3.75×1020

4.  7.48×1020

Subtopic:  Faraday’s Law of Electrolysis |
 78%
From NCERT
NEET - 2016
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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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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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