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 |
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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 |
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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 = 1.60x 10-19 C)

1.  $6×{10}^{23}$

2.  $6×{10}^{20}$

3.  $3.75×{10}^{20}$

4.  $7.48×{10}^{20}$

Subtopic:  Faraday’s Law of Electrolysis |
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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 |
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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 |
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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 (ECE of chlorine is 0.367 X 10-6 kgC-1)

1.

2.

3.

4.

Subtopic:  Faraday’s Law of Electrolysis |
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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 |
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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, what mass of aluminium is produced ?

(Assume 100 % current efficiency, 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 |
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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 |
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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 |
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