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Electrolysis and Electrolytes

A 4.0 molar a...

Question

A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrode.

[Atomic mass: Na = 23, Hg = 200; 1 Faraday = 96500 coulombs]

The total charge (coulombs) required for complete electrolysis is:

A

24125

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B

48250

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C

96500

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D

193000

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Solution

The correct option is D 193000
Faraday's Laws of Electrolysis Calculations of Current in Coulomb: $Q = n (e^{-}) \times F$

In the cell $2 m o l e s$ of electrons (2 Faraday) are required.

$Q = 2 \times 96500 C = 193000 C$

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Q. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrode.

[Atomic mass: Na = 23, Hg = 200; 1 Faraday = 96500 coulombs]

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Q. A 4.0 M aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass of Na is 23 and Hg is 200)

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Q. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrode.

[Atomic mass: Na = 23, Hg = 200; 1 Faraday = 96500 coulombs]

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Q. A 4.0 M aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass of Na is 23 and Hg is 200)

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Chemical reactions involve the interactions of atoms and molecules. A large number of atoms/molecules (approximately

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A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200; 1 faraday =96500 coulombs).
The total charge (coulombs) required for complete electrolysis is:

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