Calculate the quantity of electricity required to liberate 0.1 mole of chlorine gas during electrolysis of molten sodium chloride.

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The reaction at the anode during the electrolysis of molten sodium chloride is:

$2 C l^{-} \to C l_{2} + 2 e^{-}$

From the stoichiometry of the reaction, $1$ mole of $C l_{2}$ gas is liberated by $2$ moles of electrons.

Therefore, $0.1$ mole of $C l_{2}$ gas will require $0.1 \times 2 = 0.2$ moles of electrons.

The quantity of electricity required for $1$ mole of electrons is $1$ Faraday ( $1$ F $= 96500$ C).

Quantity of electricity required $= 0.2 \times 96500$ C $= 19300$ C.

Answer: 19300 C

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