Which of the following is released at anode during electrolysis of aqueous and concentrated copper chloride using inert electrodes?

H_{2} (g)

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O_{2} (g)

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C l_{2} (g)

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H C l (g)

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Solution

The correct option is C $C l_{2} (g)$
In electrolysis of aqueous and concentrated $C u C l_{2}$ using inert electrodes :
At anode:
Possible reactions are:
$2 H_{2} O (l) ⇌ 4 H^{+} (a q) + O_{2} (g) + 4 e^{-}$
$E_{H_{2} O / H_{2}}^{0} = - 1.23 V$

$2 C l^{-} (a q) ⇌ C l_{2} (g) + 2 e^{-}$
$E_{C l^{-} / C l_{2}}^{0} = - 1.36 V$

Even if $E_{C l^{-} / C l_{2}}^{0} < E_{H_{2} O / O_{2}}^{0}$
Kinetically rate of oxidation of water is very slow. To increase its rate, the greater potential difference is applied called as overpotential. Because of this overpotential (which is the extra potential required to start a reaction), oxidation of $C l^{-}$ ions becomes more feasible
The reaction that occurs at anode is :
$2 C l^{-} (a q) ⇌ C l_{2} (g) + 2 e^{-}$

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