Molten CuCl $_{2}$ is electrolyzed using platinum electrodes. The reaction occurring at anode is :

2 C l^{-} \to C l_{2 (g)} + 2 e^{-}

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C l_{2 (g)} + 2 e^{-} \to 2 C l^{-}

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C u^{2 +} + 2 e^{-} \to C u (s)

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C u (s) \to C u^{2 +} + 2 e^{-}

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Solution

The correct option is A $2 C l^{-} \to C l_{2 (g)} + 2 e^{-}$
Molten $C u C L_{2}$ contains movable $C u^{2 +}$ and $2 C l^{-}$ ions.
At anode, oxidation takes place
therefore rection at anode is oxidation of $C l^{-}$ ions and it losses electrons as:
$2 C l^{-} \to C l_{2} (g) + 2 e^{-}$
A is correct.

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Similar questions

C u C l_{2}

Identify the correct reaction from the options given below for the electrolysis of $C u C l_{2}$ .

E_{R P}

2 C l^{-} (a q .) \to C l_{2} (g) + 2 e^{-}

C u S O_{4}

C u_{(s)} \to C u^{2 +} + {2 e}^{-}

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