Molten $\mathrm{CuCl}_2$ is electrolysed using platinum electrodes. The reaction occurring at anode is

Molten $\mathrm{CuCl}_2$ is electrolysed using platinum electrodes. The reaction occurring at anode is
  1. $2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2(g)+2 e^{-}$
  2. $\mathrm{Cl}_2(g)+2 e^{-} \longrightarrow 2 \mathrm{Cl}$
  3. $\mathrm{Cu}^{2+}+2 e^{-} \longrightarrow \mathrm{Cu}(s)$
  4. $\mathrm{Cu}(s) \longrightarrow \mathrm{Cu}^{2+}+2 e^{-}$

Solution

In the electrolysis of $\mathrm{CuCl}_2$, At anode, $2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2(g)+2 e^{-}$ ,

Asked in: JEE-TOPICTESTS-CHEMISTRY

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