(C) The aqueous solution of $CuCl_2$ dissociates as: $CuCl_2 \longrightarrow Cu^{2+}_{(aq)} + 2 Cl^{-}_{(aq)}$.At the cathode,$Cu^{2+}$ ions have a hi

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$Cu^{2+}_{(aq)} + 2 e^{-} \longrightarrow Cu_{(s)}$; $2 Cl^{-}_{(aq)} \longrightarrow Cl_{2(g)} + 2 e^{-}$

(C) The aqueous solution of $CuCl_2$ dissociates as: $CuCl_2 \longrightarrow Cu^{2+}_{(aq)} + 2 Cl^{-}_{(aq)}$.At the cathode,$Cu^{2+}$ ions have a higher reduction potential than $H_2O$ molecules,so $Cu^{2+}$ ions are reduced to $Cu$ metal:$Cu^{2+}_{(aq)} + 2 e^{-} \longrightarrow Cu_{(s)}$.At the anode,$Cl^{-}$ ions are oxidized to $Cl_2$ gas:$2 Cl^{-}_{(aq)} \longrightarrow Cl_{2(g)} + 2 e^{-}$.

Class 12 Chemistry Electrochemistry Electrolytes and Electrolysis

Medium

When an aqueous solution of $CuCl_2$ is electrolysed using $Pt$ inert electrodes,the reactions at the cathode and anode respectively are:

AP EAMCET 2018 All AP EAMCET

A
$4 H_2O_{(l)} + 4 e^{-} \longrightarrow 2 H_{2(g)} + 4 OH^{-}_{(aq)}$; $2 H_2O_{(l)} \longrightarrow O_{2(g)} + 4 H^{+}_{(aq)} + 4 e^{-}$
B
$2 Cu^{2+}_{(aq)} + 4 e^{-} \longrightarrow 2 Cu_{(s)}$; $2 H_2O_{(l)} \longrightarrow O_{2(g)} + 4 H^{+}_{(aq)} + 4 e^{-}$
C
$Cu^{2+}_{(aq)} + 2 e^{-} \longrightarrow Cu_{(s)}$; $2 Cl^{-}_{(aq)} \longrightarrow Cl_{2(g)} + 2 e^{-}$
D
$2 H_2O_{(l)} + 2 e^{-} \longrightarrow H_{2(g)} + 2 OH^{-}_{(aq)}$; $2 Cl^{-}_{(aq)} \longrightarrow Cl_{2(g)} + 2 e^{-}$