Consider a cell given below $Cu \,|\, Cu^{2+} \,|\, | \, Cl^{-} \,|\, Cl_2$,$Pt$. Write the reactions that occur at anode and cathode.

(N/A) In the given cell representation,the left side represents the anode and the right side represents the cathode.
Oxidation reaction at the anode: $Cu_{(s)} \rightarrow Cu^{2+}_{(aq)} + 2e^-$
Reduction reaction at the cathode: $Cl_{2(g)} + 2e^- \rightarrow 2Cl^-_{(aq)}$
At the anode,$Cu$ undergoes oxidation by losing electrons,and at the cathode,$Cl_2$ undergoes reduction by gaining electrons.