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Question
Consider a cell given below:
\[\ce{Cu | Cu^{2+} || Cl^{-} | Cl_{2},Pt}\]
Write the reactions that occur at anode and cathode
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Solution
Anode: \[\ce{Cu -> Cu^{2+} + 2e^{-}}\]
Cathode: \[\ce{Cl_2 + 2e^{-} -> 2Cl^{-}}\]
\[\ce{Cu}\] is anode as it is getting oxidised.
\[\ce{Cl2}\] is cathode as it is getting reduced.
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