Consider a cell given below. `Cu|Cu^(2+)|Cl^(-)|Cl_(2).Pt` Write the reactions that occur at anode and cathode.

Consider a cell given below. `Cu|Cu^(2+)|Cl^(-)|Cl_(2).Pt` Write the r

1.	Consider a cell given below. `Cu\|Cu^(2+)\|Cl^(-)\|Cl_(2).Pt` Write the reactions that occur at anode and cathode.
Answer» The reaction taking place at the two electrodes are : At anode : `Cu(s) to Cu^(2+)(aq) +2e^(-)` At cathode : `Cl_(2)(g) +2e^(-) to 2Cl^(-)(aq)` Thus,Cu(s) is oxidised to `Cu^(2+)`(aq) ions at anode while `Cl_(2)`(g) is reduced to `Cl^(-)` (aq) ions at cathode.

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What are elementary reactions ?

Consider a cell given below. `Cu|Cu^(2+)|Cl^(-)|Cl_(2).Pt` Write the reactions that occur at anode and cathode.

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