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Write the Nernst equation for the cell reaction in the Daniel cell. How will the $E_{\text {cell }}$ be affected when concentration of $\mathrm{Zn}^{2+}$ ions is increased?
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The two half cell reactions are given as following:
At anode : $\mathrm{Cu} \longrightarrow \mathrm{Cu}^{2+}+2 e^{-}$
At cathode : $\mathrm{Cl}_2+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}$
Copper is getting oxidised at anode. $\mathrm{Cl}_2$ is getting reduced at cathode.
At anode : $\mathrm{Cu} \longrightarrow \mathrm{Cu}^{2+}+2 e^{-}$
At cathode : $\mathrm{Cl}_2+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}$
Copper is getting oxidised at anode. $\mathrm{Cl}_2$ is getting reduced at cathode.
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