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(C) The standard electrode potentials are $E^o_{Ag^+/Ag} = +0.80 \ V$ and $E^o_{Cu^{2+}/Cu} = +0.34 \ V$. For a spontaneous cell reaction,the electrod

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Copper electrode works as anode,then $E_{cell}^o$ is $+0.46 \ V$

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(C) The standard electrode potentials are $E^o_{Ag^+/Ag} = +0.80 \ V$ and $E^o_{Cu^{2+}/Cu} = +0.34 \ V$. For a spontaneous cell reaction,the electrode with the higher reduction potential acts as the cathode. Since $0.80 \ V > 0.34 \ V$,the silver electrode acts as the cathode and the copper electrode acts as the anode. The cell reaction is $Cu_{(s)} + 2Ag^+_{(aq)} 	o Cu^{2+}_{(aq)} + 2Ag_{(s)}$. The standard cell potential is calculated as: $E_{cell}^o = E_{cathode}^o - E_{anode}^o = 0.80 \ V - 0.34 \ V = +0.46 \ V$. Thus,when the copper electrode works as the anode,the $E_{cell}^o$ is $+0.46 \ V$.

Standard electrode potential of $Ag^{+}/Ag$ and $Cu^{2+}/Cu$ is $+0.80 \ V$ and $+0.34 \ V$ respectively. These electrodes are joined together by a salt bridge. If:

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