To find the standard potential of `M^(3+)//M` electrode, the following cell is constituted : `Pt|M|M^(3+) (0.0018 mol^(-1) L)||Ag^(+) (0.01 mol^(-1) L(|Ag` The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the half reaction `M^(3+)+3e^(-) rarr M`. `E_(Ag^(+)//Ag)^(@)=0.80` volt.

To find the standard potential of `M^(3+)//M` electrode, the following

1.	To find the standard potential of `M^(3+)//M` electrode, the following cell is constituted : `Pt\|M\|M^(3+) (0.0018 mol^(-1) L)\|\|Ag^(+) (0.01 mol^(-1) L(\|Ag` The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the half reaction `M^(3+)+3e^(-) rarr M`. `E_(Ag^(+)//Ag)^(@)=0.80` volt.
Answer» The cell reaction is `M+3Ag^(+) rarr 3Ag+M^(3+)` Applying Nernst equation, `E_(cell)=E_(cell)^(@)-0.0591/3"log" ([M^(3+)])/([Ag^(+)]^(3))` `0.42=E_(cell)^(@)-0.0591/3"log"((0.0018))/((0.01)^(3))=E_(cell)^(@)-0.064` `E_(cell)^(@)=(0.42+0.064)=0.484` volt `E_(cell)^(@)=E_("Cathode")^(@)-E_("Anode")^(@)` or `E_("Anode")^(@)=E_("Cathode")^(@)-E_(Cell)^(@)` `=(0.80-0.484)=0.32` volt

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