Answer: The standard potential of the cell is 3.17 V
Explanation:
The substance having highest positive [tex]E^o[/tex] potential will always get reduced and will undergo reduction reaction.
The half reactions for the cell is:
Oxidation half reaction (anode): [tex]Mg(s)\rightarrow Mg^{2+}+2e^-;E^o_{Mg^{2+}/Mg}=-2.37V[/tex]
Reduction half reaction (cathode): [tex]Ag^{+}+e^-\rightarrow Ag(s);E^o_{Ag^+/Ag}=+0.80V[/tex]
Substance getting oxidized always act as anode and the one getting reduced always act as cathode.
To calculate the [tex]E^o_{cell}[/tex] of the reaction, we use the equation:
[tex]E^o_{cell}=E^o_{cathode}-E^o_{anode}[/tex]
Putting values in above equation, we get:
[tex]E^o_{cell}=0.80-(-2.37)=3.17V[/tex]
Hence, the standard potential of the cell is 3.17 V
