Initially the concentration of `Ag^(+) and Cu^(2+)` is 1 (M) each in the electrolytic cell, `Ag|Ag^(+)||Cu^(2+)|Cu`. If 9.65 A of current is passed through the cell for one hour, what will be the change in the cell potential?

Explanation

`{:(" "2Ag+2erarr2Ag),(" "CurarrCu^(+)+2e),(bar(2Ag^(+)+CurarrCu^(2+)+2Ag)):}`
Initially, `E_("cell")=E_("cell")^(@)-(0.059)/(2)log.([Ag^(+)]^(2))/([Cu^(2+)])`
`=E_("cell")^(@)-(0.059)/(2)log.(1)/(1)=E_("cell")^(@)`
Amount of electricity (Q)
`=Ixxt=9.65xx60xx60=34740C.`
`"34740 electricity produce "(1)/(96500)xx34740="0.36 mol"`
`"Ag at cathode and "(1)/(2xx9650)xx34740="0.18 mol "Cl_(2)" at anode."`
At this stage, `[Ag^(+)]=1-0.36=0.64(M)`
and `[Cu^(2+)]=1+0.18=1.18(M)`
`therefore" "E'_("cell")=E_("cell")^(@)-(0.059)/(2)log.((0.64)^(2))/(1.18)=E_("cell")^(@)-0.13`
`therefore" "E_("cell")-E'_("cell")=0.013V`