The following galvanic cell was
`underset(100mL) (Zn|Zn^(2+) (1M) )|| underset("100mL")(Cu^(2+) (1M) |Cu)`
operated as an electrolytic cell using Cu as anode and Zn cathode. A current of 0.48A was passed for 10 hrs then cell was allowed to function as galvanic cell. What would be the emf the cell at `25^(@)C? ` Assume that the only electrode reactions occuring were those involving.

Explanation

`q=(0.48 xx 10 xx 60 xx 60)/(96500)=0.18F`
Eq of `Cu^(2+)" formed"=Eq Zn^(2+)" deposited =0.18"`
Or Mole of `Cu^(2+)"formed =Mole of "Zn^(2+)" deposited" =(0.18)/(2)=0.09`
or Millimole of `Zn^(2+)` deposited `=0.09 xx 1000=90`
Millimole of `Zn^(2+) ("final")=100 xx 1-90=10`
Millimole of `Cu^(2+) ("final")=100 xx 1+90=190`
As both are present in 100 mL solution of each
`E_("cell")=E_("cell")^(0)-(0.0591)/(2) log ([Zn^(2+)])/([Cu^(2+)])`
`E_("cell")=0.76 +0.34-(0.0591)/(2) log"" (190)/(10)`
=1.137 V