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The E^(@) values corresponding to the fo...

The `E^(@)` values corresponding to the following reduction electrode process are :
(i) `Cu^(+)//Cu =+0.52 "V ",` (ii) `Cu^(2+)//Cu^(+)=+0.16" V "`
Formulate the galvanic cell for their combination. What will be the standard cell potential for it ? Calculate `DeltaG` for the cell reaction. (`F=96500" C "mol^(-1)`)

Text Solution

Verified by Experts

Cathode: `Cu^(+)+e^(-) to Cu`
Anode : `Cu^(+) to Cu^(2+)+e^(-)`
Cell representation : `Cu^(+)|Cu^(2+)||Cu^(+)|Cu`.
`E_(cell)^(@)=E_(cathode)^(@)-E_(anode)^(@)=0.52-0.16=0.36" V "`
`DeltaG^(@)=-nFE_(cell)^(@)=-(1 mol)xx(96500" C mol"^(-1))xx(0.36" V ")`
`=-34740" CV"=-34740 J`.
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