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For the cell, Zn|ZnO(4)||AgNO(3)|Ag, the...

For the cell, `Zn|ZnO_(4)||AgNO_(3)|Ag`, the cell reaction is : `Zn+2Ag^(+)rarr Zn^(2+)+2Ag.` If `E_("cell")^(@)=+0.36V`, then calculate `Delta^(@)` for the cell reaction of that cell.

Text Solution

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`{:("Anode reaction: "Zn(s)" "rarr" "Zn^(2+)(aq)+2e),("Cathode reaction : "2Ag^(+)(aq)+2e" "rarr" "2Ag(s)),(bar(" Cell reaction: "Zn(s)+2Ag^(2+)(aq)" "rarr" "Zn^(2+)(aq)+2Ag(s))):}`
As 2 mol electrons are involved in the cell reaction, n = 2.
`therefore" The standard free energy change,"`
`DeltaG^(@)=-nFE^(@)`
`=-(2xx96500xx0.36)=-69480V.C=-69480J`
`=-69.48kJ" "[because " 1 volt - coulomb = 1 joule"]`
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