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For the following cell reaction, Ag | Ag...

For the following cell reaction,
`Ag | Ag^(+) | AgCl | Cl^(-) | Cl_(2) , Pt`
`Delta G_(f)^(0) (AgCl) =-109 kJ//mol`
`Delta G_(f)^(0) (Cl ) = -129kJ//mol`
`Delta G_(f)^(0) (Ag^(+)) = 78 kJ//mol`
`E^@` of the cell is

A

`-0.60V`

B

`0.60V`

C

`6.0V`

D

None

Text Solution

Verified by Experts

The correct Answer is:
B
`AgrarrAg^(+)+"le"^(-)`
`1//2Cl_(2)+"le"^(-)rarrCl^(-)`
`DeltaG^(@)=G_("Product")^(@)-G_("Reactant")^(@)`
`DeltaG^(@)=-nFE^(@)`
`E^(@)=(DeltaG^(@))/(nF)`
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