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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

-0.60 V

B

0.60 V

C

6.0 V

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
A
The net cell reaction from given cell is
`AgCl to Ag^(+) + Cl^(-)`
`therefore Delta G^@=sum Delta G_(P)^@- sum Delta G_(R)^@`
(78-129)-(-109)
`= + 58 Kj//mol`
`= + 58 xx10^(3) j//mol`
` therefore Delta G_(R)^@=-nFE^@`
` 58 xx 10^(3)= -1 xx 96500 xx E^@`
`implies E^@=- (58xx10^(3))/(1xx96500)= -0.601V`
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