For the reduction of silver ions with copper metal, the standard cell potential was foound to be `+0.46 V` at `25^(@) C`. The value of standard Gibbs energy, `DeltaG^(@)` will be `(F = 96,500C mol^(-1))`:

Options

A. `-89.0 kJ`
B. `-89.0J`
C. `-44.5 kJ`
D. `-98.0 kJ`

Answer

A

Explanation

(a) We know that , standard Gibbs energy, `DeltaG^(@)=-nFE_(cell)^(@)`
For the cell reaction,
`2Ag^(+)+Cu to Cu^(2+) +2Ag`
`DeltaE_(cell)^(@)=+0.46 V`
`DeltaG^(@)=-nFE_(cell)^(@)`
`n=2`
`DeltaG^(@)=-2xx96500xx0.46`
`=-88780 J`
`=- 88.7 kJ ~~-89.0 kJ`