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

Answer

A

Explanation

The cell reaction can be written as
`Cu + 2 Ag^(+) to Cu^(2+) + 2 Ag`
We know , `Delta G^(@) = - n FE_(cell)^(@)`
= `-2 xx 96500 xx 0.46 = - 88780 J`
`= -88.780 k J = -89 kJ`