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))`:A. `-98.00 kJ`B. `-89.0 kJ`C. `-89.0 J`D. `-44.5 kJ`

For the reduction of silver ions with copper metal, the standard cell

1.	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))`:A. `-98.00 kJ`B. `-89.0 kJ`C. `-89.0 J`D. `-44.5 kJ`
Answer» Correct Answer - B The relationship between `E_("cell")^(@)` for a galvanic cell and `Delta_(r)G^(@)`, the standard Gibbs energy change, for the chemical reaction of the cell is `Delta_(r)G^(@) = -nFE_("cell")^(@)` For the cell reaction `2Ag^(+)(aq.)+Cu(s) rarr Cu^(2+)(aq.)+2Ag(s)` We have `n = 2 mol` `E_("cell")^(@) = +0.46 V` Therefore `Delta_(r)G^(@) = (-2 mol)(96,500 C mol^(-1))(+0.46 V)` `= -88780 J = -88.780 kJ` `= -89.0 kJ`

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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))`:A. `-98.00 kJ`B. `-89.0 kJ`C. `-89.0 J`D. `-44.5 kJ`

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