The driving force `DeltaG` diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both `DeltaG` and the corresponding cell potential `(E=-(DeltaG)/(nF))` are zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as : `E=E^(@)-0.059/n log Q` The key to the relationship is the standard cell potential `E^(@)`, derived from the standard free energy changes as : `E^(@)=-(DeltaG^(@))/(nF)` At equilibrium, the Nernst equation is given as : `E^(@)=0.059/n log K` The equilibrium constant `K_(c)` for the reaction : `Cu(s)+2Ag^(+) (aq.)+2Ag(s)" "(E_(cell)^(@)=0.46 V)` will be :A. antilog 15.6B. antilog 2.5C. antilog 1.5D. antilog 12.2

The driving force `DeltaG` diminishes to zero on the way to equilibriu

1.	The driving force `DeltaG` diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both `DeltaG` and the corresponding cell potential `(E=-(DeltaG)/(nF))` are zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as : `E=E^(@)-0.059/n log Q` The key to the relationship is the standard cell potential `E^(@)`, derived from the standard free energy changes as : `E^(@)=-(DeltaG^(@))/(nF)` At equilibrium, the Nernst equation is given as : `E^(@)=0.059/n log K` The equilibrium constant `K_(c)` for the reaction : `Cu(s)+2Ag^(+) (aq.)+2Ag(s)" "(E_(cell)^(@)=0.46 V)` will be :A. antilog 15.6B. antilog 2.5C. antilog 1.5D. antilog 12.2
Answer» Correct Answer - A

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What are elementary reactions ?

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