The drinvin force `/_\G` diminishes to zero on the way to equilibrium just as in any other spontaneous process, Both `/_\G` and the cell potential `(E=-(/_\G)/(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^0=E^0-(0.059)/nlog_(10)Q`
The key to the relationship is the standard cell potential `E^0`, derived from the standard free energy change as :
`E^0=(/_\G^0)/(nF)`
At equilibrium, the Nemst equation is given as :
`E^0=(0.059)/log_(10)K`
`E^0` for the electrochemical cell,
`Zn(s)|Zn^(2+)(1M)aq||Cu^(2+)(1M)aq||Cu(s)` is 1.10 volt at `25^(@)`C.
The equilibrium constant for the cell reaction:
`Zn(s)+Cu^(2+)(aq) will be-

Options

A. `10^(-37)`
B. `10^(37)`
C. `10^(-39)`
D. `10^(39)`

Answer

A