For the disproportion of copper:
`2 Cu^(+) to Cu^(+2) + Cum E^(0)` is :- Given `E^(0)` for `Cu^(+2)//Cu` is 0.34 V & `E^(0)` for `Cu^(+2)//Cu^(+)` is 0.15 V:

For the disproportion of copper: 2 Cu^(+) to Cu^(+2) + Cu E^(0) is :- Given E^(0) for Cu^(+2)//Cu is 0.34 V & E^(0) for Cu^(+2)//Cu^(+) is 0.15 V:

For the disproportion of copper: 2 Cu^(+) to Cu^(+2) + Cu E^(0) is :- Given E^(0) for Cu^(+2)//Cu is 0.34 V & E^(0) for Cu^(+2)//Cu^(+) is 0.15 V:

E^(@) for Fe//Fe^(2+) is +0.44 V and E^(@) for Cu//Cu^(2+) is -0.32 V . Then, in the cell,

(CU^(+) ((aq)) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu_((aq))^(+) Cu_((aq))^(2+) +Cu_((s)) choose E^(@) for the above reaction if E_(Cu^(2+)//Cu^(@))= 0.34V and E_(Cu^(2+)//Cu^(+) )= 0.15V

(CU^(+) ((aq)) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu_((aq))^(+) Cu_((aq))^(2+) +Cu_((s)) choose E^(@) for the above reaction if E_(Cu^(2+)//Cu^(@))= 0.34V and E_(Cu^(2+)//Cu^(+) )= 0.15V

E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V . If E_(Cu^(2+) // Cu)^(0) is | 0.34 V , E_(Ag^(+)//Ag)^(0) is

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell