`Cu^(+) + e rarr Cu, E^(@) = X_(1)` volt,
`Cu^(2+) + 2e rarr Cu, E^(@) = X_(2)`X_(2) volt
For `Cu^(2+) + e rarr Cu^(+), E^(@)` will be :

Cu^(+) + e rarr Cu, E^(@) = X_(1) volt, Cu^(2+) + 2e rarr Cu, E^(@) = X_(2) volt For Cu^(2+) + e rarr Cu^(+), E^(@) will be :

Cu^(+) + e^(-) rightarrow Cu , E^(@) = x1volt , Cu^(2+) + 2e^(-) rightarrow Cu , E^(@) = x_(2) volt, then for Cu^(2+) + e^(-) rightarrow Cu^(+), E^(@) (volt) will be :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The E^(@) for the reaction : 2Cu^(+) rarr Cu^(2+) + Cu is:

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The E^(@) for Cu rarr Cu^(2+) + 2e is :

Goven : (i) CU^(2+) + 2e^- rarr Cu, E^@ = 0.337 V (ii) Cu^(2+) +e^- rarr Cu^(+) , E^2=0.1 5 3 V .

Given , Cu^(2+) + e^(-) to Cu^(+) E^(@) = 0.15 " volt " , Cu^(+) + e^- to Cu E^(@) = 0.5 volt Calculate potential for Cu^(2+) + 2e^(-) to Cu

Given: (i) Cu^(2+)+2e^(-) rarr Cu, E^(@) = 0.337 V (ii) Cu^(2+)+e^(-) rarr Cu^(+), E^(@) = 0.153 V Electrode potential, E^(@) for the reaction, Cu^(+)+e^(-) rarr Cu , will be