Civen `E^@` for ` Cu^(2+) rarr Cu^+ ` is ` + 0.15 V` and ` Cu^+ rarr Cu ` is ` +0.05 V`
Calculate ` E^@` for ` Cu^(2+) rarr Cu`.

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

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:

Cu^(2+)+ 2e rarr Cu and Cu-Ze rarr Cu6(2+) . Which one occurs at cathod?

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: (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

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

The electrode potential for Cu^(2+)(aq)+e rarr Cu^(+)(aq) and Cu^(+)(aq)+e rarr Cu(s) are 0.15V and 0.50V respectively. The value of E_(Cu^2+)|Cu^(@) will be -