`E^(@)` of Cu is +0.34 V while that of Zn is -0.736 V. Explain.

E^(Theta) of Cu is +0.34V while that of Zn is -0.76 V. Explain.

The E^(@) value of Zn is -0.76 V while that of Cu is +0.34 V. Do these values help in locating the relative positions of the electrodes in the electrochemical series ?

The standard electrode potential of Zn^(2+) // Zn is -0.76V and that of Ca^(2+) // Cu is 0.34V . The emf(V) and the free energy change (kJ "mol"^(-1)) , respectively , for a Daniel cell will be

E^@ values for the half cell reactions are given below : Cu^(2+) + e^(-) to Cu^(+) , E^@ =0.15 V Cu^(2+) + 2e^(-) to Cu, E^@ =0.34 V What will be the E^@ of the half-cell : Cu^(+) + e^(-) to Cu ?

The standard oxidation potential of Zn referred to SHE is 0.76 V and that of Cu is -0.34V at 25^(@)C when excess of Zn is added to CuSO_(4) , Zn displaces Cu^(2+) till equilibrium is reached. What is the approx ratio of Zn^(2+) to Cu^(2+) ios at equilibrium?

The e.m.f of galvanic cell , with oxidation potentials of Zn = +0.76 V and that of Cu = -0.34 V , is ________.