The standard electrode potential of `Cu^(2+)|Cu` half cell is `+0.34V`. What does it mean?

Consider the following four electrodes : P=Cu^(2+)"(0.001 M)|Cu(s) Q=Cu^(2+)("(0.1 M)"|Cu(s) R=Cu^(2+)"(0.01 M)"|Cu(s) S=Cu^(2+)"(0.001)"|Cu(s) If the standard electrode potential of Cu^(2+)|Cu is +0.34V , the reduction potential in volts of the above electrodes follows the order-

The standard electrode potential of Daniell cell is 1.1V. Calculate the standard Gibbs energy for the reaction : Zn(s)+Cu^(2+)(aq)rarr Zn^(2+)(aq)+Cu(s)

The standard reduction potential of Zn^(2+)|Zn electrode is -0.76 V . What will be the electrode reactions if this electrode is coupled with a standard hydrogen electrode?

The standard reduction potential of Zn is -0.76V and that of Cu is +0.34V . What do they indicate?

The positive value of the standard electrode potential of Cu^(2+)|Cu indicates that -

At 25^(@)C , the reduction potential of Cu^(2+)|Cu half - cell is 0.28V. If E^(@) of Cu^(2)|Cu half-cell is +0.34V , find the molar concentration of Cu^(2+) ion in the half - cell.

Determination of the electromotive force of a galvanic cell. Given: Standard electrode potential of the half - cells & molar concentrations of different constituents participating in cell reaction.

Standard reduction potential for Cu^(2+)|Cu is +0.34V . Calculate the reduction potential at pH = 14 for the above couple. K_(sp) of Cu(OH)_(2) is 1.0xx10^(-19) .

A cell is prepared by dipping a zinc rod in 1(M) ZnSo_4 solution. The standard electrode potential for Pb^(2+)/ Pb and Zn^(2+) /Zn electrodes are -0.126V and -0.763 V respectively. Write the half cell reactions and overall cell reaction.

A cell is prepared by dipping a zinc rod in 1(M) ZnSo_4 solution. The standard electrode potential for Pb^(2+)/ Pb and Zn^(2+) /Zn electrodes are -0.126V and -0.763 V respectively. How will you represent the cell?