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

The standard reduction potential of Zn-electrode is -0.76V. The standard oxidation potential of the electrode will be ______________.

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

Zn - granules are added in excess to 500 mL of 1.0 M nicke nitrate solution at 25^(@)C until the equilibrium is reached. If standard reduction potential of Zn^(2+)|Zn and Ni^(2+)|Ni are -0.75V and -0.24V , respectively, find out the concentration of Ni^(2+) in solution at equilibrium.

The standard reduction potential of metals A, B and C are -2.37V, +1.85V and +1.36V , respectively. What will be the order of reducing power of the metals?

The standard reduction potential of metals A, B, C and D are +0.80V, -0.76V, +0.20V and +0.38V respectively. Arrange the metals in the ascending order of their electropositivity.

The standard reduction potential for the reaction Sn^(4+) + 2erarr Sn^(2+) is + 0.15 V . Calculate the free energy change of the reaction.

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-

Why standard reduction potential (E^(0)) of Zn^(2+)|Zn system is more negative than expected ?