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?

Standard electrode potential of three metals X, Y and Z are -1.2V, 0.5V and-3.0V respectively. The reducing power of these metals will be -

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

The standard reduction potentials for Zn^(2+)|Zn, Ni^(2+)|Ni and Fe^(2+)|Fe are -0.76, -0.23 and 0.44V respectively. The reaction x+y^(2+)rarr x^(2+)+y will be spontaneous when -

The standard electrode potantials of the half cells Ag^(+)//Ag and Fe^(3+),Fe^(2+)//Pt are 0.7991V and 0.771V respectively. Calculate the equilibrium constant of the reaction : Ag_((s))+Fe^(3+)hArr Ag^(+)+Fe^(2+)

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

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.

Write the electrode reaction occurring in H_(2)-O_(2) fuel cell.

A galvanic cell is made by dipping a Zn - rod in 0.1 (M) Zn(NO_(3))_(2) and a Pb - rod in 0.25 (M) Pb(NO_(3))_(2) solution. Calculate EMF of the cell, write the cell reaction and represent the cell. Given : E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Zn^(2+)|Zn)^(@)=-0.77V.