The standard reduction potential of Pb and Zn electrodes are `-0.126` and `-0.763 V` respectively. The cell equation will be

The standard reduction potential of Pb and Zn electrodes are -0.126 and -0.763 volts respectively . The e.m.f of the cell Zn|Zn^(2+)(0.1M)||Pb^(2+)(1M)Pb is

The standard reduction potential of Pb and Zn electrodes are -0.12 6 and -0.763 volts respectively . The e.m.f of the cell Zn|Zn^(2+)(0.1M)||Pb^(2+)(1M)|Pb is

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?

The standard reduction potentials of magnesium and iron electrodes are -2.73 V and -0.44 V respectively. Which electrode will undergo oxidation and which electrode reduction ?

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.

Fill in the blanks : The standard reduction potentials of Cu and Zn are 0.34V and -0.76 V respectively. The emf of the cell formed by combining the two electrodes will be ………….

The standard reduction potential for Fe^(2+) | Fe and Sn^(2+) | Sn electrodes are -0.44V and -0.14V respectively. For the cell reaction, Fe^(2+)+Sn rarr Fe +Sn^(2+) , the standard emf is :

The standard electrode potential for Pb^(2+)"|"Pb and Zn^(2+)"|"Zn are -0.126 V and -0.763 V respectively. The e.m.f. of the cell Zn"|"Zn^(2+)(0.1M)"||"Pb^(2+)(0.1M)"|"Pb is :

The e.m.f. of the cell Zn"|"Zn^(2+)(0.1M)"||"Pb^(2+)(0.1M)"|"Pb is ( standard electrode potentials for Pb^(2+)"|"Pb "and " Zn^(2+)"|"Zn electrode are - 0.126 V and - 0.763 V respectively.)