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

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

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 -0.126 and -0.763 V respectively. The cell equation will be

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 standard electrode potential of Zn^(2+)|ZnandCu^(2+)|Cu are - 0.76 and 0.34 V respectively . The standard e.m.f. of the cell 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?

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.

The standard reduction potential of Zn^(2+)|Zn and Cu^(2+)|Cu are -0.76V and +0.34 V respectively. What is the cell e.m.f (in V) of the following cell? ((RT)/(F)=0.059) Zn//Zn^(2+)" "(0.05M)//Cu^(2+)(0.005M)//Cu