The e.m.f of the cell
`Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1xx10^-xM)|Cu` is 2.651 V. The standard e.m.f of the cell is 2.71 V. the value of x is

The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is

For the cell, Tl|Tl^+(0.001)||Cu^(2+)(0.1M)|Cu , E_(cell) at 25^@C is 0.826V. The e.m.f can be increased

Write the half cell reaction and the overall cell reaction for the electrochemical cell: Zn|Zn^(2+)(1.0M)||Pb^(2+)(1.0M)|Pb Calculate the standard e.m.f. for the cell if standard electrode potentials for Pb^(2+)|Pb and Zn^(2+)|Zn electrodes are -0.126V and -0.763V respectively.

The e.m.f of the cell Cu|Cu^(2+)(aq)||Ag^(+)(aq)|Ag is 0.46V. The e.m.f for the following cell reaciton: 3Cu+6Ag^+ (aq)rarr3Cu^(2+)+6Ag is 0.46y V. The value of y is

Calculate the e.m.f. of the following cell at 298 K, Mg|Mg^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag

What is the standard e.m.f. of the cell containing Sn^(2+)|Sn and Br_2|Br^- electrodes?

Derive Nernst equation for the following cell: NiNi^(2+)(0*2M)||Cu^(2+)(0*2M)|Cu .

Write Nernst equation and calculate e.m.f. of the cell at 298 k. Mg(s)|Mg^(2+)(0.001 M)||Cu^(2+)(0.0001M)|Cu(s)

Give the Nernst equation of the cell: Ni(s)|NI^(2+)(aq)(0.1M)||Ag^(+)(aq)(0.1M)|Ag(s) and also find the cell potential. given that E^@(Ag^+|Ag)=0.80V, E^@(Ni^(2+)|Ni)=-0.25V

Calculate the e.m.f. of the following cell at 298 K. Mg_((s))|Mg^(2+)(0.001M)||Cu^(2+)(0.0001M)|Cu_((s)) Given E^(@)(Cu^(2+)|Cu)=0.34V and E^(@)(Mg^(+)|Mg)=-2.37V .