Write each half cell reaction of the following electrochemical cell:
`Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)`

Write each half cell reaction of the following electrochemical cell: Al(s)|Al^(3+)(1M)||Zn^(2+)(1M)|Zn(s)

Write each half cell reaction of the following electrochemical cell: Na(s)|Na^(+)(1M)||Fe^(3+)(1M)|Fe(s)

Derive Nernst equation for the following cell: Cu|Cu^(2+)(0.1M)||Ag^(+)(0*1M)|Ag

Write Nernst equation and cell reaction of the following cell: Zn|Zn^(2+)||Cu^(2+)|Cu

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.

For an electrochemical cell Cu//Cu^(2+) (XM)||Ag^(+) (Ym)//Ag . The cell reaction is

Write Nernst equation and calculate the e.m.f. of the following cell at 298 K: Cu(s)|Cu^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag(s) Given that: E_(Cu^(2+)//Cu)^(@)=+0.34V and E_(Ag^(+)//Ag)^(@)=+0.80V (log 0.130=-1.1139).

Write Nernst equation and calculate e.m.f. of the following cell at 298 k. Mg(s)|Mg^(2+)(0.130M)||Ag^+(0.0001M)|Ag(s) Given E^o(Mg^(2+)//Mg)=-2.37 V E^o(Ag^(+)//Ag)=0.80 V (log 1.3=0.1130)

Represent the cell in which the following reaction takes place: Mg(s)+Cu^(2+)(0.0001M) to Mg^(2+)(0.1M)+Cu(s) . Calculate its E, if E^(@) is 2.71V .

Write Nernst equation and calculate emf for the following cell: Zn|Zn^(2+)(0*01M)||Ag^(+)(0*01M)|Ag .