What is the electochemical series? Write one application of electochemical series. Calculate the standard electrode potential of `Ni^(2+)|Ni` electrode, if the cell potential fo the cell:
`Ni|NI^(2+)(0.01M)||Cu^(2+)(0.1M)|Cu` is 0.59V.

Calculate the standard electrode potential of Ni2+/Ni electrode if emf of the cell Ni |Ni2+(0.01 M)||Cu2+(0.1 M)| Cu(s) is 0.59 V at 25°C [Given: Ecu2+Icu = +0.34 v]

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

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

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)

Write the Nernst equation and emf of the following cells at 298 K: Mg(s)|Mg^(2+)(0.001M) || Cu^(2+)(0.0001 M)| Cu(s)

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 standard reduction potential for Cu^(2+)|Cu is +0.34V. Calculate the reduction potential at pH=14 for above couple. K_(sp) of Cu(OH)_2 is 1.0xx10^-19 .

Calculate the reduction potential of the following electrode at 298K Pt,Cl_2(2.5atm)|HCl(0.01M), E^@ Cl_2|2Cl^-=1.36V .

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

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