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

Explanation

`Ni//Ni^(2+)(0*2M)||Cu^(2+)(0*2M)|Cu`
The reaction involved an this cell are:
Oxidation: `Ni(s) to Ni^(2+)(aq)+2e^(-)`
Reduction: `Cu^(2+)(aq)+2e^(-) to Cu(s)`
Over all: `Cu^(2+)(aq)+Ni(s)toCu(s)+Ni^(2)(aq)`
Here n=2
`therefore`Nernst equator for the cell is,
`EMF=EMF^(@)-(2*303RT)/(nF)logQ_(C)`
`EMF=EMF^(@)-(0.0591)/(2)"log"([Ni^(2+)])/([Cu^(2+)])` at (298 K)