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`.

Explanation

Cell reaction is as follows : `Mg(s)+2Ag(aq)rarrMg^(2+)(aq)+2Ag(s)`
According to Nernst equation
`E_("Cell")=E_("Cell")^(@)-(0.0591)/(n)log""([Mg^(2+)])/([Ag^(+)]^(2))E_("cell")^(@)=3.17V`
`E_("Cell")=3.17-(0.0591)/(2)log""(0.130)/(0.0001)`
`E_("Cell")=3.17-(0.0591)/(2)[log0.130-log10^(-4)]`
`E_("Cell")=3.17-(0.0591)/(2)[-1.139+4]`
`E_("Cell")=3.17-(0.0591)/(2)[2.861]=3.17-0.08=3.0V`