Represent the cell in which following reaction takes place `:`
`Mg(s)+2Ag^(o+)(0.0001M)rarr Mg^(2+)(0.130M)+2Ag(s)` calculate its `E_(cell)` if `E^(c-)._(cell)=3.17V. `

Explanation

The cell may be represented as `Mg|Mg^(2+) (0.130 M) || Ag^(+) (0.0001 M) |Ag`
The cell reaction for the cell is
`Mg (s) + 2 Ag^(+) (aq) to Mg^(2+) (aq) + 2 Ag (s)`
The Nernst equation for the cell is
`E = E^(Theta) - (0.059)/(2 ) "log" ([Mg^(2+)])/([Ag^(+)]^(2))`
`= 3.17 - (0.059)/(2) "log" ((0.130))/((0.0001)^(2))`
= `3.17 - 0.21 = 2.96 V `