Represent the cell in which the following reaction takes place `Mg(s) + 2Ag^+(0.0001M) to Mg^(2+)(0.130M) + 2Ag(s)` Calculate its `E_(cell)` if `E_(cell)` = 3.17 V.

Explanation

Cell reaction is,
`Mg(s)+2Ag^(+)(aq) to Mg^(2+)(aq)+2Ag(s)`
Half cell reactions and overall reaction are,
`Mg(s) to Mg^(2+)(aq) +2e^(-)`
`2Ag^(+)(aq)+2e^(-) to 2Ag(s)`
`2Ag^(+)(aq)+Mg(s) to Mg^(2+)(aq)+2Ag(s)`
Cell representative `Mg|Mg^(2+)||Ag^(+)|Ag`
Here n=2
Nernst equation (at 298K) is,
`EMF=EMF^(@)-(0.0591V)/(n)logQ_(C)`
`=EMF^(@)-(0.0591V)/(2)"log"([Mg^(2+)])/([Ag^(+)]^(2))`
`3.17V-(0.0591V)/(2)"log"(0.130)/((0*0001)^(2))`
`=3*17V-0.0295V"log"(1.3xx10^(-1))/([10^(-3)]^(2))`
`=3.17V-0.0295V" "log1.3xx10^(7)`
`=3.17V-0.0295V[7*1139]`
`=(3.17-0.21)V`
`=2.96V`