Represent a cell consisting of `Mg | Mg^(2+)` ||`Ag^(+) | Ag` half cell and write the cell reaction. `(E_(Ag^+//Ag)^(@)=0.799V, E_(Mg^(2+)//Mg)^(@)=-2.37V)`

Explanation

`Mg_((s))|Mg_((aq))^(2+)||Ag_((aq))^(+)|Ag_((s))`
At anode :
`Mg_((s))rarr Mg_((aq))^(2+)+2e^(-)`
At cathode :
`Ag_((aq))^(+)+e^(-)rarrAg_((s))`
Net reaction :
`Mg_((s))+2Ag_((aq))^(+)rarrMg_((aq))^(2+)+2Ag_((s))`
`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)`
`=0.799-(-2*37)`
`=3*169`