Consider the cell: `Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s)` its e.m.f. is `2.96V.` calculate `E_("cell")^(@)` `(R=8.314JK^(-1),1F=96500Cmol
Consider the cell:
`Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s)`
its e.m.f. is `2.96V.` calculate `E_("cell")^(@)`
`(R=8.314JK^(-1),1F=96500Cmol^(-1))`
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1 Answers
Given: For electro chemical cell `Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s),E_(cell)=2.96V`
Asked `E_(cell)=E_(cell)^(@)-(0.0591)/(n)log((["product"])/(["reactant"]))`
Expalanation `E_(cell)^(@)="standard" e.m.f of cell
`E_(cell)=e.m.f` of cell
Substitution and calculation
`Mg(s)toMg^(2+)(aq)+2e^(-)` underline(2Ag^(+)(aq)2e^(-)to2Ag(s))`
`underline(Mg(s)+2Ag^(2+)(aq)toMg^(2+)(aq)+2Ag(s))`
`E_(cell)^(@)=E_(cell)^(@)=-(0.591)/(2)log(([Mg^(2+)])/([Ag^(+)]^(2)))implies+2.96V=E_(cell)^(@)-(0.0591)/(2)log((0.13)/((10^(-4))^(2)))`
`E_(cell)^(@)=3.169V`
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