Question

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

Answer 1

The cell is represented as mg `[Mg^(2+)(0.130M)|Ag^(+)(0.0001M)]Ag`
`E_("cell")=E_((cell)) ^(Θ)-(RT)/(2F) ln ""([Mg^(2)+])/([Ag^(+)]^(2))`
`=3.17V-(0.59V)/(2)log ""(1.130)/((0.0001)^(2))=3.17 V-0.21V=2.96V`