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Represent the cell in which the following reaction takes place Mg(s)+2Ag^(+)(0.001M) to Mg^(2+)(0.130)+2Ag(s) Calculate E_("cell")" if "E_("cell")^(0)=3.17V. |
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Answer» Solution :Represent of the cell `Mg//Mg^(2+)(0.130M)||Ag^(+)(0.01M)//Ag` Cell reaction `Mg+2Ag^(+) to Mg^(2+)+2Ag` FORMULA: `E_("cell")=E_("cell")^(0)-(0.059)/(N)LOG""([Mg^(2+)])/([Ag^(+)]^(2)]` Substitution `E_("cell")=3.17-(0.059)/(2)log"" ([0.130])/([0.0001)]^(2))` =2.96V |
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