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Represent the cell in which the followig reaction takes place, Mg_((s))+2Ag_((0.0001M))^(+)to Mg_((0.130M))^(2+)+2Ag_((s)) Calculate its E_(cell) if E_(cell)^(Theta)=3.17V |
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Answer» Solution :In this cell `Mg_((s))|Mg^(2+)` is anode because Mg get oxidized and also `Ag^(+)` is reduced in Ag so on cathode `Ag^(+)|Ag` will be on RIGHT side. Between these two ELECTRODES salt bridge is DENOTED by two verticle line || and hence the symbolic representation of cell will be `Mg_((s))|Mg_((0.130M))^(2+)||Ag_((0.0001M))^(+)|Ag_((s))` Calculation for `E_(cell)` potential is as follows: `E_(cell)=E_(cell)^(Theta)-(RT)/(nF)LN([Mg^(2+)])/([Ag^(+)]^(2))` `therefore E_(cell)=3.17V-(0.0591)/(2)"log"([Mg^(2+)])/([Ag^(+)]^(2))` `=3.17V-(0.0591)/(2)"log"(0.130)/((0.0001)^(2))` `=3.17-0.2955log(1.33xx10^(+7))` `=3.17-0.2955(+7.1139)` `=3.17-0.2099=3.17-0.21=2.96V` |
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