Consider the following electrochemical cell. (a). Write a balanced net ionic equation for the spontaneous reaction that take place in the cell. (b). Calculate the standard cell potential E^(0) for the cell reaction. (c). If the cell emf is 1.6V what is the concentration of Zn^(2+)? (d). How will the cell potential be affected if Kl is added to Ag^(+) half-cell?

Consider the following electrochemical cell. (a). Write a balanced

1.	Consider the following electrochemical cell. (a). Write a balanced net ionic equation for the spontaneous reaction that take place in the cell. (b). Calculate the standard cell potential E^(0) for the cell reaction. (c). If the cell emf is 1.6V what is the concentration of Zn^(2+)? (d). How will the cell potential be affected if Kl is added to Ag^(+) half-cell?
Answer» Solution :(a) The SPONTANEOUS reaction taking place in the cell is : `Zn(s)+2AG^(+)(aq) to Zn^(2+)(aq)+2Ag(s)` (b) `E_(cell)^(@)=E_(cathode)^(@)-E_(anode)^(@)=0.80-(-0.76)=1.56V` (c ) ACCORDING to Nernst equation : `E_(cell)=E_(cell)^(@)-(0.0591)/(2)"log"([Zn^(2+)])/([Ag^(+)]^(2))` `1.60=1.56-(0.0591)/(2)"log"([Zn^(2+)])/((0.1)^(2))` `0.04=-0.02955" log"([Zn^(2+)])/((0.01))` `"log"([Zn^(2+)])/((0.01))=(0.04)/((-0.02955))=-1.356` `([Zn^(2+)])/(0.01)="Antilog"(-1.356)="Antilog"(overset(-)(2).644)4.4xx10^(-2)` `[Zn^(2+)]=4.4xx10^(-4)M` (d) On adding KI solution to `Ag^(+)//Ag` half-cell (cathode half cell) `Ag^(2+)` ions will be precipiated as Agl. Thus, the `[Ag^(+)]` will decrease and `E_(cell)` will reduce according to the Nernst equation. `Ag^(+)+I to Agl`.