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

(a). The spontaneous cell reaction: `Zn+2Ag^(+)(aq)hArrZn^(2+)(aq)+2Ag(s)`
(b). `1.56V`
(c). `[Zn^(2+)[=4xx10^(-4)M`
(d). As we add Kl to cathode chamber, some `Ag^(+)` wll precipitate out as:
`Ag^(+)+I^(-)toAgl`
The above reaction reducing `[Ag^(+)]` from cathode chamber. this will reduce `E_(cell)` according to nernst's equations