Depict the galvanic cell in which the reaction
`Zn(s)+2Ag^(+)(aq)toZn^(2+)(aq)+2Ag(s)` takes place. Further show:
(i) which of the electrode is negatively charged?
(ii). The carriers of the current in the cell.
(iii). Individual reaction at each electrode.

Explanation

The given reaction can be split into two half-cell reactions as :
At anode: `Zn(s) to Zn_((aq))^(2+) + 2e^(-)` (oxidation)
At cathode : `2Ag_((aq))^(+) +2e^(-) to 2Ag(s)` (reduction)
Since oxidation occurs at the anode or negative electrode of the cell, the anode is represented as `Zn//Zn^(2+)`.
As the reduction takes place at the cathode, or positive electrode of the cell, cathode is represented as `Ag^(+)//Ag`.
Combining the anode and cathode electrodes, using salt bridge, the galvanic cell is depicted as:
`Zn(s) "|"Zn^(2+) (aq)"||"Ag^(+)(aq) "|"Ag(s)`
(i) Zinc electrode (anode) is negatively charged.
(ii) The reaction taking place are as shown above.
(iii) The current is carried by ions within the cell, i.e., `Zn^(2+)` and `Ag^(+)` ions and by electrons outside the cell.