Zn2+
(aq) + 2Ag(s) takes place. Further tell
(i) Which of the electrode is
negatively charged.
(ii) The carriers of the current
in the cell
(iii) Individual reaction at each electrode.
Answer:
The cell is depicted as:
Zn | Zn2+ (aq) || Ag+ (aq)| Ag
(i) Zinc electrode is negatively
charged electrode.
The electrons thus released move
through the metal to reach another spot where H+ ions and the
dissolved oxygen take up these electrons and reduction reaction takes place.
Hence, this spot acts as the cathode:
O2(g) + 4H+
(aq) + 4e? 
2H2O(l)
The overall reaction is:
Thus, an electrochemical cell is
set up on the surface.
Ferrous ions are further oxidized
by the atmospheric oxygen to ferric ions which combine with water molecules to
form hydrated ferric oxide, Fe2O3.xH2O, which
is rust.
(ii) The ions formed i.e., Zn2+
and Ag+ in the solution are the carriers of the current with in the
cell.
(iii) At anode: 
At cathode: 
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