Question

Depict the galvanic cell in which the reaction \[\ce{Zn(s) + 2Ag+(aq) → Zn^{2+}(aq) + 2Ag(s)}\] takes place. Further show:

1. Which of the electrode is negatively charged?
2. The carriers of the current in the cell.
3. Individual reaction at each electrode.

Answer 1

The set-up will be similar to as shown below:

The cell will be represented as:

\[\ce{Zn(s) | Zn^{2+}(aq) || Ag^+(aq) | Ag(s)}\]

1. Anode, i.e., zinc electrode, will be negatively charged.
2. The current will flow from silver to zinc in the external circuit.
3. At anode: \[\ce{Zn(s) -> Zn^{2+}(aq) + 2e–}\]
   At cathode: \[\ce{Ag+(aq) + e– -> Ag(s)}\]