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 that 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: \[\ce{Ag+_{( aq)} + e- -> Ag_{(s)}}\]