Question

Depict the galvanic cell in which the reaction takes place.

\[\ce{Zn_{(s)} + 2Ag+_{ (aq)} -> Zn^{2+}_{ (aq)} + 2Ag_{(s)}}\]

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 galvanic cell corresponding to the given redox reaction can be represented as:

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

1. Zn electrode is negatively charged because at this electrode, Zn oxidizes to Zn²⁺and the leaving electrons accumulate on this electrode.
2. Ions are the carriers of current in the cell.
3. The reaction taking place at Zn electrode can be represented as:
   \[\ce{Zn_{(s)} -> Zn^{2+}_{ (aq)} + 2e-}\]
   And the reaction taking place at Ag electrode can be represented as:
   \[\ce{Ag^+_{ (aq)} + e- -> Ag_{(s)}}\]