Question

Depict the galvenic cell in which the reaction
Zn_(s) + 2Ag⁺_(aq) → Zn²⁺_(aq) + 2Ag_(s) takes place. Further, show,
(i) Which of the electrodes is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

Answer 1

The given chemical reaction is as follows
Zn_(s) + 2Ag⁺_(aq) → Zn²⁺_(aq) + 2Ag_(s)
Cell can be represented as,
Zn_(s)/Zn²⁺_(aq) || Ag⁺_(aq)/Ag_(s)
(i) The electrode at which oxidation takes place, behaves as anode and it is negatively charged. Hence zinc electrode is negatively charged.
(ii) In the cell, the carriers of the current are electrons. and the current will flow from silver to copper in the external circuit.
(iii) The reactions on each electrode are as follows.
At anode: Zn_(s) → Zn²⁺_(aq) + 2e^–
At cathode: Ag⁺_(aq) + e^– → Ag_(s)
It can be represented by the following diagram.