Depict the galvanic cell in which the reaction Zn(s)+2Ag⁺(aq) → Zn²⁺(aq)+2Ag(s) takes place. Further show: (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.
The zinc (Zn) electrode is negatively charged.
Electrons are the carriers of the current in the external circuit.
Anode (Oxidation): Zn(s) → Zn²⁺(aq) + 2e⁻ Cathode (Reduction): 2Ag⁺(aq) + 2e⁻ → 2Ag(s)
Explanation
The answer is derived by comparing the given reaction to the Daniell cell example provided in the context. The context establishes that Zinc acts as the anode (oxidation) and is placed on the left, while the other species (Ag⁺) acts as the cathode (reduction) on the right. Since the text states that electrons flow from the Zn rod, the Zn electrode is the negative terminal. The reactions are written as half-cells similar to the examples given for Zn and Cu in the text.