Ni(s) + 2Ag+ (aq) → Ni2+ (aq) + 2Ag(s)
For the above reaction depict the cell, individual half reactions and predict which one is cathiode and anode.
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The galvanic cell in which the given reaction takes place is depicted as:
Zn(s)∣Zn
2+
(aq)∣∣Ag
+
(aq)∣Ag(s)
(i) The negatively charged electrode is the zinc electrode. It acts as an anode.
(ii) In the external circuit, the current will flow from silver to zinc.
(iii) Oxidation at anode: Zn(s)→Zn
2+
(aq)+2e
−
Reduction at cathode: Ag
+
(aq)+e
−
→Ag(s)
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