In the galvanic cell Zn(s)│Zn2+(aq) || Ag+(aq)│Ag(s), which species is reduced at the cathode?

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Multiple Choice

In the galvanic cell Zn(s)│Zn2+(aq) || Ag+(aq)│Ag(s), which species is reduced at the cathode?

Explanation:
In a galvanic cell, the cathode is where reduction happens, with electrons flowing toward it from the anode. Here, zinc metal is oxidized at the anode to Zn2+(aq), releasing electrons: Zn(s) → Zn2+(aq) + 2 e−. Those electrons travel to the cathode, where they reduce the silver ions in solution: Ag+(aq) + e− → Ag(s). So the species being reduced at the cathode is the silver ions in solution, Ag+(aq). The other listed species either are oxidized at the anode (Zn(s) and Zn2+(aq) are related to the oxidation process) or are the solid product formed by reduction (Ag(s) is the reduced metal, formed from Ag+(aq)).

In a galvanic cell, the cathode is where reduction happens, with electrons flowing toward it from the anode. Here, zinc metal is oxidized at the anode to Zn2+(aq), releasing electrons: Zn(s) → Zn2+(aq) + 2 e−. Those electrons travel to the cathode, where they reduce the silver ions in solution: Ag+(aq) + e− → Ag(s). So the species being reduced at the cathode is the silver ions in solution, Ag+(aq). The other listed species either are oxidized at the anode (Zn(s) and Zn2+(aq) are related to the oxidation process) or are the solid product formed by reduction (Ag(s) is the reduced metal, formed from Ag+(aq)).

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