Depict the galvanic cell in which the reaction $Z n (s) + 2 A g^{+} (a q) \to Z n^{2 +} (a q) + 2 A g (s)$ 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.

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Solution

The galvanic cell in which the given reaction takes place is depicted as:
$Z n (s) | Z n^{2 +} (a q) | | A g^{+} (a q) | A g (s)$
(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: $Z n (s) \to Z n^{2 +} (a q) + 2 e^{-}$
Reduction at cathode: $A g^{+} (a q) + e^{-} \to A g (s)$

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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.

Depict the galvanic cell in which the reaction $Z n (s) + 2 A g^{+} (a q) \to Z n^{2 +} (a q) + 2 A g (s)$ 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.