8.30. 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 current in the cell and
(iii) Individual reaction at each electrode. (Advance)

<p>The given redox reaction can be depicted as</p><p>Zn (s) + 2Ag⁺ (aq) <strong>→ </strong>Zn²⁺ (aq) + 2Ag (s)<br>Since Zn gets oxidised to Zn²⁺&nbsp;ions, and Ag⁺&nbsp;gets reduced to Ag metal, therefore, </p><p>Oxidation occurs at the zinc electrode and reduction occurs at the silver electrode. Thus, galvanic cell corresponding to the above redox reaction may be depicted as:</p><p>Zn|Zn²⁺ (aq) | Ag⁺ (aq) | Ag</p><p><strong> (i) </strong>Zinc electrode is negatively charged because oxidation occurs at the zinc electrode (i.e. electrons accumlulate on the zinc electrode)</p><p>&nbsp;</p><p><strong> (ii)</strong> The ions carry current. The electrons flow from Zn to Ag electrode while the current flows from Ag to Zn electrode.</p><p>&nbsp;</p><p><strong> (iii)</strong> Reaction occurring at each electrode are:</p><p>Zn (s) → Zn²⁺ (aq) + 2e^-</p><p>Ag⁺ (aq) + e^- → Ag (s)</p>

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