Electrochemistry - Result Question 72
####20. The reaction,
$$ \frac{1}{2} H _2(g)+AgCl(s) \rightleftharpoons H^{+}(a q)+Cl^{-}(a q)+Ag(s) $$
occurs in the galvanic cell
$(1985,1 M)$
(a) $Ag|AgCl(s)| KCl$ (soln) $\left|AgNO _3\right| Ag$
(b) $Pt\left|H _2(g)\right| HCl$ (soln) $\mid AgNO _3$ (soln) $\mid Ag$
(c) $Pt \mid H _2(g) HCl$ (soln) $|AgCl(s)| Ag$
(d) $Pt\left|H _2(g)\right| KCl($ soln $)|AgCl(s)| Ag$
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Solution:
- In a galvanic cell, oxidation occur in the left hand electrode chamber and reduction in right hand electrode chamber. In the following cell.
$$ Pt\left|H _2(g)\right| HCl(l) | AgCl(s) \mid Ag(s) $$
The cell reactions are :
$$ \begin{gathered} \frac{1}{2} H _2(g) \longrightarrow H^{+}+e^{-} \quad \begin{array}{l} \text { At anode } \ AgCl(s)+e^{-} \longrightarrow Ag+Cl^{-} \quad \text { At cathode } \end{array} \ \text { Net }: \frac{1}{2} H _2(g)+AgCl(s) \longrightarrow H^{+}+Ag(s)+Cl^{-} \end{gathered} $$
