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A galvanic cell is constructed using the redox reaction,
$\frac{1}{2} \mathrm{H}_{2}(g)+\operatorname{AgCl}(s) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{Cl}^{-}(a q)+\operatorname{Ag}(s)$
it is represented as
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$\frac{1}{2} \mathrm{H}_{2}(g)+\operatorname{AgCl}(s) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{Cl}^{-}(a q)+\operatorname{Ag}(s)$
it is represented as
Solution:
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Verified Answer
The correct answer is:
$\mathrm{Pt}\left|\mathrm{H}_{2}(g), \mathrm{HCl}(\operatorname{sol})\right||\operatorname{AgCl}(s)| \mathrm{Ag}$
At anode, oxidation occurs of $\mathrm{H}_{2}$ (gas), while at cathode reduction of $\mathrm{AgCl}$ take place.
$\therefore$ The cell notation is
$\mathrm{Pt}\left|\mathrm{H}_{2}(\mathrm{~g}), \mathrm{HCl}(\mathrm{sol}) \| \mathrm{AgCl}(s)\right| \mathrm{Ag}$
$\therefore$ The cell notation is
$\mathrm{Pt}\left|\mathrm{H}_{2}(\mathrm{~g}), \mathrm{HCl}(\mathrm{sol}) \| \mathrm{AgCl}(s)\right| \mathrm{Ag}$
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