The reaction \(\frac{ 1}{2}\)H2(g) + AgCl(s) → H+(aq) + Cl-(aq) + Ag(s) occurs in which of the given galvanic cell.
- Ag | AgCl(s) | KCl(sonn) || AgNO3 | Ag
- Pt | H2(g) | HCl(soln) || AgNO3 (soln) | Ag
- Pt | H2(g) | HCl(soln) || AgCl(s) | Ag
- Pt | H2(g) | KCl(soln) || AgCl(s) | Ag
The Correct Option is C
Solution and Explanation
The given reaction involves the oxidation of hydrogen gas to H$^+$ ions and the reduction of AgCl to Ag. This is consistent with the following electrode reactions:
Anode (oxidation): H$_2 \to$ 2H$^+ + 2e^-$
Cathode (reduction): AgCl + e$^- \to$ Ag + Cl$^-$ \end{itemize}
The correct galvanic cell setup corresponding to this reaction is: \[ \text{Pt} \vert \text{H}_2(\text{g}) \vert \text{HCl(sol$^n$)} \vert \text{AgCl(s)} \vert \text{Ag} \] Here, the HCl provides the H$^+$ ions required for the anode reaction, and AgCl serves as the source of Ag$^+$ for the cathode reaction.
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