Question

The reaction \(\frac{ 1}{2}\)H₂(g) + AgCl(s) → H⁺(aq) + Cl^-(aq) + Ag(s) occurs in which of the given galvanic cell.

• A. Ag | AgCl(s) | KCl(sonⁿ) || AgNO₃ | Ag
• B. Pt | H₂(g) | HCl(solⁿ) || AgNO₃ (solⁿ) | Ag
• C. Pt | H₂(g) | HCl(solⁿ) || AgCl(s) | Ag
• D. Pt | H₂(g) | KCl(solⁿ) || AgCl(s) | Ag

Answer 1

The Correct Option is C

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.