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

To understand in which galvanic cell the reaction \(\frac{1}{2}\)H₂(g) + AgCl(s) → H⁺(aq) + Cl^-(aq) + Ag(s) occurs, let's analyze the given options and the corresponding reactions: 

1. Ag | AgCl(s) | KCl(solⁿ) || AgNO₃ | Ag:
   • This configuration does not involve the required hydrogen electrode for the reaction with H₂ gas, making it unrelated to the given reaction.
2. Pt | H₂(g) | HCl(solⁿ) || AgNO₃ (solⁿ) | Ag:
   • This setup involves a hydrogen electrode, but the presence of AgNO₃ on the other side is not suitable for the deposition of Ag from AgCl, not fulfilling the given reaction.
3. Pt | H₂(g) | HCl(solⁿ) || AgCl(s) | Ag:
   • This setup is the correct configuration. Here's why:
     • The left side is a hydrogen electrode where \(\frac{1}{2}\)H₂(g) can produce H⁺ ions.
     • The right side has AgCl(s) which disassociates to Cl^- and allows Ag(s) to precipitate.
     • The given reaction shows H₂ reacting with AgCl, making this galvanic cell the correct match.
4. Pt | H₂(g) | KCl(solⁿ) || AgCl(s) | Ag:
   • Although AgCl and Ag are present, the KCl solution does not provide the necessary HCl for the reaction, unlike the HCl solution needed to provide H⁺ ions for the specified reaction.

On reviewing all the options, the galvanic cell Pt | H₂(g) | HCl(solⁿ) || AgCl(s) | Ag is the one where the reaction efficiently proceeds as described, involving the correct components and conditions.