The reaction;
1/2 H_(2( g))+AgCl₍ₛ₎ → H_((aq))⁺+Cl_((aq))⁻+Ag₍ₛ₎
occurs in which of the following galvanic cell :

Solution

Chemistry ma’am · 3 steps

Split the reaction into its two half-reactions, then find the cell that has both electrodes and HCl.

1. Anode half. Hydrogen is oxidised: 1/2 H₂ → H⁺ + e⁻. That needs a hydrogen electrode, Pt | H₂(g), dipping into a solution that holds H⁺ ions.
2. Cathode half. Silver chloride is reduced: AgCl(s) + e⁻ → Ag(s) + Cl⁻. That is the silver–silver chloride electrode, AgCl(s) | Ag. Solid AgCl must appear in the cell, and Ag⁺ ions in solution play no part.

   Cell	Right electrode	Electrolyte	Matches?
   (a)	Ag⁺ | Ag, no AgCl	HCl and AgNO₃	No
   (b)	Ag⁺ | Ag	KCl, no H₂ electrode	No
   (c)	AgCl | Ag	KCl, no H⁺	No
   (d)	AgCl | Ag	HCl, gives H⁺ and Cl⁻	Yes

3. So. The products H⁺ and Cl⁻ together are just HCl(aq). Both electrodes dip into one HCl solution, so the cell is (d): Pt | H₂(g) | HCl | AgCl(s) | Ag.

The idea to keep. To match a cell to a reaction, write the oxidation and reduction halves first. Each half tells you which electrode to use, and the ions in the reaction tell you the electrolyte.

Answer from the NTA final answer key. Solution by PrepWiser.