A reaction `:`
`(1)/(2)H_(2)(g)+AgCl(s)hArrH^(o+)(aq)+Cl^(Θ)(aq)+Ag(s)`
occurs in a galvanic cell. The structure of the cell will be

Options

A. `Ag,AgCl(s)|KCl(sol)|AgNO_(3)(sol),Ag`
B. `Pt,H_(2)(g)|HCL(sol)|AgNO_(3)(sol),Ag`
C. `Pt,H_(2)(g)|HCl(sol)|AgCl(s),Ag`
D. `Pt,H_(2)(g)|KCl(sol)|AgCl(s),Ag`

Explanation

To determine the structure of the galvanic cell for the given reaction:

\[ \frac{1}{2} H_2(g) + AgCl(s) \rightleftharpoons H^+(aq) + Cl^-(aq) + Ag(s) \]

we will follow these steps:

### Step 1: Identify the Half-Reactions
The first step is to identify the oxidation and reduction half-reactions occurring in the cell.

- **Oxidation Half-Reaction**:
\[ \frac{1}{2} H_2(g) \rightarrow H^+(aq) + e^- \]
Here, hydrogen gas is oxidized to hydrogen ions.

- **Reduction Half-Reaction**:
\[ Ag^+(aq) + e^- \rightarrow Ag(s) \]
Silver ions are reduced to solid silver.

### Step 2: Determine the Anode and Cathode
In a galvanic cell:
- The **anode** is where oxidation occurs.
- The **cathode** is where reduction occurs.

From the half-reactions:
- **Anode**: \(\frac{1}{2} H_2(g) \rightarrow H^+(aq) + e^-\)
- **Cathode**: \(Ag^+(aq) + e^- \rightarrow Ag(s)\)

### Step 3: Construct the Cell Representation
The cell representation follows the format:
\[ \text{Anode} | \text{Anode Solution} || \text{Cathode Solution} | \text{Cathode} \]

For our case:
- **Anode**: \(H_2(g)\)
- **Anode Solution**: \(H^+(aq)\) (from HCl)
- **Cathode Solution**: \(Ag^+(aq)\) (from AgCl)
- **Cathode**: \(Ag(s)\)

### Step 4: Final Cell Representation
Combining all components, we can represent the galvanic cell as:
\[ Pt | H_2(g) | HCl(aq) || AgCl(s) | Ag(s) \]

### Conclusion
The correct representation of the galvanic cell for the given reaction is:
\[ \text{Pt} | \text{H}_2(g) | \text{HCl(aq)} || \text{AgCl(s)} | \text{Ag(s)} \]