Following reactions are taking place in a Galvanic cell , `Zn to Zn^(2+) + 2e^(-) , Ag^(+) + e^(-) to Ag`
Which of the given representations is the correct method of depicting the cell ?

Options

A. `Zn_((s)) | Zn_((aq))^(2+)"||"Ag_((aq))^+ | Ag_((s))`
B. `Zn^(2+)| Zn||Ag|Ag^+`
C. `Zn_((aq))|Zn_((s))^(2+) "||"Ag_((s))^+ | Ag_((aq))`
D. `Zn_((s)) | Ag_((aq))^+ "||" Zn_((aq))^(2+) | Ag_((s))`

Explanation

To determine the correct representation of the galvanic cell based on the given reactions, we can follow these steps:

### Step 1: Identify the Oxidation and Reduction Reactions
The reactions provided are:
1. **Oxidation:** \( \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^{-} \)
2. **Reduction:** \( \text{Ag}^{+} + e^{-} \rightarrow \text{Ag} \)

In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode.

### Step 2: Identify the Anode and Cathode
- **Anode:** The electrode where oxidation occurs. In this case, zinc (Zn) is oxidized to zinc ions (\( \text{Zn}^{2+} \)).
- **Cathode:** The electrode where reduction occurs. Here, silver ions (\( \text{Ag}^{+} \)) are reduced to solid silver (Ag).

### Step 3: Write the Cell Notation
The standard notation for a galvanic cell is:
\[ \text{Anode} | \text{Anode solution} || \text{Cathode solution} | \text{Cathode} \]

For our reactions:
- Anode: \( \text{Zn} | \text{Zn}^{2+} \)
- Cathode: \( \text{Ag}^{+} | \text{Ag} \)

Thus, the cell notation becomes:
\[ \text{Zn} | \text{Zn}^{2+} || \text{Ag}^{+} | \text{Ag} \]

### Step 4: Choose the Correct Representation
From the options provided, we need to select the one that matches our cell notation \( \text{Zn} | \text{Zn}^{2+} || \text{Ag}^{+} | \text{Ag} \).

### Conclusion
The correct representation of the galvanic cell based on the given reactions is:
\[ \text{Zn} | \text{Zn}^{2+} || \text{Ag}^{+} | \text{Ag} \]