The cell reaction
`Zn(s)+2Ag^(+)(aq)rarrZn^(2+)(aq)+Ag(s)`
is best represented by

Options

A. `Ag|Ag^(+)||Zn|Zn^(2+)`
B. `Zn|Zn^(2+)||Ag^(+)|Ag`
C. `2Ag|Ag^(+)||Zn|Zn^(2+)`
D. `Zn|Zn^(2+)||2Ag|Ag^(+)`

Explanation

To represent the given cell reaction `Zn(s) + 2Ag^+(aq) → Zn^(2+)(aq) + 2Ag(s)` in cell notation, we will follow these steps:

### Step 1: Identify the Oxidation and Reduction Processes
- In the reaction, zinc (Zn) is oxidized to zinc ions (Zn²⁺), which means it loses electrons.
- Silver ions (Ag⁺) are reduced to solid silver (Ag), which means they gain electrons.

### Step 2: Determine the Anode and Cathode
- The anode is where oxidation occurs. Here, zinc is oxidized:
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+}(aq) + 2e^- \]
- The cathode is where reduction occurs. Here, silver ions are reduced:
\[ \text{Ag}^+(aq) + e^- \rightarrow \text{Ag(s)} \]

### Step 3: Write the Half-Reactions
- **Anode Half-Reaction**:
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+}(aq) + 2e^- \]
- **Cathode Half-Reaction**:
\[ 2\text{Ag}^+(aq) + 2e^- \rightarrow 2\text{Ag(s)} \]

### Step 4: Combine the Half-Reactions into Cell Notation
- In cell notation, we write the anode half-reaction on the left and the cathode half-reaction on the right, separated by a double vertical line (||) which represents the salt bridge.
- The overall cell notation will be:
\[ \text{Zn(s)} | \text{Zn}^{2+}(aq) || \text{Ag}^+(aq) | \text{Ag(s)} \]

### Final Cell Notation
Thus, the best representation of the cell reaction in cell notation is:
\[ \text{Zn(s)} | \text{Zn}^{2+}(aq) || \text{Ag}^+(aq) | \text{Ag(s)} \]

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