The cell reaction `Zn(s) + Cu^(+2)rarr Zn^(+2) + Cu(s)` is best represented as :

Options

A. `Cuabs(Cu^(+2))abs(Zn^(+2))Zn`
B. `Znabs(Zn^(+2))abs(Cu^(+2))Cu`
C. `Cu^(+2)abs(Cu)abs(Zn)Zn^(+2)`
D. `Ptabs(Zn^(+2))abs(Pt)Cu^(+2)`

Answer

To represent the cell reaction \( \text{Zn(s)} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu(s)} \) correctly, we can break it down into the half-reactions occurring at the anode and cathode.

### Step-by-Step Solution:

1. **Identify the Oxidation and Reduction Reactions:**
- In the given reaction, zinc (Zn) is oxidized to zinc ions (\( \text{Zn}^{2+} \)), and copper ions (\( \text{Cu}^{2+} \)) are reduced to copper metal (Cu).
- The oxidation half-reaction is:
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+} + 2e^- \]
- The reduction half-reaction is:
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu(s)} \]

2. **Combine the Half-Reactions:**
- When we combine the oxidation and reduction half-reactions, we have:
\[ \text{Zn(s)} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu(s)} \]
- This shows that zinc is losing electrons (oxidation) and copper ions are gaining electrons (reduction).

3. **Identify the Anode and Cathode:**
- The anode is where oxidation occurs. In this case, zinc is oxidized at the anode.
- The cathode is where reduction occurs. Here, copper ions are reduced to copper metal at the cathode.

4. **Representation of the Electrochemical Cell:**
- The electrochemical cell can be represented as:
\[ \text{Zn(s)} | \text{Zn}^{2+} || \text{Cu}^{2+} | \text{Cu(s)} \]
- This notation indicates that zinc is in the solid state and is oxidized to zinc ions, while copper ions in solution are reduced to solid copper.

5. **Role of the Salt Bridge:**
- A salt bridge is used in the electrochemical cell to maintain ionic balance by allowing the flow of ions between the two half-cells.

### Final Representation:
Thus, the overall cell reaction can be represented as:
\[ \text{Zn(s)} | \text{Zn}^{2+} || \text{Cu}^{2+} | \text{Cu(s)} \]