The electrochemical cell representing the given reaction
`Ni(s)+Cu^(2+) rarr Ni^(2+)+Cu(s)`

Options

A. `Ni(s)|Cu^(2+)||Ni^(2+)|Cu(s)`
B. `Ni(s)|Ni^(2+)||Cu^(2+)|Cu`
C. `Cu(s)|Cu^(2+)||Ni(s)|Ni^(2+)`
D. `Cu(s)|Cu^(2+)||Ni^(2+)|Ni(s)`

Answer

To represent the electrochemical cell for the reaction \( \text{Ni(s)} + \text{Cu}^{2+} \rightarrow \text{Ni}^{2+} + \text{Cu(s)} \), we need to follow these steps:

### Step-by-Step Solution:

1. **Identify the Oxidation and Reduction Reactions:**
- **Oxidation:** Nickel (Ni) is oxidized to nickel ions (\( \text{Ni}^{2+} \)):
\[ \text{Ni(s)} \rightarrow \text{Ni}^{2+} + 2e^- \]
- **Reduction:** Copper ions (\( \text{Cu}^{2+} \)) are reduced to copper (Cu):
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu(s)} \]

2. **Determine the Anode and Cathode:**
- The anode is where oxidation occurs. Here, nickel is oxidized at the anode.
- The cathode is where reduction occurs. Here, copper ions are reduced at the cathode.

3. **Write the Cell Representation:**
- The standard format for representing an electrochemical cell is:
\[ \text{Anode} \, | \, \text{Anode Solution} \, || \, \text{Cathode Solution} \, | \, \text{Cathode} \]
- For our reaction:
- Anode: \( \text{Ni(s)} \) converting to \( \text{Ni}^{2+} \)
- Cathode: \( \text{Cu}^{2+} \) converting to \( \text{Cu(s)} \)

4. **Combine the Components:**
- The cell representation will be:
\[ \text{Ni(s)} | \text{Ni}^{2+} \, || \, \text{Cu}^{2+} | \text{Cu(s)} \]

5. **Final Answer:**
- The electrochemical cell representation for the reaction is:
\[ \text{Ni(s)} | \text{Ni}^{2+} \, || \, \text{Cu}^{2+} | \text{Cu(s)} \]