In the given cell representation `Zn|Zn^(2+)|| Cu^(2+)|Cu` , which is the negative electrode ?

Options

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

Answer

To determine the negative electrode in the given cell representation `Zn|Zn^(2+)|| Cu^(2+)|Cu`, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Components of the Cell:**
- The cell representation `Zn|Zn^(2+)|| Cu^(2+)|Cu` indicates that zinc (Zn) is on the left side and copper (Cu) is on the right side.
- The double vertical line `||` represents the salt bridge separating the two half-cells.

2. **Determine the Oxidation and Reduction Reactions:**
- In electrochemical cells, oxidation occurs at the anode and reduction occurs at the cathode.
- Zinc (Zn) is oxidized to zinc ions (Zn²⁺) by losing electrons:
\[ \text{Zn (s)} \rightarrow \text{Zn}^{2+} (aq) + 2 \text{e}^- \]
- Copper ions (Cu²⁺) are reduced to solid copper (Cu) by gaining electrons:
\[ \text{Cu}^{2+} (aq) + 2 \text{e}^- \rightarrow \text{Cu (s)} \]

3. **Identify the Anode and Cathode:**
- The anode is where oxidation occurs, which in this case is zinc (Zn).
- The cathode is where reduction occurs, which is copper (Cu).

4. **Determine the Negative Electrode:**
- The anode is the negative electrode because it is the source of electrons. In this cell, zinc is the anode.
- Therefore, the negative electrode is zinc (Zn).

### Final Answer:
The negative electrode in the cell representation `Zn|Zn^(2+)|| Cu^(2+)|Cu` is **Zinc (Zn)**.