The standard electrode potential a `Ag^(+)//Ag` is +0.80 V and of `Cu^(2+)//Cu` is +0.34 V. These electrodes are connected through a salt bridge and if :

Options

A. copper electrode acts as cathode, then `E_(cell)^(@)` is +0.46 volt
B. silver electrode acts as anode, then `E_(cell)^(@)` is + 0.46 volt
C. copper electrode acts as cathode, then `E_(cell)^(@)` is - 0.34 volt
D. silver electrode acts as anode, then `E_(cell)^(@)` is + 1.14 volt

Answer

To solve the problem, we need to determine which electrode acts as the anode and which acts as the cathode when the silver and copper electrodes are connected through a salt bridge. We will also calculate the standard cell potential (E°cell) for the electrochemical cell.

### Step-by-Step Solution:

1. **Identify the Standard Electrode Potentials:**
- The standard electrode potential for the silver half-cell (Ag⁺/Ag) is given as **+0.80 V**.
- The standard electrode potential for the copper half-cell (Cu²⁺/Cu) is given as **+0.34 V**.

2. **Determine the Reduction Reactions:**
- For silver: \( \text{Ag}^+ + e^- \rightarrow \text{Ag} \) (Reduction)
- For copper: \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \) (Reduction)

3. **Compare the Electrode Potentials:**
- The reduction potential of silver (+0.80 V) is greater than that of copper (+0.34 V).
- This means that silver has a stronger tendency to gain electrons (be reduced) compared to copper.

4. **Identify the Anode and Cathode:**
- The electrode with the higher reduction potential (silver) will act as the **cathode** (where reduction occurs).
- The electrode with the lower reduction potential (copper) will act as the **anode** (where oxidation occurs).

5. **Write the Oxidation Reaction for Copper:**
- The oxidation reaction at the anode (copper) can be written as:
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \]

6. **Calculate the Standard Cell Potential (E°cell):**
- The standard cell potential is calculated using the formula:
\[ E°_{cell} = E°_{cathode} - E°_{anode} \]
- Substituting the values:
\[ E°_{cell} = E°_{Ag/Ag^+} - E°_{Cu/Cu^{2+}} = 0.80 \, \text{V} - 0.34 \, \text{V} = 0.46 \, \text{V} \]

7. **Conclusion:**
- The silver electrode acts as the **cathode** and the copper electrode acts as the **anode**.
- The standard cell potential (E°cell) is **+0.46 V**.

### Summary of Findings:
- **Cathode:** Silver (Ag⁺/Ag)
- **Anode:** Copper (Cu²⁺/Cu)
- **Standard Cell Potential (E°cell):** +0.46 V