Write cell reaction of the following cells :
`Pt,Cl_2|Cl^-(aq)||Ag^(+)aq_|Ag`

Answer

To write the cell reaction for the given electrochemical cell represented as `Pt, Cl2 | Cl^-(aq) || Ag^(+)aq | Ag`, we need to identify the half-reactions occurring at the anode and cathode, and then combine them to get the overall cell reaction.

### Step-by-Step Solution:

1. **Identify the Components**:
- The anode half-cell consists of chlorine gas (Cl2) and chloride ions (Cl^-).
- The cathode half-cell consists of silver ions (Ag^+) and solid silver (Ag).

2. **Determine the Half-Reactions**:
- At the anode (oxidation occurs), chloride ions (Cl^-) are oxidized to chlorine gas (Cl2):
\[ 2Cl^- \rightarrow Cl_2 + 2e^- \]
- At the cathode (reduction occurs), silver ions (Ag^+) are reduced to solid silver (Ag):
\[ Ag^+ + e^- \rightarrow Ag \]

3. **Balance the Half-Reactions**:
- The oxidation half-reaction produces 2 electrons, while the reduction half-reaction consumes only 1 electron. To balance the electrons, we multiply the reduction half-reaction by 2:
\[ 2Ag^+ + 2e^- \rightarrow 2Ag \]

4. **Combine the Half-Reactions**:
- Now, we can add the balanced half-reactions together:
\[ 2Cl^- + 2Ag^+ \rightarrow Cl_2 + 2Ag \]

5. **Final Cell Reaction**:
- The overall cell reaction is:
\[ 2Cl^-(aq) + 2Ag^+(aq) \rightarrow Cl_2(g) + 2Ag(s) \]

### Summary of the Cell Reaction:
The cell reaction for the given electrochemical cell is:
\[ 2Cl^-(aq) + 2Ag^+(aq) \rightarrow Cl_2(g) + 2Ag(s) \]