The cell reaction `Cu+2Ag^(+)toCu^(+2)+Ag` is best represented by

Options

A. `Cu_((s))|Cu_((aq))^(+2)||Ag_((aq))^(+)|Ag`
B. `Pr|Cu^(+2)||Ag_((aq))^(+)|Ag_((s))`
C. `Cu^(+2)|Cu||Pt|Ag`
D. None of the above representation

Answer

To solve the given cell reaction \( \text{Cu} + 2\text{Ag}^+ \rightarrow \text{Cu}^{2+} + 2\text{Ag} \), we need to break it down into oxidation and reduction half-reactions.

### Step 1: Identify Oxidation and Reduction
- **Oxidation** is the loss of electrons, and in this reaction, copper (Cu) is being oxidized to copper ions (\( \text{Cu}^{2+} \)).
- **Reduction** is the gain of electrons, and silver ions (\( \text{Ag}^+ \)) are being reduced to silver metal (Ag).

### Step 2: Write the Oxidation Half-Reaction
The oxidation half-reaction can be written as:
\[ \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \]
This indicates that copper loses two electrons to form copper ions.

### Step 3: Write the Reduction Half-Reaction
The reduction half-reaction can be written as:
\[ 2\text{Ag}^+ + 2e^- \rightarrow 2\text{Ag} \]
This indicates that silver ions gain two electrons to form silver metal.

### Step 4: Combine the Half-Reactions
Now, we combine the oxidation and reduction half-reactions to get the overall cell reaction:
\[ \text{Cu} + 2\text{Ag}^+ \rightarrow \text{Cu}^{2+} + 2\text{Ag} \]
This shows the complete reaction where copper is oxidized and silver ions are reduced.

### Conclusion
The cell reaction \( \text{Cu} + 2\text{Ag}^+ \rightarrow \text{Cu}^{2+} + 2\text{Ag} \) is best represented by the oxidation of copper and the reduction of silver ions.

### Final Answer
The best representation of the cell reaction is:
- Oxidation: \( \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \)
- Reduction: \( 2\text{Ag}^+ + 2e^- \rightarrow 2\text{Ag} \)