For the galvanic cell : `Pt(s) abs(Fe^(2+), Fe^(2+) ) abs(Fe^(2+))Fe` cell reaction will be :

Options

A. `3Fe^(2+) + Fe(s)rarr 2Fe^(3+)`
B. `3Fe^(2+) rarr Fe (s) + 2 Fe^(3+)`
C. `Fe(s) + 2Fe^(3+) rarr 3 Fe^(2+)`
D. None of these

Answer

To determine the cell reaction for the given galvanic cell: `Pt(s) | Fe^(2+) | Fe^(3+) || Fe`, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Half-Reactions**:
- The oxidation half-reaction involves the conversion of Fe²⁺ to Fe³⁺. This process involves the loss of one electron:
\[ \text{Oxidation: } \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + e^- \]
- The reduction half-reaction involves the conversion of Fe³⁺ to Fe. This process involves the gain of three electrons:
\[ \text{Reduction: } \text{Fe}^{3+} + 3e^- \rightarrow \text{Fe} \]

2. **Balance the Electrons**:
- To balance the electrons in both half-reactions, we need to multiply the oxidation half-reaction by 3:
\[ 3 \text{Fe}^{2+} \rightarrow 3 \text{Fe}^{3+} + 3e^- \]

3. **Combine the Half-Reactions**:
- Now we can combine the balanced half-reactions:
\[ 3 \text{Fe}^{2+} \rightarrow 3 \text{Fe}^{3+} + 3e^- \quad \text{(oxidation)} \]
\[ 3 \text{Fe}^{3+} + 3e^- \rightarrow \text{Fe} \quad \text{(reduction)} \]
- Adding these two reactions together, the electrons will cancel out:
\[ 3 \text{Fe}^{2+} + 3 \text{Fe}^{3+} \rightarrow 3 \text{Fe}^{3+} + \text{Fe} \]

4. **Final Balanced Reaction**:
- The final balanced cell reaction is:
\[ 3 \text{Fe}^{2+} \rightarrow \text{Fe} + 2 \text{Fe}^{3+} \]

### Final Answer:
The cell reaction for the galvanic cell is:
\[ 3 \text{Fe}^{2+} \rightarrow \text{Fe} + 2 \text{Fe}^{3+} \]