Calculate `E_(cell)^(@)` for the following reaction at 298 K :
`2 Cr (s ) + 3 Fe^(2+) (0.01 M) to 2 Cr^(3+) (0.01 M) + 3 Fe (s) `
Given : `E_(cell) = 0.261 V`

Explanation

To calculate \( E^\circ_{cell} \) for the given reaction at 298 K, we will use the Nernst equation. The reaction is:

\[ 2 \text{Cr (s)} + 3 \text{Fe}^{2+} (0.01 \, M) \rightarrow 2 \text{Cr}^{3+} (0.01 \, M) + 3 \text{Fe (s)} \]

### Step 1: Write the Nernst Equation

The Nernst equation is given by:

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