Calculate `E_(cell)^(@)` for the following reaction at `25^(@)C`.
`A+B^(2+)(0.001 M) to A^(2+)(0.0001 M)+B`
(Given. `E_(cell)=2.6805 V, 1 F=96500 C mol^(-1)`

Explanation

To calculate the standard cell potential \( E_{cell}^\circ \) for the reaction \( A + B^{2+} (0.001 \, M) \rightarrow A^{2+} (0.0001 \, M) + B \) at \( 25^\circ C \), we will use the Nernst equation. Here are the steps:

### Step 1: Write the Nernst Equation
The Nernst equation is given by:
\[ E_{cell} = E_{cell}^\circ - \frac{0.0591}{n} \log Q \]
where:
...