The measured e.m.f. at `25^(@)C` for the cell reaction,
`Zn(s) +XCu^(2+)._((eq))(0.1M) rarr Cu(s) ._((aq)) +Zn^(2+)(1.0M)` is 1.3 volt, calculate `E^(@)` for the cell reaction.

Explanation

To calculate the standard cell potential \( E^\circ \) for the given cell reaction, we can use the Nernst equation. Let's break down the solution step by step.

### Step 1: Write the Nernst Equation
The Nernst equation is given by:

\[ E_{\text{cell}} = E^\circ_{\text{cell}} - \frac{0.059}{n} \log \frac{[\text{products}]}{[\text{reactants}]} \]
...