Consider the cell:
`Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s)`
its e.m.f. is `2.96V.` calculate `E_("cell")^(@)`
`(R=8.314JK^(-1),1F=96500Cmol^(-1))`

Explanation

To calculate the standard electrode potential \( E^\circ_{\text{cell}} \) for the given electrochemical cell, we will follow these steps:

### Step 1: Write the Nernst Equation
The Nernst equation relates the cell potential (E) to the standard cell potential (\( E^\circ_{\text{cell}} \)), temperature (T), and the concentrations of the reactants and products. The equation is given by:

\[ E = E^\circ_{\text{cell}} - \frac{0.059}{n} \log \left( \frac{[\text{products}]}{[\text{reactants}]} \right) \]
...