`E_(cell)^(@)` for the given redox reaction is 2.71 V
`Mg_((s))+Cu_((0.01 M))^(2+)toMg_((0.001 M))^(2+)+Cu_((s))`
Calculate `E_(cell)` for the reaction. Write the direction of flow of current when an external opposite potential applied is
(i) less than 2.71 V and (ii) greater than 2.71 V.

Explanation

To calculate the cell potential \( E_{cell} \) for the given redox reaction, we will use the Nernst equation. The reaction provided is:

\[ \text{Mg}_{(s)} + \text{Cu}^{2+}_{(0.01 M)} \rightarrow \text{Mg}^{2+}_{(0.001 M)} + \text{Cu}_{(s)} \]

### Step 1: Identify the standard cell potential \( E^\circ_{cell} \)
The standard cell potential \( E^\circ_{cell} \) is given as 2.71 V.

### Step 2: Write the Nernst equation
...