Given : `E_(Fe^(3+)//Fe)^(@) = -0.036V, E_(FE^(2+)//Fe)^(@)= -0.439V`. The value of electrode potential for the change, `Fe_(aq)^(3+) + e^(-)rightarrow Fe^(2+) (aq)` will be :

Options

A. (-o.072V)
B. (o.385V)
C. `(0.770V)`
D. `(0.270)`

Explanation

To find the electrode potential for the reaction \( \text{Fe}^{3+}_{(aq)} + e^- \rightarrow \text{Fe}^{2+}_{(aq)} \), we can use the given standard electrode potentials for the reactions involving iron.

### Step-by-Step Solution:

1. **Identify the Given Reactions and Their Potentials:**
- The first reaction is:
\[
\text{Fe}^{3+} + 3e^- \rightarrow \text{Fe} \quad (E^\circ = -0.036 \, \text{V})
...