Can `Fe^(3+)` oxidize `Br^(-) " to "Br_2` at 1 M concentration ?
`E^@(Fe^(3+)|Fe^(2+)=0.77V and E^@(Br|Br^(-))=1.09V`

Explanation

To determine whether \( \text{Fe}^{3+} \) can oxidize \( \text{Br}^{-} \) to \( \text{Br}_2 \) at 1 M concentration, we need to analyze the given standard reduction potentials and apply the concept of redox reactions.

### Step-by-Step Solution:

1. **Identify the half-reactions and their standard reduction potentials:**
- The reduction half-reaction for \( \text{Fe}^{3+} \) is:
\[
\text{Fe}^{3+} + e^- \rightarrow \text{Fe}^{2+} \quad E^\circ = 0.77 \, \text{V}
...