Predict if the reaction between is feasible :
`Br_2 (aq) ` and `Fe^(2+)` (aq)
Given standard electrode potentials :
`E_(1//2)^(Theta) I_(2)//I^(-) = 0.54 V , E_(1//2)^(Theta) Cu^(2+)//Cu = 0.34 V , E_(1//2)^(Theta) Br_(2) //Br^(-) = 1.09 V, E_(1//2)^(Theta) Ag^(+)//Ag = 0.80`V and `E_(1//2)^(Theta) Fe^(3+)// Fe^(2+) = 0.77 V`

Explanation

To determine if the reaction between \( \text{Br}_2 (aq) \) and \( \text{Fe}^{2+} (aq) \) is feasible, we can follow these steps:

### Step 1: Write the balanced cell reaction
The reaction can be represented as:
\[ \text{Br}_2 (aq) + \text{Fe}^{2+} (aq) \rightarrow \text{Br}^- (aq) + \text{Fe}^{3+} (aq) \]
To balance the reaction, we need to add a coefficient of \( \frac{1}{2} \) in front of \( \text{Br}_2 \):
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