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Question
Using the standard electrode potential, predict if the reaction between the following is feasible:
Br2(aq) and \[\ce{Fe^{2+}_{( aq)}}\]
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Solution
A reaction is feasible if the value of \[\ce{E^{\circ}_{cell}}\] is positive.
The reaction is as follows:
\[\ce{Fe^{2+}_{( aq)} + 1/2Br2_{( aq)} -> Fe^{3+}_{( aq)} + Br^-_{( aq)}}\]
According to this, the cell will be as follows:
\[\ce{Fe^{2+}_{( aq)} | Fe^{3+}_{( aq)} || 1/2Br2_{( aq)} | Br^-_{( aq)}}\]
∴ \[\ce{E^{\circ}_{cell} = E^{\circ}_{\frac{1}{2} Br_2/Br^-} - E^{\circ}_{Fe^{3+}/Fe^{2+}}}\]
= 1.09 − 0.77
= 0.32 V
Since the value of \[\ce{E^{\circ}_{cell}}\] is positive, the reaction is feasible.
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