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Questions
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{Br^-_{ (aq)}}\]
Using the standard electrode potentials, predict the reaction, if any, that occurs between the following:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{Br^-_{ (aq)}}\]
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Solution
A reaction is feasible if the value of \[\ce{E^{\circ}_{cell}}\] is positive.
The reaction is as follows:
\[\ce{Br^-_{ (aq)} + Fe^{3+}_{ (aq)} -> 1/2Br2_{(aq)} + Fe^{2+}_{ (aq)}}\]
According to this, the cell will be as follows:
\[\ce{Br^-_{ (aq)} | 1/2Br2_{(aq)} || Fe^{3+}_{ (aq)} | Fe^{2+}_{ (aq)}}\]
∴ \[\ce{E^{\circ}_{cell} = E^{\circ}_{Fe^{3+}/Fe^{2+}} - E^{\circ}_{\frac{1}{2}Br_2/Br^-}}\]
= 0.77 − 1.09
= −0.32 V
Since the value of \[\ce{E^{\circ}_{cell}}\] is negative, the action is not feasible.
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