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Questions
Using the standard electrode potential, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{I^-_{ (aq)}}\]
Using the standard electrode potential, predict the reaction, if any, that occurs between the following:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{I^-_{ (aq)}}\]
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Solution
A reaction is feasible if the value of \[\ce{E{^{\circ}_{cell}}}\] is positive.
According to the question, the reaction is as follows:
\[\ce{Fe^{3+}_{ (aq)} + I^-_{ (aq)} -> Fe^{2+}_{ (aq)} + I2_{(s)}}\]
According to this, the cell will be as follows:
\[\ce{Pt | I2_{(s)} | I^-_{ (aq)} || Fe^{3+}_{ (aq)} | Fe^{2+}_{ (aq)}}\]
∴ \[\ce{E{^{\circ}_{cell}} = E{^{\circ}_{Fe^{3+}/Fe^{2+}}} - E^{\circ}_{\frac{1}{2}I_2/I^-}}\]
= 0.77 − 0.54
= 0.23 V
Since the value of \[\ce{E{^{\circ}_{cell}}}\] is positive, the reaction is feasible.
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