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Question
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{( aq)}}\] and \[\ce{I^-_{( aq)}}\]
Solution
A reaction is feasible if the value of `"E"_"cell"^Θ` is positive.
According to the question, the reaction is as follows –
\[\ce{Fe^{3+}_{( aq)} + I^-_{( aq)} -> Fe^{2+}_{( aq)} + 1/2I2_{(s)}}\]
According to this the cell will be as follows –
\[\ce{Pt | I2_{(s)} | I^-_{( aq)} || Fe^{3+}_{( aq)} | Fe^{2+}_{( aq)} | Pt}\]
∴ `"E"_("Cell")^Θ = "E"_("Fe"^{3+}//"Fe"^{2+})^Θ - "E"_(1/2"I"_2//"I" ^-)^Θ`
= 0.77 − 0.54
= 0.23 V
Since the value of `"E"_"cell"^Θ` is positive, hence the reaction is feasible.
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