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Question
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{( aq)}}\] and \[\ce{Br^-_{( aq)}}\]
Solution
A reaction is feasible if the value of `"E"_"cell"^Θ` 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 –
\[\ce{Br^-_{( aq)} | 1/2Br2_{( aq)} || Fe^{3+}_{( aq)} | Fe^{2+}_{( aq)}}\]
∴ `"E"_("cell")^Θ = "E"_("Fe"^(3+)//"Fe"^(2+))^Θ - "E"_(1/2"Br"_2//"Br"^-)^Θ`
= 0.77 − 1.09
= −0.32 V
Since the value of `"E"_"cell"^Θ` is negative, hence the reaction is not feasible.
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