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Question
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Br2_{(aq)}}\] and \[\ce{Fe^{2+}_{( aq)}}\]
Solution
A reaction is feasible if the value of `"E"_"cell"^Θ` 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 –
\[\ce{Fe^{2+}_{( aq)} | Fe^{3+}_{( aq)} || 1/2Br2_{( aq)} | Br^-_{( aq)}}\]
∴ `"E"_("cell")^Θ = "E"_(1/2"Br"_2//"Br"^-)^Θ - "E"_("Fe"^(3+)//"Fe"^(2+))^Θ`
= 1.09 − 0.77
= 0.32 V
Since the value of `"E"_"cell"^Θ` is positive, hence the reaction is feasible.
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