Least thermodynamically stable species is :

F e O_{4}^{2 -}

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{F e}^{3 +}

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{F e}^{2 +}

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F e

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Solution

The correct option is C ${F e}^{2 +}$
As we know,

$Δ G^{0} = - n F E^{0}$

So, for $F e$ , $Δ G^{0} = - 2 \times F \times - 0.44 = + 84920$

As it has positive free energy, it is thermodynamically least stable species and reverse reaction is favoured.

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Similar questions

F e O_{4}^{2 -}, {F e}^{3 +}, {F e}^{2 +}

F e

F e O_{4}^{2 -} E^{o} = + 2.20 V - ------ \to F e^{3 +} E^{o} = 0.77 V - ----- \to F e^{2 +} F e^{2 +} E^{o} = 0.445 V - ------ \to F e^{0}

E_{F e O_{4}^{2 -} / F e^{2 +}}^{o}

F e | F e^{2 +} | | F e^{3 +} | F e

F e | F e^{2 +} | | F e^{3 +}, F e^{2 +} | P t

F e | F e^{3 +} | | F e^{3 +}, F e^{2 +} | P t

E_{F e^{2 +} / F e}^{\circ} = - 0.44 V and E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.77 V

E_{F e^{3 +} / F e}^{\circ}

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