The standard electrode potential ( $E^{\circ}$ ) for the half-cell reaction ${Fe}^{3 +} + e^{-} \rig

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The standard electrode potential ( $E^{\circ}$ ) for the half-cell reaction ${Fe}^{3 +} + e^{-} ightarrow {Fe}^{2 +}$ at 298 K is (Given: $E^{\circ}\left( {Fe}^{3 +}/Fe ight) = - 0.04	ext{ }V$ and $E^{\circ}\left( {Fe}^{2 +}/Fe ight) = - 0.44	ext{ }V$ at 298 K )

Accepted Answer

Sol. [Key Concept: Standard electrode potential of Fe³⁺/Fe²⁺]$$\begin{matrix} & \Delta G^{\circ}{\lbrack Fe}^{3 +}/Febrack = \Delta G^{\circ}{\lbrack Fe}^{3 +}/{Fe}^{2 +}brack + \Delta G^{\circ}{\lbrack Fe}^{2 +}/Febrack \ & \ - {nFE}^{\circ} = - {nFE}^{\circ} + - {nFE}^{\circ} \ & \ - 3	ext{ }F( - 0.04) = - 1{FE}^{\circ} + 2	ext{ }F(0.44) \ & 3	ext{ }F(0.04) = - {Fe}^{\circ} + 0.88	ext{ }F \ & 0.12 = - E^{\circ} + 0.88 \ & 0.12 - 0.88 = - E^{\circ} \ & \ - 0.76 = - E^{\circ} \ & E^{\circ} = 0.76	ext{ }V \end{matrix}$$

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