Given: E^_Fe^3+/Fe = -0.036 V , E^_Fe^2+/Fe = -0.439 V . The value of standard electrode potential for the change, Fe^3+(aq) + e^- → Fe^2+(aq) will be - Chemistry MCQ AIEEE 2009 2026 | ExamTest.live

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Given: E_{Fe^{3 +} / Fe}^{\circ} = - 0.036 V, E_{Fe^{2 +} / Fe}^{\circ} = - 0.439 V . The value of standard electrode potential for the change, Fe^{3 +} (a q) + e^{-} \to Fe^{2 +} (a q) will be:

Solution & Step-by-step Explanation

(1) Fe^{3 +} + 3 e^{-} \to Fe, Δ G_{1}^{\circ} = - 3 F (- 0.036) = 0.108 F (2) Fe^{2 +} + 2 e^{-} \to Fe, Δ G_{2}^{\circ} = - 2 F (- 0.439) = 0.878 F (3) Target: Fe^{3 +} + e^{-} \to Fe^{2 +} .This can be obtained by (1) - (2): Δ G_{3}^{\circ} = Δ G_{1}^{\circ} - Δ G_{2}^{\circ} = 0.108 F - 0.878 F = - 0.770 F - 1 F E_{3}^{\circ} = - 0.770 F ⟹ E_{3}^{\circ} = 0.770 V .

Try it yourself before checking the explanation above.

Given: E_{Fe^{3 +} / Fe}^{\circ} = - 0.036 V, E_{Fe^{2 +} / Fe}^{\circ} = - 0.439 V . The value of standard electrode potential for the change, Fe^{3 +} (a q) + e^{-} \to Fe^{2 +} (a q) will be:

- 0.072 V

0.385 V

0.770 V

- 0.270 V

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