Under standard conditions, permanganate ion in acidic solution oxidizes iron(II) ion according to the unbalanced equation below.
MnO₄⁻(aq) + Fe²⁺(aq) → Mn²⁺(aq) + Fe³⁺(aq)
Relevant standard reduction potentials are provided.
MnO₄⁻(aq) + 8 H⁺(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l) E° = +1.51 V
Fe³⁺(aq) + e⁻ → Fe²⁺(aq) E° = +0.77 V
The Faraday constant is F = 9.65 × 10⁴ C mol⁻¹.
(a) Write the balanced overall reaction for the oxidation of Fe²⁺ by MnO₄⁻ in acidic solution, including physical states.
(b) Determine the value of E°cell for the balanced reaction.
(c) State the value of n for the balanced reaction and calculate ΔG° in kJ for the reaction as written in part (a).