The standard reduction potentials of the following half cell reactions are given below
Fe³⁺ + 3e⁻ → Fe; $E^{\circ} = - 0.036 V$
Fe²⁺ + 2e⁻ → Fe; $E^{\circ} = - 0.440 V$
The standard electrode potential $E^{\circ}$ for Fe³⁺ + e⁻ → Fe²⁺ is:

Question

The standard reduction potentials of the following half cell reactions are given below

Fe³⁺ + 3e⁻ → Fe; $E^{\circ} = - 0.036 V$

Fe²⁺ + 2e⁻ → Fe; $E^{\circ} = - 0.440 V$

The standard electrode potential $E^{\circ}$ for Fe³⁺ + e⁻ → Fe²⁺ is:

TestHub · Accepted Answer

(i) Fe²⁺ + 2e⁻ → Fe, so Δ G 1 ∘ ​ = − 2 × F ( − 0.44 ) = 0.88 F (ii) Fe³⁺ + 3e⁻ → Fe, Δ G 2 ∘ ​ = − 3 × F × ( − 0.036 ) = 0.108 F So, (ii) – (i) Fe³⁺ + e⁻ → Fe²⁺. Δ G 3 ∘ ​ = 0.108 F − 0.88 F = − 0.772 F Therefore, E ∘ = − ( 1 × F − 0.772 F ​ ) = 0.772 V o lt .

Chemistry - Electrochemistry Question with Solution | TestHub

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