The half-cell reactions for the corrosion are:
$2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-} ⟶ 2 H_{2} O$ $E^{\circ} = 1.23 V$
$F e^{2 +} + 2 e^{-} ⟶ F e (s)$ $E^{\circ} = - 0.44 V$
Find the $Δ G^{\circ}$ (in kJ) for the overall reaction.

Question

The half-cell reactions for the corrosion are:

$2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-} ⟶ 2 H_{2} O$ $E^{\circ} = 1.23 V$

$F e^{2 +} + 2 e^{-} ⟶ F e (s)$ $E^{\circ} = - 0.44 V$

Find the $Δ G^{\circ}$ (in kJ) for the overall reaction.

TestHub · Accepted Answer

F e ⟶ F e 2 + + 2 e − 2 H + + 2 1 ​ O 2 ​ + 2 e − ⟶ H 2 ​ O E ce ll ∘ ​ = 1.23 + 0.44 = 1.67 V . Δ G ce ll ∘ ​ = − 2 F ( 1.67 ) = − 322310 J ≈ − 322 k J

Chemistry - Electrochemistry Question with Solution | TestHub

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