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Answer to Question #29891 in Physical Chemistry for Branden
Question #29891
Predict whether Fe3+ can oxidize I- to I 2 under standard-state conditions
Expert's answer
The appropriate half-reactions are
I2(s) + 2e− → 2I−(aq)
Eanode = 0.53V
Fe3+(aq) + e− → Fe2+(aq)
Ecathode = 0.77 V
Since Fe3+/Fe2+ is more positive, it should oxidize I– to I2. This makes the I2/I– half-reaction the anode. The standard emf can be found
Ecell = Ecathode − Eanode = 0.77 V − 0.53 V = 0.24 V
I2(s) + 2e− → 2I−(aq)
Eanode = 0.53V
Fe3+(aq) + e− → Fe2+(aq)
Ecathode = 0.77 V
Since Fe3+/Fe2+ is more positive, it should oxidize I– to I2. This makes the I2/I– half-reaction the anode. The standard emf can be found
Ecell = Ecathode − Eanode = 0.77 V − 0.53 V = 0.24 V
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Comments
Dear Bodacious Bonds! Thank you for adding new information.
The question was never explicitly answered. It should be stated that because E(cell) is positive this DOES indeed favor the forward reaction of Fe3+ oxidizing I2 to I-.
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