Redox Reaction: Fe(OH)_2+ O_2 -> Fe(OH)_3 Solution

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Homework Statement

Give the net redox equations for the following reactions which occur in base solution.
$$Fe(OH)_2+ O_2 \rightarrow Fe(OH)_3$$

Homework Equations

none

The Attempt at a Solution

The oxidation half reaction is $$Fe(OH)_+OH^{-1}\rightarrow Fe(OH)_3 + e^{-}$$.

How do we find the reduction reaction?

 

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Possibly oxygen is being reduced. Could one-half mole of oxygen be a good fit? Work from there and see what you find.

 

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How would we work with this problem using moles? How could we test of one half mole of oxygen would be "a good fit?"

How would we know what that $$O_2$$ would turn into after being reduced?

 

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The most obvious half reactions might be these:

Fe(OH) sub 2 + 1OH (-1 charge) ----------> Fe(OH) sub 3 +1e

O + H2O +1e ----------------> 2OH (-1 charge)
The single "O" is used here to show one half of the oxygen diatomic molecule. Right now, I do not have access to good typesetting. Understand, too that "sub x" means subscript of x.

Someone else might like to give further or better details, since I'm not too aware of much about Iron chemistry and reactions.