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

AI Thread Summary
The discussion focuses on determining the net redox equations for the reaction between Fe(OH)2 and O2 in a basic solution. The oxidation half-reaction involves Fe(OH)2 converting to Fe(OH)3 while releasing an electron. Participants consider the reduction of oxygen, suggesting that one-half mole of O2 could be relevant for the reaction. The proposed reduction half-reaction involves O2 reacting with water to form hydroxide ions and an electron. The conversation highlights the need for clarity in identifying the products of the reduction process and the overall stoichiometry of the reaction.
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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.
 
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?
 
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.
 
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