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

• cncbmb
In summary, the net redox equations for the given reactions in base solution are: Oxidation half reaction: Fe(OH)_2 + OH^- → Fe(OH)_3 + e^-Reduction half reaction: O + H_2O + e^- → 2OH^-The most obvious half reactions for these reactions are shown above. Further details and calculations can be performed using moles to determine the exact reaction.
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Homework Statement

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

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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?

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.

1. What is a redox reaction?

A redox reaction is a chemical reaction in which there is a transfer of electrons between atoms. One atom loses electrons (oxidation) while another atom gains electrons (reduction).

2. How do you determine which element is oxidized and which is reduced in this reaction?

In this reaction, iron (Fe) is being oxidized because it is losing electrons and its oxidation state is increasing from +2 to +3. Oxygen (O) is being reduced because it is gaining electrons and its oxidation state is decreasing from 0 to -2.

3. What is the oxidation state of iron in Fe(OH)2?

The oxidation state of iron in Fe(OH)2 is +2. This means that iron has two fewer electrons than it does in its neutral state.

4. What is the balanced chemical equation for this redox reaction?

2Fe(OH)2 + O2 → 2Fe(OH)3

5. How does this reaction affect the pH of the solution?

This reaction produces Fe(OH)3, which is a base, and therefore will increase the pH of the solution. This is because Fe(OH)3 will react with water to form hydroxide ions (OH-), which are basic in nature.

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