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2 months ago
A) Equation 1: Write the first possible oxidation half-reaction of Fe(s) that produces an iron ion:

B) Using oxidation numbers, describe what is happening in the above reaction.

C) Equation 2: The next possible oxidation reaction of Fe(s) that produces an iron ion is:

D)  Using oxidation numbers, describe what is happening in the above reaction.

E)  Write the oxidation equation that shows how Fe2O3 (s) is produced when the product of equation 1 reacts with H2O(l).

F) Using oxidation numbers, describe what is happening in the above reaction.

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wrote...
2 months ago
You've got two scenarios:

Fe(s) -> Fe3+ + 3e-

Fe(s) -> Fe2+ + 2e-

In both situations, iron it being oxidized into the iron ion plus electrons.
wrote...
2 months ago
So those would be my equation 1 and 2?
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2 months ago
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Could be something like this:

Eq. 1:   Fe(s) → Fe2+ + 2e-

Eq. 2:   Fe2+ → Fe3+ + e-

Iron forms a number of different ions, as shown, for example, Fe2+ and Fe3+. If you think about how these might be produced from iron metal, the 2+ ion will be formed by oxidising the metal by removing two electrons:

Fe(s) -> Fe2+ + 2e-

The iron is now said to be in an oxidation state of +2.

Removal of another electron gives the Fe3+ ion:

Fe2+ → Fe3+ + e-

The iron now has an oxidation state of +3.

Quote
E) Write the oxidation equation that shows how Fe2O3 (s) is produced when the product of equation 1 reacts with H2O(l).

Fe2+ + H2O → Fe2O3

2Fe2+ + 3H2O → Fe2O3 + 6H+ + 2e-
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