I can't quite understand how these redox reactions go.
For example:4 Fe + 3 O2 2 Fe2 O3
So the oxidation states are 0, 0, +3 and -2 respectively.
Therefore, from my understanding the half reactions should look like:
4 Fe (0)
2 Fe (3+) + 3e-
(0) + 2e-
Obviously this is wrong, since there's different # of electrons gained and lost.
The book says the correct answers are:
Fe (3+) + 3e-
Why do we leave out the 4 and 3 before Fe and O in reagents, but then write a 2 before O, but nothing for Fe from the product???
I can do the simple ones where the equations don't have to be balanced (all singular molecules/atoms), but once they have to be balanced things get too messy for me, and I can't for the life of me figure out how to do these. I've watched a bunch of videos and read plenty about it, but it's always the simple examples or just no explanaiton.
So if someone would be kind enough to explain how to do these redox half reactions when different numbers of moles are involved it would really help.