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A half-reaction is a partial breakdown of a full chemical redox reaction that shows each individual species being oxidized (loss of electrons, electrons on the product side) or being reduced (gain of electrons, electrons on the reactant side).
A half reaction is when a chemical equation is broken up into 2 pieces. One is the substance that is oxidized, and the other is the one that is reduced. When you add both together, they should add up to the original equation.
Rodrigo2J wrote:Based on what we did in class, I would say that a half reaction is split into an oxidation reaction and a reduction reaction. If you combine both reactions you should end up with the original reaction.
From the example in class, is there a reason why the oxidation reaction only had the Fe giving off electrons and the reduction reaction including hydrogen and water?
505316964 wrote:When writing half reactons why is the number of electrons written in the equation being added?
For example in this oxidation:
5Fe = Fe3+ + 5e-
Why is the 5e- added and not subtracted?
I think this is because the net number of electrons cannot change, since the reaction is balanced and no new electrons are being added or subtracted.
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