If you want to do it by half reactions, the half reactions are as follows:
MnO4^- ==> Mn^+2
Fe+2 ==> Fe^+3
If you want to do it the shorter way, the oxidation state of Mn changes from +7 on the left to +2 on the right. The oxidation state of Fe changes from +2 on the left to +3 on the right.
[Note: technically, this equation can't be balanced because you didn't include an arrow. I KNOW where the arrow goes because I know the reactants and the products. Do you? If so, place the arrow where it belongs.]
Balance the equation:
Note: If a chemical species coefficient is "1" then "1" needs to be entered in the field before that species.
MnO4– + H+ + Fe2+ Mn2+ + H2O + Fe3+
3 answers
I understand how to balance the rest of the equation, but I just don't understand how to balance the Fe^+2 and Fe^+3 ions on both sides of the equation.
Actually, would it be 3Fe^+2 and 2Fe^+3 for balancing?
1 answer