Balance the following oxidation-reduction reaction equation?

In this reaction Fe^+2 gives up an additional electron to become Fe+3. The permanganate ion (MnO4^-1) needs to lose the four oxygens while being reduced from a +7 to +2 ion (must gain 5 electrons). In addition the H3O+ is a water molecule with an extra proton, which can become a hydrogen atom with the addition of an electron. If the four oxygen atoms form into water molecules, 8 hydrogen atoms (which means 8 H30+ must be present) to form them. That will give us 8 H2O + 4 H20 formed = 12 H20 total. The production of 4 new water molecules requires 8 electrons - 5 come from the reduced Mn so three must come from Fe+2 changing into Fe+3. The net reaction then is: 3 Fe^+2 + 8 H3O^+ + MnO4^-1 ---> Mn^+2 + 12 H2O + 3 Fe^+3 ^_____________________________3 e^-________________________^ ......................................… e^-_____^ .....................^8 p^+_____+ 8 e^-______+ 4 O_________^4 H2O + 8 H20