Ok, here is another one I have, this is one of a series of half-cell questions... this one is confusing. 79. Balance the following equations by the half-cell method. Show both half-cell reactions and identify them as oxidation or reduction. b) Cl2(g) + OH- <=> Cl- + ClO3^- + H2O(l) Oxidation Reaction: Cl2 (g) <-> Cl- 2e- + Cl2 <-> 2Cl- --- Balanced Cl molecules and electrons Reduction Reaction: Cl2 (g) <-> ClO3- Cl2 + 6H2O <-> 2ClO3- + 12H+ 10e- Multiply the oxidation reaction by a factor of 5 to cross out the e- 5Cl2 <-> 10Cl- Add them together: 6Cl2 + 6H2O <-> 10Cl- + 2ClO3- + 12H+ Since this is a basic solution we must swap out the H+ with OH-... in this case adding 6OH- to each side 6Cl2 + 6H2O + 12OH- <-> 10Cl- + 2ClO3- + 12HOH This seems kinda insane but it may just be right. Can anyone give me some input on this? Thanks.