1. The problem statement, all variables and given/known data Balance the following oxidation-reduction reactions: PbO2 = Pb 2+ + O2 2. Relevant equations These are the steps I'm supposed to follow. 1. Determine the valence number (charge) for all the elements involved in the reaction. 2. Determine the number of e- given off and taken up in the reaction. Balance the transfer of electrons. 3. Balance the elements, except oxygen and hydrogen, on both sides of the equation. 4. Balance the number of oxygen atoms by adding H2O. 5. Balance the number of hydrogen atoms by adding H+ 3. The attempt at a solution 1. Reactants: Pb = +4 and O = -2. Products: Pb = +2 and O = 0. 2. To balance the transfer of electrons, multiply Pb 2+ by 2 (because O2 gained four electrons). 3. Balancing: 2PbO2 = 2Pb 2+ + O2 4. Adding H2O: 2PbO2 = 2Pb 2+ + O2 + 2H2O 5. Adding H+: 4H+ + 2PbO2 = 2Pb 2+ + O2 + 2H2O 2PbO2 + 4H+ = 2Pb 2+ + O2 + 2H2O Is this right?