Because Fe\'s oxidation state is increasing from +2 to +3, it is an oxidation reaction. electrons transferred = 1 MnO4-, reduction. O has -2 charge and the molecule itself has -1 charge, so (-2 * 4oxygen molecules) -1 (charge on molecule) = -7charge is balanced by Mn7+ Mn is going through reduction because its change 7+ is reduced to 2+. electrons transferred = 5 -increase in oxidation state is oxidation, decrease is reduction -Oxidation occurs at the anode and reduction at cathode. Reduction half-reaction:__MnO4-_-> Mn2+ +5e- Electrode this reaction occurs at:___cathode_____ Balance elements that are not H or O: Balance O with H2O: MnO4- + 5e- -> Mn2+ + 4H2O Balance H with H+ion: MnO4- + 8H+ + 5e- -> Mn2+ +4H2O Balance Charge: since 5 electrons transferred in this reaction whereas in oxidation reaction only 1 electron transferred, no need to balance this reaction. ( we are going to balance the oxidation reaction.) Oxidation half-reaction:___Fe2+ ->Fe3+ + e- __ Electrode this reaction occurs at: ___anode_ Balance eements that are not H or O: Balance O:no O Balance H: no H Balance Charge: [Fe2+ ->Fe3+ + e- ] x 5 because 5 electrons transferred in reduction reaction, we need to match this up by multiplying 5 to the reaction to balance # of electrons. Multiply one reaction by an integer to get electrons equal: ____5________ Solution Because Fe\'s oxidation state is increasing from +2 to +3, it is an oxidation reaction. electrons transferred = 1 MnO4-, reduction. O has -2 charge and the molecule itself has -1 charge, so (-2 * 4oxygen molecules) -1 (charge on molecule) = -7charge is balanced by Mn7+ Mn is going through reduction because its change 7+ is reduced to 2+. electrons transferred = 5 -increase in oxidation state is oxidation, decrease is reduction -Oxidation occurs at the anode and reduction at cathode. Reduction half-reaction:__MnO4-_-> Mn2+ +5e- Electrode this reaction occurs at:___cathode_____ Balance elements that are not H or O: Balance O with H2O: MnO4- + 5e- -> Mn2+ + 4H2O Balance H with H+ion: MnO4- + 8H+ + 5e- -> Mn2+ +4H2O Balance Charge: since 5 electrons transferred in this reaction whereas in oxidation reaction only 1 electron transferred, no need to balance this reaction. ( we are going to balance the oxidation reaction.) Oxidation half-reaction:___Fe2+ ->Fe3+ + e- __ Electrode this reaction occurs at: ___anode_ Balance eements that are not H or O: Balance O:no O Balance H: no H Balance Charge: [Fe2+ ->Fe3+ + e- ] x 5 because 5 electrons transferred in reduction reaction, we need to match this up by multiplying 5 to the reaction to balance # of electrons. Multiply one reaction by an integer to get electrons equal: ____5________.