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They must have been drunk when they were writing the electrochem chapter.
Also, unless I don't know how to add redox half-reactions... In demonstrating the half-cell method of balancing redox equations, they came up with the following. This is for balancing MnO4- +Zn --> MnO2 + Zn(OH)4 2- in basic solution
Everything looks right to me except that the 2OH- on the product side should actually be a 4OH- on the reactant side in the overall reaction.
Reducing agent: The reactant doing the reducing, getting reduced in the process
Also, unless I don't know how to add redox half-reactions... In demonstrating the half-cell method of balancing redox equations, they came up with the following. This is for balancing MnO4- +Zn --> MnO2 + Zn(OH)4 2- in basic solution
4H2O + 2MnO4- + 6e- ----> 2MnO2 +8OH-
3Zn + 12OH- ----> 3Zn(OH)4 2- + 6e-
4H2O + 2MnO4- + 3Zn ----> 2MnO2 +3Zn(OH)4 2- + 2OH-
Everything looks right to me except that the 2OH- on the product side should actually be a 4OH- on the reactant side in the overall reaction.