Balancing Oxidation-Reduction Reaction

[Dove99x]

1. Complete and balance the following equations, and identify the oxidizing and reducing agents:

2. Rules.

1) an element that is reduced Gains electrons and loses Oxygen

2) an element that is oxidized loses electrons but gains Oxygen
3. My attempt

Oxidizing Agent: 5e + 8H + MnO4 ^(1-) ---> Mn ^(2+) + 4H2O

Reducing Agent: 2H2O + CH4O ---> H2CO2 + 6H ^(1+) + 6e
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At this point I relize that what I'm doing is totally wrong. I don't know how to solve this.

4. Correct Answer from Book:

4MnO4 ^(1-) + 5 CH3OH + 12 H ^(1+) ---> 4Mn ^(2+) + 5HCO2H + 12 H2O

 

[Borek]

Oxidizing Agent: 5e + 8H + MnO4 ^(1-) ---> Mn ^(2+) + 4H2O

Correct.

Reducing Agent: 2H2O + CH4O ---> H2CO2 + 6H ^(1+) + 6e

Oxygen is not balanced.