Balancing Oxidation-Reduction Reaction

  • Thread starter Dove99x
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  • #1
Dove99x
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1. Complete and balance the following equations, and identify the oxidizing and reducing agents:

OXIDATION.png



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
--------------------------------------------------------------------


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
 

Answers and Replies

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

Correct.

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

Oxygen is not balanced.
 

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