Chemistry Forum

Hi,

I need some help with this redox question please. Should I turn the first equation, and then multiply, such I have 6e- on both equations?


"Use these half reactions to set up a total reaction and balance reaction between MnO₄- and H₂O₂:

O₂ (g) + 2 H+ (aq) + 2e- ---> H₂O₂ (aq)

MnO₄- (aq) + 2 H₂O (l) + 3e- ---> MnO₂ (s) + 4 OH-(aq) "

You have two reduction reactions. There will be no reaction between. You need one oxidation. The answer I gave already in the other forum. The first reaction has to be developed with OH- to be on the correct side. H+ and OH- will neutralize it self to water.