Balancing Equation using redox reactions?

AI Thread Summary
The discussion focuses on balancing the redox reaction of oxygen difluoride (OF2) producing fluoride ions, oxygen, and water in a basic solution. The initial steps involve breaking down the reaction into half-reactions, specifically addressing the reduction of OF2 to fluoride ions and the oxidation of hydroxide ions to oxygen. Participants express uncertainty about completing the oxidation half-reaction and whether to use oxidation numbers or half-reactions for balancing. There is also mention of the conditions under which the reaction occurs, with a preference for using half-reactions to achieve balance. The conversation highlights the importance of understanding redox processes in different pH environments.
r_swayze
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OF2 --> F- + O2 + H2O

OF2 --> F-

2H+ +OF2 --> 2F- + H2O

2H+ +OF2 + 4e- --> 2F- + H2O

This is as far as I can get. I don't know how to do the other half of the redox since the equation would be:

OF2 --> O2 + H2O

What do I do here? Maybe I am not setting this up correctly?
 
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Please elaborate a little bit.

Are you expected to use oxidation numbers or half reactions?

Anything about conditions - low pH, high pH, just hydrolysis in water?

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The problem states:

"Balance the following redox reaction:

In basic solution, oxygen difluoride reacts to produce fluoride ion, oxygen, and water."

I figured out one way of doing it by just adding H2O, H^+ ions, and OH^- ions to either side and balancing it, but I want to know how to do it using half reactions.
 
Assume OH- is being oxidized to O2 and water.

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