Balancing Equation using redox reactions?

In summary, the conversation involves a discussion about balancing a redox reaction involving oxygen difluoride in basic solution. One method involves adding H2O, H^+, and OH^- to either side, while the other method involves using half reactions and assuming OH^- is being oxidized to O2 and water. The question of whether oxidation numbers or conditions (such as low or high pH) should be considered is also raised.
  • #1
r_swayze
66
0
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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  • #2
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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  • #3
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.
 
  • #4
Assume OH- is being oxidized to O2 and water.

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Related to Balancing Equation using redox reactions?

What is the purpose of balancing equations using redox reactions?

The purpose of balancing equations using redox reactions is to ensure that the number of atoms of each element is equal on both the reactant and product sides. This is important because it follows the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

What does the term "redox" stand for?

"Redox" is a short form for "reduction-oxidation". It refers to the transfer of electrons between elements in a chemical reaction. Reduction is when an element gains electrons, while oxidation is when an element loses electrons.

How can you identify redox reactions?

Redox reactions involve changes in the oxidation states of elements. This can be identified by looking at the charges of the elements in the reactants and products. If there is a change in the charges, it is likely a redox reaction.

What are the steps for balancing equations using redox reactions?

The steps for balancing equations using redox reactions are:1. Write the unbalanced equation, with the reactants on the left and products on the right.2. Identify the elements that are undergoing oxidation and reduction.3. Balance the elements that are not involved in redox reactions.4. Balance the number of electrons transferred by adding coefficients to the elements involved in redox reactions.5. Balance the charges on both sides of the equation by adding or subtracting electrons.6. Balance the remaining elements by adding coefficients.7. Check that the number of atoms of each element is equal on both sides of the equation.

What are some common mistakes when balancing equations using redox reactions?

Some common mistakes when balancing equations using redox reactions include:- Forgetting to balance the charges on both sides of the equation.- Not identifying the correct elements undergoing oxidation and reduction.- Incorrectly balancing the number of electrons transferred.- Not checking for equal number of atoms on both sides of the equation.It is important to double check the balanced equation to avoid these mistakes.

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