Chemistry Balancing Redox Reactions

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Discussion Overview

The discussion revolves around balancing the redox reaction of hydrogen and oxygen to form water, specifically addressing the oxidation states of the elements involved and the methodology for balancing the equation. The scope includes homework-related inquiries and conceptual clarifications regarding redox reactions.

Discussion Character

  • Homework-related
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • One participant states that hydrogen has an oxidation state of +1 and oxygen -2 in water, identifying hydrogen as the reducing agent and oxygen as the oxidizing agent.
  • Another participant confirms the oxidation numbers of hydrogen and oxygen in water, noting that they cancel out to give the molecule a neutral charge.
  • A participant expresses confusion about the overall balanced reaction and the role of electrons in the redox process.
  • Some participants critique a referenced video for being chaotic and suggest that balancing the reaction as a redox process may not be necessary, questioning whether the assignment specifically requires redox balancing or just balancing in general.

Areas of Agreement / Disagreement

Participants express differing views on the necessity and approach to balancing the reaction as a redox process. Some find value in understanding the oxidation states, while others argue that balancing the reaction without focusing on redox may suffice. The discussion remains unresolved regarding the best method to approach the balancing task.

Contextual Notes

There are limitations in the understanding of the overall balanced reaction, particularly regarding the inclusion of electrons in the redox balancing process. The discussion reflects varying levels of familiarity with redox concepts and balancing techniques.

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Homework Statement



H_{2} + O_{2} \rightarrow H_{2}O

Homework Equations





The Attempt at a Solution


Well, my classmates insist that H= +1 and O= -2 (in the products side)
so, my Hydrogen will be my Reducing agent because it underwent Oxidation and my Oxygen will be my Oxidizing agent because it underwent Reduction

Reduction: O_{2} \rightarrow H_{2}O
Oxidation: H_{2} \rightarrow H_{2}O

From here on, I can't understand anything.

Well, I need to know what to do here. I was told by this video:

https://www.youtube.com/watch?v=AyKiYz-YpSw

Particularly in 4:09, in that problem, she said that H_{2}O has a charge of 0. I know that Hydrogen and Oxygen in the reactants side has 0 charge / oxidation number too because it is in its "pure" form. So, is this equation "BALANCE-able" ??
 
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Molecule of H2O is neutral (has a charge of 0), but oxidation numbers of oxygen and hydrogen in the molecule are -2 and +1 respectively. They just cancel out in the molecule.
 
Borek said:
Molecule of H2O is neutral (has a charge of 0), but oxidation numbers of oxygen and hydrogen in the molecule are -2 and +1 respectively. They just cancel out in the molecule.

ooh. Now I get it. Sorry for the dumb question. She just did it faster and not saying that the charges cancel each other. Thanks. :)
But, what is the overall reaction? The balanced one with the electrons and such. I can't understand it.
 
I don't like the video, it is slightly chaotic.

While H2/O2 is a redox reaction, trying to balance it as a redox is a waste of time. Are you asked to balance it as redox, or just to balance? Final effect will be exactly the same.
 
Borek said:
I don't like the video, it is slightly chaotic.

While H2/O2 is a redox reaction, trying to balance it as a redox is a waste of time. Are you asked to balance it as redox, or just to balance? Final effect will be exactly the same.

Yeah, we are asked to balance it (as in moles)
then as redox. Sorry for the late reply.
 

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