How can I balance this reaction using oxidation-reduction?

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Discussion Overview

The discussion revolves around balancing a chemical reaction involving BCl3 and H2O2, with a focus on oxidation-reduction processes. Participants explore methods for balancing the reaction and clarify the nature of the reaction components.

Discussion Character

  • Homework-related
  • Debate/contested
  • Exploratory

Main Points Raised

  • One participant suggests starting with individual half-cells to balance for electrons, indicating that a numerical balancing approach might also yield results.
  • Another participant points out that BCl3 undergoes hydrolysis rather than redox, asserting that the only redox process is the decomposition of hydrogen peroxide, which they classify as a disproportionation reaction.
  • A participant acknowledges confusion due to line wrapping in the text, which led to misinterpretation of the reaction components.
  • There is a mention of using valence numbers to approach the balancing, though one participant expresses that this method did not work for them.

Areas of Agreement / Disagreement

Participants express differing views on whether the reaction involves redox processes or is primarily a hydrolysis reaction. The discussion remains unresolved regarding the correct method for balancing the reaction.

Contextual Notes

There are indications of confusion regarding the representation of the chemical equation, which may have affected participants' understanding and analysis of the reaction.

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Homework Statement



BCl3+H2O2>>H3
BO3+HCl

Homework Equations



need to balanc it

The Attempt at a Solution

 
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That appears to be redox so you could start from the individual half-cells and balance first for the electrons. A sensible result might still be found just using balancing of numbers of atoms using the unbalanced reactants and products.

Try this: You see 3 chlorines on the left, and you see only 1 chlorine on the right. What must you do about this? What does this do the your balance of hydrogens? What more or next can you do?
 
symbolipoint said:
That appears to be redox so you could start from the individual half-cells and balance first for the electrons. A sensible result might still be found just using balancing of numbers of atoms using the unbalanced reactants and products.

Try this: You see 3 chlorines on the left, and you see only 1 chlorine on the right. What must you do about this? What does this do the your balance of hydrogens? What more or next can you do?

i now this i made this but the problem is at (B) i can't balance this but i need to make this with an oxidation and reducation sorry for my english .i tryed this also with valenc numbers but it dosent work
 
B is neither reduced nor oxidized, BCl3 just hydrolyses. The only redox here is hydrogen peroxide decomposition. This can be classifed as disproportionation reaction.

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methods
 
o.0 thanks got it now u right borek about BCl but i was thinkin of the preoxid and HCl about their valenz but i have it now
 
The linewrapping distracted me and I analyzed the reaction incorrectly. At my end, the H3 ended the line and the next stuff continued on a new line and I mistook what was seen. Not very careful thinking.
 
symbolipoint said:
The linewrapping distracted me and I analyzed the reaction incorrectly. At my end, the H3 ended the line and the next stuff continued on a new line and I mistook what was seen. Not very careful thinking.

yeh i now that's why i said it needs to be done with a oxido reduction beacuse it dident worked in this form
 

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