What causes the generation of oxygen in a PbS and H2O2 reaction?

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SUMMARY

The discussion centers on the generation of oxygen in the reaction between lead sulfide (PbS) and hydrogen peroxide (H2O2). Participants explore the oxidation process of sulfides, questioning the necessity of oxygen ions and the role of acidic mediums in facilitating the reaction. Key points include the oxidation of PbS to PbS(2+) and the potential for H2O2 to act as an oxidizing agent. The conversation highlights the importance of understanding the solubility of sulfides and the effects of protonation in the reaction mechanism.

PREREQUISITES
  • Understanding of oxidation-reduction reactions
  • Knowledge of lead sulfide (PbS) chemistry
  • Familiarity with hydrogen peroxide (H2O2) as an oxidizing agent
  • Concepts of solubility and acid-base reactions
NEXT STEPS
  • Research the oxidation mechanisms of lead sulfide (PbS) in acidic conditions
  • Study the role of hydrogen peroxide (H2O2) in redox reactions
  • Explore the solubility principles of sulfides in various pH environments
  • Investigate the effects of protonation on sulfide ions (S2-) in chemical reactions
USEFUL FOR

Chemistry students, researchers in inorganic chemistry, and professionals studying redox reactions and sulfide chemistry will benefit from this discussion.

Vriska
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I don't get it, how did the sulfur get an oxygen, I'm unable to find any any half reaction wherein a oxygen ion is generated. So what is happening here?
 
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You can oxidize sulfides just by roasting them in the air, there is no solution, no ions there at all. Why do you think you need "oxygen ions" for anything?
 
Borek said:
You can oxidize sulfides just by roasting them in the air, there is no solution, no ions there at all. Why do you think you need "oxygen ions" for anything?

Idea was that you'd need electrons first from PbS to start the reaction. you'd have some PbS -> PbS(2+) + 2e. Now you could have H2O2 accept electrons as an oxidising agent. But nowhere I'm seeing any half reaction that could put an oxygen there and plug that +2 charge.

But now you put it that way, it looks like simple burning. But why is acidic medium required there then? what if bubble carbon monoxide through hydrogen peroxide can I expect CO2, will this be as exothermic as burning CO?
 
Vriska said:
But why is acidic medium required there then?

What do you know about solubility of sulfides? Can you think about a way of shifting the dissolution to the right?
 
Borek said:
What do you know about solubility of sulfides? Can you think about a way of shifting the dissolution to the right?

I'm unafraid i don't follow, PbS is apparently quite insoluble in water. I'm not sure how acid will help unless there's an hydroxide on the right side which will be eaten by the acid.
 
What about protonating S2-?
 
Borek said:
What about protonating S2-?

Woah, amazing. thank you!
 
Borek said:
What about protonating S2-?

Heyyyyy wait a second what does dissolution have to do with this reaction?
 
Reactions in the liquid phase are much faster.
 
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