Hydrogen peroxide: Difference between revisions
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#:;Would [[hydrogen sulfide]] work as well? | #:;Would [[hydrogen sulfide]] work as well? | ||
#:: {{#Chem:BaO2 + H2S = BaS + H2O2 // would this work?}} | #:: {{#Chem:BaO2 + H2S = BaS + H2O2 // would this work?}} | ||
==Storage== | ==Storage== | ||
* It can be "stored" in solid form in percarbonates and perborates and quickly reconstituted by heating. | |||
==Disposal== | ==Disposal== | ||
==See Also== | ==See Also== | ||
==References== | ==References== | ||
<references/> | <references/> |
Revision as of 11:48, 28 June 2019
Chemical formula | H2O2 |
---|---|
OTP appearance | colorless liquid |
Molar Mass(g/mol) | 34 |
Density(g/cc) | 1.135 |
Melting Point(°C) | -0.43 |
Boiling Point(°C) | 150 |
NFPA 704 |
Uses
Justification Questioned
Other
- Aids in the production of nitric and sulfuric acids.
- Combined with sulfuric acid produces pirahna solution useful in metal extraction
- Rapidly catalyzed decomposition is enormously exothermic and can be used as rocket fuel, etc
- A potent oxidizer used to convert halide ions to halide molecules
- Pharm: rapid injection into puncture wounds prevents tetanus.
Natural Occurrence
- Does occur naturally in very tiny amounts in plants and animals.
Production
Synthesis
Barium Peroxide
hydrochloric acid
This is the most efficient, since dilute acids can be used. Net reaction BaO2 + H2SO4 → BaSO4 + H2O2
- Combine barium peroxide with hydrochloric acid, giving barium chloride and hydrogen peroxide.
- BaO2 + 2 HCl → BaCl2 + H2O2
- Distill the hydrogen peroxide, leaving the barium chloride
- Add barium chloride to sulfuric acid, precipitating barium sulfate and regenereating the hydrochloric acid
- BaCl + H2SO4 → BaSO4 + 2 HCl
phosphoric acid
- Combine barium peroxide with phosphoric acid giving barium phosphate and hydrogen peroxide.
- 3 BaO2 + 2 H3PO4 → Ba3(PO4)2 + 3 H2O2
sulfuric acid
- Combine barium peroxide with sulfuric acid, precipitating barium sulfate and hydrogen peroxide.
- BaO2 + H2SO4 → BaSO4 + H2O2
- Would hydrogen sulfide work as well?
- BaO2 + H2S → BaS + H2O2 // ???
Sodium peroxide
- Combine sodium peroxide with 20% sulfuric acid kept below 10°C
- Na2O2 + H2SO4 → H2O2 + Na2SO4
- Combine sodium peroxide with water, forming sodium hydroxide and hydrogen peroxide[1]
- Na2O2 + 2 H2O → 2 NaOH + 2 H2O2
- Would hydrogen sulfide work as well?
- Na2O2 + H2S → Na2S + H2O2 // ???
Electrolysis
Electrolysis of a chilled (10°C) acidic (H2SO4) solution of ammonium bisulfate[2] produces ammonium persulfate and hydrogen, which escapes. The persulfate decomposes to hydrogen peroxide and sulfuric acid, which recombines with the ammonium cations to reconstitute the original ammonium bisulfate.
- 2 NH4HSO4 → (NH4)2S2O8 + H2
- (NH4)2S2O8 + 2 H2O → 2 NH4HSO4 + H2O2
- NET: 2 H2O → H2O2 + H2
Testing
Purification
- Prepare a saturated solution of barium hydroxide
- Add dilute hydrogen peroxide, precipitating a stochiometric amount of barium peroxide
- Ba(OH)2 + H2O2 → BaO2(s) + 2 H2O
- Filter and discard filtrate, retaining the residue of barium peroxide
- Add filtrate to concentrated sulfuric acid, producing concentrated hydrogen peroxide and barium sulfate
- BaO2 + H2SO4 → BaSO4 + H2O2
- Would hydrogen sulfide work as well?
- BaO2 + H2S → BaS + H2O2 // would this work?
- BaO2 + H2SO4 → BaSO4 + H2O2
Storage
- It can be "stored" in solid form in percarbonates and perborates and quickly reconstituted by heating.
Disposal
See Also
References
- ↑ Dönges, E. (1963) "Lithium and Sodium Peroxides".
Handbook of Preparative Inorganic Chemistry 1; pp979. - ↑ US patent 2234908 "Manufacture of hydrogen peroxide", 1937
Link courtesy Google