Difference between revisions of "Ozone"

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'''[[File:Tumblr_m9fk5hBHuW1rszmkso1_500-1-.jpg|thumb|370px|Liquid ozone. Photo by kristofvagyok.]]Ozone''' or '''trioxygen''', is an inorganic molecule with the chemical formula O<sub>3</sub>. It is an allotrope of oxygen, much less stable than the common diatomic allotrope O<sub>2</sub>.
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{{Chembox
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| Name = Ozone
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| Reference =
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| IUPACName = Trioxygen
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| PIN =
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| SystematicName =
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| OtherNames = Triatomic oxygen
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| ImageFile = Liquid ozone by kristofvagyok.jpg
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| ImageSize = 300
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| ImageCaption = Liquid ozone. Photo by kristofvagyok.
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<!-- Sections -->
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| Section1 = {{Chembox Identifiers
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| 3DMet =
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| Abbreviations =
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| SMILES =
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  }}
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| Section2 = {{Chembox Properties
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| AtmosphericOHRateConstant =
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| Appearance = Pale blue gas
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| BoilingPt =
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| BoilingPtC = −112
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| BoilingPt_ref =
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| BoilingPt_notes =
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| Density = 2.144 kg/m<sup>3</sup> (at 0 °C)
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| Formula = O<sub>3</sub>
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| HenryConstant =
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| LogP =
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| MolarMass = 48.00 g/mol
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| MeltingPt =
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| MeltingPtC = −192.2
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| MeltingPt_ref =
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| MeltingPt_notes =
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| Odor = Pungent
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| pKa =
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| pKb =
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| Solubility = 1.05 g/L (at 0 °C)
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| SolubleOther = Very soluble in [[Carbon tetrachloride|CCl<sub>4</sub>]], [[chloroform]], conc. [[sulfuric acid]]
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| Solubility1 = 0.0245 g/100 ml (20 °C)<br>0.0154 (40 °C)<br>0.0173 (60 °C)<br>0.00768 (78 °C)
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| Solvent1 = acetic acid
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| Solubility2 = ''aqueous''<br>0.0012 g/100 ml (25 °C)<br>0.00099 g/100 ml (35 °C)<br>0.00078 g/100 ml (45 °C)<br>0.00039 g/100 ml (68 °C)
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| Solvent2 = nitric acid
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| Solubility3 = 0.00077 g/100 ml (16 °C)<br>0.00019 g/100 ml (26 °C)<br>0.00017 g/100 ml (35 °C)<br>0.00014 g/100 ml (45 °C)
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| Solvent3 = aq. NaOH
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| VaporPressure = >1 atm (20 °C)
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  }}
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| Section3 = {{Chembox Structure
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| Coordination = Digonal
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| CrystalStruct =
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| MolShape = Dihedral
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  }}
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| Section4 = {{Chembox Thermochemistry
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| DeltaGf = 160.77 kJ/mol
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| DeltaHc =
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| DeltaHf = 142.67 kJ/mol
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| Entropy = 238.92 J·K<sup>−1</sup>·mol<sup>−1</sup>
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| HeatCapacity = 39 J·K<sup>−1</sup>·mol<sup>−1</sup>
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  }}
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| Section5 = {{Chembox Explosive
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| ShockSens =
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| FrictionSens =
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| DetonationV =
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| REFactor =
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  }}
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| Section6 = {{Chembox Hazards
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| AutoignitionPt = Non-flammable
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| ExploLimits =
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| ExternalMSDS = [http://www.ozoneapplications.com/info/Ozone%20Solutions%20MSDS%20Ozone.pdf OzoneSolutions]
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| FlashPt = Non-flammable
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| LD50 =
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| LC50 =
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| MainHazards = Corrosive<br>Oxidizer<br>Toxic
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| NFPA-F =
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| NFPA-H =
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| NFPA-R =
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| Section7 = {{Chembox Related
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| OtherAnions =
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| OtherCations =
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| OtherFunction =
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| OtherFunction_label =
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| OtherCompounds = [[Oxygen]]
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  }}
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}}
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'''Ozone''' or '''trioxygen''', is an inorganic molecule with the chemical formula '''O<sub>3</sub>'''. It is an allotrope of [[oxygen]], much less stable than the common diatomic allotrope O<sub>2</sub>.
  
 
==Properties==
 
==Properties==
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:NO + O<sub>3</sub> → NO<sub>2</sub> + O<sub>2</sub>
 
:NO + O<sub>3</sub> → NO<sub>2</sub> + O<sub>2</sub>
−
:NO<sub>2</sub> + O<sub>3</sub> → NO<sub>3</sub> + O<sub>2</sub>
+
:NO<sub>2</sub> + O<sub>3</sub> → NO<sub>3</sub>· + O<sub>2</sub>
−
:NO<sub>3</sub> + NO<sub>2</sub> → N<sub>2</sub>O<sub>5</sub>
+
:NO<sub>3</sub>· + NO<sub>2</sub> → N<sub>2</sub>O<sub>5</sub>
 +
 
 
Solid [[nitronium perchlorate]] can be made from NO<sub>2</sub>, ClO<sub>2</sub>, and O<sub>3</sub>:
 
Solid [[nitronium perchlorate]] can be made from NO<sub>2</sub>, ClO<sub>2</sub>, and O<sub>3</sub>:
 
:2 NO<sub>2</sub> + 2 ClO<sub>2</sub> + 2 O<sub>3</sub> → 2 NO<sub>2</sub>ClO<sub>4</sub> + O<sub>2</sub>
 
:2 NO<sub>2</sub> + 2 ClO<sub>2</sub> + 2 O<sub>3</sub> → 2 NO<sub>2</sub>ClO<sub>4</sub> + O<sub>2</sub>
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:S + H<sub>2</sub>O + O<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub>
 
:S + H<sub>2</sub>O + O<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub>
  
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Ozone reacts with carbon to form [[carbon dioxide]], even at room temperature:
+
Ozone reacts with [[carbon]] to form [[carbon dioxide]], even at room temperature:
  
 
:C + 2 O<sub>3</sub> → CO<sub>2</sub> + 2 O<sub>2</sub>
 
:C + 2 O<sub>3</sub> → CO<sub>2</sub> + 2 O<sub>2</sub>
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:2 NH<sub>3</sub> + 4 O<sub>3</sub> → NH<sub>4</sub>NO<sub>3</sub> + 4 O<sub>2</sub> + H<sub>2</sub>O
 
:2 NH<sub>3</sub> + 4 O<sub>3</sub> → NH<sub>4</sub>NO<sub>3</sub> + 4 O<sub>2</sub> + H<sub>2</sub>O
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Ozone also reacts with organic compounds to form various substances.
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 +
Ozone also reacts with organic compounds, such as unsaturated compounds to form ozonides.
 +
 
 
===Physical===
 
===Physical===
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Ozone is a pale blue gas with a distinctively pungent smell commonly described as that of copy machines, due to commercial copy machine producing small amounts. Its liquid form is dark blue and it forms a violet-black solid at extremely low temperatures. It is also unstable at high concentrations, decaying to ordinary diatomic oxygen. It has a varying length half-life, in a sealed chamber at standard conditions, with fan moving the gas, ozone has a half-life of a day.
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Ozone is a pale blue gas with a distinctively pungent smell commonly described as that of copy machines, due to commercial copy machine producing small amounts. Some people describe it as "electric", reminiscent of bumper cars from amusement parks. Although electric discharges do produce small amounts of ozone, they also produce nitrous oxide gases, altering the ozone smell. Its liquid form is dark blue and it forms a violet-black solid at extremely low temperatures. It is also unstable at high concentrations, decaying to ordinary diatomic oxygen. It has a varying length half-life, in a sealed chamber at standard conditions, with fan moving the gas, ozone has a half-life of a day.
  
 
==Availability==
 
==Availability==
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==Preparation==
 
==Preparation==
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Ozone can be generated from electric discharges in air. Ozone generators work on this principle. However such method also generates nitrous oxides, as air is 78% nitrogen. Feed pure oxugen from a [[Kipp's apparatus]] into the generator to produce more ozone and no nitrous oxides.
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Ozone can be generated from electric discharges in air. Ozone generators work on this principle. However such method also generates nitrous oxides, as air is 78% nitrogen. Feed pure oxygen from a [[Kipp's apparatus]] into the generator to produce more ozone and no nitrous oxides. A compressed oxygen tube can also be used.
  
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Another method of generating ozone is decomposition of various peroxide compounds in acidic solution. An example is decomposition of [[barium peroxide]] in sulfuric acid.
+
Another method of generating ozone is decomposition of various highly oxidized or peroxide compounds in acidic solution. An example is decomposition of [[barium peroxide]] in sulfuric acid. Alternately, you can use [[potassium permanganate]] and mid-strength (50-80%) sulfuric acid. The resulting [[permanganic acid]] decomposes, liberating ozone. Avoid using concentrated sulfuric acid, this will give you the anhydride Mn<sub>2</sub>O<sub>7</sub>, which is a hair-trigger explosive (but still liberates ozone).
  
 
==Projects==
 
==Projects==
−
*Making sulfuric acid
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*Make [[sulfuric acid]]
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*Ozonides synthesis
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*Preparation of ozonides
 +
*Make [[nitronium perchlorate]]
 +
*Purify water
  
 
==Handling==
 
==Handling==
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Ozone at concentrations higher than 0.1 ppm in air is dangerous, as it will oxidize organic material indiscriminately. Ground level ozone can harm lung function and irritate the respiratory system.<ref>http://www.cdc.gov/niosh/idlh/10028156.html</ref> Ozone reacts with compounds lining the lungs to form specific, cholesterol-derived metabolites that are thought to facilitate the build-up and pathogenesis of atherosclerotic plaques (a form of heart disease).<ref>http://www.sciencedirect.com/science/article/pii/S0891584904003454</ref>
 
Ozone at concentrations higher than 0.1 ppm in air is dangerous, as it will oxidize organic material indiscriminately. Ground level ozone can harm lung function and irritate the respiratory system.<ref>http://www.cdc.gov/niosh/idlh/10028156.html</ref> Ozone reacts with compounds lining the lungs to form specific, cholesterol-derived metabolites that are thought to facilitate the build-up and pathogenesis of atherosclerotic plaques (a form of heart disease).<ref>http://www.sciencedirect.com/science/article/pii/S0891584904003454</ref>
  
−
Ozone will react with organic materials to form ozonides, that are explosive.
+
Ozone will react with organic materials to form ozonides, many being explosive.
  
 
===Storage===
 
===Storage===
−
Ozone will decompose after several hours and has to be made in situ.
+
Ozone will decompose after several hours and has to be made in situ. Cryogenic ozone can be stored (cold causes it to become more stable) but even that is dangerous because liquid ozone is a hair-trigger explosive.
  
 
===Disposal===
 
===Disposal===
−
Ozone will decompose to normal oxygen in open air.
+
Ozone will decompose to normal oxygen in open air. Make sure you release ozone only outside and never in closed chambers.
  
 
==See also==
 
==See also==
Line 61: Line 181:
 
<references/>
 
<references/>
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=8343 Electrochemical ozone generation]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=29419 Does anyone know how to make Ozone generator???]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=61440 Making an Ozone Generator]
  
 
[[Category:Chemical compounds]]
 
[[Category:Chemical compounds]]
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[[Category:Polyatomic elements]]
 
[[Category:Polyatomic elements]]
 
[[Category:Allotropes]]
 
[[Category:Allotropes]]
 +
[[Category:Oxygen compounds]]
 
[[Category:Oxidizing agents]]
 
[[Category:Oxidizing agents]]
 
[[Category:Gases]]
 
[[Category:Gases]]
 
[[Category:Choking agents]]
 
[[Category:Choking agents]]
 +
[[Category:Irritants]]

Latest revision as of 20:39, 11 September 2020

Ozone
Liquid ozone by kristofvagyok.jpg
Liquid ozone. Photo by kristofvagyok.
Names
IUPAC name
Trioxygen
Other names
Triatomic oxygen
Properties
O3
Molar mass 48.00 g/mol
Appearance Pale blue gas
Odor Pungent
Density 2.144 kg/m3 (at 0 °C)
Melting point −192.2 °C (−314.0 °F; 81.0 K)
Boiling point −112 °C (−170 °F; 161 K)
1.05 g/L (at 0 °C)
Solubility Very soluble in CCl4, chloroform, conc. sulfuric acid
Solubility in acetic acid 0.0245 g/100 ml (20 °C)
0.0154 (40 °C)
0.0173 (60 °C)
0.00768 (78 °C)
Solubility in nitric acid aqueous
0.0012 g/100 ml (25 °C)
0.00099 g/100 ml (35 °C)
0.00078 g/100 ml (45 °C)
0.00039 g/100 ml (68 °C)
Solubility in aq. NaOH 0.00077 g/100 ml (16 °C)
0.00019 g/100 ml (26 °C)
0.00017 g/100 ml (35 °C)
0.00014 g/100 ml (45 °C)
Vapor pressure >1 atm (20 °C)
Thermochemistry
238.92 J·K−1·mol−1
142.67 kJ/mol
Hazards
Safety data sheet OzoneSolutions
Flash point Non-flammable
Related compounds
Related compounds
 Oxygen
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Ozone or trioxygen, is an inorganic molecule with the chemical formula O3. It is an allotrope of oxygen, much less stable than the common diatomic allotrope O2.

Properties

Chemical

Ozone is a powerful oxidant, much more powerful than dioxygen.

Ozone will oxidize most metals (except noble metals) to oxides of the metals in their highest oxidation state. It will also oxidize nitrogen oxides up until dinitrogen pentoxide

NO + O3 → NO2 + O2
NO2 + O3 → NO3· + O2
NO3· + NO2 → N2O5

Solid nitronium perchlorate can be made from NO2, ClO2, and O3:

2 NO2 + 2 ClO2 + 2 O3 → 2 NO2ClO4 + O2

It will also oxidize sulphides to sulphates and sulfur and sulfur oxides to sulfuric acid in the presence of water.

PbS + 4 O3 → PbSO4 + 4 O2
S + H2O + O3 → H2SO4

Ozone reacts with carbon to form carbon dioxide, even at room temperature:

C + 2 O3 → CO2 + 2 O2

This is useful when cleaning glassware that have traces of carbon (such as graphite) that are hard to clean.

Ozone does not react with ammonium salts, but it will oxidize ammonia to ammonium nitrate:

2 NH3 + 4 O3 → NH4NO3 + 4 O2 + H2O

Ozone also reacts with organic compounds, such as unsaturated compounds to form ozonides.

Physical

Ozone is a pale blue gas with a distinctively pungent smell commonly described as that of copy machines, due to commercial copy machine producing small amounts. Some people describe it as "electric", reminiscent of bumper cars from amusement parks. Although electric discharges do produce small amounts of ozone, they also produce nitrous oxide gases, altering the ozone smell. Its liquid form is dark blue and it forms a violet-black solid at extremely low temperatures. It is also unstable at high concentrations, decaying to ordinary diatomic oxygen. It has a varying length half-life, in a sealed chamber at standard conditions, with fan moving the gas, ozone has a half-life of a day.

Availability

Ozone is unstable, so it must be generated in situ.

Preparation

Ozone can be generated from electric discharges in air. Ozone generators work on this principle. However such method also generates nitrous oxides, as air is 78% nitrogen. Feed pure oxygen from a Kipp's apparatus into the generator to produce more ozone and no nitrous oxides. A compressed oxygen tube can also be used.

Another method of generating ozone is decomposition of various highly oxidized or peroxide compounds in acidic solution. An example is decomposition of barium peroxide in sulfuric acid. Alternately, you can use potassium permanganate and mid-strength (50-80%) sulfuric acid. The resulting permanganic acid decomposes, liberating ozone. Avoid using concentrated sulfuric acid, this will give you the anhydride Mn2O7, which is a hair-trigger explosive (but still liberates ozone).

Projects

Handling

Safety

Ozone at concentrations higher than 0.1 ppm in air is dangerous, as it will oxidize organic material indiscriminately. Ground level ozone can harm lung function and irritate the respiratory system.[1] Ozone reacts with compounds lining the lungs to form specific, cholesterol-derived metabolites that are thought to facilitate the build-up and pathogenesis of atherosclerotic plaques (a form of heart disease).[2]

Ozone will react with organic materials to form ozonides, many being explosive.

Storage

Ozone will decompose after several hours and has to be made in situ. Cryogenic ozone can be stored (cold causes it to become more stable) but even that is dangerous because liquid ozone is a hair-trigger explosive.

Disposal

Ozone will decompose to normal oxygen in open air. Make sure you release ozone only outside and never in closed chambers.

See also

References

  1. ↑ http://www.cdc.gov/niosh/idlh/10028156.html
  2. ↑ http://www.sciencedirect.com/science/article/pii/S0891584904003454

Relevant Sciencemadness threads

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