Wikipedia

Carbon monoxide

Carbon monoxide(chemical formulaCO) is a poisonous, flammable gas that is colorless, odorless, tasteless, and slightly less dense than air. Carbon monoxide consists of onecarbonatom and oneoxygenatom connected by atriple bond.It is the simplestcarbon oxide.Incoordination complexes,the carbon monoxideligandis calledcarbonyl.It is a key ingredient in many processes in industrial chemistry.[5]

Carbon monoxide
Ball-and-stick model of carbon monoxide
Ball-and-stick model of carbon monoxide
Spamodel of carbon monoxide
Spamodel of carbon monoxide
model of carbon monoxide
Names
IUPAC name
Carbon monoxide
Other names
Carbonic oxide gas
Carbon protoxide
Oxide of carbon
Protoxide of carbon
Carbonous oxide
Carbonous acid gas
Carbon(II) oxide
Breath of carbon
Oxygenated carbon
Carbate
Carbonyl
Water gas
Hydrocarbon gas
Fuel gas
Rauchgas
Carbonic inflammable air
Heavy inflammable air
White damp
Fire Damp
Powder Gas
Illuminating gas
Dowson gas
Mond gas
Power gas
Producer gas
Blast furnace gas
Coal gas
Phlogiston
Car gas
Identifiers
3D model (JSmol)
3587264
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.010.118Edit this at Wikidata
EC Number
  • 211-128-3
421
KEGG
MeSH Carbon+monoxide
RTECS number
  • FG3500000
UNII
UN number 1016
  • InChI=1S/CO/c1-2checkY
    Key: UGFAIRIUMAVXCW-UHFFFAOYSA-NcheckY
  • InChI=1/CO/c1-2
    Key: UGFAIRIUMAVXCW-UHFFFAOYAT
  • [C-]#[O+]
Properties
CO
Molar mass 28.010g·mol−1
Appearance Colorless
Odor Odorless
Density
  • 789 kg/m3,liquid
  • 1.250 kg/m3at 0 °C, 1 atm
  • 1.145 kg/m3at 25 °C, 1 atm
Melting point −205.02 °C (−337.04 °F; 68.13 K)
Boiling point −191.5 °C (−312.7 °F; 81.6 K)
27.6 mg/L (25 °C)
Solubility soluble inchloroform,acetic acid,ethyl acetate,ethanol,ammonium hydroxide,benzene
1.04 atm·m3/mol
−9.8·10−6cm3/mol
1.0003364
0.122D
Thermochemistry
29.1 J/(K·mol)
197.7 J/(K·mol)
−110.5 kJ/mol
−283.0 kJ/mol
Pharmacology
V04CX08(WHO)
Hazards
Occupational safety and health(OHS/OSH):
Main hazards
 Poisonousbyinhalation[1]
GHSlabelling:
GHS02: FlammableGHS06: ToxicGHS08: Health hazard
Danger
H220,H331,H360,H372,H420
P201,P202,P210,P251,P260,P261,P264,P270,P281,P304+P340,P308+P313,P311,P314,P321,P377,P381,P403,P403+P233,P405,P501
NFPA 704(fire diamond)
[3]
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
4
0
Flash point −191 °C (−311.8 °F; 82.1 K)
609 °C (1,128 °F; 882 K)
Explosive limits 12.5–74.2%
Lethal doseor concentration (LD, LC):
  • 8636 ppm (rat, 15 min)
  • 5207 ppm (rat, 30 min)
  • 1784 ppm (rat, 4 h)
  • 2414 ppm (mouse, 4 h)
  • 5647 ppm (guinea pig, 4 h)[2]
  • 4000 ppm (human, 30 min)
  • 5000 ppm (human, 5 min)[2]
NIOSH(US health exposure limits):[1]
PEL(Permissible)
 TWA 50 ppm (55 mg/m3)
REL(Recommended)
  • TWA 35 ppm (40 mg/m3)
  • C 200 ppm (229 mg/m3)
IDLH(Immediate danger)
 1200 ppm
Safety data sheet(SDS) ICSC 0023
Related compounds
Otheranions
 Carbon monosulfide
Othercations
 Silicon monoxide
Germanium monoxide
Tin(II) oxide
Lead(II) oxide
Related carbon oxides
 Carbon dioxide
Carbon suboxide
Oxocarbons
Supplementary data page
Carbon monoxide (data page)
Except where otherwise noted, data are given for materials in theirstandard state(at 25 °C [77 °F], 100 kPa).

The most common source of carbon monoxide is the partialcombustionof carbon-containing compounds. Numerous environmental and biological sources generate carbon monoxide. In industry, carbon monoxide is important in the production of many compounds, including drugs, fragrances, and fuels.[6]Uponemissioninto the atmosphere, carbon monoxide affects several processes that contribute toclimate change.[7]

Indoors CO is one of the most acutely toxic contaminants affectingindoor air quality.CO may be emitted from tobacco smoke and generated from malfunctioning fuel burning stoves (wood, kerosene, natural gas, propane) and fuel burning heating systems (wood, oil, natural gas) and from blockedfluesconnected to these appliances.[8]Carbon monoxide poisoningis the most common type of fatal air poisoning in many countries.[9][8][10]

Carbon monoxide has important biological roles across phylogenetic kingdoms. It is produced by many organisms, including humans. In mammalian physiology, carbon monoxide is a classical example ofhormesiswhere low concentrations serve as an endogenousneurotransmitter(gasotransmitter) and high concentrations aretoxicresulting incarbon monoxide poisoning.It isisoelectronicwith bothcyanideanion CN−and molecularnitrogenN2.

Physical and chemical properties

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Carbon monoxide is the simplestoxocarbonand isisoelectronicwith other triply bondeddiatomicspecies possessing 10 valence electrons, including thecyanideanion, thenitrosoniumcation,boron monofluorideand molecularnitrogen.It has amolar massof 28.0, which, according to theideal gas law,makes it slightly less dense than air, whose average molar mass is 28.8.

The carbon and oxygen are connected by atriple bondthat consists of a net twopi bondsand onesigma bond.Thebond lengthbetween the carbon atom and the oxygen atom is 112.8pm.[11][12]This bond length is consistent with a triple bond, as in molecular nitrogen (N2), which has a similar bond length (109.76 pm) and nearly the samemolecular mass.Carbon–oxygen double bonds are significantly longer, 120.8 pm informaldehyde,for example.[13]The boiling point (82 K) and melting point (68 K) are very similar to those of N2(77 K and 63 K, respectively). Thebond-dissociation energyof 1072 kJ/mol is stronger than that of N2(942 kJ/mol) and represents the strongest chemical bond known.[14]

Thegroundelectronic stateof carbon monoxide is asinglet state[15]since there are no unpaired electrons.

Thermal and physical properties of carbon monoxide (CO) at atmospheric pressure[16][17]
Temperature (°C) Temperature (K) Density (kg/m3) Specific heat (J/g °C) Dynamic viscosity (cg/m s) Kinematic viscosity (cm2/s) Thermal conductivity (cW/m °C) Thermal diffusivity (cm2/s) Prandtl number
-73.15 200 1.6888 1.045 1.27 0.0752 1.7 0.0963 0.781
-53.15 220 1.5341 1.044 1.37 0.0893 1.9 0.119 0.753
-33.15 240 1.4055 1.043 1.47 0.105 2.06 0.141 0.744
-13.15 260 1.2967 1.043 1.57 0.121 2.21 0.163 0.741
6.85 280 1.2038 1.042 1.66 0.138 2.36 0.188 0.733
26.85 300 1.1233 1.043 1.75 0.156 2.5 0.213 0.73
46.85 320 1.0529 1.043 1.84 0.175 2.63 0.239 0.73
66.85 340 0.9909 1.044 1.93 0.195 2.78 0.269 0.725
86.85 360 0.9357 1.045 2.02 0.216 2.91 0.298 0.725
106.85 380 0.8864 1.047 2.1 0.237 3.05 0.329 0.729
126.85 400 0.8421 1.049 2.18 0.259 3.18 0.36 0.719
176.85 450 0.7483 1.055 2.37 0.317 3.5 0.443 0.714
226.85 500 0.67352 1.065 2.54 0.377 3.81 0.531 0.71
276.85 550 0.61226 1.076 2.71 0.443 4.11 0.624 0.71
326.85 600 0.56126 1.088 2.86 0.51 4.4 0.721 0.707
376.85 650 0.51806 1.101 3.01 0.581 4.7 0.824 0.705
426.85 700 0.48102 1.114 3.15 0.655 5 0.933 0.702
476.85 750 0.44899 1.127 3.29 0.733 5.28 1.04 0.702
526.85 800 0.42095 1.14 3.43 0.815 5.55 1.16 0.705

Bonding and dipole moment

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The strength of the C-O bond in carbon monoxide is indicated by the high frequency of its vibration, 2143 cm-1.[18]For comparison, organic carbonyls such as ketones and esters absorb at around 1700 cm-1.

Carbon and oxygen together have a total of 10electronsin thevalence shell.Following theoctet rulefor both carbon and oxygen, the two atoms form atriple bond,with six shared electrons in three bonding molecular orbitals, rather than the usual double bond found in organic carbonyl compounds. Since four of the shared electrons come from the oxygen atom and only two from carbon, one bonding orbital is occupied by two electrons from oxygen, forming a dative ordipolar bond.This causes a C←Opolarizationof the molecule, with a small negative charge on carbon and a small positive charge on oxygen. The other two bonding orbitals are each occupied by one electron from carbon and one from oxygen, forming (polar) covalent bonds with a reverse C→O polarization since oxygen is moreelectronegativethan carbon. In the free carbon monoxide molecule, a net negative charge δ–remains at the carbon end and the molecule has a smalldipole momentof 0.122D.[19]

The molecule is therefore asymmetric: oxygen is more electron dense than carbon and is also slightly positively charged compared to carbon being negative.

The most important resonance form of carbon monoxide is–C≡O+.An important minor resonance contributor is the non-octet carbenic structure:C=O.

Carbon monoxide has a computed fractional bond order of 2.6, indicating that the "third" bond is important but constitutes somewhat less than a full bond.[20]Thus, in valence bond terms,–C≡O+is the most important structure, while:C=O is non-octet, but has a neutral formal charge on each atom and represents the second most important resonance contributor. Because of the lone pair and divalence of carbon in this resonance structure, carbon monoxide is often considered to be an extraordinarily stabilizedcarbene.[21]Isocyanidesare compounds in which the O is replaced by an NR (R = alkyl or aryl) group and have a similar bonding scheme.

If carbon monoxide acts as aligand,the polarity of the dipole may reverse with a net negative charge on the oxygen end, depending on the structure of thecoordination complex.[22] See also the section"Coordination chemistry"below.

Bond polarity and oxidation state

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Theoretical and experimental studies show that, despite the greater electronegativity of oxygen, the dipole moment points from the more-negative carbon end to the more-positive oxygen end.[23][24]The three bonds are in factpolar covalent bondsthat are strongly polarized. The calculated polarization toward the oxygen atom is 71% for theσ-bondand 77% for bothπ-bonds.[25]

Theoxidation stateof carbon in carbon monoxide is +2 in each of these structures. It is calculated by counting all the bonding electrons as belonging to the more electronegative oxygen. Only the two non-bonding electrons on carbon are assigned to carbon. In this count, carbon then has only two valence electrons in the molecule compared to four in the free atom.

Occurrence

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Monthly averages of global concentrations of tropospheric carbon monoxide at an altitude of about 12,000 feet. Data were collected by the MOPITT (Measurements Of Pollution In The Troposphere) sensor on NASA's Terra satellite.[26]

Carbon monoxide occurs in various natural and artificial environments. Photochemical degradation of plant matter for example generates an estimated 60 million tons/year.[27]Typical concentrations inparts per millionare as follows:

Composition of dry atmosphere, by volume[28]
Concentration (ppmv[a]) Source
0.1 Natural atmosphere level (MOPITT)[29]
0.5–5 Average level in homes[30]
5–15 Near properly adjusted gas stoves in homes, modern vehicle exhaust emissions[31][citation needed]
17 Atmosphere of Venus
100–200 Exhaust from automobiles in the Mexico City central area in 1975[32]
700 Atmosphere of Mars
<1,000 Car exhaust fumes after passing throughcatalytic converter[33]
5,000 Exhaust from a home wood fire[34]
30,000–100,000 Undiluted warm car exhaust without acatalytic converter[33]
  1. ^Parts per millionby volume (note:volume fractionis equal tomole fractionfor ideal gas only, seevolume (thermodynamics))

Atmospheric presence

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The streak of red, orange, and yellow acrossSouth America,Africa,and theAtlantic Oceanin this animation points to high levels of carbon monoxide on September 30, 2005.
Carbon monoxide concentrations in Northern Hemisphere spring as measured with the MOPITT instrument

Carbon monoxide (CO) is present in small amounts (about 80ppb) in theEarth's atmosphere.Most of the rest comes from chemical reactions withorganic compoundsemitted by human activities and natural origins due tophotochemicalreactions in thetropospherethat generate about 5 × 1012kilograms per year.[35]Other natural sources of CO include volcanoes,forestandbushfires,and other miscellaneous forms of combustion such asfossil fuels.[36]Small amounts are also emitted from the ocean, and from geological activity because carbon monoxide occurs dissolved in molten volcanic rock at high pressures in the Earth'smantle.[37]Because natural sources of carbon monoxide vary from year to year, it is difficult to accurately measure natural emissions of the gas.

Carbon monoxide has an indirect effect onradiative forcingby elevating concentrations of directgreenhouse gases,includingmethaneandtroposphericozone.CO can react chemically with other atmospheric constituents (primarily thehydroxylradical,•OH) that would otherwise destroy methane.[38]Through natural processes in the atmosphere, it is oxidized tocarbon dioxideand ozone. Carbon monoxide is short-lived in the atmosphere (with an average lifetime of about one to two months), and spatially variable in concentration.[39]

Due to its long lifetime in the mid-troposphere, carbon monoxide is also used as a tracer for pollutant plumes.[40]

Astronomy

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Beyond Earth, carbon monoxide is the second-most common diatomic molecule in theinterstellar medium,aftermolecular hydrogen.Because of its asymmetry, thispolar moleculeproduces far brighterspectral linesthan the hydrogen molecule, making CO much easier to detect. Interstellar CO was first detected withradio telescopesin 1970. It is now the most commonly used tracer of molecular gas in general in the interstellar medium of galaxies, as molecular hydrogen can only be detected using ultraviolet light, which requiresspace telescopes.Carbon monoxide observations provide much of the information about themolecular cloudsin which moststars form.[41][42]

Beta Pictoris,the second brightest star in the constellationPictor,shows anexcess of infrared emissioncompared to normal stars of its type, which is caused by large quantities of dust and gas (including carbon monoxide)[43][44]near the star.

In theatmosphere of Venuscarbon monoxide occurs as a result of the photodissociation of carbon dioxide by electromagnetic radiation of wavelengths shorter than 169nm.It has also been identified spectroscopically on the surface of Neptune's moonTriton.[45]

Solid carbon monoxide is a component ofcomets.[46]Thevolatile or "ice"component ofHalley's Cometis about 15% CO.[47]At room temperature and at atmospheric pressure, carbon monoxide is actually only metastable (seeBoudouard reaction) and the same is true at low temperatures where CO andCO
2are solid, but nevertheless it can exist for billions of years in comets. There is very little CO in the atmosphere ofPluto,which seems to have been formed from comets. This may be because there is (or was) liquid water inside Pluto.

Carbon monoxide can react with water to form carbon dioxide and hydrogen:

CO + H2O →H
2+CO
2

This is called thewater-gas shift reactionwhen occurring in the gas phase, but it can also take place (very slowly) in an aqueous solution. If the hydrogen partial pressure is high enough (for instance in an underground sea),formic acidwill be formed:

CO + H2O → HCOOH

These reactions can take place in a few million years even at temperatures such as found on Pluto.[48]

Pollution and health effects

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Urban pollution

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Carbon monoxide is a temporary atmospheric pollutant in some urban areas, chiefly from the exhaust ofinternal combustion engines(including vehicles, portable and back-up generators, lawnmowers, power washers, etc.), but also from incomplete combustion of various other fuels (including wood, coal, charcoal, oil, paraffin, propane, natural gas, and trash).

Large CO pollution events can be observed from space over cities.[49]

Role in ground level ozone formation

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Main article:Ground level ozone

Carbon monoxide is, along withaldehydes,part of the series of cycles of chemical reactions that formphotochemical smog.It reacts with hydroxyl radical (•OH) to produce a radical intermediate•HOCO, which rapidly transfers its radical hydrogen to O2to formperoxyradical (HO2•) and carbon dioxide (CO2).[50]Peroxy radical subsequently reacts withnitrogen oxide(NO) to formnitrogen dioxide(NO2) and hydroxyl radical. NO2gives O(3P) via photolysis, thereby forming O3following reaction with O2. Since hydroxyl radical is formed during the formation of NO2,the balance of the sequence of chemical reactions starting with carbon monoxide and leading to the formation of ozone is:

CO + 2O2+ hν → CO2+ O3

(where hν refers to thephotonof light absorbed by the NO2molecule in the sequence)

Although the creation of NO2is the critical step leading to low levelozoneformation, it also increases this ozone in another, somewhat mutually exclusive way, by reducing the quantity of NO that is available to react with ozone.[51]

Indoor air pollution

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Main article:Indoor air quality

Carbon monoxide is one of the most acutely toxicindoor air contaminants.Carbon monoxide may be emitted from tobacco smoke and generated from malfunctioning fuel burning stoves (wood, kerosene, natural gas, propane) and fuel burning heating systems (wood, oil, natural gas) and from blockedfluesconnected to these appliances.[8]Indeveloped countriesthe main sources of indoor CO emission come from cooking and heating devices that burnfossil fuelsand are faulty, incorrectly installed or poorly maintained.[52]Appliance malfunction may be due to faulty installation or lack of maintenance and proper use.[8]Inlow- and middle-income countriesthe most common sources of CO in homes are burningbiomass fuelsand cigarette smoke.[52]

Mining

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Miners refer to carbon monoxide as "whitedamp"or the" silent killer ". It can be found in confined areas of poor ventilation in both surface mines and underground mines. The most common sources of carbon monoxide in mining operations are the internal combustion engine and explosives; however, in coal mines, carbon monoxide can also be found due to the low-temperature oxidation of coal.[53]The idiom "Canary in the coal mine"pertained to an early warning of a carbon monoxide presence.[54]

Health effects

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Main article:Carbon monoxide poisoning

Carbon monoxide poisoningis the most common type of fatal air poisoning in many countries. Acute exposure can also lead to long-term neurological effects such as cognitive and behavioural changes. Severe CO poisoning may lead to unconsciousness, coma and death. Chronic exposure to low concentrations of carbon monoxide may lead to lethargy, headaches, nausea, flu-like symptoms and neuropsychological and cardiovascular issues.[9][8][10]

Chemistry

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Carbon monoxide has a wide range of functions across all disciplines of chemistry. The four premier categories of reactivity involvemetal-carbonylcatalysis,radicalchemistry,cationandanionchemistries.[55]

Coordination chemistry

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Main article:Metal carbonyl
Energy level scheme of the σ and π orbitals of carbon monoxide
TheHOMOof CO is a σMO.
TheLUMOof CO is a π*antibondingMO.

Most metals formcoordination complexescontaining covalently attached carbon monoxide. These derivatives, which are calledmetal carbonyls,tend to be more robust when the metal is in lower oxidation states. For exampleiron pentacarbonyl(Fe(CO)5) is an air-stable, distillable liquid.Nickel carbonylis an example of ametal carbonyl complexthat forms by the direct combination of carbon monoxide with the metal:C. Elschenbroich (2006).Organometallics.VCH.ISBN978-3-527-29390-2.

Ni + 4 CO → Ni(CO)4(1bar,55 °C)

These volatile complexes are often highly toxic. Some metal–CO complexes are prepared by decarbonylation of organic solvents, not from CO. For instance,iridium trichlorideandtriphenylphosphinereact in boiling2-methoxyethanolorDMFto affordIrCl(CO)(PPh3)2.

As a ligand, CO binds through carbon, forming a kind of triple bond. The lone pair on the carbon atom donates electron density to form a M-COsigma bond.The two π* orbitals on CO bind to filled metal orbitals. The effect is related to theDewar-Chatt-Duncanson model.The effects of the quasi-triple M-C bond is reflected in theinfrared spectrumof these complexes. Whereas free CO vibrates at 2143 cm-1, its complexes tend to absorb near 1950 cm-1.

Organic and main group chemistry

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Main article:Carbonylation

In the presence of strong acids,alkenesreact withcarboxylic acids.Hydrolysis of this species (anacylium ion) gives the carboxylic acid, a net process known as theKoch–Haaf reaction.[56]In theGattermann–Koch reaction,arenesare converted tobenzaldehydederivatives in the presence of CO,AlCl3,andHCl.[57]

A mixture of hydrogen gas and CO reacts withalkenesto give aldehydes. The process requires the presence of metal catalysts.[58]

With main group reagents, CO undergoes several noteworthy reactions.Chlorinationof CO is the industrial route to the important compoundphosgene.WithboraneCO forms the adductH3BCO,which isisoelectronicwith theacyliumcation [H3CCO]+.CO reacts withsodiumto give products resulting from C−C coupling such assodium acetylenediolate2Na+
·C
2O2−
2.It reacts with moltenpotassiumto give a mixture of an organometallic compound,potassium acetylenediolate2K+
·C
2O2−
2,potassium benzenehexolate6K+
C
6O6−
6,[59]andpotassium rhodizonate2K+
·C
6O2−
6.[60]

The compoundscyclohexanehexoneor triquinoyl (C6O6) andcyclopentanepentoneor leuconic acid (C5O5), which so far have been obtained only in trace amounts, can be regarded as polymers of carbon monoxide. At pressures exceeding 5GPa,carbon monoxide converts topolycarbonyl,a solid polymer that is metastable at atmospheric pressure but is explosive.[61][62]

Laboratory preparation

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Carbon monoxide is conveniently produced in the laboratory by thedehydrationofformic acidoroxalic acid,for example with concentratedsulfuric acid.[56][57][63]Another method is heating an intimate mixture of powderedzincmetal andcalcium carbonate,which releases CO and leaves behindzinc oxideandcalcium oxide:

Zn + CaCO3→ ZnO + CaO + CO

Silver nitrateandiodoformalso afford carbon monoxide:

CHI3+ 3AgNO3+ H2O → 3HNO3+ CO + 3AgI

Finally, metaloxalatesalts release CO upon heating, leaving acarbonateas byproduct:

Na
2C
2O
4→Na
2CO
3+CO

Production

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Thermalcombustionis the most common source for carbon monoxide. Carbon monoxide is produced from the partial oxidation ofcarbon-containing compounds; it forms when there is not enough oxygen to producecarbon dioxide(CO2), such as when operating astoveor aninternal combustion enginein an enclosed space.

A large quantity of CO byproduct is formed during the oxidative processes for the production of chemicals. For this reason, the process off-gases have to be purified.

Many methods have been developed for carbon monoxide production.[64]

Industrial production

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A major industrial source of CO isproducer gas,a mixture containing mostly carbon monoxide and nitrogen, formed by combustion of carbon in air at high temperature when there is an excess of carbon. In an oven, air is passed through a bed ofcoke.The initially produced CO2equilibrates with the remaining hot carbon to give CO.[65]The reaction of CO2with carbon to give CO is described as theBoudouard reaction.[66]Above 800 °C, CO is the predominant product:

CO2(g) + C (s) → 2 CO (g) (ΔHr= 170 kJ/mol)

Another source is "water gas",a mixture ofhydrogenand carbon monoxide produced via the endothermic reaction ofsteamand carbon:

H2O (g) + C (s) → H2(g) + CO (g) (ΔHr= 131 kJ/mol)

Other similar "synthesis gases"can be obtained fromnatural gasand other fuels.

Carbon monoxide can also be produced byhigh-temperature electrolysisof carbon dioxide withsolid oxide electrolyzer cells.[67]One method developed at DTU Energy uses a cerium oxide catalyst and does not have any issues of fouling of the catalyst.[68][69]

2 CO2→ 2 CO + O2

Carbon monoxide is also a byproduct of the reduction of metaloxideoreswith carbon, shown in a simplified form as follows:

MO + C → M + CO

Carbon monoxide is also produced by the direct oxidation of carbon in a limited supply of oxygen or air.

2 C + O2→ 2 CO

Since CO is a gas, the reduction process can be driven by heating, exploiting the positive (favorable)entropyof reaction. TheEllingham diagramshows that CO formation is favored over CO2in high temperatures.

Use

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Chemical industry

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Carbon monoxide is anindustrial gasthat has many applications in bulk chemicals manufacturing.[70]Large quantities of aldehydes are produced by thehydroformylationreaction ofalkenes,carbon monoxide, and H2.Hydroformylation is coupled to theShell higher olefin processto give precursors todetergents.

Phosgene,useful for preparing isocyanates, polycarbonates, and polyurethanes, is produced by passing purified carbon monoxide andchlorinegas through a bed of porousactivated carbon,which serves as acatalyst.World production of this compound was estimated to be 2.74 million tonnes in 1989.[71]

CO + Cl2→ COCl2

Methanolis produced by thehydrogenationof carbon monoxide. In a related reaction, the hydrogenation of carbon monoxide is coupled to C−C bond formation, as in theFischer–Tropsch processwhere carbon monoxide is hydrogenated to liquid hydrocarbon fuels. This technology allowscoalor biomass to be converted to diesel.

In theCativa process,carbon monoxide and methanol react in the presence of a homogeneousiridiumcatalystandhydroiodic acidto giveacetic acid.This process is responsible for most of the industrial production of acetic acid.

Metallurgy

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Main article:Metallurgy

Carbon monoxide is a strong reductive agent and has been used inpyrometallurgyto reducemetalsfromoressince ancient times. Carbon monoxide strips oxygen off metal oxides, reducing them to pure metal in high temperatures, formingcarbon dioxidein the process. Carbon monoxide is not usually supplied as is, in the gaseous phase, in the reactor, but rather it is formed in high temperature in presence of oxygen-carrying ore, or a carboniferous agent such as coke, and high temperature. Theblast furnaceprocess is a typical example of a process of reduction of metal from ore with carbon monoxide.

Likewise,blast furnace gascollected at the top of blast furnace, still contains some 10% to 30% of carbon monoxide, and is used as fuel onCowper stovesand on Siemens-Martin furnaces onopen hearth steelmaking.

Proposed use as a rocket fuel

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Carbon monoxide has been proposed for use as a fuel on Mars by NASA researcherGeoffrey Landis.Carbon monoxide/oxygen engineshave been suggested for early surface transportation use as both carbon monoxide and oxygen can be straightforwardly produced from the carbon dioxideatmosphere of Marsbyzirconiaelectrolysis,without using anyMartian water resourcesto obtain hydrogen, which would be needed to make methane or any hydrogen-based fuel.[72]

Landis also proposed manufacturing the fuel from the similar carbon dioxide atmosphere of Venus for a sample return mission, in combination with solar-powered UAVs and rocket balloon ascent.[73]

Biological and physiological properties

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Physiology

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Main article:Gasotransmitter
See also:Carboxyhemoglobin

Carbon monoxide is a bioactive molecule which acts as agaseous signaling molecule.It is naturally produced by many enzymatic and non-enzymatic pathways,[74]the best understood of which is the catabolic action ofheme oxygenaseon thehemederived fromhemoproteinssuch ashemoglobin.[75]Following the first report that carbon monoxide is a normal neurotransmitter in 1993,[54]carbon monoxide has received significant clinical attention as a biological regulator.

Because of carbon monoxide's role in the body, abnormalities in its metabolism have been linked to a variety of diseases, including neurodegenerations, hypertension, heart failure, and pathological inflammation.[76]In many tissues, carbon monoxide acts asanti-inflammatory,vasodilatory,and encouragers ofneovasculargrowth.[77]In animal model studies, carbon monoxide reduced the severity of experimentally induced bacterialsepsis,pancreatitis, hepaticischemia/reperfusion injury,colitis, osteoarthritis, lung injury, lung transplantation rejection, and neuropathic pain while promoting skin wound healing. Therefore, there is significant interest in the therapeutic potential of carbon monoxide becoming pharmaceutical agent and clinical standard of care.[78]

Medicine

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Main article:Carbon monoxide-releasing molecules

Studies involving carbon monoxide have been conducted in many laboratories throughout the world for its anti-inflammatory and cytoprotective properties.[79]These properties have the potential to be used to prevent the development of a series of pathological conditions including ischemia reperfusion injury, transplant rejection, atherosclerosis, severe sepsis, severe malaria, or autoimmunity.[78]Many pharmaceutical drug delivery initiatives have developed methods to safely administer carbon monoxide, and subsequent controlled clinical trials have evaluated the therapeutic effect of carbon monoxide.[80]

Microbiology

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Microbiota may also utilize carbon monoxide as agasotransmitter.[81]Carbon monoxide sensing is a signaling pathway facilitated by proteins such asCooA.[82][83][84]The scope of the biological roles for carbon monoxide sensing is still unknown.

The human microbiome produces, consumes, and responds to carbon monoxide.[74]For example, in certain bacteria, carbon monoxide is produced via thereductionof carbon dioxide by the enzymecarbon monoxide dehydrogenasewith favorablebioenergeticsto power downstream cellular operations.[85][74]In another example, carbon monoxide is a nutrient formethanogenicarchaea which reduce it to methane using hydrogen.[86]

Carbon monoxide has certain antimicrobial properties which have been studied to treat against infectious diseases.[74]

Food science

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Carbon monoxide is used inmodified atmospherepackaging systems in the US, mainly with fresh meat products such as beef, pork, and fish to keep them looking fresh. The benefit is two-fold, carbon monoxide protects against microbial spoilage and it enhances the meat color for consumer appeal.[87]The carbon monoxide combines withmyoglobinto form carboxymyoglobin, a bright-cherry-red pigment. Carboxymyoglobin is more stable than the oxygenated form of myoglobin, oxymyoglobin, which can become oxidized to the brown pigmentmetmyoglobin.This stable red color can persist much longer than in normally packaged meat. Typical levels of carbon monoxide used in the facilities that use this process are between 0.4% and 0.5%.[87]

The technology was first given "generally recognized as safe"(GRAS) status by theU.S. Food and Drug Administration(FDA) in 2002 for use as a secondary packaging system, and does not require labeling. In 2004, the FDA approved CO as primary packaging method, declaring that CO does not mask spoilage odor.[88]The process is currently unauthorized in many other countries, including Japan,Singapore,and theEuropean Union.[89][90][91]

Weaponization

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In ancient history,HannibalexecutedRomanprisoners with coal fumes during theSecond Punic War.[54]

Carbon monoxide had been used forgenocideduringthe Holocaustat someextermination camps,the most notable bygas vansinChełmno,and in theAction T4"euthanasia"program.[92]

History

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Prehistory

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Humans have maintained a complex relationship with carbon monoxide since first learning to control fire circa 800,000 BC. Early humans probably discovered the toxicity of carbon monoxide poisoning upon introducing fire into their dwellings. The early development ofmetallurgyandsmeltingtechnologies emerging circa 6,000 BC through theBronze Agelikewise plagued humankind from carbon monoxide exposure. Apart from the toxicity of carbon monoxide, indigenousNative Americansmay have experienced the neuroactive properties of carbon monoxide throughshamanisticfireside rituals.[54]

Ancient history

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Early civilizations developed mythological tales to explain the origin of fire, such asPrometheusfromGreek mythologywho shared fire with humans.Aristotle(384–322 BC) first recorded that burning coals produced toxic fumes. Greek physicianGalen(129–199 AD) speculated that there was a change in the composition of the air that caused harm when inhaled, and many others of the era developed a basis of knowledge about carbon monoxide in the context ofcoalfume toxicity.Cleopatramay havediedfromcarbon monoxide poisoning.[54]

Pre–industrial revolution

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Georg Ernst Stahlmentionedcarbonarii halitusin 1697 in reference to toxic vapors thought to be carbon monoxide.Friedrich Hoffmannconducted the first modern scientific investigation into carbon monoxide poisoning from coal in 1716.Herman Boerhaaveconducted the first scientific experiments on the effect of carbon monoxide (coal fumes) on animals in the 1730s.[54]

Joseph Priestleyis considered to have first synthesized carbon monoxide in 1772.Carl Wilhelm Scheelesimilarly isolated carbon monoxide from charcoal in 1773 and thought it could be the carbonic entity making fumes toxic.Torbern Bergmanisolated carbon monoxide fromoxalic acidin 1775. Later in 1776, the French chemistde Lassone[fr]produced CO by heatingzinc oxidewithcoke,but mistakenly concluded that the gaseous product washydrogen,as it burned with a blue flame. In the presence of oxygen, including atmospheric concentrations, carbon monoxide burns with a blue flame, producing carbon dioxide.Antoine Lavoisierconducted similar inconclusive experiments to Lassone in 1777. The gas was identified as a compound containingcarbonandoxygenbyWilliam Cruickshankin 1800.[54][93]

Thomas BeddoesandJames Wattrecognized carbon monoxide (ashydrocarbonate) to brighten venous blood in 1793. Watt suggested coal fumes could act as an antidote to the oxygen in blood, and Beddoes and Watt likewise suggested hydrocarbonate has a greater affinity for animal fiber than oxygen in 1796. In 1854,Adrien Chenotsimilarly suggested carbon monoxide to remove the oxygen from blood and then be oxidized by the body to carbon dioxide.[54]The mechanism for carbon monoxide poisoning is widely credited toClaude Bernardwhose memoirs beginning in 1846 and published in 1857 phrased, "prevents arterials blood from becoming venous".Felix Hoppe-Seylerindependently published similar conclusions in the following year.[54]

Advent of industrial chemistry

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Carbon monoxide gained recognition as an essential reagent in the 1900s.[5]Three industrial processes illustrate its evolution in industry. In theFischer–Tropsch process,coal and related carbon-rich feedstocks are converted into liquid fuels via the intermediacy of CO. Originally developed as part of the German war effort to compensate for their lack of domestic petroleum, this technology continues today. Also in Germany, a mixture of CO and hydrogen was found to combine witholefinsto givealdehydes.This process, calledhydroformylation,is used to produce many large scale chemicals such assurfactantsas well as specialty compounds that are popular fragrances and drugs. For example, CO is used in the production ofvitamin A.[94]In a third major process, attributed to researchers atMonsanto,CO combines with methanol to giveacetic acid.Most acetic acid is produced by theCativa process.Hydroformylation and the acetic acid syntheses are two of myriadcarbonylationprocesses.

See also

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References

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