Carbon monoxide

Carbon monoxide
Carbon monoxide
Are common
Systematic ; name	Carbon monoxide
Chem. formula	CO
Rat formula	CO
Physical properties
condition	colorless gas
Molar mass	28.01 g / mol
Density	0.00125 ° C ; 0.814 -195 ° C g / cm³
Ionization energy
Thermal properties
T. melt.	−205 ° C
T. bale.	−191.5 ° C
Etc. blast
Enthalpy of Education	−110.52 kJ / mol
Steam pressure
Chemical properties
Solubility in water	0.0026 g / 100 ml
Classification
Reg. CAS number	630-08-0
PubChem
Reg. EINECS number	211-128-3
Smiles
Inchi
Reg. EC number	006-001-00-2
RTECS	FG3500000
Chebi
UN number
ChemSpider
Security
Toxicity	Highly toxic, SDYAV;
NFPA 704	four 3 0

Carbon monoxide ( carbon monoxide , carbon monoxide , carbon monoxide (II) ) is a colorless, extremely toxic gas without taste and odor, lighter than air (under normal conditions). Chemical formula - CO.

Molecule Structure

The CO molecule has a triple bond , as does the nitrogen molecule N ₂ . Since these molecules are similar in structure (isoelectronic, diatomic, have a similar molar mass), their properties are also similar - very low melting and boiling points, close values of standard entropies , etc.

Within the framework of the valence bond method, the structure of the CO molecule can be described by the formula ": C≡O:".

According to the molecular orbitals method, the electronic configuration of the unexcited CO 2 molecule
O σ 2
z π 4
x, y σ 2
C. The triple bond is formed by the σ- bond formed due to the σ _z electron pair , and the electrons of the doubly degenerate level π _{x, y} correspond to two π- bonds. The electrons on the non-binding σ _C- orbitals and σ _O- orbitals correspond to two electron pairs, one of which is localized at the carbon atom , the other - at the oxygen atom.

Due to the presence of a triple bond, the CO molecule is very strong (dissociation energy of 1069 kJ / mol , or 256 kcal / mol , which is greater than that of any other diatomic molecules) and has a small internuclear distance ( d _C≡O = 0.1128 nm or 1, 13 Å ).

The molecule is weakly polarized; its electric dipole moment is μ = 0.04⋅10 ⁻²⁹ C · m . Numerous studies have shown that the negative charge in the CO molecule is concentrated on the carbon atom C ^- ← O ⁺ (the direction of the dipole moment in the molecule is opposite to that previously assumed). The ionization energy is 14.0 eV , the binding force constant is k = 18.6 .

Properties

Carbon monoxide (II) is a colorless gas with no taste or smell. Combustible. The so-called "smell of carbon monoxide" is actually a smell of organic impurities.

The properties of carbon monoxide (II)
Gibbs standard energy of formation Δ G	−137.14 kJ / mol (g) (at 298 K)
Standard Education Entropy S	197.54 J / mol · K (g) (at 298 K)
Standard molar heat capacity C _p	29.11 J / mol · K (g) (at 298 K)
Enthalpy of melting Δ H _pl	0.838 kJ / mol
Enthalpy of boiling Δ H _bales	6.04 kJ / mol
Critical temperature t _crit	−140.23 ° C
Critical pressure P _crit	3,499 MPa
Critical density ρ _crit	0.301 g / cm³

The main types of chemical reactions in which carbon monoxide (II) is involved are addition reactions and redox reactions in which it exhibits reducing properties.

At room temperatures, CO is inactive, its chemical activity increases significantly when heated and in solutions. So, in solutions it reduces salts of Au , Pt , Pd and others to metals even at room temperature. When heated, it also reduces other metals, for example, CO + CuO → Cu + CO ₂ ↑. It is widely used in pyrometallurgy . The reaction of CO in solution with palladium chloride is based on the method for the qualitative detection of CO, see below.

The oxidation of CO in solution often proceeds at a noticeable rate only in the presence of a catalyst. When selecting the latter, the main role is played by the nature of the oxidizing agent. So, KMnO ₄ most quickly oxidizes CO in the presence of finely divided silver , K ₂ Cr ₂ O ₇ in the presence of mercury salts, KClO ₃ in the presence of OsO ₄ . In general, in its reducing properties, CO is similar to molecular hydrogen.

Below 830 ° C, a stronger reducing agent is CO, and above, hydrogen. Therefore the equilibrium reaction

{\mathsf {H_{2}O+CO\rightleftarrows CO_{2}+H_{2}}}

{\ displaystyle {\ mathsf {H_ {2} O + CO \ rightleftarrows CO_ {2} + H_ {2}}}}

up to 830 ° C shifted to the right, above 830 ° C to the left.

Interestingly, there are bacteria that can, due to CO oxidation, get the energy they need for life.

Carbon monoxide (II) burns with a blue flame ^[3] (reaction start temperature 700 ° C ) in air:

{\mathsf {2CO+O_{2}\rightarrow 2CO_{2}}}

{\ displaystyle {\ mathsf {2CO + O_ {2} \ rightarrow 2CO_ {2}}}}

( Δ G ° ₂₉₈ = −257 kJ, Δ S ° ₂₉₈ = −86 J / K).

The combustion temperature of CO can reach 2100 ° C. The combustion reaction is a chain reaction, with small amounts of hydrogen-containing compounds (water, ammonia , hydrogen sulfide , etc.) being the initiators.

Due to such a good calorific value, CO is a component of various technical gas mixtures (see, for example, generator gas ), which are also used for heating. It is explosive when mixed with air; lower and upper concentration limits of flame propagation: from 12.5 to 74% (by volume) ^[4] .

Carbon monoxide (II) reacts with halogens . The reaction with chlorine has received the greatest practical application:

{\mathsf {CO+Cl_{2}{\xrightarrow {h\nu }}COCl_{2}}}.

{\ displaystyle {\ mathsf {CO + Cl_ {2} {\ xrightarrow {h \ nu}} COCl_ {2}}}.}

The reaction is exothermic, its thermal effect is 113 kJ , in the presence of a catalyst ( activated carbon ) it proceeds even at room temperature. As a result of the reaction, phosgene is formed - a substance that is widely used in various branches of chemistry (and also as a chemical warfare agent ). By similar reactions, COF ₂ ( carbonyl fluoride ) and COBr ₂ ( carbonyl bromide) can be obtained. Carbonyl iodide not obtained. The exothermicity of reactions rapidly decreases from F to I (for reactions with F _{2, the} thermal effect is 481 kJ , with Br ₂ - 4 kJ ). You can also get mixed derivatives, for example COFCl (for more details see halogen derivatives of carbonic acid ).

By reacting CO with F ₂ , in addition to carbonyl fluoride COF ₂ , a peroxide compound (FCO) ₂ O ₂ can be obtained. Its characteristics: melting point −42 ° C , boiling +16 ° C , has a characteristic odor (similar to the smell of ozone ), when heated above 200 ° C decomposes with an explosion (reaction products CO ₂ , O ₂ and COF ₂ ), in acidic medium reacts with potassium iodide according to the equation:

{\mathsf {(FCO)_{2}O_{2}+2KI\rightarrow 2KF+I_{2}+2CO_{2}.}}

{\ displaystyle {\ mathsf {(FCO) _ {2} O_ {2} + 2KI \ rightarrow 2KF + I_ {2} + 2CO_ {2}.}}}

Carbon monoxide (II) reacts with chalcogenes . It forms carbon sulfide COS with sulfur , the reaction occurs when heated, according to the equation:

{\mathsf {CO+S\rightarrow COS}}

{\ displaystyle {\ mathsf {CO + S \ rightarrow COS}}}

( Δ G ° ₂₉₈ = −229 kJ, Δ S ° ₂₉₈ = −134 J / K).

Similar carbon selenoxide COSe and carbon telluroxide COTe were also obtained.

Recovers SO ₂ :

{\mathsf {2CO+SO_{2}\rightarrow 2CO_{2}+S.}}

{\ displaystyle {\ mathsf {2CO + SO_ {2} \ rightarrow 2CO_ {2} + S.}}}

With transition metals it forms combustible and toxic compounds - carbonyls , such as [Fe (CO) ₅ ], [Cr (CO) ₆ ], [Ni (CO) ₄ ], [Mn ₂ (CO) ₁₀ ], [Co ₂ ( CO) ₉ ] and others. Some of them are volatile.

{\mathsf {nCO+Me\rightarrow [Me(CO)_{n}]}}

{\ displaystyle {\ mathsf {nCO + Me \ rightarrow [Me (CO) _ {n}]}}}

Carbon monoxide (II) is slightly soluble in water, but does not react with it. Also, it does not react with solutions of alkalis and acids . However, it reacts with alkali melts with the formation of the corresponding formates :

{\mathsf {CO+KOH\rightarrow HCOOK.}}

{\ displaystyle {\ mathsf {CO + KOH \ rightarrow HCOOK.}}}

An interesting reaction is carbon monoxide (II) with potassium metal in an ammonia solution. In this case, an explosive compound potassium dioxodicarbonate is formed :

{\mathsf {2K+2CO\rightarrow K_{2}C_{2}O_{2}.}}

{\ displaystyle {\ mathsf {2K + 2CO \ rightarrow K_ {2} C_ {2} O_ {2}.}}}

By reacting with ammonia at high temperatures, an important industrial compound, HCN cyanide, can be obtained. The reaction proceeds in the presence of a catalyst ( thorium dioxide ThO ₂ ) according to the equation:

{\mathsf {CO+NH_{3}\rightarrow H_{2}O+HCN.}}

{\ displaystyle {\ mathsf {CO + NH_ {3} \ rightarrow H_ {2} O + HCN.}}}

The most important property of carbon monoxide (II) is its ability to react with hydrogen to form organic compounds ( Fischer-Tropsch synthesis process ):

{\mathsf {xCO+yH_{2}\rightarrow }}

{\ displaystyle {\ mathsf {xCO + yH_ {2} \ rightarrow}}}

alcohols + linear alkanes.

This process is a source of production for such important industrial products as methanol , synthetic diesel fuel, polyhydric alcohols, oils and lubricants.

Physiological Action

Toxicity

Carbon monoxide is very toxic.

TLV (US Threshold Limit Concentration): 25 ppm ; 29 mg / m³ (as TWA - average shift concentration, USA) (ACGIH 1994-1995). MAC (Maximum Allowed Concentration, USA): 30 ppm ; 33 mg / m³ ; Pregnancy: B (harmful effect is probable even at the MAK level) (1993). MPC according to Hygienic standards, GN 2.2.5.1313-03 is 20 mg / m³ (about 0.0017%).

In the exhaust of a gasoline car, up to 1.5-3% is allowed (the permissible concentration varies greatly depending on the country / applicable standards; and 3% is a lot even for an old carburetor car without a catalyst).

According to the UN classification , carbon monoxide (II) belongs to hazard class 2.3, the secondary hazard according to the UN classification: 2.1.

Carbon monoxide is very dangerous because it is odorless and causes poisoning and even death . ^[5] Signs of poisoning: headache and dizziness ; tinnitus, shortness of breath, palpitations, flickering before the eyes, redness of the face, general weakness, nausea, sometimes vomiting are noted; in severe cases, convulsions, loss of consciousness , coma ^[6] ^[3] .

The toxic effect of carbon monoxide (II) is due to the formation of carboxyhemoglobin , a much stronger carbonyl complex with hemoglobin , compared with the complex of hemoglobin with oxygen (oxyhemoglobin) ^[6] . Thus, the processes of oxygen transport and cellular respiration are blocked. A concentration in the air of more than 0.1% leads to death within one hour ^[6] .

Experiments on young rats showed that the concentration of CO in the air of 0.02% slows their growth and reduces activity compared with the control group.

Help with carbon monoxide poisoning

The combination of carbon monoxide with hemoglobin is reversible. In case of poisoning, the following actions are recommended ^[6] :

The victim should be taken out to fresh air. In case of mild poisoning, hyperventilation of the lungs with oxygen is sufficient.
Artificial ventilation of the lungs.
Lobelin or caffeine under the skin.
Carboxylase intravenously.

Reliable antidotes for use in case of carbon monoxide poisoning are unknown to world medicine ^[7] .

Carbon Monoxide (II) Protection

CO is very weakly absorbed by activated carbon from conventional filtering gas masks , therefore a special filtering element is used to protect it from it (it can also be connected in addition to the main one) - a hopcalite cartridge. Hopcalite is a catalyst that promotes the oxidation of CO to CO ₂ at normal temperatures. The disadvantage of using hopcalite is that during its use it is necessary to inhale the air heated as a result of the reaction. A common method of protection is the use of an insulating breathing apparatus ^[3] .

Endogenous Carbon Monoxide

Endogenous carbon monoxide is produced normally by cells of the human and animal body and acts as a signaling molecule. It plays a well-known physiological role in the body, in particular, it is a neurotransmitter and causes vasodilation ^[8] . Due to the role of endogenous carbon monoxide in the body, metabolic disorders are associated with various diseases, such as neurodegenerative diseases, atherosclerosis of blood vessels , hypertension , heart failure , and various inflammatory processes ^[8] .

Endogenous carbon monoxide is formed in the body due to the oxidizing effect of the hemoxygenase enzyme on heme , which is a product of the destruction of hemoglobin and myoglobin , as well as other heme -containing proteins. This process causes the formation of a small amount of carboxyhemoglobin in the blood of a person, even if a person does not smoke and does not breathe atmospheric air (always containing small amounts of exogenous carbon monoxide), but with pure oxygen or a mixture of nitrogen and oxygen.

Following the first data that appeared in 1993 that endogenous carbon monoxide is a normal neurotransmitter in the human body ^[9] ^[10] , as well as one of three endogenous gases that normally modulate the course of inflammatory reactions in the body (the other two are oxide nitrogen (II) and hydrogen sulfide ), endogenous carbon monoxide has attracted considerable attention of clinicians and researchers as an important biological regulator. It has been shown that in many tissues all three of the above gases are anti-inflammatory substances, vasodilators , and also cause angiogenesis ^[11] . However, not everything is so simple and straightforward. Angiogenesis is not always a beneficial effect, since it, in particular, plays a role in the growth of malignant tumors, and is also one of the causes of retinal damage in macular degeneration. In particular, it is important to note that smoking (the main source of carbon monoxide in the blood, giving it several times higher concentration than natural products) increases the risk of macular degeneration of the retina by 4-6 times.

There is a theory that in some synapses of nerve cells where long-term storage of information takes place, the receiving cell in response to the received signal produces endogenous carbon monoxide, which transmits a signal back to the transmitting cell, which informs it of its readiness to continue to receive signals from it and increasing the activity of the signal transmitter cell. Some of these nerve cells contain guanylate cyclase, an enzyme that is activated by exposure to endogenous carbon monoxide ^[10] .

Studies on the role of endogenous carbon monoxide as an anti-inflammatory substance and cytoprotector have been carried out in many laboratories around the world. These properties of endogenous carbon monoxide make its metabolism an interesting therapeutic target for treating such various pathological conditions as tissue damage caused by ischemia and subsequent reperfusion (and this, for example, myocardial infarction , ischemic stroke ), graft rejection, vascular atherosclerosis, severe sepsis , severe malaria , autoimmune diseases. Clinical trials were also conducted on humans, but their results have not yet been published ^[12] .

Summing up, what is known for 2015 about the role of endogenous carbon monoxide in the body can be summarized as follows ^[13] :

Endogenous carbon monoxide is one of the important endogenous signaling molecules;
Endogenous carbon monoxide modulates the functions of the central nervous system and cardiovascular system ;
Endogenous carbon monoxide inhibits platelet aggregation and their adhesion to the walls of blood vessels;
The effect on the exchange of endogenous carbon monoxide in the future may be one of the important therapeutic strategies for a number of diseases.

Discovery History

The toxicity of smoke emitted during the combustion of coal has been described by Aristotle and Galen .

Carbon monoxide (II) was first obtained by the French chemist Jacques de Lasson in 1776 when heating zinc oxide with coal, but initially it was mistaken for hydrogen, since it burned with a blue flame.

The fact that the composition of this gas includes carbon and oxygen was discovered in 1800 by the English chemist William Kruykshenk . Gas toxicity was investigated in 1846 by French physician Claude Bernard in experiments on dogs ^[14] .

Carbon monoxide (II) outside the Earth’s atmosphere was first discovered by the Belgian scientist M. Migeotte in 1949 by the presence of the main vibrational-rotational band in the infrared spectrum of the Sun. Carbon monoxide in the interstellar medium was discovered in 1970 ^[15]

Getting

Industrial Way

The effect of temperature on the equilibrium of the reaction:

{\mathsf {CO_{2}+C\rightleftarrows 2CO}}

{\ displaystyle {\ mathsf {CO_ {2} + C \ rightleftarrows 2CO}}}

It is formed during the combustion of carbon or compounds based on it (for example, gasoline ) in conditions of oxygen deficiency:

{\mathsf {2C+O_{2}\rightarrow 2CO}}

{\ displaystyle {\ mathsf {2C + O_ {2} \ rightarrow 2CO}}}

(the thermal effect of this reaction is 220 kJ ),

or when reducing carbon dioxide with hot coal:

{\mathsf {CO_{2}+C\rightleftarrows 2CO}}

{\ displaystyle {\ mathsf {CO_ {2} + C \ rightleftarrows 2CO}}}

( Δ H = 172 kJ , Δ S = 176 J / K )

This reaction occurs with the furnace furnace, when the furnace damper is closed too early (until the coals are finally burnt out). The carbon monoxide (II) thus formed due to its toxicity causes physiological disorders (“fumes”) and even death (see below), hence one of the trivial names is “carbon monoxide” ^[3] .

The reaction of reducing carbon dioxide is reversible, the effect of temperature on the equilibrium state of this reaction is shown in the graph. The reaction to the right provides the entropy factor, and to the left, the enthalpy factor. At temperatures below 400 ° C, the equilibrium is almost completely shifted to the left, and at temperatures above 1000 ° C to the right (towards the formation of CO). At low temperatures, the rate of this reaction is very low; therefore, carbon monoxide (II) is quite stable under normal conditions. This equilibrium is specifically called the Boudoir equilibrium .

Mixtures of carbon monoxide (II) with other substances are obtained by passing air, water vapor, etc. through a layer of hot coke, coal or brown coal, etc. (see generator gas , water gas , mixed gas , synthesis gas )

Lab Method

The decomposition of liquid formic acid under the action of hot concentrated sulfuric acid or the passage of gaseous formic acid over phosphorus oxide P ₂ O ₅ . Reaction Scheme:

{\mathsf {HCOOH{\xrightarrow[{H_{2}SO_{4}}]{^{o}t}}H_{2}O+CO.}}

{\ displaystyle {\ mathsf {HCOOH {\ xrightarrow [{H_ {2} SO_ {4}}] {^ {o} t}} H_ {2} O + CO.}}}

You can also treat formic acid chlorosulfonic . This reaction proceeds already at ordinary temperature according to the scheme:

{\mathsf {HCOOH+ClSO_{3}H\rightarrow H_{2}SO_{4}+HCl+CO\uparrow .}}

{\ displaystyle {\ mathsf {HCOOH + ClSO_ {3} H \ rightarrow H_ {2} SO_ {4} + HCl + CO \ uparrow.}}}

Heating a mixture of oxalic and concentrated sulfuric acids . The reaction proceeds according to the equation:

{\mathsf {H_{2}C_{2}O_{4}{\xrightarrow[{H_{2}SO_{4}}]{^{o}t}}CO\uparrow +CO_{2}\uparrow +H_{2}O.}}

{\ displaystyle {\ mathsf {H_ {2} C_ {2} O_ {4} {\ xrightarrow [{H_ {2} SO_ {4}}] {^ {o} t}} CO \ uparrow + CO_ {2} \ uparrow + H_ {2} O.}}}

Heating a mixture of potassium hexacyanoferrate (II) with concentrated sulfuric acid. The reaction proceeds according to the equation:

{\mathsf {K_{4}[Fe(CN)_{6}]+6H_{2}SO_{4}+6H_{2}O{\xrightarrow[{}]{^{o}t}}2K_{2}SO_{4}+FeSO_{4}+3(NH_{4})_{2}SO_{4}+6CO\uparrow .}}

{\ displaystyle {\ mathsf {K_ {4} [Fe (CN) _ {6}] + 6H_ {2} SO_ {4} + 6H_ {2} O {\ xrightarrow [{}] {^ {o} t} } 2K_ {2} SO_ {4} + FeSO_ {4} +3 (NH_ {4}) _ {2} SO_ {4} + 6CO \ uparrow.}}}

Reduction from zinc carbonate with magnesium when heated:

{\mathsf {Mg+ZnCO_{3}{\xrightarrow[{}]{^{o}t}}MgO+ZnO+CO\uparrow .}}

{\ displaystyle {\ mathsf {Mg + ZnCO_ {3} {\ xrightarrow [{}] {^ {o} t}} MgO + ZnO + CO \ uparrow.}}}

Determination of carbon monoxide (II)

You can qualitatively determine the presence of CO by darkening the solutions of palladium chloride (or paper impregnated with this solution). The darkening is associated with the release of finely divided metallic palladium according to the scheme:

{\mathsf {PdCl_{2}+CO+H_{2}O\rightarrow Pd\downarrow +CO_{2}+2HCl.}}

{\ displaystyle {\ mathsf {PdCl_ {2} + CO + H_ {2} O \ rightarrow Pd \ downarrow + CO_ {2} + 2HCl.}}}

This reaction is very sensitive. Standard solution: 1 gram of palladium chloride per liter of water.

Quantification of carbon monoxide (II) is based on an iodometric reaction:

{\mathsf {5CO+I_{2}O_{5}\rightarrow 5CO_{2}+I_{2}.}}

{\ displaystyle {\ mathsf {5CO + I_ {2} O_ {5} \ rightarrow 5CO_ {2} + I_ {2}.}}}

Application

Carbon monoxide (II) is an intermediate reagent used in reactions with hydrogen in the most important industrial processes for the production of organic alcohols and unbranched hydrocarbons.
Carbon monoxide (II) is used to process meat of animals and fish, gives them a bright red color and appearance of freshness, without changing the taste ( and technologies). Permissible concentration of CO is 200 mg / kg of meat.
Carbon monoxide (II) is the main component of the generator gas used as fuel in gas-generating vehicles .
Carbon monoxide from engine exhaust was used by the Nazis during the Second World War to mass kill people by poisoning.
- Gas chamber
- Gazenvagen

Carbon Monoxide (II) in the Earth's atmosphere

CO in the Earth’s atmosphere according to MOPITT

Distinguish between natural and man-made sources of entry into the Earth’s atmosphere . Under natural conditions, on the surface of the Earth, CO is formed during incomplete anaerobic decomposition of organic compounds and during the combustion of biomass, mainly during forest and steppe fires. Carbon monoxide (II) is formed in the soil both biologically (excretion by living organisms) and non-biological. The emission of carbon monoxide (II) was experimentally proved due to phenolic compounds common in soils containing OCH ₃ or OH groups in ortho or para positions with respect to the first hydroxyl group.

The overall balance of the production of non-biological CO and its oxidation by microorganisms depends on specific environmental conditions, primarily on humidity and pH . For example, from arid soils, carbon monoxide (II) is released directly into the atmosphere, thus creating local maxima of the concentration of this gas.

In the atmosphere, CO is the product of reaction chains involving methane and other hydrocarbons (primarily isoprene).

The main anthropogenic source of CO is currently the exhaust gases of internal combustion engines . Carbon monoxide is formed during the combustion of hydrocarbon fuels in internal combustion engines at inadequate temperatures or a poorly configured air supply system (insufficient oxygen is supplied to oxidize CO to CO ₂ ). In the past, a significant proportion of the anthropogenic release of CO into the atmosphere was provided by the luminescent gas used to illuminate the premises in the 19th century . In composition, it approximately corresponded to water gas , that is, it contained up to 45% carbon monoxide (II). In the utility sector, it is not applied due to the presence of a much cheaper and energy-efficient analogue - natural gas .

The receipt of CO from natural and man-made sources is approximately the same.

Carbon monoxide (II) in the atmosphere is in a rapid cycle: its average residence time is about 0.1 year . The main channel for CO loss is hydroxyl oxidation to carbon dioxide.

Carbon Monoxide (II) in Outer Space

Carbon monoxide (II) is the second most abundant (after H ₂ ) molecule in the interstellar medium ^[15] . This gas plays an important role in the evolution of molecular gas clouds in which active star formation occurs. Like other molecules, CO emits a number of infrared lines arising from transitions between the rotational levels of the molecule; these levels are already excited at temperatures of several tens of Kelvin. The concentration of CO in the interstellar medium is small enough so that (in contrast to the much more widespread H ₂ molecule) the radiation in the molecular rotational lines does not experience strong self-absorption in the cloud. As a result, energy almost unhindered leaves the cloud, which cools and contracts, triggering the star formation mechanism. In the densest clouds, where the self-absorption in the CO lines is significant, the energy loss in the lines of the rare isotopic analogue of ¹³ CO becomes noticeable (the relative isotopic abundance of ¹³ C is about 1%). Due to its stronger radiation, in comparison with atomic hydrogen, carbon monoxide (II) is used to search for such gas clusters. In February 2012, astronomers using the Planck European Space Telescope compiled the most complete map of its distribution over the celestial sphere ^[16] .

Notes

↑ Carbon Monoxide | Cameo Chemicals | Noaa
↑ ¹ ² ³ http://www.cdc.gov/niosh/npg/npgd0105.html
↑ ¹ ² ³ ⁴ Carbon monoxide (neopr.) (Inaccessible link) . Russian encyclopedia on labor protection: 3 vol. - 2nd ed., Revised. and add. - M.: Publishing House NTs ENAS, 2007. Date of treatment June 5, 2012. Archived June 22, 2012.
↑ Baratov A.N. Fire and explosion hazard of substances and materials and means for extinguishing them: Reference publication: in 2 books. - M .: Chemistry, 1990. - T. Book 2. - P. 384.
↑ Roshchin A.V., Tomilin V.V., Sternberg E.Ya. Carbon monoxide // Big Medical Encyclopedia : in 30 tons / hl. ed. B.V. Petrovsky . - 3 ed. - Moscow: Soviet Encyclopedia , 1981. - T. 17. Nilander test - Osteopathy . - 512 s. - 150,800 copies.
↑ ¹ ² ³ ⁴ Handbook of the Paramedic, ed. A. N. Shabanova. - M .: "Medicine", 1984.
↑ Scientists hunt for carbon monoxide poisoning antidote (Eng.) , Associated Press (December 9, 2016). Released September 29, 2018. "we don't have antidotes for carbon monoxide poisoning, and it's the most common poisoning."
↑ ¹ ² Wu, L; Wang, R. Carbon Monoxide: Endogenous Production, Physiological Functions, and Pharmacological Applications (English) // Pharmacol Rev : journal. - 2005 .-- December ( vol. 57 , no. 4 ). - P. 585-630 . - DOI : 10.1124 / pr . 57.4.3 . - PMID 16382109 .
↑ Verma, A; Hirsch, D .; Glatt, C .; Ronnett, G .; Snyder, S. Carbon monoxide: A putative neural messenger (Eng.) // Science. - 1993. - Vol. 259 , no. 5093 . - P. 381-384 . - DOI : 10.1126 / science.7678352 . - . - PMID 7678352 .
↑ ¹ ² Kolata, Gina . Carbon Monoxide Gas Is Used by Brain Cells As a Neurotransmitter (January 26, 1993). Date of treatment May 2, 2010.
↑ Li, L; Hsu, A; Moore, PK Actions and interactions of nitric oxide, carbon monoxide and hydrogen sulphide in the cardiovascular system and in inflammation — a tale of three gases! (English) // Pharmacology & therapeutics : journal. - 2009. - Vol. 123 , no. 3 . - P. 386-400 . - DOI : 10.1016 / j.pharmthera.2009.05.05.005 . - PMID 19486912 .
↑ Johnson, Carolyn Y .. Poison gas may carry a medical benefit (October 16, 2009). Date of appeal October 16, 2009.
↑ Olas, Beata. Carbon monoxide is not always a poison gas for the human organism: Physiological and pharmacological features of CO (Eng.) // Chemico-Biological Interactions : journal. - 2014 .-- 25 April ( vol. 222 , no. 5 October 2014 ). - P. 37-43 . - DOI : 10.1016 / j.cbi.2014.08.08.005 .
↑ Rosemary H. Waring, Glyn B. Steventon, Steve C. Mitchell. Molecules of death . - Imperial College Press, 2007. - P. 38. - ISBN 1-86094-814-6 .
↑ ¹ ² Combes, Françoise. Distribution of CO in the Milky Way (Eng.) // Annual Review of Astronomy & Astrophysics : journal. - 1991. - Vol. 29 . - P. 195 . - DOI : 10.1146 / annurev.aa.29.09019191.001211 . - .
↑ Planck compiled a map of carbon monoxide in the Galaxy ( Lenta.ru ).

Literature

Akhmetov N.S. General and inorganic chemistry. 5th ed., Rev. - M .: Higher. school; 2003 ISBN 5-06-003363-5
Nekrasov B.V. Fundamentals of General Chemistry. T. I, ed. 3rd, fix and add. Publishing house "Chemistry", 1973 p. 495–497, 511–513
Chemistry: Ref. from. / B. Schroeter, K.-H. Lautenschleger, H. Bibrak et al.: Pers. with him. 2nd ed., Stereotype. - M.: Chemistry, 2000 ISBN 5-7245-0360-3 (Russian)
Baratov A. N. Fire and explosion hazard of substances and materials and means for extinguishing them: Reference publication: in 2 books; Book 2. - M.: Chemistry, 1990 - 384s.

Links

International Chemical Safety Map for Carbon Monoxide (ICSC 0023, April 2007 )

[1] Carbon Monoxide | Cameo Chemicals | Noaa

[_a3731c1905176b30-2] ¹ ² ³ http://www.cdc.gov/niosh/npg/npgd0105.html

[охр_2012-3] ¹ ² ³ ⁴ Carbon monoxide (neopr.) (Inaccessible link) . Russian encyclopedia on labor protection: 3 vol. - 2nd ed., Revised. and add. - M.: Publishing House NTs ENAS, 2007. Date of treatment June 5, 2012. Archived June 22, 2012.

[4] Baratov A.N. Fire and explosion hazard of substances and materials and means for extinguishing them: Reference publication: in 2 books. - M .: Chemistry, 1990. - T. Book 2. - P. 384.

[БМЭ-3изд-ТОМ-17-5] Roshchin A.V., Tomilin V.V., Sternberg E.Ya. Carbon monoxide // Big Medical Encyclopedia : in 30 tons / hl. ed. B.V. Petrovsky . - 3 ed. - Moscow: Soviet Encyclopedia , 1981. - T. 17. Nilander test - Osteopathy . - 512 s. - 150,800 copies.

[Shab-6] ¹ ² ³ ⁴ Handbook of the Paramedic, ed. A. N. Shabanova. - M .: "Medicine", 1984.

[7] Scientists hunt for carbon monoxide poisoning antidote (Eng.) , Associated Press (December 9, 2016). Released September 29, 2018. "we don't have antidotes for carbon monoxide poisoning, and it's the most common poisoning."

[endogenous_co-8] ¹ ² Wu, L; Wang, R. Carbon Monoxide: Endogenous Production, Physiological Functions, and Pharmacological Applications (English) // Pharmacol Rev : journal. - 2005 .-- December ( vol. 57 , no. 4 ). - P. 585-630 . - DOI : 10.1124 / pr . 57.4.3 . - PMID 16382109 .

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[16] Planck compiled a map of carbon monoxide in the Galaxy ( Lenta.ru ).