- Melting point:−78.5 °C(lit.)
- Boiling point:-78.46°C
- Density 1.977（0℃）
- vapor density 1.52 (vs air)
- vapor pressure 56.5 atm ( 20 °C)
- refractive index 1.0004
- storage temp. −70°C
- solubility At 20 °C and at a pressure of 101 kPa, 1 volume dissolves in about 1 volume of water.
- form colorless gas
- Water Solubility mL CO2/100mL H2O at 760mm: 171 (0°C), 88 (20°C), 36 (60°C) [MER06]
- Merck 13,1819
- BRN 1900390
- Exposure limitsTLV-TWA 5000 ppm (～9000 mg/m3) (ACGIH, MSHA, and OSHA); STEL 30,000 ppm (ACGIH).
- Stability:Stable. Incompatible with chemically active metals, such as alkali metals.
- CAS DataBase Reference124-38-9(CAS DataBase Reference)
- EPA Substance Registry SystemCarbon dioxide (124-38-9)
- UsesCarbon dioxide (CO2) is the 18th most frequently produced chemical in the United States. It has numerous uses, including in refrigeration, in the manufacture of carbonated drinks (e.g., soda pop), in fire extinguishers, in providing an inert atmosphere (unreactive environment), and as a moderator for some types of nuclear reactors.
- DescriptionCarbon dioxide is a colorless, odorless gas present throughout the atmosphere and is an essential compound for life on Earth. It is found on other planets in the solar system. Mars’s icecaps are primarily frozen carbon dioxide and Venus’s atmosphere is mostly carbon dioxide.
- Chemical PropertiesCarbon dioxide,CO2, also known as carbonic anhydride and carbonic acid gas, is a colorless,odorless gas that liquifies at -65 °C(-86 OF) and solidifies in dry ice at -78.2 °C(-107 OF). It is soluble in water,alcohol, and most alkaline solutions. In a relatively slow reaction,carbon dioxide hydrates in water to become carbonic acid and is corrosive. In petroleum production, the velocity of the carbon dioxide gas can increase the corrosion rate to very high levels,with the presence of salts becoming unimportant. Carbon dioxide is used in preparing carbonated beverages, fire extinguishers, dry ice refrigerants,and as a raw material in the production of sodium carbonate and sodium bicarbonate using the Solvay procedure.
- Chemical PropertiesCarbon dioxide is a colorless, odorless, noncombustible gas.
- Chemical PropertiesCarbon dioxide occurs naturally as approximately 0.03% v/v of the atmosphere. It is a colorless, odorless, noncombustible gas with a faint acid taste. Solid carbon dioxide, also known as dry ice, is usually encountered as white-colored pellets or blocks.
- Physical propertiesColorless, odorless and tasteless gas; 1.53 times heavier than air; density 1.80 g/L at 25°C; can be liquefied under pressure; liquefies at -56.6°C at 5.2 atm; density of liquid CO2 at 0°C and 34 atm 0.914 g/mL; solidifies to white snow-like flakes known as dry ice, density 1.56 g/cm3 at -79°C; dry ice sub limes to CO2 gas at -78.5°C; critical temperature 31°C; critical pressure 72.79 atm, critical density 94 cm3/mol; moderately soluble in water, solubility 173 mL and 88mL CO2/100 mL water at 0°C and 20°C, respectively; solubility increases with pressure.
- OccurrenceCarbon dioxide is found throughout nature. Its concentration in the air is 0.036% by volume. It is the primary component of exhaled air of all animals. It also is the product of oxidation of all carbonaceous matter and an end prod?uct of complete combustion. It also is found dissolved in natural waters. It occurs in the earth’s crust and in volcanic eruptions.
All plants depend on carbon dioxide and water for their survival, making their food by the process of photosynthesis. Carbon dioxide is found in abun?dance in the atmospheres of many other planets and their moons throughout the solar system.
Carbon dioxide is a greenhouse gas, which traps the infrared radiation re?radiated back by the earth’s surface, causing global warming and, therefore, changing the climate. The CO2 concentration in the atmosphere over a 30- year period from 1960 to 1990 has increased significantly from about 320 to 356 ppm by volume, which is widely attributed to the growth of industrial and automobile CO2 emission during this period.
Carbon dioxide has extensive commercial applications. Some important applications of this compound include carbonation of beverages; as a fire extinguishing agent; in the manufacture of carbonates; as dry ice (solid CO2) for refrigeration; as an aerosol propellant; as a shielding gas for welding; as an inert atmosphere in preparation and handling of flammable substances; in cloud seeding; in fumigation of rice; to produce harmless smoke on stage; as an antiseptic; and as a supercritical fluid to extract organic pollutants for their analyses.
- HistoryThe discovery of carbon dioxide, credited to Joseph Black (1728–1799), played a critical role in supplanting the phlogiston theory and advancing the development of modern chemistry. Black, in his medical studies, was searching for a substance to dissolve kidney stones, but he switched his subject to a study of stomach acidity. Black was working with the carbonates magnesia alba (magnesium carbonate) and calcium carbonate (limestone) and observed that when magnesia alba was heated or reacted with acids, it produced a gas and a salt. Black, who published his work in 1756, called the gas “fixed air” and noted that it had properties similar to those described by Jan Baptista van Helmont (1577–1644) for spiritus sylvestrius. Spiritus sylvestrius was the gas produced during combustion processes, and van Helmont realized that this was the same gas produced during fermentation and when acids reacted with seashells.
- UsesCarbon Dioxide is a gas obtained during fermentation of glucose (grain sugar) to ethyl alcohol. it is used in pressure-packed foods as a propellant or aerating agent and is also used in the carbonation of beverages. it is released as a result of the acid carbonate reaction of leavening agents in baked goods to produce an increase in volume. as a solid, it is termed dry ice and is used for freezing and chilling.
- UsesCarbon dioxide has several major uses： Solid carbon dioxide, dry ice, is used as a refrigerant. Another major use of carbon dioxide is in the soda industry. Soda is sodium carbonate monohydrate (Na2CO3? H2O). Other forms of soda include washing soda, which is sodium carbonate decahydrate (Na2CO3? 10H2O), and baking soda, which is sodium bicarbonate (NaHCO3).Carbon dioxide is used as a gas in fire extinguishers, as an inflation gas for flotation devices, and as a propellant (for example in air guns). In recent years, the use of carbon dioxide as a supercritical fluid in green chemistry applications has increased. A supercritical fluid is a fluid with a temperature and pressure above its critical point.
- UsesIn the carbonation of beverages; manufacture of carbonates; in fire prevention and extinction; for inerting flammable materials during manufacture, handling and transfer; as propellant in aerosols; as dry ice for refrigeration; to produce harmless smoke or fumes on stage; as rice fumigant; as antiseptic in bacteriology and in the frozen food industry. Supercritical or liquid CO2 used in extraction of caffeine and hops aroma; dry cleaning; metal degreasing; cleaning semiconductor chips; paint spraying; polymer modification. Environmentally benign alternative to potentially hazardous solvents in organic and polymer chemistry.
- DefinitionChEBI: A one-carbon compound with formula CO2 in which the carbon is attached to each oxygen atom by a double bond. A colourless, odourless gas under normal conditions, it is produced during respiration by all animals, fungi and microorganism that depend directly or indirectly on living or decaying plants for food.
Carbon dioxide is produced as a by-product in many processes. It is pro duced as a by-product in the manufacture of lime from calcium carbonate:
CaCO3 →CaO + CO2
CO2 also is derived from synthesis gas which is a mixture of CO, CO2, H2 and N2 from air obtained by steam reforming. Carbon dioxide also is obtained by combustion of natural gas:
CH4 + 2O2 → CO2 + 2H2O
It also is obtained as a by-product in the Haber-Bosch process for the man ufacture of ammonia. The method involves passing steam and air over hot coke.
Carbon dioxide also is produced along with ethanol from fermentation of carbohydrates by yeast:
C6H12O6→2CO2 + 2C2H5OH
In the laboratory, CO2 may be produced by the reaction of any carbonate with a dilute mineral acid:
CaCO3 + 2HCl → CaCl2 + CO2 + H2O
- Production MethodsCarbon dioxide is obtained industrially in large quantities as a byproduct in the manufacture of lime; by the incineration of coke or other carbonaceous material; and by the fermentation of glucose by yeast. In the laboratory it may be prepared by dropping acid on a carbonate.
- Production MethodsCarbon dioxide accounts for 0.037% by volume of the atmosphere.Several methods can be used to produce large volumes of CO2. The combustion of coke or other carbonaceous substances produces results in CO2: C(coke) + O2 → CO2(g). In combustion processes, CO2 is concentrated by separating it from other gases using scrubbing and absorption techniques. Another source of CO2 involves the calcination (slow heating) of carbonates such as limestone, CaCO3: CaCO3(s)→ CaO + CO2(g).This process takes place in a lime kiln in the production of precipitated calcium carbonate at temperatures of from 500°C to 900°C. Carbon dioxide is also produced as a by-product in fermentation reactions to produce alcohols. An example is the fermentation of glucose, C6H12O6 to ethanol (C2H5OH): C6H12O6(aq)→ 2C2H5OH(aq) + 2CO2(g). Carbon dioxide is produced as a by-product in a number of syntheses, such as the Haber process, to produce ammonia.
- Definition1. The
solution of carbon dioxide in a liquid
under pressure, as in carbonated soft
2. The addition of carbon dioxide to compounds, e.g. the insertion of carbon dioxide into Grignard reagents.
- Definitioncarbon dioxide: A colourlessodourless gas, CO2, soluble in water,ethanol, and acetone; d. 1.977 g dm–3(0°C); m.p. –56.6°C; b.p. –78.5°C. It occursin the atmosphere (0.04% by volume)but has a short residence timein this phase as it is both consumedby plants during photosynthesis andproduced by respiration and by combustion.It is readily prepared in thelaboratory by the action of diluteacids on metal carbonates or of heaton heavy-metal carbonates. Carbondioxide is a by-product from themanufacture of lime and from fermentationprocesses.
Carbon dioxide has a small liquidrange and liquid carbon dioxide isproduced only at high pressures. Themolecule CO2 is linear with each oxygenmaking a double bond to the carbon.Chemically, it is unreactive andwill not support combustion. It dissolves in water to give carbonicacid.
Large quantities of solid carbondioxide (dry ice) are used in processesrequiring large-scale refrigeration. Itis also used in fire extinguishers as adesirable alternative to water formost fires, and as a constituent ofmedical gases as it promotes exhalation.It is also used in carbonateddrinks.
The level of carbon dioxide in theatmosphere has increased by some12% in the last 100 years, mainly becauseof extensive burning of fossilfuels and the destruction of largeareas of rain forest. This has beenpostulated as the main cause of theaverage increase of 0.5°C in globaltemperatures over the same period,through the greenhouse effect.Steps are now being taken to preventfurther increases in atmospheric CO2concentration and subsequent globalwarming.
- General DescriptionAn odorless, white solid. Can cause damaging frostbite. Noncombustible and nontoxic. Liquefies at -109°F. Can asphyxiate by displacement of air. Used as a refrigerant.
- Air & Water ReactionsWater soluble. Forms carbonic acid, a mild acid in water.
- Reactivity ProfileContact of very cold liquid/solid carbon dioxide with water may result in vigorous or violent boiling of the product and extremely rapid vaporization due to the large temperature differences involved. If the water is hot, there is the possibility that a liquid "superheat" explosion may occur. Pressures may build to dangerous levels if liquid gas contacts water in a closed container. With water forms weak carbonic acid in nonhazardous reaction. Dusts of magnesium, lithium, potassium, sodium, zirconium, titanium, and some magnesium-aluminum alloys, and heated aluminum, chromium, and magnesium when suspended in carbon dioxide are ignitable and explosive. This is especially true in the presence of strong oxidizers, such as peroxides. The presence of carbon dioxide in solutions of aluminum hydride in ether can cause violent decomposition on warming the residue, [J. Amer. Chem. Soc., 1948, 70, 877]. Dangers arising from the use of carbon dioxide in the fire prevention and extinguishing systems of confined volumes of air and flammable vapors are examined. The hazard associated with its use centers around the fact that large electrostatic discharges may be created that initiate explosion, [Quart. Saf. Summ., 1973, 44(1740, 10].
- HazardSolid damaging to skin and tissue; keep away from mouth and eyes. Asphyxia.
- Health HazardVapors may cause dizziness or asphyxiation without warning. Vapors from liquefied gas are initially heavier than air and spread along ground. Contact with gas or liquefied gas may cause burns, severe injury and/or frostbite.
- Health HazardCarbon dioxide is an asphyxiant. Exposureto about 9–10% concentration can causeunconsciousness in 5 minutes. Inhalation of3% CO2 can produce weak narcotic effects.Exposure to 2% concentration for severalhours can produce headache, increased bloodpressure, and deep respiration.
- Fire HazardNon-flammable gases. Containers may explode when heated. Ruptured cylinders may rocket.
- Agricultural UsesCarbon dioxide (CO2) is a compound of two oxygen
atoms covalently bonded to a carbon atom. It is a
colorless, odorless, tasteless gas, soluble in water,
ethanol and acetone, and is 15 times heavier than air.
Carbon dioxide occurs in the earth's atmosphere at an average of 0.04% by volume. The volume keeps changing, as it is consumed by plants during photosynthesis and replenished during respiration and combustion of biomass. CO2 is a major source of carbon for plants.
Carbon dioxide is readily prepared in a laboratory by the action of dilute acids on carbonates. It is also obtained as a by-product from the manufacture of lime and from fermentation processes. Chemically, CO2 is not reactive and does not support combustion. It gives carbonic acid on dissolution in water.
Carbon dioxide is one of the key materials for urea production. Liquid carbon dioxide is produced at high pressures and has a small liquid range. Solid carbon dioxide (known as dry ice), produced by subjecting gaseous carbon dioxide to pressure and temperature, is used in refrigeration, carbonated drinks and fire extinguishers. It is also a constituent of medical treatment, as it promotes exhalation.
The level of carbon dioxide in the atmosphere has increased by 12% in the last 100 years, mainly due to the burning of fossil fuels and the destruction of rain forests. The increased level of carbon dioxide is the main cause for an average increase of 0.5℃ in the mean global temperature through the greenhouse effect. Environmentalists urge that measures be taken to prevent any further increase in atmospheric carbon dioxide, and the subsequent global warming and melting of ice caps.
In calcareous soils, the partial pressure of carbon dioxide in the soil air influences its pH; it is 8.5 when free calcium carbonate in the soil is in equilibrium with atmospheric carbon dioxide. An increase in carbon dioxide in the soil air decreases the pH to around 7.3.
Applications of carbon dioxide include its use as (a) a refrigerant in either solid or liquid form, (b) an inert medium, (c) a chemical reactant, (d) a neutralizing agent for alkalis, (e) a pressurizing agent, and ( f ) an ingredient in the manufacture of aerated water.
- Agricultural UsesSolid carbon dioxide is known as dry ice. It is produced by cooling gaseous carbon dioxide under pressure.
Dry ice is used in refrigeration, carbonated drinks and fire extinguishers. It is also a constituent of medical gases, as it promotes exhalation.
- Pharmaceutical ApplicationsCarbon dioxide and other compressed gases such as nitrogen and
nitrous oxide are used as propellants for topical pharmaceutical
aerosols. They are also used in other aerosol products that work
satisfactorily with the coarse aerosol spray that is produced with
compressed gases, e.g. cosmetics, furniture polish, and window
The advantages of compressed gases as aerosol propellants are that they are less expensive; are of low toxicity; and are practically odorless and tasteless. Also, in comparison to liquefied gases, their pressures change relatively little with temperature. However, the disadvantages of compressed gases are that there is no reservoir of propellant in the aerosol and pressure consequently decreases as the product is used. This results in a change in spray characteristics. Additionally, if a product that contains a compressed gas as a propellant is actuated in an inverted position, the vapor phase, rather than the liquid phase, is discharged. Most of the propellant is contained in the vapor phase and therefore some of the propellant will be lost and the spray characteristics will be altered. Also, sprays produced using compressed gases are very wet. Valves, such as the vapor tap or double dip tube, are currently available and will overcome these problems.
Carbon dioxide is also used to displace air from pharmaceutical products by sparging and hence to inhibit oxidation. As a food additive it is used to carbonate beverages and to preserve foods such as bread from spoilage by mold formation, the gas being injected into the space between the product and its packaging.
Solid carbon dioxide is also widely used to refrigerate products temporarily, while liquid carbon dioxide, which can be handled at temperatures up to 318℃ under high pressure, is used as a solvent for flavors and fragrances, primarily in the perfumery and food manufacturing industries.
- Safety ProfileAn asphpant. See discussion of simple asphyxiants under ARGON. Experimental teratogenic and reproductive effects. Contact of solid carbon dioxide snow with the skin can cause burns. Dusts of magnesium, zirconium, titanium, and some magnesium-aluminum alloys igmte and then explode in COa atmospheres. Dusts of aluminum, chromium, and manganese ignite and then explode when heated in CO2. Several bulk metals wlll burn in CO2. Reacts vigorously with (Al + Na2O2), Cs2O, Mg(C2H5)2, Li, (Mg + Na2O2), K, KHC, Na, Na2C2, NaK, Ti. CO2 fire extingushers can produce highly incendiary sparks of 5-1 5 mJ at 10-20 kV by electrostatic discharge. Incompatible with acrylaldehyde, aziridme, metal acetylides, sodium peroxide.
- SafetyIn formulations, carbon dioxide is generally regarded as an essentially nontoxic material.
- Potential ExposureGaseous Carbon dioxide is used to carbonate beverages; as a weak acid in the textile, leather, and chemical industries; in water treatment; and in the manufacture of aspirin and white lead; for hardening molds in foundries; in food preservation, in purging tanks and pipe lines; as a fire extinguisher, in foams; and in welding. Because it is relatively inert, it is utilized as a pressure medium. It is also used as a propellant in aerosols; to promote plant growth in green houses; it is used medically as a respiratory stimulant; in the manufacture of carbonates; and to produce an inert atmosphere when an explosive or flammable hazard exists. The liquid is used in fire extinguishing equipment; in cylinders for inflating life rafts; in the manufacturing of dry ice, and as a refrigerant. Dry ice is used primarily as a refrigerant. Occupational exposure to carbon dioxide may also occur in any place where fermentation processes may deplete oxygen with the formation of carbon dioxide, e.g., in mines, silos, wells, vats, ships’ holds, etc.
- storageExtremely stable and chemically nonreactive. Store in a tightly sealed cylinder. Avoid exposure to excessive heat.
- ShippingCarbon dioxide (UN1013, UN2187), Hazard Class: 2.2; Labels: 2.2-Nonflammable compressed gas. Dry ice (UN1845), Hazard class 9 is considered a “miscellaneous hazardous material” and does not require a label. The gas and refrigerated liquid fall in Hazard Class 2.2 and there is no Packing Group; solid, dry ice falls in Hazard Class 9. Solid, dry ice carries the symbol “AW.” The letter “A” restricts the application of requirements of this subchapter to materials offered or intended for transportation by aircraft, unless the material is a hazardous substance or a hazardous waste. The letter “W” restricts the application of requirements of this subchapter to materials offered or intended for transportation by vessel, unless the material is a hazardous substance or a hazardous waste. Cylindersmust be transported in a secure upright position, in a wellventilated truck. Protect cylinder and labels from physical damage. The owner of the compressed gas cylinder is the only entity allowed by federal law (49CFR) to transport and refill them. It is a violation of transportation regulations to refill compressed gas cylinders without the express written permission of the owner.
- Purification MethodsPass the gas over CuO wire at 800o to oxidise CO and other reducing impurities (such as H2), then over copper dispersed on Kieselguhr at 180o to remove oxygen. Drying it at -78o removes the water vapour. Final purification is by vacuum distillation at liquid nitrogen temperature to remove non-condensable gases [Anderson et al. J Chem Soc 3498 1962]. Sulfur dioxide contaminant can be removed at 450o using silver wool combined with a plug of platinised quartz wool. Halogens are removed by using Mg, Zn or Cu, heated to 450o. [Glemsner in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 647 1963.]
- IncompatibilitiesThe substance decomposes on heating above 2000C producing toxic carbon monoxide. Reacts violently with strong bases and alkali metals. Various metal dusts from chemically active metals, such as magnesium, zirconium, titanium, aluminum, chromium, and manganese are ignitable and explosive when suspended and heated in carbon dioxide.
- IncompatibilitiesCarbon dioxide is generally compatible with most materials although it may react violently with various metal oxides or reducing metals such as aluminum, magnesium, titanium, and zirconium. Mixtures with sodium and potassium will explode if shocked.
- Waste DisposalReturn refillable compressed gas cylinders to supplier. Vent to atmosphere
- Regulatory StatusGRAS listed. Accepted for use in Europe as a food additive. Included in the FDA Inactive Ingredients Database (aerosol formulation for nasal preparations; IM and IV injections). Included in the Canadian List of Acceptable Non-medicinal Ingredients.
- Raw materialsEtanolAmmoniaActivated carbonCALCIUM CARBONATEMETALLURGICAL COKEDOLOMITE
- Preparation Products1,3-Thiazole-2-carbonyl chloride3,3,3-Trifluoropropionic acid4-TERT-BUTYLCYCLOHEXANECARBOXYLIC ACID2,6-Dihydroxybenzoic acid Naphthol AS-D1-Methyl-4-piperidinol hydrochloride2-(Trifluoromethyl)benzoic acid2,3,5,6-TETRAFLUORO-4-METHYLBENZOIC ACID2-Bromo-6-fluorobenzoic acid2,5-Dichloroisonicotinic acidChloroacetaldehyde diethyl acetal2-(TRIFLUOROMETHYL)-5-METHYLQUINOLINE-4-CARBOXYLIC ACIDTHIAZOLE-2-CARBOXYLIC ACID6-CHLORO-2-(TRIFLUOROMETHYL)QUINOLINE-4-CARBOXYLIC ACIDETHYL 4-PYRIDYLACETATE2-Thiophenesulfonyl chloride1-CHLOROPHTHALAZINEDL-2-Amino-4-methylpentanoic acidCinnamoyl chloride3-NITROPHENYLACETIC ACID3,6-DICHLORO-2-HYDROXY BENZOIC ACIDTANTALUM PENTAFLUORIDEZirconium carbonate oxideDimethylketeneN-(4-chlorophenyl)-2-hydroxy-9H-carbazole-3-carboxamideDiflunisal1-Hydroxy-2-naphthoic acidCyclopropylacetic acidN-Methylpyrrole-2-carboxylic acid2,6-HEPTANEDIONE4-NITROSODIPHENYLAMINE2,3,6-TRIFLUOROBENZOIC ACIDLithium acetate dihydrate1,1-diethylguanidine hydrochloride2,4,6-Trifluorobenzoic acid2,4,6-Trichlorobenzoic acidBromine chlorideRosemary Herb ExtractMagnesium acetate tetrahydrate
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