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Carbon dioxide is a colorless, odorless, noncombustible gas.

Carbon 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.

ChEBI: 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.

An odorless, white solid. Can cause damaging frostbite. Noncombustible and nontoxic. Liquefies at-109°F. Can asphyxiate by displacement of air. Used as a refrigerant.

Contact 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].

Water soluble. Forms carbonic acid, a mild acid in water.

Solid damaging to skin and tissue; keep away from mouth and eyes. Asphyxia.

Vapors 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.

Gaseous 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.

Non-flammable gases. Containers may explode when heated. Ruptured cylinders may rocket.

If dry ice gets into the eyes, get medical attention. If this chemical contacts the skin, get medical attention for frostbite. If a person breathes in large amounts of this chemical, move the exposed person to fresh air at oncend perform rescue breathing and CPR if heart action has stopped. Transfer promptly to a medical facility. If frostbite has occurred, seek medical attention immediately; do NOT rub the affected areas or flush them with water. In order to prevent further tissue damage, do NOT attempt to remove frozen clothing from frostbitten areas. If frostbite has NOT occurred, immediately and thoroughly wash contaminated skin with soap and water. Cylinders must 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.

Carbon 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.

The 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.

Carbon 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.

Return refillable compressed gas cylinders to supplier. Vent to atmosphere

Colorless, 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.

Carbon 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.

The 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.

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

Carbon 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 → CO_2(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: CaCO_3(s)→ CaO + CO_2(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): C₆H₁₂O_6(aq)→ 2C₂H₅OH_(aq) + 2CO_2(g). Carbon dioxide is produced as a by-product in a number of syntheses, such as the Haber process, to produce ammonia.

Carbon 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.

Pass 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.]

Carbon 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.

Solid 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.

Carbon 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 cleaners.
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.

In formulations, carbon dioxide is generally regarded as an essentially nontoxic material.

Carbon dioxide is nonnally present in the atmosphere at about 0.035 percent by volume. It is also a nonnal end-product of human and animal metabolism. The exhaled breath contains up to 5.6 percent carbon dioxide. The greatest physiological effect of carbon dioxide is to stimulate the respiratory center, thereby controlling the volume and rate of respiration. It is able to cause dilation and constriction of blood vessels and is a vital constituent of the acid-base mechanism that controls the pH of the blood.
Carbon dioxide acts as a stimulant and a depressant on the central nervous system. Increases in heart rate and blood pressure have been noted at a concentration of 7.6 percent, and dyspnea (labored breathing), headache, dizziness, and sweating occur if exposure at that level is prolonged. At concentrations of 10 percent and above, unconsciousness can result in I minute or less. Impainnent in perfonnance has been noted during prolonged exposure to concentrations of 3 percent carbon dioxide even when the oxygen concentration was 21 percent.

Carbon dioxide is an asphyxiant, means it causes toxicity by displacing oxygen from the breathing atmosphere primarily in enclosed spaces or in open spaces due to sudden release of massive amounts of CO2 (for example, forests fire or natural emission during a volcanic eruption) and results in hypoxia. Thehumanbody produces about 12 000–13 000 mmols per day of CO2 and is excreted primarily via lungs. The CO2 concentration in plasma is maintained within a narrow range of 40±5 mm Hg (4.7–6 KPa). At plasma concentration of 22.5mmHg (3 KPa) or less death can occur within few minutes. The cause of death in breathing high concentration ofCO2 is due to CO2 poisoning, that results in rapid decrease in blood pH (respiratory acidosis, Low concentrations of CO2 in the air, or insufficient time for CO2 in blood to exchange with oxygen (O2) in air such as in the situations of hyperventilation, can lead to an increase in blood pH (respiratory alkalosis, >pH 7.45). The reaction of CO2 with water in the body is catalyzed by the enzyme carbonic anhydrases (or carbonate dehydratases), which leads to formation of carbonic acid, followed by dissociation into protons (H+) and bicarbonate (HCO3^-
). Carbonic acid is buffered in the cell primarily by hemoglobin and proteins, which have limited capacity.

Extremely stable and chemically nonreactive. Store in a tightly sealed cylinder. Avoid exposure to excessive heat.

The CO2 cycle is part of carbon cycle in the ecosystem. Carbon dioxide cycles in the environment (atmospheric air and surface water) through respiration (aerobic and anaerobic), photosynthesis, decomposition, and release from earth’s carbon sinks (fossil fuels – coal, petroleum, methane; and calcium carbonate rocks) during combustion. In water, dissolved CO2 reacts with calcium to form calcium carbonate and precipitates to the ocean floor. Few examples of most common reactions in the CO2 and carbon cycles in animals, plants, and the environment are presented below. Most of these reactions either use or produce energy.

GRAS 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.