Carbon dioxide

"CO2" redirects here. For other uses, see CO2 (disambiguation).
Carbon dioxide
Names
Other names
Carbonic acid gas
Carbonic anhydride
Carbonic oxide
Carbon oxide
Carbon(IV) oxide
Dry ice (solid phase)
Identifiers
124-38-9 YesY
3D model (Jmol) Interactive image
Interactive image
3DMet B01131
1900390
ChEBI CHEBI:16526 YesY
ChEMBL ChEMBL1231871 N
ChemSpider 274 YesY
ECHA InfoCard 100.004.271
EC Number 204-696-9
E number E290 (preservatives)
989
KEGG D00004 YesY
MeSH Carbon+dioxide
RTECS number FF6400000
UNII 142M471B3J YesY
UN number 1013 (gas), 1845 (solid)
Properties
CO2
Molar mass 44.01 g·mol−1
Appearance Colorless gas
Odor Odorless
Density 1562 kg/m3 (solid at 1 atm and −78.5 °C)
1101 kg/m3 (liquid at saturation −37°C)
1.977 kg/m3 (gas at 1 atm and 0 °C)
Melting point −56.6 °C; −69.8 °F; 216.6 K (Triple point at 5.1 atm)
−78.5 °C; −109.2 °F; 194.7 K (1 atm)
1.45 g/L at 25 °C (77 °F), 100 kPa
Vapor pressure 5.73 MPa (20 °C)
Acidity (pKa) 6.35, 10.33
1.00045
Viscosity 0.07 cP at −78.5 °C
0 D
Structure
trigonal
linear
Thermochemistry
37.135 J/K mol
214 J·mol−1·K−1
−393.5 kJ·mol−1
Pharmacology
V03AN02 (WHO)
Hazards
Safety data sheet See: data page
Sigma-Aldrich
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
1
0
Lethal dose or concentration (LD, LC):
90,000 ppm (human, 5 min)[1]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 5000 ppm (9000 mg/m3)[2]
REL (Recommended)
TWA 5000 ppm (9000 mg/m3) ST 30,000 ppm (54,000 mg/m3)[2]
IDLH (Immediate danger)
40,000 ppm[2]
Related compounds
Other anions
Carbon disulfide
Carbon diselenide
Carbon ditelluride
Other cations
Silicon dioxide
Germanium dioxide
Tin dioxide
Lead dioxide
Related carbon oxides
Carbon monoxide
Carbon suboxide
Dicarbon monoxide
Carbon trioxide
Related compounds
Carbonic acid
Carbonyl sulfide
Supplementary data page
Refractive index (n),
Dielectric constantr), etc.
Thermodynamic
data
Phase behaviour
solidliquidgas
UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Carbon dioxide (chemical formula CO2) is a colorless and odorless gas vital to life on Earth. This naturally occurring chemical compound is made up of a carbon atom covalently double bonded to two oxygen atoms. Carbon dioxide exists in Earth's atmosphere as a trace gas at a concentration of about 0.04 percent (400 ppm) by volume.[3] Natural sources include volcanoes, hot springs and geysers, and it is freed from carbonate rocks by dissolution in water and acids. Because carbon dioxide is soluble in water, it occurs naturally in groundwater, rivers and lakes, in ice caps and glaciers and also in seawater. It is present in deposits of petroleum and natural gas.[4]

Atmospheric carbon dioxide is the primary source of carbon in life on Earth and its concentration in Earth's pre-industrial atmosphere since late in the Precambrian was regulated by photosynthetic organisms and geological phenomena. As part of the carbon cycle, plants, algae, and cyanobacteria use light energy to photosynthesize carbohydrate from carbon dioxide and water, with oxygen produced as a waste product.[5]

Carbon dioxide (CO2) is produced by all aerobic organisms when they metabolize carbohydrates and lipids to produce energy by respiration.[6] It is returned to water via the gills of fish and to the air via the lungs of air-breathing land animals, including humans. Carbon dioxide is produced during the processes of decay of organic materials and the fermentation of sugars in bread, beer and winemaking. It is produced by combustion of organic materials such as natural vegetation and crop residues, wood and fossil fuels such as coal, peat, petroleum and natural gas.

It is a versatile industrial material, used, for example, as an inert gas in welding and fire extinguishers, as a pressurizing gas in air guns and oil recovery, as a chemical feedstock and in liquid form as a solvent in decaffeination of coffee and supercritical drying. It is added to drinking water and carbonated beverages including beer and sparkling wine to add effervescence. The frozen solid form of CO2, known as "dry ice" is used as a refrigerant and as an abrasive in dry-ice blasting.

Carbon dioxide is a significant greenhouse gas, but with a lower global warming potential than methane. Since the Industrial Revolution, anthropogenic emissions from the burning of carbon-based fossil fuels and land use changes (primarily deforestation) have rapidly increased its concentration in the atmosphere, leading to global warming. It is also a major cause of ocean acidification because it dissolves in water to form carbonic acid.[7]

Background

Crystal structure of dry ice

Carbon dioxide was the first gas to be described as a discrete substance. In about 1640,[8] the Flemish chemist Jan Baptist van Helmont observed that when he burned charcoal in a closed vessel, the mass of the resulting ash was much less than that of the original charcoal. His interpretation was that the rest of the charcoal had been transmuted into an invisible substance he termed a "gas" or "wild spirit" (spiritus sylvestre).[9]

The properties of carbon dioxide were studied more thoroughly in the 1750s by the Scottish physician Joseph Black. He found that limestone (calcium carbonate) could be heated or treated with acids to yield a gas he called "fixed air." He observed that the fixed air was denser than air and supported neither flame nor animal life. Black also found that when bubbled through limewater (a saturated aqueous solution of calcium hydroxide), it would precipitate calcium carbonate. He used this phenomenon to illustrate that carbon dioxide is produced by animal respiration and microbial fermentation. In 1772, English chemist Joseph Priestley published a paper entitled Impregnating Water with Fixed Air in which he described a process of dripping sulfuric acid (or oil of vitriol as Priestley knew it) on chalk in order to produce carbon dioxide, and forcing the gas to dissolve by agitating a bowl of water in contact with the gas.[10]

Carbon dioxide was first liquefied (at elevated pressures) in 1823 by Humphry Davy and Michael Faraday.[11] The earliest description of solid carbon dioxide was given by Adrien-Jean-Pierre Thilorier, who in 1835 opened a pressurized container of liquid carbon dioxide, only to find that the cooling produced by the rapid evaporation of the liquid yielded a "snow" of solid CO2.[12][13]

Chemical and physical properties

Structure and bonding

Stretching and bending oscillations of the CO2 carbon dioxide molecule. Upper left: symmetric stretching. Upper right: antisymmetric stretching. Lower line: degenerate pair of bending modes.

The carbon dioxide molecule is linear and centrosymmetric. The two C=O bonds are equivalent and are short (116.3 pm), consistent with double bonding.[14] Since it is centrosymmetric, the molecule has no electrical dipole. Consequently, only two vibrational bands are observed in the IR spectrum – an antisymmetric stretching mode at 2349 cm−1 and a degenerate pair of bending modes at 667 cm−1. There is also a symmetric stretching mode at 1388 cm−1 which is only observed in the Raman spectrum.[15]

In aqueous solution

See also: Carbonic acid

Carbon dioxide is soluble in water, in which it reversibly forms H
2
CO
3
(carbonic acid), which is a weak acid since its ionization in water is incomplete.

CO
2
+ H
2
O
H
2
CO
3

The hydration equilibrium constant of carbonic acid is (at 25 °C). Hence, the majority of the carbon dioxide is not converted into carbonic acid, but remains as CO2 molecules, not affecting the pH.

The relative concentrations of CO
2
, H
2
CO
3
, and the deprotonated forms HCO
3
(bicarbonate) and CO2−
3
(carbonate) depend on the pH. As shown in a Bjerrum plot, in neutral or slightly alkaline water (pH > 6.5), the bicarbonate form predominates (>50%) becoming the most prevalent (>95%) at the pH of seawater. In very alkaline water (pH > 10.4), the predominant (>50%) form is carbonate. The oceans, being mildly alkaline with typical pH = 8.2–8.5, contain about 120 mg of bicarbonate per liter.

Being diprotic, carbonic acid has two acid dissociation constants, the first one for the dissociation into the bicarbonate (also called hydrogen carbonate) ion (HCO3):

H2CO3 HCO3 + H+
Ka1 = 2.5×10−4 mol/L; pKa1 = 3.6 at 25 °C.[14]

This is the true first acid dissociation constant, defined as , where the denominator includes only covalently bound H2CO3 and does not include hydrated CO2(aq). The much smaller and often-quoted value near 4.16×10−7 is an apparent value calculated on the (incorrect) assumption that all dissolved CO2 is present as carbonic acid, so that . Since most of the dissolved CO2 remains as CO2 molecules, Ka1(apparent) has a much larger denominator and a much smaller value than the true Ka1.[16]

The bicarbonate ion is an amphoteric species that can act as an acid or as a base, depending on pH of the solution. At high pH, it dissociates significantly into the carbonate ion (CO32−):

HCO3 CO32− + H+
Ka2 = 4.69×10−11 mol/L; pKa2 = 10.329

In organisms carbonic acid production is catalysed by the enzyme, carbonic anhydrase.

Chemical reactions of CO2

CO2 is a weak electrophile. Its reaction with basic water illustrates this property, in which case hydroxide is the nucleophile. Other nucleophiles react as well. For example, carbanions as provided by Grignard reagents and organolithium compounds react with CO2 to give carboxylates:

MR + CO2 → RCO2M
where M = Li or MgBr and R = alkyl or aryl.

In metal carbon dioxide complexes, CO2 serves as a ligand, which can facilitate the conversion of CO2 to other chemicals.[17]

The reduction of CO2 to CO is ordinarily a difficult and slow reaction:

CO2 + 2 e + 2H+ → CO + H2O

The redox potential for this reaction near pH 7 is about −0.53 V versus the standard hydrogen electrode. The nickel-containing enzyme carbon monoxide dehydrogenase catalyses this process.[18]

Physical properties

For more details on this topic, see Carbon dioxide data.
Carbon dioxide pressure-temperature phase diagram showing the triple point and critical point of carbon dioxide
Sample of solid carbon dioxide or "dry ice" pellets

Carbon dioxide is colorless. At low concentrations, the gas is odorless. At higher concentrations it has a sharp, acidic odor. At standard temperature and pressure, the density of carbon dioxide is around 1.98 kg/m3, about 1.67 times that of air.

Carbon dioxide has no liquid state at pressures below 5.1 standard atmospheres (520 kPa). At 1 atmosphere (near mean sea level pressure), the gas deposits directly to a solid at temperatures below −78.5 °C (−109.3 °F; 194.7 K) and the solid sublimes directly to a gas above −78.5 °C. In its solid state, carbon dioxide is commonly called dry ice.

Liquid carbon dioxide forms only at pressures above 5.1 atm; the triple point of carbon dioxide is about 518 kPa at −56.6 °C (see phase diagram at left). The critical point is 7.38 MPa at 31.1 °C.[19][20] Another form of solid carbon dioxide observed at high pressure is an amorphous glass-like solid.[21] This form of glass, called carbonia, is produced by supercooling heated CO2 at extreme pressure (40–48 GPa or about 400,000 atmospheres) in a diamond anvil. This discovery confirmed the theory that carbon dioxide could exist in a glass state similar to other members of its elemental family, like silicon (silica glass) and germanium dioxide. Unlike silica and germania glasses, however, carbonia glass is not stable at normal pressures and reverts to gas when pressure is released.

At temperatures and pressures above the critical point, carbon dioxide behaves as a supercritical fluid known as supercritical carbon dioxide.

Isolation and production

Carbon dioxide can be obtained by distillation from air, but the method is inefficient. Industrially, carbon dioxide is predominantly an unrecovered waste product, produced by several methods which may be practiced at various scales.[22]

The combustion of all carbon-based fuels, such as methane (natural gas), petroleum distillates (gasoline, diesel, kerosene, propane), coal, wood and generic organic matter produces carbon dioxide and, except in the case of pure carbon, water. As an example, the chemical reaction between methane and oxygen is given below.

CH
4
+ 2 O
2
→ CO
2
+ 2 H
2
O

It is produced by thermal decomposition of limestone, CaCO
3
by heating (calcining) at about 850 °C (1,560 °F), in the manufacture of quicklime (calcium oxide, CaO), a compound that has many industrial uses:

CaCO
3
→ CaO + CO
2

Iron is reduced from its oxides with coke in a blast furnace, producing pig iron and carbon dioxide:[23]

Carbon dioxide is a byproduct of the industrial production of hydrogen by steam reforming and ammonia synthesis. These processes begin with the reaction of water and natural gas (mainly methane).[24]

Acids liberate CO
2
from most metal carbonates. Consequently, it may be obtained directly from natural carbon dioxide springs, where it is produced by the action of acidified water on limestone or dolomite. The reaction between hydrochloric acid and calcium carbonate (limestone or chalk) is shown below:

CaCO
3
+ 2 HCl → CaCl
2
+ H
2
CO
3

The carbonic acid (H
2
CO
3
) then decomposes to water and CO
2
:

H
2
CO
3
→ CO
2
+ H
2
O

Such reactions are accompanied by foaming or bubbling, or both, as the gas is released. They have widespread uses in industry because they can be used to neutralize waste acid streams.

Carbon dioxide is a by-product of the fermentation of sugar in the brewing of beer, whisky and other alcoholic beverages and in the production of bioethanol. Yeast metabolizes sugar to produce CO
2
and ethanol, also known as alcohol, as follows:

C
6
H
12
O
6
2 CO
2
+ 2 C
2
H
5
OH

All aerobic organisms produce CO
2
when they oxidize carbohydrates, fatty acids, and proteins. The large number of reactions involved are exceedingly complex and not described easily. Refer to (cellular respiration, anaerobic respiration and photosynthesis). The equation for the respiration of glucose and other monosaccharides is:

C
6
H
12
O
6
+ 6 O
2
6 CO
2
+ 6 H
2
O

Photoautotrophs (i.e. plants and cyanobacteria) use the energy contained in sunlight to photosynthesize simple sugars from CO
2
absorbed from the air and water:

n CO
2
+ n H
2
O
(CH
2
O)
n
+ n O
2

Carbon dioxide comprises about 40-45% of the gas that emanates from decomposition in landfills (termed "landfill gas"). Most of the remaining 50-55% is methane.[25]

Uses

Carbon dioxide bubbles in a soft drink.

Carbon dioxide is used by the food industry, the oil industry, and the chemical industry.[22] The compound has varied commercial uses but one of its greatest use as a chemical is in the production of carbonated beverages; it provides the sparkle in carbonated beverages such as soda water.

Precursor to chemicals

In the chemical industry, carbon dioxide is mainly consumed as an ingredient in the production of urea, with a smaller fraction being used to produce methanol and a range of other products.[26] Metal carbonates and bicarbonates, as well as some carboxylic acids derivatives (e.g., sodium salicylate) are prepared using CO2.

In addition to conventional processes using CO2 for chemical production, electrochemical methods are also being explored at a research level. In particular, the use of renewable energy for production of fuels from CO2 (such as methanol) is attractive as this could result in fuels that could be easily transported and used within conventional combustion technologies but have no net CO2 emissions.[27]

Foods

Carbon dioxide is a food additive used as a propellant and acidity regulator in the food industry. It is approved for usage in the EU[28] (listed as E number E290), US[29] and Australia and New Zealand[30] (listed by its INS number 290).

A candy called Pop Rocks is pressurized with carbon dioxide gas at about 4 x 106 Pa (40 bar, 580 psi). When placed in the mouth, it dissolves (just like other hard candy) and releases the gas bubbles with an audible pop.

Leavening agents cause dough to rise by producing carbon dioxide. Baker's yeast produces carbon dioxide by fermentation of sugars within the dough, while chemical leaveners such as baking powder and baking soda release carbon dioxide when heated or if exposed to acids.

Beverages

Carbon dioxide is used to produce carbonated soft drinks and soda water. Traditionally, the carbonation of beer and sparkling wine came about through natural fermentation, but many manufacturers carbonate these drinks with carbon dioxide recovered from the fermentation process. In the case of bottled and kegged beer, the most common method used is carbonation with recycled carbon dioxide. With the exception of British Real Ale, draught beer is usually transferred from kegs in a cold room or cellar to dispensing taps on the bar using pressurized carbon dioxide, sometimes mixed with nitrogen.

Wine making

Carbon dioxide in the form of dry ice is often used in the wine making process to cool down clusters of grapes quickly after picking to help prevent spontaneous fermentation by wild yeast. The main advantage of using dry ice over regular water ice is that it cools the grapes without adding any additional water that may decrease the sugar concentration in the grape must, and therefore also decrease the alcohol concentration in the finished wine.

Dry ice is also used during the cold soak phase of the wine making process to keep grapes cool. The carbon dioxide gas that results from the sublimation of the dry ice tends to settle to the bottom of tanks because it is denser than air. The settled carbon dioxide gas creates a hypoxic environment which helps to prevent bacteria from growing on the grapes until it is time to start the fermentation with the desired strain of yeast.

Carbon dioxide is also used to create a hypoxic environment for carbonic maceration, the process used to produce Beaujolais wine.

Carbon dioxide is sometimes used to top up wine bottles or other storage vessels such as barrels to prevent oxidation, though it has the problem that it can dissolve into the wine, making a previously still wine slightly fizzy. For this reason, other gases such as nitrogen or argon are preferred for this process by professional wine makers.

Inert gas

It is one of the most commonly used compressed gases for pneumatic (pressurized gas) systems in portable pressure tools. Carbon dioxide is also used as an atmosphere for welding, although in the welding arc, it reacts to oxidize most metals. Use in the automotive industry is common despite significant evidence that welds made in carbon dioxide are more brittle than those made in more inert atmospheres, and that such weld joints deteriorate over time because of the formation of carbonic acid. It is used as a welding gas primarily because it is much less expensive than more inert gases such as argon or helium. When used for MIG welding, CO2 use is sometimes referred to as MAG welding, for Metal Active Gas, as CO2 can react at these high temperatures. It tends to produce a hotter puddle than truly inert atmospheres, improving the flow characteristics. Although, this may be due to atmospheric reactions occurring at the puddle site. This is usually the opposite of the desired effect when welding, as it tends to embrittle the site, but may not be a problem for general mild steel welding, where ultimate ductility is not a major concern.

It is used in many consumer products that require pressurized gas because it is inexpensive and nonflammable, and because it undergoes a phase transition from gas to liquid at room temperature at an attainable pressure of approximately 60 bar (870 psi, 59 atm), allowing far more carbon dioxide to fit in a given container than otherwise would. Life jackets often contain canisters of pressured carbon dioxide for quick inflation. Aluminium capsules of CO2 are also sold as supplies of compressed gas for airguns, paintball markers, inflating bicycle tires, and for making carbonated water. Rapid vaporization of liquid carbon dioxide is used for blasting in coal mines. High concentrations of carbon dioxide can also be used to kill pests. Liquid carbon dioxide is used in supercritical drying of some food products and technological materials, in the preparation of specimens for scanning electron microscopy and in the decaffeination of coffee beans.

Fire extinguisher

Carbon dioxide can be used to extinguish flames by flooding the environment around the flame with the gas. It does not itself react to extinguish the flame, but starves the flame of oxygen by displacing it. Some fire extinguishers, especially those designed for electrical fires, contain liquid carbon dioxide under pressure. Carbon dioxide extinguishers work well on small flammable liquid and electrical fires, but not on ordinary combustible fires, because although it excludes oxygen, it does not cool the burning substances significantly and when the carbon dioxide disperses they are free to catch fire upon exposure to atmospheric oxygen. Their desirability in electrical fire stems from the fact that, unlike water or other chemical based methods, Carbon dioxide will not cause short circuits, leading to even more damage to equipment. Because it is a gas, it is also easy to dispense large amounts of the gas automatically in IT infrastructure rooms, where the fire itself might be hard to reach with more immediate methods because it is behind rack doors and inside of cases. Carbon dioxide has also been widely used as an extinguishing agent in fixed fire protection systems for local application of specific hazards and total flooding of a protected space.[31] International Maritime Organization standards also recognize carbon dioxide systems for fire protection of ship holds and engine rooms. Carbon dioxide based fire protection systems have been linked to several deaths, because it can cause suffocation in sufficiently high concentrations. A review of CO2 systems identified 51 incidents between 1975 and the date of the report, causing 72 deaths and 145 injuries.[32]

Supercritical CO2 as solvent

Liquid carbon dioxide is a good solvent for many lipophilic organic compounds and is used to remove caffeine from coffee. Carbon dioxide has attracted attention in the pharmaceutical and other chemical processing industries as a less toxic alternative to more traditional solvents such as organochlorides. It is used by some dry cleaners for this reason (see green chemistry). It is used in the preparation of some aerogels because of the properties of supercritical carbon dioxide.

Agricultural and biological applications

Plants require carbon dioxide to conduct photosynthesis. The atmospheres of greenhouses may (if of large size, must) be enriched with additional CO2 to sustain and increase the rate of plant growth.[33][34] At very high concentrations (100 times atmospheric concentration, or greater), carbon dioxide can be toxic to animal life, so raising the concentration to 10,000 ppm (1%) or higher for several hours will eliminate pests such as whiteflies and spider mites in a greenhouse.[35]

In medicine, up to 5% carbon dioxide (130 times atmospheric concentration) is added to oxygen for stimulation of breathing after apnea and to stabilize the O
2
/CO
2
balance in blood.

It has been proposed that carbon dioxide from power generation be bubbled into ponds to stimulate growth of algae that could then be converted into biodiesel fuel.[36]

Oil recovery

Carbon dioxide is used in enhanced oil recovery where it is injected into or adjacent to producing oil wells, usually under supercritical conditions, when it becomes miscible with the oil. This approach can increase original oil recovery by reducing residual oil saturation by between 7 per cent to 23 per cent additional to primary extraction.[37] It acts as both a pressurizing agent and, when dissolved into the underground crude oil, significantly reduces its viscosity, and changing surface chemistry enabling the oil to flow more rapidly through the reservoir to the removal well.[38] In mature oil fields, extensive pipe networks are used to carry the carbon dioxide to the injection points.

Bio transformation into fuel

Researchers have genetically modified a strain of the cyanobacterium Synechococcus elongatus to produce the fuels isobutyraldehyde and isobutanol from CO2 using photosynthesis.[39]

Refrigerant

Comparison of phase diagrams of carbon dioxide (red) and water (blue) as a log-lin chart with phase transitions points at 1 atmosphere

Liquid and solid carbon dioxide are important refrigerants, especially in the food industry, where they are employed during the transportation and storage of ice cream and other frozen foods. Solid carbon dioxide is called "dry ice" and is used for small shipments where refrigeration equipment is not practical. Solid carbon dioxide is always below −78.5 °C at regular atmospheric pressure, regardless of the air temperature.

Liquid carbon dioxide (industry nomenclature R744 or R-744) was used as a refrigerant prior to the discovery of R-12 and may enjoy a renaissance due to the fact that R134a contributes to climate change. Its physical properties are highly favorable for cooling, refrigeration, and heating purposes, having a high volumetric cooling capacity. Due to the need to operate at pressures of up to 130 bar (1880 psi), CO2 systems require highly resistant components that have already been developed for mass production in many sectors. In automobile air conditioning, in more than 90% of all driving conditions for latitudes higher than 50°, R744 operates more efficiently than systems using R134a. Its environmental advantages (GWP of 1, non-ozone depleting, non-toxic, non-flammable) could make it the future working fluid to replace current HFCs in cars, supermarkets, and heat pump water heaters, among others. Coca-Cola has fielded CO2-based beverage coolers and the U.S. Army is interested in CO2 refrigeration and heating technology.[40][41]

The global automobile industry is expected to decide on the next-generation refrigerant in car air conditioning. CO2 is one discussed option.(see Sustainable automotive air conditioning)

Coal bed methane recovery

In enhanced coal bed methane recovery, carbon dioxide would be pumped into the coal seam to displace methane, as opposed to current methods which primarily rely on the removal of water (to reduce pressure) to make the coal seam release its trapped methane.[42]

Niche uses

Carbon dioxide is the lasing medium in a carbon dioxide laser, which is one of the earliest type of lasers.

Carbon dioxide can be used as a means of controlling the pH of swimming pools, by continuously adding gas to the water, thus keeping the pH from rising. Among the advantages of this is the avoidance of handling (more hazardous) acids. Similarly, it is also used in the maintaining reef aquaria, where it is commonly used in calcium reactors to temporarily lower the pH of water being passed over calcium carbonate in order to allow the calcium carbonate to dissolve into the water more freely where it is used by some corals to build their skeleton.

Used as the primary coolant in the British advanced gas-cooled reactor for nuclear power generation.

Carbon dioxide induction is commonly used for the euthanasia of laboratory research animals. Methods to administer CO2 include placing animals directly into a closed, prefilled chamber containing CO2, or exposure to a gradually increasing concentration of CO2. In 2013, the American Veterinary Medical Association issued new guidelines for carbon dioxide induction, stating that a displacement rate of 10% to 30% of the gas chamber volume per minute is optimal for the humane euthanization of small rodents.[43]

Carbon dioxide is also used in several related cleaning and surface preparation techniques.

In Earth's atmosphere

The Keeling Curve of atmospheric CO2 concentrations measured at Mauna Loa Observatory

Carbon dioxide in Earth's atmosphere is a trace gas, currently (early 2016) having an average concentration of 402 parts per million by volume[3][44][45] (or 611 parts per million by mass). Atmospheric concentrations of carbon dioxide fluctuate slightly with the seasons, falling during the Northern Hemisphere spring and summer as plants consume the gas and rising during northern autumn and winter as plants go dormant or die and decay. Concentrations also vary on a regional basis, most strongly near the ground with much smaller variations aloft. In urban areas concentrations are generally higher[46] and indoors they can reach 10 times background levels.

Yearly increase of atmospheric CO2: In the 1960s, the average annual increase was 37% of the 2000–2007 average.[47]

The concentration levels of carbon dioxide have risen due to human activities since WWII. [48]Combustion of fossil fuels and deforestation have caused the atmospheric concentration of carbon dioxide to increase by about 43% since the beginning of the age of industrialization.[49] Most carbon dioxide from human activities is released from burning coal and other fossil fuels. Other human activities, including deforestation, biomass burning, and cement production also produce carbon dioxide. Volcanoes emit between 0.2 and 0.3 billion tons of carbon dioxide per year, while human activities emit about 29 billion tons.[50]

Carbon dioxide is a greenhouse gas, absorbing and emitting infrared radiation at its two infrared-active vibrational frequencies (see Structure and bonding above). This process causes carbon dioxide to warm the surface and lower atmosphere, while cooling the upper atmosphere. The increase in atmospheric concentration of CO2, and thus in the CO2-induced greenhouse effect, is the reason for the rise in average global temperature since the mid-20th century. Although carbon dioxide is the greenhouse gas primarily responsible for the rise, methane, nitrous oxide, ozone, and various other long-lived greenhouse gases also contribute. Carbon dioxide is of greatest concern because it exerts a larger overall warming influence than all of those other gases combined, and because it has a long atmospheric lifetime.

CO2 in Earth's atmosphere if half of global-warming emissions are not absorbed.[51][52][53][54]
(NASA computer simulation).

Not only do increasing carbon dioxide concentrations lead to increases in global surface temperature, but increasing global temperatures also cause increasing concentrations of carbon dioxide. This produces a positive feedback for changes induced by other processes such as orbital cycles.[55] Five hundred million years ago the carbon dioxide concentration was 20 times greater than today, decreasing to 4–5 times during the Jurassic period and then slowly declining with a particularly swift reduction occurring 49 million years ago.[56][57]

Local concentrations of carbon dioxide can reach high values near strong sources, especially those that are isolated by surrounding terrain. At the Bossoleto hot spring near Rapolano Terme in Tuscany, Italy, situated in a bowl-shaped depression about 100 m (330 ft) in diameter, concentrations of CO2 rise to above 75% overnight, sufficient to kill insects and small animals. After sunrise the gas is dispersed by convection during the day.[58] High concentrations of CO2 produced by disturbance of deep lake water saturated with CO2 are thought to have caused 37 fatalities at Lake Monoun, Cameroon in 1984 and 1700 casualties at Lake Nyos, Cameroon in 1986.[59]

Human-made carbon dioxide (CO2) continues to increase above levels not seen in hundreds of thousands of years. Currently, about half of the carbon dioxide released from the burning of fossil fuels remains in the atmosphere and is not absorbed by vegetation and the oceans.[51][52][53][54]

In the oceans

Main article: Carbon cycle

Carbon dioxide dissolves in the ocean to form carbonic acid (H2CO3), bicarbonate (HCO3) and carbonate (CO32−). There is about fifty times as much carbon dissolved in the oceans as exists in the atmosphere. The oceans act as an enormous carbon sink, and have taken up about a third of CO2 emitted by human activity.[60]

As the concentration of carbon dioxide increases in the atmosphere, the increased uptake of carbon dioxide into the oceans is causing a measurable decrease in the pH of the oceans, which is referred to as ocean acidification. This reduction in pH affects biological systems in the oceans, primarily oceanic calcifying organisms. These effects span the food chain from autotrophs to heterotrophs and include organisms such as coccolithophores, corals, foraminifera, echinoderms, crustaceans and mollusks. Under normal conditions, calcium carbonate is stable in surface waters since the carbonate ion is at supersaturating concentrations. However, as ocean pH falls, so does the concentration of this ion, and when carbonate becomes undersaturated, structures made of calcium carbonate are vulnerable to dissolution.[61] Corals,[62][63][64] coccolithophore algae,[65][66][67][68] coralline algae,[69] foraminifera,[70] shellfish[71] and pteropods[72] experience reduced calcification or enhanced dissolution when exposed to elevated CO
2
.

Gas solubility decreases as the temperature of water increases (except when both pressure exceeds 300 bar and temperature exceeds 393 K, only found near deep geothermal vents)[73] and therefore the rate of uptake from the atmosphere decreases as ocean temperatures rise.

Most of the CO2 taken up by the ocean, which is about 30% of the total released into the atmosphere,[74] forms carbonic acid in equilibrium with bicarbonate. Some of these chemical species are consumed by photosynthetic organisms that remove carbon from the cycle. Increased CO2 in the atmosphere has led to decreasing alkalinity of seawater, and there is concern that this may adversely affect organisms living in the water. In particular, with decreasing alkalinity, the availability of carbonates for forming shells decreases,[75] although there's evidence of increased shell production by certain species under increased CO2 content.[76]

NOAA states in their May 2008 "State of the science fact sheet for ocean acidification" that:
"The oceans have absorbed about 50% of the carbon dioxide (CO2) released from the burning of fossil fuels, resulting in chemical reactions that lower ocean pH. This has caused an increase in hydrogen ion (acidity) of about 30% since the start of the industrial age through a process known as "ocean acidification." A growing number of studies have demonstrated adverse impacts on marine organisms, including:

Also, the Intergovernmental Panel on Climate Change (IPCC) writes in their Climate Change 2007: Synthesis Report:[77]
"The uptake of anthropogenic carbon since 1750 has led to the ocean becoming more acidic with an average decrease in pH of 0.1 units. Increasing atmospheric CO2 concentrations lead to further acidification ... While the effects of observed ocean acidification on the marine biosphere are as yet undocumented, the progressive acidification of oceans is expected to have negative impacts on marine shell-forming organisms (e.g. corals) and their dependent species."

Some marine calcifying organisms (including coral reefs) have been singled out by major research agencies, including NOAA, OSPAR commission, NANOOS and the IPCC, because their most current research shows that ocean acidification should be expected to impact them negatively.[78]

Carbon dioxide is also introduced into the oceans through hydrothermal vents. The Champagne hydrothermal vent, found at the Northwest Eifuku volcano at Marianas Trench Marine National Monument, produces almost pure liquid carbon dioxide, one of only two known sites in the world.[79]

Biological role

Carbon dioxide is an end product of cellular respiration in organisms that obtain energy by breaking down sugars, fats and amino acids with oxygen as part of their metabolism. This includes all plants, algae and animals and aerobic fungi and bacteria. In vertebrates, the carbon dioxide travels in the blood from the body's tissues to the skin (e.g., amphibians) or the gills (e.g., fish), from where it dissolves in the water, or to the lungs from where it is exhaled. During active photosynthesis, plants can absorb more carbon dioxide from the atmosphere than they release in respiration.

Photosynthesis and carbon fixation

Overview of photosynthesis and respiration. Carbon dioxide (at right), together with water, form oxygen and organic compounds (at left) by photosynthesis, which can be respired to water and (CO2).
Figure 2. Overview of the Calvin cycle and carbon fixation

Carbon fixation is a biochemical process by which atmospheric carbon dioxide is incorporated by plants, algae and (cyanobacteria) into energy-rich organic molecules such as glucose, thus creating their own food by photosynthesis. Photosynthesis uses carbon dioxide and water to produce sugars from which other organic compounds can be constructed, and oxygen is produced as a by-product.

Ribulose-1,5-bisphosphate carboxylase oxygenase, commonly abbreviated to RuBisCO, is the enzyme involved in the first major step of carbon fixation, the production of two molecules of 3-phosphoglycerate from CO2 and ribulose bisphosphate, as shown in the diagram at left.

RuBisCO is thought to be the single most abundant protein on Earth.[80]

Phototrophs use the products of their photosynthesis as internal food sources and as raw material for the biosynthesis of more complex organic molecules, such as polysaccharides, nucleic acids and proteins. These are used for their own growth, and also as the basis of the food chains and webs that feed other organisms, including animals such as ourselves. Some important phototrophs, the coccolithophores synthesise hard calcium carbonate scales. A globally significant species of coccolithophore is Emiliania huxleyi whose calcite scales have formed the basis of many sedimentary rocks such as limestone, where what was previously atmospheric carbon can remain fixed for geological timescales.

Plants can grow as much as 50 percent faster in concentrations of 1,000 ppm CO2 when compared with ambient conditions, though this assumes no change in climate and no limitation on other nutrients.[81] Elevated CO2 levels cause increased growth reflected in the harvestable yield of crops, with wheat, rice and soybean all showing increases in yield of 12–14% under elevated CO2 in FACE experiments.[82][83]

Increased atmospheric CO2 concentrations result in fewer stomata developing on plants[84] which leads to reduced water usage and increased water-use efficiency.[85] Studies using FACE have shown that CO2 enrichment leads to decreased concentrations of micronutrients in crop plants.[86] This may have knock-on effects on other parts of ecosystems as herbivores will need to eat more food to gain the same amount of protein.[87]

The concentration of secondary metabolites such as phenylpropanoids and flavonoids can also be altered in plants exposed to high concentrations of CO2.[88][89]

Plants also emit CO2 during respiration, and so the majority of plants and algae, which use C3 photosynthesis, are only net absorbers during the day. Though a growing forest will absorb many tons of CO2 each year, a mature forest will produce as much CO2 from respiration and decomposition of dead specimens (e.g., fallen branches) as is used in photosynthesis in growing plants.[90] Contrary to the long-standing view that they are carbon neutral, mature forests can continue to accumulate carbon[91] and remain valuable carbon sinks, helping to maintain the carbon balance of Earth's atmosphere. Additionally, and crucially to life on earth, photosynthesis by phytoplankton consumes dissolved CO2 in the upper ocean and thereby promotes the absorption of CO2 from the atmosphere.[92]

Toxicity

Main symptoms of carbon dioxide toxicity, by increasing volume percent in air.[93]

Carbon dioxide content in fresh air (averaged between sea-level and 10 kPa level, i.e., about 30 km (19 mi) altitude) varies between 0.036% (360 ppm) and 0.041% (410 ppm), depending on the location.[94]

CO2 is an asphyxiant gas and not classified as toxic or harmful in accordance with Globally Harmonized System of Classification and Labelling of Chemicals standards of United Nations Economic Commission for Europe by using the OECD Guidelines for the Testing of Chemicals. In concentrations up to 1% (10,000 ppm), it will make some people feel drowsy and give the lungs a stuffy feeling.[93] Concentrations of 7% to 10% (70,000 to 100,000 ppm) may cause suffocation, even in the presence of sufficient oxygen, manifesting as dizziness, headache, visual and hearing dysfunction, and unconsciousness within a few minutes to an hour.[95] The physiological effects of acute carbon dioxide exposure are grouped together under the term hypercapnia, a subset of asphyxiation.

Because it is heavier than air, in locations where the gas seeps from the ground (due to sub-surface volcanic or geothermal activity) in relatively high concentrations, without the dispersing effects of wind, it can collect in sheltered/pocketed locations below average ground level, causing animals located therein to be suffocated. Carrion feeders attracted to the carcasses are then also killed. Children have been killed in the same way near the city of Goma by CO2 emissions from the nearby volcano Mt. Nyiragongo.[96] The Swahili term for this phenomenon is 'mazuku'.

Adaptation to increased concentrations of CO2 occurs in humans, including modified breathing and kidney bicarbonate production, in order to balance the effects of blood acidification (acidosis). Several studies suggested that 2.0 percent inspired concentrations could be used for closed air spaces (e.g. a submarine) since the adaptation is physiological and reversible, as decrement in performance or in normal physical activity does not happen at this level of exposure for five days.[97][98] Yet, other studies show a decrease in cognitive function even at much lower levels.[99][100] Also, with ongoing respiratory acidosis, adaptation or compensatory mechanisms will be unable to reverse such condition.

Below 1%

There are few studies of the health effects of long-term continuous CO2 exposure on humans and animals at levels below 1% and there is potentially a significant risk to humans in the near future with rising atmospheric CO2 levels associated with climate change.[101] Occupational CO2 exposure limits have been set in the United States at 0.5% (5000 ppm) for an eight-hour period.[102] At this CO2 concentration, International Space Station crew experienced headaches, lethargy, mental slowness, emotional irritation, and sleep disruption.[103] Studies in animals at 0.5% CO2 have demonstrated kidney calcification and bone loss after eight weeks of exposure.[104] A study of humans exposed in 2.5 hour sessions demonstrated significant effects on cognitive abilities at concentrations as low as 0.1% (1000ppm) CO2 likely due to CO2 induced increases in cerebral blood flow.[99] Another study observed a decline in basic activity level and information usage at 1000 ppm, when compared to 500 ppm.[100]

Ventilation

Poor ventilation is one of the main causes of excessive CO2 concentrations in closed spaces. Carbon dioxide differential above outdoor concentrations at steady state conditions (when the occupancy and ventilation system operation are sufficiently long that CO2 concentration has stabilized) are sometimes used to estimate ventilation rates per person. Higher CO2 concentrations are associated with occupant health, comfort and performance degradation. ASHRAE Standard 62.1–2007 ventilation rates may result in indoor levels up to 2,100 ppm above ambient outdoor conditions. Thus if the outdoor concentration is 400 ppm, indoor concentrations may reach 2,500 ppm with ventilation rates that meet this industry consensus standard. Concentrations in poorly ventilated spaces can be found even higher than this (range of 3,000 or 4,000).

Miners, who are particularly vulnerable to gas exposure due to an insufficient ventilation, referred to mixtures of carbon dioxide and nitrogen as "blackdamp," "choke damp" or "stythe." Before more effective technologies were developed, miners would frequently monitor for dangerous levels of blackdamp and other gases in mine shafts by bringing a caged canary with them as they worked. The canary is more sensitive to asphyxiant gases than humans, and as it became unconscious would stop singing and fall off its perch. The Davy lamp could also detect high levels of blackdamp (which sinks, and collects near the floor) by burning less brightly, while methane, another suffocating gas and explosion risk, would make the lamp burn more brightly.

Human physiology

Content

The body produces approximately 2.3 pounds (1.0 kg) of carbon dioxide per day per person,[105] containing 0.63 pounds (290 g) of carbon. In humans, this carbon dioxide is carried through the venous system and is breathed out through the lungs, resulting in lower concentrations in the arteries. The carbon dioxide content of the blood is often given as the partial pressure, which is the pressure which carbon dioxide would have had if it alone occupied the volume.[106]

In humans, the carbon dioxide contents are as follows:

Reference ranges or averages for partial pressures of carbon dioxide (abbreviated PCO2)
Unit Venous blood gas Alveolar pulmonary
gas pressures
Arterial blood carbon dioxide
kPa 5.5[107]-6.8[107] 4.8 4.7[107]-6.0[107]
mmHg 41–51 36 35[108]-45[108]

Transport in the blood

CO2 is carried in blood in three different ways. (The exact percentages vary depending whether it is arterial or venous blood).

Hemoglobin, the main oxygen-carrying molecule in red blood cells, carries both oxygen and carbon dioxide. However, the CO2 bound to hemoglobin does not bind to the same site as oxygen. Instead, it combines with the N-terminal groups on the four globin chains. However, because of allosteric effects on the hemoglobin molecule, the binding of CO2 decreases the amount of oxygen that is bound for a given partial pressure of oxygen. The decreased binding to carbon dioxide in the blood due to increased oxygen levels is known as the Haldane Effect, and is important in the transport of carbon dioxide from the tissues to the lungs. Conversely, a rise in the partial pressure of CO2 or a lower pH will cause offloading of oxygen from hemoglobin, which is known as the Bohr Effect.

Regulation of respiration

Carbon dioxide is one of the mediators of local autoregulation of blood supply. If its concentration is high, the capillaries expand to allow a greater blood flow to that tissue.

Bicarbonate ions are crucial for regulating blood pH. A person's breathing rate influences the level of CO2 in their blood. Breathing that is too slow or shallow causes respiratory acidosis, while breathing that is too rapid leads to hyperventilation, which can cause respiratory alkalosis.

Although the body requires oxygen for metabolism, low oxygen levels normally do not stimulate breathing. Rather, breathing is stimulated by higher carbon dioxide levels. As a result, breathing low-pressure air or a gas mixture with no oxygen at all (such as pure nitrogen) can lead to loss of consciousness without ever experiencing air hunger. This is especially perilous for high-altitude fighter pilots. It is also why flight attendants instruct passengers, in case of loss of cabin pressure, to apply the oxygen mask to themselves first before helping others; otherwise, one risks losing consciousness.[109]

The respiratory centers try to maintain an arterial CO2 pressure of 40 mm Hg. With intentional hyperventilation, the CO2 content of arterial blood may be lowered to 10–20 mm Hg (the oxygen content of the blood is little affected), and the respiratory drive is diminished. This is why one can hold one's breath longer after hyperventilating than without hyperventilating. This carries the risk that unconsciousness may result before the need to breathe becomes overwhelming, which is why hyperventilation is particularly dangerous before free diving.

See also

References

  1. "Carbon dioxide". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
  2. 1 2 3 "NIOSH Pocket Guide to Chemical Hazards #0103". National Institute for Occupational Safety and Health (NIOSH).
  3. 1 2 National Oceanic & Atmospheric Administration (NOAA) – Earth System Research Laboratory (ESRL), Trends in Carbon Dioxide Values given are dry air mole fractions expressed in parts per million (ppm). For an ideal gas mixture this is equivalent to parts per million by volume (ppmv).
  4. "General Properties and Uses of Carbon Dioxide, Good Plant Design and Operation for Onshore Carbon Capture Installations and Onshore Pipelines". Energy Institute. Retrieved 2012-03-14.
  5. Donald G. Kaufman; Cecilia M. Franz (1996). Biosphere 2000: protecting our global environment. Kendall/Hunt Pub. Co. ISBN 978-0-7872-0460-0. Retrieved 11 October 2011.
  6. Food Factories. www.legacyproject.org. Retrieved 2011-10-10.
  7. Ocean Acidification: A National Strategy to Meet the Challenges of a Changing Ocean. Washington, DC: National Academies Press. doi:10.17226/12904. ISBN 978-0-309-15359-1.
  8. DavidFraser Harris (September 1910). "THE PIONEER IN THE HYGIENE OF VENTILATION". The Lancet. 176 (4542): 906–908. doi:10.1016/S0140-6736(00)52420-9.
  9. Almqvist, Ebbe (2003). History of industrial gases. Springer. ISBN 9780306472770. p. 93
  10. Priestley, Joseph; Hey, Wm (1772). "Observations on Different Kinds of Air". Philosophical Transactions. 62: 147–264. doi:10.1098/rstl.1772.0021.
  11. Davy, Humphry (1823). "On the Application of Liquids Formed by the Condensation of Gases as Mechanical Agents". Philosophical Transactions. 113: 199–205. doi:10.1098/rstl.1823.0020. JSTOR 107649.
  12. Thilorier, Adrien-Jean-Pierre (1835) "Solidification de l’acide carbonique" (Solidification of carbonic acid), Comptes rendus ..., 1 : 194–196
  13. "Solidification of carbonic acid", The London and Edinburgh Philosophical Magazine, 8 : 446–447 (1836).
  14. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  15. Atkins P. and de Paula J. Physical Chemistry (8th ed., W.H. Freeman 2006) p.461 and p.464 ISBN 0-7167-8759-8
  16. Jolly, William L., Modern Inorganic Chemistry (McGraw-Hill 1984), p. 196
  17. M. Aresta (Ed.) "Carbon Dioxide as a Chemical Feedstock" 2010, Wiley-VCH: Weinheim. ISBN 978-3-527-32475-0
  18. Finn, Colin; Schnittger, Sorcha; Yellowlees, Lesley J.; Love, Jason B. (2012). "Molecular approaches to the electrochemical reduction of carbon dioxide". Chemical Communications. 2011 (10): 1392–9. doi:10.1039/c1cc15393e. PMID 22116300.
  19. "Phase change data for Carbon dioxide". National Institute of Standards and Technology. Retrieved 2008-01-21.
  20. Kudryavtseva I.V., Kamotskii V.I., Rykov S.V., Rykov V.A., "CALCULATION CARBON DIOXIDE LINE OF PHASE EQUILIBRIUM", Processes and equipment for food production, Number 4(18), 2013
  21. Santoro, M.; Gorelli, FA; Bini, R; Ruocco, G; Scandolo, S; Crichton, WA (2006). "Amorphous silica-like carbon dioxide". Nature. 441 (7095): 857–860. Bibcode:2006Natur.441..857S. doi:10.1038/nature04879. PMID 16778885.
  22. 1 2 Pierantozzi, Ronald (2001). "Carbon Dioxide". Kirk-Othmer Encyclopedia of Chemical Technology. Kirk-Othmer Encyclopedia of Chemical Technology. Wiley. doi:10.1002/0471238961.0301180216090518.a01.pub2. ISBN 0-471-23896-1.
  23. Strassburger, Julius (1969). Blast Furnace Theory and Practice. New York: American Institute of Mining, Metallurgical, and Petroleum Engineers. ISBN 0-677-10420-0.
  24. Susan Topham "Carbon Dioxide" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a05_165
  25. US EPA, "Facts About Landfill Gas"
  26. "IPCC Special Report on Carbon dioxide Capture and Storage"
  27. Badwal, Sukhvinder P. S.; Giddey, Sarbjit S.; Munnings, Christopher; Bhatt, Anand I.; Hollenkamp, Anthony F. (24 September 2014). "Emerging electrochemical energy conversion and storage technologies (open access)". Frontiers in Chemistry. 2: 79. Bibcode:2014FrCh....2...79B. doi:10.3389/fchem.2014.00079. PMC 4174133Freely accessible. PMID 25309898.
  28. UK Food Standards Agency: "Current EU approved additives and their E Numbers". Retrieved 2011-10-27.
  29. US Food and Drug Administration: "Food Additive Status List". Retrieved 13 June 2015.
  30. Australia New Zealand Food Standards Code"Standard 1.2.4 – Labelling of ingredients". Retrieved 2011-10-27.
  31. National Fire Protection Association Code 12
  32. Carbon Dioxide as a Fire Suppressant: Examining the Risks, US EPA
  33. Plant Growth Factors: Photosynthesis, Respiration, and Transpiration. Ext.colostate.edu. Retrieved 2011-10-10.
  34. Carbon dioxide. Formal.stanford.edu. Retrieved 2011-10-10.
  35. Stafford, Ned (7 February 2007). "Future crops: The other greenhouse effect". Nature. 448 (7153): 526–8. Bibcode:2007Natur.448..526S. doi:10.1038/448526a. PMID 17671477.
  36. Clayton, Mark (2006-01-11). "Algae – like a breath mint for smokestacks". The Christian Science Monitor. Retrieved 2007-10-11.
  37. "CO2 for use in enhanced oil recovery (EOR)". Global CCS Institute. Retrieved 2012-02-25.
  38. Austell, J Michael (2005). "CO2 for Enhanced Oil Recovery Needs – Enhanced Fiscal Incentives". Exploration & Production: the Oil & Gas Review. Archived from the original on 2012-02-07. Retrieved 2007-09-28.
  39. Atsum, Shota; Higashide, Wendy; Liauo, James C. (November 2009). "Direct photosynthetic recycling of carbon dioxide to isobutyraldehyde". Nature Biotechnology. 27 (12): 1177–1180. doi:10.1038/nbt.1586. PMID 19915552.
  40. "The Coca-Cola Company Announces Adoption of HFC-Free Insulation in Refrigeration Units to Combat Global Warming". The Coca-Cola Company. 2006-06-05. Retrieved 2007-10-11.
  41. "Modine reinforces its CO2 research efforts". R744.com. 2007-06-28.
  42. "Enhanced coal bed methane recovery". ETH Zurich. 31 August 2006. Archived from the original on 6 July 2011.
  43. "2013 AVMA Guidelines for the Euthanasia of Animals" (PDF). Retrieved 2014-01-14.
  44. Pashley, Alex (10 March 2016). "CO2 levels make largest recorded annual leap, Noaa data shows". The Guardian. Retrieved 14 March 2016.
  45. "Record annual increase of carbon dioxide observed at Mauna Loa for 2015". NOAA. 9 March 2016. Retrieved 14 March 2016.
  46. George, K.; Ziska, L. H.; Bunce, J. A.; Quebedeaux, B. (2007). "Elevated atmospheric CO2 concentration and temperature across an urban–rural transect". Atmospheric Environment. 41 (35): 7654–7665. Bibcode:2007AtmEn..41.7654G. doi:10.1016/j.atmosenv.2007.08.018.
  47. Tans, Pieter (3 May 2008) "Annual CO2 mole fraction increase (ppm)" for 1959–2007. National Oceanic and Atmospheric Administration Earth System Research Laboratory, Global Monitoring Division (additional details.)
  48. Li, Anthony HF. "Hopes of Limiting Global Warming? China and the Paris Agreement on Climate Change." China Perspectives 1 (2016): 49.
  49. "After two large annual gains, rate of atmospheric CO2 increase returns to average". NOAA News Online, Story 2412. 2005-03-31.
  50. "Global Warming Frequently Asked Questions - NOAA Climate.gov".
  51. 1 2 Buis, Alan; Ramsayer, Kate; Rasmussen, Carol (12 November 2015). "A Breathing Planet, Off Balance". NASA. Retrieved 13 November 2015.
  52. 1 2 Staff (12 November 2015). "Audio (66:01) - NASA News Conference - Carbon & Climate Telecon". NASA. Retrieved 12 November 2015.
  53. 1 2 St. Fleur, Nicholas (10 November 2015). "Atmospheric Greenhouse Gas Levels Hit Record, Report Says". New York Times. Retrieved 11 November 2015.
  54. 1 2 Ritter, Karl (9 November 2015). "UK: In 1st, global temps average could be 1 degree C higher". AP News. Retrieved 11 November 2015.
  55. Genthon, G.; Barnola, J. M.; Raynaud, D.; Lorius, C.; Jouzel, J.; Barkov, N. I.; Korotkevich, Y. S.; Kotlyakov, V. M. (1987). "Vostok ice core: climatic response to CO2 and orbital forcing changes over the last climatic cycle". Nature. 329 (6138): 414–418. Bibcode:1987Natur.329..414G. doi:10.1038/329414a0.
  56. "Climate and CO2 in the Atmosphere". Retrieved 2007-10-10.
  57. Berner, Robert A.; Kothavala, Zavareth (2001). "GEOCARB III: A revised model of atmospheric CO2 over Phanerozoic Time" (PDF). American Journal of Science. 301 (2): 182–204. doi:10.2475/ajs.301.2.182. Retrieved 2008-02-15.
  58. van Gardingen, P.R.; Grace, J.; Jeffree, C.E.; Byari, S.H.; Miglietta, F.; Raschi, A.; Bettarini, I. (1997). "Long-term effects of enhanced CO2 concentrations on leaf gas exchange: research opportunities using CO2 springs". In Raschi, A.; Miglietta, F.; Tognetti, R.; van Gardingen, P.R. Plant responses to elevated CO2: Evidence from natural springs. Cambridge: Cambridge University Press. pp. 69–86. ISBN 0-521-58203-2.
  59. Martini, M. (1997). "CO2 emissions in volcanic areas: case histories and hazards". In Raschi, A.; Miglietta, F.; Tognetti, R.; van Gardingen, P.R. Plant responses to elevated CO2: Evidence from natural springs. Cambridge: Cambridge University Press. pp. 69–86. ISBN 0-521-58203-2.
  60. Doney, Scott C.; Naomi M. Levine (2006-11-29). "How Long Can the Ocean Slow Global Warming?". Oceanus. Retrieved 2007-11-21.
  61. Nienhuis, S.; Palmer, A.; Harley, C. (2010). "Elevated CO2 affects shell dissolution rate but not calcification rate in a marine snail". Proceedings of the Royal Society B: Biological Sciences. 277 (1693): 2553–2558. doi:10.1098/rspb.2010.0206. PMC 2894921Freely accessible. PMID 20392726.
  62. Gattuso, J.-P.; Frankignoulle, M.; Bourge, I.; Romaine, S. & Buddemeier, R. W. (1998). "Effect of calcium carbonate saturation of seawater on coral calcification". Global and Planetary Change. 18 (1–2): 37–46. Bibcode:1998GPC....18...37G. doi:10.1016/S0921-8181(98)00035-6.
  63. Gattuso, J.-P.; Allemand, D.; Frankignoulle, M (1999). "Photosynthesis and calcification at cellular, organismal and community levels in coral reefs: a review on interactions and control by carbonate chemistry". American Zoologist. 39: 160–183. doi:10.1093/icb/39.1.160.
  64. Langdon, C; Atkinson, M. J. (2005). "Effect of elevated pCO2 on photosynthesis and calcification of corals and interactions with seasonal change in temperature/irradiance and nutrient enrichment". Journal of Geophysical Research. 110 (C09S07): C09S07. Bibcode:2005JGRC..11009S07L. doi:10.1029/2004JC002576.
  65. Riebesell, Ulf; Zondervan, Ingrid; Rost, Björn; Tortell, Philippe D.; Zeebe, Richard E. & François M. M. Morel (2000). "Reduced calcification of marine plankton in response to increased atmospheric CO
    2
    ". Nature. 407 (6802): 364–367. doi:10.1038/35030078. PMID 11014189.
  66. Zondervan, I.; Zeebe, R.E.; Rost, B.; Rieblesell, U. (2001). "Decreasing marine biogenic calcification: a negative feedback on rising atmospheric CO2". Global Biogeochemical Cycles. 15 (2): 507–516. Bibcode:2001GBioC..15..507Z. doi:10.1029/2000GB001321.
  67. Zondervan, I.; Rost, B.; Rieblesell, U. (2002). "Effect of CO2 concentration on the PIC/POC ratio in the coccolithophore Emiliania huxleyi grown under light limiting conditions and different day lengths". Journal of Experimental Marine Biology and Ecology. 272 (1): 55–70. doi:10.1016/S0022-0981(02)00037-0.
  68. Delille, B.; Harlay, J.; Zondervan, I.; Jacquet, S.; Chou, L.; Wollast, R.; Bellerby, R.G.J.; Frankignoulle, M.; Borges, A.V.; Riebesell, U.; Gattuso, J.-P. (2005). "Response of primary production and calcification to changes of pCO2 during experimental blooms of the coccolithophorid Emiliania huxleyi". Global Biogeochemical Cycles. 19 (2): GB2023. Bibcode:2005GBioC..19.2023D. doi:10.1029/2004GB002318.
  69. Kuffner, I.B.; Andersson, A.J.; Jokiel, P.L.; Rodgers, K.S.; Mackenzie, F.T. (2007). "Decreased abundance of crustose coralline algae due to ocean acidification". Nature Geoscience. 1 (2): 114–117. Bibcode:2008NatGe...1..114K. doi:10.1038/ngeo100.
  70. Phillips, Graham; Chris Branagan (2007-09-13). "Ocean Acidification – The BIG global warming story". ABC TV Science: Catalyst. Australian Broadcasting Corporation. Retrieved 2007-09-18.
  71. Gazeau, F.; Quiblier, C.; Jansen, J. M.; Gattuso, J.-P.; Middelburg, J. J. & Heip, C. H. R. (2007). "Impact of elevated CO
    2
    on shellfish calcification"
    . Geophysical Research Letters. 34 (7): L07603. Bibcode:2007GeoRL..3407603G. doi:10.1029/2006GL028554.
  72. Comeau, C.; Gorsky, G.; Jeffree, R.; Teyssié, J.-L.; Gattuso, J.-P. (2009). "Impact of ocean acidification on a key Arctic pelagic mollusc ("Limacina helicina")". Biogeosciences. 6 (9): 1877–1882. doi:10.5194/bg-6-1877-2009.
  73. Duana, Zhenhao; Rui Sun (2003). "An improved model calculating CO2 solubility in pure water and aqueous NaCl solutions from 273 to 533 K and from 0 to 2000 bar". Chemical Geology. 193 (3–4): 257–271. doi:10.1016/S0009-2541(02)00263-2.
  74. Cai, W. -J.; Chen, L.; Chen, B.; Gao, Z.; Lee, S. H.; Chen, J.; Pierrot, D.; Sullivan, K.; et al. (2010). "Decrease in the CO2 Uptake Capacity in an Ice-Free Arctic Ocean Basin". Science. 329 (5991): 556559. Bibcode:2010Sci...329..556C. doi:10.1126/science.1189338. PMID 20651119.
  75. Garrison, Tom (2004). Oceanography: An Invitation to Marine Science. Thomson Brooks. p. 125. ISBN 0-534-40887-7.
  76. Ries, J. B.; Cohen, A. L.; McCorkle, D. C. (2009). "Marine calcifiers exhibit mixed responses to CO2-induced ocean acidification". Geology. 37 (12): 1131–1134. Bibcode:2009Geo....37.1131R. doi:10.1130/G30210A.1.
  77. Climate Change 2007: Synthesis Report, IPCC
  78. "PMEL Ocean Acidification Home Page". Pmel.noaa.gov. Retrieved 2014-01-14.
  79. Lupton, J.; Lilley, M.; Butterfield, D.; Evans, L.; Embley, R.; Olson, E.; Proskurowski, G.; Resing, J.; Roe, K.; Greene, R.; Lebon, G. (2004). "Liquid Carbon Dioxide Venting at the Champagne Hydrothermal Site, NW Eifuku Volcano, Mariana Arc". American Geophysical Union. Fall. Meeting (abstract #V43F–08): 8. Bibcode:2004AGUFM.V43F..08L.
  80. Dhingra A, Portis AR, Daniell H (2004). "Enhanced translation of a chloroplast-expressed RbcS gene restores small subunit levels and photosynthesis in nuclear RbcS antisense plants". Proc. Natl. Acad. Sci. U.S.A. 101 (16): 6315–20. Bibcode:2004PNAS..101.6315D. doi:10.1073/pnas.0400981101. PMC 395966Freely accessible. PMID 15067115. (Rubisco) is the most prevalent enzyme on this planet, accounting for 30–50% of total soluble protein in the chloroplast;
  81. Blom, T.J.; W.A. Straver; F.J. Ingratta; Shalin Khosla; Wayne Brown (December 2002). "Carbon Dioxide In Greenhouses". Retrieved 2007-06-12.
  82. Ainsworth, Elizabeth A. (2008). "Rice production in a changing climate: a meta-analysis of responses to elevated carbon dioxide and elevated ozone concentration" (PDF). Global Change Biology. 14 (7): 1642–1650. doi:10.1111/j.1365-2486.2008.01594.x. Archived from the original (PDF) on 2011-07-19.
  83. Long, SP; Ainsworth, EA; Leakey, AD; Nösberger, J; Ort, DR (2006). "Food for thought: lower-than-expected crop yield stimulation with rising CO2 concentrations". Science. 312 (5782): 1918–21. Bibcode:2006Sci...312.1918L. doi:10.1126/science.1114722. PMID 16809532.
  84. F. Woodward; C. Kelly (1995). "The influence of CO2 concentration on stomatal density". New Phytologist. 131 (3): 311–327. doi:10.1111/j.1469-8137.1995.tb03067.x.
  85. Bert G. Drake; Gonzalez-Meler, Miquel A.; Long, Steve P. (1997). "More efficient plants: A consequence of rising atmospheric CO2?". Annual Review of Plant Physiology and Plant Molecular Biology. 48 (1): 609–639. doi:10.1146/annurev.arplant.48.1.609. PMID 15012276.
  86. Loladze, I (2002). "Rising atmospheric CO2 and human nutrition: toward globally imbalanced plant stoichiometry?". Trends in Ecology & Evolution. 17 (10): 457–461. doi:10.1016/S0169-5347(02)02587-9.
  87. Carlos E. Coviella; John T. Trumble (1999). "Effects of Elevated Atmospheric Carbon Dioxide on Insect-Plant Interactions". Conservation Biology. 13 (4): 700–712. doi:10.1046/j.1523-1739.1999.98267.x. JSTOR 2641685.
  88. Davey, M. P.; Harmens, H.; Ashenden, T. W.; Edwards, R.; Baxter, R. (2007). "Species-specific effects of elevated CO2 on resource allocation in Plantago maritima and Armeria maritima". Biochemical Systematics and Ecology. 35 (3): 121–129. doi:10.1016/j.bse.2006.09.004.
  89. Davey, M.; Bryant, D. N.; Cummins, I.; Ashenden, T. W.; Gates, P.; Baxter, R.; Edwards, R. (2004). "Effects of elevated CO2 on the vasculature and phenolic secondary metabolism of Plantago maritima". Phytochemistry. 65 (15): 2197–2204. doi:10.1016/j.phytochem.2004.06.016. PMID 15587703.
  90. "Global Environment Division Greenhouse Gas Assessment Handbook – A Practical Guidance Document for the Assessment of Project-level Greenhouse Gas Emissions". World Bank. Retrieved 2007-11-10.
  91. Luyssaert, Sebastiaan; Schulze, E. -Detlef; Börner, Annett; Knohl, Alexander; Hessenmöller, Dominik; Law, Beverly E.; Ciais, Philippe; Grace, John (2008). "Old-growth forests as global carbon sinks". Nature. 455 (7210): 213–5. Bibcode:2008Natur.455..213L. doi:10.1038/nature07276. PMID 18784722.
  92. Falkowski P, Scholes RJ, Boyle E, Canadell J, Canfield D, Elser J, Gruber N, Hibbard K, Högberg P, Linder S, Mackenzie FT, Moore B 3rd, Pedersen T, Rosenthal Y, Seitzinger S, Smetacek V, Steffen W (2000). "The global carbon cycle: a test of our knowledge of earth as a system". Science. 290 (5490): 291–296. Bibcode:2000Sci...290..291F. doi:10.1126/science.290.5490.291. PMID 11030643.
  93. 1 2 Friedman, Daniel. Toxicity of Carbon Dioxide Gas Exposure, CO2 Poisoning Symptoms, Carbon Dioxide Exposure Limits, and Links to Toxic Gas Testing Procedures. InspectAPedia
  94. "CarbonTracker CT2011_oi (Graphical map of CO2)". esrl.noaa.gov.
  95. "Carbon Dioxide as a Fire Suppressant: Examining the Risks". U.S. Environmental Protection Agency:.
  96. Volcano Under the City. PBS.org (1 November 2005).
  97. Glatte Jr H. A.; Motsay G. J.; Welch B. E. (1967). "Carbon Dioxide Tolerance Studies". Brooks AFB, TX School of Aerospace Medicine Technical Report. SAM-TR-67-77. Retrieved 2008-05-02.
  98. Lambertsen, C. J. (1971). "Carbon Dioxide Tolerance and Toxicity". Environmental Biomedical Stress Data Center, Institute for Environmental Medicine, University of Pennsylvania Medical Center. IFEM. Philadelphia, PA. Report No. 2-71. Retrieved 2008-05-02.
  99. 1 2 Satish U.; Mendell M. J.; Shekhar K.; Hotchi T.; Sullivan D.; Streufert S.; Fisk W.J. (2012). "Is CO2 an Indoor Pollutant? Direct Effects of Low-to-Moderate CO2 Concentrations on Human Decision-Making Performance" (PDF). Environmental Health Perspectives. 120 (12). doi:10.1289/ehp.1104789.
  100. 1 2 Joseph G. Allen; Piers MacNaughton; Usha Satish; Suresh Santanam; Jose Vallarino; John D. Spengler1Satish U. (2016). "Associations of Cognitive Function Scores with Carbon Dioxide, Ventilation, and Volatile Organic Compound Exposures in Office Workers: A Controlled Exposure Study of Green and Conventional Office Environments". Environmental Health Perspectives. 124 (6). doi:10.1289/ehp.1510037.
  101. Bierwirth P. (2014). "How will rising carbon dioxide in the atmosphere directly affect human health via breathing toxicity? A Science Review" (PDF).
  102. "Exposure Limits for Carbon Dioxide Gas – CO2 Limits". InspectAPedia.com.
  103. Law J.; Watkins S.; Alexander, D. (2010). "In-Flight Carbon Dioxide Exposures and Related Symptoms: Associations, Susceptibility and Operational Implications" (PDF). NASA Technical Report. TP–2010–216126. Retrieved 2014-08-26.
  104. Schaefer K. E. (1979). "Effect of Prolonged Exposure to 0.5% CO2 on Kidney Calcification and Ultrastructure of Lungs". Undersea Biomed Res. S6: 155–117. Retrieved 2014-10-19.
  105. "How much carbon dioxide do humans contribute through breathing?". Archived from the original on 2011-02-02. Retrieved 2009-04-30.
  106. Charles Henrickson (2005). Chemistry. Cliffs Notes. ISBN 0-7645-7419-1.
  107. 1 2 3 4 Derived from mmHg values using 0.133322 kPa/mmHg
  108. 1 2 Normal Reference Range Table. University of Texas Southwestern Medical Center at Dallas. Used in Interactive Case Study Companion to Pathologic basis of disease.
  109. 1 2 3 4 "Carbon dioxide". solarnavigator.net. Retrieved 2007-10-12.

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