Methane
| Methane | |
|---|---|
 
| |
| General | |
| Other names | Marsh gas |
| Molecular formula | CH4 |
| SMILES | C |
| Molar mass | 16.04 g/mol |
| Appearance | colorless gas |
| CAS number | [74-82-8] |
| Properties | |
| Density and phase | 0.717 kg/m3, gas |
| Solubility in water | 3.5 mL g/100 ml (17°C) |
| Melting point | −182.5 °C (90.6 K) |
| Boiling point | −161.6 °C (111.55 K) |
| Triple point | 90.7 K, 0.117 bar |
| Critical temperature | 190.5 °K (−82.6 °C) at 4.6 MPa (45 atm) |
| Structure | |
| Molecular shape | tetrahedral |
| Symmetry group | Td |
| Dipole moment | Zero |
| Hazards | |
| MSDS | External MSDS |
| EU classification | Highly flammable (F+) |
| NFPA 704 |
4
1
0
|
| R-phrases | R12 |
| S-phrases | S2, S9, S16, S33 |
| Flash point | −188 °C |
| Autoignition temperature | 537 °C |
| Maximum burning temperature: |
2,148 °C |
| Explosive limits | 5–15 percent |
| Supplementary data page | |
| Structure and properties |
|
| Thermodynamic data |
|
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Related alkanes | Ethane Propane |
| Related compounds | Methanol Chloromethane |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Methane is the simplest hydrocarbon, with the chemical formula CH4. In chemical terms, it is classified as an alkane. At ordinary temperatures and pressures, it is a gas. It is a minor constituent of the Earth's atmosphere, but it is the main component of natural gas and biogas. Large quantities of methane have been found in sediments on the ocean floor, where it is trapped in cage-like ice crystals known as methane clathrates. Methane is widely used as a fuel, but it is also a starting material for the synthesis of other compounds. In nature, it plays an important role as a "greenhouse gas"—a gas that helps trap the Earth's heat, preventing the heat from escaping into space.
Occurrence and production
The Earth's mantle is the main reservoir of methane, and large quantities of this gas have been found in geological deposits known as natural gas fields. It occurs in association with other hydrocarbons and sometimes also helium and nitrogen. In general, natural gas is present in sediments buried deeper and at higher temperatures than those that contain petroleum. Natural gas fields are currently the main source from which methane is extracted for human use.
Methane can also be extracted from coal deposits. It is the main component of the firedamp of coal mines. It is also emitted by mud volcanoes that are connected to deep geological faults.
Biogas, produced by wetlands and landfills, is another source of methane. Biogas is a mixture of methane, carbon dioxide, and small amounts of other gases. It is generated by the microbial fermentation of organic matter—including manure, wastewater sludge, municipal solid waste, or other biodegradable feedstock—under anaerobic conditions. Biogas is also called swamp gas, landfill gas, or marsh gas, depending on where it is produced.
Source: USGS
Large deposits of methane have been found in a form known as methane clathrate, under sediments on the ocean floors. Also known as methane hydrate or methane ice, it consists of methane molecules held in cage-like, crystalline structures of frozen water. Methane clathrates are thought to be formed when methane gas streams rising from geological faults come in contact with cold seawater. One liter of methane clathrate solid would contain, on average, 168 liters of methane gas (at 25 °C and 100 kPa pressure).
In addition to the above-mentioned sources, methane is produced by the digestive systems of ruminants, termites, rice paddies, and oceans [1], [2].
Until recently, the consensus view has been that most of the methane from biological sources was produced by processes in oxygen-poor environments. In January 2006, however, a group of researchers reported that plants exposed to atmospheric levels of oxygen also constitute an important source of methane [3], [4]. The researchers noted that "this newly identified source may have important implications for the global methane budget and may call for a reconsideration of the role of natural methane sources in past climate change."
Artificial synthesis
In the laboratory, methane can be produced by the direct reaction of carbon with hydrogen, or aluminum carbide with water. In industrial settings, methane is produced by chemical reactions between hydrogen and common atmospheric gases.
Properties
At room temperature and pressure, methane is a colorless, odorless gas, lighter than air. At a pressure of 1 atmosphere, its boiling point is -161.5 °C (-258.7 °F) and melting point is -182.5 °C (-296.5 °F). It is highly flammable and reacts violently with oxidizers, halogens, and some halogen compounds.
Each molecule of methane is small, consisting of four atoms of hydrogen attached to a single atom of carbon through covalent bonds. The molecule is shaped like a tetrahedron, with the carbon atom at the center and the four hydrogen atoms occupying the four corners of the tetrahedron. Unlike water molecules, which are polar and attract one another, methane molecules are non-polar and do not have much attraction for one another. This is the reason why, at room temperature, methane is a gas while water is a liquid.
Reactions of methane
Combustion
When methane is burned in the presence of oxygen, the reaction—called a combustion reaction—produces carbon dioxide, water, and a large amount of heat. In molecular terms, the chemical reaction can be represented as follows:
- CH4 + 2O2 → CO2 + 2H2O + heat
Hydrogen activation
In methane, the carbon-hydrogen covalent bond is among the strongest in all hydrocarbons. In chemical terms, there is a high "activation barrier" to break this C-H bond—in other words, considerable energy is required to break it. Nonetheless, methane is still the principal starting material for the manufacture of hydrogen. The search for catalysts that can lower the activation barrier and other small-molecule alkanes is an area of research with considerable industrial significance.
Reactions with halogens
Under the proper conditions, methane reacts with all the halogens. The general reaction can be represented as follows:
- CH4 + X2 → CH3X + HX
Here, X is either fluorine (F), chlorine (Cl), bromine (Br), or sometimes iodine (I).
This reaction may continue, so that CH3X reacts with X2 to produce CH2X2; CH2X2 in turn can react with X2 to produce CHX3; and CHX3 can react further with X2 to produce CX4.
Potential health effects
Methane is not toxic, but because it is highly flammable it can form mixtures with air that are explosive. In addition, if it displaces oxygen within an enclosed space, and the oxygen concentration drops below 18 percent, it can lead to asphyxiation. For these reasons, commercially available methane is usually mixed with small quantities of odorants—strong-smelling sulfur compounds, such as ethyl mercaptan, to enable the detection of leaks.
When structures are built on or near landfills, methane off-gas can penetrate the building interior and expose occupants to significant levels of methane. Some buildings have specially engineered recovery systems below their basements, to actively capture such fugitive off-gas and vent it away from the building.
Methane in the Earth's atmosphere
Early Earth's atmosphere
Scientists think that early in the Earth's history—about 3.5 billion years ago—there was one thousand times as much methane in the atmosphere as there is now. The earliest methane was released into the atmosphere by volcanic activity. In addition, ancient bacteria contributed to the methane concentration by converting hydrogen and carbon dioxide into methane and water. Oxygen did not become a major part of the atmosphere until photosynthetic organisms emerged later in Earth's history. In the absence of oxygen, methane stayed in the atmosphere longer and at higher concentrations than it does today.
Recent status
Currently, methane is a minor constituent of our planet's atmosphere. The average concentration of methane at the Earth's surface in 1998 has been estimated as 1,745 ppb (parts per billion) [5]. Its concentration is higher in the northern hemisphere, as most sources (natural and human) are greater there. In addition, the concentration varies seasonally, with a minimum in the late summer.
Removal processes
The main process by which methane is removed from the Earth's atmosphere is its reaction with the hydroxyl radical (·OH)—a reactive entity that may be produced when a cosmic ray strikes a molecule of water vapor. The chemical change can be written as follows.
- CH4 + ·OH → ·CH3 + H2O
Two additional sets of processes that remove minor quantities of methane are: (a) the activity of aerobic microbes in soils, and (b) reactions with ·OH, ·Cl, and ·O(1D) in the stratosphere. Based on these processes, the estimated lifetime of methane in the atmosphere has been calculated to be 8.4 years [6].
Uses
Fuel
- For more on the use of methane as a fuel, see: Natural gas.
Methane is an important fuel. Being the simplest hydrocarbon, the combustion of methane produces more heat per gram than other hydrocarbons. In addition, compared to other hydrocarbon fuels, burning methane produces less carbon dioxide for each unit of heat released.
In the form of natural gas, methane is regularly distributed via gas pipelines. In many cities, it is piped into homes for domestic heating and cooking purposes. Moreover, large quantities are burned to drive gas or steam turbines, to generate electricity.
When biogas is used as a fuel, it provides a convenient way to turn waste into electricity. The process of producing biogas decreases the amount of waste to be disposed of and destroys disease-causing microbes that are present in the waste stream.
Industrial uses
In the chemical industry, methane is the feedstock of choice for the production of hydrogen, methanol, acetic acid, and acetic anhydride. To produce any of these chemicals, methane is first made to react with steam in the presence of a nickel catalyst at high temperatures (700–1,100 °C). The chemical equation is as follows:
- CH4 + H2O → CO + 3H2
The product, known as "synthesis gas," is a mixture of carbon monoxide and hydrogen. Synthesis gas is then manipulated to produce the intended products.
Moreover, acetylene is prepared by passing methane through an electric arc. When methane is made to react with chlorine gas, various chloromethanes are produced: chloromethane, dichloromethane, chloroform, and carbon tetrachloride. The use of these chemicals, however, is declining. Acetylene may be replaced by less costly substitutes, and the chloromethanes are used less often because of health and environmental concerns.
Greenhouse gas
Methane in the Earth's atmosphere is an important "greenhouse gas" that contributes to the "greenhouse effect." The Earth absorbs some of the Sun's energy and then emits energy at longer wavelengths. Greenhouse gases (including water vapor, carbon dioxide, and methane) absorb the heat being emitted and prevent it from escaping into space. In this manner, greenhouse gases play a vital role in keeping the planet warm enough for human habitation.
The current concern about global warming is based on reports that the concentrations of greenhouse gases have risen in recent years, mainly as a result of human activities, leading to an upward trend in the Earth's temperature [7]. Some have contended that if this warming trend is not reversed, it could soon lead to dire consequences. This subject, however, is the focus of intense study and debate.
In the case of methane, its concentration has reportedly increased by about 150 percent since 1750. In addition, its "global warming potential" is estimated to be 23 over a 100-year period. In other words, when averaged over one hundred years, each kilogram of methane warms the Earth 23 times as much as the same mass of carbon dioxide. Nonetheless, the rates of emission of methane by different sources in the biosphere are highly variable and difficult to assess. Consequently, it is difficult to predict future concentrations of methane in the atmosphere [8].
Extraterrestrial methane
Methane has been detected or is believed to exist in several locations of the solar system beyond our planet, as listed below.
- Jupiter
- Mars
- Saturn
- Iapetus
- Titan
- Enceladus
- Neptune
- Triton
- Uranus
- Ariel
- Miranda
- Oberon
- Titania
- Umbriel
- Comet Halley
- Comet Hyakutake
- 2003 UB313
Traces of methane gas are present in the thin atmosphere of the Earth's Moon. Methane has also been detected in interstellar clouds.
See also
- Alkane
- Butane
- Ethane
- Hydrocarbon
- Methanogen
- Natural gas
- Propane
ReferencesISBN links support NWE through referral fees
- McMurry, John. 2004. Organic Chemistry, 6th ed. Belmont, CA: Brooks/Cole. ISBN 0534420052.
- Morrison, Robert T., and Robert N. Boyd. 1992. Organic Chemistry, 6th ed. Englewood Cliffs, NJ: Prentice Hall. ISBN 0136436692.
- Solomons, T.W. Graham, and Craig B. Fryhle. 2004. Organic Chemistry, 8th ed. Hoboken, NJ: John Wiley. ISBN 0471417998.
| Alkanes | |||||||||||||||||||||||||||||||
|
methane |
| |
ethane |
| |
propane |
| |
butane |
| |
pentane |
| |
hexane |
|||||||||||||||||||||
|
heptane |
| |
octane |
| |
nonane |
| |
decane |
| |
undecane |
| |
dodecane |
| ||||||||||||||||||||
Credits
New World Encyclopedia writers and editors rewrote and completed the Wikipedia article in accordance with New World Encyclopedia standards. This article abides by terms of the Creative Commons CC-by-sa 3.0 License (CC-by-sa), which may be used and disseminated with proper attribution. Credit is due under the terms of this license that can reference both the New World Encyclopedia contributors and the selfless volunteer contributors of the Wikimedia Foundation. To cite this article click here for a list of acceptable citing formats.The history of earlier contributions by wikipedians is accessible to researchers here:
The history of this article since it was imported to New World Encyclopedia:
Note: Some restrictions may apply to use of individual images which are separately licensed.
