WordNet
- a colorless flammable gas used chiefly in welding and in organic synthesis (同)ethyne, alkyne
PrepTutorEJDIC
- アセチレン[ガス]
Wikipedia preview
出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2015/09/02 22:24:39」(JST)
wiki ja
| アセチレン | |
|---|---|
|
IUPAC名
Ethyne[1] |
|
|
系統名
Acetylene
|
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| 識別情報 | |
| CAS登録番号 | 74-86-2 |
| ChemSpider | 6086 |
| UNII | OC7TV75O83 |
| 国連番号 | 1001 (dissolved) 3138 (in mixture with ethylene and propylene) |
| KEGG | C01548 |
| ChEBI | CHEBI:27518 |
| ChEMBL | CHEMBL116336 |
|
SMILES
|
|
|
InChI
|
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| 特性 | |
| 化学式 | C2H2 |
| モル質量 | 26.04 g mol−1 |
| 密度 | 1.097 kg m−3 |
| 融点 |
−80.8 °C, 192.4 K, −113.4 °F (三重点) |
| 沸点 |
−84 °C, 189 K, -119 °F (昇華) |
| 酸解離定数 pKa | 25 |
| 構造 | |
| 分子の形 | 直線形 |
| 熱化学 | |
| 標準生成熱 ΔfH |
+226.88 kJ/mol |
| 危険性 | |
| NFPA 704 |
4
1
3
|
| 特記なき場合、データは常温 (25 °C)・常圧 (100 kPa) におけるものである。 | |
アセチレン (acetylene) は炭素数が2のアルキンである。IUPAC系統名はエチン ethyne、分子式は C2H2である。1836年にイギリスのエドモンド・デービーによって発見され、水素と炭素の化合物であるとされた。1860年になってマルセラン・ベルテロが再発見し、「アセチレン」と命名した。アルキンのうち工業的に最も重要なものである。
酸素と混合し、完全燃焼させた場合の炎の温度は3,330 °Cにも及ぶため、その燃焼熱を目的として金属加工工場などで多く使われる。高圧ガス保安法により、常用の温度で圧力が0.2 MPa以上になるもので、現に0.2 MPa以上のもの、または、15 °Cで0.2 MPa以上となるものである場合、褐色のボンベに保管することが定められている。
目次
- 1 構造
- 2 物理的性質
- 3 化学的性質
- 3.1 付加反応
- 3.2 付加重合
- 3.3 アセチリド
- 4 所在・製法
- 5 利用
- 5.1 工業等への利用
- 5.2 照明等への利用
- 6 アセチレンから合成される化合物
- 7 参考文献
- 8 関連項目
- 9 外部リンク
構造
構造式は HC≡CH で、炭素-炭素間で三重結合を1個だけ持つ直線型分子。炭素‐炭素間でπ結合を二つ持ち、sp混成軌道を取り、結合角は180ﾟである。アルキンのうち最も簡単なものであり、異性体は存在しない。
物理的性質
常温では水に体積比 1:1 の割合で溶ける。テトラヒドロフランなどの有機溶媒にはより溶けやすい。爆発範囲は 2.5–81 vol%（空気中）である。純粋なものは無臭だが、市販されているものは通常硫黄化合物などの不純物を含むため、特有のにおいを持つ。
化学的性質
アセチレンや一般のアルキンは三重結合を持つ不飽和炭化水素のため反応性が大きく、さまざまな物質の合成の原料となる。銀、銅、水銀等の金属や金属化合物と反応し、爆発性のある金属アセチリドを生成する。人体に対して有害性はないが、可燃性である。
付加反応
アセチレンの三重結合は付加反応を受けやすい。ニッケルを触媒として水素を付加させるとエチレンになり、さらに水素を付加させるとエタンになる。
- HC≡CH + H2 Li → H2C=CH2
- H2C=CH2 + H2 Li → H3C−CH3
また、アセチレンの三重結合にはハロゲン化水素などの H−X 型の分子を容易に付加させることができる。 アセチレンに塩化水素を付加させるとクロロエチレンになり、酢酸を付加させると酢酸ビニルになる。クロロエチレンや酢酸ビニルは合成高分子化合物の原料として用いられる。
- HC≡CH + H−X Li → H2C=CHX
アセチレンに水を付加させた場合はビニルアルコールとなるが、これは容易に異性化し、速やかにアセトアルデヒドに変わる。
付加重合
アセチレンは付加重合をすることができる。アセチレン2分子が重合するとモノビニルアセチレンになる。モノビニルアセチレンはブタジエンやクロロプレンの原料として、合成ゴムをつくるときに用いられる。
- 2 HC≡CH Li → H2C=CH−C≡CH
アセチレン3分子が重合するとベンゼン、ジビニルアセチレン、アセチレニルジビニルになる。 ベンゼンを得る場合、加熱した鉄管もしくは石英管にアセチレンガスを通す方法がよく使われる。
- 3 HC≡CH Li → C6H6
さらに重合が進んで得られるポリマーがポリアセチレンで、導電性物質として利用される。
アセチリド
アセチレンをはじめとする末端アルキン上の水素は、一般的なアルケンやアルカンのものに比べて酸性が高く、適切な強塩基により引き抜いて金属イオンに置き換えることができる。例えば、アセチレンにn-ブチルリチウムを作用させるとリチウムアセチリドを与える。
- HC≡CH + n-C4H9Li → HC≡CLi + n-C4H10↑
また、硝酸銀水溶液にアセチレンを吹き込むと、銀アセチリドの白色沈殿ができる。硫酸銅に作用させると銅アセチリドの赤色沈殿が発生する。銀アセチリドも、銅アセチリドも乾燥していれば、わずかな衝撃で爆発し、銀や銅と炭素に分解する。
所在・製法
実験室やアセチレンランプなど小規模な用途では、カーバイド法を用いて生成される。これは、カーバイド（炭化カルシウム）に水を作用させる方法である。 工業用の大規模なものでは[2]、アセチレンは炭化水素の熱分解による方法(熱分解法)や、カーバイド法を用いて生成される。: CaC2 + 2H2O → C2H2 + Ca(OH)2
利用
アセチレンガスは他のLPガス等と同様に圧縮冷却すると液化できる。しかしアセチレンは3重結合の極めて不安定な物質なため分解爆発を起こす危険があることから容器内にマスと呼ばれる軽石様の多孔質物質にアセトンを染み込ませ炭酸水のようにアセトンへ溶解させて充填させている。なお、この溶解アセチレン（ボンベ製品）の2008年度日本国内生産量は14,532tである[3]。
燃焼速度が極めて速く燃焼範囲も可燃性ガスの中では一番広い（水素は２番目）ため空気中へ漏洩すると爆発の条件が揃いやすく危険な可燃性ガスでもある。
工業等への利用
- アセチレンは燃焼するときに多量の燃焼熱を発生するので、バーナーの燃料として用いられる。アセチレンと酸素を混合して完全燃焼させた酸素アセチレン炎 (3,330℃) は金属の溶接や切断に用いられる。アメリカ合衆国では、年間生産の8割が化学合成に、残りの2割がアセチレン溶接、切断に使われている。近年でも、鉄の浸炭に使われる。
照明等への利用
- かつては アセチレンランプ（カーバイドランプ）として照明用に使われていた。アセチレンランプは、上部と下部に別れ、上部の水が下部のカルシウムカーバイドに滴り落ちアセチレンが発生するのを利用している。光量の調節が容易なため、高性能の蓄電池や送電線が普及するまでは、炭鉱の坑内灯や携帯灯具（カンテラ）、蒸気機関車や自動車の前照灯などにも使われた。街灯としては、1897年7月24日にハンガリーのタタに、1898年には英国のノース・ペザトンに設置されている。
- スウェーデンのニルス・グスタフ・ダレーンは、1912年にアセチレンを利用した「灯台や灯浮標などの照明用ガス貯蔵器用の自動調節機の発明」でノーベル物理学賞を受賞した。
- 現在でも洞窟内探検（ケービング）でカンテラとして使用されることがある。
アセチレンから合成される化合物
- エチレン
- アセトアルデヒド
- ベンゼン
- アクリロニトリル
- 塩化ビニル
- 酢酸ビニル
- ビニルアセチレン
- ポリアセチレン
- 金属アセチリド
参考文献
- ^ Acyclic Hydrocarbons. Rule A-3. Unsaturated Compounds and Univalent Radicals, IUPAC Nomenclature of Organic Chemistry
- ^ 社団法人日本溶接協会 監修『新版 ガス溶接技能者教本』改訂第２版,産報出版,p22
- ^ 化学工業統計月報 - 経済産業省
関連項目
- アルキン
- エタン
- エチレン
- アセチレンランプ
外部リンク
- 日本産業ガス協会
- タツオカ - アセチレンガスの物性、化学的性質、取扱注意事項、用途
wiki en
"HCCH" redirects here. For other uses, see HCCH (disambiguation).
| Names | |
|---|---|
| IUPAC name
Ethyne
|
|
| Systematic IUPAC name
Ethyne[1]
|
|
| Identifiers | |
|
CAS Registry Number
|
74-86-2 Y |
| ChEBI | CHEBI:27518 Y |
| ChEMBL | ChEMBL116336 Y |
| ChemSpider | 6086 Y |
|
InChI
|
|
| Jmol-3D images | Image |
| KEGG | C01548 Y |
|
SMILES
|
|
| UNII | OC7TV75O83 Y |
| UN number | 1001 (dissolved) 3138 (in mixture with ethylene and propylene) |
| Properties | |
|
Chemical formula
|
C2H2 |
| Molar mass | 26.04 g·mol−1 |
| Density | 1.097 g/L = 1.097 kg/m3 |
| Melting point | −80.8 °C (−113.4 °F; 192.3 K) Triple point at 1.27 atm |
|
Sublimation
conditions |
−84 °C; −119 °F; 189 K (1 atm) |
|
Solubility in water
|
slightly soluble |
| Vapor pressure | 44.2 atm (20°C)[2] |
| Acidity (pKa) | 25[3] |
| Structure | |
|
Molecular shape
|
Linear |
| Thermochemistry | |
|
Std molar
entropy (S |
201 J·mol−1·K−1 |
|
Std enthalpy of
formation (ΔfH |
+226.88 kJ/mol |
| Hazards | |
| NFPA 704 |
4
1
3
|
|
Autoignition
temperature |
300 °C (572 °F; 573 K) |
| US health exposure limits (NIOSH): | |
|
PEL (Permissible)
|
none[2] |
|
REL (Recommended)
|
C 2500 ppm (2662 mg/m3)[2] |
|
IDLH (Immediate danger
|
N.D.[2] |
|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
|
| Y verify (what is: Y/N?) | |
| Infobox references | |
Acetylene (systematic name: ethyne) is the chemical compound with the formula C2H2. It is a hydrocarbon and the simplest alkyne.[4] This colourless gas is widely used as a fuel and a chemical building block. It is unstable in pure form and thus is usually handled as a solution.[5] Pure acetylene is odourless, but commercial grades usually have a marked odour due to impurities.[6]
As an alkyne, acetylene is unsaturated because its two carbon atoms are bonded together in a triple bond. The carbon–carbon triple bond places all four atoms in the same straight line, with CCH bond angles of 180 °. Since acetylene is a linear symmetrical molecule, it possesses the D∞h point group.[7]
Contents
- 1 Discovery
- 2 Preparation
- 3 Bonding
- 4 Physical properties
- 4.1 Changes of state
- 4.2 Other
- 5 Reactions
- 5.1 Reppe chemistry
- 6 Applications
- 6.1 Welding
- 6.2 Portable lighting
- 6.3 Niche applications
- 7 Natural occurrence
- 8 Safety and handling
- 9 References
- 10 External links
Discovery
Acetylene was discovered in 1836 by Edmund Davy, who identified it as a "new carburet of hydrogen".[8][9] It was rediscovered in 1860 by French chemist Marcellin Berthelot, who coined the name "acetylene".[10] Berthelot was able to prepare this gas by passing vapours of organic compounds (methanol, ethanol, etc.) through a red-hot tube and collecting the effluent. He also found acetylene was formed by sparking electricity through mixed cyanogen and hydrogen gases. Berthelot later obtained acetylene directly by passing hydrogen between the poles of a carbon arc.[11][12] Commercially available acetylene gas could smell foul due to the common impurities hydrogen sulphide and phosphine. However, acetylene gas with high purity would generate a light and sweet smell.
Preparation
Today acetylene is mainly manufactured by the partial combustion of methane or appears as a side product in the ethylene stream from cracking of hydrocarbons. Approximately 400,000 tonnes are produced by this method annually.[5] Its presence in ethylene is usually undesirable because of its explosive character and its ability to poison Ziegler-Natta catalysts. It is selectively hydrogenated into ethylene, usually using Pd–Ag catalysts.[13]
Until the 1950s, when oil supplanted coal as the chief source of reduced carbon, acetylene (and the aromatic fraction from coal tar) was the main source of organic chemicals in the chemical industry. It was prepared by the hydrolysis of calcium carbide, a reaction discovered by Friedrich Wöhler in 1862[14] and still familiar to students:
- CaC2 + 2H2O → Ca(OH)2 + C2H2
Calcium carbide production requires extremely high temperatures, ~2000 °C, necessitating the use of an electric arc furnace. In the US, this process was an important part of the late-19th century revolution in chemistry enabled by the massive hydroelectric power project at Niagara Falls.[15]
Bonding
In terms of valence bond theory, in each carbon atom the 2s orbital hybridizes with one 2p orbital thus forming an sp hybrid. The other two 2p orbitals remain unhybridized. The two ends of the two sp hybrid orbital overlap to form a strong σ valence bond between the carbons, while on each of the other two ends hydrogen atoms attach also by σ bonds. The two unchanged 2p orbitals form a pair of weaker π bonds.[16]
Physical properties
Changes of state
At atmospheric pressure, acetylene cannot exist as a liquid and does not have a melting point. The triple point on the phase diagram corresponds to the melting point (−80.8 °C) at the minimum pressure at which liquid acetylene can exist (1.27 atm). At temperatures below the triple point, solid acetylene can change directly to the vapour (gas) by sublimation. The sublimation point at atmospheric pressure is −84 °C.
Other
The adiabatic flame temperature in air at atmospheric pressure is 2534 °C.
Acetylene gas can be dissolved in acetone or dimethylformamide in room temperature and 1 atm.
Reactions
Main article: Alkyne
One new application is the conversion of acetylene to ethylene for use in making a variety of polyethylene plastics. An important reaction of acetylene is its combustion, the basis of the acetylene welding technologies. Otherwise, its major applications involve its conversion to acrylic acid derivatives.[5]
Compared to most hydrocarbons, acetylene is relatively acidic, though it is still much less acidic than water or ethanol. Thus it reacts with strong bases to form acetylide salts. For example, acetylene reacts with sodium amide in liquid ammonia to form sodium acetylide, and with butyllithium in cold THF to give lithium acetylide.[17]
Acetylides of heavy metals are easily formed by reaction of acetylene with the metal ions. Several, e.g., silver acetylide (Ag2C2) and copper acetylide (Cu2C2), are powerful and very dangerous explosives.[18]
Reppe chemistry
Walter Reppe discovered that in the presence of metal catalysts, acetylene can react to give a wide range of industrially significant chemicals.[19][20]
- With alcohols, hydrogen cyanide, hydrogen chloride, or carboxylic acids to give vinyl compounds:[5]
- With aldehydes to give ethynyl diols,[5] in the Favorskii reaction:
- 1,4-Butynediol is produced industrially in this way from formaldehyde and acetylene.
- With carbon monoxide to give acrylic acid, or acrylic esters, which can be used to produce acrylic glass:[21]
- Cyclicization to give benzene, cyclooctatetraene,[5] or hydroquinone:[20]
Applications
Welding
Approximately 20 percent of acetylene is supplied by the industrial gases industry for oxyacetylene gas welding and cutting due to the high temperature of the flame; combustion of acetylene with oxygen produces a flame of over 3,600 K (3,300 °C, 6,000 °F), releasing 11.8 kJ/g. Oxyacetylene is the hottest burning common fuel gas.[22] Acetylene is the third hottest natural chemical flame after dicyanoacetylene's 5260 K (4990 °C, 9010 °F) and cyanogen at 4798 K (4525 °C, 8180 °F). Oxy-acetylene welding was a very popular welding process in previous decades; however, the development and advantages of arc-based welding processes have made oxy-fuel welding nearly extinct for many applications. Acetylene usage for welding has dropped significantly. On the other hand, oxy-acetylene welding equipment is quite versatile – not only because the torch is preferred for some sorts of iron or steel welding (as in certain artistic applications), but also because it lends itself easily to brazing, braze-welding, metal heating (for annealing or tempering, bending or forming), the loosening of corroded nuts and bolts, and other applications. Bell Canada cable repair technicians still use portable acetylene fuelled torch kits as a soldering tool for sealing lead sleeve splices in manholes and in some aerial locations. Oxyacetylene welding may also be used in areas where electricity is not readily accessible. As well, oxy-fuel cutting is still very popular and oxy-acetylene cutting is utilized in nearly every metal fabrication shop. For use in welding and cutting, the working pressures must be controlled by a regulator, since above 15 psi,[23] if subjected to a shockwave (caused for example by a flashback),[24] acetylene will decompose explosively into hydrogen and carbon.
Acetylene fuel container/burner as used in the island of Bali
Portable lighting
Calcium carbide was used to generate acetylene used in the lamps for portable or remote applications. It was used for miners and cavers before the widespread use of incandescent lighting; or many years later low-power/high-lumen LED lighting; and is still used by mining industries in some nations without workplace safety laws. It was also used as an early light source for lighthouses.
Niche applications
In 1881, the Russian chemist Mikhail Kucherov[25] described the hydration of acetylene to acetaldehyde using catalysts such as mercury(II) bromide. Before the advent of the Wacker process, this reaction was conducted on an industrial scale.[26]
The polymerization of acetylene with Ziegler-Natta catalysts produces polyacetylene films. Polyacetylene, a chain of CH centres with alternating single and double bonds, was the one of first discovered organic semiconductors. Its reaction with iodine produces a highly electrically conducting material. Although such materials are not useful, these discoveries led to the developments of organic semiconductors, as recognized by the Nobel Prize in Chemistry in 2000 to Alan J. Heeger, Alan G MacDiarmid, and Hideki Shirakawa.[5]
In the early 20th Century acetylene was widely used for illumination, including street lighting in some towns.[27] Most early automobiles used carbide lamps before the adoption of electric headlights.
Acetylene is sometimes used for carburization (that is, hardening) of steel when the object is too large to fit into a furnace.[28]
Acetylene is used to volatilize carbon in radiocarbon dating. The carbonaceous material in an archeological sample is treated with lithium metal in a small specialized research furnace to form lithium carbide (also known as lithium acetylide). The carbide can then be reacted with water, as usual, to form acetylene gas to be fed into mass spectrometer to measure the isotopic ratio of carbon-14 to carbon-12.[29]
Natural occurrence
The energy richness of the C≡C triple bond and the rather high solubility of acetylene in water make it a suitable substrate for bacteria, provided an adequate source is available. A number of bacteria living on acetylene have been identified. The enzyme acetylene hydratase catalyzes the hydration of acetylene to give acetaldehyde.[30]
- C2H2 + H2O → CH3CHO
Acetylene is a moderately common chemical in the universe, often associated with the atmospheres of gas giants.[31] One curious discovery of acetylene is on Enceladus, a moon of Saturn. Natural acetylene is believed to form from catalytic decomposition of long chain hydrocarbons at temperatures of 1,770 K and above. Since such temperatures are highly unlikely on such a small distant body, this discovery is potentially suggestive of catalytic reactions within that moon, making it a promising site to search for prebiotic chemistry.[32][33]
Safety and handling
Acetylene is not especially toxic but, when generated from calcium carbide, it can contain toxic impurities such as traces of phosphine and arsine, which give it a distinct garlic-like smell. It is also highly flammable, as most light hydrocarbons, hence its use in welding. Its most singular hazard is associated with its intrinsic instability, especially when it is pressurized: under certain conditions acetylene can react in an exothermic addition-type reaction to form a number of products, typically benzene and/or vinylacetylene, possibly in addition to carbon and hydrogen. Consequently, acetylene, if initiated by intense heat or a shockwave, can decompose explosively if the absolute pressure of the gas exceeds about 200 kPa (29 psi). Most regulators and pressure gauges on equipment report gauge pressure and the safe limit for acetylene therefore is 101 kPagage or 15 psig.[34][35] It is therefore supplied and stored dissolved in acetone or dimethylformamide (DMF),[36] contained in a gas cylinder with a porous filling (Agamassan), which renders it safe to transport and use, given proper handling. Copper catalyses the decomposition of acetylene and as a result acetylene should not be transported in copper pipes. Brass pipe fittings should also be avoided.
References
- ^ Acyclic Hydrocarbons. Rule A-3. Unsaturated Compounds and Univalent Radicals, IUPAC Nomenclature of Organic Chemistry
- ^ a b c d e "NIOSH Pocket Guide to Chemical Hazards #0008". National Institute for Occupational Safety and Health (NIOSH).
- ^ [1], Gas Encyclopaedia, Air Liquide
- ^ R.H.Petrucci, W.S.Harwood and F.G.Herring "General Chemistry", 8th edn.(Prentice-Hall 2002), p.1072
- ^ a b c d e f g Pässler, Peter; Hefner, Werner; Buckl, Klaus; Meinass, Helmut; Meiswinkel, Andreas; Wernicke, Hans-Jürgen; Ebersberg, Günter; Müller, Richard; Bässler, Jürgen; Behringer, Hartmut; Mayer, Dieter (2008). "Acetylene". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a01_097.pub3. ISBN 3527306730. . Article Online Posting Date: 15 October 2008
- ^ Compressed Gas Association (1995) Material Safety and Data Sheet – Acetylene.
- ^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 94–95. ISBN 978-0131755536.
- ^ Edmund Davy (August 1836) "Notice of a new gaseous bicarburet of hydrogen,", Report of the Sixth Meeting of the British Association for the Advancement of Science … , 5 : 62-63.
- ^ Miller, S.A. (1965). Acetylene: Its Properties, Manufacture and Uses 1. Academic Press Inc.
- ^ Bertholet (1860) "Note sur une nouvelle série de composés organiques, le quadricarbure d'hydrogène et ses dérivés" (Note on a new series of organic compounds, tetra-carbon hydride and its derivatives), Comptes rendus, series 3, 50 : 805–808. (Note: Berthelot's empirical formula for acetylene (C4H2) was incorrect because chemists at that time used the wrong atomic mass for carbon (6 instead of 12).)
- ^ Berthelot (1862) "Synthèse de l'acétylène par la combinaison directe du carbone avec l'hydrogène" (Synthesis of acetylene by the direct combination of carbon with hydrogen), Comptes rendus, series 3, 54 : 640-644.
- ^ Acetylene
- ^ Acetylene: How Products are Made
- ^ Wohler (1862) "Bildung des Acetylens durch Kohlenstoffcalcium" (Formation of actylene by calcium carbide), Annalen der Chemie und Pharmacie, 124 : 220.
- ^ Freeman, Horace (1919). "Manufacture of Cyanamide". The Chemical News and the Journal of Physical Science 117: 232. Retrieved 23 December 2013.
- ^ Organic Chemistry 7th ed. by J. McMurry, Thomson 2008
- ^ Midland, M. M.; McLoughlin, J. I.; Werley, Ralph T. (Jr.) (1990). "Preparation and Use of Lithium Acetylide: 1-Methyl-2-ethynyl-endo-3,3-dimethyl-2-norbornanol". Org. Synth. 68: 14. ; Coll. Vol. 8, p. 391
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
- ^ Peter Pässler, Werner Hefner, Klaus Buckl, Helmut Meinass, Andreas Meiswinkel, Hans-Jürgen Wernicke, Günter Ebersberg, Richard Müller, Jürgen Bässler, Hartmut Behringer and Dieter Mayer (2007). "Acetylene". Ullmann's Encyclopedia of Industrial Chemistry: pg. 44. doi:10.1002/14356007.a01_097.pub2. Retrieved 26 December 2013.
- ^ a b Reppe, Walter; Kutepow, N; and Magin, A (1969). "Cyclization of Acetylenic Compounds". Angewandte Chemie International Edition in English 8 (10): 727–733. doi:10.1002/anie.196907271. Retrieved 26 December 2013.
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- ^ Acetylene - Properties, Purity and Packaging - Acetylene is simplest member of unsaturated hydrocarbons called alkynes or acetylenes. Most important of all starting materials ...
- ^ ESAB Oxy-acetylene welding handbook - Acetylene properties
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External links
| Wikiquote has quotations related to: Acetylene |
- Acetylene Production Plant and Detailed Process
- Acetylene at Chemistry Comes Alive!
- Acetylene, the Principles of Its Generation and Use at Project Gutenberg
- Movie explaining acetylene formation from calcium carbide and the explosive limits forming fire hazards
- Calcium Carbide & Acetylene at The Periodic Table of Videos (University of Nottingham)
- CDC - NIOSH Pocket Guide to Chemical Hazards - Acetylene
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English Journal
- Differential role of Snail1 and Snail2 zinc fingers in E-cadherin repression and Epithelial to Mesenchymal Transition.
- Villarejo A, Cortes-Cabrera A, Molina-Ortiz P, Portillo F, Cano A.SourceUniversidad Autonoma de Madrid (UAM); Instituto de Investigaciones Biome, Spain;
- The Journal of biological chemistry.J Biol Chem.2013 Dec 1. [Epub ahead of print]
- Snail1 (Snail) and Snail2 (Slug) are transcription factors that share a similar DNA binding structure of four and five C2H2 zinc finger motifs (ZF), respectively. Both factors bind specifically to a subset of E-box motifs (E2-box: CAGGTG/CACCTG) in target promoters like the E-cadherin promoter and a
- PMID 24297167
- Case of the missing isomer: pathways for molecular elimination in the photoinduced decomposition of 1,1-dibromoethane.
- Kalume A, George L, Cunningham N, Reid SA.SourceDepartment of Chemistry, Marquette University , Milwaukee, Wisconsin 53201-1881, United States.
- The journal of physical chemistry. A.J Phys Chem A.2013 Nov 21;117(46):11915-23. doi: 10.1021/jp403114s. Epub 2013 Jul 26.
- We report an experimental and computational study of the photodecomposition pathways of a prototypical gem-dihalide, 1,1-dibromoethane (1,1-EDB), in the condensed phase. Following photolysis of the matrix isolated parent compound in Ar at 5 K, photoproducts are observed corresponding to Br2 eliminat
- PMID 23848935
- DNA Recognition of 5-Carboxylcytosine by a Zfp57 Mutant at an Atomic Resolution of 0.97 Å
- Liu Y, Olanrewaju YO, Zhang X, Cheng X.SourceDepartment of Biochemistry, Emory University School of Medicine , 1510 Clifton Road, Atlanta, Georgia 30322, United States.
- Biochemistry.Biochemistry.2013 Nov 20. [Epub ahead of print]
- The Zfp57 gene encodes a KRAB (Krüppel-associated box) domain-containing C2H2 zinc finger transcription factor that is expressed in early development. Zfp57 protein recognizes methylated CpG dinucleotide within GCGGCA elements at multiple imprinting control regions. In the previously determined str
- PMID 24236546
Japanese Journal
- Study of electron transport in hydrocarbon gases
- Hasegawa H.,Date H.
- Journal of applied physics 117(13), 133302, 2015-04-08
- … The drift velocity and the effective ionization coefficient of electrons in the organic gases, C2H2, C2H4, C2H6, CH3OH, C2H5OH, C6H6, and C6H5CH3, have been measured over relatively wide ranges of density-reduced electric fields (E/N) at room temperature (around 300 K). …
- NAID 120005611267
- Laser-Spectroscopic Measurements of the Free Radicals Produced from the Dissociation of C2H2 with the Microwave Discharge Flow of Ar
- Ito Haruhiko,Tsudome Hiroki
- Transactions of the Materials Research Society of Japan 40(1), 33-36, 2015
- … C2(a3Πu) radicals were produced using the dissociative excitation reaction of C2H2 with the microwave discharge flow of Ar. …
- NAID 130005068867
- UBMS法によるTiCNコーティング工具の難削材切削特性:—カーボン添加方法の影響—
- 嶋村 公二,細川 晃,上田 隆司
- 砥粒加工学会誌 58(4), 241-246, 2014
- … アンバランスドマグネトロンスパッタ法（UBMS法）によるTiCNコーティングエンドミルの作製において，カーボン添加方法（グラファイトスパッタ，CH4ガスおよびC2H2ガス）が膜の機械的性質および構造に及ぼす影響を明らかにするとともに，難削材の一つであるオーステナイト系ステンレス鋼（SUS304）の切削に適用した．いずれのカーボン添加方法においても，カーボン含有量の増加とともに摩擦係数が低下する．また， …
- NAID 130004835708
Related Links
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- These tables give the physical properties of Acetylene (C 2 H 2 ) in the gaseous, supercritical and condensed phases (enthalpy, gas-liquid equilibrium, viscosity, density, flammability, transport properties ...
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| リンク元 | 「acetylene」 |
| 関連記事 | 「C2」 |
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