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Bryan, I note the very close similarity between this acetylene article and the one I put under "Links." This is almost too close for comfort...actually it is too close for comfort.
Perhaps, if the article were developed further, it wouldn't look so much like copyright infringement. --LMS
Not sure what to do with it other than simply rearranging the sentances more and perhaps substituting synonyms; this is pretty close to a simple list of facts, and facts are uncopyrightable. I'll give it a shot, though. -BD
What is the black substance that comes off from the flame and floats away into the air when starting up an oxy-acetelyne torch?
Please correct the following: a liquid does not sublime, by definition. A material can not sublime at its boiling point, again by definition (although there may be exceptions...) The boiling point can not be BELOW the melting point (under the same pressure and temperature).
The completely trivial (sorry, guys) list of side combustion products is unenlightening and certainly incomplete (eg how about NOx compounds and COR or COOR where R is multitude). The opinion that the sweet smell of pure C2H2 is pleasant is not in accord with my experience. The last paragraph is in dire need of rewriting. Its only partially intelligible and has garbled syntax and grammar. One of your links states that polymerization can occur at 15 psig. So which is it? The 1st paragraph has a run on sentence that is one for the books. Is it transported in acetone? If so then why not mention it. Whats the pressure in a tank or a tanker? No mention of toxicity. 400 C is NOT a low temperature for a hydrocarbon (with multiple bonds).
Acetylene can be easily stored in pressurized gas cylinders. What do you think how people weld? They have to tanks oxygen and acetylene. The acetylene is definetely not dissolved in acetone. It is correct that acetylene may explade at 100 kPa pressure (which is 1 atmosphere) but only in the presence of oxygen. It won't do anything on its own. Also the acetylene oxygene flame is one of the hottest burning flame of any hydrocarbon we know
Why does the article claim that the chemical name of the compound is acetylene when it should be ethyne? In alkyne it states that the acetylene is officially known as ethyne which I assume is refering to IUPAC nomenclature.
if you told me acetylene, i never would have thought it would be ethyne! stick to iupac! RaftaReads (talk) 17:07, 23 September 2020 (UTC)[reply]
Why is the compound even called acetylene at all? I see no similarities to the acetyl radical. No methyls, no carbonyls (not even an oxygen atom), nothing.
But the hydrated form is not the educt, which is called acetylene. (??!!) alternatively: acidify ethylene glycol, acetethylene(glycol)--> acet(h)ylene (ethylene glycol --> -H2O --> ethylene oxide/epoxide--> -H2O --> acetylene; epoxide may polymerize, but sulfuric acid can dehydrate the epoxide, I guess)--Smiles :( :\ :o :() (talk) 02:56, 11 April 2015 (UTC)[reply]
History and tradition, most likely some misconception by the person(s) who first discovered or synthesized it.
Look up how hydrocarbon came about from early experimenters calling them 'watered carbons' due to all the hydrogen in them which had to be an indicator of water involved in the processes that create them. Of course the assumptions were wrong but hydrocarbon stuck as the name of that class of compounds.
Here's a free e-book that contains plenty of information on the gas.
http://www.gutenberg.org/etext/7969
I've no idea how old it is, but the text has a "feel" to it that appears to date it to the early 20th century. There's no metric units mentioned and the terms 'Sulphuretted Hydrogen' instead of hydrogen sulphide and 'Phosphoretted Hydrogen' instead of phosphine are definately old terminology. Unfortunatly it's just the text, none of the illustrations are included.
I think we all agree that acetylene is a silly old confusing name- please change it to ethyne
Ethine is most DEFINITLY wrong!
Now in the past women wore corsets and were not allowed to vote! Thankfully we don't all live in the past!! :D
Times are a changing!
Acetylene does not make sense from a chemists Perspective wheras ethyne DOES
Whats the alcohol used to make vodka more than just potatoe water: is it "grain alchohol" or is it ethanol!
Give it a few years mate and you'll let women vote too!
Blonde2max 18:55, 17 June 2006 (UTC)[reply]
Ethyne may be the correct name to chemists, but everyone else calls it acetylene. There are already redirects in place for "ethine" and "ethyne". Just add a sentence in the article that explains the confusion between acetylene and ethyne and be done with it.
Bizzako 2:28, 02 August 2006 (MDT)
IUPAC nomenclature rule A-3.2 notes that
"The name "acetylene" for HC≡CH is retained."
--Spoon! 08:53, 23 December 2006 (UTC)[reply]
I'm absolutely confident that calling ethyne ethyne will not create confusion, or if only perhaps amongst people who just use it for some technical purposes and don't really care about what it actually is. And mind you, ethanoic acid, ethanal, methanal and propanone are the more commonly used forms of names in MODERN chemical literature. Trivial names are more often still used for complex yet common substances, such as toluene, glucose, etc. 129.67.54.6 (talk) 18:46, 20 January 2009 (UTC)[reply]
Ethanal etc are plainly perfectly acceptable, if not the most common forms. Booshank (talk) 19:29, 2 February 2009 (UTC)[reply]
"Oxyacetylene is the hottest burning of all fuel gases." What counts as a fuel gas? There are hotter stuffs: [1]. A whole bunch of poluynes go noncharted in thèrmokemistry. -lysdexia 20:40, 30 September 2006 (UTC)
In the "Uses" section:
"Acetylene has been proposed as a carbon feedstock for molecular manufacturing using nanotechnology. Since it does not occur naturally, using acetylene could limit out-of-control self-replication."
In the "Natural occurrence" section:
"Acetylene is a moderately common chemical in the universe... Natural acetylene..."
How could the two quotes square with each other? Given the second one, the first is conceptually flawed. Shawn D. 16:37, 25 July 2007 (UTC)[reply]
We've been studying reactions in chemistry lately, and yesterday we demonstrated the synthesis and combustion of acetylene. Did I hear my teacher wrong when he said that some acetylene torches can burn underwater? —Preceding unsigned comment added by 71.190.143.208 (talk) 19:32, 25 October 2007 (UTC)[reply]
There was a major fire in Dallas, Texas a few years ago involving an welding company's headquarters. Hundred of tanks blew up, many hit the nearby freeway, nearly hitting cars (one direction of which was closed, the other wasn't). Is there an article for this? If there is, I can't find it. One of the amazing things is no one was killed. --98.232.182.66 (talk) 04:09, 21 September 2008 (UTC)[reply]
The Compression section says "acetylene gas is fundamentally unstable, and will decompose in an exothermic reaction if compressed to any great extent." I can't find anywhere in the article, though, what it becomes when it decomposes. What are the decomposition products? Ian01 (talk) 04:14, 7 October 2008 (UTC)[reply]
I heard a rumor that you have to store and transport acetylene tanks standing up and that if you lay them on their sides they will explode?
I don't use acetylene, but I do use a GTAW welding rig with pressurized argon. My argon tank lays on its side in a cradle under my welding bench.
I think it's safer to have gas tanks lay on their sides and not standing up as they could not tip over if they are already laying on their sides.
I don't want to change the article because I only heard this as a rumor. Is there any cited source that talks about en explosion that is caused by someone laying an acetylene tank on it's side? Allyn (talk) 13:44, 25 July 2009 (UTC)[reply]
It is true that it is recommended to transport and store acetylene tanks in an upright position but not because they will explode it is because of the acetone in them. If acetone gets up to the valve and it can easily when the container is lying down you will have difficulties lighting up the torch. — Preceding unsigned comment added by 212.91.126.148 (talk) 05:59, 20 September 2011 (UTC)[reply]
I grew up with a story, from my father in some sort of chemistry, that the cylinders were acetylene in acetone in bentonite, and that laying down the cylinder would release the acetone from the bentonite and cause uncomfortable amounts of acetylene to come out of solution. I was a kid at the time, so if I've mangled the details, I won't be surprised. ArthurDent006.5 (talk) 07:03, 10 August 2014 (UTC)[reply]
The tanks can be transported on their sides, but that is not recommended procedure. No harm will come to the tank, or acetylene. If they are laid horizontal, they have to be placed upright and left to stand for a period of time ( recommended several hour minimum ) until the acetone is given time to settle. If this does not happen, then the liquid acetone can get into the regulator and hoses, and cause sputtering of the flame, and potentially damage or failure of the equipment, notable the seals. Since acetylene is extremely flammable, a leaking cylinder in an enclosed space can create a violent explosion, frequently with no resulting after fire, as it can tend to blow itself out. — Preceding unsigned comment added by 70.121.157.34 (talk) 04:38, 20 March 2016 (UTC)[reply]
Here's a link to an article that would seem to contradict the information in the Natural occurrence section.
http://www.newscientist.com/article/dn19005-hints-of-life-found-on-saturn-moon.html —Preceding unsigned comment added by SargeWallace (talk • contribs) 13:36, 6 June 2010 (UTC)[reply]
The result of the move request was: Speedy close (no move). No clear rationale provided for move and is contrary to WP:COMMONNAME so speedy close per WP:SNOW. Feel free to propose anew with a potentially persuasive rationale. Born2cycle (talk) 01:03, 15 January 2011 (UTC)[reply]
From section wha? above:
1. Beginning of old comment (added 2005 Oct.1 by numbered editor) Please correct the following: a liquid does not sublime, by definition. A material can not sublime at its boiling point, again by definition (although there may be exceptions...) The boiling point can not be BELOW the melting point (under the same pressure and temperature). Etc.
2. Added today by Marenero:
3. My comment: First, the phase behavior of acetylene is now explained in the article section Physical properties: changes of state. The triple point is at pressure higher than 1 atm, so the liquid can not exist at 1 atm (as for the better known case of CO2). The value given for the melting point is actually the triple point, and the value given for the boiling point is actually the sublimation point at 1 atm, and yes, this is lower than the triple point (again as for CO2).
Since melting point here actually means triple point, the latest value reported in the webbook is actually the 1950 value reported as a triple point, which is 192.4 K. This is close to the webbook values from before 1931, suggesting that the 1931 value is an error. The value in the article before today was actually this 1950 value fron the webbook.
Other more recent sources agree. The Handbook of Chemistry and Physics (60th edn 1979-80, page C-302) lists the melting point of ethyne as -80.8 oC, which is 192.35 K. And the Merck Index (13th edn 2001, p.17) says -81 oC with subl in parentheses. Therefore I suggest we return to the 1950 value. The infobox does note that it is the triple point at 1.27 atm, with more detailed explanation in the Physical properties section. Dirac66 (talk) 01:38, 17 July 2012 (UTC)[reply]
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I'm currently doing an apprenticeship for fabrication and in another fabrication book it notes that Acetylene has a strong garlic smell. would this be the "marked" odour that's mentioned at the beginning of this article? Wiki states that it is odourless in its pure form but has a marked odour commercially due to impurities. — Preceding unsigned comment added by 82.39.201.117 (talk) 08:49, 9 February 2021 (UTC)[reply]
Hello, may you have different references or parameters, but your density is wrong. In the English version it is written 1,097 kg/m^3 (without information about the other parameters) but in the German one (with reference) with 1,1772 kg/m^3 (at standard conditions). Please correct or specify it. [Added 29 April 2021 by editor 2003:f9:872d:f806:a5dd:6a6c:2915:874]
Prior content in this article duplicated one or more previously published sources. The material was copied from: https://www.google.co.uk/books/edition/Practical_Organic_Chemistry/SvhPAAAAYAAJ?hl=en&gbpv=1&bsq=small%20lumps. Copied or closely paraphrased material has been rewritten or removed and must not be restored, unless it is duly released under a compatible license. (For more information, please see "using copyrighted works from others" if you are not the copyright holder of this material, or "donating copyrighted materials" if you are.)
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The Discovery section now says: "By heating potassium carbide with carbon ... [Davy] produced a residue of what is now known as potassium carbide." How can potassium carbide react to form potassium carbide??
This was changed on 2022 January 2 from "By heating potassium carbonate with carbon ..." which at least had a reactant different from the product. However the reaction with carbonate was not very clear either - what happens to the oxygens?? And I cannot make much sense of the references given. Can someone make sense of this reaction and then correct the sentence? Dirac66 (talk) 03:32, 22 January 2022 (UTC)[reply]
From the "Discovery" section: "By heating potassium carbide with carbon at very high temperatures, he produced a residue of what is now known as potassium carbide, (K2C2), which reacted with water to release the new gas."
So he heated potassium carbide and got potassium carbide out of it? What is this sentence supposed to mean?
2A02:8108:96C0:6D08:1816:CC57:5704:15FB (talk) 17:52, 7 February 2022 (UTC)[reply]
Perhaps I'm being dull but I'm not sure what "reduced carbon" is. The article says "oil supplanted coal as the chief source of reduced carbon".
Does it simply mean pure carbon (graphite), or does it mean carbon with a formal charge/oxidation state less than it normally is? In typical molecules such as hydrocarbons, carbon's formal charge tends to be 0. And it doesn't tend to be reduced further in reactions.
I feel that it's possible the editor related isolating pure carbon to isolating pure metals, which do tend to have a reduced oxidation state after the purifying process. But this would be an incorrect analogy.
But I may be missing something here and I haven't found out how to read or translate the cited source, so any insight's appreciated. 35drake (talk) 13:55, 1 February 2023 (UTC)[reply]