| Pages:
1
..
13
14
15
16
17
..
26 |
benzylchloride1
Hazard to Others
Posts: 299
Registered: 16-3-2007
Member Is Offline
Mood: Pushing the envelope of synthetic chemistry in one's basement
|
|
I did not have very good success with the electrolytic preparation of benzaldehyde. I was able to produce several mililiters of benzaldehyde using
this method. I think I will have better luch with the chlorination of the toluene. I put my benzal chloride-benzyl chloride mixture back into the
chlorination apparatus and chlornated the product for another 4.5 hours. After distilling, the product had a density of 1.23 and did not have the
benzyl chloride odor. The product distilled between 180 to 190 Celsius at a pressure of around 580mm.
Amateur NMR spectroscopist
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
Neograviton method seems to work for me and after about 6 hours at about 55 degrees the smell of BnO was strong. Sadly the flask broke when I
attempted to steam it out so I will not be able to get an idea of yeild although I did manage to save quite abit but can not attempt a steam
distilling until I get all the left over toluene and mess cleared up.
Are the yeilds as Neograviton states at 70%?
Im a little confused on the first step where he stated the need for Mn(IV) IIRC would it not need a 2x molar excess of H2SO4 to form the desired salt
instead of the 1:1 he mentions.
Org posted a synthesis from Osmium that stated FeSO4/cupric acetate and sodium persulfate. Im getting ready to run this and was woundering if its
really 95% such as stated. Has anyone had experiance with this method. It seems to be largly ignored when it was posted.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
Klute
International Hazard
Posts: 1378
Registered: 18-10-2006
Location: France
Member Is Offline
Mood: No Mood
|
|
I tried it sevral times without getting any definitate results. There was benzoic acid produced, and unreacted benzyl alcohol, depending on the
reaction time. But it's worth a try IMHO, I did produce a fair amount at the end. Be carefull to heat above 70°C before adding the persulfate, as
there a run-out reaction if you heat to that temp after adding a large amount of persulfate.
\"You can battle with a demon, you can embrace a demon; what the hell can you do with a fucking spiritual computer?\"
-Alice Parr
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
I did manage to get the mess cleaned up and steam some out. What came out from the steam distilling smelled of toluene yet it seems the benzaldahyde
got let behind judging from the smell. It is quite possible that I didnt let it steam long enough but after the accident its not worth my time to
attempt to salvage it.
Hinski posted another means using just Mn(IV) in a electrochemical cell. I think I will proceed in this direction for the time being and keep the
persulfate route just for academics. I have heard of the runaway but did not realise that it was caused by preloading the persulfate so thats good to
know.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
benzylchloride1
Hazard to Others
Posts: 299
Registered: 16-3-2007
Member Is Offline
Mood: Pushing the envelope of synthetic chemistry in one's basement
|
|
Alkyl hypochlorites as reagents for the side chain halogenation of toluene.
Tert butyl hypochlorite is an interesting chlorinating/oxidizing agent. A safe synthesis of this reagent is given in Organic Synthesis Collective
volume 5. Isopropyl hypochlorite can be prepared in a similar method. A US patent describes the chlorination of theyl benzene to
a,a-dichloro-1-phenylethane in high yields. This could be applicable to toluene for the synthesis of benzal chloride and other side chain halogenated
products. This would be significantly better then passing dry chlorine through refluxing toluene for 12 hours for a 1 mole experiment. Here is an
excript from US Patent 5064518 - Method for the selective alpha halogenation of alkylaromatic compounds. Hopefully this is patnet is not totally BS.
Tert butyl hypochlorite is the preferred reagent because of its ability to form radicals, an experiment will be conducted with the more easily
prepared isopropyl hypochlorite. This may considerably simplify the synthesis of benzal chloride for the home chemist.
Preparation of 1,1-dichloroethylbenzene Using t-butyl hypochlorite.
Into a 5-neck 2-liter flask, equipped with thermometer, mechanical stirrer and a pH probe, is placed 1000 mL of an aqueous bleach solution (~5.25%
NaOCl). The flask is placed in an ice bath and cooled to 8° C. and t-butyl alcohol (56.5 mL, 0.59 mole) and glacial acetic acid (34.35 mL) are added
with stirring. The temperature rises to about 15° C. and the pH drops from about 11.3 to about 6.5. Stirring is continued for about five minutes and
then allowed to phase-separate, during which time a yellow oil floats to the surface. Ethylbenzene (36.9 mL, 0.30 mole) is added, stirring resumed and
a 275-watt sun lamp is placed over the flask. The mixture is stirred with illumination for one hour while the temperature is maintained within the
range of 8°-18° C., after which stirring is stopped and the mixture is allowed to phase-separate.
The aqueous phase is extracted with two×100 mL portions of methylene chloride and combined with the organic phase. The combined solvent and organic
phase is then dried over MgSO4 and the solvent is removed by distillation, leaving 52.01 g of oil. G.C. analysis shows that the product is 73.6%
1,1-dichloroethylbenzene, 10.34% 1-chloroethylbenzene and 10.48% acetophenone and some minor impurities.
The following three experiments (Examples 4, 5 and 6) show the use of other solvents in the reaction using t-butyl hypochlorite as the chlorinating
agent.
EXAMPLE 4
Use of Carbon tetrachloride as Solvent
A quantity of t-butyl hypochlorite (7.0 mols, 759.99 g, 775 mL) is chilled to -5° C. in a brine jacketed reaction flask equipped with mechanical
stirrer, light well, thermometer and nitrogen supply. Ethylbenzene (2.0 mole, 213.4 g, 246 mL) in CCl4 (10.4 moles, 1594 g, 1000 mL) is added to the
reactor and the reaction is started by turning on the lamp (incandescent, 25 watt lamp, General Electric model FG648-X). The reaction temperature is
allowed to rise to 10° C. and samples are taken periodically for G.C. analysis. After 4 hours the reaction is complete and the mixture is drained
from the reactor and the t-butanol is stripped using a rotary evaporator which leaves 322.62 g of a colorless oil which is 89.4%
1,1-dichloroethylbenzene by G.C. analysis (82.3% yield).
EXAMPLE 5
Use of Benzene as Solvent
The reaction of Example 4 is repeated except that benzene (11.18 moles, 874 g, 1000 mL) is used in place of carbon tetrachloride. The t-butanol is
removed on a rotary evaporator and there remains 341 g of a colorless oil which is 91.7% 1,1-dichloroethylbenzene by G.C. analysis (89.3% yield).
EXAMPLE 6
Use of t-butyl hypochlorite as Solvent
Ethylbenzene (4.0 mole, 424.68 g, 492 mL) is charged to a brine jacketed reaction flask equipped with a subsurface N2 sparge, light well, thermometer
and condenser. The t-butyl hypochlorite (14.0 mole, 1520 g, 1670 mL) is added to the reactor and the mixture is chilled to -5° C. while sparging with
N2. The same lamp employed in Example 4 is switched on to initiate the reaction which is conveniently held at 0° C. by controlling the lamps' output
with a temperature controller. Samples are taken periodically and analyzed by G.C. analysis. When the reaction is complete (3 hours) the mixture is
drained from the reactor and the t-butanol and excess t-butylhypochlorite is removed on a rotary evaporator, leaving 709.0 g of a clear oil which is
93.2% 1,1-dichloroethylbenzene by G.C. (93% yield).
[Edited on 21-5-2009 by benzylchloride1]
Amateur NMR spectroscopist
|
|
|
Eclectic
National Hazard
Posts: 899
Registered: 14-11-2004
Member Is Offline
Mood: Obsessive
|
|
Regarding isopropyl hypochlorite:
http://www.sciencemadness.org/talk/viewthread.php?tid=1896&a...
"DANGER, Will Robinson!"
|
|
|
S.C. Wack
bibliomaster
Posts: 2419
Registered: 7-5-2004
Location: Cornworld, Central USA
Member Is Offline
Mood: Enhanced
|
|
Regarding t-butyl hypochlorite:
http://www.sciencemadness.org/talk/viewthread.php?tid=1896&a...
|
|
|
benzylchloride1
Hazard to Others
Posts: 299
Registered: 16-3-2007
Member Is Offline
Mood: Pushing the envelope of synthetic chemistry in one's basement
|
|
The isopropyl hypochlorite chlorination of toluene works fairly well, not explosions or violent reactions, keep mixture below 25C at all times with
ice bath, the reaction is very mildly exothermic, the end product had the density of benzyl chloride. A 60W light was used to catalyze the reaction.
Another interesting synthesis of benzaldehyde through benzaldoxime:
Benzaldoxime in practically 100% yield based on NOCl. The nitrosyl chloride could be generated insitu by passing anhydrous HCl into a mixture of
toluene and isopropyl nitrite. The oxime can be hydrolyzed with hydrochloric acid to benzaldehyde and hydroxylamine hydrochloride.
THE REACTION OF NITROSYL CHLORIDE ON TOLUENE
BY E. V. LYNN AND HELEN I,. ARKLEY
Received January 19,1923
Some time ago one of us found' that nitrosyl chloride will readily react
with normal heptane in the sunlight to produce a blue material which
easily changes to a colorless oil. The blue compound was later shown2
to be nitroso-dipropylmethane and the rearranged oil, dipropyl-ketone
oxime. It was also demonstrated that this reaction is probably general
for all of the paraffin hydrocarbons, a conclusion reached mainly because
gasoline and petroleum ether give a similar blue color with nitrosyl
chloride.
In experimenting with various substances, it was found that benzene
could not be induced to react at all with the reagent, even in sunlight;
a sample of benzene solution was kept for months without any change in
the brown color of the nitrosyl chloride. In view of this fact, paraffin
derivatives of benzene should react in such a way that only the alkyl
radical is attacked. Toluene, the simplest alkyl drivative, should give,
according to previous experience, phenylnitrosomethane rearranging to
benzaldoxime. CsH5-CHs + NOCl ---j CeHb-CH2-N0 f HC1.
CBHS-CH~---NO --3 C6Hb-cH = N-OH. Experiment has fully
demonstrated the correctness of this reasoning, as toluene reacts readily
in the sunlight with nitrosyl chloride producing benzaldoxime, which has
been converted to benzaldehyde, benzoic acid and benzanilide in the usual
way.
Experimental Part
The nitrosyl chloride was prepared as previously described2 by the reaction
of nitrosyl sulfate and sodium chloride. The toluene was first dried
over sodium hydroxide and then distilled, the portion boiling between 110 '
and 112' being used. This was saturated with the gas, giving a dark
red-brown liquid. In the dark at room temperature there was practically
no change in the appearance, but after some time a heavy, insoluble oil
and some gas were formed. In the sunlight the reaction was quite rapid,
producing large quantities of gas, mostly hydrogen chloride, and an amount
of the heavy oil equal to about 3% of the toluene used. In later experiments
the saturated solution was exposed to the sunlight at temperatures
below 10'. In these cases the reaction proceeded somewhat more slowly
and, in place of the oil, there were deposited beautiful, white, iridescent,
feathery crystals. In all experiments the color of the solution disappeared
with the formation of the precipitate. There was, however, no intermediate
production of a blue color and one can only conclude that phenylnitrosomethane
is very unstable.
In subsequent changes the oil and crystals acted alike and, since it was
just as easy to produce the latter and more convenient to work with them,
they were employed in the reactions recorded below. The crystals had an
indefinite melting point, from 35" to 70". They were dissolved in sodium
carbonate solution and extracted with ether, evaporation of the latter
leaving characteristic crystals of P-benzaldoxime, melting at 128 '. The
primary product was, therefore, undoubtedly a mixture of the hydrochlorides
of both benzaldoximes, since the above procedure transforms the
QC to the 0 form. Hydrolysis of the oxime with dil. acid gave an oil identified
by its odor as benzaldehyde. It was oxidized by nitric acid and the
resulting benzoic acid was precipitated on cooling, and melted at 118". It
was further identified by converting to its ferric salt and to benzanilide,
m. p. 158'.
The amount of benzaldoxime crystals obtained is practically that calculated
based upon the nitrosyl chloride used, about 3% by weight of the
toluene. The time required is dependent upon the temperature and upon
the intensity of the sunlight but in no case was it longer than 2 hours.
Under the right conditions the reaction could undoubtedly be made to
proceed more rapidly and probably continuously. Whether the process
can be utilized commercially under the influence of some catalyst is a
problem which is at present engaging our attention. Furthermore, we are
studying the action of nitrosyl chloride on other substances and will report
the results later.
Summary
Nitrosyl chloride readily reacts with toluene in the sunlight to produce
crystals of benzaldoxime hydrochloride, from which benzaldoxime, benzaldehyde,
benzoic acid and benzanilide can be prepared in the usual way.
Amateur NMR spectroscopist
|
|
|
497
National Hazard
Posts: 778
Registered: 6-10-2007
Member Is Offline
Mood: HSbF6
|
|
Does anyone know how well the above stated reaction would work with substituted toluenes?
For example, how does it treat alkoxy substitutions?
|
|
|
DyD
Harmless
Posts: 4
Registered: 26-3-2009
Member Is Offline
Mood: No Mood
|
|
Wow. Has nobody mentioned the "Etard" reaction?
It appears that Chromyl Chloride [Cr(VI)O2Cl2] is excellent at partially oxidizing toluene to benzaldehyde.
While I haven't prepared benzaldehyde from toluene yet, I've successfully prepared chromyl chloride from Chromium(III) oxide via the below process:
--------------------
2 KMnO4 + Cr2O3 + 2 H2SO4 → H2Cr2O7 + 2 KHSO4 + 2MnO2
H2Cr2O7 + 4 KCl + 4 H2SO4 → 2 CrO2Cl2 + 4 KHSO4 + 3 H2O
Overall:
2 KMnO4 + Cr2O3 + 4 KCl + 6 H2SO4 → 2 CrO2Cl2 + 6 KHSO4 + 2 MnO2 + 3 H2O
--------------------
While gaseous hexavalent chromium sounds like a sure-fire recipie for lung cancer, the fumes are dense enough that I feel the risk to be within the
realm of reason.
What do you all think? I'm going to try it in the next few weeks and I'll post back with an update. Feel free to PM me with questions or comments.
|
|
|
Polverone
Now celebrating 21 years of madness
Posts: 3186
Registered: 19-5-2002
Location: The Sunny Pacific Northwest
Member Is Offline
Mood: Waiting for spring
|
|
There's considerable good reading material about this reaction in older publications. Main problems with Etard are hexavalent chromium health hazards,
expense of the reagents, violence of the initial reaction, and needing to take careful measures to protect the liberated aldehyde from further
oxidation at the end. I will look forward to the results of your experiments.
What form was your Cr2O3 initially in? Was it pottery-grade or something more reactive? Woelen reported not long ago that acid bromate solution would
dissolve pottery Cr2O3, which was something of a surprise, since usually it takes high-temperature alkaline-oxidative fusion to get to Cr(VI) from
such material. I am curious if the use of KMnO4 was inspired by his posts, derived from some other reference, or discovered independently by you.
PGP Key and corresponding e-mail address
|
|
|
DyD
Harmless
Posts: 4
Registered: 26-3-2009
Member Is Offline
Mood: No Mood
|
|
I procured the Cr2O3 from the greenish ash left over from the ammonium dichromate volcano demo performed by an old chemistry teacher for a 101 class.
I washed it with a dilute acid-peroxide solution to neutralize any residual hexavalent chromium and allowed it to dry. I then packed it into glass
vials for future use. Now I'm very happy I did so. 
The KMnO4-acid discovery was determined entirely by myself. The inspiration came after remarking to a friend that Mn2O7 could oxidize "damn near
anything."
In addition, I added some of the liquid formed by:
2 KMnO4 + Cr2O3 + 2 H2SO4 → H2Cr2O7 + 2 KHSO4 + 2MnO2
to water and observed an orange solution with brown precipitate, precisely as expected.
|
|
|
UnintentionalChaos
International Hazard
Posts: 1454
Registered: 9-12-2006
Location: Mars
Member Is Offline
Mood: Nucleophilic
|
|
This covers substituted toluenes, but is helpful at any rate for reaction conditions.
You're welcome 
Attachment: Etard Reaction.pdf (221kB)
This file has been downloaded 3130 times
[Edited on 6-29-09 by UnintentionalChaos]
Department of Redundancy Department - Now with paperwork!
'In organic synthesis, we call decomposition products "crap", however this is not a IUPAC approved nomenclature.' -Nicodem
|
|
|
entropy51
Gone, but not forgotten
Posts: 1612
Registered: 30-5-2009
Member Is Offline
Mood: Fissile
|
|
Thanks for the article, UnintentionalChaos. The preps in the article specify CCl4. Has anyone ever run this reaction in CH2Cl2?
[Edit] By that I meant actual experience, not theorizing. Adding chromyl chloride to neat toluene will result in a fire, if you're lucky.
[Edited on 30-6-2009 by entropy51]
|
|
|
DJF90
International Hazard
Posts: 2266
Registered: 15-12-2007
Location: At the bench
Member Is Offline
Mood: No Mood
|
|
CS2 and CHCl3 are also listed as alternative solvents. CHCl3 has the trouble of forming emulsions apparently, so CH2Cl2 might also suffer from this
drawback. Adding chromyl chloride dropwise to excess toluene may work, but care should be exercised when trying this as the reaction may be too
exothermic with neat liquid reactants.
|
|
|
Rattata2
Harmless
Posts: 35
Registered: 22-6-2009
Member Is Offline
Mood: No Mood
|
|
The way I thought to do it was to slowly add bromine to an excess of toluene, forming benzyl bromide. This would be separated from any remaining
toluene and hydroxylated with NaOH to form benzyl alcohol and NaBr. The salt is separated from the alcohol and recycled, while the benzyl alcohol is
then mixed with DMSO and HCl or HBr solution is added - producing benzaldehyde and dimethyl sulfate.
Bromine can of course be made by acidifying NaBr followed by simple oxidation with 3% H2O2. Since it is a liquid at feasible temperatures this would
ease the halogenation of the toluene. Since adding NaOH reforms the NaBr, it can be recycled.
acid-catalyzed DMSO can oxidize benzyl alcohol (and similar compounds) to benzaldehyde with as high as 95% yield!
|
|
|
Nicodem
Super Moderator
Posts: 4230
Registered: 28-12-2004
Member Is Offline
Mood: No Mood
|
|
When someone claims such unusual things, like that slowly adding bromine to an excess of toluene, forms benzyl bromide, or that oxidation of benzyl
alcohol with DMSO gives dimethyl sulfate besides benzaldehyde, it is expected that some references are provided.
Why would we believe you just for your word? It is experimentally known that bromine reacts only very slowly with toluene at room temperature, and
even this via the electrophilic aromatic substitution, thus giving a mixture of o- and p-bromotoluene. Essentially no benzyl bromide is formed unless
you use conditions for radical brominations (that is, radical initiators or photochemically). Also, the oxidation of benzyl alcohol with DMSO means
that DMSO is getting reduced (basic rule of redox reactions is that the oxidant gets reduced and reductor oxidized). Dimethyl sulfate is in a higher
oxidation state than DMSO, so how could it be the product of the reaction? The next sulfur lower oxidation state product forms, that is dimethyl
sulfide, as is known experimentally.
PS: You would know all these things if you would just bother to read and cite references.
|
|
|
JohnWW
International Hazard
Posts: 2849
Registered: 27-7-2004
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
DMSO (of which I have about a 500 ml bottle) would be reduced to dimethyl sulfide, which being a mercaptan would have an intense garlic odor. Also,
being highly volatile, it would probably be toxic like H2S.
|
|
|
Rattata2
Harmless
Posts: 35
Registered: 22-6-2009
Member Is Offline
Mood: No Mood
|
|
Benzyl halides are commonly made by free-radical halogenation of toluene - the same process is used to produce the chloride as is the bromide, only
bromide would probably be loads easier since it is liquid at room temperature. Using 2x the molar ratio results in the benzal halides. Given that it
was such common info I didn't see a reason to hunt down a reference for it.
http://www.erowid.org/archive/rhodium/chemistry/alcohol2alde... this describes the oxidation of benzyl alcohols to benzaldehydes using DMSO and
HBr.
OHH I did mean sulfide - totally didn't mean to type sulfate - told myself over and over not to make that typo My bad haha.
[Edited on 13-9-2009 by Rattata2]
|
|
|
Nicodem
Super Moderator
Posts: 4230
Registered: 28-12-2004
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by Rattata2  | | Benzyl halides are commonly made by free-radical halogenation of toluene - the same process is used to produce the chloride as is the bromide, only
bromide would probably be loads easier since it is liquid at room temperature. Using 2x the molar ratio results in the benzal halides. Given that it
was such common info I didn't see a reason to hunt down a reference for it. |
Using this as an example, I will try to explain in just few words why it is so important to give references and cite sources. If you would have
provided a reference for benzylic bromination of toluene, there would have (statistically) been more chances that you would had also read it, and if
you would have read it, you would have also read the experimental conditions. This would have given you the knowledge that just adding bromine to
toluene does not form benzyl bromide. Instead, you did the classical beginners mistake who seeing a reaction scheme jumps at the conclusion that you
just add this to that and out comes the product. The reaction of bromine with toluene can either proceed via electrophilic aromatic bromination or via
radical bromination, both requiring different conditions, but none proceeds to any usable extent by just "slowly adding bromine to toluene".
But why? What is the point of reacting benzyl bromide with a hydroxide (which, by the way, gives a mixture of benzyl alcohol and dibenzyl ether) just
to then oxidise the benzyl alcohol with DMSO? It sounds completely irrational when you can oxidise benzyl bromide with DMSO directly using the
Kornblum oxidation. (And this is another example of lack of reference checking. If you would have checked the references from the paper you linked to
you would have read the reference number 3 and 4 as well).
…there is a human touch of the cultist “believer” in every theorist that he must struggle against as being
unworthy of the scientist. Some of the greatest men of science have publicly repudiated a theory which earlier they hotly defended. In this lies their
scientific temper, not in the scientific defense of the theory. - Weston La Barre (Ghost Dance, 1972)
Read the The ScienceMadness Guidelines!
|
|
|
DJF90
International Hazard
Posts: 2266
Registered: 15-12-2007
Location: At the bench
Member Is Offline
Mood: No Mood
|
|
Ratatta2: Listen to Nicodem - he makes very valid points.
JohnWW: I actually had the "pleasure" of smelling DMS as a solution in DCM. It was very cabbage like (not garlic as you describe) and rather strong
smelling, although not as strong as I had anticipated (possibly due to it being in solution?). It was actually *quite nice* once the majority of the
smell had gone, leaving a faint odour in the room.
|
|
|
ketel-one
Hazard to Self
Posts: 55
Registered: 8-9-2009
Location: Pluto (planet?)
Member Is Offline
Mood: No Mood
|
|
toluene + Ca(OCl)2 @105C with no other reagents should make benzyl chloride...
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
Prove it.
Book learning is all fine and well but unless your Ca(OCl)2 is pure you will run out of room. Not to mention the ugly runaway leading to over heating.
Oh yeh did I mention the product of all that hassle was junk? Im sorry but I toyed with that method and wasted alot of toluene to accomplish nothing
useful and it caused my eyes to feel as though sand is in them. You will get a mixture of products doing it that way as well so there are other more
focused ways one could go about its synthesis.
Check out Lens threed on the topic in prepublications. You can't beat that kind of excelent work that was performed in that writeup.
BTW: The worst part of the synthesis using the hypochlorite is the runaways. This could be due to my dirty Ca(OCl)2 but either way I think this sucks.
I want so bad to try it once more because I hate like hell when a synthesis kicks my ass but I think I know when Im beat and wasting my time.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
ketel-one
Hazard to Self
Posts: 55
Registered: 8-9-2009
Location: Pluto (planet?)
Member Is Offline
Mood: No Mood
|
|
Ive never tried it, but the stuff on this site should be pretty accurate. http://www.erowid.org/archive/rhodium/chemistry/benzylchlori...
"Toluene and dry Calcium Hypochlorite (bleaching powder) are heated together to 105°C in the abscence of other reagents. This avoids by-product
formation. If equal amtounts are used, volume-wise, there is a high conversion. If more bleaching powder is used, the conversion is more robust, but
contaminants such as benzal chloride and benzotrichloride are formed [...]"
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
"there is a high conversion"
Yup that explains the itchy eyes. But the contamination is to much of a pain when there are better means that even I am able to perform. Anyone with
good gear should be able to perform other synthesis with ease instead of dicking with this. The part where is says avoids biproduct formation is a
load of shit BTW and they dont mention the fact that when it hits 105-110 it runs away to extreamly high temps. You see them little [...] there? Thats
the main problem with rhodiums archives is that it does not give the full details and don't mention what the original text states of SLOWLY adding the
Ca(OCl)2 in portions. If you can site rhodiums articals then its better to look for the references at the bottom and take the writeup with a grain of
salt. I love the fact he put this all out there but care must be taken. Its just bad form to not cross reference your sources.
[Edited on 16-9-2009 by Sedit]
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
| Pages:
1
..
13
14
15
16
17
..
26 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
