HDTenEightyP/NetNews huggingface dataset:
From: berger@atropa (Mike Berger)
Subject: Re: Sparking grapes
Organization: University of Illinois at Urbana
Date: Tue, 18 Aug 1992 19:02:32 GMT

bresler@casbah.acns.nwu.edu (Leo Bresler) writes:
>I have no explanation of this, but I conducted similar experiment with grapes.
>If you place whole grape(with seads) into a microwave, it stats shooting with
>seads.

>I suspect it has some electro-magnetic nature. Microwave probably induces
>circular current inside the grape, which makes it to speat the seeds out.

>It's definitely interesting to here the expert's opinion.
*----
More likely the seed heats up, the water inside turns to steam, the
seed breaks open somewhere, and the steam shoots it out the grape.

Most grapes are not electromagnetic in nature.
--
	Mike Berger
	Department of Statistics, University of Illinois
	AT&TNET     217-244-6067
	Internet    berger@atropa.stat.uiuc.edu
Newsgroups: sci.chem
From: mes10@po.CWRU.Edu (Mark E. Smith)
Subject: Re: Do you know how to produce STYROFOAM?
Reply-To: mes10@po.CWRU.Edu (Mark E. Smith)
Organization: Case Western Reserve University, Cleveland, OH (USA)
Date: Wed, 19 Aug 92 11:16:57 GMT


In a previous article, cabrales@vaxb.acs.unt.edu () says:

>Hi my name is Jose Cabrales. I am a 5th grade teacher. I would
>be very grateful if somebody from this group give me the information
>about the procedure of how to produce STYROFOAM in front of the students.
>I will also appreciate if you include in your information:
>1) Complete description of the procedure (Chemical reactives, quantities,etc)
>2) Safety measures
>Your prompt reply wiill be appreciated
>Jose'
>-- 
>________________________________________________________________________________
> Jose  Cabrales M           | HAMLET's pessimism:
> 			    |"How weary, stale, flat and unprofitable
>UNT Station P. O. Box 6559  |Seem to me all the uses  of this world!
>DENTON TX76203,USA	    |Fie on't, ah, fie, 'tis an unweeded garden
>Ph (817)565-1663	    |That grows to seed. Things rank and gross in nature
>			    |Posses it merely (I, ii). W. Shakespeare
>_______________________________________________________________________________
>

I fully agree with the comments presented thus far by the others.  Not a good
choice for a classroom demonstration.  I would suggest you create nylon
much easier and safer for your purpose.

~Smith
Newsgroups: sci.chem
From: lasseo@LINK.Physchem.KTH.SE (Lars \hrstr|m)
Subject: Re: "White" Carbon?  O4?
Reply-To: lasseo@LINK.Physchem.KTH.SE
Organization: Royal Institute of Technology, Stockholm
Date: Thu, 13 Aug 1992 18:39:00 GMT


White carbon, = Chaoite , yes
O4, no
According to Greenwood & Earnshaw, "Chemistry of the Elements", Pergamon, 1984

Lars Ohrstrom,
Dept. Inorg. Chem.
KTH
Stockholm, Sweden

Newsgroups: sci.chem
From: branham@binah.cc.brandeis.edu (Tom Branham, Biophysics Grad. Brandeis)
Subject: Re: the TRUTH about Methylene Chloride
Reply-To: branham@binah.cc.brandeis.edu
Organization: Brandeis University
Date: Fri, 21 Aug 1992 03:53:15 GMT

NOW I feel upto date on the question!  Thank You....
                            .Tom Branham
From: moroney@ramblr.enet.dec.com
Subject: Re: converting gypsum into sheetrock
Organization: Digital Equipment Corporation
Date: Tue, 18 Aug 1992 04:17:30 GMT

In article <9208162018.AA27888@lago>, krm@sdc.boeing.com (Keith Michaels) writes...
>I recently saw on "This Old House" a factory tour of a sheetrock factory.
>The process decribed was very simple: the gypsum is mined in an open pit,
>crushed, mixed with water, and formed continuously into sheets.
>The reaction is obviously exothermic, as the soft sheetrock is warm to 
>the touch.
> 
>What prevents this reaction from occurring when rain falls on the exposed
>gypsum in the pit?  If the reaction is just a hydration of CaSO4, why isn't
>it reversable?  There must be more to it than what was shown.

Gypsum is CaSO4.2H2O, and is the most hydrated form of Calcium Sulfate.
When gypsum is heated to 130 C it starts giving off water, forming 
the hemihydrate 2(CaSO4).H2O, better known as Plaster of Paris.

When Plaster of Paris is heated to 165C it starts to lose the rest of the water
forming "soluable anhydrite".  Both forms react exothermically with water,
reforming gypsum if enough is available.

If "soluable anhydrite" is heated above 300-400 C it changes so it reacts
only slowly with water, this form is the same as the mineral anhydrite.

I suspect they omitted showing a step where gypsum was baked forming
Plaster of Paris, before the water was (re)added forming gypsum wallboard.

The gypsum in the mine doesn't react because it's already fully hydrated.

-Mike
From: rmede@waikato.ac.nz
Newsgroups: sci.chem
Subject: MacroModel vs HyperChem?
Date: 21 Aug 92 09:38:10 +1200
Organization: University of Waikato, Hamilton, New Zealand

I am currently setting up a molecular modelling project based around a
Silicon Graphics IRIS Indigo, with the main application of the project
being conformational modelling of small-medium sized organic compounds.

As far as I am aware, MacroModel would be a pretty good bet for software,
but there is the recently released HyperChem from AutoCad that seems to
offer similar  features to MacroModel. Does anyone have any comment
(posted or E-mailed is OK) to make about the relative performance of
either software package?

Any comments/advice would be appreciated.

Rick Ede
Lecturer in Organic Chemistry
University of Waikato
Hamilton, New Zealand
rmede@waikato.ac.nz
Newsgroups: sci.chem
From: James Petts <pettsj@visigoth.demon.co.uk>
Subject: Re: "White" Carbon?  O4?
Organization: No Affiliation
Date: Thu, 13 Aug 1992 06:58:26 GMT
X-Useragent: Nuntius v1.1



In article <1992Aug13.014729.10991@engage.pko.dec.com> ,
moroney@ramblr.enet.dec.com writes:
>The CRC Handbook, in their section on the elements describes an
allotrope of
>carbon as "white" carbon, in addition to diamond and graphite
allotropes. They
>devote a couple sentences to it and state that not much is known about
it.
>Does this have anything to do with 'buckyballs'? They do not mention
them, even
>in the latest edition.  Does anyone know anything about 'white' carbon
beyond
>what's listed in the CRC?
>
>Also an old (1950s) encyclopedia lists, in addition to O2 and ozone O3,
a form
>of oxygen as O4, an unstable bluish nonmagnetic substance that readily
>decomposed to O2.  I have never seen any other reference to this.  Does
O4
>really exist?

I suggest you look up a reference book (ca 1985, I believe) called "The 
Elements" (catchy title, huh?) by Greenwood and A.N. Other. Most college 
libraries should have it. I'll try and look it up when I get the chance, 
but this is the book I would use anyway.

James

***********************************************************************
***
*    "We use the classical theory on Mondays, Wednesdays and Fridays,    
*   
*     and the quantum theory on Tuesdays, Thursdays and Saturdays."      
*
***************************************** Wm. Bragg
***********************
Newsgroups: sci.chem
From: James Petts <pettsj@visigoth.demon.co.uk>
Subject: re: Toxic Waste
Organization: No Affiliation
Date: Mon, 17 Aug 1992 07:11:05 GMT
X-Useragent: Nuntius v1.1



In article <1635@grivel.une.edu.au> Matthew GRAY, mgray1@metz.une.edu.au
writes:
>Along with carbon tet. and chloroform, dichloromethane is on the list of 
>solvents on the 'ozone list' of chemicals to be phased out of use by the
>year x(?).

Intersting point, which I have speculated upon for some time:
Carbon tet gets replaced by chloroform, chloroform by methylene
chloride. When do we start using methyl chloride???
(For those who have never come across it, MeCl is a *very* nasty
corrosive,
explosive gas)

James Petts
********************************************************************
* "We use the classical theory on Mondays, Wednesdays and Fridays, *   
*  and the quantum theory on Tuesdays, Thursdays and Saturdays."   *
************************************** Wm. Bragg *******************
Newsgroups: sci.chem
From: vsummers@polaris.cv.nrao.edu (Vince Summers)
Subject: Re: the TRUTH about Methylene Chloride
Organization: National Radio Astronomy Observatory
Date: Tue, 18 Aug 1992 13:16:18 GMT

     Very good to discourage bad info, but what info was presented that was
bad?

Vince Summers
vsummers@polaris.cv.nrao.edu
Newsgroups: sci.chem
From: ahahma@polaris.utu.fi (Arno Hahma)
Subject: Re: Let's have a laugh
Keywords: N2O nitrous oxide dinitrogen monoxide 
Organization: University of Turku
Date: Thu, 13 Aug 92 13:13:29 GMT

In article <1992Aug4.121705.14284@morgan.ucs.mun.ca> fsmith@morgan.ucs.mun.ca (Frank Smith) writes:

>Back when I was a student I learned that nitrous oxide can be made by gentle
>heating of ammonium nitrate. You also get water vapour produced as well, so
>this would have to be removed by cold trapping before you would get fairly
>pure N2O. There should not be any other oxides of nitrogen present but if
>there is any ammonium nitrite this will decompose to nitrogen gas.

That is true. However, heating pure ammonium nitrate will lead to
several kinds of decomposition and other oxides of nitrogen are
formed, although in small amounts. Others have already pointed out
that the other oxides of nitrogen are poisonous.

A better alternative is to add some water (a couple of per cent of the
weight of the ammonium nitrate) and a phosphate, say calcium
phosphate. Any phosphates will catalyze the decomposition greatly and
it will take place a few ten centigrades lower than without the
phosphate. The water is required to make the reacting mixture liquid
at a lower temperature at the start thus getting the catalyst and the
ammonium nitrate into a better contact. 

They also make N2O industrially by heating ammonium nitrate with a
phosphate catalyst. The resulting N2O will be considerably purer than
that obtained from pure AN.

>Beware that ammonium nitrate is an explosive so small quantities and gentle
>heating are imperative.

Ammonium nitrate requires a strong detonator to be detonated as such.
As a mixture with organic fuels, it requires less strong a detonator,
a few grams of a high explosive may be enough.

Alternatively, extremely large amounts of ammonium nitrate
contaminated with organic impurities may explode, if set to fire.
Extremely large amounts here means tens of tons or more. So, ammonium
nitrate is pretty safe to handle and heat in a laboratory scale.

ArNO
    2
From: tgcpwd@rw6.urc.tue.nl (Wim van Dorst)
Newsgroups: sci.chem
Subject: Re: Common ingredients info
Date: 20 Aug 92 13:26:54 GMT
Reply-To: tgcpwd@urc.tue.nl
Organization: Eindhoven University of Technology, The Netherlands

JEFF HOYLE writes:
>ANother really good source for this type of info is:
>
>Chemistry in the Marketplace by Ben Selinger, pblished in NAmerica by 
>Harcourt, Brace and Jovanovich.  Hope that helps

I second this suggestion. I recently bought this book specifically because
it explains in plain English what all these chemical things in my shampoo/
cleaners/food/... are. 

Ben Selinger (from Oz by the way) is highly recommended to all people
in sci.chem. He gives a really sound basis of the chemistry (and chemicals) 
involved in normal life. 

Met vriendelijke groeten Wim `Blue Baron' van Dorst
From: mtp@oregon.uoregon.edu (Matthias Pohl)
Newsgroups: sci.chem
Subject: Re: CLENBUTEROL?
Date: 21 Aug 92 16:17:50 GMT
Article-I.D.: nntp.1992Aug21.161750.21669
Organization: Dep. of Chemistry


> One of the athletics stars of the former GDR, Katrin Krabbe, will probably
> be suspended for four years for taking Clenbuterol.  And though it is
> technically incorrect to use the term 'steroid', I don't thinks it's
> any better then that.  And it certainly has nothing in common with
> vitamins.
> 
> -- Thomas Richter

I am not sure about the situation in Europe. But here in the US Clenbut-
erol is a non-prescription drug and is commonly available at mail order
places that cater to the body-building community, selling nutritional
supplements (sic!) :). For all of you interested in the physiological
aspects of Clenbuterol: about two or three weeks back there was a disc-
ussion about it in newsgroup MISC.FITNESS .

Matthias
From: btcl_ltd@creb.cc.rochester.edu (Brian)
Newsgroups: sci.chem
Subject: Contact lenses in lab (Was: Re: Security In Laboratory..??)
Date: 15 Aug 92 18:25:39 GMT
Organization: University of Rochester - Rochester, New York

In <10AUG199217070463@vtcc1.cc.vt.edu> merolajs@vtcc1.cc.vt.edu (JOSEPH S. MEROLA DEPT OF CHEMISTRY VPI&SU) writes:

>     Soft contact lenses are made of a polymer swelled with saline and
>fitted over the eye.  If you wear contact lenses in a laboratory 
>environment over a period of time, there is a high likelihood that
>solvent vapors will gradually be absorbed and accumulate in the lens.
>This could result in, at best, eye irritation and, at worst, sever 
>eye damage.  

>Joseph S. Merola
>Department of Chemistry
>Virginia Tech (aka VPI&SU)


Does anyone know if the same holds true for hard (rigid gas permeable) contact
lenses? These don't seem to be mentioned as often soft lenses. I'm interested
because I wear hard lenses (outside of the lab, of course).

Brian Connell
btcl_ltd@uhura.cc.rochester.edu


--


******************************************************************************
*Brian Connell                   	           University Of Rochester   *
Newsgroups: sci.chem
From: cs_jh@cox.nsac.ns.ca (JEFF HOYLE)
Subject: airbags how do they work? Chemistry??
Organization: Nova Scotia AC
Date: Fri, 14 Aug 1992 15:31:32 GMT

Some time ago I posted a request for info concerning the chemistry involved 
in air bag inflation.  I did not get any useful responses.  Is there any one 
out there who either knows and can explain the process or who has a leading 
reference to this subject.

In advance, thanks for all info....

Jeff
  ***********************************************************
  * Dr Jeff Hoyle (Organic Chemist)                         *
  * Chemistry and Soil Science Department                   *
  * Nova Scotia Agricultural College    FAX: (902)-895-4547 *                     *
  * P.O. Box 550, TRURO,              Voice: (902)-893-6630 *
  * Nova Scotia. CANADA  B2N  5E3                           *  
  *                  -----------------                      * 
  * Internet: cs_jh@cox.nsac.ns.ca  OR  jh_cs@ac.nsac.ns.ca *
  ***********************************************************
Newsgroups: sci.chem
Newsgroups: sci.chem
Subject: MO programs - ftp sites?
From: chemmail@otago.ac.nz
Date: 13 Aug 92 17:52:03 +1300
Organization: University of Otago, Dunedin, New Zealand

Could someone please post a list of ftp sites where I can find MO
calculation programs? 

Thanks

Allan                        
                     Allan Blackman
                     Department of Chemistry
                     University of Otago
                     Dunedin, New Zealand
From: dadmun@maple.circa.ufl.edu
Newsgroups: sci.chem
Subject: Methylene Chloride
Date: 17 Aug 92 12:03:02 GMT
Reply-To: dadmun@maple.circa.ufl.edu
Organization: University of Florida - CIRCA

Methylene Chloride is surely not something you want washing up on
our beaches.  Even us chemists should use gloves when handling it.
It is a popular solvent which has nasty side effects - since I don't
have a bottle here by the computer, I think it is a liver toxin.  At
any rate, it does effect some important organ in the body, and that 
is not what we want floating in the ocean.  The stuff does evaporate
rather quickly, so if you were close to it don't worry too much -
I would say you, your wife and baby are safe, but don't be satisfied
with that.  Make sure that something is being done about it...
Andrew Dadmun
dadmun@ufcc.ufl.edu
From: odriscod@topaz.ucq.edu.au
Newsgroups: sci.chem
Subject: Re: Common ingredients info
Date: 21 Aug 92 14:55:31 AET
Organization: University of Central Queensland, Australia

In article <5127@tuegate.tue.nl>, tgcpwd@rw6.urc.tue.nl (Wim van Dorst) writes:
> JEFF HOYLE writes:
>>ANother really good source for this type of info is:
>>
>>Chemistry in the Marketplace by Ben Selinger, pblished in NAmerica by 
>>Harcourt, Brace and Jovanovich.  Hope that helps
> 
> I second this suggestion. I recently bought this book specifically because
> it explains in plain English what all these chemical things in my shampoo/
> cleaners/food/... are. 
> 
> Ben Selinger (from Oz by the way) is highly recommended to all people
> in sci.chem. He gives a really sound basis of the chemistry (and chemicals) 
> involved in normal life. 
> 
> Met vriendelijke groeten Wim `Blue Baron' van Dorst

A message from Australia

The book is very good, I recommend it to all my none chemist
friends who ask..."Dave's what's in my shampoo and why does it
stuff my hair...??".

Top Stuff...If you've got the money buy it...No I don't know the 
author personally nor do I hold shares in his printing company....

David O'Driscoll
University of Central Queensland
Australia....The only place to LIVE..

Newsgroups: sci.chem
From: cs_jh@cox.nsac.ns.ca (JEFF HOYLE)
Subject: Re: Common ingredients info
Organization: Nova Scotia AC
Date: Thu, 20 Aug 1992 11:11:03 GMT

In article <19AUG199219511483@juliet.caltech.edu> natefrei@juliet.caltech.edu (Frei, Nathan A.) writes:

>In article <Bt8u3x.CDx@fc.sde.hp.com>, Gary Fritz <fritz@hpfcbig.sde.hp.com> writes...
>>Hi all,
>> 
>>I'm not a regular in this group, but I suspected you folks might be the
>>best source for some information.  Thanks in advance for any pointers.
>> 
>>I'd like to do some research on the ingredients commonly found in products
>>everybody uses all the time, like shampoos, soaps, lotions, etc.  I've heard
>>enough rumors of nasty effects of sodium lauryl sulfate and similar common
>>ingredients that I'd like to do some looking on my own.
>> 
>>Only problem is, where to look?  The only sources I've found so far are,
>>shall we say, biased.  I'd appreciate pointers to any reference books
>>or other good sources that list all these sorts of ingredients and explain
>>what they do, what they're good for, and what dangers/hazards they carry
>>in language understandable to an intelligent but non-chemist person.
>> 
>>Thanks!
>>Gary

>For a reasonably brief and intelligible description, look in _The New York 
>Public Library Desk Reference_.  A better idea, though, would probably be to
>get _The Merck Index_, or some such reference, and find a chemist to interpret,
>since most non-scientist's books on the subject that I've seen are biased
>one way or another (the reason for their publication was usually to "expose"
>something or other, or to point out all the "lies" perpetrarted by someone
>else).

>Nate

ANother really good source for this type of info is:

Chemistry in the Marketplace by Ben Selinger, pblished in NAmerica by 
Harcourt, Brace and Jovanovich.  Hope that helps
  ***********************************************************
  * Dr Jeff Hoyle (Organic Chemist)                         *
  * Chemistry and Soil Science Department                   *
  * Nova Scotia Agricultural College    FAX: (902)-895-4547 *                     *
  * P.O. Box 550, TRURO,              Voice: (902)-893-6630 *
  * Nova Scotia. CANADA  B2N  5E3                           *  
  *                  -----------------                      * 
  * Internet: cs_jh@cox.nsac.ns.ca  OR  jh_cs@ac.nsac.ns.ca *
  ***********************************************************
Newsgroups: sci.chem
From: ara@zurich.ai.mit.edu (Allan Adler)
Subject: Re: PC Version of ORTEP
Organization: M.I.T. Artificial Intelligence Lab.
Date: Sat, 15 Aug 1992 21:13:24 GMT


What does Ortep do exactly?

Allan Adler
ara@altdorf.ai.mit.edu
From: Christian_Mueller@ms.maus.de (Christian Mueller)
Newsgroups: sci.chem
Subject: air and experiment
Date: Mon, 17 Aug 92 14:27:00 GMT
Organization: MausNet
X-Gateway: MausGate/News 1.11

Hello
I need help!

I am searching some experiments (or books with illustrated experiments)
about analysis of the air.(harmfull substances as NOx,CO,CO2,...)
It's very urgent, because I need it to make my examination (teacher/chem.math)
I prefer easy experiments because they must be realize by pupils.

I'm also interest about experiments whitch can make clear the function
of a kathalysator(in a car).

Bye

Christian Mueller-Vanheiden
Hammerstrasse 105
4400 Muenster
Germany
(Net)
From: ulrich@galki.toppoint.de (Ulrich Gall)
Newsgroups: sci.chem
Subject: Re: Sparking grapes
Date: Sun, 16 Aug 92 18:50:16 GMT
Distribution: world               
Organization: private UUCP site, Kiel, Germany

bresler@casbah.acns.nwu.edu (Leo Bresler) writes:
>
> Hi, everybody!
>
> I have no explanation of this, but I conducted similar experiment with grapes.
> If you place whole grape(with seads) into a microwave, it stats shooting with
> seads.
>
> I suspect it has some electro-magnetic nature. Microwave probably induces
> circular current inside the grape, which makes it to speat the seeds out.

Sounds logical, but why does it work only with grapes and onions?

When I saw this with onions, I put a glass of water in the microwave to reduce
the energy haeting the onions - it didn't change anything! I can imagine any
fruit the size of a grape will burst really quick when powered with 600 watts.

> It's definitely interesting to here the expert's opinion.

Definitely.

Ulrich Gall, Seebrooksberg 2, W-2300 Klausdorf, Germany
Tel.: +49-431-790292, EMail: ulrich@galki.toppoint.de
Newsgroups: sci.chem
From: tony2@prefect.uucp (21131-gozdz)
Subject: Re: Request: Physical Property data / Computer-readable form?
Organization: Bellcore, Livingston, NJ
Date: Wed, 12 Aug 92 16:22:09 GMT

I've seen some info about various databases of
physico-chemical properties of various materials,
including gases, liquids, and mixtures, being sold for about
$200-$300 by NIST (National Institute of Standards and
Technology), Gaithersburg, MD (sorry, don't have their number).

--Tony

-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*
Antoni S. Gozdz                tel  (908) 758-2931  |  Bellcore  NVC 3X-261
tony2@prefect.cc.bellcore.com  FAX  (908) 741-2891  |  Red Bank, NJ 07701, USA
-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*-*
From: laborel@zig.inria.fr (Louis Laborelli)
Newsgroups: sci.chem
Subject: Comp. analysis of 2D NMR ?
Keywords: NMR ,2D , analysis
Date: 17 Aug 92 11:53:56 GMT
Organization: INRIA, Sophia-Antipolis (Fr)

Hi Chem.land ! 
I am not a chemist...therefore the following could appear naive .
What is the current status of automated analysis of 2D NMR ? 
A friend of mine says that it is actually an open problem, despite its 
general interest in industry . Is he wrong ?
I am specially interessed by the application of Artifical Neural Nets on the
subject .
Thanks .

-- 
 Louis Laborelli
 Universite de Nice Sophia Antipolis  / phone: (33) 92 94 26 89	       
 I3S LISAN - CNRS Batiment 4          \	telex: GRP 970006F
 250 rue Albert Einstein	      / fax: (33) 92 94 28 98
 Sophia Antipolis	              \ e-mail:laborel@zig.inria.fr
 06560 Valbonne FRANCE                / or laborell@mimosa.unice.fr
From: em21+@andrew.cmu.edu (Eric Edward Moore)
Newsgroups: sci.chem
Subject: Re: Contact lenses in lab (Was: Re: Security In Laboratory..??)
Date: 16 Aug 92 17:20:34 GMT
Article-I.D.: andrew.IeXjvWO00VoiI5XF5g
	<1992Aug15.182539.9874@galileo.cc.rochester.edu>
Organization: Carnegie Mellon, Pittsburgh, PA

btcl_ltd@creb.cc.rochester.edu (Brian) writes:
> Does anyone know if the same holds true for hard (rigid gas permeable) contact
> lenses? These don't seem to be mentioned as often soft lenses. I'm interested
> because I wear hard lenses (outside of the lab, of course).

Doesn't really matter.  In a chemical spash chemicals can get under
the lens and then not wash out as quickly.  This is bad.  Any contacts
in the lab are a bad thing.

	-Love, Kisses, and a Neutron Bomb
		-Eric the Finn
Newsgroups: sci.chem