HDTenEightyP/NetNews huggingface dataset:
From: dsmith@uoft02.utoledo.edu
Newsgroups: sci.chem,comp.graphics.avs
Subject: Re: AVS and chemistry
Date: 19 Nov 92 17:36:29 EST
Organization: University of Toledo, Computer Services

In article <1992Nov19.184745.18291@cc.ic.ac.uk>, rzepa@ic.ac.uk (Henry Rzepa) writes:
> An alternative [to AVS and the AVS Chemistry Viewer] is Explorer from SGI,
> which certainly costs less than AVS. 

Probably true, but AVS is platform independant and runs on about 10-12 
different vendor's hardware.  There is also the National AVS Center at the
North Carolina Supercomputer Center for support.  NCSC also maintains a
repository of free modules.  I don't think Explorer can offer all this.

> Graphically, both are stunning. From a developers view, both offer an
> excellent
> programming platform. Certainly the way to go (provided they can be
> afforded).

Very true.  Graphics is the wave of the future, and the future is now.

> _____________________________________________
> |  Dr Henry S Rzepa.                       Tel:   +44  71 225 8339 
> |  Department of Chemistry           Fax:   +44 71 589 3869  
> |  Imperial College                        Email: rzepa@ic.ac.uk
> |  LONDON SW7 2AY
> | Sent using Eudora 1.3b98.                 

Doug Smith
Assistant Professor of Chemistry
The University of Toledo
Toledo, OH  43606-3390

voice    419-537-2116
fax      419-537-4033
email    dsmith@uoft02.utoledo.edu
Newsgroups: sci.chem,comp.graphics.avs
From: rzepa@ic.ac.uk (Henry Rzepa)
Subject: Re: AVS and chemistry
X-UserAgent: Nuntius v1.1.1d12
X-XXMessage-ID: <A73191CC430150FD@macb.ch.ic.ac.uk>
Organization: Department of Chemistry, Imperial College
Date: Thu, 19 Nov 92 18:47:45 GMT
X-XXDate: Thu, 19 Nov 92 18:47:40 GMT

In article <83837@ut-emx.uucp> Renzo Balducci,
balducci@phenyl.phr.utexas.edu writes:
>I would appreciate any information regarding current chemical usage of
AVS.

AVS comes in two components, AVS Viewer, and AVC Chemistry viewer. 
The latter enables visualisation of Gaussian 92 and MOPAC files, the
former
reads PDB data etc.

An alternative is Explorer from SGI, which certainly costs less than AVS. 
We are developing many new modules for Explorer, which we will offer
shortly
via  the Explorer archive (cost yet undecided!). 

Graphically, both are stunning. From a developers view, both offer an
excellent
programming platform. Certainly the way to go (provided they can be
afforded).
_____________________________________________
|  Dr Henry S Rzepa.                       Tel:   +44  71 225 8339 
|  Department of Chemistry           Fax:   +44 71 589 3869  
|  Imperial College                        Email: rzepa@ic.ac.uk
|  LONDON SW7 2AY
| Sent using Eudora 1.3b98.                 
_____________________________________________
From: dietz@cs.rochester.edu (Paul Dietz)
Newsgroups: sci.chem
Subject: Re: Gold - future Auto Catalyst
Date: 17 Nov 92 15:49:17 GMT
Article-I.D.: cs.1992Nov17.154917.4790
Organization: Computer Science Department University of Rochester

In article <1992Nov17.152054.10043@ucsu.Colorado.EDU> knapp@spot.Colorado.EDU (David Knapp) writes:

 >>There
 >>are effectively infinite supplies of both metals at concentrations
 >      ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
 >>only a few times less than current ores.  
 >
 > Can you expound on what you mean by "effectively infinite"? I mean, is it 
 > infinite or isn't it?  Can something be 'effectively limited' and still be
 > unlimited? 


"Effectively infinite" means:  the available supplies will last
longer than any reasonable planning horizon.  For iron and aluminum,
this is because the ores being mined today are only a few times
richer than your average piece of the earth's crust.

More specifically, aluminum is today obtained from bauxite.  However,
it can also be obtained from kaolinite -- clay -- which is available
in enormous quantities.  Ultimately, it can be derived from feldspar,
if we ever run out of clay.

Thousands of years of iron are available in taconites.  Should those
run out, basalt is about 8% iron.  There are millions of cubic miles
of basalt available.


 > You've commented on mny things I didn't even mention so you might be 
 > thinking of a different post.

I made the apparently incorrect assumption that people reading
my posting would engage their brains while doing so.  

	Paul F. Dietz
	dietz@cs.rochester.edu
From: ch436@cleveland.Freenet.Edu (Eric W. Wallin)
Newsgroups: sci.chem
Subject: Undergraduate Internships
Date: 21 Nov 1992 05:50:37 GMT
Organization: Case Western Reserve University, Cleveland, Ohio (USA)
NNTP-Posting-Host: hela.ins.cwru.edu


	Hello!  I am an undergraduate student studying Chemistry nad Physics
(my majors) and would like to spend the summer of '93 doing an intership/
researhc in a government or private/ or coroporate instututions.  If anyone
can point me in the right direction with informations concerning such programs
please drop me a line, because I really don't care to be flipping burgers next
summer!  Hey, and you will be helping somone to get a good basis for a career in
the sciences.

Thanks in ADVANCE...(rally I can spell, my editor is messed up of somthing...)

Eric Wallin
Freshman Ball State University, Muncie, IN
00ewwallin@leo.bsuvc.bsu.edu

Thanks again!
From: brecher@husc8.harvard.edu (Jonathan Brecher)
Newsgroups: sci.chem
Subject: Re: Glowing Light Stick, how do they work?
Date: 19 Nov 92 09:58:47 GMT
Article-I.D.: husc8.BRECHER.92Nov19015847
Organization: Harvard Arts and Sciences Computer Services, Cambridge, MA
In-reply-to: treesh@bach.helios.nd.edu's message of 18 Nov 92 21:47:54 GMT

In article <1992Nov18.214754.23523@news.nd.edu> treesh@bach.helios.nd.edu (carey treesh) writes:
>I was wondering if anyone can tell me how these light sticks work?  What
>chemicals are they using, and how dose this reaction take place?  Is it
>possible to make my own rather they have to buy them from a supplier? 
>Would it be cost effective?  

According to my class notes from last year:
 
"...the perhydrolysis of oxalate esters in the presence of a fluorescent
 indicator gave intense emission.  This reaction proceeds with a photon
 yield of 23% and is the basis for ther commercial "Coolite" sticks."
 
                        |-         -|
       RO-+=O   H2O2    |   O-+=O   |  fluorescer
          |    ------>  |   | |     | ------------>  CO2 + C02 + hv
       RO-+=O           |   O-+=O   |
                        |-         -|
 
(I hate ASCII graphics.  Those things in the second step are big brackets.)
 
When you break the thing in the light sticks you allow the peroxide and the
esters to mix.
 
As for cost/feasibility: beats me.
 
						jonathan brecher
						brecher@husc.harvard.edu
						assistant mac.archivist
Newsgroups: sci.chem
Subject: re: H2O2 Version 2.1
From: lunazzi@boifcc.cineca.it (Mauro Andrea Cremonini)
Date: 19 Nov 92 13:03:23 +0100

In article <1992Nov19.035923.8381@news.acns.nwu.edu> dmeier@casbah.acns.nwu.edu (Douglas Meier) writes:
>I asked earlier what the reaction was between H2O2 and flesh (i.e. why the
>bubbles) and got two responses.  
>
>1)  It breaks down into H20 and O2, with some O radicals reacting with the
>skin.
>
>2)  Oxidation reaction where H2O and CO2 are the gases given off.
>
>Now I know that H2O2 can be an oxidizing agent or a reducing agent, dependent
>on the conditions, but I don't know which way this reaction occurs under
>conditions of H2O2 reacting with organic materials.  
>
>Any more suggestions?
>

What about peroxydase enzyme ?
Bye
Mauro
P.S.
In that case the gas is O2.

|===================================|    /\
|Mauro Andrea Cremonini (IW4BOX)    |   //\\
|Dept. Organic Chemistry            |  ///\\\
|University, Bologna, ITALY         |  \\\///
|e-mail lunazzi@boifcc.cineca.it    |   \\//
|===================================|    \/
From: ps02@ns1.cc.lehigh.edu (PENELOPE E. SMITH)
Newsgroups: sci.chem
Subject: Re: Gold dust a fire hazard?
Date: 17 Nov 92 19:23:06 GMT
Organization: Lehigh University

In article <1992Nov16.221038.8023@ucsu.Colorado.EDU>, knapp@spot.Colorado.EDU (D
avid Knapp) writes:
...
>I believe that many 'spontaneous' combustion demonstrations of finely
>divided metals are literally triggered by transient free oxygen from,
>of all things, cosmic rays. I wish I could remember the article I read
>this in to fend off the ensuing flames here, but I'm afraid I don't.
>So sue me.

Please appear in court 9:00 AM 22 September 1993 in the matter of.... :-)

I think that Electrostatic discharge may have a lot more to do with this,
since it is quite common below a few hundred volts and imperceptible without
instrumentation.  Of course, a cosmic ray might create a conductive path to
carry the discharge or recieve its radiation.  There is a lot more energy
available in a very short time!

    Eric Christenson
-- 
 
~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~
Penelope E. Smith               PS02@NS.CC.LEHIGH.EDU
Department of Mathematics       PS02@LEHIGH.BITNET
Lehigh University
Bethlehem, PA
Newsgroups: sci.chem
From: rajat@sunny3.che.clarkson.edu (Rajat Kapoor)
Subject: Re: Oil Spills
Organization: Clarkson University
Date: Mon, 16 Nov 1992 18:02:15 GMT

From article <74956@hydra.gatech.EDU>, by gtd205a@prism.gatech.EDU (Hody Crouch):
>   2.  Oil also begins to spread through the water.  The oil molecules attract
> H2O, and when enough water molecules surround a small oil molecule, it can 
> 'dissolve' (used in the loosest sense of the word).


This point ( Partial Coeff, though very low ), should be helpful. 
I wouldn't be surprised, if surfactants are employed for these
situations to disperse and dilute oil (after skimming) in the ocean. Aquatic
life would hardly be disturbed by oil micelles, much less for molecularly
dissolved oil.

Kapoor

Hmm... talk about the dream-fuel, water...
Newsgroups: sci.chem
From: giber@pollux.cs.uga.edu (Carolyn Giberson)
Subject: hydrogen peroxide decomposition in human tissues
Originator: giber@pollux
Organization: University of Georgia, Athens
Date: Mon, 23 Nov 1992 15:19:07 GMT


Human tissues contain an enzyme (catalase) which does indeed decompose
hydrogen peroxide.  Potatoes have a similar enzyme.  We use that
potato enzyme in a lab on enzyme activity which I would be glad to
post if there is interest.

Carolyn Giberson
University of Georgia

Newsgroups: sci.chem
From: saj@chinet.chi.il.us (Stephen Jacobs)
Subject: Re: Need info on rechargable NiCd batteries...
Summary: I think there's something a little sideways here
Organization: Chinet - Public Access UNIX
Date: Mon, 16 Nov 1992 15:08:31 GMT

In article <1e4etdINNb5g@usenet.INS.CWRU.Edu> an881@cleveland.Freenet.Edu (Dick Middaugh) writes:
>
>Long ago and far away, NiCad batteries had a "memory effect", and
>it was important to discharge them fully before recharging them.
>That is not true of present-day batteries, but the folklore 
>persists.

I think it's more like "Long ago and far away, all consumer rechargeable
batteries were NiCd ones, subject to a memory effect.  Now there are other
possibilities, and one does well to know what kind of batteries are where".

                                    Steve      saj@chinet.chi.il.us
Xref: sparky sci.chem:4787 rec.pyrotechnics:3823 rec.models.rockets:3072
From: whitbeck@equinox.unr.edu (Michael Whitbeck)
Newsgroups: sci.chem,rec.pyrotechnics,rec.models.rockets
Subject: Re: H2O2/UDMH/RFNA propellant suppliers in Los Angeles Area?
Date: 23 Nov 92 16:26:04 GMT
Followup-To: sci.chem
Organization: University of Nevada, Reno

In article <1992Nov21.085910.20125@hpcvaac.cv.hp.com> billn@hpcvaac.cv.hp.com (bill nelson) writes:
"merlin@neuro.usc.edu (merlin) writes:
": Does anyone know of a good supplier of H2O2 and UDMH (unsymmetrical
": dimethyl hydrazine) in the Los Angeles area?  We need a more or less
": decent propellant for our small liquid fueled model rocket project.
": How about red fuming nitric acid or at least the precursors thereof?
"
"H2O2, you should be able to find in any well stocked chemical lab. As

 the concentrations required for H2O2 in rocketry
 are much higher than typical of the dilute H2O2
 normally found in labs (10-30%). FMC sells/sold
 conc. H2O2 suitable for rocketry. They may no
 longer sell it. It is very dangerous stuff- long
 ago when I ordered some I had to sign all kinds of
 disclaimers in advance!


"for the UDMH or HNO3, that would depend on the lab.

Both are easy to get. Although UMDH is a bit
pricy.



Mike
Organization: Penn State University
Date: Mon, 23 Nov 1992 22:27:10 EST
From: Ted West <TRW108@psuvm.psu.edu>
Newsgroups: sci.chem
Subject: H2O2, again...

I've heard that hydrogen peroxide is not all that good at DISINFECTING a
wound, but that it is good for CLEANING it.  This is the logic:
Dirt (and whatever else is in the wound - blood???) catalyzes the reaction:
   2 H2O2 --> 2 H2O + H2 (gas).
The hydrogen gas product then carries the dirt, etc. to the surface
of the wound where it is then washed away.
_______________________________________________________________________________
TED WEST                                                      What's a 'fubar'?
TRW108 @ PSUVM.BITNET                                              814-862-7589
west @ fubar.bk.psu.edu                                        617 Mifflin Hall
trw108 @ psuvm.psu.edu                                University Park, PA 16802
-------------------------------------------------------------------------------
Newsgroups: sci.chem
From: mjf9968@rigel.tamu.edu (Pi(3.143832666))
Subject: Re: Why Not ? (Re: Ethanol fuel
News-Software: VAX/VMS VNEWS 1.41    
Organization: Texas A&M University, Academic Computing Services
Date: Mon, 16 Nov 1992 09:06:00 GMT

In article <1992Nov15.201346.9786@ucsu.Colorado.EDU>, smithrs@ucsu.Colorado.EDU (SMITH  RANDALL SCOTT) writes...
>One must also consider the fact that addition of ethanol to hydrocarbon
>fuel tends to increase the vapor pressure of the fuel.  Thus, although
>10% ethanol will decrease the CO emissions from the engine, it increases
>the hydrocarbon emissions from the fuel tank and lines.  In the end, I
>agree with Mike.  The most effective method of reducing emissions _overall_
>is to provide incentive programs to repair/upgrade old autos, to promote
>mass transit, and to develop alternitive energy sources that are _less
		      ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
>polluting_ than those currently available.
 ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
> 
>Randall Smith
>smithrs@ucsu.colorado.edu


	Such as?  I don't mean this as a flame, just an honest
	question.  The much praised act in California which
	requires auto manufactorers to sell cars which run on
	electricity does basically nothing to help pollution
	problems.  Most electricity in the US is made from burning
	fossil fuels, so electric cars don't solve air pollution,
	they just move it out of the city.

	The biggest innovation in electricity production lately
	has been using trash as fuel for the boilers.  Laudable
	for getting rid of trash, but just as polluting.

	Nuclear power has it's own special problems, solar
	power just can't produce enough for big cities, nor
	can wind.  I'm really curious at to what "alternatives"
	may be out there.

	In the end, though, I don't see the point.  Nothing will
	really change until the oil becomes prohibitively expensive
	(which it won't for, in some projections, over 150 years)
	or the enviorment becomes unlivable for people, which it
	won't for at least a few years.  We hope.

	Living better through chemistry,
	Mike "Pi" Freeman
	MJF9968@rigel.tamu.edu
Xref: sparky sci.chem:4758 rec.pyrotechnics:3807 rec.models.rockets:3054
From: merlin@neuro.usc.edu (merlin)
Newsgroups: sci.chem,rec.pyrotechnics,rec.models.rockets
Subject: H2O2/UDMH/RFNA propellant suppliers in Los Angeles Area?
Date: 20 Nov 1992 21:25:48 -0800
Organization: University of Southern California, Los Angeles, CA
NNTP-Posting-Host: neuro.usc.edu

Does anyone know of a good supplier of H2O2 and UDMH (unsymmetrical
dimethyl hydrazine) in the Los Angeles area?  We need a more or less
decent propellant for our small liquid fueled model rocket project.
How about red fuming nitric acid or at least the precursors thereof?

I suppose we could use liquid oxygen and liquid hydrogen which we
already have on hand in the lab -- but some of the designs we want
to use originally specified H2O2 and UDMH for proper mixing.

Has anyone had experience filing permits required for launching our
model rocket with the FAA, the AQMD, and/or anyone else who may care?

Thanks, Merlin
From: v111qheg@ubvmsb.cc.buffalo.edu (P.VASILION)
Newsgroups: sci.chem
Subject: RE: Chemiluminesence
Date: 24 Nov 92 04:15:00 GMT
Organization: University at Buffalo
News-Software: VAX/VMS VNEWS 1.41


	In regards to the querries about chemical light sticks and 
chemiluminesence, there are only two major components needed to make a light 
stick.  The first is the component stored in the glass ampule that you break
when you bend a light stick. This is everyday hydrogen peroxide. I suspect that
a similar compound could be used, since H2O2 gives the light stick its rather
limited shelf life. The second component is the more difficult one to obtain.
Cyalume light sticks use Luminol (5-amino-2,3-dihydro-1,4-phthalazine-dione),
C8H7N3O2. The 1989 and earlier (to at least 1952) editions of _The Merck
Index_ give a good description of Luminol. I have not found a recipe to
produce, nor a place to buy it, however. 
	Hopes this sheds some light on the matter. Good luck in finding 
Luminol. 


Peter Vasilion
SUNY @ Buffalo
v111qheg@ubvms.cc.buffalo.edu
vasilion@acsu.buffalo.edu
KB2NMV@KE2VW.#WNY.NY.USA.NA
From: 01crmeyer@leo.bsuvc.bsu.edu (Craig Meyer)
Newsgroups: sci.chem
Subject: Working Fluid for Ext. Comb. Engines
Date: 20 Nov 92 00:25:42 GMT
Organization: Ball State University, Muncie, In - Univ. Computing Svc's

A few of the netters on sci.energy and I are talking about external-combustion
engines for cars and trucks, and one of the problems we're encountering is the
fact that water can freeze.  Also, very hot steam is corrosive.

I read about a steam-like engine that used "an organic fluid several times
heavier than water."  What could that have been?

What kind of compound would you suggest?  A few criteria:

  Liquid at room temperature
  Doesn't freeze during wintertime (under 30 below, to be safe)
  Boils at a reasonably low temperature (like water)
  Isn't corrosive at circa 800C
  
  If possible, serves as a lubricant--even at 800C temperatures
    (Is it even possible for a gas to be a lubricant?)

Thanks for helping us out!

CM
  
-- 
       Craig Meyer                 01CRMEYER@LEO.BSUVC.BSU.EDU
       Indiana Academy for Science, Mathematics, and Humaities.
       Muncie, IN  47306                          317-285-7433

       Opinions expressed are mine alone, and not necessarily
       shared by the Indiana Academy.
Newsgroups: sci.chem
From: mjf9968@rigel.tamu.edu (Pi(3.143832666))
Subject: Re: Why Not ? (Re: Ethanol fuel
News-Software: VAX/VMS VNEWS 1.41    
Organization: Texas A&M University, Academic Computing Services
Date: Tue, 17 Nov 1992 00:38:00 GMT

In article <1992Nov15.201346.9786@ucsu.Colorado.EDU>, smithrs@ucsu.Colorado.EDU (SMITH  RANDALL SCOTT) writes...
>One must also consider the fact that addition of ethanol to hydrocarbon
>fuel tends to increase the vapor pressure of the fuel.  Thus, although
>10% ethanol will decrease the CO emissions from the engine, it increases
>the hydrocarbon emissions from the fuel tank and lines.  In the end, I
>agree with Mike.  The most effective method of reducing emissions _overall_
>is to provide incentive programs to repair/upgrade old autos, to promote
>mass transit, and to develop alternitive energy sources that are _less
		      ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
>polluting_ than those currently available.
 ^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^^
> 
>Randall Smith
>smithrs@ucsu.colorado.edu


	Such as?  I don't mean this as a flame, just an honest
	question.  The much praised act in California which
	requires auto manufactorers to sell cars which run on
	electricity does basically nothing to help pollution
	problems.  Most electricity in the US is made from burning
	fossil fuels, so electric cars don't solve air pollution,
	they just move it out of the city.

	The biggest innovation in electricity production lately
	has been using trash as fuel for the boilers.  Laudable
	for getting rid of trash, but just as polluting.

	Nuclear power has it's own special problems, solar
	power just can't produce enough for big cities, nor
	can wind.  I'm really curious at to what "alternatives"
	may be out there.

	In the end, though, I don't see the point.  Nothing will
	really change until the oil becomes prohibitively expensive
	(which it won't for, in some projections, over 150 years)
	or the enviorment becomes unlivable for people, which it
	won't for at least a few years.  We hope.

	Living better through chemistry,
	Mike "Pi" Freeman
	MJF9968@rigel.tamu.edu
Newsgroups: sci.chem
From: saj@chinet.chi.il.us (Stephen Jacobs)
Subject: Re: Gold dust a fire hazard?
Summary: The metal of Sheffield didn't burn 
Organization: Chinet - Public Access UNIX
Date: Mon, 16 Nov 1992 04:23:04 GMT

Since this is a sci. group, it's worth putting in a token denial of the 
statements that the metal of the destroyer Sheffield burned
after it was hit by an Exocet.  This has been gone over endlessly in 
sci.military, and consensus is very strongly that it didn't happen that way.
I am a great deal less sure of another point: while Sheffield was designed
with a very high aluminum content, I believe there was actually very much less
than intended when she entered combat.  

                                           Steve     saj@chinet.chi.il.us
Newsgroups: sci.chem
From: sundermm@columbia.dsu.edu (MARC SUNDERMEYER)
Subject: Bucky things
Organization: Dakota State University
Date: Thu, 19 Nov 1992 02:52:37 GMT

    Thank you all for the input on the bucky descriptions,  I did get a 
chance before all this to see the Nature article about the onions.  Another 
thing that I found interesting was the latice of Bucky Balls in one of the 
latest Popular Science magazines that allows only gasses smaller than carbon 
to pass through.  They say it may prve to be a usefull filter in plants that 
process methane to keep out nitrogen.
    What ever did they accomplish with the Bucky Bunny which didn't spin, is 
it a basis for the bucky onions perhaps?

Newsgroups: sci.chem
From: dexter@aries.scs.uiuc.edu (Annette Dexter)
Subject: Re: H2O2, again...
Organization: University of Illinois at Urbana
Date: Tue, 24 Nov 1992 04:57:41 GMT

Ted West <TRW108@psuvm.psu.edu> writes:

>I've heard that hydrogen peroxide is not all that good at DISINFECTING a
>wound, but that it is good for CLEANING it.  This is the logic:
>Dirt (and whatever else is in the wound - blood???) catalyzes the reaction:
>   2 H2O2 --> 2 H2O + H2 (gas).
>The hydrogen gas product then carries the dirt, etc. to the surface
>of the wound where it is then washed away.

	Doesn't sound right to me...

1) I can't see enough gas pressure being generated to carry anything away,
dirt, bacteria or whatever.

And,	

2) Even if that worked, the concentration of H2O2 needed to do it would
give you a very painful burn.  Believe me, I've spilled the concentrated
stuff on myself often enough to know.

	Annette
	dexter@aries.scs.uiuc.edu
From: mgray1@metz.une.edu.au (Matthew GRAY)
Newsgroups: sci.chem
Subject: Re: methanol "luminescence"
Date: 16 Nov 92 02:36:30 GMT


If you're shining a laser through 'pure' methanol and getting emission
of light of a different colour than that from the laser, it's possible
you're getting second harmonic generation-same as what's happening in 
the dye laser. 
Then again, it could be an impurity-from the container? You'd expect
spectroscopic grade to be 'pure' in terms of what is deliberatly
put into it, but it could be contaminated between the supplier and you.
NB methylated spirits goes blue when mixed with water, maybe atmospheric
moisture is being 'sucked' into your sample. Try superdrying it.
		All just guesses,
					yours,
					      Matthew Gray
					      mgray1@metz.une.oz.au