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Yntarius
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Exothermic reactions
Hi guys
I have being looking everywhere for a mild exothermic reaction with safe-to-use and non-toxic products (that excludes acids, strong bases, hidrogen,
etc) and non-impossible materials to get (where i live, magnesium is forbiden by law, for example).
Anyone has any idea what could i do? All i need to do is to boil some water.
Thanks a lot!
Ariel
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Waffles
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| Quote: | Originally posted by Yntarius
Hi guys
I have being looking everywhere for a mild exothermic reaction with safe-to-use and non-toxic products (that excludes acids, strong bases, hidrogen,
etc) and non-impossible materials to get (where i live, magnesium is forbiden by law, for example).
Anyone has any idea what could i do? All i need to do is to boil some water.
Thanks a lot!
Ariel |
That's not exactly mild. Water has an extremely high heat capacity.
The oxidation of iron powder in the presence of activated carbon and cellulose in hand warmers would come to mind as a 'mild' exothermic reaction. The
'safest' I can think of is potassium permanganate and glycerin, since that produces certainly high enough temperatures to boil water, and while
potassium permanganate is a powerful oxidizer, it isn't terribly toxic, and not in the league or chlorates or perchlorates or anything in terms of
stability and reactivity. Sure will stain everything around, though.
\"…\'tis man\'s perdition to be safe, when for the truth he ought to die.\"
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Yntarius
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| Quote: | Originally posted by iamthewaffler
That's not exactly mild. Water has an extremely high heat capacity.
The oxidation of iron powder in the presence of activated carbon and cellulose in hand warmers would come to mind as a 'mild' exothermic reaction. The
'safest' I can think of is potassium permanganate and glycerin, since that produces certainly high enough temperatures to boil water, and while
potassium permanganate is a powerful oxidizer, it isn't terribly toxic, and not in the league or chlorates or perchlorates or anything in terms of
stability and reactivity. Sure will stain everything around, though. |
Well i think i said it wrong. By mild, i meant it doesnt have to be very fast and explosive, but yea you are right, water takes quite some energy to
boil.
Whats are the outcome from potassium permanganate and glycerin? Are those chemicals bad to be ingested? lol
Thanks again
Ariel
[Edited on 6-12-2006 by Yntarius]
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mericad193724
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Is this for a science project of some kind?
How about a chemical reaction that generates a flammable gas which when mixed with oxygen, and burned, is VERY exothermic. If this would work for you
then try aluminum foil and Sodium Hydroxide, available as drain opener crystals(Draino). Those are very easy to get. The sodium hydroxide gets hot,
but not hot enough to boil water, the hydrogen however can be burned very HOT!
Edit: also, adding a concentrated strong acid such as sulfuric acid to water will cause it to get really hot, maybe even boil! This is pretty
dangerous since sulfuric acid eats skin pretty well!
good luck.
Mericad
[Edited on 6-12-2006 by mericad193724]
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Yntarius
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| Quote: | Originally posted by mericad193724
Is this for a science project of somekind?
How about a chemi reaction that generates a flammable gas which when mixed with oxygen, and burned, is VERY exothermic. If this would work for you
then try aluminum foil and Sodium Hydroxide, available as drain opener crystals(Draino). Those are very easy to get. The sodium hydroxide gets hot,
but not hot enough to boil water, the hydrogen however can be burned very HOT!
good luck.
Mericad |
Not exactly a science project... hehehe
I have a college project in witch I'm suposed to find alternative ways to generate power. Since everyone uses burning coal and solar energy, i
figuered to maybe try to use chemical energy to boil water and therefore spin the turbine. But since it will be an open fair, with kids and all, i
wanted to be on the safe side hehehe
Isn't burning H2 VERY dangerous? heheehe
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Ozone
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Yntarius,
There are a great many good exothermic reactions, some of which are relatively safe for the unexperienced to perform.
The safest of these, that I know off-hand, was mentioned in passing by iamthewaffler. Simply take iron powder (or filings, they are very easy to get),
add some brine (water saturated with NaCl, table salt), and some extra water. Let this sit for a while until a tiny amount of rust is formed (this is
not required, but seems to make the next part proceed with greater velocity). To this is added peroxide (H2O2), stronger is better, but beware as even
with 10% the mixture will boil--higher concentrations than this would likely be dangerous. This should work with OTC 3%, but my "expedited rust
preparations" were made using 10%.
On the same tangent is the slow (dropwise) addition of dilute H2O2 to common household bleach. Here, the H2O2 is oxidized by the NaOCl (5.9% diluted
1:1) to immediately yield O2 and NaCl (some NaClO3 is also likely formed). The Resulting O2 could be used as is to spin a small turbine...or, it could
be combined with H2 or some other fuel (which is risky because H2:O2 mixtures can spontanously ignite or explode if the proportions of each are not
correct (bad, but fun idea!). Whew, oxyhydrogen is *really* hot.
Look up hydrogen peroxide for rocket propellent, etc. for some interesting ideas!
Good luck and be careful,
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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guy
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| Quote: | Originally posted by Yntarius
| Quote: | Originally posted by mericad193724
Is this for a science project of somekind?
How about a chemi reaction that generates a flammable gas which when mixed with oxygen, and burned, is VERY exothermic. If this would work for you
then try aluminum foil and Sodium Hydroxide, available as drain opener crystals(Draino). Those are very easy to get. The sodium hydroxide gets hot,
but not hot enough to boil water, the hydrogen however can be burned very HOT!
good luck.
Mericad |
Not exactly a science project... hehehe
I have a college project in witch I'm suposed to find alternative ways to generate power. Since everyone uses burning coal and solar energy, i
figuered to maybe try to use chemical energy to boil water and therefore spin the turbine. But since it will be an open fair, with kids and all, i
wanted to be on the safe side hehehe
Isn't burning H2 VERY dangerous? heheehe |
Haha Good luck. You'll be famous if you actually discover something like that.
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Yntarius
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| Quote: | Originally posted by Ozone
Yntarius,
There are a great many good exothermic reactions, some of which are relatively safe for the unexperienced to perform.
The safest of these, that I know off-hand, was mentioned in passing by iamthewaffler. Simply take iron powder (or filings, they are very easy to get),
add some brine (water saturated with NaCl, table salt), and some extra water. Let this sit for a while until a tiny amount of rust is formed (this is
not required, but seems to make the next part proceed with greater velocity). To this is added peroxide (H2O2), stronger is better, but beware as even
with 10% the mixture will boil--higher concentrations than this would likely be dangerous. This should work with OTC 3%, but my "expedited rust
preparations" were made using 10%.
On the same tangent is the slow (dropwise) addition of dilute H2O2 to common household bleach. Here, the H2O2 is oxidized by the NaOCl (5.9% diluted
1:1) to immediately yield O2 and NaCl (some NaClO3 is also likely formed). The Resulting O2 could be used as is to spin a small turbine...or, it could
be combined with H2 or some other fuel (which is risky because H2:O2 mixtures can spontanously ignite or explode if the proportions of each are not
correct (bad, but fun idea!). Whew, oxyhydrogen is *really* hot.
Look up hydrogen peroxide for rocket propellent, etc. for some interesting ideas!
Good luck and be careful,
O3 |
Ozone, are those reactions hot enought to boil water? I remember doing some experiments with H2O2, but nothing that hot....
Anyways, its starting to become very clear to me that the best reaction to get lots of heat is oxidatting some metal, catalized with NaCl and a
sacrifice metal. I think I'm going to have to do some experiments with iron, copper, aluminium and other easy-to-get metals... I really hope this
works....
| Quote: | Originally posted by guy
Haha Good luck. You'll be famous if you actually discover something like that.
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I hope you are right guy.... I'll give the forum its credits tho  heheheh
Im open to more sugestions : )
Thanks guys!
Ariel
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Ozone
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Oh yes! The expedited oxidation of iron is quite exothermic. The bubbling is steam (the O2 is added to the iron). An excess of iron can be
continuously fed peroxide solution to yield heat and steam until the Fe is totally oxidized (which appears to take quite a while).
If I have time, I'll do the rxn tomorrow and try to get a small vid to post here.
Good luck,
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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Yntarius
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| Quote: | Originally posted by Ozone
Oh yes! The expedited oxidation of iron is quite exothermic. The bubbling is steam (the O2 is added to the iron). An excess of iron can be
continuously fed peroxide solution to yield heat and steam until the Fe is totally oxidized (which appears to take quite a while).
If I have time, I'll do the rxn tomorrow and try to get a small vid to post here.
Good luck,
O3 |
This is awesome! lol
I didnt hit the 100C yet, but i got close to 80 using powder iron, salt and 12% peroxide! I saw a 42% peroxide bottle on the store, but i bought the
12% at least to start the tests (a lot cheaper)....
Gotta love womans product section, you find a lot of chemicals in there hahahahahah
I'll keep you guys updated, including the exact weights and proportions once it works as i want : )
And im trying to catalize this reaction with some other metals... Maybe aluminum powder (being iron its sacrifice metal and since aluminum oxides a
lot faster then iron)
Thaks once more guys
Ariel
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12AX7
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Aluminum tends to be resistant to air and water...
To work with aluminum, you'll need something like lye or acid, which dissolves the aluminum and its oxide, plus something to handle the hydrogen,
perhaps MnO2 (think dry cells). But that would likely be too rapid, so zinc would be a better cadidate. In this case, you have essentially the
process inside an alkaline (if using NaOH/KOH) or dry cell (using NH4Cl I believe; NaCl should also work), but assembled in such a way that it won't
explode under short circuit.
Tim
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Dr. Beaker
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If you only need a power source to rotate a turbine then you don't really need to use steam for it - you just need a reaction that produces gas.
take powdered limestone (or sodium carbonate/bicarbonate) and add viniger or diluted acetic acid. do it in a pressure proof vessels and use the gas
pressure to make electricity.
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YT2095
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the easiest and probably safest exothermic reaction would be the addition of water to Calcium Oxide.
it`s the same method used in some of these ready meal heat packs.
EDIT: and if you`re wondering how to employ this, it`s really quite simple, you`ll meed a plastic macdonalbs straw, and then put in several large pin
holes through it along its length, put this inside a large pyrex test tube, and then fill the tube with the calcium oxide granules, when you want to
activate it, pour water inside the straw.
the water will come out of the holes you made and into the CaO.
this will start to get very hot, so put this tube in your cup of cold water and just wait
[Edited on 9-12-2006 by YT2095]
\"In a world full of wonders mankind has managed to invent boredom\" - Death
Twinkies don\'t have a shelf life. They have a half-life! -Caine (a friend of mine)
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Yntarius
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| Quote: | Originally posted by 12AX7
Aluminum tends to be resistant to air and water...
To work with aluminum, you'll need something like lye or acid, which dissolves the aluminum and its oxide, plus something to handle the hydrogen,
perhaps MnO2 (think dry cells). But that would likely be too rapid, so zinc would be a better cadidate. In this case, you have essentially the
process inside an alkaline (if using NaOH/KOH) or dry cell (using NH4Cl I believe; NaCl should also work), but assembled in such a way that it won't
explode under short circuit.
Tim |
An update to you guys
I've mixed about 4 grams of powder iron, 1g of powder aluminium, about 20g of kitchen salt (with just a little water so i could make a homogene mass
between the salt and the metal dust) and 100ml of peroxide (12%).... Reaction started instantly and got pretty hot very fast. It reached 100ºC within
the first 30 seconds and holded the 100ºC for as long as 9 minutes, when the reaction started to slow down due to the lack of more peroxide...
Still trying to find the best balance between the materials, monday I'm buying some more peroxide (50% this time) and pure (NaCl), in order to make
this a more reliable experiment. Only problem is that aluminium powder is monitored by the army, so monday i'm gonna try to find some small aluminium
scraps. So far Ive made my own hehehe
Dr. Beaker, the advantage on oxiding the metal instead of using bicarbonate and viniger is that with very little metal dust i can make the reaction
last very long, just have to keep adding peroxide (with the left over of the experiment described above, i just kept adding peroxide and it kept going
for almost 30 min without adding any adicional metal powder)
YT2095, isnt CaO not safe to handle without gloves and all? How do the heat packs work? Do you open it to put the water inside? Sounds like an
interesting reaction, I'm gonna research more on the CaO tho, see how safe it is.
This is starting to come out a lot faster then I expected, thanks for all the help guys. And keep them comming heheh
Thanks : )
Ariel
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YT2095
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the ones I`ve seen have water on one side and CaO on the other seperated by a thin metal sheet, there`s a plastic dome with a sharp plastic bit stuck
to it, you presson this dome and the sharp peice punctures the metal seperator allowing the liquid to mix with the CaO, you give it a quick shake and
just leave it to stand for a few mins.
CaO is non toxic, and quite safe to handle without gloves for short periods of time, it isn`t all that caustic, just keep it dry.
get some sea shells and smash them up, then roast them in a hot fire, that`s how the CaO is made in many of the heat packs, in fact if you take one
appart and start dissolving the caO in dilute HCl you`ll even see some bits that are quite clearly sea shell fragments
\"In a world full of wonders mankind has managed to invent boredom\" - Death
Twinkies don\'t have a shelf life. They have a half-life! -Caine (a friend of mine)
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Ozone
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Yntarius,
Interesting, your results are parallel to mine; Have you run a control experiment without the Al°--the exotherms plotted over time could tell you
quite a bit (as will the maximum).
Simple and effective; I really like this rxn! Be careful though with the stonger peroxide--it might get a bit more frisky than intended. I would keep
with the 10-20% range with continual addition, say, with a dropping funnel or the like. It should reach steady state unless 1) you run out of water,
which is unlikely with the constant addition of dilute H2O2 or, 2) you run out of iron, or 3) you blow the contents out of the vessel.
I'm not too sure about the Al°. I wanted to try it the other day, but was sidetracked by a bad tooth. I'll see about it tomorrow.
CaO is nothing to worry about, the inhaled dust is irritating however, so a dust mask (nothing fancy) might be a good idea if you notice dust
"poofing" everywhere.
Waiting for the darvocet to kick in,
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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Ozone
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Here's one...I think this would be applicable for the "water activated fire" thread found elsewhere:
Exothermic demo
John Bartmess, Charles Feigerle, George Schweitzer, Wes Fellers, Peter Smith
Department of Chemistry, University of Tennessee, Knoxville
Chemical & Engineering News (15 Jun 1998) Vol. 76, No. 24, pp. 4.
--------------------------------------------------------------------------------
We wish to point out a safety hazard with a widely performed standard chemical demonstration that caused significant damage recently in a teaching
laboratory in the chemistry department at the University of Tennessee, Knoxville.
The Belousov-Zhabotinsky oscillator reaction described in Bassam Shakhashiri's" Chemical Demonstrations: A Handbook for Teachers of Chemistry," Vol.
2, involves the cerium ammonium nitrate-catalyzed redox reaction of potassium bromate with malonic acid. This reaction was carried out in an honors
general chemistry laboratory without incident during the afternoon, but a fire was discovered in the lab two hours after everyone had left. It
destroyed the wooden drawers beneath a stone benchtop before being extinguished by the fire department.
Investigation revealed that the three chemicals used are stable when mixed dry, and react as expected when in dilute solution. However, when 0.5 g of
each are mixed together, and between one drop and 3 mL of water added, a very exothermic reaction occurs with considerable fuming. All three chemicals
are needed for this to initiate. When carried out on a piece of filter paper, ignition of the paper occurred.
We suspect that in the teaching laboratory, dry chemicals were spilled during weighing, and, rather than being disposed of in the aqueous heavy-metal
waste container, were placed in a trash can. This was stored under a sink with a leaky drainpipe, and the critical amount of moisture set off the
reaction after everyone had left the room.
There is a safety warning in the experimental procedure regarding bromates being strong oxidizing agents and indicating that mixtures with finely
divided organic materials are easily ignited. The catalytic nature of the cerium salt on this is not indicated, however. We alert people to the
hazardous nature of this particular mixture, under conditions that are not unusual.
Return to List of Safety Letters
Return to Chemical & Engineering News Home Page
--------------------------------------------------------------------------------
This page last revised December 7, 1998
© Copyright 1998 by the American Chemical Society
Interesting!
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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darkurza
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Calcium Chloride + Water should give a small exothermic reaction. I believe CaCl2 is road salt.
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Maya
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Calcium Chloride + Water should give a small exothermic reaction. I believe CaCl2 is road salt.>>>>>>>
No, that is an ENDOTHERMIC rxn which is less heat = more cold,
EXOTHERMIC is the opposite
\"Prefiero ser yo extranjero en otras patrias, a serlo en la mia\"
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UnintentionalChaos
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Actually, dissolving CaCl2 is exothermic. Try it out. It's part of the reason it's sold as ice-melt for driveways. I remember reading that making a
saturated solution can bring the temperature up to about 54C (not near boiling, but unexpectedly hot). Ammonium Nitrate will give you the dead
opposite. Sold as instant, one-use ice packs.
[Edited on 1-4-07 by UnintentionalChaos]
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Aqua_Fortis_100%
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| Quote: | originally posted by Ozone:
On the same tangent is the slow (dropwise) addition of dilute H2O2 to common household bleach. Here, the H2O2 is oxidized by the NaOCl (5.9% diluted
1:1) to immediately yield O2 and NaCl (some NaClO3 is also likely formed). The Resulting O2 could be used as is to spin a small turbine...or, it could
be combined with H2 or some other fuel (which is risky because H2:O2 mixtures can spontanously ignite or explode if the proportions of each are not
correct (bad, but fun idea!). Whew, oxyhydrogen is *really* hot.
|
VERY CARE when handling H2O2,specially conc. solutions...is just a very tracherous thing...
e.g. the reaction with conc. Na2S solution still was more violent..just thrown off almost making a mini boom and falling in my right eye..just when i
not using goggles...then i washed quickly with TONS of water.. BAH! lucky i'm not blind...
another hot (but bad )thing is put a pinch of MnO2 from dry cell baterries (or KMnO4) in some mls of conc. H2O2(i used 20ml of 50%) ...is REALLY a
good thing if you use the goggles.. and keep distance.. the bottle with the stuff instantly turns very hot and the Black H2O2 decomposing foams may
even to overflow of big bottles...
one time i (remotelly) put some alcohol in the conc. H2O2 and throw a lighted match in it..instantly throw also the MnO2 pinch.. run to behind of my
"shield" and observed (with goggles).. at the start ,isn't much violent but it's will be turns more and more violent after each second which pass...
small explosions.. and finishes in a more violent BOOM....i think which O2 released from H2O2 decomposing turns alcohol burns MUCH more violent..even
with explosions...
so again Yntarius, VERY , GREAT CARE when handling with H2O2..remember which its can also forms a "exothermic reaction" with your skin, "burning" them
with a white stain...
[Editado em 5-1-2007 por Aqua_Fortis_100%]
"The secret of freedom lies in educating people, whereas the secret of tyranny is in keeping them ignorant."
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Ozone
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Try (NH4)6Mo7O24. This is the catalyst** used (in conjunction with a trap-H2SO4 and KI) for the titrimetric assay vs. Na2S2O3.
MnO2 is fantastic (in terms of kinetics--this has to do with multiple (and high) oxidation states).
Fe3+ works, but sucks (Fenton, I know, but quite slow, by comparison, on a mol/mol basis).
As for safety, just don't tempt Lord Darwin. Wear gloves and safety glasses--at the very least 30-50% will instantly turn skin into ashy, white
leather (and catch some things on fire... ).
Reasonable dilution, good safety practice, slow addition, and *yark* common sense is key when handling strong H2O2.
Have fun, be safe (2 eyes, 10 fingers = good),
O3
[Edit] ** nevermind blood, with both the Fe and catalase (where's Chemoleo? I can go through this, but I fathom that the Biochemist might paint a more
colorful and informative picture...).
[Edited on 5-1-2007 by Ozone]
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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Aqua_Fortis_100%
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is a tipical thing which i wish keep distance ehehe...
Ozone, what the MOST tracherous and hazardous exothermic reaction which you made???
now i'm curious..
"The secret of freedom lies in educating people, whereas the secret of tyranny is in keeping them ignorant."
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Ozone
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| Quote: | Originally posted by Aqua_Fortis_100%
is a tipical thing which i wish keep distance ehehe...
Ozone, what the MOST tracherous and hazardous exothermic reaction which you made???
now i'm curious.. |
It is really quite stable--It is a solution of ammonium molybdate made with NH3OH and water. It can be kept in very concentrated form (if refrigerated
without air or light). It *is* a very efficient catalyst for decomposing H2O2, however.
As for the most exothermic reaction I've done/seen..that requires some thought as I have seen a few good ones. the first that comes to mind is
2,4-sec-butyl-dinitrophenol and concentrated sulfuric acid. The best part is the "quiet" induction period before the exotherm...
Sniff with care, my friend,
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
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Aqua_Fortis_100%
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Thanks Ozone...
when in (VERY near) future , i try this in High school. home lab should be a good thing to try reactions of this type..
this "2,4-sec-butyl-dinitrophenol" seems to me as a explosive and poisoning material, because of "dinitrophenol" termination... i will search this..
[Editado em 5-1-2007 por Aqua_Fortis_100%]
[Editado em 5-1-2007 por Aqua_Fortis_100%]
"The secret of freedom lies in educating people, whereas the secret of tyranny is in keeping them ignorant."
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