Sciencemadness Discussion Board
Not logged in [Login ]
Go To Bottom

Printable Version  
 Pages:  1  2  
Author: Subject: What do to with KMnO4?
Lambda
International Hazard
*****




Posts: 566
Registered: 15-4-2005
Location: Netherlands
Member Is Offline

Mood: Euforic Online

[*] posted on 13-8-2005 at 19:04
Women used Potassium permanganate to abort a baby


A old drugstore owner that I know, used to sell Potassium permanganate to women that wanted to abort an unwanted baby. They dissolved the Potassium permanganate in water, and with this solution they performed a vaginal rince. Not only the featus was murderd in this way, but these foolish women also became infertill if they where unlucky. The vaginal damage, was often irreversible. But remember, this was done a long time ago in Holland in a periode that it was unheard of, if a women became pregnant before marriage. They were treated as whores, and band from there villages, for they were a shame to the family and community. Prostitutes used the same procedure for an abortion. :mad: Things have changed since, for many women have children and are not married. They are not looked down on anymore.:)

[Edited on 15-8-2005 by Lambda]
View user's profile View All Posts By User
praseodym
Hazard to Others
***




Posts: 137
Registered: 25-7-2005
Location: Schwarzschild Radius
Member Is Offline

Mood: crazy

[*] posted on 13-8-2005 at 21:42


Quote:
Originally posted by Lambda
If you drop a drip of glycerine on a small pile of fine Potassium permanganate, they will spontaneously ignite after a short delay periode.

Caution: At a low temperature, this may take a long time to occure, so don't make the mistake of thinking that nothing will happen, and throw it away in the trashcan (rubishbin). They will eventually ignite !!!

[Edited on 14-8-2005 by Lambda]


I believe this is the equation for the reaction between potassium permanganate and glycerine:
14KMnO4 + 4C3H5(OH)3 ==> 7K2CO3 + 7Mn2O3 + 5CO2 + 16H2O
I believe Mn2O3 is the toxic fumes saps is talking about.
View user's profile View All Posts By User This user has MSN Messenger
unionised
International Hazard
*****




Posts: 4968
Registered: 1-11-2003
Location: UK
Member Is Offline

Mood: No Mood

[*] posted on 14-8-2005 at 12:49


How likely is it that all 18 molecules of reactants in that equation will get together in the right proportions?
The fumes are likely to contain acrolein (formed from hot glycerine) among other compounds.
View user's profile View All Posts By User
neutrino
International Hazard
*****




Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline

Mood: oscillating

[*] posted on 14-8-2005 at 15:24


It would probably be a multi-step reaction.
View user's profile View All Posts By User
The_Davster
A pnictogen
*******




Posts: 2861
Registered: 18-11-2003
Member Is Offline

Mood: .

[*] posted on 14-8-2005 at 15:26


It would definatly be multi step...Any reaction that involves more than 4 molecules colliding is nearly statistically imposible.



View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 15-8-2005 at 13:48


I believe that finely divided metal can float in the air even at modest temps. Particle size determines how dangerous they are. Inhaling such particles causes a fever. Different names apply (silicosis, smoke inhalation, welder's fever, etc) depending on what material has been inhaled. If this is true it probably isnt a good idea to heat potasium permangate without a mask...But do you think tyhat prolonged exposure to potasium permanganate and Glyceron reaction could be harmful.



Also: this is kind of off subject but does anybody else know of any chemical reactions that create spontaneous heat/flames?
View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 15-8-2005 at 15:36


the reaction should also not involve very toxic chemicals
View user's profile View All Posts By User
12AX7
Post Harlot
*****




Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline

Mood: informative

[*] posted on 15-8-2005 at 16:27


Quote:
Originally posted by saps
Also: this is kind of off subject but does anybody else know of any chemical reactions that create spontaneous heat/flames?


Uh, any reaction that has a positive enthalpy, thus releasing heat.

If you mean reactions that start at room temperature, mineral acids and reactive metals (iron, zinc, aluminum, etc.) work. Very reactive metals (magnesium, calcium, sodium, etc.) react with water at room temperature, some (sodium, potassium..) fast enough to ignite the nascent hydrogen produced. Hydrogen and oxygen ignite over a platinum catalyst. Sulfuric acid can be dropped on a sugar + chlorate mixture to ignite it. What else?

Tim




Seven Transistor Labs LLC http://seventransistorlabs.com/
Electronic Design, from Concept to Layout.
Need engineering assistance? Drop me a message!
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
The_Davster
A pnictogen
*******




Posts: 2861
Registered: 18-11-2003
Member Is Offline

Mood: .

[*] posted on 15-8-2005 at 16:48


Mn2O7 + anything :P

sodium peroxide + toilet paper + water

alkali metal +water

silver nitrate/magnesium flash + water

ammonium nitrate/ammonium chloride/zinc + water




View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 15-8-2005 at 17:38


when you state "ammonium nitrate/ammonium chloride/zinc + water " do you meen" ammonium nitrate,ammonium chloride,zinc and water all together
View user's profile View All Posts By User
The_Davster
A pnictogen
*******




Posts: 2861
Registered: 18-11-2003
Member Is Offline

Mood: .

[*] posted on 15-8-2005 at 17:42


I used the slash to indicate that they are already mixed together, then whatever follows the + sign is added.



View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 15-8-2005 at 18:02


12AX7, is there anything i can substitute for sulfuric acid, in the reaction that involves sucrose, a chlorate, and sulfuric acid?
View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 15-8-2005 at 18:27


what about reactions between reducing agents and oxidizing agents
View user's profile View All Posts By User
chemoleo
Biochemicus Energeticus
*****




Posts: 3005
Registered: 23-7-2003
Location: England Germany
Member Is Offline

Mood: crystalline

[*] posted on 15-8-2005 at 18:52


Quote:

what about reactions between reducing agents and oxidizing agents

Oh boy, don't hijack that thread for some shitty oxidiser /reductant questions please.
There are so many it'd be worth 100 threads.
I am very much tempted to close this thread, it started off well but now it's veering off into a random 'what burns' and 'what doesn't' thread.

Saps, take a break, search the forums and then come back!




Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 16-8-2005 at 09:18
Reducing agents


I'm playing around with kmno4 and its exothermic abillities to oxidize materials. right now i am oxidizing glyceron. what other reduction agents will oxidize as well as glyceron?
View user's profile View All Posts By User
solo
International Hazard
*****




Posts: 3888
Registered: 9-12-2002
Location: Estados Unidos de La Republica Mexicana
Member Is Offline

Mood: ....getting old and drowning in a sea of knowledge

[*] posted on 16-8-2005 at 10:06
oxidation reactions


First off some of the properties of the glycerin you're trying to oxidise........

http://www.sy-kogyo.co.jp/english/sei/1_gly.html

second ,

A dramatic, yet safe demonstration of an exothermic reaction and the strong oxidizing properties of potassium permanganate. Students will observe smoke and fire as glycerine is oxidized to produce carbon dioxide and water. A great amount of heat is liberated by this oxidation-reduction reaction.




here ia a list of incompatibles.....such as this

potassium permanganate: incompatible with,( ethylene glycol, glycerin, benzaldehyde, sulfuric acid )

found here......
http://chemistry.allinfoabout.com/features/incompatible.html

ans here is a link in this forum of what else can be done with Potassium Permanganate....

https://sciencemadness.org/talk/viewthread.php?tid=4251

which is probably where you should have started once searching for it with the search engine.....instead of starting a new thread......maybe the thread can be merged there........oh well I hope the information will assist you .................solo

[Edited on 16-8-2005 by solo]




It's better to die on your feet, than live on your knees....Emiliano Zapata.
View user's profile View All Posts By User
saps
Hazard to Self
**




Posts: 82
Registered: 7-3-2005
Location: New Britian
Member Is Offline

Mood: disgruntled

[*] posted on 16-8-2005 at 10:34
PROPYLENE GLYCOL


would PROPYLENE GLYCOL work as well as ethylene glycol
View user's profile View All Posts By User
12AX7
Post Harlot
*****




Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline

Mood: informative

[*] posted on 16-8-2005 at 14:09


Isn't propylene g.ol just glycerin?.... :o

Tim




Seven Transistor Labs LLC http://seventransistorlabs.com/
Electronic Design, from Concept to Layout.
Need engineering assistance? Drop me a message!
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
chemoleo
Biochemicus Energeticus
*****




Posts: 3005
Registered: 23-7-2003
Location: England Germany
Member Is Offline

Mood: crystalline

[*] posted on 16-8-2005 at 14:19


No it is CH3-CH2OH-CH2OH. Usually.

And yes, it is likely to work, too.
Like many others. Did you read solo's post, and did you check KMnO4 MSDS's to find incompatibles? Any liquid alcohol, or generally liquid org. chems with reactive oxidisable groups are likely to work with it.




Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
View user's profile View All Posts By User
neutrino
International Hazard
*****




Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline

Mood: oscillating

[*] posted on 16-8-2005 at 17:06


Glycol means two OHs, not one for every carbon.
View user's profile View All Posts By User
12AX7
Post Harlot
*****




Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline

Mood: informative

[*] posted on 16-8-2005 at 18:18


Ah, okay. So decylene glycol would be CH3(CH2)8CHOHCH2OH? I take it the OH have to be adjecent, otherwise it's a regular diol?

Tim




Seven Transistor Labs LLC http://seventransistorlabs.com/
Electronic Design, from Concept to Layout.
Need engineering assistance? Drop me a message!
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
Lambda
International Hazard
*****




Posts: 566
Registered: 15-4-2005
Location: Netherlands
Member Is Offline

Mood: Euforic Online

[*] posted on 16-8-2005 at 18:20
Making Nitric acid with Potassium permanganate, Ammonia gas and recycling the process with Air (Oxygen) ???


I have forgotten the title of this book, but I think it was written by Robert Gatling. The Paladine Press once published it, and I have the book. When I find it, a scan will be made.

What doese the author of this book claime ?:

According to the author of this book, Nitric acid can be made by bubbling Ammonia gas through a solution of Potassium permanganate. The Ammonia gas is oxidized to Nitric acid in this way. Potassium permanganate may again be obtained by bubbling Air (Oxygen) through this solution (?). And thus, the whole process may be repeated, by only applying Ammonia gas, and again recycling with Air. A continuos process, may thus be astablished for the production of Nitric Acid.:cool:

Do you think that this process is feasible ?
View user's profile View All Posts By User
neutrino
International Hazard
*****




Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline

Mood: oscillating

[*] posted on 16-8-2005 at 18:41


We can't really judge the process without some sense of the reactions that take place. Can you give us some more background?
View user's profile View All Posts By User
12AX7
Post Harlot
*****




Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline

Mood: informative

[*] posted on 16-8-2005 at 19:25


Sounds like, ahh, let's see here. Well Mn could go from +7 to +6 (only stable in base), +4 (MnO2 ppt) or +2 (Mn2+ ion) depending on maybe pH and reactants.

I'm guessing e.g.
6KMnO4 + 4NH3 = 6KMnO2 + 4NO3- + 6H2O, which ends up basic, ready for MnO4- regeneration with O2.

It could work. How long can you go until the acidity kills it and forms Mn(NO3)2 or such?

Tim




Seven Transistor Labs LLC http://seventransistorlabs.com/
Electronic Design, from Concept to Layout.
Need engineering assistance? Drop me a message!
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
Lambda
International Hazard
*****




Posts: 566
Registered: 15-4-2005
Location: Netherlands
Member Is Offline

Mood: Euforic Online

[*] posted on 16-8-2005 at 20:07


Neutrino, I don't have this book at hand. But what I can say, is that the information that I have given above, is about all that was mentioned in this book.
View user's profile View All Posts By User
 Pages:  1  2  

  Go To Top