Toxic-gas liberating explosives

Sorry to blow your theory and to send all those reactions down the drain, but phosgene is thermodynamically unstable and decomposes above 300C....

Exactly how does it decompose (equation please)?

Whaddaya think?
COCl2 -> CO + Cl2 duh......

Tsss, all those equations above and you can't figure out this one?

I have no idea why I asked that question. *smacks forehead*

How about a binary of H2 and F2 gas? They still react explosively at -200C to form HF, an extremely toxic gas.
Only problem is where to get the fluorine gas.

hehe, even better, an explosive that liberates H2 and F2 so they too explode and then form HF. pretty sick

Sorry Madscientist, but many of the equations you have given are right theorically but practically they are unfeasible or wrong!

5CH2Cl2 + 2NaNO3-->Na2O + N2 + 5CO + 10HCl
5CH2Cl2 + 4NaNO3-->2Na2O + 2N2 + 5H2O + 5COCl2
10CH2Cl2 + 12NaNO3-->6Na2O + 6N2 + 20HCl + 10CO2 + 5O2

Are absolutely wrong! CH2Cl2 boils at 40°C and the volatilisation cools down the reaction very fast; also CH2Cl2 is not very flamable, it only reacts violently with Al ultrafine powder, solid Na or K!
Also:
2HCl + 1/2O2 --> H2O + 1/2Cl2
Na2O + 2HCl --> 2NaCl + H2O
Na2O + CO2 --> Na2CO3
Na2O + Cl2C=O --> 2NaCl + CO2

CCl3-CO-NH-NO2 should be very unstable -maybe so unstable that it doesn't exists; because CCl3 is first a very electroatractive group (thus CCl3-CO- is rather acidic); a good leaving group too, nitramides are much less stable than nitramines; here you have a molecule that should be as (if not more) unstable than dinitrourea.
CCl3-CO-OCH2-CH3 + NH3(dry) -solvant-> CCl3-CO-NH2 + CH3-CH2-OH
But
CCl3-CO-OCH2-CH3 + NH4OH --> CCl3-CO2NH4 + CH3-CH2OH

Finally:
(CH2OH)2 + 2HCl --(H2SO4)--> (CH2Cl)2 + 2H2O
You forgot:
+(CH2O)2SO2 + (CH2)2O + HO-CH2-CH2-Cl

(CH2Cl)2 + 2HNO3 --(H2SO4)-->(CHClNO2)2 + 2H2O
Unfortunately no; aliphatic nitrocompounds aren't made the same way as alcenic/benzenic nitrocompounds!


(CHClNO2)2 + 2Cl2 -->(CCl2NO2)2 + 2HCl
The first one is already very dangerous and unstable see related compounds like CH2Cl-NO2 and CHCl2-NO2!

3(CCl2NO2)2 + 2Na3P --> (CClNO2)6P2 + 6NaCl
Why not, possible, no fuking ID!

(CClNO2)6P2 --> 2CO + CO2 + 3N2 + P2O5 + 3COCl2
Might be P2O3, N2, CO2, CO and Cl2!

CH2Cl2 + HNO3 --(H2SO4)--> CHCl2NO2 + H2O
Maybe at under pressure boiling at reflux (with very big risks of explosion (CH2Cl-NO2 and CHCl2-NO2).

2CHCl2NO2 --> N2 + CO2 + COCl2 + H2O
Nothing new under the sun; it is known for ages that halonitrocarbons like Trinitrotrichlorobenzene, chloropicrine (CCl3-NO2-toxic on its own), haloalkanes mixed with oxydisers like peroxydes, NH4NO3, N2O4, O3, liq O2; H2O2, HNO3 conc, HClO4 conc, ... do produce some free halide, CO and traces of X2C=O + H2O and HX!

CH3CH2OH + 3Cl2 --> CCl3CH2OH + 3HCl
I'm almost sure that will never go this way, but more this way:
CH3-CH2OH + Cl2 --> CH3-CH=O + 2HCl
CH3-CH=O + Cl2 --> CH2Cl-CH=O + HCl
CH3-CH=O <--> CH2=CH-OH
CH2=CH-OH + Cl2 --> CH2Cl-CHClOH
CH2Cl-CHClOH --> CHCl=CHCl + H2O
CH2Cl-CHClOH --> CHCl=CHOH <--> CH2Cl-CH=O
...--> CHCl2-CHCl2 and CCl3-CH=O (chloral)
The action of NaOCl (Javel water) on ethanol provides partially chloral hydrate.

CCl3CH2OH + HNO3 --(H2SO4)--> CCl3CH2NO3 + H2O
CCl3-CH2O- must be quite acidic and thus the ester will not be stable, maybe doesn't exist!

CCl3CH2NO3 --> 3COCl2 + CO + 2H2O + N2

CH3COOH + 3Cl2 --> CCl3COOH + 3HCl
This one is true

(CH2OH)2 + HF --(H2SO4)--> (CH2OH)(CH2F) + H2O
And also (CH2F)2!

(CH2OH)(CH2F) + 4Cl2 --> (CCl2OH)(CCl2F) +4HCl
See the reaction of ethanol with Cl2 and extrapolate to this twin brother!

(CCl2OH)(CCl2F) + CH3CH2OH --(H2SO4)--> (CCl2OCH2CH3)(CCl2F) + H2O
Why not!
(CCl2OCH2CH3)(CCl2F) + NH3 --> (CCl2NH2)(CCl2F) + CH3CH2OH
Maybe, maybe not; possible reaction of the halide with the amine...cf CH3-NH2 with CH3-Cl
--> CH3-NH2Cl-CH3 --> (CH3)3NHCl --> (CH3)4NCl

(CCl2NH2)(CCl2F) + HNO3 --(H2SO4)--> (CCl2NHNO2)(CCl2F) + H2O
Primary amine doesn't form nitramines in presence of H2SO4...do you do RDX with H2SO4/HNO3 or with HNO3 conc with other dehydratants than H2SO4? True that H2SO4 is used in NITRAMIDES synthesis not in nitraMINes!
(CCl2NHNO2)(CCl2F) --> 2COCl2 + HF + N2

3CH3CHO + 3H2O2 --(H2SO4)--> (CH3CHOO)3 + 3H2O
I like the idea, but nowhere I have seen any mention of acetaldehyde peroxyde; nor of formol peroxyde!This must mean they are so unstable they decompose immediately at ambiant T or while forming!

(CH3CHOO)3 + 12Cl2 --> (CCl3CClOO)3 + 12HCl
It would be more like: --> HCCl3 + H2O + HCl + CO2 + CCl3-CH=O + CH3-CO2H + CCl3-CO2H

(CCl3CClOO)3 --> 6COCl2
Noway; but CH3-CO-CH3 --> ClCH2-CO-CH3 and ClCH2-CO-CH2Cl that may form a CTAP brother halogenated that will free traces of phosgene
Those halogenated CTAP will have higher densities, better oxygen balance (since Cl2 is an oxydiser) and thus display higher VODs!
Haloacetons are very reactive compounds they can polymerise explosively on their own, they are strong lacrymator and must be suffocating gases like any halogen reactive containing compound (Cl-CN, Cl2, Cl2C=O, Cl2O, ClO2, Cl2S, TiCl4, AlCl3, NCl3, ....).

CH3CHOHCH2CH3 + HClO4 --> CH3CHClO4CH2CH3 + H2O
True but perchloric ester are spontaneously detonating compounds at ambiant T!

CH3CHClO4CH2CH3 + 9Cl2 --> (CCl3)(CCl)(ClO4)(CCl2)(CCl3) + 9HCl
Detonation will occure before the molecule has any chance to react that far!
(CCl3)(CCl)(ClO4)(CCl2)(CCl3) --> 4COCl2 + Cl2
No comments!

(CH2OH)2 + 2HCl --> (CH2Cl)2 + 2H2O
True!

(CH2Cl)2 + HNO3 --(H2SO4)--> (CHNO2Cl)(CH2Cl) + 2H2O
Only under vapour phase at high T (400°C) no need of H2SO4!

213 new ideas

chemical structure

Sorry, the picture was not submited in my last post !

Krypton,
Do you have any reference for the building bloc of your idea?
cyclo(-NH-CHNO2-CHNO2-CHNO2-CHNO2-)
Should be hell of a good explosive on its own...especially the nitramine... perfect OB
O2N-N(CHNO2-CHNO2)2 --> 4CO2 + 2H2O + 5/2N2

High density but must be sensitive!

Holy shit, that would be a lethal radius of 12.9 m or over 42 ft. If you wer considering a hemisphere instead of a sphere, that would be a radius of 16.3 m or over 53 ft.

I sincerely hope all of this is hypothetical.

"Nitrogen trichloride, also called nitrogen chloride, agene, chlorine nitride, trichloramine, trichlorine nitride, chloride of azode, or Stickstofftrichlorid, is an unstable primary explosive compound. Its preparation is not complicated and the chemicals used are simple, cheap, and readily obtainable. You could pump the stuff out by the liter if it was not so sensitive. Nitrogen trichloride will explode if heated, exposed to sunlight, or mixed with organic compounds. It does not like to be friendly around many other chemicals, shock, sparks, and it will explode if frozen and thawed. The explosive properties were first reported in the 18th century by Sir H. Davy, he had this to say: "The fulminating oil which you mentioned roused my curiosity and nearly deprived me of an eye. After some months of confinement I am again well." Ouch, that must have hurt."

Sounds interesting?
Nitrogen trichloride decomposes like this: 2NCl3->N2 + 3Cl2.
That's how it's made:

"Dissolve 30 g of ammonium nitrate in 70 mL water in a 200-mL Erlenmeyer flask. Prepare a chlorine generator as described in the synthesis section. Place a tube connected to the generator at the bottom of the flask so the chlorine gas can bubble into the liquid, a bubbler will help a lot with the reaction. Gently heat the flask to start the reaction while adding chlorine gas. An oily yellow liquid will begin to appear on the bottom of the flask, that is the nitrogen trichloride. Stop heating the flask when the drops appear. After 20 to 30 minutes the reaction should be complete. Use a medicine dropper to extract the nitrogen trichloride from the flask, transfer it to a small test tube and remove any water accidently sucked up with it. You will need a graduated cylinder for measuring liquids. This explosive will decompose within 24 hours of its preparation."

Quote:

Originally posted by vulture Sorry to blow your theory and to send all those reactions down the drain, but phosgene is thermodynamically unstable and decomposes above 300C....