Nitric-acid-based explosives

Numerous attempts were made to get around the nitric acid problems. At the time, dynamite was well understood, with one variety produced consisting of nitroglycerin absorbed on Kieselguhr (diatomaceous earth). Attempts were made to absorb Hellhoffite on Kieselguhr. Fumes were reduced, but the resulting fill still attacked wrapping paper, wood pulp, metal, and skin. Eventually, the idea of nitric-acid-based explosives was abandoned due to the existence of kinder and gentler alternatives. 

L-PHENYLDECANE (104-72-3) C, H Combustible liquid (flashpoint 225°F/107°C cc Fire Rating 1). Incompatible with strong oxidizers (may be explosive), nitric acid bases, amines, amides, inorganic hydroxides diazo compounds. Attacks some plastics, mbber, and coatings. On small fires, use dry chemical powder (such as Purple-K-Powder), foam, or COj extinguishers. DECYLENE (872-05-9) C,oH Flammable liquid. Forms explosive mixture with air (flash point 116°F/47°C Fire Rating 2). Violent reaction with strong oxidizers, bromine, perchlorates, perchromates, pyridiniiun perchlorate, peroxyacetic acid. 

TETRABUTYL TITANATE (5593-70-4) C,4H]404Ti Combustible organometallic liquid. Forms explosive mixture with air [explosion limits in air (vol %) 2.0 to 12.0 flashpoint 170°F/77°C cc Fire Rating 2]. A reducing agent. Reacts violently with strong oxidizers and many other materials. Reacts with water producing butanol and titanium dioxide, and possibly, toxic or flammable fumes. Incompatible with acids sulfuric acid, nitric acid bases, amines, amides. 

For nitric acid-based liquid explosives, macromolecule monomers, which would be cross-linked to form network structure, are used in thickening methods [24]. The initiator should be capable of generating free radicals at low temperatures in the course of the reaction. Ammonium peroxydisulfate is able to be an initiator. The initial radial reaction is given as ... 

Acid—Base Chemistry. Acetic acid dissociates in water, pK = 4.76 at 25°C. It is a mild acid which can be used for analysis of bases too weak to detect in water (26). It readily neutralizes the ordinary hydroxides of the alkaU metals and the alkaline earths to form the corresponding acetates. When the cmde material pyroligneous acid is neutralized with limestone or magnesia the commercial acetate of lime or acetate of magnesia is obtained (7). Acetic acid accepts protons only from the strongest acids such as nitric acid and sulfuric acid. Other acids exhibit very powerful, superacid properties in acetic acid solutions and are thus useful catalysts for esterifications of olefins and alcohols (27). Nitrations conducted in acetic acid solvent are effected because of the formation of the nitronium ion, NO Hexamethylenetetramine [100-97-0] may be nitrated in acetic acid solvent to yield the explosive cycl o trim ethyl en etrin itram in e [121 -82-4] also known as cyclonit or RDX. 

Ammonia from coal gasification has been used for fertilizer production at Sasol since the beginning of operations in 1955. In 1964 a dedicated coal-based ammonia synthesis plant was brought on stream. This plant has now been deactivated, and is being replaced with a new faciUty with three times the production capacity. Nitric acid is produced by oxidation and is converted with additional ammonia into ammonium nitrate fertilizers. The products are marketed either as a Hquid or in a soHd form known as Limestone Ammonium Nitrate. Also, two types of explosives are produced from ammonium nitrate. The first is a mixture of fuel oil and porous ammonium nitrate granules. The second type is produced by emulsifying small droplets of ammonium nitrate solution in oil. 

Nitric acid is one of the three major acids of the modem chemical industiy and has been known as a corrosive solvent for metals since alchemical times in the thirteenth centuiy. " " It is now invariably made by the catalytic oxidation of ammonia under conditions which promote the formation of NO rather than the thermodynamically more favoured products N2 or N2O (p. 423). The NO is then further oxidized to NO2 and the gases absorbed in water to yield a concentrated aqueous solution of the acid. The vast scale of production requires the optimization of all the reaction conditions and present-day operations are based on the intricate interaction of fundamental thermodynamics, modem catalyst technology, advanced reactor design, and chemical engineering aspects of process control (see Panel). Production in the USA alone now exceeds 7 million tonnes annually, of which the greater part is used to produce nitrates for fertilizers, explosives and other purposes (see Panel). 

NH3. Ammonia is a colorless gas. It is a strong base, forms hydrogen bonds, is soluble in water, and is a fairly reactive molecule. Each year 12.4 million metric tons are manufactured by the Haber process (N2 + 3H2 2NH3 at 400°C and 250 atm), principally for nitric acid production, which is then used to make fertilizers and explosives. As a fertilizer, ammonia can be utilized in three ways first by direct injection... 

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