Aluminum reactions

Methylene chloride is one of the more stable of the chlorinated hydrocarbon solvents. Its initial thermal degradation temperature is 120°C in dry air (1). This temperature decreases as the moisture content increases. The reaction produces mainly HCl with trace amounts of phosgene. Decomposition under these conditions can be inhibited by the addition of small quantities (0.0001—1.0%) of phenoHc compounds, eg, phenol, hydroquinone, -cresol, resorcinol, thymol, and 1-naphthol (2). Stabilization may also be effected by the addition of small amounts of amines (3) or a mixture of nitromethane and 1,4-dioxane. The latter diminishes attack on aluminum and inhibits kon-catalyzed reactions of methylene chloride (4). The addition of small amounts of epoxides can also inhibit aluminum reactions catalyzed by iron (5). On prolonged contact with water, methylene chloride hydrolyzes very slowly, forming HCl as the primary product. On prolonged heating with water in a sealed vessel at 140—170°C, methylene chloride yields formaldehyde and hydrochloric acid as shown by the following equation (6). 

Fig. 10. Sorption of phosphate (P04) (A) and desorption of arsenate (As04) (B) from two samples formed at pH 7.0 and R = 0.1, obtained coprecipitating aluminum and arsenate (7R0.1) or by adding arsenate (7AR0.1) immediately after the precipitation of aluminum. Reaction time was 24 hours. Redrawn from Violante et al. (2006).

In reaction (b) an ionic exchange and solubilization of the aluminum species takes place. In reaction (c) only the solubilization of neutral aluminum species takes place. If the chemical treatment with acid in the two-step process also involves the solubilization of framework aluminum, reaction (a) takes place. 

It seems necessary at this time to emphasize that the above generalizations may pertain only as concerns O-H-N-O explosives and that diametrically opposed conclusions may apply to aluminized mixtures. Evidence is available that kinetic factors (which extend far beyond the time of the C-J condition), rather than thermodynamic factors, govern the extent of utilization of aluminum m the detonation. If, as seems reasonable, the rates of the aluminum reactions are highly temperature dependent, and if aluminum reacts at different rates with HaO, CO, and COa, detonation properties of aluminized explosives should depend very strongly on exact equilibrium compositions of these species in the C-J condition and in the early stages of the gas expansion. For such reasons, Eqs. (1) and (7) may be inapplicable for use with aluminized mixtures. 

Modeling of Inorganic Reactions 174 Nitrogen Reactions 174 Phosphorus Reactions 177 Potassium Reactions 181 Aluminum Reactions 183 Modeling of Soil-Pesticide Interactions 183 Modeling of Organic Pollutants in Soils 186 Supplementary Reading 189... 

We also have to multiply the aluminum reaction by 2 and the magnesium reaction by 3. Notice, however, that we do not multiply their potentials. 

Bond type Neutral aluminum Reaction type... 

Ziegler and Gellert (6) in 1949 showed that aluminum hydride reacts with ethylene at 60-80 °C to yield triethylaluminura. At 100-120 C reaction with additional ethylene leads to formation of higher alkyls of aluminum (Reaction 1). At temperatures above 120 C higher aluminum alkyls react with ethylene through a... 

ELAIC ACID (II2-80-I) Combustible liquid (flash point 372°F/I89°C cc). An organic acid. Reacts, possibly violently, with strong oxidizers, alkalis, ammonia, aliphatic amines, alkanolamines, alkylene oxides, finely divided aluminum, epichlorohydrin, isocyanates, perchloric acid, sulfuric acid. Increases the explosive sensitivity of nitromethane. Attacks aluminum reaction may be violent when this material is peroxidized. 

A1(CH3NNNCH3), tris(l,3-dimethyltriazeno)aluminum Reaction with CUCI/NH3 8, 4.7.2.1 C H.gAlj... 

X on the electrophilic carbon atom (Figure 5). Since carbon is more electronegative than aluminum reaction would proceed by a), but due to the stcric hindrance (since branched alkyl groups are used) decay of the complex proceeds by b). The alkoxide may be produced in situ from aluminum trichloride and ether. This reaction proceeds in a similar way through the Lewis adduct, followed by nucleophilic displacement on carbon (Figure 6). 

Figure 5.4 Main reaction products at 10 bar (a) and adiabatic flame temperatures (b) of aluminum reaction with nitrogen.

Fig. 112. The microfabricated inductively coupled plasma-on-a-chip system is shown from the side and the top. The system includes a generator that is microfabricated on a glass wafer and a miniature aluminum reaction chamber. Reproduced with permission from Ref [492].)...

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