Ammonia decomposes

The unstable ammonium ozonide [12161 -20-5] NH O, prepared at low temperatures by reaction of ozone withHquid ammonia, decomposes rapidly at room temperature to NH NO, oxygen, and water (51). Tetrametbylammonium ozonide [78657-29-1] also has been prepared. 

All amines, except for ammonia, decompose under high temperature and pressure boiler conditions. Where hydrazine feed continues to be well in excess of scavenging needs or at pressures exceeding 800 to 850 psig (520-525 °F/271-274 °C), it begins to break down and liberate ammonia. All other functioning vapor-phase amines rapidly decompose at temperatures above 550 °F/288 °C (approximately 1,000 psig). 

Most of the reactions that we shall consider are either first or second order in each reactant, but some reactions have other orders (different values of a in Hq. 3). For example, ammonia decomposes into nitrogen and hydrogen on a hot platinum wire ... 

How do we get the temperature of the system to rise By adding heat. When we add heat, this equilibrium system reacts to reduce that stress, that is, to use up some of the added heat. It can use up heat in the reverse reaction, the decomposition of ammonia to hydrogen and nitrogen. When the substances written as products of the reaction (on the right side of the equation) react to produce more reactants (on the left side of the equation), we say that the reaction has shifted to the left. When the opposite process occurs, we say that the equilibrium has shifted to the right. Thus, raising the temperature on this system already at equilibrium causes a shift to the left some of the ammonia decomposes without being replaced. 

Colorless or translucent bard crystalline mass or white cubic crystals or powder sharp taste odor of ammonia decomposes at 58°C slow decomposition at ambient temperatures readily dissolves in cold water decomposes in hot water insoluble in liquid ammonia, alcohol and carbon disulfide. 

White or slight yellow prismatic granules deliquesc density 1.915 g/cm melts at 440°C decomposition starts at 350°C very soluble in water, 281 g/lOOmL at 0°C much more soluble in boiling water, 413 g/lOOmL at 100°C aqueous solution is alkaline slightly soluble in cold alcohol but moderately solublel in hot alcohol very soluble in hquid ammonia decomposes in acids, liberating brown NO2 fumes. 

Colorless crystals triclinic structure density 2.435g/cm3 at 13°C melts above 315°C decomposes on further heating soluble in water, 28.6 g/lOOmL at 25°C highly soluble in boiling water, lOOg/100 mL at 100°C aqueous solution strongly acidic, pH of 0.1 M solution 1.4 insoluble in liquid ammonia decomposed by alcohol into sodium sulfate and sulfuric acid... 

Hydrazulmin. C6H6N6, mw 162.16, N 51.83%, soot-black shiny leaflets. Prepd from cyanogen dry ammonia. Decomposes on heating to give paracyano-gen decomp in water Ref Beil 2, 553... 

Ammonia decomposes on zeolites (9), and the effect of this decomposition on the chlorobenzene reaction may be important. Thus, the activity of CuY zeolite for ammonia decomposition was studied. Helium was used as a carrier gas, 1 ml of ammonia was injected, and the extent of ammonia decomposition was determined as a function of temperature. The decomposition was 2.4% at 350°C, 7.8% at 450° C, and 24% at 550° C. The apparent activation energy of ammonia decomposition was estimated at 13 kcal/mole. The activation energy of ammonia decomposition is close to that of benzene formation from chlorobenzene and ammonia. Thus, benzene formation results from the reaction of chlorobenzene and hydrogen formed by the decomposition of ammonia. 

Solutions of cyanates give with AgN03, white precipitate—AgCNO, soluble in ammonia decomposed by acids with liberation of C02 and formation of an ammonium salt. 

As mentioned earlier a common way to synthesize nitrides is by reactions of ammonia with oxides. At T 823 K ammonia decomposes into active species which can both reduce and nitride to form oxynitrides or nitrides. 

Figure 6. Absorption spectrum of potassium amide in liquid ammonia (

The 15% of ammonia produced does not seem a great deal. The reason for this is the reversible nature of the reaction. Once the ammonia is made from nitrogen and hydrogen, it decomposes to produce nitrogen and hydrogen. There comes a point when the rate at which the nitrogen and hydrogen react to produce ammonia is equal to the rate at which the ammonia decomposes. This situation is called a chemical equilibrium. Because the processes... 

Janssen [74] carried out TPR experiments of M0O3 and V2O5 by ammonia and hydrogen. It was concluded that ammonia reduces the oxides forming almost exclusively water and nitrogen. Both catalysts are reduced below 873 K. Above this temperature ammonia decomposes into N2 and H2. 

Properties Violet, deliquescent crystals. D 2.4. Soluble in water and ammonia decomposed by alcohol. 

JVa = JVa ). If the reaction proceeds backwards (i.e., ammonia decomposes into nitrogen and hydrogen), then has a negative value. 

Basicity is not important for compounds that can be aminated under homogeneous conditions. Many weak bases with n-electron deficiency can be easily aminated in liquid ammonia at low temperature (Section 11,A,3 and 4). Highly TT-electron-deficient compounds, such as quinoxaline, pyrazine, pyridazine, and triazine, although readily aminated in liquid ammonia, decompose when aminated under heterogeneous conditions at elevated temperatures (86MI1). An exception is the successful amination of 5-methylpyri-midine under heterogeneous conditions (Section IV,D) (84EUP0098684A2). 

A decrease in pressure allows the volume to expand. The equilibrium composition shifts to the left and ammonia decomposes to form more nitrogen and hydrogen. 

ANTIMONIC CHLORIDE (7647-18-9) Decomposes on contact with acids, water, or other forms of moisture, producing fumes of hydrogen chloride and antimony pentoxide. Violent reaction with alkalis, ammonia. Decomposes in heat above 171°F/77°C, forming chlorine and antimony trichloride. Attacks many metals in the presence of moisture, forming explosive hydrogen gas. Reacts with air, forming heavier-than-air corrosive vapors. 

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