Ammonia (hydrogen nitride ) is a chemical compound of nitrogen and hydrogen with the formula NH 3 , under normal conditions it is a colorless gas with a sharp characteristic odor.
Ammonia | |
---|---|
Are common | |
Chem. formula | NH 3 |
Physical properties | |
condition | gas |
Molar mass | 17.0306 g / mol |
Density | 0.7723 (n.o.) |
Ionization energy | |
Thermal properties | |
T. melt. | -77.73 ° C |
T. bale. | -33.34 ° C |
T. svpl. | |
Etc. blast | |
Cr. point | 132.25 ° C |
Enthalpy of Education | -45.94 kJ / mol |
Steam pressure | |
Chemical properties | |
pK a | |
Solubility in water | 89.9 (at 0 ° C) |
Classification | |
Reg. CAS number | [7664-41-7] |
PubChem | |
Reg. EINECS number | |
Smiles | |
Inchi | |
RTECS | |
Chebi | |
UN number | |
ChemSpider | |
Security | |
Toxicity | toxic, suffocating |
NFPA 704 | one 3 0 SA |
The density of ammonia is almost half that of air , MPC.z. 20 mg / m3 - hazard class IV (low hazard substances) according to GOST 12.1.007 [4] . The solubility of NH 3 in water is extremely high - about 1200 volumes (at 0 ° C) or 700 volumes (at 20 ° C) in the volume of water. In refrigeration, it is called R717, where R is the Refrigerant ( refrigerant ), 7 is the type of refrigerant (inorganic compound), 17 is the molecular weight.
Ammonia is one of the most important products of the chemical industry ; its annual global production exceeds 180 million tons.
The ammonia molecule has the shape of a triangular pyramid with a nitrogen atom at the top. Three unpaired p-electrons of the nitrogen atom participate in the formation of polar covalent bonds with the 1s-electrons of three hydrogen atoms (N – H bonds), the fourth pair of external electrons is unshared, it can form a covalent bond with a hydrogen ion through a donor-acceptor mechanism , forming an ion ammonium NH 4 + . A non-binding two-electron cloud is strictly oriented in space, therefore, the ammonia molecule has a high polarity, which leads to its good solubility in water.
In liquid ammonia, molecules are interconnected by hydrogen bonds . Comparison of the physical properties of liquid ammonia with water shows that ammonia has lower boiling points (t bales −33.35 ° C) and melting points (t bales −77.70 ° C), as well as lower density and viscosity (7 times less viscosity of water), conductivity (almost does not conduct electric current) and dielectric constant. This is to some extent due to the fact that the strength of hydrogen bonds in liquid ammonia is significantly lower than that of water; as well as the fact that in the ammonia molecule there is only one pair of lone electrons, unlike two pairs in the water molecule, which does not make it possible to form a branched network of hydrogen bonds between several molecules. Ammonia easily passes into a colorless liquid with a density of 681.4 kg / m³, which strongly refracts light. Like water, liquid ammonia is strongly associated, mainly due to the formation of hydrogen bonds. Liquid ammonia is a good solvent for a very large number of organic, as well as for many inorganic compounds. Solid ammonia - cubic crystals.
Chemical Properties
- Due to the presence of an unshared electron pair in many reactions, ammonia acts as a Bronsted base or complexing agent (do not confuse the concepts of “nucleophile” and “Bronsted base.” Nucleophilicity is determined by the affinity for a positively charged particle. The base has an affinity for a proton. The concept of “base” is a special case the concept of "nucleophile"). So, he attaches a proton, forming an ammonium ion :
- An aqueous solution of ammonia (“ammonia”) has a slightly alkaline reaction due to the process:
- K o = 1.8⋅10 −5
- Interacting with acids, gives the corresponding ammonium salts:
- Ammonia is also a very weak acid (10,000,000,000 times weaker than water), able to form salts with metals - amides , imides and nitrides . Compounds containing NH 2 - ions are called amides, NH 2- - imides, and N 3- - nitrides. Amides of alkali metals are obtained by acting on them with ammonia:
Amides, imides and nitrides of a number of metals are formed as a result of certain reactions in liquid ammonia. Nitrides can be obtained by heating metals in a nitrogen atmosphere.
Metal amides are analogs of hydroxides. This analogy is strengthened by the fact that OH - and NH 2 - ions, as well as Н 2 O and NH 3 molecules, are isoelectronic. Amides are stronger bases than hydroxides, and therefore, undergo irreversible hydrolysis in aqueous solutions:
and in alcohols:
Like aqueous solutions of alkalis, ammonia solutions of amides conduct electricity well, due to dissociation:
Phenolphthalein in these solutions turns a crimson color, with the addition of acids, they are neutralized. The solubility of amides changes in the same sequence as the solubility of hydroxides: LiNH 2 - insoluble, NaNH 2 - sparingly soluble, KNH 2 , RbNH 2 and CsNH 2 - highly soluble.
- When heated, ammonia decomposes, exhibits reducing properties. So, it burns in an oxygen atmosphere, forming water and nitrogen. Oxidation of ammonia by air on a platinum catalyst gives nitrogen oxides, which is used in industry to produce nitric acid:
- (reaction reversible)
- (without catalyst, at elevated temperature)
- (in the presence of a catalyst, at elevated temperature)
- (without catalyst, at elevated temperature)
- (reaction reversible)
The NH 3 Cl ammonia is used on the reducing ability of NH 3 to clean the metal surface from oxides during their soldering:
Oxidizing ammonia with sodium hypochlorite in the presence of gelatin, hydrazine is obtained:
- Halogens (chlorine, iodine) form dangerous explosives with ammonia - nitrogen halides (nitrogen chloride, nitrogen iodide ).
- With haloalkanes, ammonia enters into a nucleophilic addition reaction, forming a substituted ammonium ion (a method for producing amines):
- (methylammonium hydrochloride)
- With carboxylic acids , their anhydrides , halides, esters and other derivatives gives amides. With aldehydes and ketones , Schiff bases , which can be reduced to the corresponding amines (reductive amination ).
- At 1000 ° C, ammonia reacts with coal to form hydrocyanic acid HCN and partially decomposes into nitrogen and hydrogen. It can also react with methane to form the same hydrocyanic acid:
- With salts of copper and silver forms complex salts of ammonia
History
Ammonia was first isolated in pure form by J. Priestley in 1774 , who called it “alkaline air” ( English alkaline air ) [5] . Eleven years later, in 1785, K. Bertollet established the exact chemical composition of ammonia [6] . Since that time, studies have begun in the world on the production of ammonia from nitrogen and hydrogen . Ammonia was very necessary for the synthesis of nitrogen compounds, since their receipt from Chilean nitrate was limited to the gradual depletion of the latter. The problem of reducing saltpeter reserves worsened by the end of the 19th century. Only at the beginning of the 20th century was it possible to invent an ammonia synthesis process suitable for industry. This was accomplished by F. Gaber , who began to work on this task in 1904 and by 1909 created a small contact apparatus in which he used high pressure (in accordance with the Le Chatelier principle ) and an osmium catalyst . On July 2, 1909, Gaber arranged the tests of the apparatus in the presence of K. Bosch and A. Mittash , both from the Baden Aniline and Soda Plant ( BASF ), and received ammonia. By 1911, C. Bosch created a large-scale version of the apparatus for BASF, and then it was built and on September 9, 1913 the world's first ammonia synthesis plant was put into operation, which was located in Oppau (now the district within the city of Ludwigshafen am Rhein ) and belonged to BASF. In 1918, F. Gaber won the Nobel Prize in Chemistry "for the synthesis of ammonia from its constituent elements." In Russia and the USSR, the first batch of synthetic ammonia was obtained in 1928 at the Chernorechensk chemical plant [7] .
Name Origin
Ammonia (in European languages its name sounds like “ammonia”) owes its name to Ammon's oasis in North Africa , located at the crossroads of caravan routes. In hot climates, urea (NH 2 ) 2 CO, contained in animal waste products, decomposes particularly quickly. One of the decomposition products is ammonia. According to other sources, ammonia got its name from the ancient Egyptian word Amonian . So called people worshiping the god Amon . During their ritualistic rites, they sniffed the ammonia mineral (NH 4 Cl), which evaporates ammonia when heated.
Liquid ammonia
Liquid ammonia, although to a small extent, dissociates into ions (autoprotolysis), which shows its similarity to water :
The self-ionization constant of liquid ammonia at −50 ° C is approximately 10 −33 (mol / L) ².
Liquid ammonia, like water , is a strong ionizing solvent in which a number of active metals dissolve: alkaline , alkaline earth , Mg , Al , as well as Eu and Yb . Unlike water with liquid ammonia, these metals do not react, namely, they dissolve and can be isolated in their original form by evaporation of the solvent. The solubility of alkali metals in liquid NH 3 is several tens of percent. Some intermetallic compounds containing alkali metals, for example, Na 4 Pb 9, also dissolve in liquid ammonia NH 3 .
Diluted metal solutions in liquid ammonia are colored blue, concentrated solutions have a metallic luster and look like bronze . During the evaporation of ammonia, alkali metals are released in pure form, and alkaline-earth metals - in the form of complexes with ammonia [E (NH 3 ) 6 ] with metallic conductivity. With weak heating, these complexes decompose into metal and NH 3 .
The metal dissolved in NH 3 gradually reacts with the formation of amide :
The metal amides resulting from the reaction with ammonia contain a negative ion, NH 2 - , which also forms during the self-ionization of ammonia. Thus, metal amides are analogs of hydroxides. The reaction rate increases with the transition from Li to Cs. The reaction is significantly accelerated in the presence of even small impurities of H 2 O.
Metal-ammonia solutions have metallic conductivity, in which metal atoms decompose into positive ions and solvated electrons surrounded by NH 3 molecules. Metal ammonia solutions, which contain free electrons, are the strongest reducing agents.
Complexation
Due to its electron-donating properties, NH 3 molecules can enter complex compounds as a ligand. So, the introduction of an excess of ammonia into solutions of d-metal salts leads to the formation of their amino complexes:
Complexation is usually accompanied by a change in the color of the solution. So, in the first reaction, the blue color (CuSO 4 ) changes to dark blue (complex color), and in the second reaction, the color changes from green (Ni (NO 3 ) 2 ) to blue-violet. The strongest complexes with NH 3 form chromium and cobalt in oxidation state +3.
Biological role
Ammonia is an important source of nitrogen for living organisms. Despite the high content of free nitrogen in the atmosphere (more than 75%), very few living creatures are able to use free, neutral diatomic nitrogen in the atmosphere, gas N 2 . Therefore, to include atmospheric nitrogen in biological circulation, in particular in the synthesis of amino acids and nucleotides , a process called “ nitrogen fixation ” is necessary. Some plants depend on the availability of ammonia and other nitrogen compounds formed in the soil as a result of decomposition of organic (plant and animal) residues. Others, such as legumes, take advantage of symbiosis with nitrogen-fixing bacteria (rhizobia), which are capable of synthesizing ammonia from atmospheric nitrogen [9] using enzymes called nitrogenases. Although it is unlikely that biomimetic methods will ever be invented that can compete in performance with chemical methods for the production of ammonia from nitrogen, nevertheless, scientists are making great efforts to better understand the mechanisms of biological nitrogen fixation. The scientific interest in this problem is partly motivated by the unusual structure of the active catalytic center of the nitrogen-fixing enzyme (nitrogenase), which contains an unusual bimetallic molecular ensemble of Fe 7 MoS 9 .
Ammonia is also the final by-product of the metabolism of amino acids, namely the product of their deamination, catalyzed by enzymes such as glutamate dehydrogenase. Unchanged ammonia excretion is the usual way of detoxifying ammonia in aquatic creatures (fish, aquatic invertebrates, partly amphibians). In mammals, including humans, ammonia usually quickly converts to urea , which is much less toxic and, in particular, has a less alkaline reaction and less reactivity as a reducing agent. Urea is the main component of the dry residue of urine. Most birds, reptiles, insects, arachnids, however, excrete not urea, but uric acid as the main nitrogen residue.
Ammonia also plays an important role in both normal and pathological physiology of animals. Ammonia is produced during the normal metabolism of amino acids, but is very toxic in high concentrations [10] . The animal liver converts ammonia to urea through a series of sequential reactions known as the urea cycle. A dysfunction of the liver, such as, for example, is observed with cirrhosis of the liver , can lead to a violation of the ability of the liver to neutralize ammonia and form urea from it, and, as a result, increase the level of ammonia in the blood, a condition called hyperammonemia. The presence of congenital genetic defects in the enzymes of the urea cycle, such as, for example, ornithine-carbamyl transferase, leads to a similar result - an increase in the level of free ammonia in the blood and the development of hyperammonemia. A violation of the renal excretory function in severe renal failure and uremia can also lead to the same result: as a result of a delay in the release of urea, its blood level rises so much that the urea cycle begins to work "in the opposite direction" - the excess urea is hydrolyzed back by the kidneys to ammonia and carbon gas, and, as a result, the level of ammonia in the blood increases. Hyperammonemia contributes to impaired consciousness and the development of soporotic and coma in hepatic encephalopathy and uremia, as well as the development of neurological disorders, often observed in patients with congenital defects of urea cycle enzymes or with organic aciduria [11] .
A less pronounced, but clinically significant, hyperammonemia can be observed in any processes in which increased protein catabolism is observed, for example, with extensive burns , tissue compression or crushing syndrome, extensive purulent-necrotic processes, limb gangrene, sepsis , etc., and also with some endocrine disorders, such as diabetes mellitus , severe thyrotoxicosis . Particularly high is the likelihood of hyperammonemia in these pathological conditions in those cases where the pathological condition, in addition to increased protein catabolism, also causes a pronounced violation of the detoxifying function of the liver or excretory function of the kidneys.
Ammonia is important for maintaining a normal acid-base balance in the blood. After the formation of ammonia from glutamine , alpha-ketoglutarate can be further broken down to form two bicarbonate molecules, which can then be used as a buffer to neutralize acids from food. Ammonia obtained from glutamine is then excreted in the urine (both directly and in the form of urea), which, taking into account the formation of two bicarbonate molecules from ketoglutarate, leads to a total loss of acids and a shift in the pH of the blood to the alkaline side. In addition, ammonia can diffuse through the renal tubules, combine with the hydrogen ion and be excreted together with it (NH 3 + H + => NH 4 + ), and thereby further contribute to the elimination of acids from the body [12] .
Ammonia and ammonium ions are a toxic by-product of animal metabolism. In fish and aquatic invertebrates, ammonia is released directly into the water. In mammals (including aquatic mammals), amphibians, and sharks, ammonia in the urea cycle is converted to urea, since urea is much less toxic, less chemically reactive, and can be more effectively stored in the body until it can be isolated. In birds and reptiles (reptiles), ammonia formed during metabolism is converted to uric acid, which is a solid residue and can be excreted with minimal water loss [13] .
Physiological Action
Ammonia is toxic. According to the physiological effect on the body, it belongs to the group of asphyxiating and neurotropic substances that, when inhaled, can cause toxic pulmonary edema and severe damage to the nervous system. Ammonia has both local and resorptive effects.
Ammonia vapors strongly irritate the mucous membranes of the eyes and respiratory organs, as well as the skin [14] . This person perceives as a pungent smell. Ammonia vapors cause profuse lacrimation, eye pain, chemical burns of the conjunctiva and cornea, loss of vision, coughing, redness and itching of the skin. When liquefied ammonia and its solutions come into contact with the skin, burning occurs, a chemical burn with blisters, ulcerations is possible. In addition, liquefied ammonia absorbs heat during evaporation, and when it comes into contact with skin, frostbite of various degrees occurs. The smell of ammonia is felt at a concentration of 37 mg / m³ [15] .
The maximum permissible concentration in the air of the working area of the production room ( MPC ) is 20 mg / m³ [16] . In the atmospheric air of settlements and in residential premises, the average daily concentration of ammonia ( MPC.s. ) should not exceed 0.04 mg / m³ [17] . The maximum single concentration in the atmosphere is 0.2 mg / m³. Thus, the smell of ammonia indicates an excess of permissible norms.
Irritation of the pharynx occurs when the ammonia content in the air is 280 mg / m³, the eye - 490 mg / m³. When exposed to very high concentrations, ammonia causes skin damage: 7-14 g / m³ - erythematous , 21 g / m³ or more - bullous dermatitis . Toxic pulmonary edema develops when exposed to ammonia for an hour with a concentration of 1.5 g / m³. Short-term exposure to ammonia at a concentration of 3.5 g / m³ and more quickly leads to the development of general toxic effects.
In the world, the maximum concentration of ammonia in the atmosphere (more than 1 mg / m³) is observed on the Indo-Gangetic Plain, in the Central Valley of the USA and in the Turkestan (formerly South Kazakhstan) region of Kazakhstan [18] .
Application
It is mainly used for the production of nitrogen fertilizers (ammonium nitrate and sulfate, urea ), explosives and polymers , nitric acid, soda (according to the ammonia method) and other products of the chemical industry. Liquid ammonia is used as a solvent .
In refrigeration equipment it is used as a refrigerant (R717) (see Ammonia refrigeration unit ).
In medicine, a 10% solution of ammonia, often called ammonia , is used for fainting (to stimulate breathing), to stimulate vomiting, as well as externally - neuralgia, myositis, insect bites, and to treat the surgeon's hands. If used incorrectly, it can cause burns to the esophagus and stomach (in case of taking undiluted solution), reflex respiratory arrest (if inhaled in high concentration).
Apply topically, inhaled and orally. To stimulate breathing and remove the patient from a fainting state, gently bring a small piece of gauze or cotton wool moistened with ammonia to the patient's nose (for 0.5-1 s). Inside (only diluted) to induce vomiting. With insect bites - in the form of lotions; with neuralgia and myositis - rubbing with ammonia liniment. In surgical practice, they breed in warm boiled water and wash their hands.
Since ammonia is a weak base, it reacts with acids to neutralize them.
The physiological effect of ammonia is due to the pungent smell of ammonia, which irritates specific receptors of the nasal mucosa and stimulates the respiratory and vasomotor centers of the brain, causing increased breathing and increased blood pressure.
Accelerator for dry mortars related to accelerators. The recommended dosage is 2 ... 8% of the mass of the components of the dry mixture depending on the temperature of use. Ammonia water is a product (NH 3 * H 2 O), which is gaseous ammonia NH 3 dissolved in water.
Getting
The industrial method for producing ammonia is based on the direct interaction of hydrogen and nitrogen:
- + 91.84 to J
This is the so-called Haber process (a German physicist who developed the physicochemical basis of the method).
The reaction occurs with the release of heat and a decrease in volume. Therefore, based on the Le Chatelier principle , the reaction should be carried out at the lowest possible temperatures and at high pressures - then the equilibrium will be shifted to the right. However, the reaction rate at low temperatures is negligible, and at high temperatures, the reverse reaction rate increases. Carrying out the reaction at very high pressures requires the creation of special equipment that can withstand high pressure, and, therefore, a large investment. In addition, the equilibrium of the reaction even at 700 ° C is set too slowly for its practical use.
The ammonia yield ( in volume percent ) in the Haber process at various temperatures and pressures has the following values [19] :
100 at | 300 at | 1000 at | 1500 at | 2000 at | 3500 at | |
---|---|---|---|---|---|---|
400 ° C | 25.12 | 47.00 | 79.82 | 88.54 | 93.07 | 97.73 |
450 ° C | 16,43 | 35.82 | 69.69 | 84.07 | 89.83 | 97.18 |
500 ° C | 10.61 | 26.44 | 57.47 | No data | ||
550 ° C | 6.82 | 19.13 | 41.16 |
The use of a catalyst (porous iron with impurities Al 2 O 3 and K 2 O) made it possible to accelerate the achievement of the equilibrium state. Interestingly, when searching for a catalyst for this role, more than 20 thousand different substances were tried.
Considering all the above factors, the process of producing ammonia is carried out under the following conditions: temperature 500 ° C, pressure 350 atmospheres, catalyst . The yield of ammonia under such conditions is about 30%. In industrial conditions, the principle of circulation is used - ammonia is removed by cooling, and unreacted nitrogen and hydrogen are returned to the synthesis column. This is more economical than achieving a higher reaction yield by increasing pressure.
To obtain ammonia in the laboratory, the action of strong alkalis on ammonium salts is used:
Usually, ammonia is obtained by laboratory methods by slightly heating a mixture of ammonium chloride and hydrated lime.
To drain ammonia, it is passed through a mixture of lime with sodium hydroxide.
Very dry ammonia can be obtained by dissolving metallic sodium in it and subsequently distilling it . This is best done in a system made of metal under vacuum . The system must withstand high pressure (at room temperature, the pressure of saturated ammonia vapor is about 10 atmospheres) [20] . In industry, ammonia is dried in absorption columns .
Consumption rates per ton of ammonia
On average, 1,200 nm³ of natural gas is spent on the production of one ton of ammonia in Russia, and 900 nm³ [21] [22] [23] [24] [25] in Europe.
The Belarusian “Grodno Azot” consumes 1,200 nm³ of natural gas per ton of ammonia, after modernization it is expected to reduce consumption to 876 nm³ [26] .
Ukrainian producers consume from 750 n.m³ [27] to 1170 n.m³ [28] of natural gas per ton of ammonia.
According to UHDE technology, the claimed consumption is 6.7 - 7.4 Gcal of energy per ton of ammonia [29] .
Ammonia in medicine
When insect bites, ammonia is used externally in the form of lotions. A 10% aqueous solution of ammonia is known as ammonia .
Side effects are possible: with prolonged exposure (inhalation use), ammonia can cause reflex respiratory arrest.
Topical use is contraindicated in dermatitis, eczema, other skin diseases, as well as with open traumatic injuries of the skin.
In case of accidental damage to the mucous membrane of the eye by ammonia, rinse the eyes with water (15 times every 10 minutes) or 5% boric acid solution without rubbing the eyes. Oils and ointments are not used. With damage to the nose and pharynx, a 0.5% solution of citric acid or natural juices. В случае приёма внутрь пить воду, фруктовый сок, молоко, лучше — 0,5 % раствор лимонной кислоты или 1 % раствор уксусной кислоты до полной нейтрализации содержимого желудка.
Взаимодействие с другими лекарственными средствами неизвестно.
Производители аммиака
Производители аммиака в России
Company | 2006, тыс. т | 2007, тыс. т |
---|---|---|
ОАО «Тольяттиазот» | 2 634 | 2 403,3 |
ОАО НАК «Азот» | 1 526 | 1 514,8 |
ОАО «Акрон» | 1 526 | 1 114,2 |
ОАО « Невинномысский азот », г. Невинномысск | 1 065 | 1 087,2 |
ОАО «Минудобрения» (г. Россошь) | 959 | 986,2 |
ОАО «АЗОТ» г. Кемерово [ clarify ] | 854 | 957,3 |
ОАО «Азот» [ clarify ] | 869 | 920,1 |
ОАО «ЗМУ КЧХК» | 956 | 881,1 |
ОАО Череповецкий «Азот» | 936,1 | 790,6 |
ЗАО «Куйбышевазот» | 506 | 570,4 |
ОАО «Газпром Нефтехим Салават» | 492 | 512,8 |
«Минеральные удобрения» (г. Пермь) | 437 | 474,6 |
ОАО «Дорогобуж» | 444 | 473,9 |
ОАО «Воскресенские минеральные удобрения» | 175 | 205,3 |
ОАО «Щекиноазот» | 58 | 61,1 |
АО "Аммоний" (г. Менделеевск) [1] | - | - |
Total | 13 437,1 | 12 952,9 |
На долю России приходится около 9 % мирового выпуска аммиака. Россия — один из крупнейших мировых экспортёров аммиака. На экспорт поставляется около 25 % от общего объёма производства аммиака, что составляет около 16 % мирового экспорта.
По итогам 2014 года в России было произведено 14,8 млн тонн аммиака (+2 % к 2013 году) (по данным Росстата). Производство аммиака в России сконцентрировано в Приволжском федеральном округе (46 % по итогам 2014 года). Далее следуют Центральный федеральный округ (23 %) и Северо-Западный федеральный округ (16 %).
Порядка 25 % российского производства аммиака отправляется на экспорт. Так, в 2014 году объём российского экспорта аммиака (по данным ФТС) составил составил 3,6 млн тонн (+6 % к 2013 году) на сумму 1,6 млрд долл. США.
Ключевыми странами-получателями в 2014 году стали Украина, Финляндия и Литва [30] .
Производители аммиака на Украине
Company | 2008 |
---|---|
ПАО «Концерн Стирол» | 1 331 |
Одесский припортовый завод | 1 128 |
Северодонецкое объединение Азот | 1 015 |
«Азот» (Черкассы) | 778 |
«Днепроазот» | 515 |
«Ровноазот» | 382 |
Total | 5 149 |
Interesting Facts
- Пары нашатырного спирта способны изменять окраску цветов. Например, голубые и синие лепестки становятся зелёными, ярко-красные — чёрными [31] .
- Облака Юпитера состоят из аммиака.
- Некоторые цветы, не имеющие запаха от природы, после обработки аммиаком начинают благоухать. Например, приятный аромат приобретают астры [31] .
- Нашатырный спирт реагирует с йодом с образованием крайне нестабильного аддукта ( иодистый азот ) в сухом кристаллическом состоянии, что используется как эффектный химический опыт.
See also
- Аммиакопровод
- Аммиачная холодильная установка
Notes
- ↑ 1 2 3 http://www.cdc.gov/niosh/npg/npgd0028.html
- ↑ http://www.cdc.gov/niosh/ipcsneng/neng0414.html
- ↑ Hall H. K. Correlation of the Base Strengths of Amines 1 // J. Am. Chem. Soc. / P. J. Stang — American Chemical Society , 1957. — Vol. 79, Iss. 20. — P. 5441–5444. — ISSN 0002-7863 ; 1520-5126 ; 1943-2984 — doi:10.1021/JA01577A030
- ↑ ГОСТ 6221-90. Аммиак жидкий технический. Технические условия
- ↑ Priestley, Joseph. Observations on Alkaline Air // Experiments and Observations on Different Kinds of Air . — Second edition. — 1775. — Vol. I. — P. 163-177.
- ↑ Berthollet. Analyse de'l Alkali volatil (неопр.) // Histoire de l'Académie Royale des Sciences. Année M. DCCLXXXV. Avec les Mémoires de Mathématique & de Physique pour la même Année. — 1788. — С. 316—326 .
- ↑ Малина И.К. Синтез аммиака // Книга для чтения по неорганической химии. Пособие для учащихся. Ч. II. — М. : Просвещение , 1975. — С. 52—62 .
- ↑ Karl S. Roth, MD . eMedicine Specialties > Metabolic Diseases > Hyperammonemia . Дата обращения 7 июля 2009.
- ↑ Adjei, MB; Quesenberry, KH and Chamblis, CG Nitrogen Fixation and Inoculation of Forage Legumes . University of Florida IFAS Extension (июнь 2002). Архивировано 20 мая 2007 года.
- ↑ PubChem Substance Summary . Дата обращения 7 июля 2009.
- ↑ Zschocke, Johannes, and Georg Hoffman. Vademecum Metabolism. — Friedrichsdorf, Germany: Milupa GmbH, 2004.
- ↑ Rose, Burton, and Helmut Rennke. Renal Pathophysiology. — Baltimore : Williams & Wilkins, 1994. — ISBN 0-683-07354-0 .
- ↑ Campbell, Neil A. 44 // Biology. — 6th. — San Francisco : Pearson Education, Inc, 2002. — P. 937–938. — ISBN 0-8053-6624-5 .
- ↑ Фердман Д.Л., Лепахин В.К., Марченко Е.Н., Швайкова М.Д. Аммиак // Большая медицинская энциклопедия : в 30 т. / гл. ed. Б.В. Петровский . — 3 изд. — Москва : Советская энциклопедия , 1974. — Т. 1. А — Антибиоз . - 576 p. - 150,000 copies.
- ↑ http://www.rhbz.info/rhbz3.1.5.4.html Архивная копия от 30 декабря 2011 на Wayback Machine Учебное пособие по РХБЗ. Характеристика аварийно химически опасных веществ
- ↑ ГОСТ 12.1.005-88. Система стандартов безопасности труда. Общие санитарно-гигиенические требования к воздуху рабочей зоны
- ↑ СанПиН 2.1.2.1002-00. Санитарно-эпидемиологические требования к жилым зданиям и помещениям
- ↑ «Известия». The science
- ↑ Ходаков Ю. В., Эпштейн Д. А., Глориозов П. А. § 19. Взаимодействие азота с водородом // Неорганическая химия. Учебник для 9 класса. — 7-е изд. — М. : Просвещение , 1976. — С. 38—41. — 2 350 000 экз.
- ↑ Гордон А., Форд Р. Спутник химика.//Перевод на русский язык Розенберга Е. Л., Коппель С. И. — М.: Мир, 1976. — 544 с.
- ↑ ФАКТОРЫ КОНКУРЕНТНОСТИ НА РЫНКЕ АММИАЧНО-НИТРАТНЫХ УДОБРЕНИЙ
- ↑ АММИАЧНЫЕ УСТАНОВКИ НА РОССИЙСКИХ ПРЕДПРИЯТИЯХ
- ↑ ПРОИЗВОДИТЕЛИ АММИАКА И КАРБАМИДА В РОССИИ (Часть I)
- ↑ ПРОИЗВОДИТЕЛИ АММИАКА И КАРБАМИДА В РОССИИ (Часть II)
- ↑ ПРОИЗВОДИТЕЛИ АММИАКА И КАРБАМИДА В РОССИИ (Часть III)
- ↑ Лукашенко потребовал ускорить модернизацию «Гродно Азота». 21.by
- ↑ Селитра аммиачная 095-2471996: Удар по гривне
- ↑ Селитра аммиачная 095-2471996: Наши химики — впереди российских
- ↑ Технология производства аммиака
- ↑ Четверть российского аммиака уходит на экспорт (недоступная ссылка) . Архивировано 4 марта 2016 года.
- ↑ 1 2 Искусственное изменение окраски лепестков цветов. Удивительный мир растений
Literature
- Ахметов Н. С. Общая и неорганическая химия. — М.: Высшая школа, 2001.
- Карапетьянц М. Х. , Дракин С. И. Общая и неорганическая химия. — М.: Химия, 1994.
- Акимова Л. Д. Изучающим основы холодильной техники. — М., 1996.
- Ельницкий А. П., Василевская Е. И., Шарапа Е. И., Шиманович И. Е. Химия. — Мн.: Народная асвета, 2007.
Links
- Аммиак, газ // Энциклопедический словарь Брокгауза и Ефрона : в 86 т. (82 т. и 4 доп.). - SPb. , 1890-1907.
- Аммиак водный // Энциклопедический словарь Брокгауза и Ефрона : в 86 т. (82 т. и 4 доп.). - SPb. , 1890-1907.
- Аммониак // Энциклопедический словарь Брокгауза и Ефрона : в 86 т. (82 т. и 4 доп.). - SPb. , 1890-1907.
- Аммониемия // Энциклопедический словарь Брокгауза и Ефрона : в 86 т. (82 т. и 4 доп.). - SPb. , 1890-1907.
- NIST Chemistry WebBook