Ammonia –N.H. 3

Ammonia (in European languages ​​its name sounds like “ammoniac”) owes its name to the Ammon 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 especially quickly. One of the decomposition products is ammonia. According to other sources, ammonia got its name from the ancient Egyptian word Amonian. This was the name given to people who worshiped the god Amon. During their rituals, they sniffed ammonia NH 4 Cl, which, when heated, evaporates ammonia.

1. Molecule structure

The ammonia molecule has the shape of a trigonal pyramid with a nitrogen atom at the apex. 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 outer electrons is lone, it can form a donor-acceptor bond with a hydrogen ion, forming an ammonium ion NH 4 + .

Type of chemical bond:covalent polar, three singleσ - sigma N-H bonds

2. Physical properties of ammonia

Under normal conditions, it is a colorless gas with a sharp characteristic odor (the smell of ammonia), almost twice as light as air, and poisonous.According to its physiological effect on the body, it belongs to the group of substances with asphyxiating and neurotropic effects, which, if inhaled, can cause toxic pulmonary edema and severe damage to the nervous system. Ammonia vapors strongly irritate the mucous membranes of the eyes and respiratory organs, as well as the skin. This is what we perceive as a pungent odor. Ammonia vapors cause excessive lacrimation, eye pain, chemical burns of the conjunctiva and cornea, loss of vision, coughing attacks, redness and itching of the skin. The solubility of NH 3 in water is extremely high - about 1200 volumes (at 0 °C) or 700 volumes (at 20 °C) per volume of water.

3.

In the laboratory	In industry
To obtain ammonia in the laboratory, the action of strong alkalis on ammonium salts is used: NH 4 Cl + NaOH = NH 3 + NaCl + H 2 O (NH 4) 2 SO 4 + Ca(OH) 2 = 2NH 3 + CaSO 4 + 2H 2 O Attention !Ammonium hydroxide is an unstable base, decomposes: NH 4 OH ↔ NH 3 + H 2 O When receiving ammonia, hold the receiver tube with the bottom up, since ammonia is lighter than air:	The industrial method for producing ammonia is based on the direct interaction of hydrogen and nitrogen: N 2(g) + 3H 2(g) ↔ 2NH 3(g) + 45.9k J Conditions: catalyst – porous iron temperature – 450 – 500 ˚С pressure – 25 – 30 MPa This is the so-called Haber process (a German physicist who developed the physicochemical foundations of the method).

4. Chemical properties of ammonia

Ammonia is characterized by the following reactions:

1. with a change in the oxidation state of the nitrogen atom (oxidation reaction)
2. without changing the oxidation state of the nitrogen atom (addition)

Reactions involving a change in the oxidation state of the nitrogen atom (oxidation reactions) N -3 → N 0 → N +2 NH 3 –strong reducing agent.

with oxygen 1. Ammonia combustion (when heated) 4 NH 3 + 3 O 2 → 2 N 2 + 6 H 2 0 2. Catalytic oxidation of ammonia (catalystPt – Rh, temperature) 4NH 3 + 5O 2 → 4NO + 6H 2 O Video - Experiment "Oxidation of ammonia in the presence of chromium oxide"

with metal oxides 2 NH 3 + 3CuO = 3Cu + N 2 + 3 H 2 O

with strong oxidizing agents 2 NH 3 + 3 Cl 2 = N 2 + 6 HCl (when heated)

ammonia is a weak compound and decomposes when heated 2NH 3 ↔ N 2 + 3H 2

Reactions without changing the oxidation state of the nitrogen atom (addition - Ammonium ion formation NH4+by donor-acceptor mechanism) Video - Experiment "Qualitative reaction to ammonia" Video - Experiment "Smoke without fire" Video - Experiment "Interaction of ammonia with concentrated acids" Video - Experiment "Fountain" Video - Experiment "Dissolving ammonia in water"

5. Application of ammonia

In terms of production volumes, ammonia occupies one of the first places; Every year, about 100 million tons of this compound are produced worldwide. Ammonia is available in liquid form or in the form of an aqueous solution - ammonia water, which usually contains 25% NH 3. Huge quantities of ammonia are further used to produce nitric acid which goes to fertilizer production and many other products. Ammonia water is also used directly as fertilizer, and sometimes fields are watered directly from tanks with liquid ammonia. From ammonia receive various ammonium salts, urea, methenamine. His also used as a cheap refrigerant in industrial refrigeration units.

Ammonia is also used for producing synthetic fibers, for example, nylon and nylon. In light industry he used in cleaning and dyeing cotton, wool and silk. In the petrochemical industry, ammonia is used to neutralize acidic waste, and in the natural rubber industry, ammonia helps preserve latex as it travels from plantation to factory. Ammonia is also used in the production of soda using the Solvay method. In the steel industry, ammonia is used for nitriding - saturating the surface layers of steel with nitrogen, which significantly increases its hardness.

Doctors use aqueous solutions of ammonia (ammonia) in everyday practice: a cotton swab dipped in ammonia brings a person out of a fainting state. Ammonia in this dose is not dangerous for humans.

EXERCISES

Simulator No. 1 "Ammonia combustion"

Simulator No. 2 "Chemical properties of ammonia"

ASSIGNMENT TASKS

№1. Carry out transformations according to the scheme:

a) Nitrogen → Ammonia → Nitric oxide (II)

b) Ammonium nitrate → Ammonia → Nitrogen

c) Ammonia → Ammonium Chloride → Ammonia → Ammonium Sulfate

For ORR, compile an e-balance; for RIO, complete ionic equations.

No. 2. Write four equations for the chemical reactions that produce ammonia.

Subject: Ammonia. Physical and chemical properties. Receipt and application.

Lesson objectives: know the structure of the ammonia molecule, physical and chemical properties, areas of application; be able to prove the chemical properties of ammonia: write down equations for the reactions of ammonia with oxygen, water, acids and consider them from the point of view of the theory of electrolytic dissociation and redox processes.

Lesson progress

1. Organizational moment of the lesson.

2. Studying new material.

Ammonia – NH 3

Ammonia (in European languages ​​its name sounds like “ammoniac”) owes its name to the Ammon 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 especially quickly. One of the decomposition products is ammonia. According to other sources, ammonia got its name from the ancient Egyptian word amonian. This was the name given to people who worshiped the god Amon. During their ritual ceremonies they sniffed ammonia NH 4 Cl, which when heated evaporates ammonia.

1. Molecule structure

The ammonia molecule has the shape of a trigonal pyramid with a nitrogen atom at the apex. 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 outer electrons is lone, it can form a donor-acceptor bond with a hydrogen ion, forming an ammonium ion NH 4 + .

2. Physical properties of ammonia

Under normal conditions, it is a colorless gas with a sharp characteristic odor (the smell of ammonia), almost twice as light as air, and poisonous. According to its physiological effect on the body, it belongs to the group of substances with asphyxiating and neurotropic effects, which, if 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. This is what we perceive as a pungent odor. Ammonia vapors cause excessive lacrimation, eye pain, chemical burns of the conjunctiva and cornea, loss of vision, coughing attacks, redness and itching of the skin. Solubility NH 3 in water is extremely large - about 1200 volumes (at 0 °C) or 700 volumes (at 20 °C) per volume of water.

3. Ammonia production

In the laboratory

In industry

To obtain ammonia in the laboratory, the action of strong alkalis on ammonium salts is used:

NH 4 Cl + NaOH = NH 3 + NaCl + H 2 O

(NH 4 ) 2 SO 4 + Ca(OH) 2 = 2NH 3 + CaSO 4 + 2H 2 O

Attention! Ammonium hydroxide is an unstable base, decomposes: NH 4 OH ↔ NH 3 + H 2 O

When receiving ammonia, hold the receiver tube with the bottom up, since ammonia is lighter than air:

The industrial method for producing ammonia is based on the direct interaction of hydrogen and nitrogen:

N 2(g) + 3H 2(g) ↔ 2NH 3(g) + 45.9 kJ

Conditions:

catalyst – porous iron

temperature – 450 – 500 ˚С

pressure – 25 – 30 MPa

This is the so-called Haber process (a German physicist who developed the physicochemical foundations of the method).

4. Chemical properties of ammonia

Ammonia is characterized by the following reactions:

1. with a change in the oxidation state of the nitrogen atom (oxidation reaction)

2. without changing the oxidation state of the nitrogen atom (addition)

Reactions involving a change in the oxidation state of the nitrogen atom (oxidation reactions)

N -3 → N 0 → N +2

NH 3 – a strong reducing agent.

with oxygen

1. Ammonia combustion(when heated)

4NH 3 + 3O 2 → 2N 2 + 6H 2 0

2. Catalytic oxidation of ammonia (catalyst Pt – Rh, temperature)

4NH 3 + 5O 2 → 4NO + 6H 2 O

with metal oxides

2 NH 3 + 3CuO = 3Cu + N 2 + 3 H 2 O

with strong oxidizing agents

2NH3 + 3Cl2 = N2 + 6HCl (when heated)

ammonia is a weak compound and decomposes when heated

2NH 3 ↔ N 2 + 3H 2

Reactions without changing the oxidation state of the nitrogen atom (addition - Formation of ammonium ion NH 4 + each donor-acceptor mechanism)

5. Application of ammonia

In terms of production volumes, ammonia occupies one of the first places; Every year, about 100 million tons of this compound are produced worldwide. Ammonia is available in liquid form or as an aqueous solution - ammonia water, which usually contains 25% NH 3 . Huge quantities of ammonia are then used to produce nitric acid, which is used to make fertilizers and many other products. Ammonia water is also used directly as fertilizer, and sometimes fields are watered directly from tanks with liquid ammonia. Various ammonium salts, urea, and methenamine are obtained from ammonia. It is also used as a cheap refrigerant in industrial refrigeration units.

Ammonia is also used to produce synthetic fibers, such as nylon and nylon. In light industry it is used in cleaning and dyeing cotton, wool and silk. In the petrochemical industry, ammonia is used to neutralize acidic waste, and in the natural rubber industry, ammonia helps preserve latex as it travels from plantation to factory. Ammonia is also used in the production of soda using the Solvay method. In the steel industry, ammonia is used for nitriding - saturating the surface layers of steel with nitrogen, which significantly increases its hardness.

Doctors use aqueous solutions of ammonia (ammonia)in everyday practice: a cotton swab dipped in ammonia brings a person out of a fainting state. Ammonia in this dose is not dangerous for humans.

3. Consolidation of the studied material

No. 1. Carry out transformations according to the scheme:

a) Nitrogen → Ammonia → Nitric oxide (II)

b) Ammonium nitrate → Ammonia → Nitrogen

c) Ammonia → Ammonium Chloride → Ammonia → Ammonium Sulfate

For ORR, compile an e-balance; for RIO, complete ionic equations.

No. 2. Write four equations for the chemical reactions that produce ammonia.

4. Homework

P. 24, ex. 2.3; test

Ammonia is a gaseous substance with a strong, unpleasant odor. What properties does it have and what substances does it react with?

Molecule structure

The electronic formula of ammonia is as follows:

Rice. 1. Electronic formula of ammonia.

Of the four electron pairs at the nitrogen atom, three are shared and one is lone. The formation of the NH 3 molecule involves three unpaired p-electrons of the nitrogen atom, the electron orbitals of which are mutually perpendicular, and the 1s electrons of three hydrogen atoms. The molecule has the shape of a regular pyramid: in the corners of the triangle there are hydrogen atoms, and at the top of the pyramid there is a nitrogen atom. The angle between the H-N-H bonds is 107.78 degrees.

Physical properties

Ammonia is a colorless gas with a characteristic pungent odor. The boiling point of ammonia is -33.4 degrees Celsius, the melting point is -77.8 degrees.

Ammonia is highly soluble in water (at 20 degrees, up to 700 volumes of ammonia dissolve in 1 volume of water). The concentrated solution has an ammonia density of 0.91 g/cm3.

A solution of ammonia in water is called ammonia water or ammonia. When boiling, dissolved ammonia evaporates from the solution.

Rice. 2. Ammonia.

Ammonia is somewhat less soluble in organic solvents (alcohol, acetone, chloroform, benzene). Ammonia dissolves many nitrogen-containing substances well.

Liquid ammonia has a high heat of evaporation (at -50 degrees 145 kJ/kg, at 0 degrees 1260 kJ/kg, at 50 degrees 1056 kJ/kg).

The molar mass and molecular weight of ammonia is 17

Chemical properties

Chemically, ammonia is quite active. reactions in which ammonia participates are accompanied either by a change in the oxidation state of nitrogen or by the formation of a special type of covalent bond. The high solubility of a chemical substance in water is due to the formation of hydrogen bonds between their molecules.

Ammonia can react with the following substances:

• When interacting with acids, ammonia neutralizes them, thereby forming ammonium salts:

NH 3 +HCl=NH 4 Cl

• When reacting with halogens, ammonia is usually oxidized to free nitrogen:

8NH 3 +3Br 2 =N 2 +6NH 4 Br

• When mixed with oxygen, ammonia burns with a greenish-yellow flame:

4NH 3 +3O 2 =6H 2 O+2N 2

• when heated, ammonia reduces copper (II) oxide, and itself is oxidized to free nitrogen:

3CuO+2NH 3 =3Cu+N 2 +3H 2 O

– using this reaction you can obtain oxygen in the laboratory.

Receipt and use

In the laboratory, ammonia is obtained by heating ammonium chloride NH 4 Cl with slaked lime Ca (OH) 2:

2NH 4 Cl+Ca(OH) 2 =CaCl+2NH 3 +2H 2 O

– the released ammonia contains water vapor.

In industry, ammonia is produced from nitrogen and hydrogen. The reaction of ammonia synthesis proceeds with the release of heat and a decrease in volume:

N 2 +3H 2 =2NH 3

The temperature required for ammonia synthesis is achieved by preheating the nitrogen-hydrogen mixture and by releasing reaction heat. The catalyst for ammonia synthesis is sponge iron activated by certain metals. Hydrogen sulfide, oxygen, carbon oxide and dioxide, vapors and other mixtures contained in the nitrogen-hydrogen mixture sharply reduce the activity of the catalyst. Synthesis is carried out at a temperature of 500-550 degrees and a pressure from 15 to 100 MPa.

The ammonia synthesis plant diagram looks like this:

Rice. 3. Scheme of ammonia production.

Most of the ammonia synthesized in industry is used to produce nitric acid and other nitrogen-containing substances. Its use in refrigeration units is based on easy liquefaction and subsequent evaporation with heat absorption.

Aqueous solutions of ammonia are used in chemical laboratories and industries as a weak, highly volatile base. Aqueous solutions are also used in medicine and everyday life.

What have we learned?

The study of ammonia is included in the compulsory school chemistry course. Ammonia is a chemical compound that contains nitrogen and hydrogen. The gas is a colorless substance with a pronounced odor and reacts with acids, water, halogens, oxygen and other complex and simple substances.

Test on the topic

Evaluation of the report

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Ammonia (NH 3) is one of the most common industrial chemicals used in industry and commerce.

Ammonia, why does our body need it? It turns out that it is constantly formed in all organs and tissues and is an essential substance in many biological processes, serving as a precursor for the formation of amino acids and the synthesis of nucleotides. In nature, ammonia is formed during the decomposition of nitrogen-containing organic compounds.

Chemical and physical properties of ammonia

• At room temperature, ammonia is a colorless, irritating gas with a pungent, suffocating odor;
• in its pure form is known as anhydrous ammonia;
• hygroscopic (easily absorbs moisture);
• has alkaline properties, caustic, easily soluble in water;
• easily compresses and forms a clear liquid under pressure.

Where is ammonia used?

About 80% of ammonia is used to make industrial products.

Ammonia is used in agriculture as a fertilizer.

Present in refrigeration units for purifying aqueous compositions.

Used in the production of plastics, explosives, textiles, pesticides, dyes and other chemicals.

Contained in many household and industrial cleaning solutions. Household products containing ammonia are made with the addition of 5-10% ammonia; the concentration of ammonia in industrial solutions is higher - 25%, which makes them more caustic.

How does ammonia affect the human body?

Most people come into contact with ammonia inhaling it like gas or evaporation. Since ammonia exists naturally and is found in detergents, they can be sources of it.

The widespread use of ammonia in agricultural and industrial areas also means that increased concentrations in the air can occur during accidental releases or deliberate terrorist attacks.

Anhydrous ammonia gas is lighter than air and therefore rises high, so it generally dissipates and does not accumulate in low areas. However, in the presence of dampness (high relative humidity), liquefied anhydrous ammonia forms vapor that is heavier than air. These vapors can be carried over the surface of the earth or over lowlands.

How does ammonia work?

Ammonia begins to react immediately after contact with moisture on the surface of the skin, eyes, mouth, respiratory tract and partially mucous surfaces and forms a very caustic ammonium hydroxide . Ammonium hydroxide causes tissue necrosis due to disruption of cell membranes, leads to cell destruction. Once the protein and cells are broken down, water is extracted through an inflammatory response, leading to further damage.

What are the symptoms of ammonia poisoning?

Breath. The smell of ammonia in the nose is irritating and pungent. Contact with high concentrations of ammonia in the air leads to a burning sensation in the nose, throat and respiratory tract. This can lead to bronchiolar and alveolar edema and airway damage resulting from respiratory failure. Inhalation of low concentrations may cause coughing and irritation of the nose and throat. The smell of ammonia is a fairly early warning of its presence, but ammonia also leads to a weakened sense of smell, which reduces the ability to notice it in the air at low concentrations.

Children, exposed to the same amount of ammonia as adults, receive a larger dose because the surface area of ​​their lungs relative to their body is much larger. In addition, they may be more exposed to ammonia due to their short stature - they are closer to the ground, where the concentration of vapors is higher.

Contact with skin or eyes. Contact with low concentrations of ammonia in air or liquids may cause rapid irritation of the eyes or skin. Higher concentrations of ammonia can cause serious injury and burns . Contact with concentrated ammonia liquids, such as industrial detergents, may cause corrosion damage, including skin burns, eye damage or blindness . The highest degree of eye damage may not be visible for up to a week after exposure. Contact with liquefied ammonia may also cause frostbite .

Consumption with food. Receiving high concentrations of ammonia through swallowing an ammonia solution can cause damage to the mouth, throat, and stomach.

AMMONIA [abbreviated from Greek?μμωνιακ?ς; Latin sal ammoniacus; this was the name of ammonia (ammonium chloride), which was obtained by burning camel dung in the Ammonium oasis in the Libyan Desert], the simplest chemical compound of nitrogen with hydrogen, NH 3; multi-tonnage product of the chemical industry.

Properties. The NH 3 molecule has the shape of a regular pyramid with a nitrogen atom at the top; N-H bonds are polar, N-H bond energy is 389.4 kJ/mol. The N atom has a lone pair of electrons, which determines the ability of ammonia to form donor-acceptor and hydrogen bonds. The NH 3 molecule is capable of inversion - “turning inside out” by passing a nitrogen atom through the plane of the base of the pyramid formed by hydrogen atoms.

Ammonia is a colorless gas with a pungent odor; t pl -77.7°C; t boil -33.35°C; density of gaseous NH 3 (at 0°C, 0.1 MPa) 0.7714 kg/m 3 ; heat of formation of ammonia from elements ΔН arr -45.94 kJ/mol. A dry mixture of ammonia with air (15.5-28% by weight NH 3) can explode. Liquid NH 3 is a colorless, highly refractive liquid, a good solvent for many organic and inorganic compounds. Ammonia is easily soluble in water (33.1% by weight at 20°C), somewhat less soluble in alcohol, acetone, benzene, and chloroform. A solution of ammonia in water ammonia water is a colorless liquid with an ammonia odor; a solution containing 10% by weight NH 3 has the trade name ammonia. In an aqueous solution, ammonia is partially ionized into NH + 4 and OH -, which determines the alkaline reaction of the solution (pK 9.247).

The decomposition of ammonia into hydrogen and nitrogen becomes noticeable at temperatures above 1200°C, and in the presence of catalysts (Fe, Ni) - above 400°C. Ammonia is a very reactive compound. It is characterized by addition reactions, in particular proton reactions when interacting with acids. As a result, ammonium salts are formed, which in many properties are similar to alkali metal salts. Ammonia, a Lewis base, attaches not only H +, but also other electron acceptors, for example BF 3 to form BF 3 ? NH 3. The action of NH 3 on simple or complex metal salts produces ammonia, for example cis-. Ammonia is also characterized by substitution reactions. Alkali and alkaline earth metals form amides with NH 3 (for example, NaNH 2). When heated in an ammonia atmosphere, many metals and non-metals (Zn, Cd, Fe, Cr, B, Si, etc.) form nitrides (for example, BN). At a temperature of about 1000°C, NH 3 reacts with carbon, forming hydrogen cyanide HCN and partially decomposing into N 2 and H 2. With CO 2 it forms ammonium carbamate NH 2 COONH 4 , which decomposes into water and urea at a temperature of 160-200°C and a pressure of up to 40 MPa. Hydrogen in ammonia can be replaced by halogens. Ammonia burns in an O2 atmosphere, forming water and N2. The catalytic oxidation of ammonia (Pt catalyst) produces NO (the reaction is used in the production of nitric acid), and the oxidation of ammonia mixed with methane produces HCN.

Receipt and use. In nature, ammonia is formed during the decomposition of nitrogen-containing compounds. In 1774, J. Priestley first collected ammonia in a mercury bath, formed by the action of lime on ammonium chloride. The oldest industrial method for producing NH 3 is the separation of ammonia from exhaust gases during coal coking.

The main modern method of producing ammonia is its synthesis from nitrogen and hydrogen, proposed in 1908 by F. Haber. Ammonia synthesis in industry is carried out by the reaction N 2 + ZN 2 →←2NH 3. A shift of equilibrium to the right is facilitated by an increase in pressure and a decrease in temperature. The process is carried out at a pressure of about 30 MPa and a temperature of 450-500°C in the presence of a catalyst - Fe, activated by the oxides K 2 O, Al 2 O 3, CaO, etc. With a single passage through the mass of the catalyst, only 20-25% is converted into ammonia. initial gas mixture; Repeated circulation is required for complete conversion. The main raw material for the production of H 2 in the production of ammonia is natural combustible gas, processed by the method of two-stage steam-gas reforming of methane.

Ammonia production includes the following stages: purification of natural gas from sulfur compounds by catalytic hydrogenation to H 2 S with subsequent absorption of ammonia by ZnO; steam reforming of natural gas under a pressure of 3.8 MPa at a temperature of 860°C on a Ni-Al catalyst in a tube furnace (primary reforming); steam-air conversion of residual methane in a shaft converter (secondary reforming) at 990-1000°C and 3.3 MPa on a Ni-Al catalyst; at this stage, hydrogen is enriched with nitrogen from atmospheric air to obtain a mixture of nitrogen and hydrogen (ratio by volume 1:3), supplied to the synthesis of NH 3; conversion of CO to CO 2 and H 2 first at 450°C and 3.1 MPa on a Fe-Cr catalyst, then at 200-260°C and 3.0 MPa on a Zn-Cr-Cu catalyst; purification of H 2 from CO 2 by absorption with a solution of monoethanolamine or a hot solution of K 2 CO 3 at 2.8 MPa; purification of a mixture of H 2 and N 2 by hydrogenation from residual CO and CO 2 in the presence of a Ni-Al catalyst at 280°C and 2.6 MPa; compression (compression) of purified gas to 15-30 MPa and synthesis of ammonia on a promoted iron catalyst at 400-500°C in a synthesis reactor with a packing with radial or axial gas flow. Liquid ammonia supplied to industry contains at least 99.96% NH 3 by weight. Up to 0.2-0.4% H 2 O is added to ammonia transported through a pipeline to inhibit steel corrosion.

Ammonia is used in the production of nitric acid, urea, ammonium salts, ammophos, methenamine, soda (using the ammonia method), as a liquid fertilizer, as a refrigerant, etc. A beam of NH 3 molecules was used as a working substance in the first quantum generator - a maser ( 1954).

Ammonia is toxic. When the air contains 0.02% ammonia by volume, it irritates the mucous membranes. Liquid ammonia causes severe skin burns.

World ammonia production (in terms of N) is about 125.7 million tons/year (2001), including in the Russian Federation - 11 million tons/year.

Lit.: Thermophysical properties of ammonia. M., 1978; Ammonia synthesis. M., 1982.

A. I. Mikhailichenko, L. D. Kuznetsov.