強アンモニア 化学特性,用途語,生産方法
外観
無色澄明の液体
溶解性
水、エタノール及びアセトンに混和する。
用途
農業用の液体肥料、窒素質肥料、化学繊維。
用途
化学原料 アンモニアは硝酸などの基礎化学品、硫安などチッソ肥料の原料となるため、工業的に極めて重要な物質である。 液化したアンモニアはバーチ還元の溶媒として使用される。
火力発電用燃料 前述のようにアンモニアは条件次第で燃焼し、燃やしても代表的な温暖化ガスである二酸化炭素が発生しない。このためアンモニアを火力発電用燃料として使う技術開発が行われている。
環境に有害な窒素酸化物の発生を抑制するために火力発電所のボイラーなどに設置される、選択触媒還元脱硝装置の還元剤として使用される。
効能
溶解剤, アンモニア原料
使用上の注意
不活性ガス封入
説明
Ammonia is a colorless, pungent-smelling gas that is one of the most important industrial inorganic chemicals. It is widely used in fertilizers, refrigerants, explosives, cleaning agents, and as a feedstock to produce numerous other chemicals. Ammonia ranks as one of the top 10 chemicals produced annually.
化学的特性
Strong ammonia solution occurs as a clear, colorless liquid having
an exceedingly pungent, characteristic odor. The PhEur 6.0 states
that concentrated ammonia solution contains not less than 25.0%
and not more than 30.0% w/w of ammonia (NH
3). The USP32–
NF27 states that strong ammonia solution contains not less than
27.0% and not more than 31.0% w/w of ammonia (NH
3).
化学的特性
Ammonia is a colorless, strongly alkaline, and
extremely soluble gas with a pungent, suffocating odor.
化学的特性
Ammonia, NH3, is a colorless gaseous alkaline compound. It is very soluble in water, has a highly characteristic pungent odor, is lighter than air, and is formed as a result of the decomposition of most nitrogenous organic materials. Anhydrous ammonia, a major commercial chemical, is used in the manufacture of fertilizers, HN03, acrylonitrile, and other products, and as an electrolytic solvent.
物理的性質
Colorless gas with a penetrating, pungent, suffocating odor. An experimentally determined odor
threshold concentration of 45.8 ppm
v was reported by Leonardos et al. (1969). A detection odor
threshold concentration of 11.6 mg/m
3 (16.7 ppm
v) was experimentally determined by Nishida et
al. (1974).
来歴
During the Middle Ages ammonia was produced by the distillation of animal dung, hooves, and horn. Its preparation from horn gave it another name: spirit of hartshorn. Joseph Priestley (1733–1804) isolated ammonia in 1774 and called the compound alkaline air. The modern name ammonia was given to the compound in 1782 by the Swedish chemist Torbern Bergman (1735–1784). The exact chemical composition was determined by Claude-Louis Berthollet (1748–1822) in 1785. During the 19th century ammonia was obtained from the distillation of coal tar. The importance of nitrogen fertilizers in agriculture was established during the mid-1800s, and this coupled with the growth of the chemical industry provided incentive to find a method for fixing nitrogen.
使用
Ammonia is a large-tonnage industrial product and finds its major use in the manufacture of nitric acid and fertilizers. It is the most commonly used refrigerant, particularly for large industrial installations.
使用
Fertilizer, corrosion inhibitor, purification of water supplies, component of household cleaners, as refrigerant. manufacture of nitric acid, explosives, synthetic fibers, fertilizers. In pulp and paper, metallurgy, rubber, food and beverage, textile and leather industries.
使用
Reagent for chemical vapor deposition of TiN.1
使用
Ammonia is a major feedstock for fertilizer, explosives, plastics, and other chemicals. The primary use of ammonia is in the production of fertilizers, with approximately 70% of ammonia being used for this purpose. Major fertilizers produced include ammonium nitrate, ammonium sulfate, and urea.
使用
NH
3 (ammonia) is produced in the so-called Haber Bosch process. This industrial process uses finely
divided iron as catalyst and a reaction temperature of around 450 °C at a pressure of 50 atm. Ammonia is used
to produce fertilisers, nitric acid, nylon and many more products important to our modern life style.
N
2(g) + 3H
2(g) → 2NH
3(g)
使用
Ammonia is used in the manufacture of nitricacid, hydrazine hydrate, and acrylonitrile, aswell as fertilizers, explosives, and syntheticfibers. It is also used in refrigeration.
定義
ChEBI: An azane that consists of a single nitrogen atom covelently bonded to three hydrogen atoms.
調製方法
The Haber process for the synthesis of ammonia is based on the reaction of nitrogen and hydrogen: N
2(g) + 3H
2(g) ? 2NH
3(g). Nitrogen in the reaction is obtained by separating nitrogen from air through liquefaction, and hydrogen is obtained from natural gas by steam reforming: CH
4(g) + H
2O
(g) → H
2(g) + CO
(g) According to Le Chatelier’s principle, the production of ammonia is favored by a high pressure and a low temperature. The Haber process is typically carried out at pressures between 200 and 400 atmospheres and temperatures of 500°C. In the commercial production of ammonia, NH3 is continually removed as it is produced.
定義
A colorless
gas with a characteristic pungent odor.
On cooling and compression it forms a colorless
liquid, which becomes a white solid
on further cooling. Ammonia is very soluble
in water (a saturated solution at 0°C
contains 36.9% of ammonia): the aqueous
solution is alkaline and contains a proportion
of free ammonia. Ammonia is also soluble
in ethanol. It occurs naturally to a
small extent in the atmosphere, and is usually
produced in the laboratory by heating
an ammonium salt with a strong alkali.
Ammonia is synthesized industrially from
hydrogen and atmospheric nitrogen by the
Haber process.
The compound does not burn readily in
air but ignites, giving a yellowish-brown
flame, in oxygen. It will react with atmospheric
oxygen in the presence of platinum
or a heavy metal catalyst – a reaction used
as the basis of the commercial manufacture
of nitric acid, which involves the oxidation
of ammonia to nitrogen monoxide and
then to nitrogen dioxide. Ammonia coordinates
readily to form ammines and reacts
with sodium or potassium to form inorganic
amides and with acids to form ammonium
salts; for example, it reacts with
hydrogen chloride to form ammonium
chloride:
NH
3(g) + HCl(g) → NH
4Cl(g)
Ammonia is also used commercially in
the manufacture of fertilizers, mainly ammonium
nitrate, urea, and ammonium sulfate.
It is used to a smaller extent in the
refrigeration industry. Liquid ammonia is
an excellent solvent for certain substances,
which ionize in the solutions to give ionic
reactions similar to those occurring in
aqueous solutions. Ammonia is marketed
as the liquid, compressed in cylinders (‘anhydrous
ammonia’), or as aqueous solutions
of various strengths. See also
ammonium hydroxide.
定義
ammonia: A colourless gas, NH
3, with a strong pungent odour; r.d. 0.59 (relative to air); m.p. –77.7°C; b.p. –33.35°C. It is very soluble in water and soluble in alcohol. The compound may be prepared in the laboratory by reacting ammonium salts with bases such as calcium hydroxide, or by the hydrolysis of a nitride. Industrially it is made by the Haber process and over 80 million tonnes per year are used either directly or in combination. Major uses are the manufacture of nitric acid, ammonium nitrate, ammonium phosphate, and urea (the last three as fertilizers), explosives, dyestuffs and resins.
Liquid ammonia has some similarity to water as it is hydrogen bonded and has a moderate dielectric constant, which permits it to act as an ionizing solvent. It is weakly selfionized to give ammonium ions, NH
4+and amide ions, NH
2-. It also dissolves electropositive metals to give blue solutions, which are believed to contain solvated electrons. Ammonia is extremely soluble in water giving basic solutions that contain solvated NH
3 molecules and small amounts of the ions NH
4+ and OH
-. The combustion of ammonia in air yields nitrogen and water. In the presence of catalysts NO, NO
2, and water are formed; this last reaction is the basis for the industrial production of nitric acid. Ammonia is a good proton acceptor (i.e. it is a base) and gives rise to a series of ammonium salts, e.g.NH
3 + HCl → NH
4+ + Cl
-.
It is also a reducing agent.
The participation of ammonia in the nitrogen cycle is a most important natural process. Nitrogen-flxing bacteria are able to achieve similar reactions to those of the Haber process, but under normal conditions of temperature and pressure. These release ammonium ions, which are converted by nitrifying bacteria into nitrite and nitrate ions.
調製方法
Ammonia is obtained commercially chiefly by synthesis from its
constituent elements, nitrogen and hydrogen, which are combined
under high pressure and temperature in the presence of a catalyst.
Ammonia solution is produced by dissolving ammonia gas in water.
空気と水の反応
Soluble in water with evolution of heat. The amount of heat generated may be large.
反応プロフィール
AMMONIA is a base. Reacts exothermically with all acids. Violent reactions are possible. Readily combines with silver oxide or mercury to form compounds that explode on contact with halogens. When in contact with chlorates Ammonia forms explosive ammonium chlorate [Kirk-Othmer, 3rd ed., Vol. 2, 1978, p. 470]. Reacts violently or produces explosive products with fluorine, chlorine, bromine and iodine and some of the interhalogen compounds (bromine pentafluoride, chlorine trifluoride). Mixing of bleaching powder (hypochlorite solution) with ammonia solutions produces toxic/explosive ammonia trichloride vapors. Undergoes potentially violent or explosive reactions on contact with 1,2-dichloroethane (with liquid ammonia), boron halides, ethylene oxide (polymerization), perchlorates or strong oxidants (chromyl chloride, chromium trioxide, chromic acid, nitric acid, hydrogen peroxide, chlorates, fluorine, nitrogen oxide, liquid oxygen). Reacts with silver chloride, silver oxide, silver nitrate or silver azide to form the explosive silver nitride. May react with some heavy metal compounds (mercury, gold(III) chloride) to produce materials that may explode when dry. [Bretherick, 5th ed., 1995, p. 1553].
危険性
Inhalation of concentrated fumes may be
fatal. Moderate fire risk, explosive limits in air 16–
25%. Forms explosive compounds in contact with
silver or mercury. Eye damage and upper respiratory
tract irritant.
健康ハザード
Ammonia is intensely irritating to the eyes,nose, and respiratory tract. Toxic effectsinclude lachrymation, respiratory distress,chest pain, and pulmonary edema. A concentration of 10 ppm may be detected by odor;irritation of eyes and nose is perceptible atabout 200 ppm. A few minutes of exposureto 3000 ppm can be intolerable, causing seri ous blistering of the skin, lung edema, andasphyxia, leading to death. It is corrosive toskin because it reacts with moisture to formcaustic ammonium hydroxide. Long expo sure may result in destruction of tissues
LC50 value, inhalation (mice): 4200 ppm/hr.
健康ハザード
Vapors cause irritation of eyes and respiratory tract. Liquid will burn skin and eyes. Poisonous; may be fatal if inhaled. Contact may cause burns to skin and eyes. Contact with liquid may cause frostbite.
火災危険
Mixing of ammonia with several chemicals can cause severe fire hazards and/or explosions. Ammonia in container may explode in heat of fire. Incompatible with many materials including silver and gold salts, halogens, alkali metals, nitrogen trichloride, potassium chlorate, chromyl chloride, oxygen halides, acid vapors, azides, ethylene oxide, picric acid and many other chemicals. Mixing with other chemicals and water. Hazardous polymerization may not occur.
燃焼性と爆発性
Ammonia vapor is slightly flammable (NFPA rating = 1) and ignites only with
difficulty. Ammonia forms explosive mixtures with air in the range 16 to 25%.
Water, carbon dioxide, or dry chemical extinguishers should be used for ammonia
fires.
农业用途
Anhydrous ammonia is an ammonium fertilizer made by
the Haber-Bosch process, by reacting hydrogen with
nitrogen in the ratio of 3: 1 at high temperatures (450 to
500'C) and pressure (about 500 atm) in the presence of an
iron catalyst promoted by potassium and alumina. The
nitrogen derived from air and the hydrogen obtained
from (a) synthesis gas, (b) steam reforming of naptha,
coal or coke (c) lignite, or (d) electrolysis of water, are
purified by standard procedures before use. The
anhydrous ammonia thus produced can be directly used
as a fertilizer. It can also be converted to ammonium salts
which are important fertilizers, by reacting ammonia
with nitric, sulphuric and phosphoric acids. Anhydrous
ammonia is also reacted with carbon dioxide to get urea
which is another important source of nitrogen.
Anhydrous ammonia is an important fluid fertilizer
and is the cheapest nitrogen source, having the highest
nitrogen content (about 82 %) among nitrogenous
fertilizers. However, because of safety and
environmental considerations, many dealers and users
are now switching over to other sources of nitrogen.
Anhydrous liquid ammonia can cause dehydration of
tissue and severe damage to the skin, lungs and eyes by
its freezing and caustic action. Because of the low vapor
pressure (6 bar at lO℃, 9 bar at 20℃ and 12 bar at
3O℃), anhydrous ammonia must be stored and
transported in pressure vessels.
Due to the volatile nature of anhydrous ammonia it
has to be injected with an applicator 15 to 30 cm below
the soil surface to be effective and to reduce ammonia
loss. Ammonia loss depends on the soil type,
its moisture content, and the depth to which the
applicator is injected.
Ammonia applicators range in size from small 5-row
rigs to large rigs that have a swath width of upto 20 m (65
feet) and are pulled by high-powered tractors.
Anhydrous ammonia is usually metered by a variable
orifice-type meter or by a piston pump.
Physical properties of anhydrous ammonia are
somewhat similar to other liquids under pressure like
butane or propane gas. Because of the difficulties in
handling anhydrous ammonia, water solutions of
ammonia, urea, ammonium phosphate or other soluble
solid nitrogen materials are used widely. Anhydrous
ammonia is also used in the preparation of protein feeds
for cattle and sheep, and as a defoliant to hasten the
shedding of cotton leaves to facilitate mechanical
harvesting.
农业用途
Anhydrous ammonia is the basic building block of almost
all nitrogen fertilizer materials. Most of the world's
ammonia is produced synthetically by a direct reaction of
the elements by the Haber-Bosch process. The process
involves an exothermic and reversible reaction that
proceeds with a concurrent decrease in volume.
There are certain conditions for the above reaction to
proceed optimally. These are: (a) temperature of 500℃,
(b) pressure of 270 to 350 atmospheres, (c) a catalyst
containing finely divided iron with molybdenum or
calcium as a promoter, finely divided osmium or
uranium, fmely divided nickel over pumice stone
or ferric oxide with traces of silica and potassium oxide,
and (d) pure gases (as otherwise the catalyst gets
poisoned).
Free ammonia is extremely toxic to micro-organisms,
animals and higher plants. Ammonia produced as a part
of normal metabolism is immediately converted into a
less harmful substance like urea and is excreted in urine.
Ammonia can readily penetrate cell membranes whereas
the ammonium ion is impermeable. There is a close
relationship between the pH and the concentration of the
free ammonium (NH
4+) ion. The capacity of soil to retain
ammonia increases with increasing soil moisture and clay
content.
Ammonia is the least expensive and most widely used
nitrogen fertilizer. It is used in the manufacture of other
fertilizers like urea, ammonium sulphate and ammonium
chloride.
Ammonia is also used in the manufacture of nitric
acid, hydrazine hydrate, urethane, acrylonitrile and
sodium carbonate (Solvay process). In addition,
ammonia is used as a refrigerant, in nitriding of steels, in
the petroleum industry, in the manufacture of explosives
and rocket fuel, as a yeast nutrient, etc.
Anhydrous ammonia, which has great affity for
water, contains approximately 82% nitrogen. This is the
highest nitrogen content that any nitrogen fertilizer can
have. As anhydrous ammonia is a gas at atmospheric
pressure, to avoid its loss to the atmosphere during
application, ammonia is injected at least 7 to 20 cm below
the soil.
The simplest nitrogen solution is aqua ammonia
which contains 25 to 29% ammonia by weight. Since
ammonia volatilizes above 10°C, aqua ammonia is
injected into the soil to a depth of 5 to 10 cm.
応用例（製薬）
Ammonia solution is typically not used undiluted in pharmaceutical
applications. Generally, it is used as a buffering agent or to adjust
the pH of solutions. Most commonly, ammonia solution (the
concentrated form) is used to produce more dilute ammonia
solutions.
Therapeutically, dilute ammonia solution is used as a reflex
stimulant in ‘smelling salts’, as a rubefacient, and as a counterirritant
to neutralize insect bites or stings.
工業用途
Ammonia (NH3) is an alkaline gas with a sharp, penetrating odor. Reacting nitrogen and
hydrogen under pressure, in the presence of a catalyst, produces ammonia. Gaseous
ammonia is flammable in air at concentrations of 15–28% by volume. Anhydrous liquid
ammonia is a colorless liquid with a strong odor. Ammonia, because of its unique
chemical properties to metal ions, is primarily used in hydrometallurgical processing.
In the mineral processing industry, ammonia is rarely used as a pH regulator. There was
only one operating plant in the world that used ammonia as a pH regulator in treatment
of a copper/zinc ore.
安全性
Ingestion of strong solutions of ammonia is very harmful and causes
severe pain in the mouth, throat, and gastrointestinal tract as well as
severe local edema with cough, vomiting, and shock. Burns to the
esophagus and stomach may result in perforation. Inhalation of the
vapor causes sneezing, coughing, and, in high concentration,
pulmonary edema. Asphyxia has been reported. The vapor is
irritant to the eyes. Strong solutions are harmful when applied to the
conjunctiva and mucous membranes. Topical application of even
dilute ammonia solutions, used to treat insect bites, has caused
burns, particularly when used with a subsequent dressing.
When used as an excipient, ammonia solution is generally
present in a formulation in a highly diluted form.
職業ばく露
Ammonia is used as a nitrogen source
for many nitrogen-containing compounds. It is used in the
production of ammonium sulfate and ammonium nitrate for
fertilizers; and in the manufacture of nitric acid, soda; synthetic
urea, synthetic fibers; dyes; and plastics. It is also
utilized as a refrigerant and in the petroleum refining and
chemical industries. It is used in the production of
many drugs and pesticides. Other sources of occupational
exposure include the silvering of mirrors, gluemaking, tanning
of leather; and around nitriding furnaces. Ammonia is
produced as a by-product in coal distillation and by the
action of steam on calcium cyanamide, and from the
decomposition of nitrogenous materials.
Source
Ammonia is released as a combustion product of coal, fuel oil, natural gas, wood, butane,
and propane (quoted, Verschueren, 1983).
Ammonia naturally occurs in soybean (8,600 ppm), evening-primrose seeds (2,300–2,455 ppm),
lambsquarter, and tobacco leaves (Duke, 1992).
環境運命予測
Chemical/Physical. Reacts violently with acetaldehyde, ethylene oxide, ethylene dichloride
(Patnaik, 1992).
Reacts with acids forming water soluble ammonium salts.
貯蔵
All work with ammonia should be
conducted in a fume hood to prevent exposure by inhalation, and splash goggles and
impermeable gloves should be worn at all times to prevent eye and skin contact.
Cylinders of ammonia should be stored in locations appropriate for compressed gas
storage and separated from incompatible compounds such as acids, halogens, and
oxidizers. Only steel valves and fittings should be used on ammonia containers;
copper, silver, and zinc should not be permitted to come into contact with ammonia.
貯蔵
On exposure to the air, ammonia solution rapidly loses ammonia.
Ammonia solution should be stored in a well-closed container,
protected from the air, in a cool, dry place. The storage temperature
should not exceed 208℃.
輸送方法
Shipped in tank cars, tank trucks, barges, and
steel cylinders. Labeling and restrictions vary with concentration: NA1005 Ammonia, anhydrous, Hazard
Class: 2.2; Labels: 2.2-Nonflammable compressed gas,
Domestic (U.S.), Inhalation Hazard (Special Provision 13).
UN1005 Ammonia, anhydrous, Hazard Class: 2.3; Labels:
2.3-Poison Gas, 8-Corrosive material International,
Inhalation Hazard Zone D. UN2672 Ammonia solutions,
relative density between 0.880 and 0.957 @ 15 C in water,
with .10 % but NOT . 35 % ammonia, Hazard class: 8;
Labels: 8-Corrosive material. UN2073 Ammonia solution,
relative density less than 0.880 @ 15 C in water, with .
35% but NOT . 50% ammonia, Hazard Class: 2.2;
Labels: 2.2-Nonflammable compressed gas. Note: Also
used for Ammonium hydroxide, CAS1336-21-6, Record
A:0110.
純化方法
Dry the liquid, and store it, with sodium in a steel cylinder, then distil and condense it by means of liquid air, the non-condensable gases being pumped off. In order to obtain liquid NH3 from a cylinder, turn the cylinder upside-down (i.e. with the valve at the bottom, use a metal stand to secure it in this position) and lead a plastic tube from the tap to a measuring cylinder placed in an efficient fume cupboard which is kept running. Turn the tap on and allow the ammonia to be released. At first, gas and liquid will splatter out (make sure that the plastic tube is secure), but soon the liquid will drip into the measuring cylinder. The high latent heat of evaporation will cool the ammonia so that the liquid will remain cool and not boil vigorously. If the ammonia is required dry, the necessary precautions should be taken, i.e. the gas is allowed to flow through tubes packed with coarse CaO pellets. AMMONIA (gas, liquid or aqueous solution) is very irritating and should not be inhaled in any quantity as it can lead to olfactory paralysis (temporary or permanent).
不和合性
Violent reaction with strong oxidizers
and acids. Shock-sensitive compounds may be formed with
gold, halogens, mercury, mercury oxide, and silver oxide.
Fire and explosions may be caused by trimethylammonium
amide, 1-chloro-2,4-dinitrobenzene, o-chloronitrobenzene,
platinum, trioxygen difluoride, selenium difluoride dioxide,
boron halides, mercury, chlorine, iodine, bromine, hypochlorites,
chlorine bleach, amides, organic anhydrides; isocyanates,
vinyl acetate; alkylene oxides; epichlorohydrin,
and aldehydes. Attacks some coatings, plastics, rubber,
copper, brass, bronze, aluminum, steel, tin, zinc, and their
alloys.
不和合性
Ammonia solution reacts vigorously with sulfuric acid or other
strong mineral acids and the reaction generates considerable heat;
the mixture boils.
廃棄物の処理
Dilute with water, neutralize
with HCl and discharge to sewer. Recovery is an option to
disposal which should be considered for paper manufacture,
textile treating, fertilizer manufacture and chemical process
wastes.
規制状況(Regulatory Status)
Included in the FDA Inactive Ingredients Database (oral suspensions,
topical preparations). Included in nonparenteral medicines
licensed in the UK. Included in the Canadian List of Acceptable
Non-medicinal Ingredients.
強アンモニア 上流と下流の製品情報
原材料
準備製品
