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About 90 percent of all the ammonia used in the United States goes to the production of fertilizers.

The Haber-Bosch process remains the most common form of ammonia production in many countries, including the United States.

Ammonia is used in a variety of forms as a fertilizer.

In addition to its use in the manufacture of fertilizers and explosives, smaller amounts of ammonia are used: As a refrigerant; In the manufacture of plastics; As a raw material in the manufacture of other nitrogen-containing chemicals; In the production of dyes; As a rocket fuel; For the neutralization of acids during the refining of petroleum; In order to produce specialized types of steel; and As a nutrient in yeast cultures in food processing operations.

The next largest use of ammonia is in the synthesis of nitric acid (HNO3). In a process developed by the German chemist Wilhelm Ostwald (1853–1932), ammonia, oxygen, and water are reacted together in a series of steps that results in the formation of nitric acid. Nitric acid, the thirteenth most important chemical in the United States in terms of productions, has a number of important uses, including the manufacture of explosives. Like the Haber-Bosch process, the Ostwald process contributed to the success experienced by Germany during World War I.

Both gaseous and liquid ammonia pose moderate health hazards to those who come into contact with them. For example, farmers who handle liquid ammonia risk the possibility of painful blistering of the skin or damage to the mucous membranes if they come into contact with the ferilizer. Ammonia fumes can irritate the mouth, nose, and throat, causing coughing and gagging responses. Higher levels of exposure may irritate the lungs, resulting in shortness of breath and producing headaches, nausea, and vomiting. Very high exposures can cause a buildup of fluid in the lungs that can result in death. Since ammonia is a common ingredient of many household products, everyone should be aware of its health risks, although the threat posed by such products is, in fact, very small.

hydrogen bonding

The largest use of ammonia is in fertilizers, which are applied to the soil and help provide increased yields of crops such as corn, wheat, and soybeans. Liquid ammonia, ammonia/water solutions, and chemicals made from ammonia, such as ammonium salts and urea, are all used as sources of soluble nitrogen. Urea, which is made from ammonia and carbon dioxide, can also be used as a feed supplement for cattle, aiding in the rapid building of protein by the animals.

Because of its basic properties, ammonia is able to react with acidic gases such as nitrogen oxides and sulfur oxides to form ammonium salts

oxidation of ammonia

oxidation of ammonia

oxidation of ammonia

oxidation of ammonia

oxidation of ammonia

oxidation of ammonia

oxidation of ammonia

Ammonia is used in a variety of forms as a fertilizer. It can be liquified or dissolved in water and sprayed on land, or it can be converted into any one of a number of compounds, such as ammonium nitrate, ammonium phosphate, or ammonium sulfate.

When dry, this substance is so sensitive that the lightest touch will cause it to explode with a crackling sound and a puff of purple iodine vapor.

Ammonium hydroxide exhibits the characteristics of a weak base, turning litmus paper blue, and neutralizing acids with the formation of ammonium salts.

In liquid or frozen ammonia, the molecules attract one another through sharing a hydrogen atom between one molecule and the next, called hydrogen bonding. In this attraction, called association, compounds apparently containing free electrons can be obtained by treating sodium/ammonia solutions with complexing agents.

boiling point -28.03°F [-33.35°C]

The largest use of ammonia is in fertilizers,

In ancient Egypt, ammonium compounds were used in rites honoring the god Ammon, from which came the name we still use for the gas and its compounds.

Ammonia, composed of three parts hydrogen and one part nitrogen, is a sharp-smelling, flammable, and toxic gas that is very soluble in water, where it acts as a base in its chemical reactions.

German chemists Fritz Haber and Carl Bosch

The synthesis reaction itself produces some heat, and great attention is given to heat efficiency and use of waste heat.

which amounts to about 40 pounds (18 kg) for each person on Earth.

Ammonium hydroxide exhibits the characteristics of a weak base,

Much nitrogen is normally excreted by humans (and other mammals) as urea, a water soluble solid, but fish can excrete ammonia directly.

These bacteria and algae possess an enzyme called nitrogenase that permits them to convert nitrogen to ammonia at 77°F (25°C) and 1 bar of pressure, much milder conditions than those of the Haber-Bosch process.

Although Earth's atmosphere is free of ammonia

nited

United States production of ammonia reached 17 million tons in 1991, and demand was even larger than U.S. production, leading to about two million tons of imports.

When dry, this substance is so sensitive that the lightest touch will cause it to explode with a crackling sound and a puff of purple iodine vapor.

New uses may develop, particularly for ammonia as a relatively inexpensive base with unique properties, for liquid ammonia as a solvent, and as a storage medium for hydrogen, as the nations evolve toward alternative fuels.

For this reason, capacity and production will continue to grow

200,000 tons of ammonia were released into the environment

earned to generate ammonia from animal parts such as deerhorn, and obtained ammonial preparations

In ancient Egypt, ammonium compounds were used in rites honoring the god Ammon, from which came the name we still use for the gas and its compounds.

Joseph Priestley (1733-1804) first collected and experimented with the pure substance. C. L. Berthollet (1748-1822) proved that ammonia is composed of nitrogen and hydrogen.

The copper (II) ammonia complex, in solution, is deep blue in color,

German chemists Fritz Haber and Carl Bosch learned how to make ammonia in large quantities by high-pressure catalytic reactions of nitrogen (from air) with hydrogen.

ability to dissolve cellulose, and has been used in the process for making regenerated cellulose fibers, or rayon.

Ammonia molecules possess a pyramidal shape, with the nitrogen atom at the vertex.

Ammonia molecules possess a pyramidal shape, with the nitrogen atom at the vertex.

The gases that enter the catalytic converter must be highly purified and free of sulfur compounds, which adversely affect the catalyst.

Since the hydrogen is usually derived from a natural gas called methane, the price of ammonia is very sensitive to the availability or price of fuels.

These bacteria and algae possess an enzyme called nitrogenase that permits them to convert nitrogen to ammonia at 77°F (25°C) and 1 bar of pressure, much milder conditions than those of the Haber-Bosch process.

Ammonia will continue to be important for agriculture and for the whole nitrogen chemicals industry.

In liquid or frozen ammonia, the molecules attract one another through sharing a hydrogen atom between one molecule and the next, called hydrogen bonding. In this attraction, called association, compounds apparently containing free electrons can be obtained by treating sodium/ammonia solutions with complexing agents.