A report on Fertilizer, Haber process, Nitrogen fixation and Ammonia

A farmer spreading manure to improve soil fertility

Schematic representation of the nitrogen cycle. Abiotic nitrogen fixation has been omitted.

Ball-and-stick model of the diamminesilver(I) cation, [Ag(NH3)2]+

World population supported with and without synthetic nitrogen fertilizers.

A historical (1921) high-pressure steel reactor for production of ammonia via the Haber process is displayed at the Karlsruhe Institute of Technology, Germany

Nodules are visible on this broad bean root

Ball-and-stick model of the tetraamminediaquacopper(II) cation, [Cu(NH3)4(H2O)2](2+)

Founded in 1812, Mirat, producer of manures and fertilizers, is claimed to be the oldest industrial business in Salamanca (Spain).

First reactor at the Oppau plant in 1913

Six tomato plants grown with and without nitrate fertilizer on nutrient-poor sand/clay soil. One of the plants in the nutrient-poor soil has died.

Equipment for a study of nitrogen fixation by alpha rays (Fixed Nitrogen Research Laboratory, 1926)

This high-pressure reactor was built in 1921 by BASF in Ludwigshafen and was re-erected on the premises of the University of Karlsruhe in Germany.

Lightning heats the air around it breaking the bonds of starting the formation of nitrous acid.

Total nitrogenous fertilizer consumption per region, measured in tonnes of total nutrient per year.

Modern ammonia reactor with heat exchanger modules: The cold gas mixture is preheated to reaction temperature in heat exchangers by the reaction heat and cools in turn the produced ammonia.

An apatite mine in Siilinjärvi, Finland.

Compost bin for small-scale production of organic fertilizer

Ammoniacal Gas Engine Streetcar in New Orleans drawn by Alfred Waud in 1871.

The X-15 aircraft used ammonia as one component fuel of its rocket engine

Applying superphosphate fertilizer by hand, New Zealand, 1938

Anti-meth sign on tank of anhydrous ammonia, Otley, Iowa. Anhydrous ammonia is a common farm fertilizer that is also a critical ingredient in making methamphetamine. In 2005, Iowa used grant money to give out thousands of locks to prevent criminals from getting into the tanks.

The world's longest ammonia pipeline (roughly 2400 km long), running from the TogliattiAzot plant in Russia to Odessa in Ukraine

N-Butylthiophosphoryltriamide, an enhanced efficiency fertilizer.

Hydrochloric acid sample releasing HCl fumes, which are reacting with ammonia fumes to produce a white smoke of ammonium chloride.

Fertilizer use (2018). From FAO's World Food and Agriculture – Statistical Yearbook 2020

Production trend of ammonia between 1947 and 2007

The diagram displays the statistics of fertilizer consumption in western and central European counties from data published by The World Bank for 2012.

Main symptoms of hyperammonemia (ammonia reaching toxic concentrations).

Runoff of soil and fertilizer during a rain storm

Ammonia occurs in the atmospheres of the outer giant planets such as Jupiter (0.026% ammonia), Saturn (0.012% ammonia), and in the atmospheres and ices of Uranus and Neptune.

Large pile of phosphogypsum waste near Fort Meade, Florida.

Red circles show the location and size of many dead zones.

Global methane concentrations (surface and atmospheric) for 2005; note distinct plumes

The Haber process, also called the Haber–Bosch process, is an artificial nitrogen fixation process and is the main industrial procedure for the production of ammonia today.

- Haber process

Nitrogen fixation is a chemical process by which molecular nitrogen, with a strong triple covalent bond, in the air is converted into ammonia or related nitrogenous compounds, typically in soil or aquatic systems but also in industry.

- Nitrogen fixation

The process converts atmospheric nitrogen (N2) to ammonia (NH3) by a reaction with hydrogen (H2) using a metal catalyst under high temperatures and pressures:

- Haber process

Biologically, it is a common nitrogenous waste, particularly among aquatic organisms, and it contributes significantly to the nutritional needs of terrestrial organisms by serving as a precursor to 45 percent of the world's food and fertilizers.

- Ammonia

As part of the nitrogen cycle, it is essential for agriculture and the manufacture of fertilizer.

- Nitrogen fixation

In particular, nitrogen-fixing chemical processes such as the Haber process at the beginning of the 20th century, amplified by production capacity created during World War II led to a boom in using nitrogen fertilizers.

- Fertilizer

This process was used to fix atmospheric nitrogen (N2) into nitric acid (HNO3), one of several chemical processes generally referred to as nitrogen fixation.

- Fertilizer

Only some bacteria and their host plants (notably legumes) can fix atmospheric nitrogen (N2) by converting it to ammonia.

- Fertilizer

The process was eclipsed by the Haber process, which was discovered in 1909.

- Nitrogen fixation

The Haber–Bosch process to produce ammonia from the nitrogen in the air was developed by Fritz Haber and Carl Bosch in 1909 and patented in 1910.

- Ammonia

The ammonia is used mainly as a nitrogen fertilizer as ammonia itself, in the form of ammonium nitrate, and as urea.

- Haber process

Therefore, nitrogen fixation is required for the synthesis of amino acids, which are the building blocks of protein.

- Ammonia

1 related topic with Alpha

Nitrogen

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Chemical element with the symbol N and atomic number 7.

The shapes of the five orbitals occupied in nitrogen. The two colours show the phase or sign of the wave function in each region. From left to right: 1s, 2s (cutaway to show internal structure), 2px, 2py, 2pz.

Table of nuclides (Segrè chart) from carbon to fluorine (including nitrogen). Orange indicates proton emission (nuclides outside the proton drip line); pink for positron emission (inverse beta decay); black for stable nuclides; blue for electron emission (beta decay); and violet for neutron emission (nuclides outside the neutron drip line). Proton number increases going up the vertical axis and neutron number going to the right on the horizontal axis.

Molecular orbital diagram of dinitrogen molecule, N2. There are five bonding orbitals and two antibonding orbitals (marked with an asterisk; orbitals involving the inner 1s electrons not shown), giving a total bond order of three.

Solid nitrogen on the plains of Sputnik Planitia on Pluto next to water ice mountains

Structure of [Ru(NH3)5(N2)]2+ (pentaamine(dinitrogen)ruthenium(II)), the first dinitrogen complex to be discovered

Mesomeric structures of borazine, (–BH–NH–)3

Standard reduction potentials for nitrogen-containing species. Top diagram shows potentials at pH 0; bottom diagram shows potentials at pH 14.

Nitrogen dioxide at −196 °C, 0 °C, 23 °C, 35 °C, and 50 °C. converts to colourless dinitrogen tetroxide at low temperatures, and reverts to at higher temperatures.

Fuming nitric acid contaminated with yellow nitrogen dioxide

Schematic representation of the flow of nitrogen compounds through a land environment

A container vehicle carrying liquid nitrogen.

Many industrially important compounds, such as ammonia, nitric acid, organic nitrates (propellants and explosives), and cyanides, contain nitrogen.

Synthetically produced ammonia and nitrates are key industrial fertilisers, and fertiliser nitrates are key pollutants in the eutrophication of water systems.

Nitrogen fixation by industrial processes like the Frank–Caro process (1895–1899) and Haber–Bosch process (1908–1913) eased this shortage of nitrogen compounds, to the extent that half of global food production (see Applications) now relies on synthetic nitrogen fertilisers.