Properties[change | change source]
- It is a gas at room temperature
- It is colourless
- It has a strong, sharp smell
- It is a base
- It is an alkali
- It is harmful when eaten or breathed
- It dissolves in water to form a solution called household ammonia
Uses of ammonia[change | change source]
- Making nitric acid
- Preparing wood pulp
- Dissolved in water, it is household ammonia, used in cleaning (such as glass)
- Refrigeration (making things cold)
- Creating fertilizers to use on farms
Ways it can be made[change | change source]
- Urination can be a source of Ammonia
- Distillation (boiling for separation) of nitrogenous vegetable and animal waste
- The Haber process using high temperature and pressure with catalysts (things that make reactions faster)
Ammonia in fish tanks[change | change source]
Ammonia is toxic. If a goldfish tank is dirty from their waste, the fish can suffer from ammonia burns which cause black spots or patches on their body. The tank must be large enough and have a filter.
Manufacture of ammonia[change | change source]
- See also: Haber-Bosch process
Because of its many uses, ammonia is one of the most highly produced inorganic chemicals. Dozens of chemical plants worldwide produce ammonia. The worldwide ammonia production in 2004 was 109 million metric tonnes. China produced 28.4% of the worldwide production (increasingly from coal as part of urea synthesis) followed by India with 8.6%, Russia with 8.4%, and the United States with 8.2%. About 80% or more of the ammonia produced is used for fertilizing agricultural crops.
Before the start of World War I, most ammonia was obtained by the dry distillation of nitrogenous vegetable and animal waste products, including camel dung, where it was distilled by the reduction of nitrous acid and nitrites with hydrogen; in addition, it was produced by the distillation of coal, and also by the decomposition of ammonium salts by alkaline hydroxides such as quicklime, the salt most generally used being the chloride (sal-ammoniac) thus:
- 2 NH4Cl + 2 CaO → CaCl2 + Ca(OH)2 + 2 NH3
Today, the typical modern ammonia-producing plant first converts natural gas (i.e., methane) or liquefied petroleum gas (such gases are propane and butane) or petroleum naphtha into gaseous hydrogen. The process used in producing the hydrogen begins with removal of sulfur compounds from the natural gas (because sulfur deactivates the catalysts used in subsequent steps). Catalytic hydrogenation converts organosulfur compounds into gaseous hydrogen sulfide:
- H2 + RSH → RH + H2S (g)
- H2S + ZnO → ZnS + H2O
- CH4 + H2O → CO + 3 H2
- CO + H2O → CO2 + H2
The final step in producing the hydrogen is to use catalytic methanation to remove any small residual amounts of carbon monoxide or carbon dioxide from the hydrogen:
- CO + 3 H2 → CH4 + H2O
- CO2 + 4 H2 → CH4 + 2 H2O
To produce ammonia, the hydrogen then reacts with nitrogen (derived from process air) using a magnetite catalyst under high pressure to form anhydrous liquid ammonia. This step is known as the ammonia synthesis loop (also referred to as the Haber-Bosch process):
- 3 H2 + N2 → 2 NH3
Hydrogen required for ammonia synthesis could also be produced economically using other sources like coal or coke gasification, less economically from the electrolysis of water into oxygen + hydrogen and other alternatives that are presently impractical for large scale production. At one time, most of Europe's ammonia was produced from the Hydro plant at Vemork, using electrolysis.
Related pages[change | change source]
References[change | change source]
- "United States Geological Survey publication". http://minerals.usgs.gov/minerals/pubs/commodity/nitrogen/nitromcs05.pdf. Retrieved 2009-07-07.
- "New coal-based ammonia and urea capacity.(China)". January 2004. http://www.highbeam.com/doc/1G1-113564920.html. Retrieved 2009-07-07.
- "Nobel Prize in Chemistry (1918) – Haber-Bosch process"]. http://nobelprize.org/chemistry/laureates/1918/press.html. Retrieved 2009-07-07.
- "Chemistry of the Group 2 Elements – Be, Mg, Ca, Sr, Ba, Ra". BBC.co.uk. http://www.bbc.co.uk/dna/h2g2/A1002934. Retrieved 2009-07-07.