It is lighter than air and has a sharp, stinging odour. Ammonia can be inhaled safely if it is greatly diluted in air, but concentrated ammonia gas can cause suffocation and death. Ammonia does not burn is air, but it burns in oxygen with a weak yellow flame.

Properties: - Ammonia gas is extremely soluble in water, as it is able to form hydrogen bonds with polar water molecules. It changes to a liquid at V33.35 oC. Liquid ammonia boils at the same temperature. It freezes to a clear solid at 77.7 oC. In going from a liquid back to a gas, ammonia absorbs a large amount of heat from its surroundings. Upon evaporation, one gram of ammonia absorbs 327 calories of heat. For this reason, ammonia is widely used in refrigeration equipment. Liquid ammonia is used in the chemical laboratory as a solvent. It is a better solvent for ionic and polar compounds than ethanol, but not as good as water; it is a better solvent for nonpolar covalent compounds that water, but not as good as ethanol. It dissolves alkali metals and barium, calcium and strontium by forming an uns

Ammonia is manufactured by combining nitrogen and hydrogen directly in a process known as the Haber-Bosch Process.

Because raising the temperature will increase the speed of both the forward and reverse reactions, a high temperature should bring the reaction to equilibrium rapidly. However, according to LeChatelier's Principle, raising the temperature favours the endothermic reaction, shifting the equilibrium in this case to the left, lowering the yield of ammonia and increasing the time needed to obtain a given quantity of ammonia. In fact, at 500 oC, only 0.1% of the mass at equilibrium will be ammonia if the reaction is done at 1 atmosphere of pressure. But according to LeChatelier's Principle, by increasing the pressure, the equilibrium favours the reaction in which fewer gas molecules are produced. Such a stress shifts the equilibrium to the right and produces a mixture richer in ammonia. The aim of industry is to control the reactions so that large amount of useful products are yielded quickly. In the industrial preparation of ammonia, the gasses are compressed to high pressu!

Fritz Haber discovered in 1913 the process for synthesising ammonia. It was used in the first World War to create bombs and explosives for his country. Despite this use of his project, he was still awarded the Nobel Prize for Chemistry in 1918 for his work and research. Later, in the 1930's, a German chemist, Karl Bosch, adapted this method for commercial and industrial use. Now, the Haber-Bosch Process is used in the ma

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