Haber Process?????Detail
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Haber Process
●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.
●It is named after its inventors, the German chemists Fritz Haber and Carl Bosch, who developed it in the first decade of the 20th century.
The Haber Process is used in the manufacturing of ammonia from nitrogen and hydrogen, and then goes on to explain the reasons for the conditions used in the process. The process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.
N2(g)+3H2(g)⇌2NH3(g)
with ΔH=−92.4kJ/mol.
A flow scheme for the Haber Process looks like this:
Figure \PageIndex{1}: Scheme of the Haber Process
General Conditions of the Process
The catalyst: The catalyst is actually slightly more complicated than pure iron. It has potassium hydroxide added to it as a promoter - a substance that increases its efficiency.
The pressure: The pressure varies from one manufacturing plant to another, but is always high. You cannot go far wrong in an exam quoting 200 atmospheres.
Recycling: At each pass of the gases through the reactor, only about 15% of the nitrogen and hydrogen converts to ammonia. (This figure also varies from plant to plant.) By continual recycling of the unreacted nitrogen and hydrogen, the overall conversion is about 98%.
Composition
The proportions of nitrogen and hydrogen: The mixture of nitrogen and hydrogen going into the reactor is in the ratio of 1 volume of nitrogen to 3 volumes of hydrogen. Avogadro's Law says that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. That means that the gases are going into the reactor in the ratio of 1 molecule of nitrogen to 3 of hydrogen. That is the proportion demanded by the equation.
In some reactions you might choose to use an excess of one of the reactants. You would do this if it is particularly important to use up as much as possible of the other reactant - if, for example, it was much more expensive. That does not apply in this case. There is always a down-side to using anything other than the equation proportions. If you have an excess of one reactant there will be molecules passing through the reactor which cannot possibly react because there is not anything for them to react with. This wastes reactor space - particularly space on the surface of the catalyst.
By mixing one part ammonia to nine parts air with the use of a catalyst, the ammonia will get oxidized to nitric acid.
4 NH_3 + 5 O_2 \rightarrow 4 NO + 6 H_2O
2 NO + O_2 \rightarrow 2 NO_2
2 NO_2 + 2 H_2O \rightarrow 2 HNO_3 + H_2By mixing one part ammonia to nine parts air with the use of a catalyst, the ammonia will get oxidized to nitric acid.
4 NH_3 + 5 O_2 \rightarrow 4 NO + 6 H_2O
2 NO + O_2 \rightarrow 2 NO_2
2 NO_2 + 2 H_2O \rightarrow 2 HNO_3 + H_2By mixing one part ammonia to nine parts air with the use of a catalyst, the ammonia will get oxidized to nitric acid.
4 NH_3 + 5 O_2 \rightarrow 4 NO + 6 H_2O
2 NO + O_2 \rightarrow 2 NO_2
2 NO_2 + 2 H_2O \rightarrow 2 HNO_3 + H_2
