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MANUFACTURE OF AMMONIA
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Purified
NH3
Synthesis
Gas
Oil
Filter
1 mol N2
3 mol H2
Feed
Guard
Converter
Recycle GasSmall purge stream
to preventaccumulation of
diluents such as Ar
Gas
Liquid-15C
NH3
Refrigerant Spherical tankStorage
Cooling Water
Water Chiller
Spent cooling water
Centrifugal
Recirculator
Reactor
Co
ldGas
500-600C
100-1000atms
Separato
r
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INTRODUCTION
At the beginning of the 20th century there was a shortage of
naturally occurring, nitrogen-rich fertilizers, such as Chilesaltpetre, which prompted the German Chemist Fritz Haber,and others, to look for ways of combining the nitrogen in theair with hydrogen to form ammonia, which is a convenientstarting point in the manufacture of fertilizers.
This process was also of interest to the German chemicalindustry as Germany was preparing for World War I andnitrogen compounds were needed for explosives.
The hydrogen for the ammonia synthesis was made by thewater-gas process (a Carl Bosch invention) which involvesblowing steam through a bed of red hot coke resulting in theseparation of hydrogen from oxygen.
The nitrogen was obtained by distillation of liquid air, then bycooling and compressing air.
In ammonia production, the hydrogen and nitrogen are mixedtogether in ratio of 3:1by volume and compressed to around200 times atmospheric pressure.
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PHYSICAL PROPERTIES
Molecular formula NH3
Molar mass 17.036gm/mL
Appearance
Colorless gas with
pungent odour
Density
0.6942g/cm3
Melting point
-77.73C
Boiling point -33.34C
Solubility 89.9g/100mL at 100C
Molecular shape Trigonal pyramid
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TYPES OF PROCESS
All process for synthetic ammonia are based on
the pressure, catalytic reactions of nitrogen,
hydrogen.The main classification of the ammonia process
are 1.Haber process
2.Haber-Bosch process
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CHEMICAL REACTION
N2+3H2>2NH3
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HABER PROCESS
The Haber 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.
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LE CHETALIERS PRINCIPLEByLe Chetalier's Principle:
increasing the pressure causes the equilibrium position tomove to the right resulting in a higher yeild of ammonia sincethere are more gas molecules on the left hand side of theequation (4 in total) than there are on the right hand side ofthe equation (2). Increasing the pressure means the systemadjusts to reduce the effect of the change, that is, to reduce the
pressure by having fewer gas molecules. decreasing the temperature causes the equilibrium position to
move to the right resulting in a higher yield of ammonia sincethe reaction is exothermic (releases heat). Reducing thetemperature means the system will adjust to minimise the
effect of the change, that is, it will produce more heat sinceenergy is a product of the reaction, and will therefore producemore ammonia gas as well
However, the rate of the reaction at lower temperatures isextremely slow, so a higher temperature must be used to speed
up the reaction which results in a lower yield of ammonia.
http://www.ausetute.com.au/lechatsp.htmlhttp://www.ausetute.com.au/lechatsp.html7/30/2019 III sem ICT (5)
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SOME NOTES ON THE CONDITIONS
Temperature
Pressure
Catalyst
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TEMPERATURE
Equilibrium considerations The forward reaction (the production of ammonia) is
exothermic.
According to Le Chatelier's Principle, this will befavoured if you lower the temperature. The system will
respond by moving the position of equilibrium tocounteract this - in other words by producing more heat.
In order to get as much ammonia as possible in theequilibrium mixture, you need as low a temperature as
possible. However, 400 - 450C isn't a low temperature!
The compromise
400 - 450C is a compromise temperature producing areasonably high proportion of ammonia in theequilibrium mixture (even if it is only 15%), but in a very
short time.
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PRESSURE
Equilibrium considerations
Notice that there are 4 molecules on the left-hand side of theequation, but only 2 on the right.
According to Le Chatelier's Principle, if you increase the
pressure the system will respond by favouring the reactionwhich produces fewer molecules. That will cause the pressureto fall again.
In order to get as much ammonia as possible in theequilibrium mixture, you need as high a pressure as possible.200 atmospheres is a high pressure, but not amazingly high.
The compromise
200 atmospheres is a compromise pressure chosen oneconomic grounds. If the pressure used is too high, the cost ofgenerating it exceeds the price you can get for the extraammonia produced.
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CATALYST
Equilibrium considerations
The catalyst has no effect whatsoever on the position of theequilibrium. Adding a catalyst doesn't produce any greater
percentage of ammonia in the equilibrium mixture. Its only
function is to speed up the reaction.Rate considerations
In the absence of a catalyst the reaction is so slow thatvirtually no reaction happens in any sensible time. Thecatalyst ensures that the reaction is fast enough for a dynamicequilibrium to be set up within the very short time that thegases are actually in the reactor.
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VARIOUS STEPS INVOLVED
Synthesis gas
Filtration
Feed guard converter Reaction
Separation
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1.SYNTHESIS GAS
Synthesis gas contains 1 mole of pure N2 from
the air and 3 moles of H2 from the natural gas.
Synthesis gas is compressed to the operating
pressure(100-1000 atm) depending on
conversion required.
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2.FILTRATION
Compressed gas is sent to a filter to
remove compression oil.
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3.FEED GUARD CONVERTER
Feed guard converter converts CO and CO2 to
CH4 and removes traces of H2O, H2S,
phosphorous.
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4.REACTION
The relatively cool gas is added along the
outside of converter tube to provide cooling so
that carbon steel can be used for the thick wall
pressure vessel and internal tubes. The
preheated gas flows through the inside of the
tubes which contains promoted porous iron
catalyst at 500-550C.Conversion of NH3 is 8-30%.
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5.SEPARATION
Ammonia vapours is removed by
condensation first with water cooling and then
NH3 refrigerator. The unconverted N2 and H2mixture is recirculated to allow an 85-90%
yield.
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APPLICATIONS
Industry Use
Fertilser production of:
ammonium sulfate, (NH4)2SO4
ammonium phosphate, (NH4)3PO4
ammonium nitrate, NH4NO3
Urea.
Explosives ammonium nitrate, NH4NO3
Fibres & Plastics nylon, -[(CH2)4-CO-NH-(CH2)6-NH-CO]-,and other
polyamidesRefrigeration used for making ice, large scale refrigeration plants,
air-conditioning units in buildings and plants
Pulp & Paper ammonium hydrogen sulfite, NH4HSO3, enables some
hardwoods to be used
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Chemicals synthesis of:
nitric acid, HNO3, which is used in making explosives
such as TNT (2,4,6-trinitrotoluene), nitroglycerine which
is also used as a vasodilator (a substance that dilatesblood vessels) and PETN (pentaerythritol nitrate).
sodium hydrogen carbonate (sodium bicarbonate),
NaHCO3
sodium carbonate, Na2CO3
hydrogen cyanide (hydrocyanic acid), HCN
hydrazine, N2H4 (used in rocket propulsion systems)
Pharmaceuticals used in the manufacture of drugs such as sulfonamide which
inhibit the growth and multiplication of bacteria that require p-
aminobenzoic acid (PABA) for the biosynthesis of folic acids,
anti-malarials and vitamins such as the B vitamins nicotinamide(niacinamide) and thiamine.
Cleaning ammonia in solution is used as a cleaning agent such as in
'cloudy ammonia'
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A PRESENTATION BY
DEEPTHI.R
BAGHYA LAKSHMI.M
BALAJI.R
DINESHKUMAR.S
DINESHKUMAR.M
ESSAKIRAJ
EZHILARASAN
GURUNATHAN HARISH
HARIRAMAKRISHNAN