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4/28/2008
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AmmoniaAmmonia
Background informationBackground information
Ammonia is one of the main products of chemical industry (especially for fertilizers and explosives)(especially for fertilizers and explosives)
In the past ammonia was produced as a by-product during the distillation of coal in coke ovens and gas works insufficient already at the turn of the century
Ammonia production using nitrogen from the air : Haber-Bosch process
The discovery of nitrogen fixation from air was suggested to be the most important scientific advancement of the 20th century.
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Ammonia production in numbersAmmonia production in numbers
Ammonia usesAmmonia uses
85 % of ammonia is used for nitrogen fertilizers-urea is the most important accounting for 40% of ammonia usage
Other industrial uses include the production of nitric acid, amines, nitriles, nylon and organic nitrogen compounds
Environmental applications removal of NOx from flue gases of pilot plants
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Energy data for nitrogenEnergy data for nitrogen
Value(kJ/mol)
Compare with(kJ/mol)(kJ/mol) (kJ/mol)
Bond dissociation energy 945 C-H in CH4: 439Ionization energy 1503 O2: 1165Electron affinity 34900 O2: 43
H = -91 44 kJ/molH = -91.44 kJ/mol
Ammonia production from airAmmonia production from air
Problems: Bond dissociation energy and electron affinity very high
ti ti b i i ti l i iblactivation by ionization nearly impossible
Fraction of NH3 in a 3:1 mixture of H2 and N2 at 1290 K: 0,01%
Industrial production only possible if good catalysts are found
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Haber Haber Bosch Bosch process developmentprocess development
Haber and Bosch developed a process for the production of ammonia from nitrogen in 1908 1913
Testing 6500 catalysts they discovered the high activity of iron based catalysts.
Modern catalysts are still closely related to original ones
ThermodynamicsThermodynamics
High pressure and low temperature are needed At temperatures lower than 670 K the rate of the reaction is very
llow minimum temperature required to reach the equilibrium sufficiently fast
Typical reaction conditions: 675 K at inlet; 720 770 K at outlet 100 250 bar100 250 bar
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ThermodynamicsThermodynamics
Catalysts for ammonia synthesis
The iron catalyst consists of magnetite (Fe3O4) which is enriched(promoted) most frequently with Al- and K- (or Ca, Mg, Si)-oxides. The promoters are dissolved in the magnetite or form metal ferrites
Composition: 89-95% Fe3O4, 2-4% Al2O3, 0.5-1% K2O, 2-4% CaO Catalyst is produced by fusing (melting) magnetite ore with the other
promoters at 1700oC and pouring melt into water to form fine particles
Iron being a transition metal with partially occupied d-bands represents asurface suitable for adsorption and dissociation of N2 molecules
Not only iron based catalysts are active for ammonia synthesis Os, Ru are equally active with Fe Ru is most active in ammonia decomposition Mo, U and Mn show quite high activity in ammonia synthesis
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Role of catalyst promoters Role of catalyst promoters -- Poisons for ammonia synthesisPoisons for ammonia synthesis
The addition of Al and K promoters drastically increases the activity K acts as an electron donor that increases the electron density and thus
provides a higher number of active sites on the surface
Water, hydrogen sulfide and halogens are strong poisons as they adsorb strongly on the surface
H O causes site blocking but it is reversible
g Al influences the morphology of the catalyst, increasing its porosity and free
surface area
H2O causes site blocking but it is reversible 2S also blocks the surface by S* irreversibly. Large partial pressures
of H2S may cause the formation of FeS
Oxygen concentration should be kept low < 50 ppm as it is adsorbed strongly
Reduction of the catalystsReduction of the catalysts
Before use, the catalyst is reduced with H2 at 500C for up to 100h to be converted to the active structure to provide metallic Fe removal of oxygen makes the material porous specific surface area increases
The promoters are in still oxidic phase after the reduction The surface are of the reduced catalyst is around 290 m2/g
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General mechanism of ammonia synthesis
The reaction follows a Langmuir-Hinshelwood (LH) mechanism both reactants are dissociatively adsorbed on the surface before reaction
The dissociative adsorption of N2 is the rate determining step
Calculated reaction pathways for ammonia synthesis over
Ru catalyst
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Reactor designReactor designRequirements to reactors: Gas phase reactor with a solid catalyst Temperature control as the reaction is exothermic Two methods applied Two methods applied
Quench reactor in which cold gas is inserted at different heights of the reactor
Reactor with heat exchangers between the catalyst beds
The ICI The ICI quench reactorquench reactor
Part of the cold feed flows down on the outer shell ofthe reactor to cool it (feature used in most converters).
It is then heated in the effluent heat exchanger before entering the catalyst bed
One single catalyst bed containing of three zones separated by gas distributors.
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Kellogg vertical quench reactorKellogg vertical quench reactor
Feed enters at the bottom and cools theshell while flowing upwards
Four separated catalyst beds
Inlet of quench gas between the beds
Haldor TopsHaldor Topse radicale radical--flow reactorflow reactor
Main difference compared to other reactors:
di l fl th h t l t b dradial flow through catalyst bed reduces pressure drop allows smaller particles more catalytic area per unit volume
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Integrated ammonia plantIntegrated ammonia plant
Pressure to improve the economy is very highPressure to improve the economy is very high
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Ammonia synthesis loop
The yield of ammonia per pass ranges between 20 and 30% Unconverted synthesis gas leave the reactor together with
ammonia
Trends in catalysts for ammonia synthesisTrends in catalysts for ammonia synthesis
TEM image of the Ba-Ru/MgO catalyst after reduction at 783 K
Catalytic activity of a)the bari m promoted catal st (Ba R /MgO)a)the barium-promoted catalyst (Ba-Ru/MgO),b) the cesium-promoted catalyst (Cs-Ru/MgO),c) the industrial iron catalyst, d, e) unpromoted Ru/MgO catalysts (Ru/MgO), f) ammonia mole fractions at equilibrium
M. Muhler, O. Hinrichsen Angew. Chem. 2001