produccion de acido acetico a partir de la oxidacion de etileno
TRANSCRIPT
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Catalysis Surveys from Japan 3 (1999) 5560 55
A new process for acetic acid production by direct oxidation ofethylene
Ken-ichi Sano a, Hiroshi Uchida b and Syoichirou Wakabayashi b
a Catalysis Section, Central Research Laboratory, Showa Denko K.K., 5-1 Ogimachi, Kawasaki, Kanagawa 210-0867, Japanb Technology and Development Department, Oita Works, Showa Denko K.K., 2 Nakanosu, Oita 870-0189, Japan
A new process for acetic acid production by direct oxidation of ethylene which was established and commercialized is described.
The catalyst system consisting of Pd and heteropoly acid exhibits excellent activity and selectivity. The addition of Se or Te to the
catalyst system is effective to suppress the formation of carbon dioxide. This new process is applicable to a plant of a wide range of
size corresponding to the local demand. Because this new process produces little waste water, it is very friendly to the environment.
Keywords: acetic acid, oxidation, Pd, heteropoly acid, ethylene
1. Background [1]
1.1. A short history of acetic acid manufacturing
technologies
Among the organic compounds, acetic acid has been
very familiar to mankind since it has been used as vinegar
for a long time. Vinegar was produced by alcohol fermen-
tation before Christ, and even now this brewing method is
used for vinegar production.As the demand for acetic acid grew in a wide range
of fields, pyroligneous acid, which is produced by the dry
distillation of wood, and used by alchemists in medieval
Europe, became a world-wide manufacturing process un-
til the middle of the 20th century. This pyroligneous acid
method was replaced by synthetic processes and is scarcely
used now. In 1914, the acetaldehyde oxidation process was
industrialized in Germany. Acetaldehyde was synthesized
by hydration of acetylene produced from carbide at that
time. The epoch-making process, the so-called Hoechst-
Wacker process which uses ethylene as the raw material,
was developed in 1959. The conventional process for thepreparation of acetaldehyde from acetylene was mostly re-
placed by this process. At the same period, the technology
of hydrocarbon oxidation made progress. Then oxidation
ofn-butane in liquid phase to produce acetic acid was in-dustrialized in 1952, and liquid phase oxidation of naphtha
to produce acetic acid was commercialized in 1956.
In the mean time, the manufacturing process of acetic
acid by the carbonylation of methanol was developed. This
process uses methanol and carbon monoxide as raw ma-
terials which are produced from natural gas, coal, heavy
residual oil, and others. BASF (Germany) industrialized
this process in 1960, and Monsanto (USA) industrialized itin 1970. Especially the latter process, known as Monsanto
process, has become the dominant industrial route for acetic
acid manufacturing.
1.2. Uses of acetic acid
Acetic acid has the demand of about 5.4 million
tons/year in the world in 1997. It is used in vinyl acetate,
solvent for production of pure terephthalic acid (PTA),
acetic anhydride, acetates, and others, as shown in ta-
ble 1 [2].
2. Industrial manufacturing process [1]
2.1. Methanol carbonylation process
This process, which is called Monsanto process, uses
methanol and carbon monoxide as the raw materials to syn-
thesize acetic acid. Because the price of naphtha has risen
and the relatively cheap methanol, produced from off gas,
natural gas, and so on, has been available after the oil cri-
sis, this process has rapidly become prevalent. At present,
this process accounts for 60% of the production capacity of
the world.
CH3OH+ CO
CH3COOH (1)In the Monsanto process, the selectivities to acetic acid
based on methanol and carbon monoxide are 99% and 90%,
respectively, when rhodium is used as a catalyst and iodine
as an activator. These days, most of the methanol carbony-
lation processes have adopted this catalyst system.
Table 1
Demand for acetic acid by applications (1,000 t/y).
1995 1997
Vinyl acetate monomer 1,812 1,996
Acetic anhydride 713 743
PTA 727 955
Acetates 636 661
Others 1,036 1,030
Total 4,924 5,385
Baltzer Science Publishers BV
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56 K.-i. Sano et al. / Acetic acid production by direct oxidation of ethylene
Figure 1. Process flowsheet of Monsantos acetic acid process.
The flowsheet is shown in figure 1 [3]. Methanol and
carbon monoxide are supplied continuously into the reac-
tor. The exhaust gas from the reaction section, together
with exhaust gas from the purification section, are washed
in the scrubber, then the light-ends are recovered and recy-
cled to the reaction section. On the other hand, the reaction
product (crude acetic acid) is sent to the light-ends column,
and acetic acid is taken out as a side-cut. The overhead and
the bottoms including the catalyst are returned to the reac-
tion section. Side-cut acetic acid is sent to the dehydration
column, then the mixture of water and acetic acid is taken
out from the top, and returned to the reaction section. Thebottoms of the dehydration column are sent to the subse-
quent product column. A small amount of the heavy-ends,
which contain propionic acid, is taken out from its bottom.
The overhead is further purified in the next fractionation
column, and purified acetic acid is obtained as a side-cut.
The overhead and the bottoms of the fractionation column
are recycled into the reaction section.
2.2. Acetaldehyde oxidation process
First, ethylene is oxidized into acetaldehyde with a
PdCl2CuCl2 catalyst, which is subsequently oxidized toacetic acid with a manganese acetate catalyst. This process
was prevalent before the appearance of the methanol car-
bonylation process. At present, however, the share of this
process has fallen to 22% of the world production.
C2H4 + (1/2)O2 CH3CHO (2)
CH3CHO+ (1/2)O2 CH3COOH (3)
The flowsheet of this process is shown in figures 2 and
3 [4]. Acetaldehyde vapor produced in the reactor leaves
the gas-liquid separator together with water vapor and un-
reacted gases. After cooling, acetaldehyde is absorbed with
water and the remaining gas is recycled to the reactor. Thelight-ends are removed at the light-ends column. Next, by-
products, such as methyl acetate and crotonaldehyde, are
removed as a side-cut from the product column. Further-
more, by-product acetic acid, together with water, is re-
moved from the bottom, and acetaldehyde is obtained from
the top.
In the oxidation process to acetic acid, acetaldehyde is
supplied near the top of the reactor and oxidized with the
rising oxygen gas introduced from the bottom. The liq-
uid reaction product, which is taken out from the reactor,
contains by-products, such as formic acid, methyl acetate,
ethylidene diacetate and others as well as a small amount
of unreacted acetaldehyde, water, and catalyst. Thus, the
light-ends are removed and the catalyst is recovered in the
purification section. The heavy-ends are removed from thebottom of the fractionation column, then purified acetic acid
is obtained. Acetic acid contained in the bottoms of the
fractionation column is recovered at the recovery column,
and the heavy-ends are removed. The recovered catalyst is
recycled.
2.3. Hydrocarbon (butane, naphtha) oxidation process
Hydrocarbons, such as butane and naphtha, are oxidized
directly into acetic acid, and 9% of the worlds production
capacity owes this process. Acetate catalysts, for exam-
ple, cobalt acetate and manganese acetate, are used. Since
this method uses hydrocarbons with high numbers of car-
bon atom as raw materials, not only acetic acid but acetone,
formic acid, propionic acid, and others are coproduced. Ac-
cordingly, the yield of acetic acid is much lower than those
of the other processes, but this process has advantages when
manufacturing various acids simultaneously is desired.
3. Direct oxidation of ethylene. A new Showa Denko
K.K. process
Showa Denko K.K. has developed a one-stage process
of acetic acid production by direct oxidation of ethylene.In this process, acetic acid is manufactured with high
selectivity from a mixture of ethylene and oxygen in the
vapor-phase at 160210 C over a solid catalyst. The main
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K.-i. Sano et al. / Acetic acid production by direct oxidation of ethylene 57
Figure 2. Process flowsheet of ethylene oxidation to acetaldehyde.
Figure 3. Process flowsheet of acetaldehyde oxidation to acetic acid.
reaction for acetic acid is shown below, together with the
major side-reactions, which are the combustion of ethylene
and the production of acetaldehyde.
In addition, small amounts of several compounds with
low and high boiling points are formed.
A great amount of heat is generated in this reaction, and
it is recovered as steam which is used for the heat source
in the purification section.
(Main reaction) C2H4 + O2 CH3COOH (4)
(Side reactions) C2H4 + 3O2 2CO2 + 2H2O (5)
C2H4 + (1/2)O2 CH3CHO (2)
The flowsheet of this process is shown in figure 4. The
product gas from the reactor is cooled to ambient temper-
ature. Thereby the reaction products such as acetic acid,
organic by-products, and water are condensed and are sep-
arated from un-condensed gas. The condensate is pulled
out of the reaction section and led to the crude acetic acid
tank which is connected to the purification section. The
un-condensed gas is recycled to the reactor after it is pres-
surized by the compressor.
The crude acetic acid stored in the crude acetic acid
tank is sent to the light-ends column. In this column, thelight-end by-products, such as acetaldehyde, ethyl acetate,
ethanol, and others, are removed from acetic acid by dis-
tillation. Then water is separated by extraction.
The acetic acid, free from water and the light-ends,
is sent to the final purification section. In this section,
both trace amounts of impurities and the heavy-ends are
removed, and highly pure acetic acid is obtained as the
product.
The chemical processes are required to be both compet-
itive and environmentally friendly: Showa Denko K.K.s
new process meets these requirements. Usually the pu-
rification of acetic acid is very energy consuming, since a
great amount of water is used in the oxidation reaction. To
solve this problem, Showa Denko K.K. has developed an
energy saving process by combining the extraction and the
distillation operation in which water is efficiently separated
from acetic acid [57]. This process is also very friendly
to the environment, because it generates little waste ow-
ing to the high selectivity of the reaction. No toxic waste,
and only a small volume of waste water were produced.
Moreover, it has a great advantage since no special mate-
rial is required for the construction of plants; adequately
used stainless steel is good enough for the facilities, be-
cause the process does not treat any corrosive compounds
except for acetic acid.
Showa Denko K.K. constructed the first commercial
plant based on the new process. It has the capacity of100,000 tons/year of acetic acid in Oita, Japan. The plant
was completed in August 1997. After the trial run, the plant
has been operated successfully since November 1997 [15].
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58 K.-i. Sano et al. / Acetic acid production by direct oxidation of ethylene
Figure 4. Process flowsheet of direct oxidation to ethylene into acetic acid.
Table 2
Proposed catalysts for direct oxidation of ethylene.
Catalyst Temperature Pressure Selectivity STY Ref.
(C) (kg/cm2G) (%) (g/lh)
PdCr/Al2 O3 180 1 60 [5]
PdV2O5 248 1 74 2 [6]
PdV2O5Sb2O5/Al2O3 250 1 84 27 [7]
PdH3PO4/SiO2 150 1 90 56 [8]
PdAuH2SO4/active carbon 150 3.4 85 107 [9]
4. Catalyst development for the direct oxidation
process
Several catalyst systems were proposed in the past for
the direct oxidation of ethylene to acetic acid, as shown
in table 2, for example. However, these catalysts havenot exhibited satisfactory performance for the industrial-
scale production of acetic acid. Here it is noteworthy that
acetic acid is obtained with relatively high selectivity by
the combination of Pd metal and acid catalysts.
4.1. Reaction mechanism
The following two reaction schemes may be considered
for the direct oxidation of ethylene to acetic acid. One
is the route where ethanol is formed by the hydration of
ethylene and then it is oxidized to acetic acid. In this
route, if the ethanol formed is irreversibly oxidized intoacetic acid, these reactions can to proceed under relatively
moderate conditions. It is considered that with catalysts
PdH3PO4/SiO2 and PdAuH2SO4/active carbon shown
in table 2, the reaction mainly proceeds by this mecha-
nism.
C2H4 +H2O CH3CH2OH (6)
CH3CH2OH+O2 CH3COOH+ H2O (7)
The other is the route where ethylene is first converted
into acetaldehyde by the Wacker type reaction, and the ac-
etaldehyde is oxidized into acetic acid. It is considered thatPd2+ basically acts as active species, and consequently the
reoxidation of Pd is necessary to achieve the catalytic reac-
tion. The catalyst systems, for example, PdCr/Al2O3, Pd
Table 3
Combination of Pd and heteropoly acid.a
Catalyst STYb Selectivity (%)
HOAcc
HAcd
CO2
PdH4SiW12O40 93.1 78.5 5.5 14.2
PdH3PW12O40 83.3 78.0 5.0 16.0
PdH4SiMo6W6O40 91.2 77.6 4.4 17.5
PdH3PMo6W6O40 75.1 76.5 4.1 19.2
PdH3PMo12O40 68.5 77.5 4.6 17.8
PdGa0.05H3.85SiW12O40 90.4 80.1 4.1 15.6
PdMg0.05H3.9SiW12O40 90.8 79.7 5.5 14.6
PdGa0.05H2.85PW12O40 75.6 74.8 3.2 21.8
PdLi0.05H3.95SiW12O40 91.0 79.9 3.9 16.1
PdCu0.05H3.9SiW12O40 90.9 78.6 4.9 16.4
Pd 0 0 0 100
H3PW12O40 0 0 0 0
PdH5PMo10V2O40 94.0 61.4 19.4 17.6
a Reaction conditions: reaction pressure = 5 kg/cm2G; reaction
temperature = 150 C; GHSV = 3,000/h; gas component (C2H4/O2/
H2O/inert gas = 50/7/30/13).b STY = space time yield (g/l-catalysth).c HOAc = acetic acid.d HAc = acetaldehyde.
V2O5, or PdV2O5Sb2O5/Al2O3 shown in table 2, mainly
follow this mechanism.
C2H4 + (1/2)O2 CH3CHO (2)
CH3CHO+ (1/2)O2 CH3COOH (3)
In spite of extensive efforts based on the second route,
any industrially promising results have not been obtained.
On the other hand, the first route, via ethanol intermedi-
ate, has at least a high selectivity. Showa Denko K.K.,
therefore, has chosen the R&D strategy based on the first
reaction mechanism, and has made efforts for the improve-
ment of catalyst performance.
4.2. Catalyst systems consisting of Pd and heteropoly
acids
We found that even a simple combination of Pd and a
heteropoly acid shows a relatively high yield of acetic acid,
as shown in table 3 [13].When only Pd was supported on silica, no partial oxida-
tion products of ethylene were obtained, and only carbon
dioxide, a deep oxidation product, was generated. On the
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60 K.-i. Sano et al. / Acetic acid production by direct oxidation of ethylene
of carbon monoxide production is also necessary. Conse-
quently the process requires heavy investments in facility
and is hardly profitable unless the production capacity is
equal to or more than 200,000 tons/year. On the other hand,Showa Denko K.K.s new process becomes profitable even
in the case of middle-scale facilities such as about 100,000
tons/year, and the investment can be substantially reduced
as compared with the methanol carbonylation process of
the same capacity. Since the new process is applicable to
a plant of a widely variable size, corresponding to the lo-
cal demand, the plant can be placed near the market. The
variable cost of acetic acid production depends mainly on
the price of methanol or ethylene in each case.
5.2. Comparison with acetaldehyde oxidation process
In the acetaldehyde oxidation process, the reaction is
two-staged, and many kinds of by-products complicate the
purification process. The acetaldehyde production needs
rubber and bricks for the materials of the reactor, because
aqueous hydrochloric acid is used. For these reasons, the
facility cost of the acetaldehyde oxidation process becomes
high. With the new process, the facility cost can be reduced
to 6070% for the same production capacity. Moreover, a
great amount of water is required for the acetaldehyde pro-
duction. This means that a large-scale facility becomes
necessary to treat the waste water. On the other hand, the
waste water from the new process is about 1/15 of that
from the acetaldehyde oxidation process. The new process
is in this respect much more friendly to the environment.
Although the selectivity of each step is high in the acetalde-hyde oxidation process, the overall selectivity of two-stage
oxidation is inferior to that of the new process. As a re-
sult, the unit consumption of ethylene of this new process
is better than that of the acetaldehyde oxidation process.
References
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