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introdaction ,backgruond about production of ethanol from co2
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1
CHAPTER.1
Introduction
1.1 background :
Ethanol, both a liquor and a fuel, has been around in the form of
Moonshine Whiskey since 15th Century Scotland. In 1908, Ford Motor
Company's first car, The Model T, used ethanol corn alcohol gasoline as
fuel energy. Since 2003, ethanol has grown rapidly as the oxygenating
factor for gasoline. Ethanol replaced MTBE for oxygenating fuel, since
almost all states now have banned MTBE, due to groundwater
contamination, health and environmental concerns. Ethanol blend fuels
for gas powered engines have been around for over 100 years, Ethanol is
now found at most public gas stations nationwide, due to mandates/laws
and recommendations in the Alternative Motor Fuels Act (1988), Clean
Air Act (1990), Energy Policy Act (2005) and most importantly - The
Renewable Fuel Standard Program (RFS) - Signed September 2006.The
push for ethanol as an alternative to imported oil spurred the construction
of 172 plants in 25 states by the end of 2008. But during 2009 falling oil
prices has made ethanol less cost effective. More than 20 plants have
recently closed. Despite 10% being the universally accepted legal limit
for ethanol in conventional gas-powered engines, in March 2009 ACE,
Growth Energy and 54 ethanol producers submitted a waiver application
2
1.2 History:
1826 Samuel Morey developed an engine that ran on ethanol and
turpentine.1850's During the Civil War, a liquor tax was placed on
ethanol whisky, also called Moonshine, to raise money for the war.
1876 Otto Cycle was the first combustion engine designed to use alcohol
and gasoline. 1896 Henry Ford built his first automobile, the quadricycle,
to run on pure ethanol.1920's Standard Oil began adding ethanol to
gasoline to increase octane and reduce engine knocking. 1908 The first
Ford Motor Company automobile, Henry Ford's Model T, was designed
to use corn alcohol, called ethanol. The Model T ran on (ethanol) alcohol,
fuel or a combination of the two fuels. 1940's First U.S. fuel ethanol plant
built. The U.S. Army built and operated an ethanol plant in Omaha,
Nebraska, to produce fuel for the army and to provide ethanol for
regional fuel blending. 1940's to late 1970's Virtually no commercial fuel
ethanol was sold to the general public in the U.S. - due to the low price of
gasoline fuel. 1975 U.S. begins to phase out lead in gasoline. MTBE
eventually replaced lead. Later, between 2004 to 2006, MTBE banned in
almost all states, due to groundwater contamination and health risks.
1980's Oxygenates added to gasoline included MTBE (Methyl Tertiary
Butyl Ether - made from natural gas and petroleum) and ETBE (Ethyl
Tertiary Butyl Ether -made from ethanol and petroleum).1988 Denver,
Colorado, was the first state to mandate ethanol oxygenates fuels for
winter use to control carbon monoxide emissions. Other cities soon
followed.1990 Clean Air Act Amendments - Mandated the winter use of
oxygenated fuels in 39 major carbon monoxide non-attainment areas
(based on EPA emissions standards for carbon dioxide not being met) and
required year-round use of oxygenates in 9 severe ozone non-attainment
areas in 1995. 1992 The Energy Policy Act of 1992 (EPAct) was passed
by Congress to reduce our nation's dependence on imported
3
petroleum by requiring certain fleets to acquire alternative fuel vehicles,
which are capable of operating on nonpetroleum fuels. The Clean Air Act
(1990) and Alternative Motor Fuels Act (1998 & 1992) contain
provisions for mandating oxygenated fuel (RFG =Ethanol and MTBE).
Requirements set for 2 types of clean-burning gasoline, RFG Federal
Reformulated Gasoline and Wintertime Oxygenated Fuel. 1995 The EPA
began requiring the use of reformulated gasoline year round in
metropolitan areas with the most smog.
1.3 Definition of ethanol:
Ethanol (ethyl alcohol, grain alcohol) is a clear, colorless liquid with a
characteristic, agreeable odor. In dilute aqueous solution, it has a
somewhat sweet flavor, but in more concentrated solutions it has a
burning taste. Ethanol, CH3CH2OH, is an alcohol, a group of chemical
compounds whose molecules contain a hydroxyl group, –OH, bonded to a
carbon atom. The word alcohol derives from Arabic al-kohl, which
denotes a fine powder of antimony used as an eye makeup. Alcohol
originally referred to any fine powder.
4
1.4 Objectives :
1- Reducing the carbon dioxide emissions to air.
2- Using carbon dioxide as raw material to production many
product.
3- Production ethanol from carbon dioxide.
5
CHAPTER.2
2.Lierature Review
2.1 Properties of carbon dioxide:-
2.1.1 Physical properties of carbon dioxide
Table 2.1 carbon dioxide physical properties
Property Value
Molecular weight 44.01
Specific gravity 1.53 at 21 oC
Critical density 468 kg/m3
Concentration in air 370.3 × 107 ppm
Stability High
Liquid Pressure < 415.8 kPa
Solid Temperature < -78 oC
Henry constant for solubility 298.15 mol/ kg.bar
Water solubility 0.9 vol/vol at 20 o
The critical point 7.38 MPa at 31.1 °C
the triple point 518 kPa at −56.6 °C
2.1.2 Chemical Properties:
2.1.2.1 Structure and Bonding:
The carbon dioxide molecule is linear and centrosymmetric. The
two C-O bonds are equivalent and are short (116.3 pm), consistent with
double bonding. Since it is centrosymmetric, the molecule has no
electrical dipole. Consistent with this fact, only two vibrational bands are
observed in the IR spectrum – an antisymmetic stretching mode at
2349 cm−1 and a bending mode near 666 cm−1. There is also a symmetric
6
stretching mode at 1388 cm−1 which is only observed in the Raman
spectrum.
Carbon dioxide is soluble in water, in which it reversibly converts
to H2CO3 (carbonic acid).The hydration equilibrium constant ofcarbonic
acidis (at 25 °C). Hence, the majority of the carbon dioxide is not
converted into carbonic acid, but remains as CO2 molecules not affecting
the pH.The relative concentrations of CO2, H2CO3, and the deprotonated
forms HCO−3 (bicarbonate) and CO32− (carbonate) depend on the pH
2.1.2.2 Chemical Reactions of CO2:
CO2 is a weak electrophile. Its reaction with basic water illustrates
this property, in which case hydroxide is the nucleophile. Other
nucleophiles react as well. For example, carnations as provided by
Grignard reagents and organ lithium compounds react with
CO2togivecarboxylates:
MR + CO2 → RCO2M (2.1)
(where M = Li or Mg Br and R = alkyl or aryl).
In metal carbon dioxide complexes, CO2 serves as a ligand, which can
facilitate the conversion of CO2 to other chemicals.
The reduction of CO2 to CO is ordinarily a difficult and slow reaction:
CO2 + 2 e− + 2H+ → CO + H2O (2.2)
2.2 Properties of ethanol :
2.2.1 Physical Properties :-
Ethyl alcohol under ordinary conditions is a volatile, flammable,
clear, colorless liquid. Its odor is pleasant, familiar, and characteristic. In
dilute aqueous solution, it has a somewhat sweet flavor, but in more
concentrated solutions it has a burning taste. It is completely mixable
with water with any concentration associated with heat and volume
reduction and also with organic solvents and is very hydroscopic. Ethanol
7
burns in air with a blue flame . Nearly all the ethanol used industrially is a
mixture of 95% ethanol and 5% water, which is known simply as 95%
alcohol. Although pure ethyl alcohol (known as absolute alcohol) is
available, it is much more expensive and is used only when definitely
required. Ethanol is very strong solvent come after water in solving
materials and can dissolve gases and many organic compounds which are
insoluble in water, most amazing property of ethanol is the volume
shrinkage that occurs when it is mixed with water, or the volume
expansion that occurs when it is mixed with gasoline. One volume of
ethanol plus one volume of water results in only 1. 92 volumes of
mixture. Ethanol is stable under ordinary conditions of use and storage.
Rapidly absorbs water from air. A summary of physical properties of
ethyl alcohol is presented in Table (2.2) Detailed information on the
vapor pressure, density, and others properties.
8
Table (2.2) Ethanol physical properties
Property Value
Molecular Weight 46.069
Critical Temperature 513.92 K
Critical Pressure 60.67605 atm
Melting point 159.05 K
Normal boiling point 351.44 K
Critical Volume 2.675083 ft3/lbmol
IG heat of formation -2.3495e+008 J/kmol
IG Gibbs of formation -1.6785e+008 J/kmol
Solubility parameter 26130 (J/m3
Density at 20 oC 689kg/m3
Heat of vaporization 3.874467e+007 J/kmol
Molecular diameter 4.31 angstroms
Specific gravity 60 F 0.7963032
Freezing point -114.1 Oc
2.2.3 Chemical Properties of Ethanol:-
2.2.3.1 Combustion of Ethanol
Ethanol burns with a pale blue, non luminous flame to form carbon
dioxide and steam.
C2H5OH + 3O2 ==> 2CO2 + 3H2O (2.3)
2.2.3.2 Oxidation of Ethanol:-
with acidified Potassium Dichromate, K2Cr2O7, or with acidified
Sodium Dichromate, Na2Cr2O7, or with acidified potassium
permanganate, KMnO4,
9
The ethanal is further oxidized to ethanoic acid (i.e. acetic acid) if the
oxidizing agent is in excess.
[O]
C2H5OH ==> CH3CHO + H2O (2.4)
The oxidizing agent usually used for this reaction is a mixture of sodium
dichromate or potassium dichromate and sulphuric acid which react
together to provide oxygen atoms as follows.
Na2Cr2O7 + 4 H2SO4 ==> Na2SO4 + Cr2(SO4)3 + 4H2O + 3[O] (2.5)
2.2.3.3 Dehydration of Ethanol:
When ethanol is mixed with concentrated sulphuric acid with the acid in
excess and heated to 170 deg C, ethylene is formed. (One mole of ethanol
loses one mole of water)
H2SO4
C2H5OH =======> C2H4 + H2O (2.6)
170 deg C
When ethanol is mixed with concentrated sulphuric acid with the alcohol
in excess and heated to 140 0C, diethyl ether distils over (two moles of
ethanol loses one mole of water) .
H2SO4
2C2H5OH ====> C2H5OC2H5 + H2O (2.7)
10
2.2.3.4 Reaction of Ethanol with Sodium:
Sodium reacts with ethanol at room temp to liberate hydrogen. The
hydrogen atom of the hydroxyl group is replaced by a sodium atom,
forming sodium ethoxide.
C2H5OH + Na ==> C2H5ONa + H2 (2.8)
Apart from this reaction, ethanol and the other alcohols show no acidic
properties.
2.2.3.5 Dehydrogenation of Ethanol:
Ethanol can also be oxidized to ethanal (i.e. acetaldehyde) by passing its
vapor over copper heated to 300 deg C. Two atoms of hydrogen are
eliminated from each molecule to form hydrogen gas and hence this
process is termed dehydrogenation.
C2H5OH ==> CH3CHO + H2 (2.9)
2.2.3.6 Esterification of Ethanol:
Ethanol, C2H5OH, reacts with organic acids to form esters.
H(+)
C2H5OH + CH3COOH ==> CH3COOC2H5 + H2O (2.10)
2.2.3.7 Halogenations or Substitution of Ethanol with PCl5:
Ethanol reacts with phosphorus pentachloride at room temperature to
form hydrogen chloride, ethyl chloride (i.e. chloroethane) and phosphoryl
chloride.
C2H5OH + PCl5 ==> C2H5Cl + POCl3 + HCl (2.11)
11
2.2.3.8 Halogenation or Substitution of Ethanol with HCl:
Ethanol reacts with hydrogen chloride to form ethyl chloride (i.e.
chloroethane) and water. A dehydrating agent (e.g. zinc chloride) is used
as a catalyst.
2.3 Uses of ethanol :
2.3.1 As a fuel:
Fuel ethanol is traditionally used as a gasoline extender or additive. As a
fuel extender it is often used as a blending ingredient at 5% to 10%
concentrations in gasoline creating a product called gasohol. As an
additive, ethanol increases the octane level of gasoline and adds oxygen
that lowers carbon monoxide emissions during the combustion process.
MTBE, a petrochemical currently used mostly in the US as an oxygenate
in gasoline, is being phased out of use in California and other US states
due to concerns of its effect on groundwater. Ethanol is foreseen as the
most logical replacement for MTBE. Ethanol has other current and future
motor fuel applications.
12
2.3.2 Personal care products & cleaning products:
Ethanol used in cosmetics, hair spray, mouthwash, after shave lotion,
cologne, perfume, deodorants, lotions, hand sanitizers, soaps and
shampoos.
2.3.3 Pharmaceuticals:
As a prime carrier, found in medicines such as cough treatments,
decongestants, iodine solution, and many others. As a solvent, used for
processing antibiotics, vaccines, tablets, pills, and vitamins.
2.3.4. Industrial uses:
in production of vinegar and yeast.
Chemical intermediate in chemical processing (in the manufacture
of ethanal, (i.e. acetaldehyde, and ethanoic acid).
Food products like extracts, flavorings, and glazes.
Energy source in some liquid animal feed products .
As the fluid in thermometers.
In preserving biological specimens.
2.4. Method Manufacturing of ethanol:
Industrial ethyl alcohol can be produced by many approaches. the more
two common are:
1. producing ethanol from ethylene gas.
2. producing by fermentation.
2.4 Greenhouse effect:
The greenhouse effect is a process by which thermal radiation from a
planetary surface is absorbed by atmospheric greenhouse gases, and is re-
radiated in all directions. Since part of this re-radiation is back towards
the surface and the lower atmosphere, it results in an elevation of the
average surface temperature above what it would be in the absence of the
13
gases. Solar radiation at the frequencies of visible light largely passes
through the atmosphere to warm the planetary surface, which then emits
this energy at the lower frequencies of infrared thermal radiation. Infrared
radiation is absorbed by greenhouse gases, which in turn re-radiate much
of the energy to the surface and lower atmosphere. The mechanism is
named after the effect of solar radiation passing through glass and
warming a greenhouse, but the way it retains heat is fundamentally
different as a greenhouse works by reducing airflow, isolating the warm
air inside the structure so that heat is not lost by convection. If an ideal
thermally conductive blackbody were the same distance from the Sun as
the Earth is, it would have a temperature of about 5.3 °C. However, since
the Earth reflects about 30% of the incoming sunlight, this idealized
planet's effective temperature (the temperature of a blackbody that would
emit the same amount of radiation) would be about −18 °C. The surface
temperature of this hypothetical planet is 33 °C below Earth's actual
surface temperature of approximately 14 °C. The mechanism that
produces this difference between the actual surface temperature and the
effective temperature is due to the atmosphere and is known as the
greenhouse effect. Earth’s natural greenhouse effect makes life as we
know it possible. However, human activities, primarily the burning of
fossil fuels and clearing of forests, have intensified the natural
greenhouse effect, causing global warming.
14
2.4.1 Mechanism:
The Earth receives energy from the Sun in the form UV, visible, and near
IR radiation, most of which passes through the atmosphere without being
absorbed. Of the total amount of energy available at the top of the
atmosphere (TOA), about 50% is absorbed at the Earth's surface. Because
it is warm, the surface radiates far IR thermal radiation that consists of
wavelengths that are predominantly much longer than the wavelengths
that were absorbed (the overlap between the incident solar spectrum and
the terrestrial thermal spectrum is small enough to be neglected for most
purposes). Most of this thermal radiation is absorbed by the atmosphere
and re-radiated both upwards and downwards; that radiated downwards is
absorbed by the Earth's surface. This trapping of long-wavelength
thermal radiation leads to a higher equilibrium temperature than if the
atmosphere were absent. This highly simplified picture of the basic
mechanism needs to be qualified in a number of ways, none of which
affect the fundamental process.
Figure (2.1)
The solar radiation spectrum for direct light at both the top of the
Earth's atmosphere and at sea level.
15
The incoming radiation from the Sun is mostly in the form of
visible light and nearby wavelengths, largely in the range 0.2–
4 μm, corresponding to the Sun's radiative temperature of 6,000 K.
Almost half the radiation is in the form of "visible" light, which our
eyes are adapted to use.
About 50% of the Sun's energy is absorbed at the Earth's surface
and the rest is reflected or absorbed by the atmosphere. The
reflection of light back into space largely by clouds does not much
affect the basic mechanism this light, effectively, is lost to the
system.
The absorbed energy warms the surface. Simple presentations of
the greenhouse effect, such as the idealized greenhouse model,
show this heat being lost as thermal radiation. The reality is more
complex: the atmosphere near the surface is largely opaque to
thermal radiation (with important exceptions for "window" bands),
and most heat loss from the surface is by sensible heat and latent
heat transport. radiative energy losses become increasingly
important higher in the atmosphere largely because of the
decreasing concentration of water vapor, an important greenhouse
gas. It is more realistic to think of the greenhouse effect as
applying to a "surface" in the mid-troposphere, which is effectively
coupled to the surface by a lapse rate.
The simple picture assumes a steady state. In the real world there is
the diurnal cycle as well as seasonal cycles and weather. Solar
heating only applies during daytime. During the night, the
atmosphere cools somewhat, but not greatly, because its emissivity
is low, and during the day the atmosphere warms. Diurnal
temperature changes decrease with height in the atmosphere.
16
Within the region where radiative effects are important the
description given by the idealized greenhouse model becomes
realistic: The surface of the Earth, warmed to a temperature around
255 K, radiates long-wavelength, infrared heat in the range 4–
100 μm. At these wavelengths, greenhouse gases that were largely
transparent to incoming solar radiation are more absorbent Each
layer of atmosphere with greenhouses gases absorbs some of the
heat being radiated upwards from lower layers. It re-radiates in all
directions, both upwards and downwards; in equilibrium (by
definition) the same amount as it has absorbed. This results in more
warmth below. Increasing the concentration of the gases increases
the amount of absorption and re-radiation, and thereby further
warms the layers and ultimately the surface below.
Greenhouse gases including most diatomic gases with two different
atoms (such as carbon monoxide, CO) and all gases with three or
more atoms are able to absorb and emit infrared radiation. Though
more than 99% of the dry atmosphere is IR transparent (because
the main constituents N2, O2, and Ar are not able to directly absorb
or emit infrared radiation), intermolecular collisions cause the
energy absorbed and emitted by the greenhouse gases to be shared
with the other, non-IR-active, gases.
2.4.2 Greenhouse gases :
Main article: Greenhouse gas
By their percentage contribution to the greenhouse effect on Earth the
four major gases are:
water vapor, 36–70%
carbon dioxide, 9–26%
17
methane, 4–9%
ozone, 3–7%
The major non-gas contributor to the Earth's greenhouse effect, clouds,
also absorb and emit infrared radiation and thus have an effect on
radiative properties of the atmosphere.
Role in climate change
Main article: Global warming
Figure (2.2)
The Keeling Curve of atmospheric CO2 concentrations measured at
Mauna Loa Observatory.
Strengthening of the greenhouse effect through human activities is known
as the enhanced (or anthropogenic) greenhouse effect.] This increase in
radiative forcing from human activity is attributable mainly to increased
atmospheric carbon dioxide levels According to the latest Assessment
Report from the Intergovernmental Panel on Climate Change, "most of
the observed increase in globally averaged temperatures since the mid-
20th century is very likely due to the observed increase in anthropogenic
greenhouse gas concentrations".CO2 is produced by fossil fuel burning
and other activities such as cement production and tropical deforestation.
Measurements of CO2 from the Mauna Loa observatory show that
concentrations have increased from about 313 ppm in 1960 to about 389
18
ppm in 2010. It reached the 400ppm milestone on May 9, 2013. The
current observed amount of CO2 exceeds the geological record maxima
(~300 ppm) from ice core data.[ The effect of combustion-produced
carbon dioxide on the global climate, a special case of the greenhouse
effect first described in 1896 by Svante Arrhenius, has also been called
the Callendar effect. Over the past 800,000 years, ice core data shows that
carbon dioxide has varied from values as low as 180 parts per million
(ppm) to the pre-industrial level of 270ppm. Paleoclimatologists consider
variations in carbon dioxide concentration to be a fundamental factor
influencing climate variations over this time scale.
2.5 Carbon Dioxide as a Raw Material:
There has been an increased attention for the use of carbon dioxide as a
raw material over the past two decades. There have been five
international conferences and numerous articles in the past twenty years
on carbon dioxide reactions that consider using ,it as a raw material
Increased utilization of carbon dioxide is desirable as it is an inexpensive
and nontoxic starting material. In view of the vastness of its supply,
carbon dioxide represents a possible potential source for feed stocks for
the manufacture of chemicals and fuels, alternative to the current
predominant use of petroleum-derived sources .
19
CHAPTER.3
3.1 Process description :
For potentially new processes for ethanol from carbon dioxide, Inui
(2002).reviewed five experimental processes for synthesis of ethyl
alcohol from the hydrogenation over a Cu-Zn-Fe-K catalyst .
hydrogenation of carbon dioxide with the same ratio of H2 to CO2 = 3:1,
5 MP a pressure and 513 K operating temperature, feed ration H2/CO2 =
3, flow-rate of 100cm3/min. in the first case Cu-Zn-Fe-K catalyst, 49 atm
pressure, 513-533 K temperature range, 21.2% conversion of CO2, 21.2%
selectivity to ethanol. In the second case Fe-Cu-Zn-Al-K catalyst, 20,000
h-1 space velocity, 80 atm pressure, 583 K, 28.5%conversion of CO2,
28.5% selectivity to ethanol. in third case (Fe-Cu-Zn-Al-K) catalyst
packed in series, 70,000 h-1 space velocity, 80 atm pressure, 623 K,
12.8% conversion of CO2, 12.8% selectivity to ethanol. In fourth case
(Fe-Cu-Al-K) (Cu-Zn-Al-K. Ga .Pd) catalysts physically mixed, 50,000
h-1 space velocity, 80 atm pressure, 603 K, 25.1% conversion of CO2,
25.1% selectivity to ethanol. then transmits a mixture of water and
ethanol for distillation tower to be of separating the ethanol from the
water in the first part in the distillation tower (1) , separate the mixture
ethanol and water then transmits for the second distillation tower to final
separating ethanol and water .
2CO2 + 6H2 → C2H5OH + 3H2O (3.1)
3.2 Reaction method
A pressurized continuous flow reactor was used. Usually, a 0.5 g portion
of a catalyst was packed into the stainless-steel reactor of 10 mm inner
diameter. Before the reaction test, the catalyst was heated in a hydrogen
flow composed of 10 vol.% H2 and 90 vol.% N2 at 450°C under
20
atmospheric pressure. The reactor was cooled down and the reduction gas
was replaced by the reaction gas composed of 25 mol% CO2–75 vol.%
H2. The reaction gas was allowed to flow under 80 atm, with a space
velocity (SV) ranging from 20,000 to 70,000 h−1 at a temperature
ranging from 270°C to 370°C. The products were analyzed by using three
sets of gas chromatographs equipped with integrators. Activated Carbon
column was used for the analysis of H2, N2, CO, CO2, and CH4, and
columns of PORAPACKQ and VZ-10 were used for the analyses of
hydrocarbon, alcohol and oxygenate produced. Pd- modified Cu-Zn-Al-K
mixed oxide combed with the Fe-based catalyst,330°C, 80atm, CO2/H2 =
1/3, SV = 20,000h-1, the space yield of ethanol = 476g/l·h (Yamamoto
and Inui,1998).
3.3 Ethanol from CO2 Hydrogenation over Cu-Zn-Fe-K catalyst:
The experimental study by Inui, 2002, for the production of ethanol by
CO2hydrogenation over a Cu-Zn-Fe-K catalyst .
flow sheet for this process is shown in Figure (3.1) . The conversion of
CO2 per single pass was 21.2% (Inui, 2002). The un reacted CO2 and H2
were recycled, as shown in Figure(3.1) Thus, a total conversion of CO2
was obtained. The following reaction occurs in this study.
2CO2 + 6H2 → C2H5OH + 3H2O ΔHº = -173 kJ/mol, ΔGº = -65 kJ/mol
(3.2)
The ethanol production capacity of the simulated plant was selected to be
104,700metric tons per year (11, 950 kg/hr). This production capacity
was based on Shepherd Oil, an ethanol plant located in Jennings, LA, and
the production capacity of this plant is36 million gallons of ethanol per
year (107,500 metric tons/year The ethanol produced in this process was
88% pure the energy required for this process was 276 x 106kJ/hr. The
21
HP steam required to supply this energy was 166 x 103 kg/hr, The energy
liberated from this process was 373 x 106 kJ/hr, and the cooling water
required to absorb this heat was 446 x 104 kg/hr.
Table (3.1)
The equipments of flow sheet in figure (3.1)
MX-100,101,102. Mixtures
EX-100,101,102,103,104,105,106. Heat exchanger
CRV-100,101,102,103. reactor
Prods-1,3,5,7. Ethanol +water
Prods-2,4,6,8. Water
T-100,101. Distillation tower
22
23
CHAPTER.4
4.Conclusionand recommendations
4.1Conclusion :
In this research unit is designed for the production of ethanol from carbon
dioxide by hydrogenation catalysts over Cu-Zn-Fe-K catalyst and the
topics addressed by the research:
Introduction and historical stages develop ethanol used as a fuel in
addition to the historical progress for fuel ethanol industry,
The use of carbon dioxide as a store of energy and raw material for the
production of many types of fuel. global warming and its impact on the
environment and the significant impact of carbon dioxide in this problems
.The physical properties of carbon dioxide and the physical properties and
chemical properties of ethanol .The use of ethanol in the various fields of
industrial, medical and other fields. Ethanol is safety, and a friend to the
environment. Outline shows the process of producing ethanol by
hydrogenation over catalysts. The description of the process as well as to
explain the scheme and the type of equipment and chemicals used to
clarify the reaction conditions at each stage.
24
4.2 Recommendations:
Given the importance of the subject, the controversy raised about
what it would be serious implications on the economic level and
the world: Opinion, it is our duty to put in front of our institutions
as follows:
Reduction of greenhouse gas emissions may possible to maintain a
clean environment free of contaminants.
absorption of gases carbon dioxide resulting from the factories,
processed and not released directly to air it because of the negative
effects on the environment.
The use of carbon dioxide as a raw material for the production of
different types of vehicles such as ethanol, methanol, formic acid
and other DME.
To encourage researchers to develop the area to take advantage of
harmful gases to the environment and their use in the production
of useful products.
The use of alternative energies instead of fossil energies fuel.
planting trees around industrial facilities to reduce carbon dioxide
emissions.
25
4.3 References :
CHEMICAL PRODUCTION COMPLEX OPTIMIZATION,
POLLUTION REDUCTION AND SUSTAINABLE
DEVELOPMENT by ( Aimin Xu B.S., Tianjin University, 1997
M.S., Tianjin University,1999 December, 2004).
DEVELOPMENT AND INTEGRATION OF NEW
PROCESSES CONSUMING CARBON DIOXIDE IN
MULTI-PLANT CHEMICAL PRODUCTION COMPLEXES
by (Sudheer Indala B.Tech., Andhra University, India, 2001 May,
2004 ).
WWW.Ethanolpruduction .com
(Louisiana Chemical &Petroleum Products List, 1998).