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).