PRODUCTION OF ETHYLENE GLYCOL

Manufacturing process Discrimination

The different processes followed for the production of ethylene glycol includes:

Ethylene carbonate process:

In this method, ethylene oxide is converted to an intermediate, ethylene carbonate, by reaction with carbon dioxide, which is then hydrolyzed by water to give ethylene glycol. This process was in use in the 1970s, but this process was replaced later by combined ethylene oxide-glycol plants.

Halcon Acetoxylatin Process:

Two reaction steps were used in the Oxirane plant. In the first, ethylene glycol diacatate is obtained by the oxidation of ethylene in an acetic acid solution, catalyzed by tellurium and a bromine compound. The reaction complex, which is quite complicated, proceeds via a tellurium-bromoethylene complex. The oxidation, which is carried out at 90-200 C and 20-30 atm pressure, results in a mixture of acetates due to partial hydrolysis of the diacetate. The reaction liquid effluent is withdrawn and processed to recover glycol acetates and glycol and provide the recycle streams back to oxidation. In the second step of the process, the glycol acetates are hydrolyzed to ethylene glycol and acetic acid.The process is obviously relatively more complex and will amount to huge capital cost and Literature also shows that it has operating difficulties. A plant started at Channelview in United State to produce 800 million lb/yr of ethylene glycol was shut down after difficulties in start up.

Esterification:

Ethylene glycol can be produced by reaction of formaldehyde with carbon monoxide. This route first produces glycolic acid which is converted by esterification and hydrogenolysis to ethylene glycol.

HCHO +CO + H20 HOCH2COOH

HOCH2COOH +ROH HOCH2COOR + H20

HOCH2COOR + 2H2 HOCH2CH2OH + ROH

Teijin Oxychlorination Process:

This process produces ethylene glycol by the reaction of ethylene with thallium salts in the presence of water and chloride or bromide ions. A redox metal compound (such as copper) oxidizable with molecular oxygen is added to the reaction medium to permit the regeneration of the thallium salt. The Teijin process is still in the works and yet to be commercialized.

Union Carbide Syngas Process:

The following process developed by Union Carbide, Inc. Uses synthesis gas for the production of ethylene glycol. Glycerol and propylene oxide are the major byproducts.Methanol, methyl formate and water are also produced as shown below.2CO + 3H2 HOCH2CH2OH An expensive rhodium based catalyst catalyzes the reaction. The process is yet to be commercialized. Union Carbide has already started work on a modified process in association with Ube Industries. It plans to set up a commercial scale plant soon.

Oxidation of Ethylene:

This process involves the oxidation of ethylene to ethylene glycol in an aqueous medium using an iron copper catalyst to produce Ethylene Glycol as represented in the reaction below. Fe-Cu CH2=CH2 + O2 + H20 HOCH2CH2OH

Hydrolysis of Ethylene Oxide:

The reaction chemistry is quite simple; it is either acid or thermally catalyzed. It is summarized as follows: ethylene oxide reacts with water to form ethylene glycol, and then further reacts with ethylene glycol and higher homologues in a series of consecutive reactions as shown in the following equations:

CH2CH2O + H2O HOCH2CH2O ethylene glycol

2CH2CH2O + H2O HOCH2CH2OCH2CH2OH diethylene glycol

3CH2CH2O + H2O HOCH2CH2OCH2CH2OCH2CH2O triethylene glycol

Production Process Description

In the process either a 0.5 to 1.0% sulphuric acid (H2SO4) catalyst is used at 50 to 70oC for 30 minutes or, in the absence of the acid, a temperature of 195oC and 185 psi for 1 hour will form the diol. The formation of higher glycols is inevitable because ethelene oxide reacts faster with ethylene glycols faster than with water. The most important variable is the water-to-oxide ration, and the production of diethylene glycol (DEG) and triethylene glycol (TEG) can be reduced by using a large excess of water. A 90 percent yield is realized when the ethylene oxide/water molar ratio is 1:5-8.The advantage of the acid-catalyzed reaction is no high pressure, however the thermal reaction needs no corrosion resistance and no acid separation step.The crude glycols are dehydrated and then recovered individually as highly pure overhead streams from a series of vacuum-operated purification columns. Ethylene glycol (boiling point: 197.6oC) is readily vacuum distilled and separated from the diethylene glycol (boiling point: 246oC, density: 1.118, flash point: 124oC) and triethylene glycol (boiling point: 288oC, density: 1.1274, flash point: 177oC).Since ethylene glycol is produced in relatively high purity, differences in quality are not expected. The directly synthesized product meets the high quality demands (polyester grade glycol).

Other Alternatives:

Other Possible catalyst for this reaction includes quaternary ammonium and phosphonium salts. A more recently developed catalyst system is based on use of Pd (II) complexes. A mixture of PdCl2, LiCl and NaNO3 in acetic acid and acetic anhydride has been shown to give a 95% selectivity During this process, Pd(II) is reduced to Pd(0). If PdCl2-CuCl2-CuOCOCH3 is used, reaction proceeds under mild conditions without formation of a precipitate. A yield of over 90% is obtained.

ETHYLENE GLYCOL PRODUCTION

The production of ethylene glycol by the hydrolysis of ethylene oxide has been selected in the following Design Thesis because it is by far the most widely used method for the production of ethylene glycol. It is relatively economical, simple reliable and can be used in plants that manufacture ethylene oxide and glycol together. For this Project design there is a modification to the common Flow sheet used for the Hydrolysis of Ethylene Oxide process that has been shown above. This modified unit arrangement will still achieve the production of Ethylene Glycol at a lower Capital cost. As stated above this reaction can be acid or based catalysed but for this work a choice of a neutral and high pressure and temperature reaction is made because it has the economic advantage of having no need for corrosion resistance and no acid separation step.The chemistry of the reaction is summarized as follows: ethylene oxide reacts with water to form ethylene glycol, and then further reacts with ethylene glycol and higher homologues in a series of consecutive reactions as shown in the following equations:

Step 1CH2CH2O + H2O HOCH2CH2O ethylene glycol

Step 22CH2CH2O + H2O HOCH2CH2OCH2CH2OH diethylene glycol

Step 33CH2CH2O + H2O HOCH2CH2OCH2CH2OCH2CH2O triethylene glycol

The aim of this work is the yield of Ethylene Glycol not those of higher glycol does this reaction is modified in such a way as to favour reaction step one and disfavour the other two steps and this is achieved by using excess of water for the reaction to dilute the concentration of the ethylene glycol produced to discourage the formation of higher glycols. Production Process Description

Ethylene Oxide and water a passed into a Continous Stirring Tank Reactor which operates a temperature of 195oC and pressure 185 psi for 1 hour will form the diol. Since the formation of higher glycols is inevitable because ethelene oxide reacts faster with ethylene glycols faster than with water then the water-to-oxide ration must be manipulated to reduce if not eliminate the production of diethylene glycol (DEG) and triethylene glycol (TEG). This is done by using a large excess of water. In this work, the ethylene oxide/water molar ratio is 1: 7 and the yield of Ethylene glycol is 90%. This Plant is designed to produced 10000kg/yr of Ethylene Glycol.

The crude Ethylene produced from the reactor is dehydrated and recovered as highly pure overhead stream from a distillation column with a partial condenser. The Distillate from the partial condenser is mainly water and is recycled back to the reactor and mixed with incoming water. The flow sheet for this sequence is shown below

PFig: Shows the Flow sheet for the Production of Ethylene Glycol Simulated on Aspen Hysis

MATERIAL BALANCE FOR THE REACTOR

Reaction Stoichiometry:CH2CH2O + H2O HOCH2CH2O ethylene glycol

Molecular weight of Species:CH2CH2O = (12x2+1x4+16) = 44kg/kmol

HOCH2CH2O = (12x2+1x6+16x2) =62kg/kmol

Material Balance for Ethylene Oxide:The target is 10,000kg/yr

10,000kg/yr of HOCH2CH2O = 10,000/62 = 1612.9kmol/yr = 5.33x10-5kmol/sec HOCH2CH2O

The Ethylene glycol/Water splitter column can only achieve a 99% separation for the ethylene glycol thus 5.33x10-5/0.99 = 5.38x10-5kmol/sec of ethylene glycol must be produced from the reactor to be feed into the column.

From Literature, the yield of Ethylene Glycol in the reactor is 90%Yield of 90% impliesMoles of ethylene oxide used up in the reaction/total moles of ethylene Oxide = 90/100

5.38x10-5kmol/moles of ethylene oxide = 0.9Therefore, moles of ethylene oxide = 5.38x10-5/0.9 = 5.97x10-5kmol of ethylene Oxide is used up during the reaction but 5.97x10-5/0.9 = 6.63x10-5kmol/sec of Ethylene is actually feed into the reactor

Mass of ethylene Oxide required per second = 44kg/kmol x 6.63x10-5kmol = 2.92x10-3kg

Unreacted Ethylene oxide = 6.63x10-5kmol/sec - 5.38x10-5kmol/moles = 6.6x10-6kmol/moles

Material balance for Water:From Literature,Since the feed ratio is 1: 7 therefore the moles of water feed = 7 x 6.63x10-5kmols = 4.64x10-4kmolsMass flow rate of water required = 18kg/kmols x 4.64x10-4kmol = 8.35x10-3kg/secTaking density of water = 1000kg/m3 The volume of water required per year = 8.35x10-3/1000 = 8.35x10-6m3/sec of water

Unconverted WaterThe reacting moles are same for water and ethylene oxide, therefore the amount of water reacting = amount in moles of ethylene oxide=5.97x10-5kmol.Therefore Amount of water left unconverted = Total Water fed Amount that took part in the reaction = 4.64x10-4kmol 5.97x10-5kmol = 4.04x10-4kmol=4.04x10-4kmol x 18kg/kmols = 7.27x10-3kg/sec of Water=7.27x10-3/1000 = 7.27x10-6m3/sec of Water

ENERGY BALANCE FOR THE REACTOR

Equation of the reaction

C2H4(g) + H20(g) = C2H6O2(l)

Standard Heat of formation data for this condition

Ethylene Oxide = -52.6kj/molWater = -241.8kj/molEthylene glycol = - 460kj/mol

Heat of reaction = Summation of the heat of formation for product summation of the heat of formation of the reactants

= (1 x -460) ((1 x -52.6) + (1 x -241.8)) = -165.6kj/mol

Therefore DHR (Heat of the reaction) = +165.6kj/mol

The reaction is exothermic so a cooler is incorporated take out the heat produced/mol as the reaction progresses.

Heat generated by the reaction (Q) = Heat taken by cooling water (Q)

Q = mCPDT of water

Heat generated by the reaction (Q) = 165.6 x 5.38x10-5 (moles of Ethylene oxide produced) = 8.91x10-3kj/s

WhereWhere 250c the Temperature of water availableDegree of approach is taken as 100cCP of water = 4.180kj/kgk

Thus8.91x10-3kj/s = mCPDT = m x 4.180 x (35-25) +273kWhere 250c the Temperature of water availableDegree of approach is taken as 100cCP of water = 4.180kj/kgk

m = 8.91x10-3 / 1162.04= 7.67 x 10-6 kg/sThus 7.67 x 10-6 kg/s of water must be feed into the cooler system around the reactor to maintain at operational temperature.MATERIAL BALANCE FOR THE DISTILLATION COLUNM

Ethylene Glycol has a boiling point of 197.60c while water has a boiling point of 1000c showing that water will boil over first leaving the Ethylene glycol in the bottoms.From Literature, Relative volatility of Ethylene glycol versus water = 15.1

Specification for the column

Feed rate=F=Amount of water unconverted + Unreacted Ethylene oxide + Ethylene glycolF=4.04x10-4kmol/s+6.6x10-6kmol/s+5.38x10-6kmol/s=4.64x10-4kmol/s

Which implies thatWater 0.87 molesEthylene Glycol 0.12 molesEthylene Oxide 0.01 moles

Bottoms (B)Specification99% Ethylene Glycol with flow rate of 5.38x10-5x0.99 = 5.33x10-5kmol/s1% water with flow rate of 4.04x10-4x0.01 = 4.04x10-6kmol/s

ThereforeBottoms (B) = 5.33x10-5kmol/s + 4.04x10-6kmol/s = 5.734x10-5kmol/s

Distillate (D)Specification100% WaterDistillate (D) = F B = 4.64x10-4kmol/s - 5.734x10-5kmol/s = 4.07x10-4kmol/s

L+D=T Where L=Flow of Condensate returned to the columnD=Flow of condensate taken out as DistillateT=Flow of vapour leaving the first stage of the column

Reflux Ration = L/D

At 2.5reflux, L/D=2.5L=2.5D = 2.5x4.07x10-4kmol/s = 1.02x10-3kmol/s

T=2.5D+D=3.5D=1.4x10-3kmol/s

At total Reflux; the theoretical number of trays can be calculated with relative volatility of Ethylene glycol versus water = 15.1

Using Fenskes Equation

Nm+1 = log (XD/1-XD 1-XB/XB)/log

=log(0.98/0.12 x 0.99/0.01)/log15.1Nm= (2.908/1.178) 1 = 2.46 1 =1.46

Using Gillilands rule of thumb, the actual number of tray = 2.5xNm = 2.5x1.46 =3.65traysCorrecting for Tray Efficiencies assuming the efficiency to be 60% = 3.65/0.60 = 6.108= 7 trays

SIMULATION OF THE DISTILLATION COLUNMThe column was simulated using ASPEN HYSIS with the main aim of obtaining the energy balance of the system and the reboiler and condenser duties. The above calculated value for the Feed rate and mole composition of the species, reflux ratio, Distillate flow rate, and number of trays were inputed into the software. Peng Robinson was used as the fluid package and the specification of the composition of ethylene glycol in the bottoms was specified as 0.99. It was noted that the HYSIS Estimate of the other Distillate flow, Bottoms flow etc were very close to the manual calculations made for them. The result of the simulation is shown below along with the condenser and heater duties.

ETHYLENE GLYCOL/WATER SPLITTER FLOW SHEET

SPECIFICATION FOR THE REACTOR EFFLUENT (COLUMN INPUT)

DISTILLATE ESTIMATE

BOTTOMS ESTIMATE