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Polymers and oligomers
Synthetically useful small molecules
Ethylene oxide 21 million tons/year
Vinyl chloride 13 million tons/year Styrene
5 million tons/year
Ethylene Applications
(a) Levdikova, T. PR Web. http://www.prweb.com/releases/2014/02/prweb11543300.htm (accessed 4/3/14). (b) James, S. PR Web. http://www.prweb.com/releases/Acetic-Acid-Market/GrandViewResearch/prweb11623679.htm (accessed 4/3/14).
1
Polymers: n
LDPE: (low density)
HDPE: (high density) Plastic wrap, laminate coatings,
plastic bags, snap-on lids
3,100 tons/year 5,700 tons/year Bottle caps, chemical resistant pipes, milk jugs, garbage cans, toys
Poly(ethylene) - PE
Oligomers:
Waxes α-olefins
C12-C18 olefins mostly for detergents 1.9 million tons/year
40-50% Mol %
C number C12 C18
(a) Chem. Eng. News. 2002, (June 24) p. 42; (b) Keim, W. Angew. Chem. Int. Ed. 2013, 52, 12492-12496; (c) Mol, J.C. J. Molec. Catal. A, 2004, 213, 39-45
Figure 1. Schulz-Flory distribution of olefin products from Shell Higher Olefin Process
2
23.3 million tons/year 143 million tons/year
enzymatic metabolism
15-35 °C
chemical catalysis
300-1000 °C
Man versus Nature
(a) Sawada, S., Totsuka, T. Atmos. Environ. 1986, 20, 821-832 (b) True, W. Oil and Gas J. [Online] 2013, 111, 1-6 . Available from OGJ Archives. http://www.ogj.com/articles/print/volume-111/issue-7.html (accessed March 4, 2014).
3
Thermal Cracking of Hydrocarbons
750-1000 °C
ΔH298K = 33 kcal/mol
Oxidative Dehydrogenation of Ethane
ΔH298K = - 25 kcal/mol
400-600 °C
Dehydration of Ethanol
Methanol to Olefins
Oxidative Coupling of Methane
300-400 °C
ΔH298K = 11 kcal/mol
(a) van Goethem, M.W.M., Barendregt, S., Grievink, J., Moulijn J.A., Verheijen, P.J.T. Ind. Eng. Chem. Res. 2007, 46, 4045-4062 (b) Gartner, C.A., van Veen, A.C., Lercher, J.A. ChemCatChem, 2013, 5, 3196-3217; (c) Zavyalova, U., Holena, M., Schlogl, R., Baerns, M. ChemCatChem, 2011, 3, 1935-1947
300-500 °C
ΔH298K = 15 kcal/mol
650-900 °C
ΔH298K = - 30 kcal/mol
Mankind’s Syntheses 4
Nature’s Synthesis: Plants
L-methionine
S-adenosylmethionine SAM
1-aminocyclopropanecarboxylic acid ACC
5
Nature’s Synthesis: Microbes
2-ketoglutarate pathway: Plant pathogens
2-ketoglutarate oxygenase
EC: 1.13.12.19
Successive fermentation and elimination: Man and nature
6
U.S. Energy Information Administration, www.eia.gov (accessed Mar. 24)
Readily Available Hydrocarbons
Figure 2. Common fossil fuel sources and wells required to extract gas or oil
Component Range (wt %)
Methane 87-97
Ethane 1.5-7
Propane 0.1-1.5
Butane 0.01-0.03
C5-C10 0.02
Table 1. Average composition of North American fossil fuel gases
Component Range (wt %)
Paraffins 15-60
Naphthenes 30-60
Aromatics 3-30
Table 2. Fractions of crude oil
7
C1-C4
CO2
H2S
H2O
70-100 bar
2-3 bar
sweetened gas
(a) Huttenhuis P.J.G.; Agrawal, N.J.; Hogendoorn, J.A.; Versteeg, G.F. J. Pet. Sci. Tech. 2007, 55, 122-134. (b) Banat, F.; Younas, O.; Didarul, I. J. Nat. Gas Sci. Eng. 2014, 16, 1-7.
Sweetening Natural Gas 8
(a) Petzny, W.J. WO2013150467, 2013. (b) Industrial Organic Chemicals, 3rd ed., Wittcoff, Reuben, Plotkin (Wiley, Hoboken, 2013). (c) Petrochemical Processes, 1. Synthesis-Gas Derivatives and Major Hydrocarbons, Chauvel, Lefebvre (Editions Technip, Paris, 1989)
Fraction Boiling Point Range °C Gases < 32
Light naphtha 32-88 Heavy naphtha 88-193
Kerosene 193-271 Atmospheric gas oil 271-343
Atmospheric residuum 343+ Vacuum gas oil 343-538
Vacuum residuum 538+
Crude Oil Distillation
Table 3. Distillation fractions of crude oil and average boiling point ranges
9
Fig. 4
Figure 3. Equilibrium conversion for dehydrogenation of ethane, propane, and butane at 1 bar
(a) The Properties of Gases and Liquids, 4th ed., Ried, Prausnitz, Poling (McGraw-Hill, New York, 1988). (b) Noureddine, H.; Nahla, F.; Zouhour, K.; Marie-Noelle, P. Energy Convers. Manag. 2013, 70, 174-186
ΔH298K = 33 kcal/mol
Δ
Process Conditions
750-1000 °C
0.01-0.5 s
ΔH298K = 18 kcal/mol
10
(a) Pyl, S.P.; Scietekat, C.M.; Reyniers, M-.F.; Abhari, R.; Marin, G.B.; Van Geem, K.M. Chem. Eng. J. 2011, 176-177, 178-187. (b) Sohn, S.W.; Rice, L.H.; Kulprathipanja, S. (UOP LLC, USA). Ethylene production by steam cracking of normal paraffins. US Patent 20110245556, October 6, 2011. (c) Schrod, H.M. (Saudi Basic Industries Co., SA). Process for production of hydrocarbon chemicals from crude oil. WIPO Patent 2013150467, October 10, 2013
Hydrocarbon Cracking Pilot Plant
Figure 4. Schematic overview of pilot plant setup
Product yield (wt%)
δ = 30% δ = 45% δ = 70%
Methane 16.58 16.28 16.38 Ethylene 29.86 30.85 32.54 Ethane 4.68 4.16 3.69
Propene 17.73 17.59 17.57 Propane 4.68 4.16 3.69 Benzene 5.66 5.68 5.64 Toluene 2.32 2.23 2.34 Styrene 0.70 0.59 0.62
Table 4. Influence of steam dilution (δ) on product distribution from pure ethane feed.
11
ΔH298K = 90 kcal/mol
ΔH298K = 36 kcal/mol
ΔH298K = - 3 kcal/mol
ΔH298K = - 24 kcal/mol ΔH298K = - 104 kcal/mol
ΔH298K = - 69 kcal/mol
Initiation:
ΔH298K = 101 kcal/mol Propagation:
Termination:
(a) van Goethem, M.W.M.; Barendregt, S.; Grievink, J.; Verheijen, P.J.T.; Dente, M.; Ranzi, E. Chem. Eng.Res. Des. 2013, 91, 1106-1110. (b) Ranjan, P.; Kannan, P.; Al-Shoaibi, A.; Srinivasakannan, C. Chem. Eng. Tech. 2011, 6, 1093-1097.
Thermal Cracking Ethane 12
(a) Dijkmans, T.; Pyl, S.P.; Reyniers, M-.F.; Abhari, R.; Van Geem, K.M.; Marin, G.B. Green Chem. 2013, 15, 3064-3076. (b) Pyl, S.P.; Dijkmans, T.; Antonykutty, J.M.; Reyniers, M-.F.; Harlin, A.; Van Geem, K.M.; Marin, G.B. Bioresour. Technol. 2012, 126, 48-55.
Thermal Cracking Higher Hydrocarbons
Dehydrogenation
Primary Cracking
Secondary Cracking
13
Oxidative Dehydrogenation of Ethane
(a) Kustov, L.M.; Kucherov, A.V.; Finashina, E.D.; Simanzhenkov, V.; Krzywicki, A. (Nova Chemicals, Intl.) Membrane-supported catalysts and the process of oxidative dehydrogenation of ethane using the same. US Patent 20130072737, March 21, 2013. (b) Achieva, D.; Brzic, D.; Peglow, M.; Heinrich, S.; Morl, L. Chemie. Ingenieur. Technik. 2004, 76, 1295-1296.
750-1000 °C
ΔH298K = 33 kcal/mol
ΔH298K = - 25 kcal/mol
400-600 °C
Figure 5. Dependence of ethylene yield on C2H6:O2 ratio over Al2O3 supported VO4. Temperature of reaction is 590 °C.
C2H6 : O2
Eth
ylen
e Yi
eld
[%]
ΔH298K = - 247 kcal/mol
Δ
14
Mars and Van Krevelen Mechanism: VOx example
(a) Zhu, H.; Ould-Chikh, S.; Anjum, D.H.; Sun, M.; Biausque, G.; Basset, J-.M.; Caps, V. J. Catal. 2012, 285, 292-303. (b) Agouram, S.; Dejoz, A.; Ivars, F.; Vazquez, I.; Lopez Nieto, J.M.; Solsona, B. Fuel Process. Technol. 2014, 119, 105-113. (c) Chen, K.; Bell, A.T.; Iglesia, E. J. Catal. 2002, 209, 35-42.
O2
15
Ethylene from Bioethanol
Braskem’s Triunfo plant – San Paulo, Brazil
Figure 6. Microbial fermentation of glucose to produce ethanol
Braskem Ethanol to Ethylene Plant, Brazil. http://www.chemicals-technology.com/projects/braskem-ethanol/ (accessed 4/12/14).
16
Dehydration of Ethanol Easily Occurs Over Heterogeneous Catalysts
Al2O3
400-450 °C Conversion: 80%
(a) Chen, Y.; Wu, Y.; Tao, L.; Dai, B.; Yang, M.; Chen, Z.; Zhu, X. J. Ind. Eng. Chem. 2010, 16, 717-722. (b) Solvay, Bruxelles, Process for the manufacture of ethylene by dehydration of ethanol. European Patent 2594546, November 17, 2011.
HZSM-5
300 °C Conversion: 98%
Si/AlPO4
320 °C Conversion: 90%
• Water deactivates active sites
• Dry ethanol not needed
• No coking on milder acid sites
• Coking deactivates catalyst
17
Ethylene from Bioethanol is Commercially Utilized
Terephthalic acid
Polyethylene terephthalate
PlantBottleTM Technology. http://www.coca-colacompany.com/plantbottle-technology/ (Accessed 4/15/14)
Ag0
O2
18
H3O+
(a) Christiansen, M.A.; Mpourmpakis, G., Vlachos, D.G. ACS Catal. 2013, 3, 1965-1975. (b) Solvay, Bruxelles, Process for the manufacture of ethylene by dehydration of ethanol. European Patent 2594546, November 17, 2011. (c) Knoezinger, H., Koehne, R. J. Catal. 1966, 5, 264-270.
Pathway B
Pathway A Pathway A
Temperature Dependence of Dehydration Pathway
T > 300 °C favors path B T < 300 °C favors path A Figure 7. Dependence of ethanol decomposition
on catalyst temperature.
Partia
l Pre
ssur
e (To
rr)
Temperature (° C)
Alcohol
Water
Ether
Olefin
19
EaE2 = 37 kcal/mol
Alumina-catalyzed E2 Elimination
(a) DeWilde, J.F.; Chiang, H.; Hickman, D.A.; Ho, C.R.; Bhan, A. ACS Catal. 2013, 3, 798-807. (b) Christiansen, M.A.; Mpourmpakis, G.; Vlachos, G.D. ACS Catal. 2013, 3, 1965-1975. (c) Zhang, M.; Yu, Y. Ind. Eng. Chem. Res. 2013, 52, 9505-9514
Product C2H5OD C2D5OD Ethylene 0.89 + 0.14 2.42 + 0.19
Diethyl Ether 0.97 + 0.12 1.01 + 0.14
Table 5. Kinetic isotope effects for ethylene and diethyl ether formation over γ-Al2O3 at 215 °C
EaE1 = 57 kcal/mol
20
Ea = 35 kcal/mol
(a) Bhan, A. et al. ACS Catal. 2013, 3, 798-807; (b) Christiansen, M.A., Mpourmpakis, G., Vlachos, G.D. ACS Catal. 2013, 3, 1965-1975; (c) Zhang, M., Yu, Y. Ind. Eng. Chem. Res. 2013, 52, 9505-9514
Alumina-catalyzed E2 Elimination
EaE2 = 38 kcal/mol
EaE1 = 52 kcal/mol
21
Component Range (mol %)
Methane 87-97
Ethane 1.5-7
Propane 0.1 – 1.5
Butane 0.01-0.3
Pentanes plus (C5H12 – C10H22) 0.02
Impurities (N2, CO2, H2S, water) < 7
Table 6. Average concentration of components in natural gas wells in western Canada, Ontario, and U.S. plays
Getting the Most Out of Fossil Fuels 650-900 °C
(a) Zavyalova, U.; Holena, M.; Schloegl, R.; Baerns, M. ChemCatChem, 2011, 3, 1935-1947. (b) Cizeron, J.M.; Scher, E.; Zurcher, F.R.; Schammel, W.P.; Nyce, G.; Rumplecker, A.; McCormick, J.; Alcid, M.; Gamoras, J.; Rosenberg, D.; Ras. E-.J. (Siluria Technologies, Inc. USA). Catalysts for petrochemical catalysis. US 20130023709, January 24, 2013
ΔH1073K = - 124 kcal/mol
ΔH1073K = - 191 kcal/mol
800 °C
800 °C
ΔH1073K = - 33 kcal/mol
22
Direct Coupling of Methane
Catalyst Types
1) Reducible metal oxide
V2O5, MoO3
2) Non-reducible rare-earth oxides LaO3, CeO2
3) Mixed metal oxides Au/Co3O4, Co/MnO
ΔH298K = - 30 kcal/mol
(a) Zavylova, U.; Holena, M.; Schloegl, R.; Baerns, M. ChemCatChem, 2011, 3, 1935-1947. (b) Cizeron, J.M.; Scher, E.; Zurcher, F.R.; Schammel, W.P.; Nyce, G.; Rumplecker, A.; McCormick, J.; Alcid, M.; Gamoras, J.; Rosenberg, D.; Ras, E-.J. (Siluria Technologies, Inc., USA) Catalysts for Petrochemical Catalysis. US Patent 20130023709, January 24, 2013. (c) Li, Z-.Y.; Yuan, Z.; Zhao, Y-X.; He, S-.G. Chem. Eur. J. 2014, 20, 1-8.
Figure 8. Various unsupported single oxides tested in OCM reaction. S(C2) = selectivity for C2H6 and C2H4
23
Key Steps in Oxidative Coupling of Methane
(a) Lunsford, J.H. Angew. Chem. Int. Ed. Engl. 1995, 34, 970-980. (b) ) Cizeron, J.M.; Scher, E.; Zurcher, F.R.; Schammel, W.P.; Nyce, G.; Rumplecker, A.; McCormick, J.; Alcid, M.; Gamoras, J.; Rosenberg, D.; Ras, E-.J. (Siluria Technologies, Inc., USA) Catalysts for Petrochemical Catalysis. US Patent 20130023709, January 24, 2013.
24
(a) Union Gas http://www.uniongas.com/about-us/about-natural-gas/Chemical-Composition-of-Natural-Gas (b) El-Halwagi, M. et al. ACS Sust. Chem. Eng. 2014, 2, 30-37
ΔH298K = -8 kcal/mol
ΔH298K = -10 kcal/mol
ΔH298K = -12 kcal/mol
Indirect Use of Methane
300-500 °C
ΔH298K = 15 kcal/mol
Figure 10. SEM image of SAPO-34 with cartoon of active cages
25
Hydrocarbon Pool Mechanism
Figure 11. Original hydrocarbon pool mechanism as proposed by Dahl and Kolboe
(a) Dahl, I.M., Kolboe, S. J. Catal. 1994, 149, 458-464 (b) Lie, Z. et al. Catal. Commun. 2014, 46, 36-40
Figure 13. 13C incorporation into products and entrained species after 12C-methanol feed is switched to a 13C-methanol feed.
Figure 12. Current understanding of HP mechanism
26
Competing Pathways: Side-Chain v. Paring
(a) Lesthaeghe, D. et al. Chem. Eur. J. 2009, 15, 10803-10808 (b) Ilias, S., Bhan, A. J. Catal. 2014, 311, 6-16. (c) Arstad, B.; Kolboe, S.; Swang, O. J. Phys. Chem. A 2005, 109, 8914-8922.
Side-chain Paring
CH3OH
CH3OH
H2O
H2O
2 CH3OH
27
S-adenosylmethionine Synthetase: EC 2.5.1.6
(a) Van de Poel, B.; Bulens, I.; Oppermann, Y.; Hertog, M.L.A.T.M.; Nicolai, B.M.; Sauter, M.; Geeraerd, A.H. Physiol. Plant. 2013, 148, 176-188. (b) Komoto, J.; Yamada, T.; Takata, Y.; Markham, G.M.; Takusagawa, F. Biochem. 2004, 43, 1821-1831.
S-adenosylmethionine
Asp16
Lys17
29
Capitani, G. et al. J. Mol. Biol. 1999, 294, 745-756
ACC Synthase: EC 4.4.1.14
1-aminocyclopropylcarboxylic acid ACC
Pyridoxal-5’-phosphate PLP
PLP-bound SAM
S-adenosylmethionine SAM
Methylthioadenosine MTA
30
(a) Yoo, A.; Seo, Y.S.; Jung, J-.W.; Sung, S-.K.; Kim, W.T.; Lee, W.; Yang, D.R. J. Struct. Biol. 2006, 156, 407-420. (b) Rocklin, A. M.; Kato, K.; Liu, H-.W.; Que Jr., L.; Lipscomb, J.D. J. Biol. Inorg. Chem. 2004, 9, 171-182. (c) Meng, D.; Shen, L.; Yang, R.; Zhang, X.; Sheng, J. Biochem. Biophys. Acta 2014, 1840, 120-128.
ACC Oxidase: EC 1.14.17.4 ACC
2 H2O O2
HCO3-
ascorbate dehydroascorbate
- OH
H2O + HCO3-
CO2 + HCN
31
Li, N.; Jiang, X.N.; Cai, G.P.; Yang, S.F. J. Biol. Chem. 1996, 271, 25738-25741
Figure 17. Production of ethylene by bifunctional hybrid enzyme in which (1mM) S-AdoMet was used as the ethylene precursor
Heterologous Expression of Ethylene Forming Enzymes
Figure 16. Expression of bifunctional fusion protein in E. coli. (A) Hybrid enzyme inserted into pET-14b. (B) Purification of protein samples.
Escherichia coli
32
Figure 18. Budding Saccharomyces cerevisiae, commonly refered to as “bakers’ yeast.”
S. cerevisiae: Ethanol Factories
Scheme 1. Glycolysis and fermentation of glucose to ethanol in S. cerevisiae
glycolysis
pyruvate
coenzyme A
NADH
acetyl CoA
NADH
(a) Quevedo-Hidalgo, B.; Monsalve-Marin, F.; Narvaez-Rincon, P.C.; Pedroza-Rodriquez, A.M.; Velasquez-Lozano, M.E. World J. Microbiol. Biotechnol. 2013, 49, 459-466. (b) MetaCyc Pathway: Pyruvate Fermentation to Ethanol I. http://www.biocyc.org/META/NEW-IMAGE?type=PATHWAY&object=PWY-5480&detail-level=4&detail-level=3 (accessed 4/4/14).
33
Microbial Ethanol to Ethylene
Phaseollidin hydrate Phaseollidin
Phaseollidin hydratase
EC 4.2.1.97
S. cerevisiae
(a) Marliere, P. EP 2336340, June 22, 2011. (b) Singh, A.; Bajar, S.; Bishnoi, N.R. Fuel, 2014, 116, 699-702
Phaseollidin hydratase
EC 4.2.1.97
34
Ketoglutarate to Ethylene
L-glutamate oxidase
EC 1.4.3.2
Microbial 2-ketoglutarate pathway:
2-ketoglutarate oxygenase
EC 1.13.12.19
(a) Guerro, F.; Carbonell, V.; Cossu, M.; Correddu, D.; Jones, P.R. PLoS ONE, 2012, 7, 1-11. (b) Johansson, N.; Quehl, P.; Norbeck, J.; Larsson, C. Microb. Cell Fact. 2013, 12, 89-95.
Oxidation of Glutamate
35
Microbial Production of Glutamate
Figure 19. Electron micrograph of Methanomonas methylovora
Figure 20. Time course of L-glutamic acid accumulation by M. methylovora. , L-glutamic acid; , bacterial growth.
L-glutamic acid
28 °C Co
mpon
ent G
rowt
h in B
uffer
Med
ium
(a) Oki, T.; Sayama, Y.; Nishimura, Y.; Ozaki, A. Agr. Biol. Chem. 1968, 32, 119-120. (b) Oki. T.; Kitai, A.; Kouno, K.; Ozaki, A. J. Gen. Appl. Microbiol. 1973, 19, 79-83.
2% CH3OH buffer solution
36
Thermal Cracking of Hydrocarbons
750-1000 °C
ΔH298K = 33 kcal/mol
Oxidative Dehydrogenation of Ethane
ΔH298K = - 25 kcal/mol
400-600 °C
Dehydration of Ethanol
Methanol to Olefins
Oxidative Coupling of Methane
300-400 °C
ΔH298K = 11 kcal/mol
(a) van Goethem, M.W.M., Barendregt, S., Grievink, J., Moulijn J.A., Verheijen, P.J.T. Ind. Eng. Chem. Res. 2007, 46, 4045-4062 (b) Gartner, C.A., van Veen, A.C., Lercher, J.A. ChemCatChem, 2013, 5, 3196-3217; (c) Zavyalova, U., Holena, M., Schlogl, R., Baerns, M. ChemCatChem, 2011, 3, 1935-1947
300-500 °C
ΔH298K = 15 kcal/mol
650-900 °C
ΔH298K = - 30 kcal/mol
Mankind’s Syntheses 38