This document outlines Kyle D. Crosby's M.S. defense presentation on hydrogen storage research using LiBH4. The presentation covers hydrogen storage background and challenges, research objectives to improve LiBH4 properties through nanoengineering, mechanical activation and additive effects. Major findings showed ball milling factors like time and temperature improved properties. Additives like graphite and transition metals enhanced hydrogenation/dehydrogenation kinetics and capacities. In conclusion, the research demonstrated diffusion-controlled kinetics and capacity improvements through destabilization, nanostructuring and additive effects.
2. Outline
H2 storage background – Motivation
Freedom CAR targets
Research objectives using LiBH4
Thermodynamic destabilization
Nanoengineering
Mechanical activation
Transition metal addition
Major findings
Ball milling factors
Effects of milling additives
Concluding Remarks
3. Why H2 Energy?
Fossil Fuel issues
Pollution (CO2 & CO)
Limited resource
○ Destructive drilling/mining to obtain
Fuel cell technology, H2
Byproduct of energy is merely H2O
Economic benefit of domestic production
Limitations/Dangers
○ Pressure (700 bar gas cylinder)
○ Temperature (>350°C)
○ Volumetric (<1/3 volumetric density of gasoline)
○ High cost/pollution of H2 production
○ Explosive when oxygen (air) and ignition (electronics of car)
source present
4. Fossil Fuel Issues
Transportation sector = 17.6% of energy
Gasoline internal combustion engine
“dirty” fuel
1/3 the energy content of H2 on a weight basis
○ (48.6 MJ/kg vs. 140.4 MJ/kg)
Rohde, R. Global Warming Art. National Oceanic and Atmospheric Administration.
http://www.globalwarmingart.com/wiki/File:Mauna_Loa_Carbon_Dioxide_png
5. PEMFC
•High energy density
•Low operating temperature
•Only byproduct is water
•Could recycled and used for
onboard H2 production
•Requires highly purified H2 fuel
•Impurities in fuel are deposited in
the hydride pores = loss in storage
capacity as sites for H bonding are FCtec. Proton Exchange Membrane Fuel Cells.
blocked Concurrent Technologies Corporation. 2001 - 2009.
Anode Reactions: 2H2 => 4H+ + 4e-
Cathode Reactions: O2 + 4H+ + 4e- => 2 H2O
Overall Cell Reactions: 2H2 + O2 => 2 H2O
6. H2 Storage
Compressed gas hydrogen
Liquefied hydrogen
Solid state materials
U.S. DOE. Energy Efficiency and Renewable Energy. Fuel Cell Technologies Program. 2008.
http://www1.eere.energy.gov/hydrogenandfuelcells/storage/basics.html
7. Metal Hydride Storage Physics
H2 is physisorbed on surface of metal
particle
H2 dissociates on surface of metal before
absorption
Host metal dissolves H as a solid solution
(α-phase)
H atoms locate at interstitials of host metal
As H concentration increases, local H-H
interaction dominates
(β-phase) nucleates to saturation
8. Honda FCX Clarity – 1st consumer FC Vehicle
American Honda Motor Co., Inc. Honda FCX Clarity. 2009. http://automobiles.honda.com/fcx-clarity/how-fcx-works.aspx
61 mpg, 240 mile range, 100 kW peak output
3.92 kg H2 @ 5000 psi (~350 bar)
$600/month lease in isolated markets
9. 5.5. wt% 7.5 wt%
Freedom CAR targets
• Ford
• GM
• DaimlerChrysler
• BP
• Chevron
• ConocoPhillips
• Exxon Mobile
• Shell
10. Research Objectives
To reduce hydrogenation/dehydrogenation temperature while
simultaneously improving the hydrogen sorption/desorption kinetics in
the LiBH4-based hydrogen storage system via.....
Kinetic = Nanoengineering and mechanical activation
○ Long time ball milling
○ Ball milling at liquid nitrogen temperature (LN2)
Thermodynamic = MgH2 destabilization
○ MgH2 decomposes into Mg and H2
○ Mg catalyzes dehydrogenation of LiBH4
Processing agent = graphite addition
○ Graphite occludes the hydride particle, protecting freshly created surfaces from
oxidation
○ Graphite allows small particles to slide past balls easily (solid lubricant) while forcing
large particles to be refined further, resulting in a highly homogeneous product
Lattice distortion = transition metal addition (Mn & V)
11. Research Approach
Nanoengineering
○ Reduce diffusion distance by reducing particle and
crystallite sizes
Diffusion kinetics are exponentially dependent on distance
Reduction in size of 100x = 10,000x times faster reaction
Kinetic modeling reveals diffusion controlled rate limiting
Mechanical activation
○ Introduce a large number of defects and create fresh
surfaces
Increase # of sites for H2 sorption = increased capacity
Create fresh surfaces = increases reactivity, reduces
sorption/desorption temperature
Dfree surface >> Dg.b. >> Dbulk
12. Research Approach
Thermodynamic destabilization
○ Introduce alternate lower energy reaction pathway
into system
Lowers thermodynamic driving force necessary to react
= lowers sorption/desorption temperature
G = H – TS
ΔHLiBH4 = 67 kJ/mol ΔHLiBH4 + MgH2 = 44 kJ/mol
Transition metal additive enhancement (Mn/V)
○ Disperse additional elements to decrease the
activation energy, Q, for diffusion of the rate
limiting species
D = D0e(-Q/RT)
13. Effect of ball milling time
2LiH + MgB2
10
8
6
Hydrogen (wt%)
3 hr as milled
4
24 hr as milled
24 hr as milled
2
120 hr as milled
120 hr as milled
0
0 1 2 3 4 5 6 7 8
-2
-4
Time (hr)
14. (Mg1-xLi2x)B2 Formation
2LiBH4 (s) + MgH2 (s) 2LiH (s) + MgB2 (s) + 4H2 (g)
Direct, reversible reaction
Actually proceeds through (Mg1-xLi2x)B2 before forming LiBH4
Hu, J. Z.; Kwak, J. H.; Yang, Z.; Wan, X.; Shaw, L. “Direct observation of ion exchange in mechanically activated LiH+MgB2 system using ultra-high field
nuclear magnetic resonance spectroscopy,” Appl. Phys. Lett. 2009, 94, 141905.
15. Effect of Ball Milling Temperature
Rise in local temp. at ball collision site can be
>300°C
Tm = 280°C for LiBH4
Ball milling at room temp. (25°C) leads to >325°C
indicating melting, agglomeration, and sintering
Ball milling at LN2 (-196°C) leads to >104°C
indicating no melting and a decrease in cold welding,
agglomeration still witnessed however
16. Effect of processing agent, C
w/o C
2LiBH4 + MgH2
with 5 vol% C 3 hr LN2 ball milling
2°C/min ramp to 265°C
35
Si MgH2 LiBH4
30
2LiBH4 + MgH2
25 ball milled 3 hr @ LN2
Cu Kα
Relative Intensity
20
2LiBH4 + MgH2 + 5 vol% C
15 hand mixed
10
2LiBH4 + MgH2 + 5 vol% C
ball milled 3 hr @ LN2
5
0
10 20 30 40 50 60 70 80
2 Theta
23. Kinetic Modeling
Diffusion Control
Moving Interface Control
Gas Adsorption Control
Nucleation and Growth
Control
[Wan, X.; Markmaitree, T.; Osborn, W.; Shaw, L. “Nanoengineering-enabled solid-state hydrogen uptake and release in the LiBH4 plus MgH2 system,”
J. Phys. Chem. C 2008, 112, 18232-18243 .
24. Kinetic Modeling - Solid State (T = 265°C)
Nucleation and Growth Control
ln{ln(1/1-f’f)} = -13.355 + 1.3002lnt
with R2 = 0.6724
Gas Desorption Control
(f’f) = 0.0853 + 0.00002(t + Δt)
with R² = 0.7652
Moving Interface Control
(1-f’f)1/3 = 0.9727 - 0.000007(t + Δt)
with R² = 0.7984
Diffusion control
(1- f’f)1/3 = 1.0041 - 0.0012(t + Δt)1/2
with R² = 0.9143
25. Kinetic Modeling – Solid State (T = 265°C)
Release under 4-bar backpressure results in unambiguous diffusion controlled
reaction because H2 suppresses formation of elemental Mg, thus MgH2 does
not contribute to diffusion, thus a single species mechanism is accurate (R2 ↑).
26. Kinetic Modeling – Liquid State
Gas Desorption Control
(f’f) = -0.0034 + 0.00008t
with R² = 0.9952
T = 280°C
Gas Desorption Control
(f’f) = -0.0068 + 0.00006t
with R² = 0.9986
T = 275°C
Diffusion Control
(1-f’f)1/3 = 0.9913 - 0.0008(t + Δt)1/2
with R² = 0.849
T = 275°C
28. Effect of Mn/V addition
7
6
5
4 No Addition
2LiH + MgB2
Hydrogen (wt%)
3 No Addition 24 hr R.T. ball milling
2 With Mn 2°C/min ramp to 265°C
1 With Mn
With V
0
0 2 4 6 8 With V
-1
-2 35
-3
Time (hr) 30
Relative Intensity 25
20
Unmilled
15 3 hr as milled
Cu Kα 10 24 hr as milled
5
0
35 40 45 50 55
2 Theta
29. Concluding Remarks
Increasing ball milling duration results in more favorable hydrogenation/dehydrogenation attributes because of the
mechanical activation and nanoengineering effects (i.e. ball milling produces particles with refined crystallites,
increased defect concentrations, increased grain boundary area, fresh reactive particle surfaces, and homogeneous
mixtures of the metal hydride reactants)
Ball milling at LN2 temperature further enhances the mechanical activation and nanoengineering processes
because the equivalent energy transfer is applied to a particle that is now more brittle than for identical mixtures ball
milled at room temperature (i.e. brittle particles experience more efficient fracture with less cold welding)
MgH2 destabilization shows a nearly fivefold increase in the storage capacity (4.0 wt% vs. <0.5 wt%) of the LiBH4
system by creating an alternate lower energy reaction pathway for the uptake/release of hydrogen (i.e. MgH2 first
decomposes into Mg and H2 wherein the Mg catalyzes the dehydrogenation of LiBH4)
Graphite solid lubrication enhances ball milling efficiency by preventing cold welding and caking (i.e. graphite
particles encapsulate the metal hydride reactants during ball milling, effectively preventing intimate contact and
providing a buffer on the surface of the particle to prevent oxidation. Thus, cold welding and sintering do not occur
during ball milling and the result is a highly homogeneous product.)
Hydrogenation and dehydrogenation rate limiting kinetics are shown to be diffusion-controlled for the overall H2
uptake and release processes in the 2LiBH4 + MgH2 mixtures.
Mn and V addition demonstrate the need for proper choice in additive (i.e. Mn enhances only the hydrogenation
reaction of 2LiH + MgB2 mixtures via enhancement the diffusion coefficient of Mg in the (Mg1-xLi2x)B2 compound. As
the diffusion coefficient of the rate limiting species is increased, the overall kinetic rate is increased. V enhances
only the dehydrogenation reaction by improving the decomposition rate of MgH2, allowing free Mg to catalyze the
decomposition reaction of LiBH4, thus increasing dehydrogenation kinetics.)
30. Acknolwedgements/Thanks
This work was supported under the U.S. Department of
Energy (DOE) Contract No. DE-FC36-05GO15008.
The vision and support of Dr. Ned T. Stetson, DOE
Technology Managers, are greatly appreciated.
Thank you......
Family and friends for supporting me throughout my
academic career
UConn and IMS for offering the opportunity to pursue
higher education
Dr Shaw for providing the project and funding opportunity
Dr. Brody and Dr. Huey for sacrificing their time during
finals to serve on my panel
31. Works Cited
[1] Gupta, R. Hydrogen Fuel: Production, Transport and Storage. CRC Press. New York. 2009.
[2] Rohde, R. Global Warming Art. National Oceanic and Atmospheric Administration.
http://www.globalwarmingart.com/wiki/File:Mauna_Loa_Carbon_Dioxide_png
[3] Marban, G. and Valdes-Solis, T. Towards the Hydrogen Economy? Int. J. Hydrogen Energy, 32(12), 1625-1637, 2007.
[4] United States Department of Energy. Energy Efficiency and Renewable Energy Program Multi-Year Research,
Development, and Demonstration Plan. Hydrogen Storage, April 2009.
http://www1.eere.energy.gov/hydrogenandfuelcells/mypp/pdfs/storage.pdf
[5] Satyapal, S. “Hydrogen Storage Sub-Program Overview,” United States Department of Energy Hydrogen Program.
2008 Annual Progress Report. http://www.hydrogen.energy.gov/pdfs/progress08/iv_0_hydrogen_storage_overview.pdf
[6] Schlapbach, L.; Zuttel, A. “Hydrogen-storage materials for mobile applications,” Nature 2001, 414, 353-358.
[7] Soulie, J.; Renaudin, G.; Cerny, R.; Yvon, K. “Lithium borohydride LiBH4: I. Crystal Structure” J. Alloys Compd. 2002,
346, 200-205.
[8] Zuttel, A.; Rentsch, S.; Fischer, P.; Wenger, P.; Sudan, P.; Mauron, Ph.; Emmenegger, Ch. “LiBH4 a new hydrogen
storage material,” J. Power Sources 2003, 118, 1-7.
[9] Zuttel, A.; Rentsch, S.; Fischer, P.; Wenger, P.; Sudan, P.; Mauron, Ph.; Emmenegger, Ch. “Hydrogen storage
properties of LiBH4,” J. Alloys Comp. 2003, 356-357, 515 -520.
[10] Kostka, J.; Lohstroh, W.; Fichtner, M.; Hahn, H. “Diborane release from LiBH4/silica-gel mixtures and the effect of
additives,” J. Phys. Chem. C 2007, 111, 14026-14029.
32. Works Cited
[11] Yu, X. B.; Wu, Z.; Chen, Q. R.; Li, Z. L.; Weng, B. C.; Huang, T. S. “Improved hydrogen storage properties of LiBH4
destabilized by carbon,” Appl. Phys. Lett. 2007, 90, 034106.
[12] Fang, Z. Z.; Wang, P.; Rufford, T. E.; Kang, X. D.; Lu, G. Q.; Cheng, H. M. “Kinetic- and thermodynamic-based
improvements of lithium borohydride incorporated into activated carbon,” Acta Mater. 2008, 56, 6257-6263.
[13] Zhang, Y.; Zhang, W.-S.; Wang, A.-Q.; Sun, L.-X.; Fan, M.-Q.; Chu, H.-L.; Sun, J.-C.; Zhang, T. “LiBH4 nanoparticles
supported by disordered mesoporous carbon: hydrogen storage performances and destabilization mechanisms,” Int. J.
Hydrogen Energy 2007, 32, 3976-3980.
[14] A. Zuttel, S. Rentsch, P. Fischer, P. Wenger, P. Sudan, Ph. Mauron, and Ch. Emmenegger, “Hydrogen storage
properties of LiBH4,” J. Alloys Comp., 2003, 356-357, 515.
[15] P. Mauron, F. Buchter, O. Friedrichs, A. Remhof, M. Bielmann, C. N. Zwicky, and A. Zuttel, “Stability and reversibility
of LiBH4,” J. Phys. Chem. B, 2008, 112, 906-910.
[16] A. F. Gross, J. J. Vajo, S. L. Van Atta, and G. L. Olson, “Enhanced hydrogen storage kinetics of LiBH4 in nanoporous
carbon scaffolds,” J. Phys. Chem. C, 2008, 112, 5651-5657.
[17] Vajo, J. J.; Skeith, S. L.; Mertens, F. “Reversible storage of hydrogen in destabilized LiBH4,” J. Phys. Chem. B 2005,
109, 3719-3722.
[18] Yu, X. B.; Grant, D. M.; Walker, G. S. “A new dehydrogenation mechanism for reversible multicomponent borohydride
systems – the role of Li-Mg alloys,” Chem. Commun. 2006, 3906-3908.
[19] Pinkerton, F. E.; Meyer, M. S.; Meisner, G. P.; Balogh, M. P.; Vajo, J. J. “Phase boundaries and reversibility of
LiBH4/MgH2 hydrogen storage material,” J. Phys. Chem. C 2007, 111, 12881-12885.
[20] Nakagawa, T.; Ichikawa, T.; Hanada, N.; Kojima, Y.; Fujii, H. “Thermal analysis on the Li-Mg-B-H systems,” J. Alloys
Comp. 2007, 446-447, 306-309.
33. Works Cited
[21] Walker, G. S.; Grant, D. M.; Price, T. C.; Yu, X. B.; Legrand, V. “High capacity multicomponent hydrogen storage
materials: investigation of the effect of stoichiometry and decomposition conditions on the cycling behavior of LiBH4-MgH2,”
J. Power Sources 2009, 194, 1128-1134.
[22] Yang, J.; Sudik, A.; Wolverton, C. “Destabilizing LiBH4 with a metal (M = Mg, Al, Ti, V, Cr, or Sc) or metal hydride
(MH2 = MgH2, TiH2, or CaH2),” J. Phys. Chem. C 2007, 111, 19134-19140.
[23] Wan, X.; Markmaitree, T.; Osborn, W.; Shaw, L. “Nanoengineering-enabled solid-state hydrogen uptake and release in
the LiBH4 plus MgH2 system,” J. Phys. Chem. C 2008, 112, 18232-18243.
[24] Hu, J. Z.; Kwak, J. H.; Yang, Z.; Wan, X.; Shaw, L. “Direct observation of ion exchange in mechanically activated
LiH+MgB2 system using ultra-high field nuclear magnetic resonance spectroscopy,” Appl. Phys. Lett. 2009, 94, 141905.
[25] Yang, Z.-G.; Shaw, L. “Synthesis of nanocrystalline SiC at ambient temperature through high energy reaction milling,”
Nanostruct. Mater. 1996, 7, 873-886.
[26] Klug, H. P.; Alexander, L. E. X-ray diffraction procedures for polycrystalline and amorphous materials; John Wiley &
Sons, Inc.: New York, NY, 1974.
[27] Stokes, A. R.; Wilson, A. J. C. “The diffraction of X-rays by distorted crystal aggregates - I,” Proc. Phys. Soc. London,
1944, 56, 174-181.
[28] Shaw, L.; Villegas, J.; Luo, H.; Miracle, D. “Thermal stability of nanostructured Al93Fe3Ti2Cr2 alloys prepared via
mechanical alloying,” Acta Mater. 2003, 51, 2647-2663.
[29] Ortiz, A. L.; Shaw, L. “X-ray diffraction analysis of a severely plastically deformed aluminum alloy,” Acta Mater. 2004,
52, 2185-2197.
[30] Brunauer, S.; Emmett, P. H.; Teller, E.; “Adsorption of gases in multimolecular layers,” J. Am. Chem. Soc. 1938, 60,
309-319.
34. Works Cited
[31] Davis, R. M.; McDermott, B.; Koch, C. C. “Mechanical alloying of brittle materials,” Mater. Trans. 1988, 19A, 2867-
2874.
[32] Miller, P. J.; Coffey, C. S.; DeVast, V. F. “Heating in crystalline solids due to rapid deformation,” J. Appl. Phys. 1986,
59, 913-916.
[33] Joardar, J.; Pabi, S. K.; Murty, B. S. “Estimation of entrapped powder temperature during mechanical alloying,” Scr.
Mater. 2004, 50, 1199-1202.
[34] Shaw, L.; Yang, Z.-G.; Ren, R.-M. “Synthesis of nanostructured Si3N4/SiC composite powders through high energy
reaction milling,” Mater. Sci. Eng. 1998, A244, 113-126.
[35] Bogdanovic, B.; Bons, P.; Schwickardi, M.; Seevogel, K. “Tetrahydrofuran-soluble magnesium dihydride by catalytic
hydrogenation of magnesium,” Chem. Ber. 1991, 124, 1041-1050.
[36] Huang, Z. G.; Guo, Z. P.; Calka, A.; Wexler, D.; Wu, J.; Notten, P. H. L.; Liu, H. K. “Noticeable improvement in the
desorption temperature from graphite in rehydrogenated MgH2/graphite composite,” Mater. Sci. Eng. A 2007, 447, 180-
185.
[37] Zeng, K.; Klassen, T.; Oelerich, W.; Bormann, R. “Critical assessment and thermodynamic modeling of the Mg-H
system,” Int. J. Hydrogen Energy 1999, 24, 989-1004.
[38] Bouaricha, S.; Dodelet, J. P.; Guay, D.; Huot, J.; Schulz, R. “Activation characteristics of graphite modified hydrogen
absorbing materials,” J. Alloys Compd. 2001, 325, 245-251.
[39] Guvendiren, M.; Bayboru, E.; Ozturk, T. “Effects of additives on mechanical milling and hydrogenatioin of magnesium
powders,” Int. J. Hydrogen Energy 2004, 29, 491-496.
[40] Wu, C. Z.; Wang, P.; Yao, X.; Liu, C.; Chen, D. M.; Lu, G. Q.; Cheng, H. M. “Hydrogen storage properties of
MgH2/SWNT composite prepared by ball milling,” J. Alloys Compd. 2006, 420, 278-282.
[41] Mao, J. F.; Wu, Z.; Chen, T. J.; Weng, B. C.; Xu, N. X.; Huang, T. S.; Guo, Z. P.; Liu, H. K.; Grant, D. M.; Walker, G.
S.; Yu, X. B. “Improved hydrogen storage of LiBH4 catalyzed magnesium,” J. Phys. Chem. C 2007, 111, 12495-12498.
[42] Zaluska, A.; Zaluski, L.; Strom-Olsen, J. O. “Structure, catalysis and atomic reactions on the nano-scale: a systematic
approach to metal hydrides for hydrogen storage,” Appl. Phys. A 2001, 72, 157-165.
35. Works Cited
[43] Huot, J.; Liang, G.; Schulz, R. “Mechanically alloyed metal hydride systems,” Appl. Phys. A 2001, 72, 187-195.
[44] Tien, H.-Y.; Tanniru, M.; Wu, C.-Y.; Ebrahimi, F. “Effect of hydride nucleation rate on the hydrogen capacity of Mg,”
Int. J. Hydrogen Energy 2009, 34, 6343-6349.
[45] Tanniru, M.; Ebrahimi, F. “Effect of Al on the hydrogenation characteristics of nanocrystalline Mg powder,” Int. J.
Hydrogen Energy 2009, 34, 7714-7723.
[46] Markmaitree, T.; Ren, R; Shaw, L. Enhancement of lithium amide to lithium imide transition via mechanical activation.
J. Phys. Chem. B 2006, 110, 20710.
[47] Welsch, G., Desai, P. D., Eds. Oxidation and Corrosion of Intermetallic Alloys; Purdue Research Foundation: West
Lafayette, IN, 1996.
[48] Christian, J. W. The Theory of Transformations in Metals and Alloys; Pergamon: Oxford, U.K., 2002; Part I.
36. LiBH4
LiBH4 crystal structure
•low temp (<110°C) = orthorhombic (top)
•high temp = hexagonal (bottom)
Grey = B
[BH4]-
Red = H
Blue = Li+
Interstitial sites
Octahedral – red
Tetrahedral - blue
Hartman, M., Rush, J., Udovic, T., Bowman, R.,
Hwang, S.J. “Sturcture and Vibrational Dynamics of
Isotropically Labeled Lithium Borohydride Using
Neutron Diffraction and Spectroscopy,” J. of Solid
State Chem. 2007, 180, 1298-1305.
37. Storage Improvement Methods
Structure directing agents
Carbon aerogels
○ Confinement of particles restricts grain growth
during thermal cycling
initial particle size retained throughout
hydro/dehydrogenation
Surface activation treatment
Ni catalyzes surface dissociation of H2
○ Increase kinetics of system
High SSA materials
Maxsorb carbon (3000 m2/g)
39. No SEM/TEM
Weak scattering by light elements (H, Li, B) restricts direct
observation
High SSA, hydrophilic nanopowders are extremely reactive
in air
Samples oxidize and “foam” up upon loading into
SEM/TEM
Beam damage
LiBH4 low melting temp, particles vaporize under beam
41. XRD Analysis
Sherrer Formula – crystallite size
Stokes-Wilson Formula – internal strain
Appearance of new peaks – new phase(s)
Peak shifting – solid solution formation
Orthorhombic
1/d2 = h2/a2 + k2/b2 + l2/c2
Hexagonal
1/d2 = 4/3(h2 + hk + k2/a2) + l2/c2
42. RGA Background
Quadrupole gas analyzer
Quadrupole analyzer uses four rods (two tandems) with
oscillating voltage
RF voltage applied to one set of rods such that only ions
of a specific mass/charge (m/z) will reach the detector all
other ions will oscillate with unstable trajectories and
collide with the rod
Voltage can be scanned continuously or set to detect a
single species
43. FTIR Background
Types of bond detection using FTIR
Measures absorbance or transmittance of IR wavelength – shows
molecular structure of the material
44. Raman
Types of energy shifts detected by Raman
Absorption
Rayleigh means equal before and after
Stokes means final state is more energetic than initial
Anit-Stokes means initial state is more energetic than final
45. BET
Gas adsorption in monolayers on the surface of a solid material based on
equilibrium and saturation pressures of the gas
47. H2 Production
Production
Natural gas refining (48%)
○ Requires carbon sequestration
Petroleum refining (30%)
○ Net usable is 0% : consumed internally in the
refinery
Water electrolysis (4%)
DOE target is $2.00-3.00/gge