Contents

Cover

Title page

Copyright page

Preface

Part I: Chemical and Electrochemical Hydrogen Storage

Chapter 1: Metal Hydride Hydrogen Compression Systems – Materials, Applications and Numerical Analysis
1. 1.1 Introduction
2. 1.2 Adoption of a Hydrogen-Based Economy
3. 1.3 Hydrogen Compression Technologies
4. 1.4 Metal Hydride Hydrogen Compressors (MHHC)
5. 1.5 Numerical Analysis of a Multistage MHHC System
6. 1.6 Conclusions
7. Acknowledgments
8. Nomenclature
9. References
Chapter 2: Nitrogen-Based Hydrogen Storage Systems: A Detailed Overview
1. 2.1 Introduction
2. 2.2 Amide/Imide Systems
3. 2.3 Ammonia (NH₃) as Hydrogen Storage Media
4. 2.4 Future Prospects
5. References
Chapter 3: Nanostructured Mg-Based Hydrogen Storage Materials: Synthesis and Properties
1. 3.1 Introduction
2. 3.2 Experimental Details
3. 3.3 Synthesis Results of the Nanostructured Samples
4. 3.4 Hydrogen Absorption Kinetics
5. 3.5 Hydrogen Storage Thermodynamics
6. 3.6 Novel Mg-TM (TM=V, Zn, Al) Nanocomposites
7. 3.7 Summary and Prospects
8. Acknowledgments
9. References
Chapter 4: Hydrogen Storage in Ti/Zr-Based Amorphous and Quasicrystal Alloys
1. 4.1 Introduction
2. 4.2 Production of Ti/Zr-Based Amorphous and Quasicrystal Alloys
3. 4.3 Hydrogen Storage in T-Zr-Based Amorphous Alloys
4. 4.4 Hydrogen Storage in the Ti/Zr-Based Quasicrystal Alloys
5. 4.5 Comparison of Amorphous and Quasicrystal Phases on the Hydrogen Properties
6. 4.6 Conclusions
7. References
Chapter 5: Electrochemical Method of Hydrogenation/Dehydrogenation of Metal Hydrides
1. 5.1 Introduction
2. 5.2 Electrochemical Method of Hydrogenation of Metal Hydrides
3. 5.3 Electrochemical Method of Dehydrogenation of Metal Hydrides
4. 5.4 Discussion
5. 5.5 Conclusions
6. References

Part II: Carbon-Based Materials for Hydrogen Storage

Chapter 6: Activated Carbon for Hydrogen Storage Obtained from Agro-Industrial Waste
1. 6.1 Introduction
2. 6.2 Experimental
3. 6.3 Results and Discussion
4. 6.4 Conclusions
5. Acknowledgments
6. References
Chapter 7: Carbonaceous Materials in Hydrogen Storage
1. 7.1 Introduction
2. 7.2 Materials Consisting of Only Carbon Atoms
3. 7.3 Materials Containing Carbon and Other Light Elements
4. 7.4 Composite Materials Made by Polymeric Matrix
5. 7.5 Waste and Natural Materials
6. 7.6 Conclusions
7. References
Chapter 8: Beneficial Effects of Graphene on Hydrogen Uptake and Release from Light Hydrogen Storage Materials
1. 8.1 Introduction
2. 8.2 General Aspects of Graphene
3. 8.3 Beneficial Effect of Graphene: Key Results with Light Metal Hydrides (e.g., LiBH₄, NaAlH₄, MgH₂)
4. 8.4 Alanates as HS Materials
5. 8.5 Magnesium Hydride as HS Material
6. 8.6 Summary and Future Prospects
7. Acknowledgment
8. References
Chapter 9: Hydrogen Adsorption on Nanotextured Carbon Materials
1. 9.1 Introduction
2. 9.2 Hydrogen Storage in Carbon Materials
3. 9.3 Conclusion
4. Acknowledgments
5. References
6. Appendix

Index

End User License Agreement

List of Illustrations

Chapter 2

Figure 1.1 Density of the compressed hydrogen as pressure function at six different temperatures [18].
Figure 1.2 Schematic of a two-stage mechanical compressor.
Figure 1.3 Schematic of a hydraulic liquid ionic compressor (LINDE) [26].
Figure 1.4 Schematic of a diaphragm compression system [28].
Figure 1.5 Basic components and the operational principle of the electrochemical compressor.
Figure 1.6 A simplified scheme of a two-stage metal hydride hydrogen compression system.
Figure 1.7 The van’t Hoff diagram describing the operation steps of a two-stage metal hydride hydrogen compressor (a) and P-c-T plot describing the operation steps of a two-stage metal hydride hydrogen compressor (b).
Figure 1.8 P-c-T curves at different temperatures (a) and van’t Hoff plot (b). The upper left lattice represents the solid solution phase (α-phase), the lower left lattice represents the co-existence of the solid solution and the hydride phase (in the cycle) and finally the middle right lattice represents the hydride phase (β-phase).
Figure 1.9 Representation of the hysteresis between the hydrogenation process (black isotherm) and the dehydrogenation process (red isotherm) and the slope of the plateau region.
Figure 1.10 Schematic of a cylindrical metal hydride tank. The tank is filled up to 50% of the total volume of the tank due to the expansion of the metal hydride lattice during the hydrogen sorption.
Figure 1.11 Schematic of a cylindrical metal hydride tank used for the validation process. The tank is filled up to 50% of the total volume of the tank due to the expansion of the metal hydride lattice during the hydrogen sorption. A thermocouple was installed to measure the temperature of the hydride during the hydrogenation/dehydrogenation.
Figure 1.12 Validation of the predicted temperature profile (red) and the hydrogen storage capacity (black) for MmNi_4.6Al_0.4.
Figure 1.13 Bed average temperature evolution during the complete three-stage compression process when using LaNi₅, MmNi_4.6Al_0.4 and AB₂ Laves phase Intermetallic as the stages of the compression.
Figure 1.14 Bed average pressure evolution during the complete three-stage compression process when using LaNi₅, MmNi_4.6Al_0.4 and AB₂-Intermetallic as the stages of the compression.

Chapter 2

Figure 2.1 The conventional unit cell of LiNH₂, with Li, N, and H represented by green (large), blue (medium), and purple (small) spheres, respectively. T and O (small black spheres) denote one of the tetrahedral and octahedral sites of the N sublattice, respectively. (Reproduced from [16] with permission of American Physical Society)
Figure 2.2 Weight variations during hydrogen absorption and desorption processes over Li₃N samples. (Reproduced from [3] with permission of Nature Publishing Group)
Figure 2.3 Ambient-pressure crystal structure of NaNH₂ in space group Fddd. The coordinate system is indicated to show the orientations of the unit cell. The color codes for atoms are pink (sodium), blue (nitrogen), and white (hydrogen). (Reproduced from [36] with permission of American Chemical Society)
Figure 2.4 (a) H₂, N₂ and NH₃ MS profile for (i) NaNH₂ and (ii) NaNH₂-NaH decomposition (Reproduced from [41] with permission of Elsevier). (b) IR spectra of the as-synthesized NaNH₂, the reaction products after heating at 400 °C under the gas trap, and the vacuum condition (Reproduced from [43] with permission of Elsevier).
Figure 2.5 (a) Unit cell of Mg(NH₂)₂. The big yellow balls denote the Mg atom, the medium pink, green, and dark brown balls denote the N1, N2, and N3 atoms, respectively, and the small grey, red, blue, and light brown balls denote the H1, H2, H3, and H4 atoms, respectively (Reproduced from [47] with permission of Elsevier). (b) Structure representation of a small part (three units) of the infinite sequence of face sharing Mg₆N₆ units in magnesium imide. Mg₆N₆ hexagonal prisms are highlighted in gray; Magnesium atoms are in yellow; Nitrogen atoms are in green; Deuterium atoms are in red. (Reproduced from [48] with permission of American Chemical Society).
Figure 2.6 (Top) Part of the structure of Ca(ND₂)₂ including the amide ion orientation (Reproduced from [56] with permission of American Chemical Society). (Bottom Left) Structure of CaNH and (Bottom Right) Structure of Ca₂NH (Reproduced from [57] with permission of Elsevier).
Figure 2.7 Schematic diagram of the synthesis and decomposition processes of Ca(NH₂)₂. Synthesis: CaH₂ reacts with ammonia to produce Ca(NH₂)₂ during milling, but still exists in a core part. Decomposition: Ca(NH₂)₂ decomposes to CaNH by heating, then CaNH reacts with CaH₂ in the core part at high temperatures and desorbs H₂. (Reproduced from [58] with permission of Elsevier)
Figure 2.8 Crystal structures of Li₃Na(NH₂)₄ (left), and LiNa₂(NH₂)₃ (right); with Li represented as red spheres, Na as blue spheres, N as green spheres and H as white spheres. (Reproduced from [60] with permission of Royal Society of Chemistry)
Figure 2.9 The sorption mechanism of LiNH₂-NaH system. (Reproduced from [40] with permission of American Chemical Society)
Figure 2.10 (a) Structure of a-Li₂Mg(NH)₂. Nitrogen atoms (dark grey), protons (white), mixed lithium and magnesium sites (small light grey) and vacancies (large transparent grey) are shown; (b) Structure of β-Li₂Mg(NH)₂. Nitrogen atoms (dark grey), protons (white), lithium (light grey bcc site), two distinct mixed lithium and magnesium sites (small dark grey) and vacancies (large translucent grey) are shown; (c) Structure of γ-Li₂Mg(NH)₂. Nitrogen atoms (dark grey), protons (white), and mixed lithium, magnesium, and vacancy sites (small grey) are shown. (Reproduced from [65] with permission of Elsevier)
Figure 2.11 (a) Hydrogen absorption in a Li₂Mg(NH)₂ sample and desorption from Mg(NH₂)₂ + 2LiH sample (Reproduced from [69] with permission of Elsevier); (b) Pressure-composition isotherms at 220 ºC for (2LiNH₂ + MgH₂). Isotherms at 285 ºC for (LiNH₂ + LiH) are included for comparison (Reproduced from [70] with permission of Elsevier).
Figure 2.12 Temperature dependences of H₂ and NH₃ release from the potassium-modified (—) and the pristine (—-) samples. (Reproduced from [83] with permission of John Wiley and Sons)
Figure 2.13 (Left) Off-[110] view of the refined trigonal structure of Li₂Ca(NH)₂. Ca(NH)₆ octahedra are in green; Li(NH)₄ tetrahedra are in yellow. Ca, Li, and N atoms are represented by large pink, yellow, and blue spheres, respectively. H atoms are randomly distributed at one of the three white sites around each N atom. (Right) The layered structure of Li₂Ca(NH)₂ viewed as a “combined imide” consisting of ordered CaNH layer and Li₂NH layer. (Reproduced from [94] with permission of American Chemical Society)
Figure 2.14 Hydrogen desorption from LiAlH₄-LiNH₂/HMPA; inset shows the schematic mechanism of dehydrogenation. (Reproduced from [108] with the permission of Royal Society of Chemistry)
Figure 2.15 (a) Schematic model of Ru-loaded C12A7:e^–. High-density electrons (2.0 × 1021 cm^–3) are distributed statistically in the subnanometer-sized cages of C12A7 as counteranions and electrons encaged in C12A7 can be exchanged by H- ions under an H₂ atmosphere; (b) TOFs for high-pressure ammonia synthesis over 1 wt% Ru/C12A7:e^– and 6 wt% Ru-Cs/MgO. (Reproduced from [157] with permission of Nature Publishing Group)
Figure 2.16 Proposed reaction mechanism of ammonia synthesis over Ru/C12A7:e^–. (Reproduced from [159] with permission of American Chemical Society)
Figure 2.17 Calculated turnover frequencies for ammonia synthesis as a function of the adsorption energy of nitrogen. (Reproduced from [160] with permission of American Chemical Society)
Figure 2.18 Temperature programmed desorption of ammonia from Ca(NH₃)₈Cl₂ and Mg(NH₃)₆Cl₂. (Reproduced from [130] and [181] with permission of Royal Society of Chemistry and American Chemical Society respectively)
Figure 2.19 PC isotherms for NH₃ absorption of different borohydrides. (Reproduced from [189] with permission of American Chemical Society)

Chapter 3

Figure 3.1 Schematic diagram of the equipment setup for synthesis of metal nanoparticles by HPMR method. It includes arc melting chamber, water-cooled copper stand, tungsten electrode, heat exchanger, nanoparticle collecting room with filter, vacuum pump and DC power source. The inserts are (a) a photo of the apparatus and (b) a real photo of the plasma during synthesis.
Figure 3.2 XRD curves and TEM images of the metal nanoparticle samples synthesized by HPMR method: (a, b) Mg, (c, d), Ni, (e, f) Co, and (g, h) Cu.
Figure 3.3 X-ray curves and TEM images of the (a, b) Mg₂Ni, (c, d) Mg₈₅Ni₁₅, (e, f) Mg₂Co and (g, h) Mg₂Cu alloys synthesized from Mg, Ni, Co and Cu metal nanoparticles.
Figure 3.4 (a) Hydrogen absorption curves of various Mg-M-based nanoparticle samples (Mg, Mg₂Ni, Mg₂Cu, Mg₂Co and Mg₈₅Ni₁₅). (b) Absorption curves in 5 cycles of the Mg₂Ni nanoparticle sample.
Figure 3.5 A schematic showing the effect of nanosizing on the absorption kinetics in Mg-based hydrogen storage materials. (Reproduced with permission from [62])
Figure 3.6 Pressure-composition isotherms (PCTs) of hydrogen absorption/desorption steps of different Mg-M-H (M = none, Ni, Co and Cu) systems in nanometer scale.
Figure 3.7 The van’t Hoff plots of the desorption reactions for four different MgH₂–Mg systems synthesized by different methods (HPMR method, catalyzed chemical solution synthesis, high-pressure reactive ball milling under 30 MPa hydrogen and the commercial one from Alfa Aesar). (Reproduced with permission from [3])
Figure 3.8 The van’t Hoff plots for desorption reactions of Mg-H, Mg-Ni-H, Mg-Co-H and Mg-Cu-H nanoparticle samples. (Reproduced with permission from [50])
Figure 3.9 XRD pattern (a) and TEM (b) images of Mg-Al nanocomposite, the inset figure is the HRTEM image of the Mg-Al nanocomposite; XRD pattern (c) and TEM (d) images of the Mg–V nanocomposite, the inset figure is the SAED image of the Mg–V nanocomposite; XRD pattern (e) and TEM (d) images of the Mg-Zn nanocomposite, the inset figure is the SAED of the Mg-Zn nanocomposite.
Figure 3.10 Hydrogen absorption curves under 4 MPa hydrogen pressure of the Mg-Al, Mg-V, and Mg-Zn nanocomposites at (a) 623 K, (b) 573 K and (c) 523 K.
Figure 3.11 XRD patterns of the Mg-Al, Mg-V, and Mg-Zn nanocomposites: (a) after hydrogenation in 4 MPa hydrogen at 673 K, (b) after dehydrogenation under 100 Pa at 673 K.

Chapter 4

Figure 4.1 The bright field images and the corresponding selected area diffraction patterns for the Ti₄₅Zr₃₈Ni₁₇ powders: (a) after MA and subsequent annealing, and (b) after the hydrogen absorption/desorption cycle, and (c) the high- resolution transmission electron microscopic (HREM) image with the corresponding fast Fourier transform (FFT) image; (d) the inverse FFT image derived from the FFT image for the powders after MA and subsequent annealing.
Figure 4.2 Comparison of both sides of the ribbon and the SEM images for the Ti₄₅Zr₃₈Ni₁₇ i-phase: (a) X-ray diffraction pattern of the air-side surface; (b) SEM image of the air-side surface; (c) X-ray diffraction pattern of the wheel-side surface; (d) SEM image of the wheel-side surface.
Figure 4.3 The SEM images of (a) the air side of the ribbon (low magnification); (b) the air side of the ribbon (different region of phases: the quasicrystal [the i-phase] and the amorphous [the AMO-phase]); (c) a topography image of the quasicrystalline surface (EBSD - the topography mode); (d) EBSD - the dark field diffraction contrast mode.
Figure 4.4 (a) In-situ synthesis of the amorphous Ti₄₅Zr₃₈Ni₉Fe₈ hydrides/deuterides as seen by neutron diffraction performed under 0.4 MPa of D₂ pressure at 20 ºC; (b) SAD-TEM image of the synthesized amorphous hydride; (c) neutron diffraction patterns before and after deuteration; (d) hydrogen uptake occurring during collecting of the neutron diffraction patterns; and (e) thermal evolution of the deuterided amorphous alloy.
Figure 4.5 Comparison of thermal evolution of the main reflections for the amorphous (a) Ti₄₅Zr₃₈Ni₁₃Fe₄ and (b) Ti₄₅Zr₃₈Ni₁₃Fe₄D₁₄₈.
Figure 4.6 The composition-temperature phase diagrams of several Ti₄₅Zr₃₈Ni_17-xT_x alloys [19].
Figure 4.7 The absorption and desorption pressure-composition isotherms for the Ti₄₅Zr₃₈Ni₁₇ i-phase powders produced by mechanical alloying and subsequent annealing [10].
Figure 4.8 Thermal evolution of the deuterated Ti₄₅Zr₃₈Ni₁₇ quasicrystal as seen by neutron diffraction.
Figure 4.9 The Nyquist plot for the i-phase electrodes at 50% DOD at the 1st discharge cycle: (a) after substitution of Ni for Ti or Ni, (b) after substitution of Pd for Ni, and (c) the equivalent circuit used for fitting of the data.
Figure 4.10 The charge transfer resistances for the i-phase electrodes as a function of DOD during the (a) 1st and (b) 3rd cycle.
Figure 4.11 The maximum discharge capacity as a function of a cycle number for the i-phase electrodes.
Figure 4.12 The grain boundary resistances for the i-phase electrodes as a function of DOD (1st cycle).
Figure 4.13 (a) The absorption pressure-composition isotherms measured at low hydrogen pressures, and (b) the estimated density of sites for the Ti₄₅Zr₃₈Ni₁₇ amorphous and i-phase powers produced by MA and subsequent annealing respectively [50].

Chapter 5

Figure 5.1 The experimental setup to study the process of gas release from the heated electrodes: (1) manometer, (2) intake chamber accumulating gas, (3) thermocouple, (4) retort, (5) tap, (6) muffle furnace, (7) metal thermal chamber, (8) rubber plug with a tube for gas extraction, (9) standard coil and (10) heater.
Figure 5.2 Changes of hydrogen evolution rate versus time for oxide-nickel and cadmium electrodes of the KSX-25 battery at 800 °C.
Figure 5.3 Oxide-nickel electrode of KSX-25 battery after thermal runaway.
Figure 5.4 Change in parameters of the KSX-25 battery during thermal runaway: I is the charging current of the battery, U is the voltage of the battery terminals, H is the hydrogen desorbed, T is the temperature of the battery positive terminal.

Chapter 6

Figure 6.1 Spatial arrangement of cellulose hemicellulose and lignin in the cell walls of lignocellulosic biomass.
Figure 6.2 A general schematic view of the structural components of the feather rachis.
Figure 6.3 Thermal pyrolysis of turkey feathers.
Figure 6.4 Thermogravimetric curve for palm kernal shell.
Figure 6.5 Thermogravimetric curve for chicken feathers crude.
Figure 6.6 ZnCl₂ effect in lignocellulosic materials.
Figure 6.7 Effect in the hydrogen storage: Time of irradiation.
Figure 6.8 Isosteric enthalpy of adsorption of various effective widths for H₂ at 77K.

Chapter 7

Figure 7.1 SEM image of as-produced turbostratic CNF. (Reproduced with permission of Elsevier)
Figure 7.2 CNFs SEM and TEM images before (a,b) and after (c,d) thermal treatment. (Reproduced with permission of Elsevier)
Figure 7.3 H₂ galvanostatic discharge measurements. (Reproduced with permission of Elsevier)
Figure 7.4 (a) Hydrogen adsorption/desorption cycles, (b) H₂ physisorption and chemisorption after cycles. (Reproduced with permission of Elsevier)
Figure 7.5 Sample with 7, 20 and 80 wt% Mn oxide. (Reproduced with permission of Elsevier)
Figure 7.6 SPMnO XRD comparison. (Reproduced with permission of Elsevier)
Figure 7.7 SPMnO15 wt% H₂ sorption. (Reproduced with permission of Elsevier)
Figure 7.8 SPMnO20 wt% H₂ sorption. (Reproduced with permission of Elsevier)
Figure 7.9 SPMnO78 wt% H₂ sorption. (Reproduced with permission of Elsevier)
Figure 7.10 (a) H₂ sorption test and (b) H₂ ads/des cycles. (Reproduced with permission of Elsevier)

Chapter 8

Figure 8.1 Penetration mechanism for nanocatalysts towards graphene sheets. (Reproduced with permission from [53]).
Figure 8.2 TEM micrographs of graphene prepared by microwave and thermal reduction method. (Reproduced with permission from [80])
Figure 8.3 (a) SEM and (b) XRD patterns of synthesized carbon nanomaterials. (Reproduced with permission from [90]).
Figure 8.4 (i) (a) TEM micrographs of GNS, inset is the SAED of GNS; (b) XPS Spectra; (c) C1s and O1s XPS spectra of GNS. (ii) XRD patterns of MGH₂+5GNS (a) before and (b) after cycling. (iii) TEM micrograph of MgH2+5GNs (a) before and (b) after cycling; HAADF STEM micrograph and elemental mapping (c) before and (d) after cycling. (Reproduced with permission from [117])
Figure 8.5 (i) TEM micrograph of CeF4@Gr; (ii) corresponding SAED pattern and (iii) XRD patterns of CeF4, CeF4@Gr, MgH2;CeF4@Gr, where δ represents peak of CeF4, & represents the peak of MgH2. (Reproduced with permission from [120])
Figure 8.6 (i) (a) XRD Patterns of Go, rGO, and Ni@rGO, (b) SEM image of Ni@rGO, (c) TEM image of Ni@rGO, (d) HRTEM image of Ni@rGO, inset in (c) magnified image of individual Ni nanoparticles and inset in (d) the SAED pattern of Ni@rGO nanocomposite. (ii) Raman spectra of Ni@rGO composite before and after cycling. (Reproduced with permission from [121])
Figure 8.7 (i) Illustration of the steps involved in the synthesis of Ni₂P@GNS. (ii) SEM, TEM and RTEM images of Ni₂P sample (a–c) and Ni2P@GNSs sample (d–f) respectively. (Reproduced with permission from [122])
Figure 8.8 (i) SEM image (a) and TEM image (b) of Ni-CeOx@GNSs. (ii) DSC profile of different samples used in the study. (Reproduced with permission from [123])

Chapter 9

Figure 9.1 Hydrogen density profile inside a slit-shaped pore at T = 300 K and P = 10 MPa, as a function of pore width. (Adapted with permission from [24]. Copyright © 2018 American Chemical Society)
Figure 9.2 Excess, absolute and total hydrogen uptake for the commercial carbon AX-21 at 77 K and in the pressure range 0–10 MPa.
Figure 9.3 Excess hydrogen adsorption on ACs reported by recent works at: (a) 77 K, and (b) 298 K. The labels indicate the corresponding references. (∙ 0.1 MPa, + 1.2 MPa, ▲ 2 MPa, ♦ 3 MPa, ○ 4 MPa, x10 MPa, ■ 20 MPa).
Figure 9.4 Different typologies of carbon nanomaterials investigated for hydrogen adsorption ((a) graphene; (b) fullerene; (c) single-walled carbon nanotube; (d) multiwalled carbon nanotube; (e) carbon nanofiber [platelet-type]).
Figure 9.5 Hydrogen storage capacities on graphene, CNTs and GNFs reported by recent works at: (a) 77 K, and (b) 298 K. The labels indicate both the typology of carbon (G=graphene, CNT=carbon nanotube, GNF=graphite nanofiber) and the corresponding references. For clarity, the data are grouped by ranges of pressures (∙ 0.1 MPa, ▲1–2 MPa, ◊ 3–5 MPa, + 6 MPa, O 7–10 MPa, ■ 12 MPa).
Figure 9.6 Schematic view of carbon materials preparation from MOFs. (Adapted from [153] with permission of Royal Society of Chemistry).
Figure 9.7 Hydrogen storage capacities of templated carbons and MOFs-derived carbons reported in recent works at: (a) 77 K, and (b) 298 K. The labels indicate the corresponding reference (∙ Zeolite-carbons 0.1 MPa, ∙ MOF-carbons 0.1 MPa, ▲ Zeolite-carbons 2 MPa, ▲ MOF-carbons 2 MPa, O MOF-carbons 4 MPa, ◊ Silica-carbons 7-8 MPa, ◊ Silica-carbons 2 MPa, X MOF-carbons 10 MPa).
Figure 9.8 SEM images of: (a) carbon nanorods, (b) carbon nanohorns and (c) carbon nanospheres. (Adapted from (a) [179], (b) [185] and (c) [186] with permission of Elsevier).
Figure 9.9 Hydrogen storage capacities on exotic carbons reported by recent works at: (a) 77 K, and (b) 298 K. The labels indicate both the typology of carbon (C=carbides; HYB=hybrid carbons; HCLP=hyper-cross-linked polymers-derived carbons; N=carbon nitrides; SPH=carbon nanospheres; AG=carbon aerogels) and the corresponding references (∙ 0.1 MPa, + 1 MPa, ▲2 MPa, ○ 6 MPa, × 10 MPa).

List of Tables

Chapter 1

Table 1.1 Comparison between the most common technologies for hydrogen storage in terms of volumetric capacity and technological drawbacks [15].
Table 1.2 Overview of solid hydrogen storage options.
Table 1.3 Values of the equilibrium pressures for the selected materials at the desired storage/release temperatures.

Chapter 3

Table 3.1 The van’t Hoff equations, enthalpy and entropy values for desorption reaction of different Mg-based nanostructured systems [47, 48, 50, 53, 54]. (Reproduced with permission from [21]).

Chapter 4

Table 4.1 Comparison of the hydrogen uptakes for the Ti-Zr-Ni-T amorphous alloys.
Table 4.2 Hydrogen concentrations achieved for the i-phase.

Chapter 5

Table 5.1 Hydrogen content in oxide-nickel and cadmium electrodes of the KSX-25 batteries with different service life.^a
Table 5.2 Oxide-nickel electrodes etching in sulfuric acid.
Table 5.3 Hydrogen content in metal-ceramic nickel matrixes of oxide-nickel electrodes of the KSX-25 batteries with different service life.^a
Table 5.4 DOE technical targets: onboard hydrogen storage systems.

Chapter 6

Table 6.1 Physical parameters of gasoline and hydrogen fuel.
Table 6.2 Maximum capacities of storage systems.
Table 6.3 Composition of agro-industrial and poultry residues.
Table 6.4 Proximate analysis precursors.
Table 6.5 Zn concentration effect on development of microporosity.
Table 6.6 Textural parameters of AC from palm kernel shells: Chemical activation (LiOH/microwaves).

Chapter 7

Table 7.1 Main results on H₂ uptake using waste and natural materials under different conditions.

Chapter 8

Table 8.1 DOE target value for HS materials.
Table 8.2 General properties of graphene.

Chapter 9

Table 9.1
Table 9.2
Table 9.3
Table 9.4
Table 9.5
Table 9.6
Table 9.7

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Library of Congress Cataloging-in-Publication Data

ISBN 978-1-119-45988-0

Preface

Our heavy dependence on fossil fuel resources, which is the cause of worldwide problems, has to be reduced in order to improve the environment and, in turn, the impact it has on human health. Hydrogen has drawn great attention as a nonpolluting energy carrier due to its diverse methods of production and storage. In the first volume of our series, Advances in Hydrogen Production and Storage, we thoroughly introduced hydrogen production technologies. However, since hydrogen storage is considered a key technology for stationary and portable power generation, especially for transportation, the second volume of the series is devoted to hydrogen storage technologies. This volume covers the novel technologies used to efficiently store and distribute hydrogen. Discussed are the underlying basics, as well as advanced details, of hydrogen storage technologies, which is highly beneficial for science and engineering students as well as experienced engineers and researchers. Additionally, the book was written to provide a comprehensive approach to the area of hydrogen storage for readers from a wide variety of backgrounds. The intent of the book is to satisfy the need for a broad coverage of the hydrogen storage technologies. Therefore, it was written by distinguished authors with knowledge and expertise in areas of hydrogen storage, whose contributions can benefit readers from universities and industries. The editors wish to thank the authors for their efforts in writing their chapters.

We have separated the book into two major parts: Chemical and Electrochemical Hydrogen Storage and Carbon-Based Materials for Hydrogen Storage. In Part I, hydrogen storage technologies within the context of chemical and electrochemical methods are clearly discussed in five chapters. Chapter 1 focuses on a multistage compression system based on metal hydrides for hydrogen storage. It also includes the development of a validated numerical analysis of a three-stage compression system. Chapter 2 discusses metal-N-H systems and their physicochemical properties for hydrogen storage. Mg-based nanomaterials with enhanced sorption kinetics for hydrogen storage are thoroughly introduced in Chapter 3. Next, in Chapter 4, evaluation of gaseous and electrochemical hydrogen storage performances of Ti-Zr-Ni alloys are analyzed. The final chapter of Part I, Chapter 5, deals with the electrochemical methods for hydrogenation/dehydrogenation of metal hydrides. The five chapters in Part II are devoted to carbon-based materials for hydrogen storage. Chapter 6 covers the activated carbon obtained from agro-industrial waste for use in hydrogen storage. Chapter 7 introduces the concept of hydrogen storage with carbonaceous materials. Next, Chapter 8 provides a fairly comprehensive introduction to hydrogen storage characteristics of graphene addition in hydrogen storage materials. Part II concludes with a discussion in Chapter 9 of the crucial features of hydrogen adsorption of nanotextured carbon-based materials.

Series Editors
Mehmet Sankır, PhD. and Nurdan Demirci Sankır, PhD.
Department of Materials Science and Nanotechnology Engineering,
TOBB University of Economics and Technology

Hydrogen Storage Technologies

Preface

Part I
CHEMICAL AND ELECTROCHEMICAL HYDROGEN STORAGE