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Post-combustion Carbon Dioxide Capture Materials
Preface
Contents
Chapter 1 - Carbon-based CO2 Adsorbents
1.1 Introduction
1.2 Porous Carbons
1.2.1 Chemical Activation
1.2.1.1 KOH as an Activating Agent
1.2.1.2 Other Chemicals as Activating Agents
1.2.2 Physical Activation
1.2.2.1 CO2 as an Activating Agent
1.2.2.2 Steam as an Activating Agent
1.2.3 Metal Ion Activation
1.2.4 Templating Method
1.2.4.1 Porous Silica as a Hard Template
1.2.4.2 Zeolite as a Hard Template
1.2.4.3 Porous Organic Frameworks as Self-templates
1.2.4.4 Carbide Lattices as Self-templates
1.2.4.5 Triblock Copolymer as a Soft Template
1.2.5 Combined Method of Templating and Activation
1.2.5.1 Two-step Process
1.2.5.2 One-step Process
1.3 Graphene-based Porous Materials
1.3.1 Graphene-based Adsorbents by Chemical Activation
1.3.2 Graphene-based Adsorbents by Physical Activation
1.3.3 Graphene-based Adsorbents by Other Techniques
1.4 Carbon Nanotubes
1.5 Carbon-based Hybrid Adsorbents
1.5.1 Carbon-Organic Hybrid Adsorbents
1.5.2 Carbon-Inorganic Hybrid Adsorbents
1.6 Effect of Carbon Structure on CO2 Adsorption
1.6.1 Pore Size Effect
1.6.1.1 Analysis of Porosity
1.6.1.2 Micropore Filling Mechanism of CO2 Adsorption
1.6.1.3 Pore Size Effect at Different Sorption Pressures
1.6.1.4 Pore Size Effect at Different Adsorption Temperatures
1.6.2 Surface Chemistry Effect on CO2 Adsorption
1.6.2.1 Effect of Nitrogen Doping
1.6.2.2 Effect of Other Heteroatom-doping
1.7 Summary and Outlook
Acknowledgements
References
Chapter 2 - Zeolite and Silica-based CO2 Adsorbents
2.1 Introduction
2.2 (Alkali) Silicates
2.2.1 Silicate Amine-based Adsorbents
2.2.1.1 CO2 Absorption in Aqueous Alkanolamine Solutions.
2.2.2 Synthesis of Amine-Silica Adsorbents
2.2.2.1 Impregnation Method
2.2.2.2 Post-synthesis Grafting
2.2.2.3 Direct Condensation
2.2.3 CO2 Capture by Amine-Silica-based Adsorbents
2.2.3.1 Amine Impregnated on Silica
2.2.3.1.1 Effect of Temperature.As demonstrated by Xu et al.,48,54 a decrease in temperature from 75 °C to 25 °C causes a dramatic decreas...
2.2.3.1.2 Effect of CO2 Partial Pressure.CO2 adsorption capacity is also influenced by the partial pressure of CO2 in the gas feed. Regard...
2.2.3.1.3 Effect of Water.Xu et al. also studied the influence of water on CO2 adsorption capacity using PEI (50 wt%)/MCM-41. The authors ...
2.2.3.1.4 Effect of Percentage of Impregnation.According to the work of Xu et al.,48 the amount of amine (PEI) deposited on MCM-41 mesopor...
2.2.3.1.5 Effect of the Support Structure.There is also a correlation between the CO2 adsorption capacities of amines impregnated on diffe...
2.2.3.1.6 Effect of the Mesopores Structuring Agent.CO2 capture was tested with tetraethylenepentamine (TEPA) impregnated on MCM-41 and SB...
2.2.3.2 Amine Grafted on Silica
2.2.3.2.1 Effect of CO2 Partial Pressure.In the case of APTES (3-aminopropyltriethoxysilane)-type aminosilanes for grafting on MCM-48-type...
2.2.3.2.2 Effect of Water.Similar to the results obtained in the case of amines impregnated on silica, the presence of water during CO2 ad...
2.2.3.2.3 Effect of the Support.As shown in Table 2.5, the important influence of the support on CO2 adsorption capacities can also be dem...
2.2.3.2.4 Effect of Organosilane Type.Hiyoshi et al.74 have shown that the nature of the aminosilanes used in the synthesis of amine-graft...
2.3 Alkali Silicate-based Sorbents
2.3.1 Calcium Silicate (CaSiO3)
2.3.2 Sodium Metasilicate (Na2SiO3).
2.3.3 Lithium Orthosilicate (Li4SiO4) and Other Lithium Silicates
2.3.3.1 Li4SiO4
2.3.3.1.1 Influence of the Operating Conditions.Theoretically, Li4SiO4 can adsorb up to 0.367 g of CO2 per gram of Li4SiO4 (∼8.34 mmol CO2...
2.3.3.1.2 Improvement of the Absorption Performance of Li4SiO4.The improvement of the CO2 adsorption performance of Li4SiO4 requires modif...
2.3.3.2 Other Lithium Silicates
2.4 Clays-based Adsorbents
2.4.1 Phyllosilicates
2.4.2 Clays for CO2 Capture
2.4.2.1 Smectite
2.4.2.2 Montmorillonite
2.4.2.3 Bentonite
2.4.2.4 Saponite
2.4.2.5 Hectorite
2.4.2.6 Laponite
2.4.2.7 Sepiolite
2.5 Mineral Silicates for Carbonation
2.5.1 Mineral Carbonation
2.5.2 Silicates as Natural Minerals for Carbonation
2.5.3 Mineral Pre-treatments
2.5.4 Thermodynamics of Mineral Carbonation
2.5.5 Processes for Mineral Carbonation
2.5.5.1 Mineral Carbonation Ex Situ
2.5.5.1.1 Mineral Carbonation 'Ex-Situ': Aqueous Carbonation.Mineral carbonation in an aqueous medium occurs according to three important ...
2.5.5.1.2 Mineral Carbonation 'Ex-Situ': Gas-Solid Route.The gas-solid method is the easiest approach towards mineral carbonation. The mag...
2.5.5.2 Mineral Carbonation In Situ
2.5.5.3 Other Mineral Carbonation Routes
2.6 Zeolites and Related Materials
2.6.1 Foreword
2.6.2 Peculiarities of Zeolites
2.6.3 CO2 Sorption in Zeolites: Main Issues
2.6.3.1 Preamble
2.6.3.2 Key Parameters and Mechanistic Considerations
2.6.3.3 Zeolite Acid-Base Properties: How Do They Impact the Sorption Features
2.6.3.4 CO2 Sorption in Alkali-exchanged Zeolites: the 'Li' Paradox
2.6.4 Miscellaneous Parameters
2.6.4.1 Impact of the Presence of Water
2.6.4.2 Impact of Sorbent Particle Size and Morphology
2.6.4.3 Selectivity
2.6.4.4 Possibility of Dual-site Adsorption.
2.6.5 Zeolite-like Materials as Precursors to Design Performant Li-silicate Sorbents: How to Bridge the Gap Between High Affinity...
2.7 Outline: Towards an Efficient Chemical Transformation of CO2 into Fuels
2.7.1 Potential Chemical Valorization of Carbon Dioxide
2.7.2 Synthesis of Energy Carriers
2.7.3 Future Prospects
2.8 Conclusion
Acknowledgements
References
Chapter 3 - Metal-Organic Framework (MOF)-based CO2 Adsorbents
3.1 Introduction
3.2 CO2 Adsorption by MOFs With Open Metal Sites
3.3 CO2 Adsorption by Amine-functionalized MOFs
3.3.1 In situ Synthesized Amine-functionalized MOFs
3.3.1.1 Amine-functionalized MOFs With a Structural Motif
3.3.1.2 Amine-functionalized MOFs Without a Structural Motif
3.3.2 Post-synthesis Amine-functionalized MOFs
3.3.2.1 Post-synthesis Functionalization of MOFs via Covalent Bonding
3.3.2.2 Post-synthetic Functionalization of MOFs via Coordination Bonding
3.3.3 Physical Incorporation of Amines into Unmodified MOFs
3.4 CO2 Adsorption by Mixed-ligand-based MOFs
3.4.1 Pillared-layer Mixed-ligand MOFs (PL-MOFs)
3.4.2 Cluster-based Mixed-ligand MOFs
3.5 CO2 Adsorption by Flexible Ligand-based MOFs (FL-MOFs)
3.5.1 Increasing the Free Pore Volume in FL-MOFs
3.5.2 Maintaining Porosity in FL-MOFs After the Removal of the Solvent
3.5.3 Increasing the Gas Binding Affinity in FL-MOFs
3.6 CO2 Adsorption by MOFs with Interpenetration
3.7 CO2 Adsorption by Zeolitic Imidazolate Frameworks (ZIFs)
3.8 CO2 Adsorption by Composite MOFs
3.8.1 MOF-Carbon Composites
3.8.2 Composites of MOFs with Other Support Materials
3.9 CO2 Adsorption by MOFs under Humid Conditions
3.10 Conclusion and Perspectives
Acknowledgements
References
Chapter 4 - Alkali-metal-carbonate-based CO2 Adsorbents
4.1 Introduction.
4.1.1 Sodium Carbonate (Na2CO3)
4.1.2 Potassium Carbonate (K2CO3)
4.2 CO2 Capture of Na2CO3 and K2CO3 Under Moist Conditions
4.2.1 CO2 Capture of Na2CO3 Under Moist Conditions
4.2.1.1 Experimental
4.2.1.1.1 Sample Preparation.Analytical reagent grade sodium bicarbonate (NaHCO3) was used during experiments of decomposition of NaHCO3 a...
4.2.1.1.2 Bicarbonate Formation Measurements.The obtained samples were processed with the TG-DTA apparatus using a gas composition of CO2 ...
4.2.1.1.3 Crystal Structure and Morphology Measurements.The crystal structures of the products after CO2 occlusion reactions with 10, 20, ...
4.2.1.2 Results and Discussion
4.2.1.2.1 CO2 Capture of Na2CO3 at Different Temperatures.The decomposition of NaHCO3 occurred with TG-DTA under pure N2 gas via the rever...
4.2.1.2.2 CO2 Capture of Na2CO3 Under Various CO2 Concentrations.The dependence of the sorptivity of Na2CO3 on CO2 concentration was shown...
4.2.1.2.3 CO2 Capture of Na2CO3 Under Various H2O Concentrations.As mentioned in Section 4.2.1.2.2, the bicarbonate formation of Na2CO3 pr...
4.2.1.3 Conclusions
4.2.2 Capture of CO2 of K2CO3 Under Moist Conditions
4.2.2.1 Experimental
4.2.2.1.1 Sample Preparation.KHCO3 (99.5% chemical purity) was used during the experiments of decomposition of KHCO3 and bicarbonate forma...
4.2.2.1.2 Bicarbonate Formation Measurements.K2CO3 bicarbonate formation was measured with the TG-DTA apparatus, as shown in Section 4.2.1...
4.2.2.1.3 Crystal Structure and Morphology Measurements.The crystal structures of the products after reaction times of 1, 5, 20, 40, 60, a...
4.2.2.2 Results and Discussion
4.2.2.2.1 Bicarbonate Formation of K2CO3.KHCO3 decomposed to K2CO3, CO2, and H2O as per the reverse of reaction (4.15). This was confirmed.
4.2.2.2.2 Exothermic Properties and Temperature Variation.Since the process of bicarbonate formation of K2CO3 leads to a temperature eleva.
Post-combustion Carbon Dioxide Capture Materials
Preface
Contents
Chapter 1 - Carbon-based CO2 Adsorbents
1.1 Introduction
1.2 Porous Carbons
1.2.1 Chemical Activation
1.2.1.1 KOH as an Activating Agent
1.2.1.2 Other Chemicals as Activating Agents
1.2.2 Physical Activation
1.2.2.1 CO2 as an Activating Agent
1.2.2.2 Steam as an Activating Agent
1.2.3 Metal Ion Activation
1.2.4 Templating Method
1.2.4.1 Porous Silica as a Hard Template
1.2.4.2 Zeolite as a Hard Template
1.2.4.3 Porous Organic Frameworks as Self-templates
1.2.4.4 Carbide Lattices as Self-templates
1.2.4.5 Triblock Copolymer as a Soft Template
1.2.5 Combined Method of Templating and Activation
1.2.5.1 Two-step Process
1.2.5.2 One-step Process
1.3 Graphene-based Porous Materials
1.3.1 Graphene-based Adsorbents by Chemical Activation
1.3.2 Graphene-based Adsorbents by Physical Activation
1.3.3 Graphene-based Adsorbents by Other Techniques
1.4 Carbon Nanotubes
1.5 Carbon-based Hybrid Adsorbents
1.5.1 Carbon-Organic Hybrid Adsorbents
1.5.2 Carbon-Inorganic Hybrid Adsorbents
1.6 Effect of Carbon Structure on CO2 Adsorption
1.6.1 Pore Size Effect
1.6.1.1 Analysis of Porosity
1.6.1.2 Micropore Filling Mechanism of CO2 Adsorption
1.6.1.3 Pore Size Effect at Different Sorption Pressures
1.6.1.4 Pore Size Effect at Different Adsorption Temperatures
1.6.2 Surface Chemistry Effect on CO2 Adsorption
1.6.2.1 Effect of Nitrogen Doping
1.6.2.2 Effect of Other Heteroatom-doping
1.7 Summary and Outlook
Acknowledgements
References
Chapter 2 - Zeolite and Silica-based CO2 Adsorbents
2.1 Introduction
2.2 (Alkali) Silicates
2.2.1 Silicate Amine-based Adsorbents
2.2.1.1 CO2 Absorption in Aqueous Alkanolamine Solutions.
2.2.2 Synthesis of Amine-Silica Adsorbents
2.2.2.1 Impregnation Method
2.2.2.2 Post-synthesis Grafting
2.2.2.3 Direct Condensation
2.2.3 CO2 Capture by Amine-Silica-based Adsorbents
2.2.3.1 Amine Impregnated on Silica
2.2.3.1.1 Effect of Temperature.As demonstrated by Xu et al.,48,54 a decrease in temperature from 75 °C to 25 °C causes a dramatic decreas...
2.2.3.1.2 Effect of CO2 Partial Pressure.CO2 adsorption capacity is also influenced by the partial pressure of CO2 in the gas feed. Regard...
2.2.3.1.3 Effect of Water.Xu et al. also studied the influence of water on CO2 adsorption capacity using PEI (50 wt%)/MCM-41. The authors ...
2.2.3.1.4 Effect of Percentage of Impregnation.According to the work of Xu et al.,48 the amount of amine (PEI) deposited on MCM-41 mesopor...
2.2.3.1.5 Effect of the Support Structure.There is also a correlation between the CO2 adsorption capacities of amines impregnated on diffe...
2.2.3.1.6 Effect of the Mesopores Structuring Agent.CO2 capture was tested with tetraethylenepentamine (TEPA) impregnated on MCM-41 and SB...
2.2.3.2 Amine Grafted on Silica
2.2.3.2.1 Effect of CO2 Partial Pressure.In the case of APTES (3-aminopropyltriethoxysilane)-type aminosilanes for grafting on MCM-48-type...
2.2.3.2.2 Effect of Water.Similar to the results obtained in the case of amines impregnated on silica, the presence of water during CO2 ad...
2.2.3.2.3 Effect of the Support.As shown in Table 2.5, the important influence of the support on CO2 adsorption capacities can also be dem...
2.2.3.2.4 Effect of Organosilane Type.Hiyoshi et al.74 have shown that the nature of the aminosilanes used in the synthesis of amine-graft...
2.3 Alkali Silicate-based Sorbents
2.3.1 Calcium Silicate (CaSiO3)
2.3.2 Sodium Metasilicate (Na2SiO3).
2.3.3 Lithium Orthosilicate (Li4SiO4) and Other Lithium Silicates
2.3.3.1 Li4SiO4
2.3.3.1.1 Influence of the Operating Conditions.Theoretically, Li4SiO4 can adsorb up to 0.367 g of CO2 per gram of Li4SiO4 (∼8.34 mmol CO2...
2.3.3.1.2 Improvement of the Absorption Performance of Li4SiO4.The improvement of the CO2 adsorption performance of Li4SiO4 requires modif...
2.3.3.2 Other Lithium Silicates
2.4 Clays-based Adsorbents
2.4.1 Phyllosilicates
2.4.2 Clays for CO2 Capture
2.4.2.1 Smectite
2.4.2.2 Montmorillonite
2.4.2.3 Bentonite
2.4.2.4 Saponite
2.4.2.5 Hectorite
2.4.2.6 Laponite
2.4.2.7 Sepiolite
2.5 Mineral Silicates for Carbonation
2.5.1 Mineral Carbonation
2.5.2 Silicates as Natural Minerals for Carbonation
2.5.3 Mineral Pre-treatments
2.5.4 Thermodynamics of Mineral Carbonation
2.5.5 Processes for Mineral Carbonation
2.5.5.1 Mineral Carbonation Ex Situ
2.5.5.1.1 Mineral Carbonation 'Ex-Situ': Aqueous Carbonation.Mineral carbonation in an aqueous medium occurs according to three important ...
2.5.5.1.2 Mineral Carbonation 'Ex-Situ': Gas-Solid Route.The gas-solid method is the easiest approach towards mineral carbonation. The mag...
2.5.5.2 Mineral Carbonation In Situ
2.5.5.3 Other Mineral Carbonation Routes
2.6 Zeolites and Related Materials
2.6.1 Foreword
2.6.2 Peculiarities of Zeolites
2.6.3 CO2 Sorption in Zeolites: Main Issues
2.6.3.1 Preamble
2.6.3.2 Key Parameters and Mechanistic Considerations
2.6.3.3 Zeolite Acid-Base Properties: How Do They Impact the Sorption Features
2.6.3.4 CO2 Sorption in Alkali-exchanged Zeolites: the 'Li' Paradox
2.6.4 Miscellaneous Parameters
2.6.4.1 Impact of the Presence of Water
2.6.4.2 Impact of Sorbent Particle Size and Morphology
2.6.4.3 Selectivity
2.6.4.4 Possibility of Dual-site Adsorption.
2.6.5 Zeolite-like Materials as Precursors to Design Performant Li-silicate Sorbents: How to Bridge the Gap Between High Affinity...
2.7 Outline: Towards an Efficient Chemical Transformation of CO2 into Fuels
2.7.1 Potential Chemical Valorization of Carbon Dioxide
2.7.2 Synthesis of Energy Carriers
2.7.3 Future Prospects
2.8 Conclusion
Acknowledgements
References
Chapter 3 - Metal-Organic Framework (MOF)-based CO2 Adsorbents
3.1 Introduction
3.2 CO2 Adsorption by MOFs With Open Metal Sites
3.3 CO2 Adsorption by Amine-functionalized MOFs
3.3.1 In situ Synthesized Amine-functionalized MOFs
3.3.1.1 Amine-functionalized MOFs With a Structural Motif
3.3.1.2 Amine-functionalized MOFs Without a Structural Motif
3.3.2 Post-synthesis Amine-functionalized MOFs
3.3.2.1 Post-synthesis Functionalization of MOFs via Covalent Bonding
3.3.2.2 Post-synthetic Functionalization of MOFs via Coordination Bonding
3.3.3 Physical Incorporation of Amines into Unmodified MOFs
3.4 CO2 Adsorption by Mixed-ligand-based MOFs
3.4.1 Pillared-layer Mixed-ligand MOFs (PL-MOFs)
3.4.2 Cluster-based Mixed-ligand MOFs
3.5 CO2 Adsorption by Flexible Ligand-based MOFs (FL-MOFs)
3.5.1 Increasing the Free Pore Volume in FL-MOFs
3.5.2 Maintaining Porosity in FL-MOFs After the Removal of the Solvent
3.5.3 Increasing the Gas Binding Affinity in FL-MOFs
3.6 CO2 Adsorption by MOFs with Interpenetration
3.7 CO2 Adsorption by Zeolitic Imidazolate Frameworks (ZIFs)
3.8 CO2 Adsorption by Composite MOFs
3.8.1 MOF-Carbon Composites
3.8.2 Composites of MOFs with Other Support Materials
3.9 CO2 Adsorption by MOFs under Humid Conditions
3.10 Conclusion and Perspectives
Acknowledgements
References
Chapter 4 - Alkali-metal-carbonate-based CO2 Adsorbents
4.1 Introduction.
4.1.1 Sodium Carbonate (Na2CO3)
4.1.2 Potassium Carbonate (K2CO3)
4.2 CO2 Capture of Na2CO3 and K2CO3 Under Moist Conditions
4.2.1 CO2 Capture of Na2CO3 Under Moist Conditions
4.2.1.1 Experimental
4.2.1.1.1 Sample Preparation.Analytical reagent grade sodium bicarbonate (NaHCO3) was used during experiments of decomposition of NaHCO3 a...
4.2.1.1.2 Bicarbonate Formation Measurements.The obtained samples were processed with the TG-DTA apparatus using a gas composition of CO2 ...
4.2.1.1.3 Crystal Structure and Morphology Measurements.The crystal structures of the products after CO2 occlusion reactions with 10, 20, ...
4.2.1.2 Results and Discussion
4.2.1.2.1 CO2 Capture of Na2CO3 at Different Temperatures.The decomposition of NaHCO3 occurred with TG-DTA under pure N2 gas via the rever...
4.2.1.2.2 CO2 Capture of Na2CO3 Under Various CO2 Concentrations.The dependence of the sorptivity of Na2CO3 on CO2 concentration was shown...
4.2.1.2.3 CO2 Capture of Na2CO3 Under Various H2O Concentrations.As mentioned in Section 4.2.1.2.2, the bicarbonate formation of Na2CO3 pr...
4.2.1.3 Conclusions
4.2.2 Capture of CO2 of K2CO3 Under Moist Conditions
4.2.2.1 Experimental
4.2.2.1.1 Sample Preparation.KHCO3 (99.5% chemical purity) was used during the experiments of decomposition of KHCO3 and bicarbonate forma...
4.2.2.1.2 Bicarbonate Formation Measurements.K2CO3 bicarbonate formation was measured with the TG-DTA apparatus, as shown in Section 4.2.1...
4.2.2.1.3 Crystal Structure and Morphology Measurements.The crystal structures of the products after reaction times of 1, 5, 20, 40, 60, a...
4.2.2.2 Results and Discussion
4.2.2.2.1 Bicarbonate Formation of K2CO3.KHCO3 decomposed to K2CO3, CO2, and H2O as per the reverse of reaction (4.15). This was confirmed.
4.2.2.2.2 Exothermic Properties and Temperature Variation.Since the process of bicarbonate formation of K2CO3 leads to a temperature eleva.