Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies

Topic Information

Dear Colleagues,

The energetic transition requires the replacement of fossil fuels with renewable energy sources, along with the development of innovative decarbonation technologies and the establishment of a circular economy model. Developing and deploying carbon capture (from fixed sources) or removal (from the atmosphere) technologies using innovative CO₂ capture materials and CO₂ valorization in short- or long-lived biofuels or green products are essential to reach carbon neutrality or negative emissions targets. This Special Topic, “Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies”, will address topics related, but not limited to:

• Advances in CO₂ sorbent properties for carbon removal (e.g., direct air capture, mineralization, biochar) and capture (e.g., post-combustion and pre-combustion conditions);
• Enhancement of natural and synthetic sorbent materials properties for CO₂ uptake;
• Stability, activity, and regeneration of sorbents under different technological applications at low, medium, or high temperatures;
• Dual-function materials for CO₂ capture and conversion;
• Development of catalysts for CO₂ conversion to biofuels and green products;
• Thermal-, photo-, electro-, bio- and plasma catalysis applications in CO₂ conversion;
• Carbon capture from power plants and industrial sectors and carbon removal from the air—novel technologies, integrated concepts, and methodologies;
• Conversion of CO₂ into fuels and chemicals through biological, thermal, electrochemical, and photochemical processes. In this topic, original papers or reviews are welcome.

Dr. Paula Teixeira
Dr. María Pilar Lisbona
Dr. Carmen Bacariza
Topic Editors

Keywords

Participating Journals

Journal Name	Impact Factor	CiteScore	Launched Year	First Decision (median)	APC
Catalysts catalysts	3.8	6.8	2011	12.9 Days	CHF 2200	Submit
Clean Technologies cleantechnol	4.0	6.1	2019	30 Days	CHF 1600	Submit
Energies energies	3.0	6.2	2008	17.5 Days	CHF 2600	Submit
Gases gases	-	-	2021	23.4 Days	CHF 1000	Submit
Sustainability sustainability	3.3	6.8	2009	20 Days	CHF 2400	Submit

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Published Papers (5 papers)

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All Catalysts Clean Technol. Energies Gases Sustainability

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18 pages, 5073 KiB  

Open AccessArticle

Metal Oxalates as a CO₂ Solid State Reservoir: The Carbon Capture Reaction

by Linda Pastero, Vittorio Barella, Enrico Allais, Marco Pazzi, Fabrizio Sordello, Quentin Wehrung and Alessandro Pavese

Clean Technol. 2024, 6(4), 1389-1406; https://doi.org/10.3390/cleantechnol6040066 - 14 Oct 2024

Viewed by 745

Abstract

To maintain the carbon dioxide concentration below the no-return threshold for climate change, we must consider the reduction in anthropic emissions coupled to carbon capture methods applied in synergy. In our recent papers, we proposed a green and reliable method for carbon mineralization [...] Read more.

To maintain the carbon dioxide concentration below the no-return threshold for climate change, we must consider the reduction in anthropic emissions coupled to carbon capture methods applied in synergy. In our recent papers, we proposed a green and reliable method for carbon mineralization using ascorbic acid aqueous solution as the reducing agent for carbon (IV) to carbon (III), thus obtaining oxalic acid exploiting green reagents. Oxalic acid is made to mineralize as calcium (as the model cation) oxalate. Oxalates are solid-state reservoirs suitable for long-term carbon storage or carbon feedstock for manufacturing applications. The carbon mineralization reaction is a double-step process (carbon reduction and oxalate precipitation), and the carbon capture efficiency is invariably represented by a double-slope curve we formerly explained as a decrease in the reducing effectiveness of ascorbic acid during reaction. In the present paper, we demonstrated that the reaction proceeds via a “pure CO₂-capture” stage in which ascorbic acid oxidizes into dehydroascorbic acid and carbon (IV) reduces to carbon (III) and a “mixed” stage in which the redox reaction competes with the degradation of ascorbic acid in producing oxalic acid. Despite the irreversibility of the reduction reaction, that was demonstrated in abiotic conditions, the analysis of costs according to the market price of the reagents endorses the application of the method. Full article

(This article belongs to the Topic Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies)

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Figure 1
<p>General trend in the carbon capture curves as determined during capture experiments (B-setup, <a href="#app1-cleantechnol-06-00066" class="html-app">Figure S1 in the Supplementary Materials</a>). The double slope was roughly associated with the kinetics of the redox reaction, i.e., fast at the initial stages when H₂A-reducing power was high and then slowed down by the degradation of H₂A [<a href="#B55-cleantechnol-06-00066" class="html-bibr">55</a>,<a href="#B57-cleantechnol-06-00066" class="html-bibr">57</a>].</p> Full article ">Figure 2
<p>Trend of d¹³C measured in the mineralizing system (solid diamond-, liquid circles-, and gas squares phases) vs. time. No handling in the second run allowed a better quality of data, highlighting the first-order decay of d¹³C in the dissolved CO₂. The points related to the d¹³C of the CO₂ from the canister and H₂A (squares) are reported to be compared with the trend of the dissolved carbon. A single value for the solid fraction is reported (diamond) because of the experimental procedure intended to limit the artifacts’ appearances in the measurements as explained in the text.</p> Full article ">Figure 3
<p>The general carbon capture curve via carbon mineralization into oxalates explained: in the light-grey area, the efficient pure carbon capture process during the “low-oxidation stage” of the H₂A as determined by CV and LC measurements; in the dark-grey area, the mixed process of capture and H₂A degradation occurring when the H₂A reaches higher degree of oxidation (30–40% from CV measurements) and the H₂A degradation cascade is running.</p> Full article ">Figure 4
<p>Calcium oxalate is the only product of the mineralization reaction. (<b>a</b>) Calcium oxalate crystals from a B-setup carbon mineralization experiment; (<b>b</b>) XRPD pattern of the precipitate (red bars: weddellite pattern from Tazzoli and Domeneghetti, 1980 [<a href="#B105-cleantechnol-06-00066" class="html-bibr">105</a>]).</p> Full article ">

21 pages, 550 KiB  

Open AccessReview

Carbon Market for Climate Projects in Russia: An Overview of Nature-Based and Technological Carbon Offsets

by Tatiana Nevzorova

Gases 2024, 4(3), 153-173; https://doi.org/10.3390/gases4030009 - 8 Jul 2024

Viewed by 1446

Abstract

Climate projects can become one of the key tools for decarbonization in Russia. They have powerful potential in terms of solving the problems of reducing emissions and increasing the absorption of greenhouse gases, as well as monetization potential for businesses. Despite the geopolitical [...] Read more.

Climate projects can become one of the key tools for decarbonization in Russia. They have powerful potential in terms of solving the problems of reducing emissions and increasing the absorption of greenhouse gases, as well as monetization potential for businesses. Despite the geopolitical crisis and sanctions imposed on Russia, certain opportunities for implementing climate projects have remained accessible. This study aims to provide a comprehensive analysis of the current status, including the regulations and approved methodologies, prospects, and challenges for climate projects in the carbon market in Russia. It also offers an overview of international carbon market mechanisms and analyses the advantages and disadvantages of the nature-based and technological solutions of climate projects for carbon sequestration. This, in turn, can facilitate the realization of future strategies for realizing the bigger potential of Russian climate projects in the domestic and international carbon markets. This research also provides up-to-date data on the current situation of the carbon market in Russia. Full article

(This article belongs to the Topic Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies)

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<p>Accounting methods and tools under Federal Law No. 34.</p> Full article ">

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Supplementary File 1 (ZIP, 998 KiB)

16 pages, 7283 KiB  

Open AccessArticle

Investigation and Comparison of Catalytic Methods to Produce Green CO₂-Containing Monomers for Polycarbonates

by Daniel Christian Brüggemann, Philipp Harry Isbrücker, Dzenna Zukova, Franz Robert Otto Heinrich Schröter, Yen Hoang Le and Reinhard Schomäcker

Catalysts 2024, 14(6), 362; https://doi.org/10.3390/catal14060362 - 1 Jun 2024

Viewed by 1170

Abstract

The preparation of CO₂-containing polymers with improved degradation properties is still very challenging. An elegant method for preparing these polymers is to use CO₂-containing monomers in ring-opening polymerizations (ROP) which are particularly gentle and energy-saving methods. However, cyclic carbonates [...] Read more.

The preparation of CO₂-containing polymers with improved degradation properties is still very challenging. An elegant method for preparing these polymers is to use CO₂-containing monomers in ring-opening polymerizations (ROP) which are particularly gentle and energy-saving methods. However, cyclic carbonates are required for this which are not readily available. This paper therefore aims to present the optimization and comparison of two synthesis methods to obtain cyclic carbonates for ROP. Within this work, cyclic styrene carbonate was synthesized from readily available raw materials by using a Jacobsen catalyst for the reaction of styrene oxide and carbon dioxide or an organocatalyst for the transesterification of methyl carbonate with 1-phenyl-1,2-ethanediol. The latter performed with 100% selectivity to the desired styrene carbonate, which was succesfully tested in ROP, producing an amorphous thermoplastic polymer with a T_G of 185 °C. Full article

(This article belongs to the Topic Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies)

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Graphical abstract

Graphical abstract
Full article ">Figure 1
<p>Large-scale synthesis of cyclic ethylene carbonate (cEC) via the Omega process.</p> Full article ">Figure 2
<p>Possible production routes from CO₂ to the CO₂-containing polymer.</p> Full article ">Figure 3
<p>Structure of the Jacobsen catalyst (<b>M</b> = Mn or Co).</p> Full article ">Figure 4
<p>Identification of the polymeric (blue), linear (red), and cyclic (black) carbonate band through (<b>a</b>) ATR-IR spectra and (<b>b</b>) HPLC-ESI-DAD measurements.</p> Full article ">Figure 5
<p>(<b>a</b>) ATR-IR spectra of the basic experiment (120 °C, 15 bar), (<b>b</b>) resolution change to the relevant peak for the standard reaction, (<b>c</b>) ATR-IR spectra for experiment with lower concentration of TBAB, (<b>d</b>) ATR-IR spectra for experiment with higher concentration of TBAB.</p> Full article ">Figure 6
<p>ATR-IR spectrum of the reaction at 3 eq. DMC and 65 °C reaction temperature.</p> Full article ">Figure 7
<p>¹H-NMR spectrum styrene carbonate reference substance purchased from Sigma Aldrich (Saint Louis, MO, USA).</p> Full article ">Figure 8
<p>¹H-NMR spectrum of styrene carbonate of the reaction at 3 eq. DMC and 65 °C reaction temperature.</p> Full article ">Figure 9
<p>(<b>a</b>) HPLC-DAD chromatogram of the starting material phenylethane-1,2-diol. (<b>b</b>) HPLC-DAD chromatogram of the styrene carbonate reference substance, obtained from Sigma Aldrich. (<b>c</b>) HPLC-DAD chromatogram of the styrene carbonate produced from the organocatalytic production of styrene carbonate.</p> Full article ">Figure 10
<p>(<b>a</b>) Recording of the probe ATR-IR spectrum during the formation of cSC with subsequent ROP. (<b>b</b>) Chronological view with focus on the changing bands of the ATR IR spectrum during the formation of cyclic styrene carbonate with subsequent ROP.</p> Full article ">Figure 11
<p>DSC spectrum of the products of the ROP of styrene carbonate.</p> Full article ">Figure 12
<p>Reaction setup for the high-pressure homogeneous synthesis of styrene carbonate.</p> Full article ">Figure 13
<p>Synthesis of cyclic styrene carbonate by reaction of phenyl ethanediol with dimethyl carbonate.</p> Full article ">Figure 14
<p>Experimental setup for the organocatalytic synthesis of styrene carbonate.</p> Full article ">Figure 15
<p>Synthesis of Polystyrene carbonate by ROP of styrene carbonate with phenylacetic acid.</p> Full article ">

16 pages, 3156 KiB  

Open AccessArticle

Carbon Dioxide Capture under Low-Pressure Low-Temperature Conditions Using Shaped Recycled Fly Ash Particles

by Sherif Fakher, Abdelaziz Khlaifat and Abdullah Hassanien

Gases 2024, 4(2), 117-132; https://doi.org/10.3390/gases4020007 - 23 May 2024

Cited by 3 | Viewed by 2013

Abstract

Carbon-capture technologies are extremely abundant, yet they have not been applied extensively worldwide due to their high cost and technological complexities. This research studies the ability of polymerized fly ash to capture carbon dioxide (CO₂) under low-pressure and low-temperature conditions via [...] Read more.

Carbon-capture technologies are extremely abundant, yet they have not been applied extensively worldwide due to their high cost and technological complexities. This research studies the ability of polymerized fly ash to capture carbon dioxide (CO₂) under low-pressure and low-temperature conditions via physical adsorption. The research also studies the ability to desorb CO₂ due to the high demand for CO₂ in different industries. The adsorption–desorption hysteresis was measured using infrared-sensor detection apparatus. The impact of the CO₂ injection rate for adsorption, helium injection rate for desorption, temperature, and fly ash contact surface area on the adsorption–desorption hysteresis was investigated. The results showed that change in the CO₂ injection rate had little impact on the variation in the adsorption capacity; for all CO₂ rate experiments, the adsorption reached more than 90% of the total available adsorption sites. Increasing the temperature caused the polymerized fly ash to expand, thus increasing the available adsorption sites, thus increasing the overall adsorption volume. At low helium rates, desorption was extremely lengthy which resulted in a delayed hysteresis response. This is not favorable since it has a negative impact on the adsorption–desorption cyclic rate. Based on the results, the polymerized fly ash proved to have a high CO₂ capture capability and thus can be applied for carbon-capture applications. Full article

(This article belongs to the Topic Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies)

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Figure 1
<p>CO₂ adsorption experimental setup.</p> Full article ">Figure 2
<p>General plot for trend clarification.</p> Full article ">Figure 3
<p>CO₂ adsorption/desorption at 30 °C using a 3 slpm helium desorption rate and using a CO₂ injection rate of (<b>a</b>) 0.05 slpm, (<b>b</b>) 0.1 slpm, (<b>c</b>) 0.15 slpm, and (<b>d</b>) 0.2 slpm.</p> Full article ">Figure 4
<p>CO₂ adsorption/desorption at 30 °C using a 0.15 slpm CO₂ injection rate and using a helium desorption/injection rate of (<b>a</b>) 0.5 slpm, (<b>b</b>) 2 slpm, (<b>c</b>) 3 slpm, and (<b>d</b>) 4 slpm.</p> Full article ">Figure 5
<p>CO₂ adsorption/desorption at 30 °C using a 0.15 slpm injection rate and 3 slpm helium desorption rate.</p> Full article ">Figure 6
<p>CO₂ adsorption/desorption at (<b>a</b>) 40 °C and (<b>b</b>) 50 °C using a 0.15 slpm CO₂ injection rate and 3 slpm helium desorption rate.</p> Full article ">Figure 7
<p>CO₂ adsorption/desorption at 30 °C using 0.15 slpm rate and 708 cm² surface area.</p> Full article ">Figure 8
<p>CO₂ adsorption/desorption at 30 °C using a 0.15 slpm rate and 364 cm² surface area.</p> Full article ">Figure 9
<p>Adsorption to desorption ratio at different CO₂ injection rates.</p> Full article ">Figure 10
<p>Adsorption to desorption ratio at different helium injection rates.</p> Full article ">Figure 11
<p>Adsorption to desorption ratio at different temperatures.</p> Full article ">

20 pages, 5875 KiB  

Open AccessFeature PaperArticle

Production of Sustainable Adsorbents for CO₂ Capture Applications from Food Biowastes

by Fernando Rubiera, Carlos Córdoba, Tamara Pena and Marta G. Plaza

Energies 2024, 17(5), 1205; https://doi.org/10.3390/en17051205 - 3 Mar 2024

Viewed by 1534

Abstract

Traditional methods to develop biomass-based carbon adsorbents generally involve carbonization followed by chemical or physical activation. However, routes involving the hydrothermal treatment of biomass are receiving growing interest. In this work, two different strategies for the synthesis of sustainable CO₂ adsorbents are [...] Read more.

Traditional methods to develop biomass-based carbon adsorbents generally involve carbonization followed by chemical or physical activation. However, routes involving the hydrothermal treatment of biomass are receiving growing interest. In this work, two different strategies for the synthesis of sustainable CO₂ adsorbents are compared, i.e., in situ ionic activation and hydrothermal treatment followed by activation with CO₂. The latter is a green and simple procedure that does not require the addition of chemicals or acid-washing stages, and which leads to carbon adsorbents with relatively high CO₂ adsorption capacity at low pressures, up to 0.64 mmol g⁻¹ at 15 kPa and 50 °C, conditions relevant for postcombustion CO₂ capture applications. On the other hand, in situ ionic activation can lead to carbon adsorbents with superior CO₂ adsorption capacity in the aforementioned conditions, 0.78 mmol g⁻¹, and with reduced cost and environmental impact compared to conventional chemical activation. Full article

(This article belongs to the Topic Carbon Dioxide Capture or Removal and Valorisation: Advances in the Development of Materials and Technologies)

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<p>Picture of: (<b>a</b>) Cyperus sculentus tubers (also known as tiger nuts, earth almonds, or <span class="html-italic">chufas</span>); (<b>b</b>) HSW.</p> Full article ">Figure 2
<p>Schematic representation of the carbon synthesis protocol consisting on hydrothermal treatment followed by activation with CO₂.</p> Full article ">Figure 3
<p>Schematic representation of the carbon synthesis through in situ ionic activation.</p> Full article ">Figure 4
<p>SEM micrograph of the raw <span class="html-italic">horchata</span> solid waste (HSW).</p> Full article ">Figure 5
<p>SEM micrographs of HSWH-190-3: (<b>a</b>) general view of the pellet surface; (<b>b</b>) detail of silicophytolith accumulation.</p> Full article ">Figure 6
<p>SEM micrographs of: (<b>a</b>) HSWHC-190-3-800-90; (<b>b</b>) HSWC-900-60.</p> Full article ">Figure 7
<p>Narrow micropore size distribution of samples HSWHC-150-3-800-60, HSWHC-170-3-800-60, and HSWHC-190-3-800-60.</p> Full article ">Figure 8
<p>CO₂ adsorption isotherms of carbons HSWHC-150-3-800-60, HSWHC-170-3-800-60, and HSWHC-190-3-800-60 at: (<b>a</b>) 25 °C; (<b>b</b>) 50 °C.</p> Full article ">Figure 9
<p>Narrow micropore size distribution of carbons HSWHC-190-3-800-60, HSWHC-190-3-800-90, and HSWHC-190-3-800-120.</p> Full article ">Figure 10
<p>CO₂ adsorption isotherms at 50 °C of carbons HSWHC-190-3-800-60, HSWHC-190-3-800-90, and HSWHC-190-3-800-120.</p> Full article ">Figure 11
<p>SEM micrograph of carbon HSWIA-190-8-600.</p> Full article ">Figure 12
<p>Narrow micropore size distribution of carbons HSWIA-160-8-600, HSWIA-190-8-600, HSWIA-160-8-800, and HSWIA-190-8-800.</p> Full article ">Figure 13
<p>CO₂ adsorption isotherms at 50 °C of HSWIA carbons activated at: (<b>a</b>) 600 °C; (<b>b</b>) 800 °C.</p> Full article ">Figure 14
<p>Narrow micropore size distribution of carbons HSWGIA-160-8-600 and HSWGIA-190-8-600.</p> Full article ">Figure 15
<p>CO₂ adsorption isotherms at 50 °C of carbons HSWGIA-160-8-600 and HSWGIA-190-8-600.</p> Full article ">Figure 16
<p>Comparison of the narrow micropore size distribution of carbons HSWHC-190-3-800-90, HSWIA-160-8-800 and reference commercial activated carbon Norit R 2030 CO2.</p> Full article ">Figure 17
<p>(<b>a</b>) Comparison of the CO₂ adsorption isotherms at 50 °C of carbons HSWHC-190-3-800-90, HSWIA-160-8-800 and reference commercial activated carbon Norit R 2030 CO2 (full symbols represent adsorption data and empty symbols desorption data); (<b>b</b>) Isosteric heat of adsorption of CO₂ versus loading for carbons HSWHC-190-3-800-90, HSWIA-160-8-800 and reference commercial activated carbon Norit R 2030 CO2.</p> Full article ">Figure 18
<p>(<b>a</b>) N₂ adsorption isotherms at 50 °C of carbons HSWHC-190-3-800-90, HSWIA-160-8-800 and reference commercial activated carbon Norit R 2030 CO2; (<b>b</b>) CO₂/N₂ equilibrium selectivity at 50 °C and 101.325 kPa of carbons HSWHC-190-3-800-90, HSWIA-160-8-800 and commercial activated carbon Norit R 2030 CO2.</p> Full article ">

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