Skip to main content

Thank you for visiting You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

Carbon mineralization pathways for carbon capture, storage and utilization

Carbon mineralization is a versatile and thermodynamically downhill process that can be harnessed for capturing, storing, and utilizing CO2 to synthesize products with enhanced properties. Here the author discusses the advances in and challenges of carbon mineralization, and concludes that tuning the chemical interactions involved will allow us to unlock its potential for advancing low carbon energy and resource conversion pathways.

Advancing novel chemical processes to reduce the carbon intensity of our energy and resource conversion processes is one of our major scientific challenges. Diverse interventionist technologies to capture current CO2 emissions, reuse and store CO2 continue to be developed. One of the common themes across these different technologies is the role of inorganic solid carbonate transformations using anthropogenic CO2 and the development of predictive controls over these pathways. CO2 conversion to solid inorganic carbonates, also known as carbon mineralization, is a thermodynamically downhill route that can be adapted for integration with CO2-emitting energy and resource generating processes1. Despite the simplicity of the stoichiometric reactions describing the formation of Ca- or Mg-carbonates, complex chemo-morphological interactions result in non-monotonic kinetics of carbonate nucleation and growth.

In situ and ex situ carbon mineralization

The availability of Ca- and Mg-bearing resources is crucial for implementing carbon mineralization pathways. About 10,000–1000,000 Gt of total carbon can be stored in naturally occurring mineral deposits2. Mine tailings resulting from nickel extraction3 and diamond production4 and chrysotiles (fibrous hydrated magnesium silicates) in asbestos5 are additional sources of alkalinity for carbon mineralization. Alkaline industrial residues such as fly ash (e.g., Class C fly ash produced by burning lignite or coal has a higher lime content compared to anthracite and bituminous coals that result in Class F fly ash with lower lime content6), cement kiln dust, steel slag, and red mud can store about 200–300 Mt of CO2 annually2. Co-generated CO2 and alkaline industrial residues can be reacted to produce Ca- or Mg-carbonates at the location of interest. Prior to mastering these transformations, it is important to consider how these pathways can be integrated into energy and resource conversion processes. CO2 generated from power plants or industrial sources can be captured, compressed, and stored in reactive geologic formations where CO2 in the fluid form mineralizes to produce water-insoluble calcium or magnesium carbonates, in a process known as in situ carbon mineralization. Alternatively, ex situ carbon mineralization pathways can be developed where the captured CO2 is mineralized into carbonates in engineered processes. Ex situ carbon mineralization can serve as a thermodynamically downhill strategy to capture and remove CO2 from energy and resource conversion processes7,8 that utilize fossil fuels and contribute to more than 70% of anthropogenic greenhouse gas emissions in the United States9. One of the advantages of ex situ processes is that products that can be employed for various applications such as inorganic carbonate can be produced, and therefore can be harnessed as CO2 utilization pathways.

Integration of carbon mineralization with energy and resource conversion pathways

Various energy conversion pathways involving carbon-based resources (e.g., coal, natural gas, biomass, waste plastics) such as combustion, gasification, and anaerobic digestion are accompanied by the evolution of CO2. The emitted CO2 can be directly removed using Ca- and Mg-bearing precursors to produce Ca- and Mg-bearing carbonates. In the context of CO2 capture alone, calcium looping has been proposed in which calcium oxide is used to capture CO2 from flue gas streams to produce calcium carbonate. Calcium carbonate is heated at 900–950 °C to produce pure CO2 and regenerate calcium oxide10. The pure CO2 generated is then utilized and stored. The cycling efficiency of these approaches is dependent on the chemical and mechanical integrity of the oxide materials through multiple operating cycles.

As an alternative to calcium looping as a capture approach alone, capture and removal strategies via ex situ carbon mineralization can be implemented by using calcium and magnesium silicate or alumino-silicate rich minerals and industrial residues. The use of acids to dissolve the alkaline minerals and residues was proposed, followed by the sequential use of bases and then CO2 to produce calcium or magnesium carbonates. As an alternative to concentrated inorganic acids such as nitric or hydrochloric acid, mineral acids such as acetic acid or citric acid produced via microbial pathways have been proposed11. In addition to generating protons needed for dissolution, acetate or citrate ions serve as magnesium or calcium chelating agents, thus enhancing the availability of these cations for carbonate formation. Silica chelating agents such as metal organic frameworks12 and catechol have also been proposed to enhance dissolution of silicate minerals. Advancements in regenerable additives to enhance silicate dissolution at ambient temperature are needed.

Another challenge associated with carbon mineralization lies in enhancing the concentration of carbonate and bicarbonate ions needed for producing solid carbonates. Biological enzymes such as carbonic anhydrase were used to enhance CO2 hydration behavior13,14. As an alternative economical option to carbonic anhydrase, the use of recyclable aqueous CO2 capture solvents such as sodium glycinate15, monoethanolamine (MEA)16,17, and 2-amino-2-methyl-1-propanol18 are used to capture CO2. These CO2-loaded solvents enhance the supply of bicarbonate and carbonate ions, which are essential for precipitating Ca- and Mg-carbonates. The aqueous solvents are regenerated as the solid carbonates are precipitated. Near complete conversion of CaO to CaCO3 is achieved at 50 °C in 3 h using 30 wt% MEA or 1-M sodium glycinate with solid compositions of 15 wt% in well-mixed environments15,17. The inherent chemical regeneration of the solvents with carbonate formation occurs at 50–75 °C, which is significantly below the thermal regeneration of solvents at 100–120 °C.

Alternatively, Ca- and Mg-bearing sorbents can be directly utilized during the energy conversion process. One example is the enhanced conversion of H2 using alkaline sorbents such as Ca(OH)2 and Mg(OH)2 integrated with the water–gas shift reaction (WGSR) as represented by this overall reaction: CaO + CO + H2O = CaCO3 + H2. The WGSR is a versatile pathway to produce H2 and CO2 from CO and water, the products of gasification or reforming of carbon-based resources including biomass19 as represented by this reaction: CO + H2O = CO2 + H2. Given this challenge, conventional modes of operation involve two catalytic systems, one operating between 310 and 450 °C and another between 200 and 250 °C to achieve high conversion20. The pressure is in the range of 20–30 bar. Integrating alkaline sorbents with the WGSR for concurrent CO2 capture shifts the thermodynamic equilibrium toward enhanced H2 production. Proposed advances include the direct use of calcium or magnesium silicates to produce H2 and calcium or magnesium carbonates. This approach eliminates the intermediate step to produce Ca- and Mg-hydroxides or oxides. The hypothesis that the two-step catalytic WGSR can be replaced by a single-step approach by integrating with carbon mineralization is being probed21. The promise in the direct utilization of Ca- and Mg-bearing silicates emerges from evidence showing complete conversions of calcium silicate (CaSiO3) and higher than 80% conversion of magnesium silicate (Mg2SiO4) to their respective carbonates at temperatures in the range of 150–200 °C17,22,23,24, which align with the WGSR conditions. The thermodynamic feasibility of this pathway is represented by the following reactions. Equation (1) below represents syn gas generation. Equations (2)–(4) represent the carbon mineralization of magnesium silicate. The overall combination reaction in Eq. (5) shows that coupling carbon mineralization with the WGSR is overall thermodynamically favorable.

$$2{\mathrm{CO}} + 2{\mathrm{H}}_2{\mathrm{O}} = 2{\mathrm{CO}}_2 + 2{\mathrm{H}}_2\,(\Delta {\mathrm{H}} = - 82.4\,{\mathrm{kJ}}/{\mathrm{mol}})$$
$${\mathrm{Mg}}_2{\mathrm{SiO}}_4 + 2{\mathrm{H}}_2{\mathrm{O}} = 2\,{\mathrm{Mg}}\left( {{\mathrm{OH}}} \right)_2 + {\mathrm{SiO}}_2\,(\Delta {\mathrm{H}} = - 99.7\,{\mathrm{kJ}}/{\mathrm{mol}})$$
$$2{\mathrm{Mg}}\left( {{\mathrm{OH}}} \right)_2 = 2{\mathrm{MgO}} + 2{\mathrm{H}}_2{\mathrm{O}}\,(\Delta {\mathrm{H}} = 162.4\,{\mathrm{kJ}}/{\mathrm{mol}})$$
$$2{\mathrm{MgO}} + 2{\mathrm{CO}}_2 = 2\,{\mathrm{MgCO}}_3\,(\Delta {\mathrm{H}} = - 235.6\,{\mathrm{kJ}}/{\mathrm{mol}})$$
$${\mathrm{Mg}}_2{\mathrm{SiO}}_4 + 2{\mathrm{CO}} + 2{\mathrm{H}}_2{\mathrm{O}} = \,2{\mathrm{MgCO}}_3 + {\mathrm{SiO}}_2 \\ + 2{\mathrm{H}}_2\,(\Delta {\mathrm{H}} = - 255.3\,{\mathrm{kJ}}/{\mathrm{mol}})$$

Another complimentary strategy is to produce bio-hydrogen with carbon removal via mineralization. Renewability, the potential for distributed energy generation, and the opportunity to convert heterogeneous residues such as food waste to useful fuels and products are unique to biomass as an energy resource25. The integration of carbon mineralization with renewable biomass resources has been proposed to accelerate H2 production with the inherent conversion of organic carbon present to inorganic carbonates, as represented by the following reaction19:

$${\mathrm{C}}_{x}{\mathrm{H}}_{y}{{\mathrm{O}}_{z}} + {x}{\mathrm{CaO}} + \left( {2{x}} - {z} \right){\mathrm{H}}_2{\mathrm{O}} \to {x}{\mathrm{CaCO}}_3 + (2{x} - {z} + 0.5{y}){\mathrm{H}}_2$$

The standard heats of reaction for various biomass oxygenates for Eq. (6) are shown in Table 1. This approach has the potential to meet distributed energy needs using a clean energy carrier with inherent carbon removal. Alkaline sorbents such as CaO or Ca(OH)2 enhance the cleavage of C–C bonds and capture the generated CO2 concurrently as the reaction progresses. For example, more than 90% conversion of cellulose to H2 occurred above 500 °C when mixed with stoichiometric proportions of solid Ca(OH)2 and in the presence of Ni/ZrO2 catalyst26. As opposed to generating oxides and hydroxides of Ca and Mg from carbonates, alternative routes of synthesizing these materials from silicate precursors need to be investigated. Figure 1 is a schematic representation of the integration of carbon mineralization pathways with flue gas streams, biomass utilization, and syn gas generation.

Table 1 Standard heats of reaction (kJ/mol) for the conversion of biomass oxygenates to hydrogen with carbon removal through the following reaction: CxHyOz + xCaO + (2x − z)H2O → xCaCO3 + (2x − z + 0.5y)H219.
Fig. 1: Schematic representation of the integration of carbon mineralization pathways and energy conversion processes.

The aqueous alkaline amine looping reactor captures CO2 from flue gas using aqueous solvents such as amines and amino acid salts, and the high concentrations of carbonate and bicarbonate ions react to produce calcium or magnesium carbonates, with the inherent regeneration of the solvent. This reactor is integrated with various CO2 emitting energy conversion processes. Carbon mineralization can be integrated with the water–gas-shift reaction or biomass conversions to enhance H2 formation and remove CO2 as calcium or magnesium carbonates.

In the context of resource utilization, determining the fate of hazardous elements co-present with alkaline industrial residues is an important consideration. Carbon mineralization can reduce the mobility of elements of potential environmental concern, such as Zn, Cu, and Pb as amphoteric constituents and facilitate the partial immobilization of Cr for carbonated Ca-rich slag27. This approach enables the reuse of alkaline materials and reduces the cost of landfilling. Incorporating compositions as low as 10 wt% of carbonate-bearing steel slag in construction materials has shown to enhance the compressive strength from about 33–50 MPa28. CO2 curing of synthetic calcium silicate to produce high strength carbonate-bearing construction materials has now been translated into practice29.

Advancing the science of carbon mineralization also has a translational impact on informing the fate of CO2 injected into subsurface formation bearing reactive calcium and magnesium silicates, also known as in situ carbon mineralization. Field-scale studies such as the injection of pressurized CO2 in reactive basalt formations in Iceland30 and in Washington State31 demonstrated that the Ca- and Mg-silicate constituents of basalt converted to Ca- and Mg-carbonates over the course of a few years. These geochemical conversions were mimicked at representative subsurface conditions of elevated temperature (e.g., 100–200 °C22,23,24) and CO2 partial pressures (e.g., 50–200 atm22,23,24) with high surface area particles and sizes in the range of 5–100 μm. Near complete conversion of calcium silicate minerals such as wollastonite (CaSiO3) and magnesium silicate minerals such as olivine ((Mg,Fe)2SiO4) were achieved on reacting for 3–6 h22,23,24. In contrast, the reactivities of alumino-silicate bearing minerals and rocks do not exceed 50% at comparable reaction conditions22. Carbonates and silica are co-present in the materials obtained after reacting with CO2 at conditions relevant to the subsurface environments. Silicate weathering and carbonate formation mechanisms in the subsurface environments are needed to predict the fate of CO2 injected into reactive subsurface environments. The silica content and its reactivity influence the utilization potential of alkaline industrial residues and minerals.


Despite the advancements made in producing Ca- and Mg-bearing carbonates from anthropogenic CO2, several scientific challenges remain. The chemical compositions and morphologies of alkaline sources such as naturally occurring minerals or alkaline industrial residues are heterogeneous. The influence of silica and iron constituents on the mechanisms and rates of carbonate formation in diverse fluidic environments need to be elucidated. Often, the kinetics of carbonate formation starting from multicomponent precursors can be non-monotonic and developing predicting controls remains a challenge.

As an alternative to existing acid and base consumptive methods to produce Ca- and Mg-bearing carbonates, there is a need for solvents or sorbents that can supply CO2 and can be regenerated in situ as carbonates are formed. Novel chemical pathways to synthesize high purity, nano-scale, and meso-scale Ca- and Mg-carbonates from anthropogenic CO228,32 with few additional unit operations and regenerable solvents are needed. These materials have wide-ranging applications in the paper industry and as filler materials.

Carbonates from anthropogenic CO2 are typically formed in multiphase environments. Characterizing the evolution of the fluid chemistry and the structure and morphologies of carbonates and development of the underlying mechanisms requires the use of novel in operando cross-scale and multimodal characterization methods such as X-ray and neutron scattering, spectroscopy, and tomography at representative temperature and pressure conditions. Advanced characterization of the carbonate products is needed based on the end use of these materials. For example, the use of metastable hydrated magnesium carbonate as algae feed requires the quantification of these phases in the end product33. When considering the use of carbonate-bearing construction materials, linking the carbonate phases and content to the mechanical strength of these materials is crucial.

A fundamental understanding of the dissolution and carbonate formation mechanisms in silicate minerals has a translational impact on our understanding of the storage of CO2 in subsurface geologic formation. Rapid conversion of the injected CO2 into water-insoluble carbonates reduces the mobile fraction of CO2 and the need to monitor the fate of mobile CO2. Dynamic changes in the dissolution and carbonate formation behavior along with the associated changes in the pore and fracture morphology need to be accounted for when evaluating the fate of CO2 in the subsurface environments. Thus, advancing the science of carbon mineralization in subsurface and engineered systems is integral to our carbon management efforts.


  1. 1.

    Gadikota, G. Designing multiphase carbon mineralization pathways for the reactive separation of CO2 and directed synthesis of H2. Nat. Rev. Chem. 4, 78–89 (2020).

    CAS  Article  Google Scholar 

  2. 2.

    Sanna, A., Hall, M. R. & Maroto-Valer, M. Post-processing pathways in carbon capture and storage by mineral carbonation (CCSM) towards the introduction of carbon neutral materials. Energy Environ. Sci. 5, 7781–7796 (2012).

    CAS  Article  Google Scholar 

  3. 3.

    Power, I. M., Dipple, G. M., Bradshaw, P. M. D. & Harrison, A. L. Prospects for CO2 mineralization and enhanced weathering of ultramafic mine tailings from the Baptiste nickel deposit in British Columbia, Canada. Int. J. Greenh. Gas. Control 94, 102895 (2020).

    CAS  Article  Google Scholar 

  4. 4.

    Mervine, E. M. et al. Potential for offsetting diamond mine carbon emissions through mineral carbonation of processed kimberlite: an assessment of De Beers mine sites in South Africa and Canada. Mineral. Petrol. 112, 755–765 (2018).

    CAS  Article  Google Scholar 

  5. 5.

    Gadikota, G., Natali, C., Boschi, C. & Park, A.-H. A. Morphological changes during enhanced carbonation of asbestos containing material and its comparison to magnesium silicate minerals. J. Hazard. Mater. 264, 42–52 (2014).

    CAS  Article  Google Scholar 

  6. 6.

    Jala, S. & Goyal, D. Fly ash as a soil ameliorant for improving crop production—a review. Bioresour. Technol. 97, 1136–1147 (2006).

    CAS  Article  Google Scholar 

  7. 7.

    Kirchofer, A., Brandt, A., Krevor, S., Prigiobbe, V. & Wilcox, J. Impact of alkalinity sources on the life-cycle energy efficiency of mineral carbonation technologies. Energy Environ. Sci. 5, 8631–8641 (2012).

    CAS  Article  Google Scholar 

  8. 8.

    Kirchofer, A., Becker, A., Brandt, A. & Wilcox, J. CO2 mitigation potential of mineral carbonation with industrial alkalinity sources in the United States. Environ. Sci. Technol. 47, 7548–7554 (2013).

    CAS  Article  Google Scholar 

  9. 9.

    U. S. Energy Information Administration (EIA). Energy and the environment explained: where greenhouse gases come from (accessed 30 June 2020);

  10. 10.

    Erans, M., Manovic, V. & Anthony, E. J. Calcium looping sorbents for CO2 capture. Appl. Energy 180, 722–742 (2016).

    CAS  Article  Google Scholar 

  11. 11.

    Zhao, H., Park, Y., Lee, D. H. & Park, A.-H. A. Tuning the dissolution kinetics of wollastonite via chelating agents for CO2 sequestration with integrated synthesis of precipitated calcium carbonates. Phys. Chem. Chem. Phys. 15, 15185–15192 (2013).

    CAS  Article  Google Scholar 

  12. 12.

    Di Lorenzo, F. et al. The carbonation of wollastonite: a model reaction to test natural and biomimetic catalysts for enhanced CO2 sequestration. Minerals 8, 209 (2018).

    Article  Google Scholar 

  13. 13.

    Patel, T. N., Park, A. H. A. & Banta, S. Periplasmic expression of carbonic anhydrase in Escherichia coli: a new biocatalyst for CO2 hydration. Biotechnol. Bioeng. 110, 1865–1873 (2013).

    CAS  Article  Google Scholar 

  14. 14.

    Mirjafari, P., Asghari, K. & Mahinpey, N. Investigating the application of enzyme carbonic anhydrase for CO2 sequestration purposes. Ind. Eng. Chem. Res. 46, 921–926 (2007).

    CAS  Article  Google Scholar 

  15. 15.

    Liu, M. & Gadikota, G. Single-step, low temperature and integrated CO2 capture and conversion using sodium glycinate to produce calcium carbonate. Fuel 275, 117887 (2020).

    CAS  Article  Google Scholar 

  16. 16.

    Liu, M., Asgar, H., Seifert, S. & Gadikota, G. Novel aqueous amine looping approach for the direct capture, conversion and storage of CO2 to produce magnesium carbonate. Sustain. Energy Fuels 4, 1265–1275 (2020).

    CAS  Article  Google Scholar 

  17. 17.

    Liu, M. & Gadikota, G. Integrated CO2 capture, conversion, and storage to produce calcium carbonate using an amine looping strategy. Energy Fuels 33, 1722–1733 (2018).

    Article  Google Scholar 

  18. 18.

    Kang, J. M. et al. Energy-efficient chemical regeneration of AMP using calcium hydroxide for operating carbon dioxide capture process. Chem. Eng. J. 335, 338–344 (2018).

    CAS  Article  Google Scholar 

  19. 19.

    Lima Da Silva, A. & Müller, I. L. Hydrogen production by sorption enhanced steam reforming of oxygenated hydrocarbons (ethanol, glycerol, n-butanol and methanol): thermodynamic modelling. Int. J. Hydrog. Energy 36, 2057–2075 (2011).

    CAS  Article  Google Scholar 

  20. 20.

    Rhodes, C., Hutchings, G. J. & Ward, A. M. Water-gas shift reaction: finding the mechanistic boundary. Catal. Today 23, 43–58 (1995).

    CAS  Article  Google Scholar 

  21. 21.

    Fricker, K. J. & Park, A. H. A. Effect of H2O on Mg(OH)2 carbonation pathways for combined CO2 capture and storage. Chem. Eng. Sci. 100, 332–341 (2013).

    CAS  Article  Google Scholar 

  22. 22.

    Gadikota, G., Matter, J., Kelemen, P., Brady, P. V. & Park, A.-H. A. Elucidating the differences in the carbon mineralization behaviors of calcium and magnesium bearing alumino-silicates and magnesium silicates for CO2 storage. Fuel 277, 117900 (2020).

    CAS  Article  Google Scholar 

  23. 23.

    Gadikota, G., Matter, J., Kelemen, P. & Park, A.-H. A. Chemical and morphological changes during olivine carbonation for CO2 storage in the presence of NaCl and NaHCO3. Phys. Chem. Chem. Phys. 16, 4679–4693 (2014).

    CAS  Article  Google Scholar 

  24. 24.

    Gerdemann, S. J., O’Connor, W. K., Dahlin, D. C., Penner, L. R. & Rush, H. Ex situ aqueous mineral carbonation. Environ. Sci. Technol. 41, 2587–2593 (2007).

    CAS  Article  Google Scholar 

  25. 25.

    National Academy of Sciences, National Academy of Engineering, and National Research Council. Liquid transportation fuels from coal and biomass: technological status, costs, and environmental impacts (The National Academies Press, 2009).

  26. 26.

    Stonor, M. R., Ouassil, N., Chen, J. G. & Park, A. H. A. Investigation of the role of Ca(OH)2 in the catalytic Alkaline Thermal treatment of cellulose to produce H2 with integrated carbon capture. J. Energy Chem. 26, 984–1000 (2017).

    Article  Google Scholar 

  27. 27.

    Santos, R. M. et al. Accelerated mineral carbonation of stainless steel slags for CO2 storage and waste valorization: Effect of process parameters on geochemical properties. Int. J. Greenh. Gas. Control 17, 32–45 (2013).

    CAS  Article  Google Scholar 

  28. 28.

    Gadikota, G., Fricker, K., Jang, S.-H., Park, A.-H. A. Carbonation of silicate minerals and industrial wastes and their potential use as construction materials. In Advances in CO2 capture, sequestration, and conversion (eds Jin, F., He, L.-N. & Hu, Y. H.) 295–322 (American Chemical Society, 2015).

  29. 29.

    Riman, R. E. & Atakan, V. Systems and methods for carbon capture and sequestration and compositions derived therefrom. US8114367B2 (2012).

  30. 30.

    Snæbjörnsdóttir, S. Ó. et al. Carbon dioxide storage through mineral carbonation. Nat. Rev. Earth Environ. 1, 90–102 (2020).

    Article  Google Scholar 

  31. 31.

    Schaef, H. T., McGrail, B. P. & Owen, A. T. Basalt-CO2–H2O interactions and variability in carbonate mineralization rates. Energy Procedia 1, 4899–4906 (2009).

    CAS  Article  Google Scholar 

  32. 32.

    Werner, M., Hariharan, S. & Mazzotti, M. Flue gas CO2 mineralization using thermally activated serpentine: from single-to double-step carbonation. Phys. Chem. Chem. Phys. 16, 24978–24993 (2014).

    CAS  Article  Google Scholar 

  33. 33.

    Ye, Z., Abraham, J., Christodoulatos, C. & Prigiobbe, V. Mineral carbonation for carbon utilization in microalgae culture. Energy Fuels 33, 8843–8851 (2019).

    CAS  Article  Google Scholar 

Download references


This work is supported by the US Department of Energy, Office of Science, Basic Energy Sciences under the Award #DE-SC0020263.

Author information



Corresponding author

Correspondence to Greeshma Gadikota.

Ethics declarations

Competing interests

The author declares no competing interests.

Additional information

Publisher’s note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Rights and permissions

Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in a credit line to the material. If material is not included in the article’s Creative Commons license and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this license, visit

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Gadikota, G. Carbon mineralization pathways for carbon capture, storage and utilization. Commun Chem 4, 23 (2021).

Download citation


Quick links

Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing