Establishing ultraporous permanently polarized hydroxyapatite as a green and highly efficient catalyst for carbon dioxide conversion in continuous flow under mild conditions

Abstract

We present the use of an ultraporous permanently polarized hydroxyapatite (upp-HAp) catalyst for continuous and highly efficient production of formic acid (predominant) and acetic acid using wet CO₂ (i.e. CO₂ bubbled into liquid water) as a reagent. In all cases, reactions were conducted at temperatures ranging from 95 to 150 °C, using a CO₂ constant flow of 100 mL s⁻¹, and without applying any external electric field and/or UV radiation. Herein, we study how to transfer such a catalytic system from batch to continuous reactions, focusing on the water supply (proton source): (1) wet CO₂ or (2) liquid water in small amounts is introduced in the reactor. In general, the reduction of CO₂ to formic acid predominates over the C–C bond formation reaction. On the other hand, when liquid water is added, two interesting outcomes are observed: (1) the yield of products is higher than in the first scenario (>2 mmol g_c⁻¹·min⁻¹) while the initial liquid water remains largely available due to the mild reaction temperature (95 °C); and (2) a high yield of ethanol (>0.5 mmol g_c⁻¹·min⁻¹) is observed at 120 °C, as a result of the increased efficiency of the C–C bond formation. Analysis of kinetic studies through temporal and temperature dependence shows that CO₂ fixation is the rate limiting step, ruling out the competing effect of proton adsorption on the binding sites and confirming the crucial role of water. The activation energy for the CO₂ fixation reaction has been determined to be 66 ± 1 kJ mol⁻¹, which is within the range of conventional electro-assisted catalysts. Finally, mechanistic insights on the CO₂ activation and role of the binding sites of upp-HAp are provided through isotopic-labeling (¹³CO₂) and near-ambient pressure X-ray photoelectron spectroscopy (NAP-XPS) studies.

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Sustainability spotlight

The catalytic conversion of carbon dioxide (CO₂) into value-added chemical products (CO₂-revalorization) is interesting because of its potential to close the carbon cycle while generating green circular economies. However, truly sustainable CO₂-revalorization processes are normally restricted by the use of noble metal-based catalysts and/or intensive reaction conditions. Accordingly, we explore the use of ultraporous permanently polarized hydroxyapatite (upp-HAp) as a catalyst for green CO₂-revalorization. upp-HAp is abundant and biocompatible (main inorganic component of biological hard tissues). Besides, upp-HAp is capable of performing successful reactions under mild conditions (achievable through renewable sources) and in batch/continuous configurations, representing a viable alternative to conventional catalysts. This work is aligned with the SDG7 (affordable and clean energy) and SDG13 (climate action) UN sustainable development goals.

Introduction

The concentration of carbon dioxide (CO₂), the most significant greenhouse gas in the atmosphere, has significantly increased in recent years mainly due to the combustion of fossil fuels.^1–4 This environmental impact has accelerated research activities to capture CO₂, and thus avoid or minimize CO₂ release into the atmosphere. Two research approaches have been prioritized looking for net zero emissions: (1) CO₂ capture and long term geological storage or reutilization in several innovative ways;^5–10 and (2) catalytic conversion of CO₂ into value-added compounds of chemical and industrial interest using efficient catalysts and low energy consuming processes (i.e. CO₂ reutilization and valorization).^11–19

Although many noble metal-based catalysts have been investigated for CO₂ conversion into chemicals of industrial interest (e.g. Rh, Ru, Pt, Au and Pd),^15,20–31 simple systems based on non-precious metal catalysts are preferred due to their lower cost and higher sustainability (e.g. Fe, Cu, Zn, and Co among others).^32–40 Similarly, although efficient catalytic processes have been developed to transform CO₂ into valuable chemicals using harsh reaction conditions (i.e. high temperature and/or pressure), processes involving mild reaction conditions are the most desired to avoid contradictions related to energy/mass balance inefficiencies, for example that the energy consumption and CO₂ emission associated with the elimination of this greenhouse gas is higher than the CO₂ transformed.^41–45 A large number of studies have been devoted to the catalytic conversion of CO₂ into organic products (e.g. alcohols and acids with one or more carbon atoms), with the main results being compiled in recent reviews.^28,46–54

In a recent study we proposed a polarized bioceramic, a sustainable metal-free catalyst, for the conversion of CO₂ into ethanol using mild reaction conditions.⁵⁵ This catalyst consisted of hydroxyapatite (HAp), a naturally occurring mineral with the formula Ca₅(PO₄)₃(OH), that is non-toxic and biocompatible and, therefore, frequently used for biomedical applications.^56–59 HAp was permanently polarized by applying a thermally stimulated polarization (TSP) process at high temperature. The resulting material (named pp-HAp) became catalytically active due to extraordinary charge accumulation on its surface. Thus, pp-HAp was found to exhibit not only vacancies and charge accumulation at the HAp crystal lattice but also charge accumulation at the boundaries among the microscopic HAp crystal grains.^60,61 Compact pp-HAp discs, which were prepared by applying a pressure of 620 MPa to HAp powder before applying the TSP, were found to convert CO₂ into a mixture of ethanol (predominant) and some other minor compounds (i.e. acetic acid, formic acid, methanol and acetone) using a starting mixture of CO₂ and CH₄ (3 bar each) and 1 mL of liquid water.⁵⁵ However, the yield of the reaction (expressed in μmol per gram of catalyst; μmol g_c⁻¹), which was performed in a batch reactor at 140 °C, was very low after 72 h: 18.6 ± 1.9, 2.7 ± 0.6, 1.9 ± 0.6, 1.5 ± 0.3 and 0.9 ± 0.2 μmol g_c⁻¹ for ethanol, acetic acid, formic acid, methanol, and acetone, respectively.

More recently, the performance of the pp-HAp catalyst was significantly improved by modifying the synthesis process to provide ultra-porosity and printability.⁶² Thus, printable inks were prepared by mixing HAp powder with Pluronic® F-127 hydrogel. The latter was removed after 3D printing the scaffold (but before applying the TSP process) by calcining the samples at 1000 °C. The resulting catalyst exhibited spherical HAp nanoparticles with an average diameter of 159 ± 43 nm. More specifically, this printed catalyst consisted of a 3D network forming branches made of coalesced nanoparticles separated by nanometric pores (average size: 167 ± 51 nm). The performance of the ultraporous pp-HAp catalyst (hereafter named upp-HAp) for the production of ethanol was studied by loading a CO₂°:°CH₄ mixture (3 bar each) and 1 mL of liquid water into the batch reactor and applying 140 °C for 48 h. The ethanol yield increased up to 55.0 ± 4.9 μmol g_c⁻¹, which represented an outstanding increment of the catalytic performance (by a factor of 2.9).

Despite that, most of the studies reported focus on the enhanced electrical properties of the material, rather than elucidating the catalytic mechanisms involved. In this work, we go one step further by transferring the use of the upp-HAp catalyst from the batch reactor to a continuous process where the kinetics of the conversion of CO₂ into ethanol have been studied. Because of the extremely high yields obtained, we have focused on the catalytic activity of upp-HAp to clarify, for the first time, the fundaments of upp-HAp as a highly efficient and sustainable catalyst. For this purpose, first we have examined the formation of products in the different phases (i.e. adsorbed on the catalyst surface, liquid water and gas phase, as this is a heterogeneous catalytic process) as a function of the time using a batch process. Next, the influence of water, which is rapidly consumed in the continuous process, and how it is supplied have been examined (i.e. wet CO₂ or liquid water). Third, the catalytic performance of upp-HAp has been studied by varying the temperature and reaction time to determine the kinetics of the reaction. Finally, isotope-labeling ¹³CO₂ reactions and near ambient pressure X-ray photoelectron spectroscopy (NAP-XPS) studies have been performed to support the results presented. Accordingly, the catalytic mechanism of CO₂ activation has been experimentally determined further establishing upp-HAp as a green catalyst for CO₂ fixation.

Experimental methods

Synthesis of the ultraporous pp-HAp catalyst

Synthesis of hydroxyapatite (HAp). 15 mL of 0.5 M (NH₄)₂HPO₄ in deionized water were added at a constant rate of 2 mL min⁻¹ to 25 mL of a 0.5 M Ca(NO₃)₂ solution in ethanol with pH previously adjusted to 11 using NH₄OH solution. The mixture was left aging for 1 h under gentle agitation (150 rpm) at room temperature. Hydrothermal treatment at 150 °C was applied using an autoclave Digestec DAB–2 for 24 h. The autoclave was allowed to cool down before opening. The precipitate was separated by centrifugation and washed with water and a 60/40 v/v mixture of ethanol/water (twice). After lyophilizing it for 3 days, a white powder was obtained. The HAp powder was extensively ground to reduce aggregates and homogenize the grain size, this step being crucial for the nanostructure of the HAp scaffold (see below).

Synthesis of Pluronic® F-127 hydrogel. 25 g of distilled water was mixed with 25 g of Pluronic® F-127 polymer using a FlackTek SpeedMixer at 3500 rpm for 5 minutes. After that, 50 g of Pluronic® polymer were added and vigorously stirred under the same conditions. The resultant hydrogel was stored at 4 °C.

Synthesis of ultraporous pp-Hap (upp-HAp). HAp powder was extensively ground to reduce aggregates and to homogenize the grain size, this step being crucial for achieving the nanostructure of the HAp scaffold. Then, 60% wt of previously prepared Pluronic® F-127 hydrogel was slowly added to the ground HAp powder in a cold room at 4 °C. In order to achieve a homogeneous mixture, this additive process was periodically interrupted for stirring at 2500 rpm for 2 min using a Fisherbrand™ Digital Vortex Mixer. The obtained white paste was left to age at 4 °C for 24 h to ensure the homogeneous distribution of the hydrogel. The resulting ink was modeled using a cold spatula (<4 °C) to obtain 3D HAp scaffolds with the desired shape. The utilization of the cold spatula allowed the friction between the metal and the paste to be reduced without compromising the homogeneity of the shaped samples. Finally, the mixture was calcined at 1000 °C using a muffle Carbolite ELF11/6B/301 for 2 h. In this step, the Pluronic® F-127 hydrogel was completely removed from the resulting HAp modeled structure.

The calcined HAp porous structures were thermally and electrically activated to achieve the catalytic properties by placing the samples between two stainless steel plates (AISI 304), which acted as electrodes. The HAp sample was left in control with the negative electrode, while the positive electrode was separated 4 cm from the calcined sample. A constant DC voltage of 500 V was applied for 1 h with a GAMMA power supply, while the temperature was kept at 1000 °C. Samples were allowed to cool down maintaining the applied electric potential for 30 minutes, and finally, the whole system was powered off and left to cool down overnight.

Characterization of the upp-HAp catalyst

Raman analyses were performed by means of an inVia Qontor confocal Raman microscope (Renishaw) equipped with a Renishaw Centrus 2957T2 detector and a 532 nm laser. In order to obtain representative data, 32 single point spectra were averaged.

X-ray diffraction (XRD) studies were conducted using a Bruker D8 Advance model with Bragg–Brentano 2θ configuration and Cu K_α radiation (λ = 0.1542 nm). Measurements were performed in a 2θ range of 20°–60° in steps of 0.02°, and a scan speed of 2 s using a one-dimensional Lynx Eye detector.

Scanning electron microscopy (SEM) images were obtained using a Zeiss Neon40 microscope equipped with a SEM GEMINI column.

High resolution transmission electron microscopy (HRTEM) was performed using a JEOL 2010F microscope equipped with a field emission electron source and operated at an accelerating voltage of 200 kV. The point-to-point resolution was 0.19 nm, and the resolution between lines was 0.14 nm. Samples were dispersed in an aqueous (Milli-Q) suspension in an ultrasonic bath, and a drop of the suspension was placed over a grid with holey-carbon film. Images were not filtered or treated by means of digital processing and they correspond to raw data.

Near-Ambient Pressure X-ray Photoelectron Spectroscopy (NAP-XPS) experiments were performed with a SPECS Surface Nano Analysis GmbH (Berlin Germany) system. The spectrometer was equipped with an Al (XR50) anode operating at 400 W and with a Phoibos 225 (SPECS) detector (hemispherical energy analyzer, HAS). The pass energy of the hemispherical analyzer was set to 20 eV and the energy step of high resolution spectra was set at 0.1 eV. The temperature of the analysis was controlled using an Electron Beam Heater (EBH-150, SPECS Surface Nano Analysis GmbH) which has been monitored during the whole experiment through a thermocouple sensor. The C 1s peak was used as an internal reference with a binding energy of 284.5 eV. The obtained experimental spectra were fitted using a Gaussian–Lorentzian curve.

Batch reactions

The reactor consisted of an inert reaction chamber (120 mL) coated with a perfluorinated polymer where both the catalyst and water were placed. All surfaces were coated with a thin film of perfluorinated polymer in order to avoid any contact between the reactants, catalyst and the stainless steel reactor surfaces, in order to rule out other catalytic effects. The reactor was equipped with an inlet valve for the entry of gases and an outlet valve to recover the gaseous reaction products.

Both the upp-HAp catalyst and deionized liquid water (20 mL) were introduced into the reactor. After exhaustive purging with CO₂, the chamber pressure was increased up to 6 bar of CO₂ (measured at room temperature). The reaction was conducted for 1, 4, 8 and 18 h at 120 °C. All processes were performed in triplicate. The isotope-labeling experiment was carried out using ¹³CO₂ purchased from Cambridge Isotope Laboratories INC (purity: ¹³C 99%). 1 bar of ¹³CO₂ and 5 bar of ¹²CO₂ were introduced in the reactor. The reaction temperature was set at 120 °C for 72 h.

Continuous flow reactions

The continuous CO₂ conversion into valuable chemicals was carried out using a commercial borosilicate glass continuous-flow reactor (novaLight CUBE 100, Peschl Ultraviolet GmbH, Germany). All reactions were conducted using a constant CO₂ flow of 100 mL s⁻¹. Despite the reactor being designed to allow UV irradiation, all reactions were conducted without UV light since previous studies using a batch reactor showed that such energy supply is not required when pp-HAp or upp-HAp catalysts are used.^55,62 Reactions were performed introducing 1 mL of liquid water into the reactor. When performed without liquid water this is explicitly indicated for each case below. All the studied processes were performed in triplicate.

Analysis of the reaction products

The reaction products dissolved in the liquid water (batch reactions), the reaction products condensed by the cold trap (continuous reaction), and the reaction products adsorbed on the catalyst were analyzed by ¹H NMR spectroscopy. In order to desorb the reaction products from the catalyst, samples were dissolved in a solution containing 100 mM HCl and 50 mM NaCl with the final addition of deuterated water. All ¹H NMR spectra were acquired with a Bruker Avance III-400 spectrometer operating at 400.1 MHz. The chemical shift was calibrated using tetramethylsilane as the internal standard. 256 scans were recorded in all cases to obtain an optimum signal-to-noise-ratio for proper area integration. In order to compare the different products obtained from the studied reactions, the areas associated with the proton contribution were normalized and regularly calibrated through external references to ensure a high accuracy of the measurements.

After the batch reactions, the gas was collected by means of an MSHA portable pump and stored in a Tedlar® gas sampling bag (LB-2 Septa) and analyzed on a Trace1300 gas chromatograph equipped with a valve for gas injection fitted with a thermal conductivity detector (ThermoFisher Scientific). Prior to the measurements, the samples were transferred from the Tedlar® bags to multi-sorbent bed tubes (Carbotrap, Carbopack X and Carboxen 569) to ensure proper storage and manipulation.

Results and discussion

Design and characterization of the catalyst

The upp-HAp catalyst was prepared as is described in the Experimental methods section. The new properties of this catalytically active ceramic rely on the enhanced charge accumulation and boosted electron transport properties achieved through intensive lattice refinement. As depicted in Scheme 1, while vacancy engineering (i.e. generation of OH⁻ vacancies) is considered to increase the quantity of available charges (Fig. S1 and S2†), and thus, the activity of the naturally occurring acid binding sites (Ca²⁺ as Lewis and P–OH as Brønsted acidic sites) and basic Lewis binding sites (O²⁻ atoms of PO₄³⁻ and OH⁻) of HAp,⁶³ the TSP treatment imposes a specific global orientation to the hydroxyl groups oriented in columns along the c-axis that boosts the electron transport (Fig. S3†), and consequently, favors the catalytic conversion of carbon dioxide to new products. Note that although upp-HAp could be strictly referred to as a thermal catalyst (i.e. neither external electric currents nor UV irradiation are needed for the reaction) the nature of the catalyst strongly relies on its refined electrical properties. Hence, upp-HAp finds more similarities to the classical electroreduction mechanisms and formulations reported in the literature. In this sense, this dual approach proposes upp-HAp as a sustainable green candidate to replace the current metal-based thermocatalysts, further competing directly with the efficiencies obtained by means of conventional electrocatalysis. Such features have been widely studied in the literature in terms of the customization of the enhanced electrical properties (material characterization approach), reporting exhaustive structural analyses to ensure its proper catalytic activation.^{55,60–62,64–69}

Scheme 1 Structure of HAp as a catalyst. (a) HAp unit cell P6₃/m. (b) (001) crystallographic plane observed from the c-axis direction. The OH⁻ channels and the Ca(I) 6-fold coordination are highlighted. (c) Structural changes and lattice refinement strategies adopted to achieve the catalytic activation of HAp.

Accordingly, the Raman spectrum of upp-HAp (Fig. 1a) displays the characteristic active modes of HAp with ν₁ = 962 cm⁻¹ (P–O symmetric stretching), ν₂ = 400–480 cm⁻¹ (doubly degenerated O–P–O bending), ν₃ = 570–625 cm⁻¹ (P–O triply degenerated asymmetric stretching), ν₄ = 1020–1095 cm⁻¹ (triply degenerated O–P–O bending mode) and ν₅ = 3574 cm⁻¹ (O–H stretching).⁶³ Besides, the peaks at 878, 844 and 794 cm⁻¹ are attributed to the formation of brushite (CaHPO₄·2H₂O) due to the polarization process, thus proving the correct catalytic activation of HAp.⁶⁶ Consistently, the XRD diffractogram of upp-HAp (Fig. 1b) shows the typical HAp reflections at 2θ = 25.9° (002), 31.8° (211), 32.3° (112) and 33.0° (300), while the presence of brushite is confirmed by the peak at 31.1° (121).⁶⁶ Also, comparison with the Raman spectrum and XRD diffractogram of calcined HAp samples (i.e. just before applying the TSP process), which are shown in Fig. S4,† confirms the success of the treatment used to induce permanent polarization.

Fig. 1 (a) Raman spectrum, (b) XRD diffractogram, (c) SEM and (d) HRTEM micrographs, and (e) fast Fourier transform of the HRTEM micrograph for upp-HAp. In (a) the characteristic HAp (ν₁–ν₅) and brushite (diamonds) Raman vibrational modes are displayed. In (b), the characteristic HAp (spots) and brushite (diamonds) reflections are indicated.

SEM and HRTEM micrographs of upp-HAp are shown in Fig. 1c–e. As can be seen, the SEM image reflects the ultraporous structure of the catalyst with an average pore size of 156 ± 32 nm. The porosity, which was estimated considering five independent SEM images, was 17% ± 2%. The crystallinity of the samples was confirmed by the lattice fringes observed in HRTEM images (Fig. 1d). Fast Fourier transform of the upp-HAp fringes (Fig. 1e) allowed not only the distinction between the (002) and (112) crystallographic planes of HAp at 3.40 Å and 2.75 Å, respectively, but also the identification of the characteristic polarized superstructure (001) at 6.87 Å d-spacing.

From batch to continuous reactions

In previous studies, the efficiency of pp-HAp and upp-HAp catalysts to convert CO₂ alone⁶⁷ or mixed with CH₄ (ref. 55 and 62) into ethanol (predominant) and other valuable chemicals was examined, quantifying by ¹H NMR the amount of reaction products dissolved in the liquid water (hereafter named “supernatant”) and adsorbed on the catalyst. Thus, we assumed that the content of products in the gas phase was negligible in comparison to those in the supernatant and on the catalyst. In this work, as a first step and before transferring the process to a continuous-flow reactor, we experimentally examined the time evolution of the gas composition compared to the supernatant and the catalyst of the batch reactions. The results presented in Fig. 2 are expected to provide better understanding about the distribution of products among the different phases in the continuous-flow process described in the next section.

Fig. 2 Variation of the different product yields in the gas, adsorbed on the catalyst and dissolved in the supernatant vs. the reaction time obtained from batch reactions catalyzed by upp-HAp. Reactions were conducted at 120 °C using 6 bar of CO₂ and 20 mL of liquid water. The total yield, which corresponds to the sum of the yields of all the individual products, is presented as well. The yields are expressed in μmol of product per gram of catalyst (μmol g_c⁻¹).

The variations of the product yields over time confirm that the resulting species are partially adsorbed on the solid catalyst and mainly dissolved in the supernatant. Thus, the yields of the different products are one and two orders of magnitude smaller in the gas than in the catalyst and the supernatant, respectively. Furthermore, the three analyzed phases present reaction products containing two or three carbon atoms (C2 and C3, respectively), while products with one carbon atom (C1) are only detected in the catalyst and supernatant (i.e. methanol and formic acid). This feature suggests that C1 products evolve into C2 and C3 before migrating to the gas phase. The thermodynamics of water splitting and CO₂ reduction into formic acid, which is an exhaustively studied reaction,^68–76 have been discussed in a recent review.⁷⁷ Besides, all C2 products seem to be inter-related in the sense that acetic acid and acetaldehyde probably come from the complete or partial oxidation of ethanol, respectively. Similarly, acetone is catalytically hydrogenated to isopropanol at low pressure and temperature when the mass transfer between the liquid and the gas is high enough.⁷⁸ Further analysis of the results is provided in the ESI.†

On the other hand, the water content available in the reactor also merits special attention when moving from batch to continuous reactions. That is because water not only provides a medium to collect the products desorbed from the catalyst (i.e. supernatant) but also acts as the proton source. Accordingly, in Scheme 2 and Fig. S5† the batch and continuous reactor systems used are compared. Thus, for the continuous reactions two different scenarios were considered: (1) liquid water is directly introduced into the reactor (1 mL) and (2) CO₂ is bubbled into liquid water to produce wet CO₂ (see Scheme 2b). Both reaction approaches were carried out at 95 °C and 120 °C analyzing the products obtained in the cold trap (Scheme 2b) after 15 minutes. Representative ¹H NMR spectra are presented in Fig. 3a (complete spectra are shown in Fig. S6†), while the yields of the reaction are provided in Fig. 3b and c for scenarios (1) and (2), respectively. Moreover, a blank (i.e. reaction without the upp-HAp catalyst at 120 °C using the same experimental conditions as those in the upp-HAp catalyzed reactions) was also conducted (Fig. 3a) to rule out other carbon sources.

Scheme 2 (a) Scheme of the batch reactor used. (b) Scheme of the continuous reactor used. The continuous reactor was filled with four upp-HAp catalysts (3.60 × 5.00 × 0.44 mm³ each) and 1 mL of deionized water which was homogeneously distributed (approach 1). The outlet valve of the reactor was connected to a cold trap to condense the reaction products obtained in the gas phase, while the inlet valve was connected to a CO₂ cylinder to achieve a constant flow of 100 mL s⁻¹, which was controlled using a back-pressure regulator. This high flow was selected to mimic the conditions at the pre-pilot scale. To have the required moisture, as water is the proton source, CO₂ was bubbled into liquid water to produce wet CO₂, the bubbler being located between the CO₂ cylinder and the inlet valve (approach 2).

Fig. 3 Continuous reaction studies. (a) Representative ¹H NMR spectra used to identify the reaction products for the continuous processes catalyzed by upp-HAp and performed at 95 and 120 °C using a CO₂ flow of 100 mL s⁻¹ and 1 mL of liquid water. The spectrum of a blank (i.e. without catalyst) at 120 °C is also displayed. Each spectrum corresponds to the liquid collected in the cold trap after 15 min of reaction. (b) Yield of the reaction products for the continuous process described in (a). The yields were calculated from the ¹H NMR spectra of the liquids collected in the cold trap after 15 min of reaction. The total reaction yield (i.e. sum of the yields of the individual products) is also displayed. (c) Yield of the reaction products for the continuous process catalyzed by upp-HAp at 95 °C and 120 °C but without including liquid water in the reactor. The yields were derived from the ¹H NMR spectra of the liquids collected in the cold trap after 15 min of reaction. (d) Evolution of the non-accumulated yields of the reaction products identified by ¹H NMR against the reaction time for the continuous processes conducted including 1 mL of liquid water in the reactor and catalyzed by upp-HAp at 95 °C. (e) Variation of the temperature for a process conducted up to 30 min. In all cases, the reactions were catalyzed by upp-HAp and using wet CO₂ but without including liquid water in the reactor. (f) Reaction products adsorbed on the upp-HAp catalyst after several continuous-flow catalytic processes at 120 °C without including liquid water in the reactor. The amount of product was calculated from the ¹H NMR spectrum collected after dissolving the catalyst using an aqueous solution containing 100 mM HCl and 50 mM NaCl. The total yield, which is the sum of the yields of all the individual products, is also presented. The yields are expressed as mmol of product per gram of catalyst per min (mmol g_c⁻¹·min⁻¹).

As can be observed, the collected spectra showed some important differences, which suggested that the evaporation rate of water plays a crucial role in the reaction mechanisms. The reaction at 95 °C led to the formation of formic acid identified by the singlet at 8.36 ppm as the predominant product and acetic acid denoted by the CH₃ singlet at 1.95 ppm as the residual product. Thus, the reaction exhibited not only a high yield of formic acid (expressed as mmol of product per gram of catalyst per minute), 1.97 ± 0.06 mmol g_c⁻¹·min⁻¹, but also a very high selectivity (∼95%, comparable to the photocatalysts)⁷⁹ towards such C1 product, the ratio of formic acid/acetic acid yields being around 20 (Fig. 3b). Compared to the literature, the results reported here represent a compelling step forward in the field of heterogeneous catalysis which is extremely competitive not only when considering the total yield obtained (124 mmol g_c⁻¹·h⁻¹ for upp-HAp compared with the standard range of 2–20 mmol g_c⁻¹·h⁻¹)⁷⁹ but also because of the greener and more sustainable reaction conditions achieved (i.e. mild conditions, use of water instead of H₂, avoiding the use of electrical supply or UV irradiation, use of a green and abundant catalyst). Table 1 compares all the features obtained with respect the conventional heterogeneous catalysts used (more detailed information can be also found in Table S1†). Surprisingly, the total yield of products at 95 °C (2.07 ± 0.07 mmol g_c⁻¹·min⁻¹) decreased by half at 120 °C (1.04 ± 0.05 mmol g_c⁻¹·min⁻¹) and the reaction became much less selective. Thus, in addition to formic acid (0.49 ± 0.03 mmol g_c⁻¹·min⁻¹), both ethanol (C2) and acetone (C3) were clearly detected at 120 °C. The yield of ethanol (0.52 ± 0.02 mmol g_c⁻¹·min⁻¹), which was identified by the quartet from CH₂ at 3.53 ppm and the triplet from CH₃ at 1.06 ppm (Fig. 3a), was comparable to that of formic acid. Conversely, acetone, with the CH₃ singlet at 2.11 ppm (Fig. 3a), remained as a residual product (0.03 ± 0.01 mmol g_c⁻¹·min⁻¹). These observations indicate that such conditions (i.e. temperature high enough to promote the rapid evaporation of liquid water) favor the catalytic formation of C–C bonds, although they are detrimental to the efficiency of the overall CO₂ conversion process (Fig. 3b).

Table 1 Comparison between the most relevant features of this work and the standard conditions reported for heterogeneous catalysis⁷⁹

	Catalyst	Proton source	T (°C)	Maximum selectivity (%)	Productivity (mmol gc^−1·h^−1)
Heterogeneous catalysis^79	Pd, Au, Cu–ZnO, M–ZrOx,…	H2	220–300	>70 (Methanol)	2–29 (Total products)
This work	upp-HAp	H2O	95	∼95 (Formic acid)	124 (Total products)

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In the batch reactions, which were conducted using 20 mL of liquid water, ethanol was the predominant product in both the supernatant and the catalyst, while the content of formic acid was residual (Fig. 2). Instead, ethanol and formic acid were formed with similar yields when only 1 mL of liquid water was introduced in the continuous reactor. This feature suggests that, in the batch process, the excess evaporated water favors the formation of ethanol (i.e. generation of a C–C bond and hydrogenation) over the reduction of CO₂ to formic acid (C1), while the continuous flow of CO₂ and the decrease of available water molecules promote the conversion of CO₂ to formic acid instead of producing ethanol.

This hypothesis can be further corroborated by analyzing the yields of the products obtained using wet CO₂ (approach 2). As seen in Fig. 3c, both formic and acetic acid are obtained, whereas ethanol and acetone were not detected. Comparison of the yields, which are shown in Fig. 3c, with Fig. 3b reveals a reduction in the total yield of two and one order of magnitude at 95 and 120 °C, respectively. Furthermore, in the absence of liquid water, the yields of the two reaction products increased with temperature, as expected. Overall, these results demonstrate that liquid water is responsible for both the variety of products and the large yields reflected in Fig. 3b.

All these features can be clearly observed when merging both approaches (i.e. wet CO₂ and addition of 1 mL of liquid water in the reactor) in a single long term (4 hours) continuous reaction depicted in Fig. 3d and exhaustively described in the ESI.† Considering a CO₂ flow of 100 mL s⁻¹ (0.24 mol min⁻¹), the yields reported at 15 min in Fig. 3d in the lab scale indicate that conversion of CO₂ into products is around 1%. The yields at 95 °C (Fig. 3d) stabilized at 7.4 ± 0.4 and 4.0 ± 0.4 mmol g_c⁻¹·h⁻¹ for formic acid and acetic acid, respectively. These values were significantly higher than those reported in the literature for the photocatalytic and the electrocatalytic reduction and hydrogenation of CO₂.^80,81

To better understand the reaction sequence, the yields of the individual products and the total yield were analyzed as a function of the temperature after 30 min of reaction. Results for reactions performed at 95, 110, 120 and 150 °C, which are plotted in Fig. 3e, showed that all yields increased with the temperature, even though two regimes were observed. At temperatures ≤120 °C, the yields of formic acid and acetic acid, as well as the total yield, increased linearly with the temperature. However, at 150 °C, the yield of acetic acid remained unchanged while that of formic acid increased significantly, suggesting an enhancement in the dominance of the CO₂ reduction to formic acid with respect to the formation of C–C bonds. After these assays, the products adsorbed in the catalyst were analyzed by ¹H NMR. Accordingly, results presented in Fig. 3f have been further discussed in the ESI.†

Another important observation refers to the catalytic stability of upp-HAp for both batch and continuous processes, which was evidenced by the fact that the yields were maintained in all repetitions carried out (i.e. the same catalyst samples were always used). Fig. S7,† which compares the Raman spectra of the catalyst before and after reaction, confirms such stability. As can be observed, the main vibration (ν₁ peak at 962 cm⁻¹), which was assigned to the main symmetric stretching P–O mode, does not show any significant difference. It is worth mentioning that any loss of electrical and, consequently, catalytic activity would be detected by a widening and/or splitting of the ν₁ band in the Raman spectrum. In this sense, this study is in agreement with the results reported in a recent work from where the complete stability of the upp-HAp catalysts is studied through different characterization techniques and under a wide range of temperatures.⁸²

Mechanistic insights on CO₂ activation: NAP-XPS studies and isotope-labeling reaction

Due to the novelty of the catalyst and the relevance of converting the thermodynamically stable CO₂ molecule in value-added molecules, significant effort has been made to experimentally explore the initial steps of CO₂ adsorption and activation on the upp-HAp surface. Firstly, we performed isotope-labeling experiments by loading ¹³CO₂ and 5 bar of ¹²CO₂ in a batch reactor (20 mL liquid water and 120 °C for 72 hours) to isotopically confirm the CO₂ fixation reaction. Fig. 4a compares the ¹H NMR spectra collected from the supernatant of a standard (i.e. 6 bar of ¹²CO₂) and the isotope-labeling reaction, focusing on the region of acetic acid (1.6–2.4 ppm). As can be seen, the distinctive doublet of ¹³CH₃COOH can be observed to be shifted ∼0.3 ppm from the ¹²CH₃COOH peak at 1.95 ppm.⁸³

Fig. 4 (a) Isotope-labeling experiments. High resolution NAP-XPS studies using ¹²CO₂ of the P 2p (b), Ca 2p (c) and C 1s (d). (e) Fixation mechanism derived from ¹H NMR and NAP XPS results.

Additionally, near-ambient pressure X-ray photoelectron spectroscopy (NAP-XPS) studies using 0.2 mbar of CO₂ and at different reaction temperatures has been further performed to better understand the role of the binding sites of upp-HAp. Accordingly, Fig. 4b and c show the high-resolution spectra of the P 2p and Ca 2p regions, respectively. As soon as the CO₂ is introduced in the analysis chamber, the characteristic peaks of P 2p at 134.7 eV (P 2p_3/2) and 135.5 eV (P 2p_1/2) experience a clear shift of 1.6 eV attributed to the adsorption of CO₂ on the PO₄³⁻ basic sites. Moreover, at 95 °C the new species at 132.1 eV (P 2p_3/2) and 132.9 eV (P 2p_1/2) shifted an additional 1 eV, suggesting the subsequent fixation steps of the adsorbed CO₂ molecules. On the other hand, Ca 2p (Fig. 4c) is also affected by the CO₂ atmosphere, shifting from the original binding energy under ultra-high vacuum (UHV) conditions of 348.5 eV (Ca 2p_3/2) and 352.1 eV (Ca 2p_1/2) by 1.3 eV and 2 eV.

As expected, due to its acidic nature, the Ca species remains stable (compared to P) when temperature is increased. Thus, the shift observed is attributed to the 6-fold coordination with the oxygen atoms of the lattice. Moreover, the fact that two different species appear is in agreement with the fact that two distinctive crystallographic sites exist for calcium cations. More specifically, Ca(I) is strictly coordinated with the oxygens from the PO₄³⁻ tetrahedra, while Ca(II) is also coordinated with a hydroxyl group.⁸⁴

The C 1s region has also been examined to further confirm the results obtained. Several interesting insights can be derived from the acquired spectra presented in Fig. 4d. Firstly, the shift of 1.1 eV observed when comparing the CO₂ gas measured far from the surface of upp-HAp (dashed grey line; characteristic peak at 293.7 eV for C 1s which is in agreement with the literature)⁸⁵ confirms the adsorption and activation of the CO₂ molecule (*CO₂) on the surface of upp-HAp, showing an outstanding atomic *CO₂/P ratio of ∼3. These results suggest that apart from the PO₄³⁻ sites, the CO₂ adsorption might also occur on the OH⁻ binding sites. This preliminary experimental evidence of the active role of several binding sites might support the strong affinity towards the catalytic production of C2 and C3 products obtained. This conclusion merits special attention due to the possibility of developing upp-HAp dual site catalysts.

As suggested in Fig. 4d, the initial steps of CO₂ activation can be initiated at 95 °C. Accordingly, an increment of the peak at 288.1 eV, attributed to the O–C=O species, can be observed showing a ratio with adventitious carbon (284.5 eV) of 0.31 (24 °C) and 0.41 (95 °C). Note that during all the experiments samples were kept inside the analysis chamber avoiding the presence and absorption of other carbon-based products on the upp-HAp surface. In contrast, desorption of C–O (contamination during sample preparation) due to temperature can be also observed. To obtain more insights on the fixation mechanism, the temperature of the experiment was finally raised to 120 °C. As can be observed in the inset of Fig. 4d, a small peak appears at 282.1 eV which has been attributed to a partially dissociated C≡O species anchored on the catalyst (resulting in carbidic species). This result supports the unique structural and electronic properties derived from the vacancy engineering and TSP treatments (i.e. superior crystallinity and high charge delocalization) favoring the fast evolution of the generated carbon intermediates. Overall, the combined ¹H NMR and NAP-XPS results allow the first catalytic CO₂ fixation mechanism on upp-HAp (see Fig. 4e) to be proposed which not only supports experimentally the theoretical pathways proposed for HAp⁶⁷ and/or other classical electro-mechanisms²⁸ but also proves the feasibility of performing extremely efficient CO₂ fixation reactions under strictly mild reaction conditions using only upp-HAp as a sustainable and green catalyst. It is worth highlighting the fact that the mechanism proposed involves the C–C coupling by means of a dimerization process, supported by the literature.⁶⁷ This mechanistic pathway requires a high abundance of HCOO⁻ species simultaneously adsorbed on the surface of the catalyst. According to Fig. 4e the presence of water is crucial to do so, which further corroborates the experimental results discussed above.

Kinetics of the CO₂ fixation reaction

Herein, we present a kinetic model for the CO₂ fixation reaction over upp-HAp, which has been developed combining the fixation mechanisms described in the literature⁶⁶ with the experimental results obtained in this work. The main challenge resides in discerning the crucial reaction steps governing the kinetics of the CO₂ fixation, which is essential to discern among the complex known network of intermediate pathways.⁶⁷ Fig. 3d shows that both the total yield and the yields for the individual products present an initial linear behavior (first-order reaction) followed by a stabilization regime (zero-order reaction). This fact clearly indicates a competing phenomenon between the adsorption of reactants and desorption of products. For this reason, the Langmuir–Hinshelwood–Hougen–Watson (LHHW) and the Eley–Rideal (ER) approaches, which are frequently used to model heterogeneous catalysis,^86,87 have been considered to derive the expression of the reaction rate, according to a classical electroreduction mechanism, as follows:

Water splitting:

CO₂ adsorption:

CO₂ fixation:

Chain reaction:

Product desorption:

where * (written as plain text) corresponds to a free binding site while when written as a superscript it is used to denote an adsorbed species (i.e. ). It should be emphasized that the already reported unique electrical and charge storage properties of upp-HAp are, in general, consistent with this classical reduction mechanism.^51,52

In eqn (1)–(7), we propose a four step chain mechanism consisting of:^53,54,67 (1) an initial water splitting reaction in the acid sites (*_a) corresponding to the Ca²⁺ sites of upp-HAp (eqn (1)), occurring simultaneously with CO₂ adsorption in the basic sites (*_b) mainly attributed to the OH⁻ and PO₄³⁻ sites (eqn (2));^87,88 (2) CO₂ fixation into HCOO⁻ due to the addition of a neighboring proton (eqn (3)), which is going to be initially considered as the rate determining step (RDS); (3) chain reaction with adsorbed formic acid (eqn (4)) or less likely, with adsorbed acetic acid (eqn (5)) due to the C–C coupling of two HCOO⁻ adsorbed species through a dimerization process;⁵³ and (4) product desorption (eqn (6) and (7)). Foremost and derived from point (1), the fraction of vacant sites (θ) defined according to the LHHW model has to be described separately for both acid and basic binding sites:

According to the results displayed in Fig. 3f, the term in eqn (9), which accounts for the contribution of the rest of the products adsorbed in the catalyst (including acetic acid), has been assumed to be negligible in light of the adsorbed formic acid content.

Due to the complexity of the system, interesting questions arise related to the contribution of the different chain reactions to the overall kinetics (which might regulate the RDS) and to the competing nature of the water splitting reaction (as a result of the huge proton demand needed to generate the reported products). In order to shed some light, we modeled the kinetics of the CO₂ fixation reaction under different hypotheses and compared the resulting statistical parameters. For this purpose, the minimum value for the sum of squared errors (SSE) was chosen. Also, the variance of the error and the Model Selection Criterion (MSC, eqn S1†),⁸⁹ commonly used in kinetic analyses, were calculated to further confirm the results. The minimum value for variance and higher value for MSC were chosen. A comparison of the different assumptions (hereafter denoted A#) is summarized in Table 2.

Table 2 Statistical parameters obtained from the rate of the expressions considering different assumptions. The principal differences compared to eqn (4)–(9) have been highlighted in different colors (red: different RDSs; blue: water splitting)

Approach	Assumption	SSE (×10^−7)	MSC	Variance error (×10^−7)
A1		6.38	2.953	1.06
A2		2.30	4.196	0.37
A3		3.56	3.759	0.56
	(Modeling the kinetics of total CO2 fixation)
A3*		0.20	6.380	0.03
	(Modeling the kinetics of CH3COOH alone)
A4	– experimentally ruled out	—	—	—
A5		2.27	4.194	0.37

---

As a starting point, assumption A1 was modeled considering that the RDS was eqn (6) and assuming chain reaction with both formic and acetic acids.⁵³ The results showed the worst data correlation (Table 2) and were ruled out. In scenarios A2 and A3, the chain reaction with formic acid alone and the dimerization process (eqn (5)), respectively, were considered as RDS.⁵³ Although both assumptions provided much better statistical data than A1, A2 showed lower SSE and higher MSC values, indicating that the kinetics of the CO₂ fixation is primarily governed by the first fixation step (eqn (3)) and its evolution to formic acid alone. This conclusion is supported by recently reported density functional theory (DFT) calculations used to study the conversion of CO₂ into formic acid.⁹⁰ Moreover, ruling out the A1 approach is also in agreement with other CO₂ fixation mechanisms proposed for both electrocatalysts and thermocatalysts.^53,54,90,91

On the other hand, the synthesis of acetic acid remains extremely limited to eqn (5) (C–C coupling), which acts as the RDS for the latter product in agreement with the experimental results. Accordingly, the expression of the rate from A3 was used to fit the experimental data obtained for acetic acid only (instead of the total CO₂ fixation, A3*), showing excellent statistical results. Despite the fact that the aforementioned conclusion explains the small presence of C2 and C3 adsorbed products (Fig. 3f), the non-negligible amount of acetic acid detected might be contradictory. While remarkable differences in the desorption constants of C2 products (i.e. acetic acid vs. ethanol) have been ruled out, the possibility of re-adsorption of formic acid and its subsequent reaction with adsorbed HCOO⁻ is more plausible. In order to demonstrate this hypothesis, a batch reaction consisting on an inert N₂ atmosphere, with 1 mL of formic acid and 20 mL of water, at 95 °C and for 2 h was carried out. The recorded ¹H NMR showed the unequivocal existence of acetic acid both adsorbed in the catalyst and dissolved in the supernatant (Fig. S8†). Hence, although A3* provides good statistical results, it has to be considered as the very first approach to the specific kinetics of C2 and C3 products, as it has been demonstrated that the re-adsorption and subsequent reaction of C1 products play a considerable role in the final model, increasing remarkably the complexity of the system. This mechanism is currently under study under in situ and operando conditions to support this hypothesis with experimental evidence.

Finally, the nature of the water splitting reaction has been explored. It was experimentally ruled out as the RDS since a first-order reaction regime was found by changing the water content from 1 mL to 80 mL in the batch reactor (Fig. S9†), which is inconsistent with the yields reported in Fig. 3d. Despite this fact, the extensive proton demand suggests that k₁ ≫ k_j. Thus, A5 assumes an almost instantaneous desorption of protons, which results in a non-competing behavior, resembling the ER approach. Surprisingly, statistical data showed slightly better results than A2, implying that the generation of products linearly depends on the initial water concentration without expecting any stagnation. This result is in total agreement with the experimental measurements presented in Fig. 3d. The high proton reactivity and mobility were previously explained from a structural perspective since upp-HAp showed enhanced proton conductivity along different crystalline domains.⁶⁰ Therefore, protons might not be chemisorbed in the acid sites or completely desorbed in the reaction atmosphere but electrostatically attracted to the surface of the catalyst due to the reported charge surface accumulation. Consistently, the null catalytic CO₂ fixation activity found for non-polarized HAp should be related with the lack of protons supplied to the adsorbed CO₂, clearly limiting the RDS.

Due to the resemblance among some results (Table 2) and the mathematical restrictions, the final expression for the rate of total CO₂ fixation reaction was expressed as follows considering A2:

where k₃(T) is the specific constant of the reaction rate (mmol_product·g_cat⁻¹·s⁻¹), k₁ is the water splitting reaction constant (m³ mmol⁻¹), k₆ is the formic acid desorption constant (mmol m⁻³) and [HCOOH] and [H₂O] are the concentrations of the formic acid and water, respectively (mmol m⁻³).

The activation energy E_a was obtained using the temperature studies reported in Fig. 3e and the Arrhenius relation (eqn S2†). Analysis of the kinetic models supports the conclusions derived from the behavior observed in Fig. 3e. Thus, the linear increase of formic acid with temperature, while acetic acid remains stable, is in agreement with assumptions A2 and A3.

Fig. 5a displays the fittings obtained from both total carbon fixation and acetic acid models in conjunction with the experimental results. For the sake of completeness and due to their intrinsic similarities, the same model (eqn (10)) was used to fit the synthesis of formic acid alone. In order to show the good correlation between the experimental data and the points estimated with the kinetic model, a parity plot is presented in Fig. 5b. As can be observed, the predicted model shows an excellent correlation with the experimental results without showing any systematic deviations. Thus, almost all of the points are found inside the ± 10% interval range, with more than 50% of the points located in the ± 5% interval range. Finally, Fig. 5c proves the good correlation (R² = 0.989) between the experimental data and the Arrhenius relation.

Fig. 5 Comparison between the experimental data and the fitting model: (a) fitting of the different experimental yields obtained from the kinetic models proposed; (b) parity plot; and (c) linearization of the Arrhenius expression.

The resulting kinetic parameters are reported in Table 3. k₃(T = 95 °C) presents the smallest value (supporting the RDS A2 assumption), while k₁ (related with the water splitting reaction) is two orders of magnitude higher than the RDS. The value for the activation energy (E_a = 66 ± 1 kJ mol⁻¹) falls within the range of values reported in the literature (40–100 kJ mol⁻¹).^92–95 This can be considered as an outstanding result, as upp-HAp (a biocompatible and cheap ceramic) shows the same catalytic potential than conventional metal-based catalysts (e.g. Cu- and Ni-based)^93,94 with the great advantage that no electric potential (which has been demonstrated to clearly affect the E_a) is applied.

Table 3 Kinetic parameters with their confidence intervals for the CO₂ fixation reaction over p-HAp

Parameter
k1	15.17 ± 1.5 m^3 mmol^−1
k6	0.37 ± 0.06 mmol m^−1−3
k3 (T = 95 °C)	1.43 ± 0.23 × 10^−2 mmolproduct (gc^−1·s^−1)
k0	2.20 ± 0.07 × 10^7 mmolproduct (gc^−1·s^−1)
Ea	66 ± 1 kJ mol^−1

---

Conclusions

We have shown the use of metal-free upp-HAp as a catalyst for the continuous production of formic acid and acetic acid using wet CO₂ as a reagent. Firstly, the distribution of reaction products in the gas, liquid and solid phases, as a function of the reaction time, was investigated for the CO₂ fixation heterogeneous catalytic process using mild reaction conditions (95–120 °C) and both CO₂ gas (6 bar) and liquid water (20 mL) as reagents. Results evidenced the key role of upp-HAp as a catalytic substrate able to adsorb an extremely high ratio of CO₂ in the temperature regime and water during the formation of chemically valuable products that were found to be C1, C2 and C3 reflecting the competition of the two processes: the reduction of CO₂ and the formation of C–C bonds.

A noticeable increment of the reaction yield was observed when the CO₂ conversion process was switched from batch to continuous-flow mode, using identical catalysts. Certainly, the yield obtained (>2 mmol g_c⁻¹·min⁻¹) supposes a great step forward for the use of a competitive green heterogeneous catalyst under strictly mild conditions. Two factors were found to be crucial for the continuous-flow process: (1) the addition of liquid water at the beginning of the process, which can provide an excess of water molecules compared to the process using wet CO₂ as a source of hydrogen, and therefore, enormously increasing the yield of the reaction; and (2) the reaction temperature, depending on whether it is performed above or below 100 °C, since it drastically alters the liquid–gas balance of the water molecules coming from the liquid supplied at the beginning of the process and/or from the wet CO₂, affecting the distribution of the reaction products and the selectivity.

The thermodynamic and kinetic studies performed for the continuous-flow process without considering liquid water as a reactant have provided information on the relevant reaction steps of the mechanism, primarily pointing out the first CO₂ fixation step as the RDS. Although the C–C bond formation is extremely challenging, the kinetic model highlights the fast and independent generation of formic acid (C1 product), boosting the total CO₂ fixation yield. Besides, the competitive adsorption of species in the binding sites has exhaustively been examined, ruling out the contribution of proton adsorption to the overall kinetics, which represents a great advantage in terms of yield optimization and industrial scalability. Finally, the activation energy for the total CO₂ fixation, which has been estimated to be 66 ± 1 kJ mol⁻¹, is within the range of conventional electro-assisted catalysts. In this sense, NAP-XPS experiments further confirm the reaction pathway and mechanism for CO₂ activation occurring in the basic sites of upp-HAp (PO₄³⁻ and OH⁻). Therefore, these preliminary results suggest a synergy between the different binding sites (i.e. dual site catalysis) which would promote the generation of C2 and C3 products. Indeed, the outstanding catalytic activity of upp-HAp for CO₂ fixation and to generate low organic carbon molecules has been demonstrated, representing a feasible, highly efficient, sustainable, green, cheap, and energetically low-demand alternative to conventional electro-assisted catalysts.

Data availability

The data supporting this article have been included as part of the ESI.†

Conflicts of interest

Authors declare that the preparation and application of permanently polarized hydroxyapatite as a catalyst was patented by the Universitat Politècnica de Catalunya and B. Braun Surgical S.A. (EP16382381, EP16382524, P27990EP00, PCT/EP2017/069437, P58656 EP, P59205 EP, P59091 EP, P59008 EP, P59528 EP, 2021P00074 EP, P 59985 EP).

Acknowledgements

This publication and other research outcomes are supported by the predoctoral program AGAUR-FI ajuts (2023 FI-100056) Joan Oró, which is backed by the Secretariat of Universities and Research of the Department of Research and Universities of the Generalitat of Catalunya. This work is part of Maria de Maeztu Units of Excellence Programme CEX2023-001300-M funded by MCIN/AEI/10.13039/501100011033. Authors also acknowledge the Agència de Gestió d'Ajuts Universitaris i de Recerca (2021 SGR 00387) and B. Braun Surgical S. A. U. for their financial support. Support for the research done by C. A. was also received through the prize “ICREA Academia” for excellence in research funded by the Generalitat de Catalunya. J. S. thanks the Spanish Ministry of Universities for the support through a Margarita Salas postdoctoral grant, funded by European Union – NextGenerationEU.

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Footnote

† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d4su00305e

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