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Direct insights into the role of epoxy groups on cobalt sites for acidic H2O2 production


Hydrogen peroxide produced by electrochemical oxygen reduction reaction provides a potentially cost effective and energy efficient alternative to the industrial anthraquinone process. In this study, we demonstrate that by modulating the oxygen functional groups near the atomically dispersed cobalt sites with proper electrochemical/chemical treatments, a highly active and selective oxygen reduction process for hydrogen peroxide production can be obtained in acidic electrolyte, showing a negligible amount of onset overpotential and nearly 100% selectivity within a wide range of applied potentials. Combined spectroscopic results reveal that the exceptionally enhanced performance of hydrogen peroxide generation originates from the presence of epoxy groups near the Co–N4 centers, which has resulted in the modification of the electronic structure of the cobalt atoms. Computational modeling demonstrates these electronically modified cobalt atoms will enhance the hydrogen peroxide productivity during oxygen reduction reaction in acid, providing insights into the design of electroactive materials for effective peroxide production.


Hydrogen peroxide (H2O2) is an important chemical commodity that has been widely used as an environmentally benign oxidant and a potential energy carrier in various applications, including wastewater treatment1, disinfection, chemical synthesis2,3, paper/pulp bleaching, semiconductor cleaning4, and fuel cells5. The global demand of H2O2 is growing rapidly, reaching US$4.0 billion in 2017 and is expected to further increase to around US$5.5 billion by 20236. Currently, over 95% of H2O2 is produced in a concentrated form using the anthraquinone process. This centralized production requires a huge infrastructure investment and high energy inputs, as well as poses safety concerns during the product distribution7. As a matter of fact, in many applications, only dilute H2O2 is required, indicating the concentrated peroxide agent needs to be diluted before usage. Moreover, the generation of organic byproducts and the hazard of handling the concentrated hydrogen peroxide make the anthraquinone method un-ecofriendly and uneconomic. Thus, it is highly desirable to develop green and cost-effective techniques for onsite H2O2 synthesis. Recently, the electrochemical reduction (ER) of oxygen via a selective two-electron transfer pathway has attracted extensive research interest as a promising alternative to the anthraquinone process. The oxygen reduction reaction (ORR) method will enable the decentralized production of H2O2 per demand under ambient reaction conditions without any hazardous byproducts8,9. Furthermore, if the ORR process is integrated with renewable electricity supplies (e.g., generation by photovoltaic cells or wind turbines), the H2O2 generated can be regarded as a renewable chemical10.

More recently, there has been a surge of interest in developing metal-free carbon catalysts for the electro-synthesis of H2O2 via O2 reduction11,12. The electronic structure of these carbon materials can be easily tuned by heteroatom-doping13,14,15 or defect-engineering16,17, thus endowing them high activity and selectivity towards H2O2 production in alkaline electrolytes. However, the production of H2O2 in alkaline media is somewhat constrained by the following limitations: (i) the H2O2 (or HO2 at a pH value above 11.6) tends to readily decompose at basic conditions18; (ii) chelating agents (e.g., ethylenediamine tetraacetic acid) are required to prevent the tramp-metal-ion-induced H2O2 decomposition, thus resulting in the increased operation costs19; (iii) devices (such as fuel cell) based on hydroxide-conducting polymeric electrolytes exhibit low membrane stability, poor water management and low hydrogen oxidation activity20,21. Therefore, it is more desirable to generate H2O2 in acids via ORR. Currently, the state-of-the-art electrocatalysts for H2O2 production in acid are still restricted to the precious-metal-based (e.g., Pt–Hg and Pd–Hg) alloys or amalgams22,23, while their high cost and scarcity have severely hindered their commercial viability. Mesoporous carbon with nitrogen dopants24 or a defective structure25 has emerged as a type of promising catalysts for H2O2 electrosynthesis in acids, owing to their high H2O2 selectivity and low cost. Nevertheless, large amounts of overpotential (>400 mV) are normally associated with these materials to achieve high productivity and selectivity26,27, which has rendered the production process energy inefficient. Hence, the development of highly selective and active catalysts with low cost for electrolytic H2O2 production in acids is highly sought after.

In acids, the selective production of H2O2 via ORR requires the catalyst materials to adsorb the reaction intermediate, namely OOH*, with a suitable binding energy that could facilitate its single-electron reduction to H2O2, but suppress it from being further reduced or dissociated to O* and OH* that will eventually form H2O7,22. Thus far, porphyrins containing 3d transition metals (such as Fe, Ni, and Co) with an optimal binding energy toward OOH* are found to be a type of effective and selective homogeneous catalysts for the electrolytic production of H2O2 in acids28, while the unstable N ligands under the harsh reaction conditions will inevitably result in rapid performance losses29. Therefore, it is of paramount importance to develop an effective method to stabilize these metal-N active species as well as maintain their high selectivity towards H2O2 production under the corrosive reaction environments, such as strong acids.

Forming single-atom catalysts (SACs) on a carbon substrate seems an appealing solution to stabilize the N-coordinated transition-metal centers (metal-Nx). Apart from that, the conductive nature of a carbon substrate will also enable the maximal exposure of the active metal-Nx sites. Compared with other transition metals (like Fe), Co-based composites exhibit less deleterious effects (like the active sites demetalation and Fenton reaction issue) that would eventually lead to the deactivation of the catalysts in acid30. Thus, in this work, a Co and N co-doped carbon nanotubes (CoN@CNTs) composite is prepared and employed as an electrocatalyst for ORR to produce H2O2 in acids. Moreover, by modifying the oxygen functionalities around the Co–Nx sites, significantly enhanced H2O2 catalytic performances can be obtained, showing both high activity (nearly zero overpotential) and selectivity (~100%), and exceeding nearly all the state-of-the-art catalysts and benchmarks reported in literature. Identification of specific oxygen functional groups in promoting the H2O2 production is carried out through a suite of spectroscopic measurements, revealing a synergy between epoxy O and Co–N4 centers, as further confirmed by computational modeling. Finally, by employing the epoxy functionalized CoN@CNTs as the cathode catalyst, a customized H2O2 electrolyzer is fabricated that can easily produce over 0.1 wt% (1199 ppm) H2O2 within 30 min, satisfying most of applications with an electro-Fenton process in water treatment (>10 ppm)1.


Synthesis and characterizations of CoN@CNTs catalysts

The CoN@CNTs composite was prepared by pyrolyzing the carbon and metal precursors in Ar, followed by an acid leaching to remove the accessible metallic debris (see details in the “Methods” section). To characterize the typical structural morphologies of CoN@CNTs, the scanning electron microscopy (SEM) and transition electron microscopy (TEM) were firstly employed. The SEM images (Fig. 1a) show that numerous carbon nanotubes were formed after pyrolysis. Besides that, a bamboo-like feature of the nanotube structure is revealed by the TEM images (Fig. 1b and Supplementary Fig. 1), showing diameters ranging from 50 to 200 nm. Further conducting the high-resolution TEM (HR-TEM) (Supplementary Fig. 1e–g) confirms the graphitic characteristic of the nanotube composite, showing an interlayer spacing of ~0.35–0.36 nm on the CoN@CNTs, which could be ascribed to the (002) plane of graphitic carbon. Notably, the slightly larger d-spacing of the (002) plane than that in a well-ordered structure of graphite (0.33 nm) indicates a somewhat disordered structure of the carbon basal plane in CoN@CNTs, which might be caused by the incorporation of N and Co31. The energy dispersive X-ray spectroscopy (EDS) elemental mapping of a selected area on the CoN@CNTs composite (Fig. 1c and Supplementary Fig. 2) exhibits uniform distributions of the Co, N, O, and C elements across the tubular structure, demonstrating the successful incorporation of Co, N, and O into the carbon substrate. To identify the status of the Co species in CoN@CNTs, the high-angle annular dark field-scanning transmission electron microscopy (HAADF-STEM) measurement was conducted. As shown in Fig. 1d, the bright dots corresponding to Co atoms are homogenously dispersed throughout the CNTs. The statistical distribution of 50 pairs of two adjacent cobalt atoms shows that the Co–Co distances are in the range from 0.2 to 0.8 nm and the majority (~80%) exhibits a distance >0.4 nm (Supplementary Fig. 3), which suggests the dissociation of OOH* intermediate or re-adsorption of hydrogen peroxide by the adjacent Co atoms (less than 4 Å) for the further reduction to water is less likely7. Electron energy loss spectroscopy (EELS) analysis (Fig. 1e) of an area within Fig. 1d further reveals the existence of isolated Co atoms in the carbon matrix. In addition, a very limited amount of Co nanoparticles encapsulated inside 5 to 7 layers of graphitic carbon shells are also observed at the closed end of several carbon nanotubes (Supplementary Fig. 4), while this Co/C core-shell structure imposes negligible impacts on the electrolytic H2O2 production (see details in Supplementary Materials). The X-ray photon spectroscopy (XPS) elemental survey (Fig. 1f) also confirms the existence of Co, N, O, and C on the CoN@CNTs. To further reveal the nature of the isolated Co atoms in CoN@CNTs, X-ray absorption near-edge structure (XANES) and extended X-ray absorption fine structure (EXAFS) measurements (Supplementary Fig. 5) were performed. The higher white line intensity and position compared with Co0 indicates the existence of positively charged Co with an oxidation state in CoN@CNTs. Furthermore, the slightly lower absorption edge position than that of cobalt(II) phthalocyanine (CoPc) suggests the valence state of atomic Co is situated between 0 and 2+. The nearly absent appearance of a pre-edge feature (arisen from the forbidden 1s-to-3d transition) at ~7709 eV in the CoN@CNTs indicates a symmetric coordination environment of Co, e.g., Co–N432. Notably, the Fourier transformed (FT) Co K-edge EXAFS spectra exhibit the signal of light scattering nearest neighbors at ~1.5 Å, corresponding to the Co–N/C scattering pair33,34 and further corroborating the existence of tetrahedrally coordinated Co (e.g., Co–N4)35,36 as revealed by fitting analysis (Supplementary Table 1). The weak signals originated from the Co–Co scattering path in a metallic feature might be ascribed to the rare appearance of Co nanoparticles.

Fig. 1: Microstructural analysis of the CoN@CNTs catalyst.

a SEM images of CoN@CNTs. Inset is the high-resolution SEM image of a selected area of CoN@CNTs. b TEM image of CoN@CNTs showing a bamboo-like structure of the carbon nanotubes. c HAADF–STEM image and corresponding EDS maps of CoN@CNTs for O, N, and Co. d HAADF-STEM image of the CoN@CNTs showing many Co atoms (circled in red) well-dispersed in the carbon layers. e EELS analysis of selected area in d showing the signals of Co. f XPS elemental survey of CoN@CNTs.

Electrochemical measurements and study of active sites

The electrocatalytic performances and efficiency of CoN@CNTs for H2O2 production via ORR were examined in O2-saturated 0.1 M HClO4 using a rotating ring-disk electrode (RRDE) setup. The Pt ring electrode was held at 1.2 V to quantify the amount of H2O2 produced on the disk electrode (see calculation details in the “Methods” section). Figure 2a shows the polarization curve obtained on CoN@CNTs, with the oxygen reduction current measured on the disk electrode (solid lines) and the H2O2 oxidation current measured on the Pt ring electrode (dashed lines). It is apparent that the CoN@CNTs composite exhibits a decent catalytic activity towards the electrolytic production of H2O2 in acid, showing obvious H2O2 oxidation currents at a potential range below 0.7 V. Notably, the majority of electrons is consumed by a 2-electron pathway on the CoN@CNTs, showing a high H2O2 selectivity (~80% from 0.5 to 0.7 V, Supplementary Fig. 6), as determined by RRDE measurements. In contrast, the FeN@CNTs and NiN@CNTs composites prepared via a similar method with an analogous nanotube structure (Supplementary Fig. 7) both exhibit a low H2O2 productivity and selectivity (<40%) within the same potential range, demonstrating the intrinsic active nature of Co–N4 species in selectively reducing O2 to H2O237. Moreover, the Tafel slope of CoN@CNTs is much lower than that of FeN@CNTs and NiN@CNTs (Supplementary Fig. 8), indicating faster ORR kinetics on CoN@CNTs and further suggesting the superior role of Co–N4 species in reducing oxygen.

Fig. 2: Oxygen reduction performance of CoN@CNTs.

a RRDE voltammograms of CoN@CNTs and NG at 1600 rpm in an O2-saturated 0.1 M HClO4 electrolyte with disc current and ring current. b RRDE voltammograms of fresh and aged CoN@CNTs at 1600 rpm in an O2-saturated 0.1 M HClO4 electrolyte with disc current and ring current. All potentials are recorded without iR correction. c XPS elemental survey of CoN@CNTs and aged CoN@CNTs. d XPS O 1s spectra of CoN@CNTs and aged CoN@CNTs.

Furthermore, in the absence of Co species, nitrogen-doped graphene (NG) with a similar amount of N dopants (Supplementary Table 2) to the CoN@CNTs composite exhibits negligible H2O2 production within the whole potential range tested herein (Fig. 2a, blue lines), confirming the prerequisite role of Co–N4 in enabling the efficient H2O2 generation via ORR. The same conclusion can also be obtained with the poisoning experiment, where a significantly receded jdisk was detected after the Co–N4 centers were poisoned by thiocyanate ions (SCN) (details can be found in Supplementary Fig. 9). Similarly, single Co atom embedded mesoporous carbon (M–CoNC, Supplementary Fig. 10) prepared via a different method also exhibits a H2O2-favored ORR process within the same range of potentials, demonstrating the 2-electron-transfer pathway is dominating the O2 reduction process on the Co–N4 sites in acid and precluding the possible effect from the Co/C core-shell structure. Notably, during a three-hour H2O2 production session (Supplementary Fig. 11), the selectivity is maintained at ~78% with negligible drop, showing a decent stability on the CoN@CNTs under the static operation conditions.

However, despite its high catalytic performance, after a long-term (~30 days) exposure to air, the selectivity of the CoN@CNTs composite towards H2O2 production falls dramatically. Figure 2b compares the RRDE curves obtained with freshly prepared CoN@CNTs and CoN@CNTs that has been exposed to air for one month (named as aged CoN@CNTs). It can be seen from Fig. 2b that jring on the aged CoN@CNTs drops significantly meanwhile the jdisk remains almost unchanged (compared with CoN@CNTs), leading to the H2O2 selectivity <30% over the whole potential range. This phenomenon indicates the occurrence of some unwanted oxidation process on the CoN@CNTs composite during the air exposure that has jeopardized its H2O2 productivity. This assumption is further confirmed by the electrochemical measurements of the CoN@CNTs composite that has been stored in vacuum for the same duration, exhibiting almost identical ORR activity and H2O2 selectivity (Supplementary Fig. 12). XPS was utilized to reveal the chemical changes between the CoN@CNTs and aged CoN@CNTs composites. As displayed in Fig. 2c, Supplementary Fig. 13 and Supplementary Table 2, the only noticeable change between these two samples is the increment of O concentration, which rises from 3.50 at% in CoN@CNTs to 5.17 at% in aged CoN@CNTs. More details are provided by the high-resolution XPS O 1s spectra (Fig. 2d) of the two composites, which involve four oxygen components38,39: (i) ketonic oxygen (C=O, O1, 531.2 ± 0.2 eV), (ii) oxygen atoms in epoxy (C–O–C) or hydroxyl groups and carbonyl oxygen in ester groups (O2, 532.3 ± 0.2 eV), (iii) the epoxy oxygen in ester groups (O3, 533.3 ± 0.2 eV), and (iv) oxygen atoms in carboxyl groups (O4, 534.2 ± 0.2 eV). Among all the four O functionalities detected within the composite, only the ketonic groups (O1) have gone through a noticeable increment, of which the concentration has increased from merely 0.84 at% in the fresh sample to 2.64 at% in the aged sample (Supplementary Table 3). This observation suggests that the ketonic groups might be responsible for the receded H2O2 productivity on the aged CoN@CNTs. Therefore, further study is warranted to find an effective method to mitigate the influence of this negative effect.

Electrochemical treatment (ET) is selected here as an approach to in situ re-construct the surface oxygen functionalities on the carbon-based materials. Nevertheless, simply doing ER is hard to remove those oxygen functional groups (like ketonic O) that are thermodynamically more stable than the carboxyl groups40. As expected, the aged CoN@CNTs before and after ER treatment exhibits almost identical chemical properties (Supplementary Fig. 14) as well as H2O2 productivity (Supplementary Fig. 15), suggesting the ineffectiveness of ER in reconstructing the oxygen functionalities on CoN@CNTs. Compared with the ER process, the electrochemical oxidation (EO) treatment is more effective in rebuilding the surface oxygen functional groups on carbon-based materials41. Thus, herein, a two-step electrochemical process combing both EO and ER is adopted to treat the aged CoN@CNTs to modify the O functionalities. Firstly, the aged CoN@CNTs was electrochemically oxidized in the 0.1 M HClO4 solution (EO-CoN@CNTs) by an anodic linear sweep voltammetric scan (details can be referred to Supplementary Fig. 16). Based on the post-reaction XPS measurements (Fig. 3b), the EO treatment endows the aged CoN@CNTs composite a higher O content (12.66 at%, Supplementary Table 2) owing to the highly positive potential applied that caused carbon oxidation. Specifically, the EO-CoN@CNTs exhibits a higher ratio of O2 and O4, while that of ketonic O (O1) decreases, indicating the electrochemical generation of epoxy and carboxyl groups on the CoN@CNTs and a possible conversion of C=O into other O species during this treatment. Then, the EO-CoN@CNTs was subjected to an ER treatment to afford the electrochemically activated CoN@CNTs (EA-CoN@CNTs, Supplementary Fig. 17). From the XPS O 1s spectrum (Fig. 3c) of the EA-CoN@CNTs, it is interesting to note that, after ER process, the ratios of O3 and O4 both drop dramatically (from 33.2 and 24.7% to 15.9 and 6.9% respectively) while that of the O2 becomes dominant (55.8%) compared with those of EO-CoN@CNTs (Supplementary Fig. 18). The significantly reduced amount of O3 and O4 can be correlated to the reduction of some O functional groups (like ester and carboxyl) under a cathodic potential, coinciding with the observations in the previous work40. Epoxy groups are thermodynamically more stable than ester/carboxyl groups38,40, and they are hard to be removed by ER. Therefore, compared with the aged CoN@CNTs, the exclusively increased O2 species in the EA-CoN@CNTs can be attributed to the apparent emergence of epoxy groups on the catalysts. Fourier-transform infrared spectroscopy (FTIR) measurements (Fig. 3d) further confirm the appearance of these epoxy functionalities on the EA-CoN@CNTs, showing a strong and broad absorption band (alkoxy or epoxy C–O) at a region from 1000 to 1200 cm−1 as reported in recent studies42,43.

Fig. 3: Electrochemical activation (EA) of CoN@CNTs.

XPS O 1s spectra of a aged CoN@CNTs, b EO-CoN@CNTs and c EA-CoN@CNTs. d Background-corrected FTIR spectra of CoN@CNTs before and after ETs. e RRDE voltammograms of CoN@CNTs after EA (including EO and then ER) at 1600 rpm in an O2-saturated 0.1 M HClO4 electrolyte with disc current and ring current. f Calculated H2O2 selectivity on CoN@CNTs, aged CoN@CNTs and EA-CoN@CNTs based on the RRDE measurements. g H2O2 production amount (determined via the potassium permanganate titration) as a function of time on the EA-CoN@CNTs. Current (red curve) and concentration (blue ) behavior with time for the electrochemical H2O2 production is shown.

To understand the impact of O functionalities on the Co–N4 centers, N 1s and Co 2p XPS spectra were analyzed on the electrochemically treated samples. The N 1s spectrum shows that pyridonic N has increased substantially after ETs (details can be referred to Supplementary Fig. 19) while the concentration of pyridinic N has decreased, suggesting a possible conversion between these two N species. Thus, it is plausible to postulate that during the ETs, the epoxy groups produced will preferably bond to C atoms that are adjacent to the pyridinic N (coordinated with Co atoms), and consequently transform the pyridinic N to pyridonic N44. This postulation is further supported by the Co 2p3/2 XPS spectrum presented in Supplementary Fig. 20, where the Co–N peak in EA-CoN@CNTs shifts positively to a higher binding energy side (~780.7 eV) than that in the pristine CoN@CNTs (~780.4 eV)45, demonstrating the electro-generated O groups (e.g. epoxy) could be in the vicinity of Co–Nx centers and pose an electron-withdrawing effect that has affected the electronic structure of the Co atoms. In contrast, the ETs show no obvious influence on the valence state of Co species, reflected by the similar spin-energy separation values of samples before and after ETs (Supplementary Fig. 20). Moreover, no leaching of Co in the electrolyte was detected by the inductively coupled plasma mass spectroscopy (ICP-MS) measurement during the ETs, indicating the chemically stable property of the Co sites.

To testify the effectiveness of the ETs, electrolytic H2O2 production over the EA-CoN@CNTs was also evaluated in O2-sat. 0.1 M HClO4 solution. Surprisingly, EA-CoN@CNTs exhibits a superior H2O2 productivity that is even higher than the freshly prepared CoN@CNTs. Specifically, the onset potentials of EA-CoN@CNTs at the ring and disk coincide at ~0.7 V (Fig. 3e), which is the thermodynamic onset potential of the genuine 2-electron pathway of ORR in acid for H2O2 production22. As the overpotential increases, most of the jdisk recorded on EA-CoN@CNTs can be accounted for the production of H2O2. The selectivity of H2O2 production is well above 90% within a region between 0.3 and 0.6 V (Fig. 3f) based on the RRDE measurement, indicating a nearly complete 2-electron ORR process on the EA-CoN@CNTs. Also, at a potential of 0.3 V, the j on the disk (0.125 cm2) achieves 3 mA cm−2, which is close to the theoretical mass transport limit for the 2-electron reduction of oxygen22. To investigate the Faradaic efficiency (FE) and stability of EA-CoN@CNTs during bulk electrolysis, the electrocatalytic H2O2 production and accumulation through ORR was carried out in a H-cell setup separated by a Nafion membrane with continuous O2 bubbling. The FE was verified for the purpose of a more intuitive demonstration employing permanganate titration (average of three repetitions)22 within a range of potentials from 0.45 to 0.65 V. Of note, the titration results (Supplementary Fig. 21) exhibit a FE as high as 95%, which coincides with the RRDE results. The long-term stability performed via a chronoamperometric measurement at 0.45 V for 12 h (Fig. 3g) yields a current of ~10 mA, during which the concentration of accumulated H2O2 also increased continuously. The slight drop in current was attributed to the possible attachment of some species (like cations or H2O2) on the surface of electrode, and this can be recovered after changing the electrolyte and rinsing the electrode (Supplementary Fig. 22). From the electrochemical results shown above, it is evident that the synergistic effect between Co–N4 centers and their adjacent C–O–C groups plays an advocating role in reducing oxygen exclusively to H2O2, which makes the EA-CoN@CNTs among the most effective catalyst for electrolytic H2O2 production in acids (Supplementary Table 4).

C–O–C groups on carbon can also be introduced through chemical approaches and H2O2 treatment (HT) was previously found to be an effective method46. Hence, to further understand the critical role of epoxy functionalized Co–N4 centers in promoting the 2-electron ORR for H2O2 production, aged CoN@CNTs sample was chemically treated in 0.1 M HClO4 solution containing 5 wt% H2O2 at 70 °C for 2 h. A dominant presence of epoxy groups is detected by both XPS (Supplementary Fig. 23a) and FTIR (Supplementary Fig. 23b) on the H2O2-treated CoN@CNTs (HT-CoN@CNTs), accompanied by a significantly reduced intensity of the ketonic group, suggesting the effectiveness of this treatment. As expected, HT-CoN@CNTs exhibits a much higher H2O2 selectivity (Supplementary Fig. 24a) as well as productivity (Supplementary Fig. 24b) than the aged CoN@CNTs, echoing the findings from the ETs. Thus, to further enhance the H2O2 productivity of the CoN@CNTs composite, both HT and electrochemical activation (EA) methods were applied together (see details in the “Methods” section) on the aged CoN@CNTs sample to obtain the HE-CoN@CNTs. As expected, a high content of O (12.3 at%) and the highest ratio of epoxy groups (71.3%) among all samples prepared were obtained (Supplementary Fig. 25a and Table 3), accompanied by an obviously increased ratio of pyridonic N (Supplementary Fig. 25b). The HE-CoN@CNTs exhibits, to the best of our knowledge, a record-breaking catalytic performance towards H2O2 production in acid. Shown in Fig. 4a, b, with the onset potential at 0.7 V, the HE-CoN@CNTs composite is capable of maintaining a nearly 100% selectivity of H2O2 production within a wide potential range from 0.3 to 0.6 V (>95%), exceeding the catalytic performances of those benchmarks and state-of-the-art catalysts, including precious metals, their alloys and recently reported carbon-based materials (Fig. 4c, Supplementary Table 4), in terms of both overpotential and selectivity. In contrast, the NG exhibits a much lower H2O2 current within the same potential range even after the H2O2 treatment and ETs (Supplementary Fig. 26), further advocating the importance of synergies between CoN4 active sites and nearby C–O–C groups. Post-reaction characterizations (XPS and FTIR, Supplementary Figs. 27 and 28) show negligible changes on the HE-CoN@CNTs after a 12-h reaction session, evidencing the fact that not only the Co species, but also the epoxy groups are stable during ORR. In addition, the catalytic activity and H2O2 selectivity is kept almost unchanged on the HE-CoN@CNTs sample even after long-term aging period in air. This is due to the chemically stable property of these epoxy functionalities on catalysts that eventually benefit a well retained H2O2 selectivity after aging, as revealed by FTIR and XPS O 1s spectra (Supplementary Fig. 29). Moreover, within a gas diffusion electrode (GDE, Supplementary Fig. 30) setup, the H2O2 concentration could be easily accumulated to 1199 ppm within 30 min at 0 V, which is sufficient for direct usage in industries like water disinfection and bleaching1. At a more moderate potential (0.3 V, Supplementary Fig. 31), 5525 ppm of H2O2 is produced within 12 h, giving the energy-efficient feature of this process as less overpotentials are required. Notably, even when the reaction is conducted using air bubbling (Fig. 4b), the H2O2 selectivity is still maintained at >80% within the whole voltage range, demonstrating its potential to be applied in practical applications.

Fig. 4: ORR activities of HE-CoN@CNTs and DFT results of different types of epoxy-modified Co–N4 sites.

a RRDE measurements of HE-CoN@CNTs for ORR in 0.1 M HClO4 solution purged with O2 and air. b Calculated H2O2 selectivity on HE-CoN@CNTs in O2- and air-saturated 0.1 M HClO4 based on the RRDE measurements. c H2O2 selectivity on HE-CoN@CNTs and other recently reported catalysts (Supplementary Table 4) in acidic media. d Calculated Sabatier volcano plot for the 2-electron ORR to H2O2 for bare CoN4 moiety and CoN4 moieties with different epoxy oxygen coverages obtained from DFT simulations. The UL is plotted as a function of \(\Delta {\mathrm{G}}_{{\mathrm{HOO}}^ \ast }\). The black solid lines represent the theoretical Sabatier volcano22. The black squares are the data adapted from ref. 22. e The optimized geometry structures of bare CoN4 moiety and CoN4 moieties with different epoxy oxygen coverages, which were chosen to calculate the ORR activities in this work. Here, CoN4 indicates bare CoN4 moiety. CoN4 (1O), CoN4 (2O), and CoN4 (3O) indicate CoN4 moieties with 1, 2 or 3 epoxy oxygen, respectively. The gray, blue, orange and red balls represent C, N, Co and O atoms, respectively.

To further corroborate the correlation between the emerged epoxy oxygen and the enhanced H2O2 selectivity, near-edge X-ray absorption fine structure (NEXAFS) measurements were performed on the post-treated CoN@CNTs samples. As shown in Supplementary Fig. 32a, high-resolution oxygen K-edge NEXAFS results of EO-CoN@CNTs, EA-CoN@CNTs, HT-CoN@CNTs and HE-CoN@CNTs all exhibit obvious features at ~533.4 and 534.8 eV, corresponding to transitions of O 1s core level electrons to final states of π* symmetry localized at C–O bond of epoxy groups14,47,48,49. The intense peak arisen at around 539 eV in the spectra curves of those samples after chemical and/or ETs can be ascribed to the transitions to σ* states of C–O bonding from ring C–O–C functionalities48, further confirming the emergence of epoxy O. Notably, the bisphenol A diglycidyl ether (BADGE) composite gives rise to obvious π* and σ* resonances at around 534.2 and 539.0 eV (Supplementary Fig. 32a), respectively, signifying the emergence of C–O–C groups in our samples. The split of antibonding π* symmetry of C–O bond in the post-treatment CoN@CNTs is probably ascribed to the high coverages of epoxy functionalities on the surface of carbon basal plane47. In addition, Co L-edge spectra (Supplementary Fig. 32b) show significant fine-structure at L3 peak due to the multiplet structure from electron-electron interaction, which depends greatly on the local coordination symmetry of Co sites. As expected, the CoN@CNTs sample exhibits the signatures of CoNx moieties very close to Co–N–C catalysts in previous reports30, suggesting a tetrahedrally coordinated (Td) symmetry of Co atoms in our catalysts, which is consistent with the XANES Co K-edge results. The spectra of EA-CoN@CNTs, HE-CoN@CNTs and EO-CoN@CNTs show promiment fine-structure features at 778.5 and 779.0 eV, which are similar to the oxygen-induced distored CoN4 functionalities as reported previously50, causing a “octahedral-like” symmetry on the Co sites by nearby O atoms. Notably, the increases in overall intensity for those epoxy-modified samples (EA-CoN@CNTs, HE-CoN@CNTs and EO-CoN@CNTs) are acribed to electrons transferring away from the Co atoms, strongly implicating that nearby O atoms from epoxy groups are modifying the electronic structure of the Co sites (e.g., electron-withdrawing effect) and thus their ability to selectively produce hydrogen peroxide. NEXAFS Co L-edge spectrum from bulk Co3O4 reference is shifted to higher energy as expected for increase in oxidation state, suggesting that bulk oxidiation is not found in our materials during the electrochemical and chemical treatments.

Theoretical simulations

The above experimental results demonstrated that the electrochemical/chemical treatments of CoN@CNT generate abundant amounts of epoxy groups, which may tailor the electronic structure of the CoN4 moieties and significantly improve their 2-electron-pathway ORR activity for the H2O2 production. To elucidate the mechanism within this enhancement effect, density functional theory (DFT) calculations were performed. Extensive details regarding the calculations are available in the Supplementary Materials. Here we considered epoxy oxygen on CoN4 catalysts with different coverage and locations (Supplementary Figs. 33 and 34), and chose the possible structures (Fig. 4e) with low epoxy oxygen formation energy (\(E_{{\mathrm{ep}} - {\mathrm{O}}}^F\)) to calculate the ORR activity. Supplementary Fig. 35 shows the free-energy diagrams for the 2-electron ORR to H2O2 at the equilibrium potential (\(U_{{\mathrm{O}}_2/{\mathrm{H}}_2{\mathrm{O}}_2}^0 = 0.70\,{\mathrm{V}}\)), and the theoretically calculated ORR volcano plot for the 2-electron pathways is given in Fig. 4d. It can be seen from Fig. 4d and Supplementary Fig. 35 that the introduction of epoxy groups close to CoN4 moiety dramatically weaken the binding strength of HOO* on the Co atoms. Especially for the structures of CoN4 moiety with 2 or 3 epoxy oxygens, the computed values of \(\Delta G_{{\mathrm{HOO}}^ \ast }\) for CoN4 (2O) and CoN4 (3O) are 4.22 and 4.20 eV, respectively, which are located at the peak of the 2-electron volcano with UL = 0.70 and 0.68 V, respectively. These results suggest that the CoN4 moiety with nearby epoxy groups exhibits their superior activity and selectivity of the 2-electron ORR to H2O2 with the overpotentials less than 0.02 V, which are comparable or even lower than that of the state-of-the-art PtHg4 for the 2-electron ORR to H2O2 in acidic conditions (η < 0.10 V)22. In contrast, the epoxy oxygen formed at the carbon atoms far from the Co–N4 centers (Supplementary Fig. 33) exhibits negligible effect in optimizing the binding energy of HOO* intermediate at Co sites, indicating the importance of synergies between CoN4 moieties and those nearby epoxy groups. The Bader analysis reveals that the decrease of \({\mathrm{\Delta }}G_{{\mathrm{HOO}}^ \ast }\) for CoN4 moiety with epoxy groups is due to the electro-withdrawing groups51, i.e., epoxy oxygen, deplete the electrons on Co atom of CoN4 moiety. For example, the electrons on Co are +0.92e and +0.97e for CoN4 and CoN4 (3O), respectively, based on the Bader analysis, echoing with the electron-transferring effect between Co and nearby O atoms observed in NEXAFS measurements. Furthermore, the climbing image nudged elastic band (CI-NEB) method is also performed to calculate the chemical dissociation barrier of HOO* on the active site, elucidating the origin of the H2O2 selectivity on the epoxy-modified CoN4 sites. As expected, the dissociation energy of HOO* on the CoN4 sites is high (1.4 eV), and that can be further increased after epoxy-modification (Supplementary Fig. 36), suggesting the possible O–O bond session could be effectively suppressed on the epoxy-modified CoN4 moieties that in turn benefit an improved H2O2 selectivity. This is further supported by the previous hypothesis that the chemical cleavage of O–O bond by the adjacent carbon atoms near the M–N sites could be sterically blocked by their surrounding oxygen groups46.


While the above results unequivocally confirm the synergies between epoxy oxygen and CoN4 species in promoting the H2O2 productivity, the possible effect of limited amount of hydroxyl groups in influencing the ORR selectivity cannot be fully excluded. Thus, the role of hydroxyl oxygen on the H2O2 productivity is also evaluated as it may cast a similar influence on the CoN4 centers. As expected, simulation results reveal a similar electron-withdrawing effect of –OH functionalities on the CoN4 species (Supplementary Fig. 37), which might facilitate the H2O2 formation. Nevertheless, the binding energy of OOH* on the hydroxyl-modified CoN4 centers is still not as optimal as that on the epoxy-modified active sites (Supplementary Fig. 35). Moreover, in this study, the possible origin of H2O2 selectivity from the synergies between –OH species and CoN4 sites are further precluded by a set of experiments. Hot-alkaline treatment is regarded as effective in introducing –OH groups as well as converting C–O–C functionalities into other species52. Thus, the aged CoN@CNTs sample was heated in concentrated KOH solution (see details in “Methods”), generating an ample amount of hydroxyl oxygen but no obvious C–O–C groups were observed (Supplementary Fig. 38). Notably, no enhancement of H2O2 selectivity was identified on the hot-alkaline-treated sample, suggesting a limited effect of –OH groups in affecting the H2O2 formation. Therefore, it can be concluded that the significantly enhanced H2O2 selectivity on the CoN4 active sites is mainly due to the emergence of epoxy oxygen rather than hydroxyl groups near the Co atoms. Previous reports suggest that oxidation of carbon can significantly influence the H2O2 performance on M–N–C (M = Co, Fe, Mn) catalysts46,53. However, no direct correlations between specific oxygen functionalities and H2O2 selectivity has been established, causing a debate on the real origin of H2O2 selectivity as the influence of diverse O groups cannot be universal. Herein, the enhancement effect of epoxy groups on H2O2 selectivity is answered systematically, providing guidelines in not only design of efficient catalysts for peroxide production but also stabilizing the performance of SACs in acidic fuel cells. Further, all these experiments and simulations strongly prove the effectiveness of our electrochemical/chemical approach in tuning the selectivity of O2 reduction through surface reconstruction on carbon-based materials, which could be readily adopted for other selectivity-critical electrochemical reactions, like N2 or CO2 reduction.

In summary, the DFT calculation provides an explanation for the synergistic effects observed experimentally over the EA-CoN@CNTs and HE-CoN@CNTs composites with significantly improved activity as well as selectivity towards H2O2 production in acidic electrolytes. The electronic structure of Co–N4 centers has been tuned by the presence of epoxy groups that are adjacent to them, resulting in the close-to-ideal binding energy that allows the ORR to proceed via a nearly complete two-electron transfer pathway to produce H2O2. Both the EA-CoN@CNTs and HE-CoN@CNTs composites exhibit record-breaking H2O2 productivity, outperforming nearly all the catalyst materials reported previously. Further optimizations of the catalyst materials as well as devices obtained in this study, including improved long-term stability (up to several thousand hours), faster mass transport in the electrolyzer and accelerated H2O2 production rate in air54,55, will be carried out to warrant their future practical applications.



All reaction reagents and chemicals were obtained and used in their as-received form without any further purification. Dicyandiamide, Co(NO3)2·6H2O, Ni(NO3)2·6H2O, Fe(NO3)3·9H2O, Nafion solution (5 wt%) and cobalt(II) phthalocyanine (CoPc) were obtained from Sigma-Aldrich. Deionized water was obtained through the water purification system (Milli-Q water) in the lab.

Synthesis and surface treatments of CoN@CNTs

Typically, to prepare the CoN@CNTs catalyst, 3.5 mmol Co(NO3)2·6H2O, 35 mmol dicyandiamide and 2 mL ethanol were mixed in an agate mortar, followed by continuous grinding until the mixture forms a uniform pink paste. The as-obtained mixture was placed into a crucible boat and heated to 800 °C with a ramping rate of 3 °C min−1 for 3.5 h under Ar atmosphere. The impurities and undesirable nanoparticles outside the carbon nanotubes were removed through an acid leaching process in 0.5 M H2SO4 at 90 °C for 4 h, followed by repeatedly filtered and washed process in deionized water. The FeN@CNTs and NiN@CNTs were prepared using the similar pyrolysis process by changing the type of metal nitrate in the precursors. The effect of carbonization time on H2O2 productivity was investigated in detail, and we found that CoN@CNTs pyrolyzed at 800 °C for 3.5 h yields the highest ORR activity towards H2O2 production (Supplementary Fig. 39). The M–CoNC composite was synthesized via a modified method as reported previously56. The polymerized OPD (Phenylenediamine, Sigma Aldrich, 99.99%) in presence of hydrochloric acid and APS (Ammonium persulfate, Sigma Aldrich, 99.99%) was mixed with Co(NO3)2·6H2O and then pyrolyzed at 900 °C under Ar for 2 h to form M–CoNC. NG was directly purchased from Sigma Aldrich (99.99%). To obtain the HT-CoN@CNTs, the CoN@CNTs powder was dispersed and heated in 50 mL 0.1 M HClO4 solution containing 5 wt% H2O2 under 70 °C for 2 h. The EA-CoN@CNTs was obtained by oxidizing the CoN@CNTs electrochemically through conducting an anodic linear sweep voltammetric scan from 1.2 to 2.4 V vs. RHE, followed by an ER process via a cathodic linear sweep voltammetric scan from 0.6 to −0.6 V vs. RHE. To prepare the HE-CoN@CNTs, the CoN@CNTs sample was treated through a combined HT and EA process. Hot-alkaline treatment was conducted by heating the aged CoN@CNTs sample in 6 M KOH solution with an autoclave reactor under 180 °C for 12 h.

Physicochemical characterizations

Transmission electron microscopy (TEM) was carried out on a Phillips/CM 200 microscope operated at an accelerating voltage of 200 kV. SEM was conducted on a JEOL 7001F operated at 5 kV. FTIR measurements were conducted on a PerkinElmer FTIR Spectrometer. X-ray photoelectron spectroscopy (XPS) measurements were carried out on a Thermo ESCALAB250Xi X-ray photoelectron spectrometer using Cu Kα X-rays as the excitation source with a voltage of 12.5 kV and power of 250 W. High-angle annular dark field-scanning transmission electron microscopy (HAADF-STEM) and energy dispersive X-ray (EDX) mapping were obtained on a spherical aberration corrected transmission electron microscope (FEI Titan G2 80–200) which was operated at 200 kV. ICP-MS was carried out using a PerkinElmer quadrapole Nexion instrument. Co K-edge X-ray absorption spectroscopy (XAS) measurements were performed at the 10-ID-B beamline of the Advanced Photon Source (APS), Argonne National Laboratory (ANL). Data were collected using a fluorescence geometry and scanned from 200 eV below the Co K-edge (7709 eV) to ~1000 eV past the edge. Data reduction and subsequent modeling efforts were performed using the Demeter software package57. Modeling results used a Co-(N3C2)2 cluster to modeling Co–N and Co–C backscattering paths58. An S02 value of 0.776 was used for all models and obtained from modeling a reference Co foil. O K-edge and Co L-edge NEXAFS measurements were performed at the SXR beamline of the Australian Synchrotron. Powders were pressed onto Ir foil and mounted onto metallic sample holders for measurements under partial electron yield (PEY) mode. O K-edge measurements were performed from 520 eV to 580 eV while Co L-edge measurements were performed from 770 to 810 eV and internally calibrated using MnO and Co foil reference samples respectively. All data processing, energy calibrations, and normalization was performed using the program QANT.

DFT calculations

All of the spin-polarized DFT calculations were performed using the VASP program59,60,61, which uses a plane-wave basis set and a projector augmented wave method (PAW) for the treatment of core electrons59. The Perdew, Burke, and Ernzerhof exchange-correlation functional within a generalized gradient approximation (GGA-PBE)62 was used in our calculations, and the van der Waals (vdW) correction proposed by Grimme (DFT-D3) was employed due to its good description of long-range vdW interactions63. For the expansion of wavefunctions over the plane-wave basis set, a converged cutoff was set to 400 eV. Dipole correction was considered in all cases. Extensive details were given in from Supplementary Figs. 3337.

Electrochemical measurements

The electrochemical tests were all performed in 0.1 M HClO4 aqueous solution within a three-electrode system at room temperature on a computer-controlled potentiostat (CH Instrument, CHI 760E). The oxygen reduction activity and selectivity were investigated by polarization curves and rotating ring-disk electrode (RRDE) measurements in oxygen-saturated electrolyte with a scan rate of 5 mV s−1. A glassy carbon electrode loaded with catalyst was used as the working electrode. A graphite rod and a saturated calomel electrode were used as counter and reference electrode respectively. To prepare the working electrode loaded with the catalyst, typically, 5 mg as-prepared catalyst and 25 μL Nafion solution (Sigma Aldrich, 5 wt %) were dispersed in 1 mL ethanol aqueous solution (50%) to form a homogeneous ink with the help of a sonication process for 30 min. Then, 6.5 μL of the ink was dropcasted onto the surface of a polished glassy carbon electrode and dried under room temperature in atmosphere. The final loading of the catalysts on working electrode was 0.25 mg cm−2. Commercially available Pt/C catalyst (20 wt% of Pt, Sigma-Aldrich) was employed as the benchmark for 4e ORR process to testify the electrochemical testing conditions in acid (Supplementary Fig. 40). All of the obtained potentials were calibrated to a reversible hydrogen electrode (RHE, ERHE = ESCE + 0.2415 + 0.059 × pH). No correction of the system resistance was employed. The Tafel slope was calculated using the Tafel equation: η = b log (j/jo) (η, b, j, and jo represent the overpotential, Tafel slope, current density and exchange current density respectively).

H2O2 selectivity of the catalysts was calculated from the current of both disc and ring electrodes using the following equation:

$${\mathrm{H}}_{\mathrm{2}}{\mathrm{O}}_{\mathrm{2}}\left( {\mathrm{\% }} \right) = {\mathrm{200}} \times {\mathrm{I}}_{\mathrm{r}}{\mathrm{/N/}}\left( {{\mathrm{I}}_{\mathrm{d}}{\mathrm{ + I}}_{\mathrm{r}}{\mathrm{/N}}} \right)$$

where Id is disk current, Ir is ring current, and N is current collection efficiency of the Pt ring. N was determined to be 0.32 in our system after calibration using the reversible [Fe(CN)6]4−/3− redox couple (+0.36 vs. SHE). A potential of 1.2 V vs. RHE was applied on the Pt ring of the working electrode at a speed of 1600 r.p.m. during the entire testing process.

FE and electrocatalytic production of H2O2 were measured in a two-compartment cell with Nafion membrane as separator. Both the cathode compartment (75 mL) and anode compartment were filled with 0.1 M HClO4 aqueous solution. Oxygen was continuously purged into the cathode (working) compartment under vigorous stirring. A graphite rod and a saturated calomel electrode were used as counter and reference electrode respectively. A hydrophobic carbon fiber paper (CFP) loaded with as-prepared CoN@CNTs catalyst (0.5 mg cm−2) was used as the working electrode.

To quantify the amount of H2O2 produced, we carried out an independent test not based on electrochemical methods: permanganate titration. Typically, samples with a volume of 1 mL collected at certain time intervals were diluted into 10 mL and titrated with 0.005 M KMnO4 aqueous solution. The concentration of H2O2 produced was calculated according to the following equation:

$${\mathrm{C}}_{{\mathrm{H2O2}}} = {\mathrm{ 5C}}_{{\mathrm{KMnO4}}} \times {\mathrm{V}}_{{\mathrm{KMnO4}}} \div {\mathrm{2V}}_{{\mathrm{H2O2}}}$$

where CH2O2 is the H2O2 concentration (mol L−1), CKMnO4 is the precise concentration of KMnO4 solution (mol L−1), VKMnO4 is the volume of KMnO4 solution consumed during titration (mL), VH2O2 is the volume of H2O2 solution.

Data availability

The data that support the plots within this paper and other findings of this study are available from the corresponding author upon reasonable request.


  1. 1.

    Brillas, E., Sirés, I. & Oturan, M. A. Electro-fenton process and related electrochemical technologies based on fenton’s reaction chemistry. Chem. Rev. 109, 6570–6631 (2009).

    CAS  PubMed  Google Scholar 

  2. 2.

    Puértolas, B., Hill, A. K., García, T., Solsona, B. & Torrente-Murciano, L. In-situ synthesis of hydrogen peroxide in tandem with selective oxidation reactions: a mini-review. Catal. Today 248, 115–127 (2015).

    Google Scholar 

  3. 3.

    Agarwal, N. et al. Aqueous Au-Pd colloids catalyze selective CH4 oxidation to CH3OH with O2 undermild conditions. Science 358, 223–227 (2017).

    ADS  CAS  PubMed  Google Scholar 

  4. 4.

    Seh, Z. W. et al. Combining theory and experiment in electrocatalysis: insights into materials design. Science 355, eaad4998 (2017).

    PubMed  Google Scholar 

  5. 5.

    Fukuzumi, S., Lee, Y. M. & Nam, W. Solar-driven production of hydrogen peroxide from water and dioxygen. Chem. A Eur. J. 24, 5016–5031 (2018).

    CAS  Google Scholar 

  6. 6.

    Imarc group, “Hydrogen Peroxide Market Trends, Share, Growth and Forecast 2018–2023”. (2019).

  7. 7.

    Yang, S. et al. Toward the decentralized electrochemical production of H2O2: a focus on the catalysis. ACS Catal. 8, 4064–4081 (2018).

    CAS  Google Scholar 

  8. 8.

    Berl, E. A new cathodic process for the production of H2O2. J. Electrochem. Soc. 76, 359–369 (1939).

    Google Scholar 

  9. 9.

    Zheng, Z., Ng, Y. H., Wang, D. W. & Amal, R. Epitaxial growth of Au–Pt–Ni nanorods for direct high selectivity H2O2 production. Adv. Mater. 28, 9949–9955 (2016).

    CAS  PubMed  Google Scholar 

  10. 10.

    Chen, Z. et al. Development of a reactor with carbon catalysts for modular-scale, low-cost electrochemical generation of H2O2. React. Chem. Eng. 2, 239–245 (2017).

    Google Scholar 

  11. 11.

    Jiang, Y. et al. Selective electrochemical H2O2 production through two-electron oxygen electrochemistry. Adv. Energy Mater. 8, 1801909 (2018).

    Google Scholar 

  12. 12.

    Melchionna, M., Fornasiero, P. & Prato, M. The rise of hydrogen peroxide as the main product by metal-free catalysis in oxygen reductions. Adv. Mater. 31, 1802920 (2018).

    Google Scholar 

  13. 13.

    Lu, Z. et al. High-efficiency oxygen reduction to hydrogen peroxide catalysed by oxidized carbon materials. Nat. Catal. 1, 156–162 (2018).

    CAS  Google Scholar 

  14. 14.

    Kim, H. W., Ross, M. B., Kornienko, N., Zhang, L. & Guo, J. Efficient hydrogen peroxide generation using reduced graphene oxide based oxygen reduction electrocatalysts. Nat. Catal. 1, 282–290 (2018).

    Google Scholar 

  15. 15.

    Chen, S. et al. Designing boron nitride islands in carbon materials for efficient electrochemical synthesis of hydrogen peroxide. J. Am. Chem. Soc. 140, 7851–7859 (2018).

    CAS  PubMed  Google Scholar 

  16. 16.

    Han, L. et al. In-plane carbon lattice-defect regulating electrochemical oxygen reduction to hydrogen peroxide production over nitrogen-doped graphene. ACS Catal. 9, 1283–1288 (2019).

    CAS  Google Scholar 

  17. 17.

    Sa, Y. J., Kim, J. H. & Joo, S. H. Active edge-site-rich carbon nanocatalysts with enhanced electron transfer for efficient electrochemical hydrogen peroxide production. Angew. Chem. Int. Ed. 58, 1100–1105 (2019).

    CAS  Google Scholar 

  18. 18.

    Campos-Martin, J. M., Blanco-Brieva, G. & Fierro, J. L. G. Hydrogen peroxide synthesis: an outlook beyond the anthraquinone process. Angew. Chem. Int. Ed. 45, 6962–6984 (2006).

    CAS  Google Scholar 

  19. 19.

    Hess, W. T. “Hydrogen Peroxide” in Kirk-Othmer Encyclopedia of Chemical Technology. ed. 4, Vol. 13, 961–995 (Wiley, New York, 1995). .

  20. 20.

    Ayers, K. E., Dalton, L. T. & Anderson, E. B. Efficient generation of high energy density fuel from water. ECS Trans. 41, 27–38 (2012).

    CAS  Google Scholar 

  21. 21.

    Sheng, W., Gasteiger, H. A. & Shao-Horn, Y. Hydrogen oxidation and evolution reaction kinetics on platinum: acid vs alkaline electrolytes. J. Electrochem. Soc. 157, B1529 (2010).

    CAS  Google Scholar 

  22. 22.

    Siahrostami, S. et al. Enabling direct H2O2 production through rational electrocatalyst design. Nat. Mater. 12, 1137–1143 (2013).

    ADS  CAS  PubMed  Google Scholar 

  23. 23.

    Verdaguer-Casadevall, A. et al. Trends in the electrochemical synthesis of H2O2: enhancing activity and selectivity by electrocatalytic site engineering. Nano Lett. 14, 1603–1608 (2014).

    ADS  CAS  PubMed  Google Scholar 

  24. 24.

    Fellinger, T. P., Hasché, F., Strasser, P. & Antonietti, M. Mesoporous nitrogen-doped carbon for the electrocatalytic synthesis of hydrogen peroxide. J. Am. Chem. Soc. 134, 4072–4075 (2012).

    CAS  PubMed  Google Scholar 

  25. 25.

    Liu, Y., Quan, X., Fan, X., Wang, H. & Chen, S. High-yield electrosynthesis of hydrogen peroxide from oxygen reduction by hierarchically porous carbon. Angew. Chem. Int. Ed. 54, 6837–6841 (2015).

    CAS  Google Scholar 

  26. 26.

    Iglesias, D. et al. N-doped graphitized carbon nanohorns as a forefront electrocatalyst in highly selective O2 reduction to H2O2. Chem 4, 106–123 (2018).

    CAS  Google Scholar 

  27. 27.

    Sun, Y. et al. Efficient electrochemical hydrogen peroxide production from molecular oxygen on nitrogen-doped mesoporous carbon catalysts. ACS Catal. 8, 2844–2856 (2018).

    CAS  Google Scholar 

  28. 28.

    Gouérec, P. & Savy, M. Oxygen reduction electrocatalysis: ageing of pyrolyzed cobalt macrocycles dispersed on an active carbon. Electrochim. Acta 44, 2653–2661 (1999).

    Google Scholar 

  29. 29.

    Mase, K., Ohkubo, K. & Fukuzumi, S. Efficient two-electron reduction of dioxygen to hydrogen peroxide with one-electron reductants with a small overpotential catalyzed by a cobalt chlorin complex. J. Am. Chem. Soc. 135, 2800–2808 (2013).

    CAS  PubMed  Google Scholar 

  30. 30.

    He, Y. et al. Highly active atomically dispersed CoN4 fuel cell cathode catalysts derived from surfactant-assisted MOFs: carbon-shell confinement strategy. Energy Environ. Sci. 12, 250–260 (2019).

    CAS  Google Scholar 

  31. 31.

    Wu, G., More, K. L., Johnston, C. M. & Zelenay, P. High-performance electrocatalysts for oxygen reduction derived from polyaniline, iron, and cobalt. Science 332, 443–447 (2011).

    ADS  CAS  PubMed  Google Scholar 

  32. 32.

    Wang, X. X. et al. Nitrogen-coordinated single cobalt atom catalysts for oxygen reduction in proton exchange membrane fuel cells. Adv. Mater. 30, 1706758 (2018).

    Google Scholar 

  33. 33.

    Yin, P. et al. Single cobalt atoms with precise N-coordination as superior oxygen reduction reaction. Catalysts. Angew. Chem. Int. Ed. 55, 10800–10805 (2016).

    CAS  Google Scholar 

  34. 34.

    Zhang, L. et al. Coordination of atomic Co–Pt coupling species at carbon defects as active sites for oxygen reduction reaction. J. Am. Chem. Soc. 140, 10757–10763 (2018).

    CAS  PubMed  Google Scholar 

  35. 35.

    Gong, W. et al. Nitrogen-doped carbon nanotube confined Co-Nx sites for selective hydrogenation of biomass-derived compounds. Adv. Mater. 31, 1808341 (2019).

    Google Scholar 

  36. 36.

    Sun, X. et al. Single cobalt sites in mesoporous N-doped carbon matrix for selective catalytic hydrogenation of nitroarenes. J. Catal. 357, 20–28 (2018).

    Google Scholar 

  37. 37.

    Sun, Y. et al. Activity–selectivity trends in the electrochemical production of hydrogen peroxide over single-site metal–nitrogen–carbon catalysts. J. Am. Chem. Soc. 141, 12372–12381 (2019).

    CAS  PubMed  Google Scholar 

  38. 38.

    Figueiredo, J. L., Pereira, M. F. R. & Freitas, M. M. A. Modification of the surface chemistry of activated carbons. Carbon 37, 1379–1389 (1999).

    CAS  Google Scholar 

  39. 39.

    Lee, S. W. et al. High-power lithium batteries from functionalized carbon-nanotube electrodes. Nat. Nanotechnol. 5, 531–537 (2010).

    ADS  CAS  PubMed  Google Scholar 

  40. 40.

    Guo, H., Wang, X., Qian, Q., Wang, F. & Xia, X. A green approach to the synthesis of graphene nanosheets. ACS Nano 3, 2653–2659 (2009).

    CAS  PubMed  Google Scholar 

  41. 41.

    Yoon, C. M. et al. Electrochemical surface oxidation of carbon nanofibers. Carbon 49, 96–105 (2011).

    CAS  Google Scholar 

  42. 42.

    Acik, M. et al. Unusual infrared-absorption mechanism in thermally reduced graphene oxide. Nat. Mater. 9, 840–845 (2010).

    ADS  CAS  PubMed  Google Scholar 

  43. 43.

    Acik, M. et al. The role of oxygen during thermal reduction of graphene oxide studied by infrared absorption spectroscopy. J. Phys. Chem. C 115, 19761–19781 (2011).

    CAS  Google Scholar 

  44. 44.

    Guo, D. et al. Active sites of nitrogen-doped carbon materials for oxygen reduction reaction clarified using model catalysts. Science 351, 361–365 (2016).

    ADS  CAS  PubMed  Google Scholar 

  45. 45.

    Chong, L. et al. Ultralow-loading platinum-cobalt fuel cell catalysts derived from imidazolate frameworks. Science 362, 1276–1281 (2018).

    ADS  CAS  PubMed  Google Scholar 

  46. 46.

    Choi, C. H. et al. Achilles’ heel of iron-based catalysts during oxygen reduction in acidic medium. Energy Environ. Sci. 11, 3176–3182 (2018).

    CAS  Google Scholar 

  47. 47.

    D’Angelo, D. et al. Oxygen functionalities evolution in thermally treated graphene oxide featured by EELS and DFT calculations. J. Phys. Chem. C 121, 5408–5414 (2017).

    Google Scholar 

  48. 48.

    Kortright, J. B., Sun, J., Spencer, R. K., Jiang, X. & Zuckermann, R. N. Oxygen K-edge scattering from bulk comb diblock copolymer reveals extended, ordered backbones above lamellar order disorder transition. J. Phys. Chem. B 121, 298–305 (2017).

    CAS  PubMed  Google Scholar 

  49. 49.

    Ganguly, A., Sharma, S., Papakonstantinou, P. & Hamilton, J. Probing the thermal deoxygenation of graphene oxide using high-resolution in situ X-ray-based spectroscopies. J. Phys. Chem. C 115, 17009–17019 (2011).

    CAS  Google Scholar 

  50. 50.

    Miedema, P. S. et al. Oxygen binding to cobalt and iron phthalocyanines as determined from in situ X-ray absorption spectroscopy. J. Phys. Chem. C 115, 25422–25428 (2011).

    CAS  Google Scholar 

  51. 51.

    Henkelman, G., Arnaldsson, A. & Jónsson, H. A fast and robust algorithm for Bader decomposition of charge density. Comput. Mater. Sci. 36, 354–360 (2006).

    Google Scholar 

  52. 52.

    Yang, D., Guo, G., Hu, J., Wang, C. & Jiang, D. Hydrothermal treatment to prepare hydroxyl group modified multi-walled carbon nanotubes. J. Mater. Chem. 18, 350–354 (2008).

    CAS  Google Scholar 

  53. 53.

    Suk, M., Chung, M. W., Han, M. H., Oh, H.-S. & Choi, C. H. Selective H2O2 production on surface-oxidized metal-nitrogen-carbon electrocatalysts. Catal. Today 5, 1–7 (2019).

    Google Scholar 

  54. 54.

    Perry, S. C. et al. Electrochemical synthesis of hydrogen peroxide from water and oxygen. Nat. Rev. Chem. 3, 442–458 (2019).

    CAS  Google Scholar 

  55. 55.

    Xia, C., Xia, Y., Zhu, P., Fan, L. & Wang, H. Direct electrosynthesis of pure aqueous H2O2 solutions up to 20% by weight using a solid electrolyte. Science 366, 226–231 (2019).

    ADS  CAS  PubMed  Google Scholar 

  56. 56.

    Daiyan, R. et al. Electroreduction of CO2 to CO on a mesoporous carbon catalyst with progressively removed nitrogen moieties. ACS Energy Lett. 3, 2292–2298 (2018).

    CAS  Google Scholar 

  57. 57.

    Ravel, B. & Newville, M. ATHENA, ARTEMIS, HEPHAESTUS: data analysis for X-ray absorption spectroscopy using IFEFFIT. J. Synchrotron Radiat. 12, 537–541 (2005).

    CAS  PubMed  Google Scholar 

  58. 58.

    Jain, A. et al. Commentary: The Materials Project: a materials genome approach to accelerating materials innovation. APL Mater. 1, 011002 (2013).

    ADS  Google Scholar 

  59. 59.

    Kresse, G., Furthmüller, J. & Hafner, J. Ab initio molecular-dynamics simulation of the liquid-metal–amorphous-semiconductor transition in germanium. Phys. Rev. B 49, 1452 (1996).

    Google Scholar 

  60. 60.

    Kresse, G. & Joubert, D. From ultrasoft pseudopotentials to the projector augmented-wave method. Phys. Rev. B 59, 1758–1775 (1999).

    ADS  CAS  Google Scholar 

  61. 61.

    Kresse, G. & Furthmüller, J. Efficient iterative schemes for ab initio total-energy calculations using a plane-wave basis set. Phys. Rev. B - Condens. Matter Mater. Phys. 54, 11169–11186 (1996).

    ADS  CAS  Google Scholar 

  62. 62.

    Perdew, J. P., Burke, K. & Ernzerhof, M. Generalized gradient approximation made simple. Phys. Rev. Lett. 77, 3865–3868 (1996).

    ADS  CAS  PubMed  Google Scholar 

  63. 63.

    Grimme, S., Antony, J., Ehrlich, S. & Krieg, H. A consistent and accurate ab initio parametrization of density functional dispersion correction (DFT-D) for the 94 elements H-Pu. J. Chem. Phys. 132, 154104 (2010).

    ADS  PubMed  Google Scholar 

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We thank UNSW Mark Wainwright Analytical Center for providing access to the SEM, TEM, FTIR, XPS and other facilities. We thank Dr Bin Gong from MWAC for the XPS measurements. We also thank Dr David Mitchell from University of Wollongong Electron Microscopy Centre for his assistance in HAADF-STEM measurements. XAS experiments were performed at the 10-ID-B beamline of the Advanced Photon Source, a U.S. Department of Energy (DOE) Office of Science User Facility operated for the DOE Office of Science by Argonne National Laboratory under Contract No. DE-AC02-06CH11357. This research used the SXR beamline of the Australian Synchrotron, part of the Australian Nuclear Science and Technology Organization and funded by the Australian Government. The work was supported by the Australian Research Council (ARC) under the Laurate Fellowship Scheme FL-140100081, Discovery Early Career Researcher Award DE170100375 and Linkage Projects funding scheme LP170100691. This research was also undertaken with the assistance of resources provided by the National Computational Infrastructure (NCI) facility at the Australian National University; allocated through both the National Computational Merit Allocation Scheme supported by the Australian Government and the Australian Research Council grant LE190100021 (Sustaining and strengthening meritbased access to the NCI National Facility, 2019–2021). We gratefully acknowledge the support from the Tianjushi Engineering Technology Group. We further acknowledge traveling funding from the Australian Synchrotron Access Program as well. Q.Z. also acknowledges the financial support from the Chinese Scholarship Council and University of New South Wales.

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R.A. and X.L. directed the project. X.L. conceived the concept. R.A. X.L., and Q.Z. designed the experiments. Q.Z. carried out the experiments. N.M.B. and L.T. performed the XAS experiments and analysis the data. X.T. and S.S. performed computational modeling. R.A., X.L., Q.Z., and Z.H. analysed the data. R.A., X.L., Q.Z., and X.T. co-wrote the manuscript.

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Correspondence to Rose Amal or Xunyu Lu.

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Zhang, Q., Tan, X., Bedford, N.M. et al. Direct insights into the role of epoxy groups on cobalt sites for acidic H2O2 production. Nat Commun 11, 4181 (2020).

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