English

• The production of ammonia (NH₃) through the reduction of nitrogen gas (N₂) at ambient conditions is a topic of significant interest. The traditional Haber-Bosch process, which has been developed over a century, demands for high pressure (> 10 MPa) and temperature (> 300 ℃) to produce NH₃. This process emits a large amount of carbon footprints and consumes intensive energy [1–3]. Therefore, there has been a pursuit to find an alternative and greener way to produce NH₃. One promising approach is the electrocatalytic reduction reaction (NRR), which replaces the steam reforming unit, and therefore lowers the energy consumption and the gas emission. This method brings about the following benefits: (1) converting alternative energy in rural parts to portable chemicals; (2) eliminating CO₂ emissions; (3) providing a simpler system for localized and on-site/demand ammonia production; (4) presenting a modular technology that is advantageous to the imitation of electrochemical technique [4–7].

  Thus far, the design of highly efficient electrocatalysts to overcome the indolence and stability of N₂ molecule [8–10] and further enhance NRR efficiency has been a specific focus of the electrochemical reduction method [11–15]. Among them, hetero-phase structures possess a heterogeneous region between which could produce integrated characteristics caused by interaction coupling, which are over the prediction by the rule-of-mixtures. Hetero-phase structures applied to NRR include the following advantages: (1) Hetero-phase materials have a high proportion of atoms at their phase interfaces, resulting in a very high number of unsaturated bonds, suspended bonds, dislocations and defects, which are very conducive to creating catalytic active sites to accelerate the catalytic reaction [16]. (2) The heterogeneous zone could promote the contact between N₂ and the catalyst, causing the enrichment of N₂ concentration and the evacuation of proton concentration, thereby inhibiting the occurrence of hydrogen evolution reaction, which is a competition side reaction of NRR [17]. Moreover, such hetero-phase structures have been rarely reported for NRR yet.

  Herein, we provide a facile strategy for synthesizing hetero-phase materials. By pyrolysis of metal−organic frameworks (MOFs) integrated with Au as the precursor, and controlling the pyrolysis temperature, Au/ZrO₂ with heterogeneous monoclinic and tetragonal phase structure could be easily synthesized. The design of the as-synthesized material is mainly based on the following advantages: (1) MOFs are porous materials consisting of metal nodes linked by organic ligands, have been applied in electrocatalysis owing to their tailorable structure, high porosity, well-defined pore size distribution, high surface area, and low density [18–20]. The use of MOFs as precursors for preparing MOF derivatives for NRR as they can provide plenty of exposed active sites for electron transfer, N≡N cleavage, and N₂ adsorption. (2) Au is rich in valence electrons and unoccupied orbitals, and has been arguably as one of the most promising electrocatalysts for NRR [17,21,22]. To make more efficient use of the precious Au, it is often dispersed onto an inert substrate [23–26]. Metal particles dispersed on support usually have a low coordination number and can serve as metal active centers, in addition, the metal particles own a strong coupling with the carrier, which can enhance the catalytic activity of gold-based catalysts. (3) Zirconium dioxide have been shown to inhibit hydrogen precipitation for efficient nitrogen fixation [27]. Moreover, ZrO₂ has a multi-phase structure, and the interfaces created by the phase boundaries will introduce defects and facilitate electronic transportion. Among the templates for synthesizing ZrO₂, MOFs play a vital role in forming the combining of monoclinic and tetragonal phases. The catalyst with integrated phases exhibits superior performance to its counterparts. Specifically, Au/ZrO₂–800 catalyst achieves an ammonia yield of 22.32 µg h⁻¹ mg_cat.⁻¹ and the corresponding FE of 16.93% at −0.1 V vs. reversible hydrogen electrode (RHE) in 0.1 mol/L KOH solution, with a highest Faradaic efficiency (FE) of 31.92% and the homologous ammonia yield of 13.63% at −0.04 V vs. RHE. This work has significant implications for exploring hetero-phase nanostructures in advancing the electrocatalytic NRR.

  UiO-66 (Zr₆O₄(OH)₄(BDC)₆; BDC: 1, 4-benzenedicarboxylate), a kind of MOF, was synthesized first and then confined with Au ions by a hydrothermal method, followed by being annealed at 300 ℃ to form Au/UiO-66. Transmission electron microscopy (TEM) image shows that Au nanoparticles (NPs) with the size range of 4–7 nm are well distributed on the surface of UiO-66 (Fig. S1 in Supporting information). To verify the conversion process of UiO-66 to ZrO₂, thermogravimetric analysis (TGA) measurement was adopted (Fig. S2 in Supporting information), which reveals two distinct mass drops. The first stage varying from 25 ℃ to 200 ℃ should be attributed to the evaporation of some small molecules such as water, while the second stage from 400 ℃ to 500 ℃ is caused by the degradation of the ligand and the demolition of the UiO-66 carbon framework. At around 530 ℃, the UiO-66 structure utterly collapses, and in fact, the practical calcination temperature was much higher than 530 ℃, which ensures the decomposition of UiO-66 and the formation of ZrO₂. The weight loss calculated theoretically from UiO-66 to ZrO₂ as the total molecular weight of UiO-66 (C₄₈H₂₄O₃₀Zr₆) is 1628.03 and after subtracting the molecular weight 600.72 of C and H atoms, it is found that the weight loss ratio 36.89% matches well with the experimental result of TGA curve. After tardily calcinating Au/UiO-66 at various temperature ranging from 700 ℃ to 900 ℃ under an Ar atmosphere for 3 h, Au/ZrO₂-T with mixed-composition phases were obtained (Fig. 1a).

  Figure 1

  

  Figure 1.  (a) Scheme image of preparation of hetero-phase Au/ZrO₂. (b) XRD patterns of hetero-phase Au/ZrO₂. (c) TEM image of Au/ZrO₂–800 composites. HRTEM images of (d) Au/ZrO₂–700, (e) Au/ZrO₂–800 and (f) Au/ZrO₂–900. (g) STEM image and the corresponding EDX elemental mapping images of Au/ZrO₂–800 composites.

  DownLoad: Full-Size Img PowerPoint

  As shown in Fig. 1b, X-ray diffraction (XRD) analysis indicates that the pyrolysis of Au/UiO-66 yield monoclinic/tetragonal hetero-phase Au/ZrO₂. The XRD patterns of Au/ZrO₂–700, Au/ZrO₂–800, Au/ZrO₂–900 derived from Au/UiO-66 at different temperatures and that of Au-ZrO₂-commercial at 800 ℃ were compared and analyzed. The characteristic diffraction peaks of ZrO₂ at 24.0°, 28.2°, 31.5° correspond respectively to the (110), (), and (111) lattice planes of monoclinic ZrO₂ (PDF#86–1449), while those at 30.2° and 35.3°, are respectively attributed to the (101) and (200) lattice planes of tetragonal ZrO₂ (PDF#88–1007). The ratio of phase transition is calculated based on the refinement of the XRD peaks by Rietveld [28]. The peak positions are adjusted by the successive refinement of systematic errors, taking into consideration zero-shifting and sample-shifting errors (Figs. S3-S6 in Supporting information). The tetragonal and monoclinic phase percentages for each catalyst are recapitulated in Table S1 (Supporting information). The successful synthesis of stable hetero-phase structure requires precise control of the carbonization temperature, as pyrolysis at 700 ℃, the main product obtained is tetragonal phase; while pyrolysis at high temperature of 900 ℃, the main stuff obtained is monoclinic phase; when carbonization is performed with the commerical ZrO₂ loaded Au, a pure monoclinic phase of ZrO₂ is obtained; only the temperature is controlled to 800 ℃, a considerable proportion of hetero-phase structure could be obtained.

  Transmission electron microscopy (TEM) measurement was used to investigate the morphology (Fig. 1c). The phase locations in Au/ZrO₂–700, 800, 900 catalysts were further analyzed by high-resolution TEM (HRTEM) in the fast Fourier transform (FFT) (Figs. 1d–f). The distinct lattice fringes of 0.283, 0.318, and 0.363 nm are accredited to (111), (), and (110) planes of monoclinic ZrO₂, respectively, and 0.295 nm is identified to (101) plane of tetragonal ZrO₂. The existence form of Au in Au/ZrO₂–800 is also characterized, from HRTEM image in Fig. S7 (Supporting information), the distinct lattice fringe of 0.235 nm is accredited to (111) planes of Au NPs (PDF#99–0056). Scanning transmission electron microscopy energy dispersive X-ray spectroscopy (STEM-EDX) was employed for mapping analysis of Zr, O and Au elements distribution in Au/ZrO₂–800 (Fig. 1g). It reveals that the Zr and O elements are homogeneously distributed over the selected area, while Au is mainly concentrated in the bright region, thus further confirming the existence of Au NPs in ZrO₂.

  Further analysis of Au/ZrO₂–800 by X-ray photoelectron spectroscopy (XPS) probes the chemical valence of the surface elements and the interaction between metal and hetero-phase carrier. XPS survey spectrum reveals that Au/ZrO₂–800 is mainly composed of O, Zr and Au elements (Fig. 2a). In the fine spectrum of Au element, two pairs of spin-orbit doublets indicate the existence of Au⁰ (Au-Au bonding energy peaks at 84.0 and 87.7 eV) and Au^δ+ (Au-O bonding energy peaks at 85.9 and 88.8 eV) (Fig. 2b), which is consistent with the previously published results [29,30]. Furthermore, in the fine spectrum of Zr (Fig. 2c), the binding energies at 182.0 eV and 184.4 eV can be ascribed to the characteristic peaks of Zr 3d_5/2 and Zr 3d_3/2, which is lower than the values of ZrO₂ (182.8 and 185.3 eV) reported in the literature [31]. The presence of Au^δ+ and the negative displacement of Zr⁴⁺ in this sample indicate the electron transfer from the metal particles to the oxide carrier, suggesting that the Au particles may form Au-O-Zr bonding with the ZrO₂ carrier. In addition to strong-metal support interation, small sized metal particles own high surface energy, a strong chemical bonding between metal and the coordinated lattice oxygen of oxides is always formed in order to keep the metal stability [32–34]. The O 1s spectra of Au/ZrO₂ annealed at different temperatures can be fitted to two peaks, i.e., lattice oxygen (O_L) and oxygen vacancy (O_V), and all peaks of O_L and O_V are located at 529.9 and 531.5 eV, respectively (Fig. 2d). O_V is believed to promote N₂ adsorption and activation in the NRR process, and therefore affect the NRR performance [35–39]. The O_V contents of Au/ZrO₂–700, 800, 900 can be estimated from the area ratio of the XPS fit as 20.12%, 23.02% and 17.73%, respectively, which indicates that when Au/ZrO₂ is annealed, the interface forming at the phase boundary introduces defects, and Au/ZrO₂ with roughly close proportions of mixed-composition phases can produce more O_V.

  Figure 2

  

  Figure 2.  (a) XPS spectra of Au/ZrO₂–800. The corresponding fine spectra of (b) Au 4f (c) Zr 3d and (d) O 1s.

  DownLoad: Full-Size Img PowerPoint

  The electrocatalytic NRR performance was measured in H-type cell with N₂-saturated 0.1 mol/L KOH as the electrolyte under ambient conditions, and all potentials were converted to the RHE scale (Fig. S8 in Supporting information). Electrolytes were collected at the end of the test, ammonia concentrations were measured plying Nessler's reagent spectrophotometry, and the concentration of the possible by-product hydrazine was determined utilizing the Watt and Chrisp method [40]. Calibration curves for the determination of ammonia and hydrazine were plotted respectively (Figs. S9 and S10 in Supporting information). The as-synthesized Au/ZrO₂-T was then used as catalyst to study its NRR catalytic performance. To determine the potential of the electrochemically active region of NRR, linear-sweep voltammetric (LSV) curves were measured in both N₂- and Ar-saturated electrolytes (Fig. 3a), which exhibit similar shapes. However, there is an increase in current density below 0.0 V in N₂-saturated electrolyte, indicating the formation of NH₃ from N₂ at the reduction potential.

  Figure 3

  

  Figure 3.  Electrocatalytic NRR on Au/ZrO₂–800 catalyst in 0.1 mol/L KOH electrolyte. (a) LSV curves in N₂- and Ar-saturated electrolytes. (b) NH₃ yield at different applied potentials. (c) FEs at diverse applied potentials. (d) Chronoamperometry test at –0.1 V for 24 h. (e) Comparison of electrocatalytic NRR on Au/ZrO₂–700, Au/ZrO₂–800 and Au/ZrO₂–900 catalysts in 0.1 mol/L KOH electrolyte. (f) UV–vis absorption spectra under different conditions.

  DownLoad: Full-Size Img PowerPoint

  Furthermore, electrocatalytic tests were carried out on Au/ZrO₂–800 catalyst at an given potential from 0.0 V to −0.3 V to study its catalytic activity and the optimal working potential for NRR. The current density increases markedly as the applied potential moves from 0.0 V to −0.3 V (Fig. S11 in Supporting information). After two hours of the electrolysis process, the electrolyte is collected and then quantified by Nessler's reagent to determine the NH₃ yield and the corresponding Faradaic efficiency by formulae (see Supporting information). The highest NH₃ yield with 22.32 µg h⁻¹ mg_cat.⁻¹ is obtained at −0.1 V with a FE of 16.93%. The highest FE of 31.92% is obtained at −0.04 V with a NH₃ yield of 13.63%, both high yield and high efficiency are achieved at very low voltages (Figs. 3b and c). The corresponding ultraviolet-visible (UV–vis) absorption curves of the electrolytes are presented in Fig. S12 (Supporting information). Simultaneously, a 24 h long-term electrocatalytic test was performed at −0.1 V. After electrolysis for 24 h, chronoamperometry curve of Au/ZrO₂–800 shows negligible decrease in current density (Fig. 3d), reflecting the excellent stability of Au/ZrO₂–800. In addition, the possible by-product hydrazine is not detected at each potential, indicating the excellent selectivity of Au/ZrO₂–800 (Fig. S13 in Supporting information).

  To investigate the importance of the hetero-phase structures for boosting NH₃ performance, Au/ZrO₂ with different ratios of monoclinic and tetragonal phases were prepared by controlling the pyrolysis temperature. In Table S1, Au/ZrO₂–800 shows monoclinic and tetragonal phase ratios of 37% and 60.9%, respectively, which are relatively closer compared with other samples. Notably, MOFs play a vital role in forming the hetero-phase structures compared to other templates for synthesizing Au/ZrO₂. The pure tetragonal phase of Au/ZrO₂-commercial were achieved when we utilized the commercially purchased ZrO₂ directly instead of MOF to load Au. The electrocatalytic NRR performances of samples Au/ZrO₂-T were also tested at −0.1 V (Fig. 3e and Fig. S14 in Supporting information). Compared with Au/ZrO₂–700 (12.50 µg h⁻¹ mg_cat.⁻¹), Au/ZrO₂–900 (12.32 µg h⁻¹ mg_cat.⁻¹) and Au/ZrO₂-commercial (0.95 µg h⁻¹ mg_cat.⁻¹), Au/ZrO₂–800 achieves the highest NH₃ yield rate of 22.32 µg h⁻¹ mg_cat.⁻¹ and the highest FE of 31.92%, indicating the closer ratios of the monoclinic phase and tetragonal phase, the higher performance the catalyst will achieve. Furthermore, in order to clarify whether the origin of the catalytic activity is due to the interaction between Au and the hetero-phase carrier, ZrO₂-800 without introduction of metal was also designed. The NH₃ yield of ZrO₂–800 was tested at −0.1 V, which was only a quarter of that of Au/ZrO₂–800 (Fig. S14).

  To gain insights into the reasons behind the NRR performance differences, the electrochemically active surface area (ESCA) was further studied. The cyclic voltammetry (CV) curves of Au/ZrO₂–700, 800, 900 in N₂-saturated 0.1 mol/L KOH electrolyte were tested. The double-layer capacitance (C_dl) of the catalytic surface was measured by CV in a Faradaic silence potential range of 0.02 ∼ −0.08 V vs. Ag/AgCl using different scan rates, which is generally used to represent the corresponding ESCA. As shown in Fig. S15 (Supporting information), Au/ZrO₂–800 exhibits a higher C_dl value of 0.0648 mF/cm² than Au/ZrO₂–700, 900 of 0.0585 mF/cm² and 0.0495 mF/cm², respectively, indicating that the integration of the monoclinic and tetragonal phases in Au/ZrO₂–800 can enhance the ESCA effectively.

  To investigate if the detected NH₃ is a result of the electrocatalytic NRR process, control experiments were performed (Fig. 3f and Fig. S16 in Supporting information), including: (1) electrolysis for 2 h at open-circuit voltage; (2) electrolysis for 2 h at −0.1 V in Ar atmosphere; (3) electrolysis for 2 h at −0.1 V using carbon paper as the working electrode. It is found that NH₃ is barely yielded in the control experiments, which confirms that NH₃ is produced by electrocatalytic NRR of Au/ZrO₂–800 catalyst.

  This work synthesized nanomaterials with hetero-phase structures as NRR catalysts by simply changing the reaction temperature to pyrolyze MOF precusors. MOFs play a vital role in forming the mixed-component phases compared with other templates for synthesizing metal oxide. The obtained electrocatalyst Au/ZrO₂–800 possessing roughly close proportions of monoclinic and tetragonal phases affords an excellent NRR performance with a high NH₃ yield of 22.32 µg h⁻¹ mg_cat.⁻¹ and a Faradaic efficiency of 31.92% at low overpotential. We believe this work will pave the way for exploring controllable preparation and precise synthesis of nano-hetero-phase structures.

  Declaration of competing interest

  The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.

  Acknowledgments

  This work was supported by the National Natural Science Foundation (Nos. 22075133 and 21701086).

  Supplementary materials

  Supplementary material associated with this article can be found, in the online version, at doi:10.1016/j.cclet.2023.108654.

  
  
• 1. [1]

     W. Lin, H. Chen, G. Lin, et al., Angew. Chem. Int. Ed. 61 (2022) e202207807. doi: 10.1002/anie.202207807

  2. [2]

     S. Qiang, F. Wu, J. Yu, et al., Angew. Chem. Int. Ed. 62 (2023) e202217265. doi: 10.1002/anie.202217265

  3. [3]

     B.H.R. Suryanto, K. Matuszek, J. Choi, et al., Science 372 (2021) 1187–1191. doi: 10.1126/science.abg2371

  4. [4]

     Y. Li, Y. Liu, X. Liu, et al., Nano Res. 15 (2022) 6026–6035. doi: 10.1007/s12274-022-4298-2

  5. [5]

     M. Guo, L. Fang, L. Zhang, et al., Angew. Chem. Int. Ed. 62 (2023) e202217635. doi: 10.1002/anie.202217635

  6. [6]

     J. Liu, L. He, S. Zhao, et al., Adv. Sci. 10 (2023) 2205786. doi: 10.1002/advs.202205786

  7. [7]

     Z. Yao, S. Liu, H. Liu, et al., Adv. Funct. Mater. 33 (2023) 2209843. doi: 10.1002/adfm.202209843

  8. [8]

     G. Qing, R. Ghazfar, S.T. Jackowski, et al., Chem. Rev. 120 (2020) 5437–5516. doi: 10.1021/acs.chemrev.9b00659

  9. [9]

     X. Zhao, G. Hu, G.F. Chen, et al., Adv. Mater. 33 (2021) e2007650. doi: 10.1002/adma.202007650

  10. [10]

      C. Xue, X. Zhou, X. Li, et al., Adv. Sci. 9 (2022) 2104183. doi: 10.1002/advs.202104183

  11. [11]

      I.E. Khalil, C. Xue, W. Liu, et al., Adv. Funct. Mater. 31 (2021) 2010052. doi: 10.1002/adfm.202010052

  12. [12]

      Q.R. Wang, J. Pan, J.P. Guo, et al., Nat Catal. 4 (2021) 959–967. doi: 10.1038/s41929-021-00698-8

  13. [13]

      Y. Wang, N. Yang, X. Xin, et al., Chin. Chem. Lett. 34 (2023) 107841. doi: 10.1016/j.cclet.2022.107841

  14. [14]

      R.B. Zhao, C.W. Liu, X.X. Zhang, et al., J. Mater. Chem. A 8 (2020) 77–81. doi: 10.1039/c9ta10346e

  15. [15]

      X. Zhao, G. Hu, G.F. Chen, et al., Adv. Mater. 33 (2021) 2007650. doi: 10.1002/adma.202007650

  16. [16]

      D. Zhang, Y. Liu, B. Mao, et al., ACS Sustain. Chem. Eng. 9 (2021) 2844–2853. doi: 10.1021/acssuschemeng.0c08708

  17. [17]

      J. Zhang, B. Zhao, W. Liang, et al., Adv. Sci. 7 (2020) 2002630. doi: 10.1002/advs.202002630

  18. [18]

      L. Cha, Z. Hao, L. Ming, et al., Ind. Chem. Mater. 1 (2023) 9–38. doi: 10.5771/9783835385610-9

  19. [19]

      H. He, H.M. Wen, H.K. Li, et al., Coord. Chem. Rev. 471 (2022) 214761. doi: 10.1016/j.ccr.2022.214761

  20. [20]

      Y. Peng, S. Sanati, A. Morsali, et al., Angew. Chem. Int. Ed. 62 (2023) e2022147.

  21. [21]

      M.M. Shi, D. Bao, B.R. Wulan, et al., Adv. Mater. 29 (2017) 1606550. doi: 10.1002/adma.201606550

  22. [22]

      J. Zhang, Y. Ji, P. Wang, et al., Adv. Funct. Mater. 30 (2020) 1906579. doi: 10.1002/adfm.201906579

  23. [23]

      D. Kim, G. Dimitrakopoulos, B. Yildiz, J. Am. Chem. Soc. 144 (2022) 21926–21938. doi: 10.1021/jacs.2c08422

  24. [24]

      Y. Zhang, J. Zhang, B. Zhang, et al., Nat. Commun. 11 (2020) 41467.

  25. [25]

      M. Xie, F. Dai, J. Li, et al., Angew. Chem. Int. Ed. 60 (2021) 14370–14375. doi: 10.1002/anie.202103652

  26. [26]

      X. Qin, S. He, J. Wu, et al., ACS Cent. Sci. 6 (2020) 247–253. doi: 10.1021/acscentsci.9b01205

  27. [27]

      H. Tao, C. Choi, L. -X. Ding, et al., Chem 5 (2019) 204–214. doi: 10.1016/j.chempr.2018.10.007

  28. [28]

      G. Garnweitner, L.M. Goldenberg, O.V. Sakhno, et al., Small 3 (2007) 1626–1632. doi: 10.1002/smll.200700075

  29. [29]

      W. McLean, C.A. Colmenares, R.L. Smith, et al., J. Phys. Chem. 87 (1983) 788–793. doi: 10.1021/j100228a018

  30. [30]

      D.T. Jayne, N.S. Fatemi, V.G. Weizer, J. Vac. Sci. Technol. A 9 (1991) 1410–1415. doi: 10.1116/1.577637

  31. [31]

      Z. Sun, X. Zhang, N. Na, et al., J. Phys. Chem. B 110 (2006) 13410–13414. doi: 10.1021/jp0616359

  32. [32]

      J. Xing, J.F. Chen, Y.H. Li, et al., Chem. Eur. J. 20 (2014) 2088. doi: 10.1002/chem.201304764

  33. [33]

      X.K. Gu, B. Qiao, C.Q. Huang, et al., ACS Catal. 4 (2014) 3886–3890. doi: 10.1021/cs500740u

  34. [34]

      A. Bruix, J.A. Rodriguez, P.J. Ramirez, et al., J. Am. Chem. Soc. 134 (2012) 8968–8974. doi: 10.1021/ja302070k

  35. [35]

      K. Chu, F. Liu, J. Zhu, et al., Adv. Energy Mater. 11 (2021) 2003799. doi: 10.1002/aenm.202003799

  36. [36]

      G. Zhang, Q. Ji, K. Zhang, et al., Nano Energy 59 (2019) 10–16. doi: 10.1016/j.nanoen.2019.02.028

  37. [37]

      C. Fang, T. Bi, X. Xu, et al., Adv. Mater. Interfaces 6 (2019) 1901034. doi: 10.1002/admi.201901034

  38. [38]

      Y. Liu, X. Kong, X. Guo, et al., ACS Catal. 10 (2020) 1077–1085. doi: 10.1021/acscatal.9b03864

  39. [39]

      W. Song, J. Wang, L. Fu, et al., Chin. Chem. Lett. 32 (2021) 3137–3142. doi: 10.1016/j.cclet.2021.02.043

  40. [40]

      T. Dambrauskas, H.H. Cornish, Am. Ind. Hyg. Assoc. J. 23 (1962) 151–156. doi: 10.1080/00028896209343218

• 

  Figure 1  (a) Scheme image of preparation of hetero-phase Au/ZrO₂. (b) XRD patterns of hetero-phase Au/ZrO₂. (c) TEM image of Au/ZrO₂–800 composites. HRTEM images of (d) Au/ZrO₂–700, (e) Au/ZrO₂–800 and (f) Au/ZrO₂–900. (g) STEM image and the corresponding EDX elemental mapping images of Au/ZrO₂–800 composites.

  下载: 全尺寸图片 幻灯片
  

  Figure 2  (a) XPS spectra of Au/ZrO₂–800. The corresponding fine spectra of (b) Au 4f (c) Zr 3d and (d) O 1s.

  下载: 全尺寸图片 幻灯片
  

  Figure 3  Electrocatalytic NRR on Au/ZrO₂–800 catalyst in 0.1 mol/L KOH electrolyte. (a) LSV curves in N₂- and Ar-saturated electrolytes. (b) NH₃ yield at different applied potentials. (c) FEs at diverse applied potentials. (d) Chronoamperometry test at –0.1 V for 24 h. (e) Comparison of electrocatalytic NRR on Au/ZrO₂–700, Au/ZrO₂–800 and Au/ZrO₂–900 catalysts in 0.1 mol/L KOH electrolyte. (f) UV–vis absorption spectra under different conditions.

  下载: 全尺寸图片 幻灯片
•