The lack of efficient catalysts for ammonia synthesis from N2 and H2 gases at the lower temperature of ca. 50 °C has been a problem not only for the Haber–Bosch process, but also for ammonia production toward zero CO2 emissions. Here, we report a new approach for low temperature ammonia synthesis that uses a stable electron-donating heterogeneous catalyst, cubic CaFH, a solid solution of CaF2 and CaH2 formed at low temperatures. The catalyst produced ammonia from N2 and H2 gases at 50 °C with an extremely small activation energy of 20 kJ mol−1, which is less than half that for conventional catalysts reported. The catalytic performance can be attributed to the weak ionic bonds between Ca2+ and H− ions in the solid solution and the facile release of hydrogen atoms from H− sites.
The Haber–Bosch process currently enables the provision of food for over 70% of the world’s population, consuming 2% of global energy and generating 3% of global CO2 emissions1,2. These values would steeply increase by a rapid increase of the human population. Highly efficient conversion of N2 and H2 to ammonia with low-energy consumption has remained a challenge since the creation of the Haber–Bosch process, where sustainable ammonia production using natural energy is the ultimate goal. Ammonia is equilibrated in N2 and H2. Figure 1a demonstrates the correlation of the theoretical ammonia yield with reaction pressure and temperature. As the reaction temperature increases, ammonia decomposition as an endothermic reaction exceeds ammonia formation, an exothermic reaction, which decreases the ammonia yield. For this reason, the reaction system must therefore be further pressurized with an increase in the reaction temperature to obtain the same ammonia yield; high reaction temperature causes high pressurization, which requires large energy consumption for both heating and pressurization. The iron-based catalysts used in the present Haber–Bosch process are effective for ammonia synthesis above 350 °C, so that the maximum ammonia yield is at most 30−40%, despite excess pressurization (>10–20 MPa) accompanied by large energy consumption. This is a serious drawback in sustainable ammonia production without the use of fossil fuels. While wind power generation has been reported to be compatible with the Haber–Bosch process, the process itself consumes 40–50% of the electric power generated by wind turbine, and thereby electric power available for H2 production is considerably limited3. Figure 1a also indicates that the ammonia yield exceeds 98% at ca. 50 °C regardless of pressures, and there is no significant difference in ammonia yield among pressures below this temperature. Thus, a lower temperature is favorable for ammonia production with respect to yield and energy consumption, and more efficient ammonia production is required to overcome the kinetic barrier at lower temperature to achieve the equilibrium. However, conventional catalysts equally lose the catalytic activity for ammonia formation from N2 and H2 at 100–200 °C, even if they exhibit high catalytic performance at high temperatures, as shown in Fig. 1a. Lowering the temperature for a loss of activity below 50 °C would largely enhance the catalytic activity for ammonia synthesis at low-temperature range below 300 °C. While there has been significant progress in homogeneous catalytic systems to synthesize ammonia from N2 and H+ activated by specific and nonreusable reagents below room temperature4,5, guiding principles to lower the temperature for a loss of activity on ammonia synthesis from N2 and H2 have yet to be clarified.
Thus, the lack of catalysts that are workable at lower temperatures has remained a problem for the Haber–Bosch process for over a century, and has also prevented sustainable ammonia production toward zero CO2 emissions. We have begun to re-examine the low-temperature kinetics of ammonia synthesis catalysts to find a route for low-temperature ammonia production. Figure 1b shows Arrhenius plots for a commercial Fe catalyst6 with ammonia formation rates that were both measured (rMNH3) and estimated from the Arrhenius equation (rENH3). The reaction rate follows the Arrhenius equation as long as the reaction mechanism is unchanged in the temperature range; therefore, the reaction rate at a specific temperature was estimated using the Arrhenius equation. The difference between rMNH3 and rENH3 increases with a decrease in the temperature below 300 °C. The Arrhenius equation predicted a sufficient amount of ammonia to form at 100 °C. However, no ammonia formation was detected below 150 °C, which brought the natural logarithm of the rate close to –∞. Even if the catalyst amount and space velocity were increased significantly, ammonia formation was not observed below 150 °C. Taking into account the detection sensitivity of the ammonia analysis methods, the rate of ammonia formation was expected to be less than nano mol h−1 g−1. This means that the catalyst cannot act for ammonia synthesis at all below the temperature. The same phenomenon was confirmed in several representative catalytic systems for the synthesis of ammonia from N2 and H2 (Supplementary Table 1). This cannot be simply attributed to deactivation by ammonia adsorbed on the catalyst, because ammonia that adsorbs on transition metals (TMs) such as Fe and Ru will desorb below room temperature7. Ammonia formation from N2 and H2 over catalysts proceeds through the dissociative adsorption of N2 (N2 → 2 N), followed by the hydrogenation of nitrogen adatoms (N → NH3). The former step has a higher energy barrier than the latter that proceeds on TM surfaces at room temperature to 100 °C8. It is well-known that the cleavage of N2 molecules with ammonia synthesis catalysts is largely enhanced by electron donation from electron-donating materials into the π* orbitals of N ≡ N via the d-orbitals of TMs9,10,11, and the electron-donating capability of the TM itself is almost independent of the temperature below 200 °C12,13 (see Supplementary Discussion). A decrease in the electron-donating capability has been purported as one possible explanation for the lack of ammonia synthesis by catalysis at low temperatures. Therefore, stable materials that exhibit high electron-donating capability at low temperatures may lead to the realization of low-temperature ammonia synthesis.
Here we present a new approach for low-temperature ammonia synthesis that uses a stable electron-donating heterogeneous catalyst, Ru nanoparticle-deposited cubic CaFH solid solution. The catalyst produces ammonia from N2 and H2 gases at 50 °C with an extremely small activation energy of 20 kJ mol−1, which is less than half that for conventional catalysts reported. The catalytic performance can be attributed to the weak ionic bonds between Ca2+ and H− ions in the solid solution and the facile release of hydrogen atoms from H− sites.
CaFH solid solution as a strong electron-donating material
As a first step to verify the working hypothesis and to prepare such electron-donating materials, we have focused on calcium hydride (CaH2), a familiar dehydrating agent, because of its simplicity. TM nanoparticles deposited on CaH2 abstract H atoms from the near-surface CaH2 due to substantial interaction between the TM and H–, and the H atoms move on to the metal nanoparticles and desorb as H2 molecules, leaving electrons in the H– vacancy of CaH2 (CaH2 → Ca2+H–(2–x)e–x + xH)14. The resulting Ca2+H–(2–x)e–x behaves as a stable surface electride with a small work function (Φ = 2.7 eV) comparable with that of metallic Li15. The strong electron donation from Ca2+H–(2–x)e–x to the TM nanoparticles enhances the cleavage of N2 molecules, which leads to high catalytic performance for ammonia synthesis14. Supplementary Table 1 shows that the difference between the rMNH3 and rENH3 rates for the formation of ammonia over Ru-deposited CaH2 (Ru/CaH2) was not negligible at ≤ 200 °C, as with other catalysts; however, the catalyst was not at all active for ammonia formation at 150 °C. The temperature that eliminates the activity of Ru/CaH2 is therefore between 150 and 200 °C, which is similar to that for conventional catalysts (Supplementary Table 1). A H2-temperature-programmed desorption (TPD) profile for Ru/CaH2 (Fig. 2a) revealed that the H2 desorption-onset temperature was almost identical to the temperature where the catalytic activity of Ru/CaH2 is lost. Formation of a strong electron-donating material is a determinant for ammonia formation over Ru/CaH2 at low temperatures. Therefore, lowering of the onset temperature for H2 desorption would lead to a catalytic system for ammonia synthesis at lower temperatures.
Here, we have adopted a new strategy based on classical theory to lower the electride formation temperature: the introduction of F– anions into CaH2. F– is an extremely hard base in hard and soft acids and bases (HSAB), and the Ca−F ionic bond (529 kJ mol−1) is harder than the Ca−H bond (224 kJ mol−1)16. Replacing a part of H– in CaH2 with F– would weaken ionic bonds between Ca2+ and H–, thereby lowering the temperature for the release of H atoms from the material. This replacement would increase the energy of electrons trapped at H– vacancies due to electron repulsion between the electron and F–, which would cause a reduction in the work function of the surface region and in turn enhance the electron-donating power. In this study, F– was introduced into CaH2 by heating a simple mixture of CaH2 and BaF2 powders in a flow of H2 at 340 °C. A wide-range X-ray diffraction (XRD) pattern (Fig. 2b) of the resultant sample (Ca/Ba atomic ratio = 98:2) indicated that the sample is mainly composed of CaH2. Diffraction peaks of BaF2 or CaF2 were not observed in the XRD pattern, whereas the diffraction peaks due to BaH2 were apparent (Supplementary Fig. 1). Consequently, CaF2 is not formed in the heated mixture, despite the complete replacement of F– in BaF2 with H– derived from CaH2. CaH2–BaF2 mixtures in various CaH2/BaF2 ratios were heated in H2 to identify the material formed in the heated CaH2–BaF2 mixture. Figure 2c shows narrow-range XRD patterns (2θ = 31–35°) of heated CaH2–BaF2 mixtures (Ca/Ba atomic ratios of 98:2, 9:1, 5:1, and 3:1), where an asymmetrical diffraction assignable to (200) of the cubic CaF1.0H1.0 solid solution appears at 2θ = 32.7°17. It is well-known that orthorhombic CaH2 is transformed into a cubic structure in the formation of cubic CaFH solid solution17. The diffraction peak intensity increased, but was not shifted with an increase in the Ba content. In order to clarify the characteristics of CaF1.0H1.0 solid solution formed on CaH2–BaF2 mixtures, CaFxH2–x solid solution (denoted as CaFxH2–x–CaF2) was prepared by heating mixtures of orthorhombic CaH2 and cubic CaF2 at 550 °C, a conventional method17. XRD patterns of CaFxH2–x–CaF2 (1.0 ≤ x ≤ 1.6) (Supplementary Fig. 2) elucidated that the (200) diffraction for the cubic CaFxH2–x–CaF2 is sensitive to the F− concentration and shifts from 2θ = 32.7° to lower angles with decreasing F− concentration17. These results suggest that heating a CaH2–BaF2 mixture at 340 °C forms the most stable CaF1.0H1.0 on CaH2. In X-ray photoelectron spectroscopy (XPS) measurements for heated CaH2–BaF2 mixtures (Ca/Ba atomic ratio of 98:2), CaFxH2–x–CaF2 (x = 1) and CaH2 (Supplementary Fig. 3), the Ca 2p peaks for both heated CaH2–BaF2 mixtures and CaFxH2–x–CaF2 (x = 1) appeared at 346.5 eV, which is lower than that for CaH2 (347.3 eV) and supports the formation of the CaF1.0H1.0 solid solution on the surface of a small amount of BaF2-added CaH2. Next, Ru nanoparticles (12 wt%) were deposited on CaF1.0H1.0 phase obtained by heating a CaH2–BaF2 (Ca:Ba=98:2) mixture at 340 °C (denoted as Ru/CaFH), and Ru/CaFH after ammonia synthesis reaction over 30 h at 340 °C was examined by H2-TPD (Fig. 2a). The starting temperature for H2 desorption was lowered to the range of room temperature to 50 °C, compared with that for Ru/CaH2. Supplementary Fig. 4 is the H2-TPD profile of the Ru-deposited CaFxH2–x–CaF2 (denoted as Ru/CaFxH2–x–CaF2 (x = 1)), which also indicates that H2 begins to desorb from the material at ca. 50 °C. This implies that the formation of the CaFH solid solution, i.e., the formation of Ca2+−F− ionic bonds, clearly weakens the Ca2+−H− bond and lowers the temperature for the hydrogen release reaction. A notable feature in the H2-TPD profile for Ru/CaFH is that it overlaps the H2-TPD profiles of Ru/CaH2 (Fig. 2a) and Ru/CaFxH2–x–CaF2 (x = 1) (Supplementary Fig. 4). As a result, the CaFH solid solution may coexist with CaH2 on the surface of Ru/CaFH.
To evaluate the electron-donating capability of CaFH, the work function of CaFH with H‒ vacancies was estimated by density-functional theory (DFT) computations (“Methods”, Supplementary Fig. 5). The work function on the most stable surface (111) of CaFH calculated by DFT was 2.2 eV, which is smaller than that (2.7 eV) for CaH2 with H− defects because electron repulsion between electrons and F– increases the energy of electrons trapped at H– vacancies. These results indicate that the abstraction of H atoms from CaFH forms a strong electron-donating material, which has a work function comparable to that of metallic potassium (Φ = 2.3 eV).
Morphological information for Ru/CaFH is summarized in Supplementary Fig. 6. Ru/CaFH with a surface area of 30 m2 g−1 consists of irregular-shaped particles of 0.5–3 μm in diameter. The particle size of Ru deposited on CaFH was estimated to be 3–4 nm. XPS measurements for F 1 s and Ca 2p revealed that the surface atomic ratio of F to Ca (F/Ca) in Ru/CaFH was 0.08, which is much smaller than that expected from CaF1.0H1.0, and also supports the coexistence of CaFH and CaH2.
Catalytic performance for ammonia synthesis at low temperatures
The catalytic performance for ammonia formation from N2 and H2 for tested catalysts is summarized in Fig. 3. Figure 3 also contains the results for CaH2 (Ru/CaH2), a BaH2–BaO mixture (Ru/BaH2–BaO)18, and Cs-doped MgO (Cs–Ru/MgO)6,10 loaded with Ru nanoparticles, and a commercial Fe catalyst6 for comparison. Cs–Ru/MgO has a higher catalytic activity for ammonia synthesis than the commercial Fe catalyst above 300–400 °C. Ru/BaH2–BaO acts as a highly active ammonia synthesis catalyst18 that is comparable with Ru nanoparticles immobilized on Ca(NH2)2 containing Ba2+ (Ru/Ba–Ca(NH2)2), which exhibits the highest catalytic performance for ammonia synthesis among the reported catalysts over wide temperature (200–450 °C) and pressure ranges (0.1–0.9 MPa)6. Supplementary Table 2 shows the physicochemical information (surface area, porosity, and Ru particle size) and the rates of ammonia formation for Ru/CaFH, Ru/CaH2, Ru/Ba–Ca(NH2)2, Ru/BaO–BaH2, Ru/C12A719, Cs–Ru/MgO, and a commercial Fe catalyst as benchmark catalysts at 100–340 °C. It was confirmed that the catalytic activities of the commercial Fe catalyst and Cs–Ru/MgO benchmark catalysts were comparable with those reported by other groups19,20,21. These conventional catalysts did not exhibit activity for ammonia synthesis below 100–200 °C, whereas Ru/CaFH synthesized ammonia at 50 °C. The ammonia formation over the catalyst at 50 °C was confirmed by both direct mass spectrometry and ion chromatography, and is not derived from N species formed on the catalyst during the catalyst activation at 340 °C (see Supplementary Discussion). The ammonia formation rate of Ru/CaFH increased with the temperature and was unchanged even after the rate measurement was repeated, which indicates that Ru/CaFH is a stable catalyst. There was no significant difference in XRD pattern between Ru/CaFH after reaction and CaH2–BaF2 mixture heated at 340 °C (Ca/Ba atomic ratio = 98:2, Fig. 2b, c). The apparent activation energy for ammonia synthesis over the catalyst in the range of 50–150 °C was estimated to be 20 kJ mol−1, which is less than half that of reported catalysts (from 40 kJ mol−1)6,14,18,19,21. Furthermore, Ru/CaFH as a stable catalyst surpasses conventional catalysts at higher temperatures. Figure 3 gives the catalyst weight required for the equilibrium yield (CWEY) of ammonia at 200 °C (see Supplementary Discussion). The rates of ammonia formation and CWEYs for all tested catalysts, including Ru/Ba–Ca(NH2)2, and the recently reported highly active catalysts at 200–350 °C are summarized in Supplementary Table 322,23,24,25. Although Ru/Ba–Ca(NH2)2 and Ru/BaO–BaH2 have had much smaller CWEYs among the reported highly active catalysts, the CWEY of Ru/CaFH was only half that of both catalysts at 200 °C. In the case of Ru/CaFH, the apparent activation energy (Ea = 20 kJ mol−1) and coefficient due to the collision frequency (A = 10) in the Arrhenius equation estimated from the rates of ammonia formation at 50, 75, 100, and 125 °C were almost the same as those (Ea = 23 kJ mol−1, A = 12) obtained by the ammonia formation rates at 275–340 °C. In addition, there was no significant difference in Ea and A for ammonia formation over Ru/CaFH at 0.1 and 0.9 MPa. This suggests that the same active sites on Ru/CaFH form ammonia through a reaction mechanism in a wide range of reaction conditions (≥ 50 °C, ≥ 0.1 MPa). It was also confirmed in ammonia synthesis (240–400 °C) over a commercial Fe catalyst used in this study that Ea and A at 0.1 MPa are identical with those at 0.9 MPa6. Furthermore, Ru/CaFH produced ammonia without a decrease in activity for long periods of time and at higher temperatures (200 and 340 °C) (Supplementary Figs. 7 and 8). Ammonia formation over Ru/CaFH was close to the equilibrium yield, even at ca. 300 °C, because of the high catalytic performance. As a result, ammonia synthesis over Ru/CaFH in Supplementary Fig. 8 reaches the equilibrium. Despite such equilibrium conversion (i.e., catalyst deactivation test conditions), the rate of ammonia formation over Ru/CaFH was constant for over 100 h. The amount of ammonia produced by Ru/CaFH at 340 °C exceeded the amount of the used catalyst (ca. 24 mmol) within 100 min. The XRD pattern and surface atomic ratio of F to Ca (F/Ca = 0.08) for Ru/CaFH were unchanged after reaction for 100 h, which was consistent with the lack of F species such as HF detected during the reaction. These results are clearly indicative of the stability of the Ru/CaFH catalyst.
The surface areas of the supports and ammonia formation rates (340 °C) of Ru/CaFH, Ru-deposited BaH2 (Ru/BaH2), and Ru/CaFxH2–x–CaF2 (x = 1) where Ru nanoparticles are deposited on the CaF1.0H1.0 solid solution formed by heating mixtures of orthorhombic CaH2 and cubic CaF2 at 550 °C are summarized in Supplementary Table 4. BaH2 and CaF1.0H1.0 solid solution are expected to be formed on Ru/CaFH, and either or both of them can contribute to the catalytic performance of Ru/CaFH. However, Ru/BaH2 had a much smaller catalytic activity for ammonia synthesis than Ru/CaFxH2–x–CaF2 (x = 1), which indicates that the catalysis of Ru/CaFH is derived from the CaF1.0H1.0 solid solution. Supplementary Table 4 also shows Ru/CaFxH2–x–CaF2 (x = 1) to be inferior to Ru/CaFH with respect to ammonia synthesis. This can be attributed to the conventional preparation method for the CaF1.0H1.0 solid solution. Ru/CaFxH2–x–CaF2 (x = 1) was prepared by the deposition of Ru nanoparticles. CaFxH2–x–CaF2 (x = 1) synthesized by high-temperature solid-state reaction at ≥550 °C for 20 h and the resultant surface area was very small (1 m2 g−1), which limits the catalytic activity of Ru/CaFxH2–x–CaF2 (x = 1). On the other hand, in the case of CaFH prepared by the new method, CaFH solid solution was formed on the surface with a surface area of 10 m2 g−1. This is considered to be the reason for the difference in activity between Ru/CaFH and Ru/CaFxH2–x–CaF2 (x = 1).
Electron-donating capability and reaction mechanism of Ru/CaFH
Ammonia synthesis from N2 and D2 over Ru/CaFH was examined to clarify the reaction mechanism. Ru/CaFH prepared at 340 °C in a flow of H2 alone was cooled down from 340 °C to 180 °C in a flow of Ar, and then N2–D2 was passed into Ru/CaFH at temperature under atmospheric pressure (see “Methods”). The experimental reaction time profiles for ammonia synthesis from N2 and D2 over Ru/CaFH are shown in Fig. 4. Soon after an increase in the m/z = 17 signal (NH3 and NDH as fragments of ND2H and NDH2), the signal of m/z = 18 (NDH2 and ND2 as a fragment of ND3) increased. The m/z = 19 (ND2H) signal was observed after ca. 3 min from the introduction of N2−D2. The fragment ratio of m/z = 17 (NH3), 16 (NH2), and 15 (NH) in pure NH3 was ca. 100:80:8, so that each fragment intensity did not exceed the parent intensity. The formation of ND3 (m/z = 20) was not observed within 10 min from the beginning of the reaction. As a result, NH3 was first formed, followed by the formation of NDH2 and ND2H; ammonia species containing H was formed at the early stage of ammonia synthesis from N2 and D2 over Ru/CaFH. These results indicate that H in the CaFH bulk is used for ammonia formation at the early stage of reaction, and H can move from CaFH bulk to the Ru surface to react with N adatoms. The same phenomenon had been observed on Ru nanoparticle-deposited Ca2NH (calcium nitride hydride)14.
XPS Ru 3p3/2 of Ru/CaFH was used to evaluate the electron-donating capability from CaFH to Ru (Supplementary Fig. 9). Ru 3p3/2 for Ru/CaFH appeared at a slightly lower binding energy than that for metallic Ru particles deposited on SiO2 (Ru/SiO2), which indicates that Ru on CaFH is more negative than Ru on SiO2. However, the difference was not so large, because XPS reflects only Ru atoms near the edges of Ru particles connected to CaFH from the point of view of the escape depth of photoelectrons. For this reason, we have adopted Fourier transform- infrared (FT-IR) spectroscopy measurements using N2 as a probe molecule, which is a more sensitive method (FT-IR, Fig. 5). Figure 5a measured at 25 °C showed N ≡ N stretching (νN2) bands of N2 adsorbed on Ru/CaH2 at 2100–2250 cm−1, lower than that of gaseous N2 (2744 cm−1), which indicated that the electron donation from the catalyst to the antibonding π* orbitals of adsorbed N2 via Ru d-orbitals (i.e., back donation) weakens the N ≡ N bond. The νN2 bands have been reported to appear at 2100–2300 cm−1 in highly active catalysts for ammonia synthesis19,26. However, these catalysts cannot function at low temperatures; such electron donation capability is insufficient to realize low-temperature ammonia synthesis. In the case of Ru/CaFH, νN2 was observed in the range of 2030–2150 cm−1, which is much lower than that reported for efficient catalysts, including Ru/CaH2. This can be clearly attributed to the high electron-donating capability of Ru/CaFH at room temperature. H2-TPD (Fig. 2a) and DFT experiments revealed that the abstraction of H atoms from CaFH by Ru forms CaFH with H− defects trapping electrons at ca. 50 °C, resulting in strong electron-donating power. Supplementary Fig. 10 shows an FT-IR spectrum (1550–1700 cm−1) for N-adsorbed Ru/CaFH at 25 °C (N2: 12 kPa) and a band assignable to δNH bending, which can be attributed to adsorbed ammonia from the broad band at ca. 1600 cm−1. This indicates that N2 molecules are dissociated into N adatoms, which react with H from CaFH even at 25 °C, and is consistent with the H2-TPD results and ammonia synthesis from N2 and D2.
To summarize these results, Fig. 5b shows a proposed reaction mechanism. In Ru/CaFH where a (111) surface is probably formed in the CaFH solid solution due to its stability, the bond strength of Ca−F surpasses that of Ca−H, which weakens Ca−H bonds in the CaFH solid solution, so that Ru can abstract H atoms from H‒ sites in CaFH to leave electrons (e‒) in these sites, even at ca. 50 °C. The resultant CaFH with H‒ vacancies that trap e‒ behaves as a surface electride with a small work function (Φ = 2.2 eV) that is much smaller than that of CaH2 (2.7 eV) and comparable with that of metallic potassium (2.3 eV). This high electron-donating capability originates from the strong electron repulsion between e‒ in the H‒ and F‒ vacancies, which significantly enhances electron donation from the electride to the π* orbitals of N2 molecules through the 3d orbitals of Ru. This facilitates the dissociative adsorption of N2, which results in ammonia formation at low temperatures.
Preparation of CaH2–BaF2 mixture and Ru/CaFH
First, a mixture of 87 mol% BaF2 (Wako Chemicals) and 13 mol% BaH2 (Stream Chemicals) was heated at 400 °C for 10 h in a flow of Ar (15 mL min–1) to put large and rigid BaF2 particles into disorder. The XRD pattern of the resulting material (modified BaF2) consisted of broad diffraction peaks due to BaF2 (Supplementary Fig. 11). No diffraction peaks due to BaH2 were observed in the XRD pattern of modified BaF2. Next, a simple mixture of CaH2 (Sigma-Aldrich) and the resulting modified BaF2 powders (Ca/Ba atomic ratios of 98:2, 9:1, 5:1, and 3:1) was heated at 340 °C for 10 h in a flow of H2 (2.5 mL min–1).
Ru/CaFH was prepared by two methods based on chemical vapor deposition using ruthenium acetylacetonate (Ru(acac)3). In Method 1, the resulting material (Ca/Ba atomic ratios of 98:2) obtained by the above procedure was heated with Ru(acac)3 (Sigma-Aldrich) for deposition of 12 wt% Ru at 260 °C for 2 h and at 340 °C for 10 h in a flow of H2 (2.5 mL min–1). In Method 2, Ru nanoparticles were loaded onto a mixture of CaH2 and BaF2 by chemical vapor deposition using Ru(acac)3 for deposition of 12 wt% Ru. The mixture of 98 mol% CaH2, 2 mol% modified BaF2, and Ru(acac)3 corresponding to 12 wt% Ru was heated at 260 °C for 2 h and at 340 °C for 10 h in a flow of H2 (2.5 mL min–1). There was no significant difference in ammonia synthetic activity and structure between the catalysts prepared by both methods. The results for the catalyst prepared by simple Method 2 are shown in this paper.
Preparation of solid solution CaFxH2–x–CaF2 and Ru/CaFxH2–x–CaF2
Appropriate amounts of CaF2 (Wako Chemicals) and CaH2 were mixed by grinding, and the mixture was heated at 550 °C for 20 h in a flow of Ar (15 mL min–1), which resulted in CaFxH2–x solid solutions (1.0 ≤ x ≤ 1.6). Ru/CaFxH2–x–CaF2 (x = 1) was prepared by heating CaFxH2–x–CaF2 (x = 1) and Ru(acac)3 corresponding to 12 wt% Ru at 260 °C in a flow of H2 (2.5 mL min–1). After 2 h, the sample was heated at 340 °C for 10 h in the H2 flow.
Preparation of Ru/CaH2, Ru/BaH2, and Ru/BaH2–BaO
According to previous reports18, Ru/CaH2, Ru/BaH2, and Ru/BaH2–BaO were prepared by heating CaH2, BaH2, and a mixture of 3 mol% BaO (Kojundo Chemical) and 97 mol% CaH2, respectively, with Ru(acac)3 corresponding to 10 wt% Ru at 260 °C in a flow of H2 (2.5 mL min–1). After 2 h, the samples were heated at 340 °C for 10 h in the H2 flow. The activities of both catalysts for ammonia synthesis increased with the Ru loading and reached their respective maximum at a loading of 10 wt% Ru.
Preparation of Cs–Ru/MgO
Cs–Ru/MgO was prepared according to previous reports2. MgO (Ube, 500A) was heated in high vacuum at 500 °C for 6 h and then stirred in a solution of Ru3(CO)12 in THF for 4 h at room temperature. After evaporating the solvent, the obtained powder was slowly heated to 450 °C in high vacuum to decompose the carbonyl precursor. The amount of Ru loading was 10 wt%. After the obtained gray powder was stirred in a solution of Cs2CO3 in dehydrated ethanol for 3 h, the solvent was evaporated. The resulting catalyst was dried in vacuum. The catalytic activity of Cs–Ru/MgO reached a maximum at loading of 10 wt% Ru.
Evaluation of catalytic performance
Typical ammonia synthesis was conducted in a silica-glass fixed-bed reactor (catalyst: 0.1 g) in a flow of N2 − H2 (N2:H2 = 1:3, 60 mL min–1, weight hourly space velocity (WHSV): 36,000 mL gcat–1 h–1) under atmospheric pressure (0.1 MPa). First, ammonia synthesis over each tested catalyst was conducted at 340 °C under the specified reaction conditions. When no increase or decrease in activity was observed for over 30 h, the catalyst was cooled down below 20 °C in a flow of N2 at a flow rate of 60 mL min–1 and then held under this flow for 5 h. After no ammonia was detected, the catalyst was heated at specific temperatures in a flow of N2−H2 (N2:H2 = 5:1, 60 mL min–1). Ammonia was analyzed by both direct mass spectrometry (BELMass, MicrotracBEL, Japan) and ion chromatography. There was no difference in ammonia formation rate between both methods. In the case of ion chromatography, the ammonia produced was trapped in 5 mM H2SO4 aqueous solution, and the amount of NH4+ generated in the solution was estimated using an ion chromatograph (LC-2000 plus, Jasco) equipped with a conductivity detector. The rate of ammonia formation was repeatedly measured more than three times after the ammonia formation rate remained constant for over 1 h. It was verified that the measured rate had an error of less than 10%. There was no difference in ammonia formation rate between direct mass spectrometry and ion chromatography.
Ammonia synthesis from N2 and D2
A mixture of 98 mol% CaH2, 2 mol% modified BaF2, and Ru(acac)3 corresponding to 12 wt% Ru was heated in the reactor at 260 °C for 2 h and at 300 °C for 10 h in a flow of H2 (2.5 mL min–1). The resultant Ru/CaFH was cooled down from that temperature to 180 °C in a flow of Ar at a flow rate of 2.5 mL min–1 and held under this flow for 5 h. After each mass signal intensity was kept constant, N2−D2 (N2: 5 mL min−1, D2: 15 mL min−1) was passed into Ru/CaFH at that temperature under atmospheric pressure. The outlet gas from the reactor was analyzed using mass spectrometry (BELMass, MicrotracBEL, Japan).
XRD (D8 Advance, Bruker) patterns were obtained using Cu Kα radiation. Nitrogen adsorption–desorption isotherms were measured at –196 °C with a surface-area analyzer (BELSORP-mini ΙΙ, MicrotracBEL) to estimate the Brunauer–Emmett–Teller (BET) surface areas. The morphology of the samples was examined using scanning electron microscopy (SEM, S-5500, Hitachi) equipped with an energy-dispersive X-ray spectroscopy (EDX, EMAX EX-250, Horiba) detector. The microstructural characteristics of the samples were determined from transmission electron microscopy (TEM, JEM-ARM 200 F, Jeol) observations. H2-TPD measurements were conducted by heating (1 °C min–1) a sample (ca. 100 mg) in a stream of Ar (30 mL min–1), and monitoring of the concentration of H2 with a thermal conductivity detector (TCD) and a mass spectrometer (BELMass, MicrotracBEL, Japan). FT-IR spectroscopy measurements of adsorbed N2 were conducted using a spectrometer (FT/IR-6100, Jasco) equipped with a mercury–cadmium–tellurium detector at a resolution of 4 cm−1. Samples were pressed into self-supported disks. A disk was placed in a sealed and Ar-filled silica-glass cell equipped with NaCl windows to a closed gas-circulation system to allow thermal adsorption–desorption experiments. The disk was heated under vacuum at 200 °C for 90 min. After the pretreatment, the disk was cooled to 25 °C under vacuum to obtain a background spectrum from the spectra of the N2-adsorbed samples. Pure N2 (99.99995%) was supplied to the system through a liquid-nitrogen trap. In all, 12 wt% Ru/CaH2 and 12 wt% Ru/CaFH were used for FT-IR measurements. XPS (ESCA-3200, Shimadzu, Mg Kα, 8 kV, 25 mA) was performed in conjunction with an Ar-filled glovebox. The samples were moved to the ultra-high-vacuum (UHV) XPS apparatus through the Ar-filled glovebox without exposure to the ambient air. The binding energy was corrected with respect to the Au 4f7/2 peak of Au-deposited samples.
The work functions of near-surface ions were calculated using the slab supercell model on the (111) plane, which is the most experimentally (cleavage plane) and theoretically (smallest surface energy) stable plane for fluorite crystals. The slabs were constructed by relaxing a bulk unit cell of cubic CaFH (5.465 A)17 and then stacking up the relaxed cell to form a slab. The slab was repeated periodically in the  direction with a vacuum gap of >20 Å to form a supercell. Surface relaxation was taken into account by further relaxation of the two layers on each surface of the slabs. Relaxation was terminated when the force on each atom became less than 0.01 eV Å−1. All the slab calculations were performed with a cut-off energy of 500 eV and a k mesh of 2 × 2 × 1. The slab thickness was varied between seven and ten layers to ascertain convergence with respect to thickness. The band structures for CaFH(111) solid solutions with H− or F− defects (CaFH1–x, CaF1–xH) were computed in this study. The results are shown in Supplementary Fig. 5. The work function of CaFH1–x was identical to that of CaF1–xH, and was estimated to be 2.2 eV. This value is smaller than that for CaH2 (2.7 eV), which suggests that fluorine with a larger electronegativity pushes the energy level of electrons up by electrostatic repulsion.
All relevant data that support the findings of this study are presented in the paper and supporting information. Source data are available from the corresponding author upon reasonable request.
Song, P., Kang, L., Wang, H., Guo, R. & Wang, R. Nitrogen (N), phosphorus (P)-codoped porous carbon as a metal-free electrocatalyst for N2 reduction under ambient conditions. ACS Appl. Mater. Interfaces 11, 12408–12414 (2019).
Hara, M., Kitano, M. & Kamata, K. Ru-loaded C12A7:e– electride as a catalyst for ammonia synthesis. ACS Catal. 7, 2312–2324 (2017).
Morgan, E. R., Manwell, J. F. & McGowan, J. G. Sustainable ammonia production from U.S. offshore wind farms: a techno economic review. ACS Sustain. Chem. Eng. 5, 9554–9567 (2017).
Yandulov, D. V. & Schrock, R. R. Catalytic reduction of dinitrogen to ammonia at a single molybdenum center. Science 301, 76–78 (2003).
Arashida, K., Miyake, Y. & Nishibayashi, Y. A molybdenum complex bearing PNP-type pincer ligands leads to the catalytic reduction of dinitrogen into ammonia. Nat. Chem. 3, 120–125 (2011).
Kitano, M. et al. Self-organized ruthenium-barium core-shell nanoparticles on a mesoporous calcium amide matrix for efficient low-temperature ammonia synthesis. Angew. Chem. 130, 2678–2682 (2018).
Lin, B., Wei, K., Ma, X., Lin, J. & Ni, J. Study of potassium promoter effect for Ru/AC catalysts for ammonia synthesis. Catal. Sci. Technol. 3, 1367–1374 (2013).
Dietrich, H., Jacobi, K. & Etrl, G. Vibrational analysis of the NH + N coadsorbate on Ru (0001). Surf. Sci. 377–379, 308–312 (1997).
Strongin, D. R. & Somorjai, G. A. The effects of potassium on ammonia synthesis over iron single-crystal surfaces. J. Catal. 109, 51–60 (1988).
Aika, K., Takano, T. & Murata, S. Preparation and characterization of chlorinefree ruthenium catalysts and the promoter effect in ammonia-synthesis. 3. A magnesia-supported ruthenium catalyst. J. Catal. 136, 126–140 (1992).
Rosowski, F., Hornung, A., Hinrichsen, O., Herein, D., Muhler, M. & Ertl, G. Ruthenium catalysts for ammonia synthesis at high pressures: preparation, characterization, and power-law kinetics. Appl. Catal. A 151, 443–460 (1997).
Harle, H., Mendel, K., Metka, U., Volpp, H. R., Willms, L. & Wolfrum, J. Temperature dependence (90-440 K) of the vibrational spectra of CO adsorbed on Platinum (111) studied by sum-frequency generation. Chem. Phys. Lett. 279, 275–281 (1997).
Carlsson, A. F., Baumer, M., Risse, T. & Freund, H. J. Surface structure of Co–Pd bimetallic particles supported on thin films studied using infrared reflection absorption spectroscopy of CO. J. Chem. Phys. 119, 10885–10894 (2003).
Kitano, M. et al. Essential role of hydride ion in ruthenium-based ammonia synthesis catalysts. Chem. Sci. 7, 4036–4043 (2016).
Ong, P. V., Johnson, L. E., Hosono, H. & Sushko, P. V. Structure and stability of CaH2 surfaces: on the possibility of electron-rich surfaces in metal hydrides for catalysis. J. Mater. Chem. A 5, 5550–5558 (2017).
Luo, Y. R. Comprehensive Handbook of Chemical Bond Energies (CRC Press, Boca Raton, FL, 2007).
Mizoguchi, H. et al. Cubic fluorite-type CaH2 with a small bandgap. J. Am. Chem. Soc. 139, 11317–11320 (2017).
Hattori, M. et al. Enhanced catalytic ammonia synthesis with transformed BaO. ACS Catal. 8, 10977–10984 (2018).
Kitano, M. et al. Ammonia synthesis using a stable electride as an electron donor and reversible hydrogen store. Nat. Chem. 4, 934–940 (2012).
Liu, H., Nian, X. & Hu, Z. Development of novel low temperature and low pressure ammonia synthesis catalyst. Appl. Catal. Gen. 142, 209–222 (1996).
Sato, K. et al. A low-crystalline ruthenium nano-layer supported on praseodymium oxide as an active catalyst for ammonia synthesis. Chem. Sci. 8, 674–679 (2017).
Wang, P. K. et al. Breaking scaling relations to achieve low-temperature ammonia synthesis through LiH-mediated nitrogen transfer and hydrogenation. Nat. Chem. 9, 64–70 (2017).
Gao, W. B. et al. Barium hydride-mediated nitrogen transfer and hydrogenation for ammonia synthesis: a case study of cobalt. ACS Catal. 7, 3654–3661 (2017).
Ogura, Y. et al. Efficient ammonia synthesis over a Ru/La0.5Ce0.5O1.75 catalyst pre-reduced at high temperature. Chem. Sci. 9, 2230–2237 (2018).
Ogura, Y. et al. Ru/La0.5Pr0.5O1.75 catalyst for low-temperature ammonia synthesis. ACS Sustain. Chem. Eng. 6, 17258–17266 (2018).
Kubota, J. & Aika, K. Infrared studies of adsorbed dinitrogen on supported ruthenium catalysts for ammonia synthesis: effects of the alumina and magnesia supports and the cesium compound promoter. J. Phys. Chem. 98, 11293–11300 (1994).
This work was supported by a fund from the Grants-in-Aid for Japan Society for the Promotion of Science (JSPS) Fellows and for Scientific Research from the Ministry of Education, Culture, Science, Sports, and Technology (MEXT) of Japan (19K15358, 18H05251, and 17H06153).
The authors declare no competing interests.
Peer review information Nature Communications thanks the anonymous reviewers for their contribution to the peer review of this work. Peer reviewer reports are available.
Publisher’s note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.
About this article
Cite this article
Hattori, M., Iijima, S., Nakao, T. et al. Solid solution for catalytic ammonia synthesis from nitrogen and hydrogen gases at 50 °C. Nat Commun 11, 2001 (2020). https://doi.org/10.1038/s41467-020-15868-8
Scientific Reports (2021)