Improved catalytic combustion of methane using CuO nanobelts with predominantly (001) surfaces

  1. Qingquan Kong1ORCID Logo,
  2. Yichun Yin2,
  3. Bing Xue3,4,
  4. Yonggang Jin5,
  5. Wei Feng1,
  6. Zhi-Gang Chen6,
  7. Shi Su5 and
  8. Chenghua Sun7ORCID Logo

1School of Mechanical Engineering, Chengdu University, Chengdu 610106, Sichuan, PR China
2School of Chemistry, Faculty of Science, Monash University, VIC 3800 Australia
3CSIRO Energy, PO Box 883, Kenmore, QLD 4069 Australia

4School of Environment and Resources, Southwest University of Science and Technology, Mianyang 621000, PR China
5CSIRO Energy, 1 Technology Court, Pullenvale QLD 4069, Australia
6Centre for Future Materials, University of Southern Queensland, Springfield QLD 4300, Australia
7Department of Chemistry and Biotechnology, Faculty of Science, Engineering & Technology, Swinburne University of Technology, Hawthorn, VIC 3122, Australia

  1. Corresponding author email

Associate Editor: J. J. Schneider
Beilstein J. Nanotechnol. 2018, 9, 2526–2532.
Received 12 Jun 2018, Accepted 10 Sep 2018, Published 24 Sep 2018


Through computational calculations, CuO(001) has been identified as an active surface for methane oxidation. Experimental validation with CuO nanobelts comprised of predominantly (001) surfaces has been performed and it is confirmed that the performance of such nanobelts is much higher than normal nanoparticles and nanowires. First principle calculations further clarified that two-coordinated oxygen plays a key role for methane adsorption and oxidation.

Keywords: catalytic oxidation; copper oxide; density functional theory; methane


Methane (CH4), as the main component of natural gas, offers significant environmental advantages over conventional gasoline and diesel [1-3]. However, its thermal combustion is often at a flame temperature up to ≈2,000 K [4], which favours the formation of nitrogen oxide (NOx) pollutants. To suppress such reactions, a lower flame temperature is targeted, but this potentially results in incomplete combustion with large CO and unburned hydrocarbon (UHC) emissions [5], which underlines the need to develop high-performance catalysts for CH4 oxidation at low temperature. Except as fuel in natural gas, much of the CH4 that is released is from industrial applications, such as ventilation air methane (VAM) from underground coal mining. This is a serious issue because CH4 has severe global warming effects, around 25 times greater than that of carbon dioxide (CO2). For a more efficient use of natural gas and to minimize the direct emission of CH4, the catalytic oxidation of CH4 at low temperature has been investigated extensively over the last decades [5-8].

Noble metals have been reported as effective catalysts for the complete oxidation of methane [2,5,9-17], particularly supported Pd nanoparticles [15-17], while the high price and poor thermal stability limit their large scale application. To address this issue, low-cost alternatives, such as transition metal (TM) oxides and various complex structures (e.g., perovskite, spinel and hexaaluminate) have been tested as catalysts for CH4 oxidation. But so far their performance is still much lower than noble metals. An ideal catalyst for CH4 oxidation should have a high capacity to adsorb CH4 (particularly important for CH4 oxidation at low concentration, for example, VAM mitigation), activate the C–H bond and split the O2 molecule. However, exposed catalyst surfaces are often highly stable and thus can hardly satisfy all of the above criteria, which explains the poor performance of most metal oxides.

To improve the reactivity of metal oxides, surfaces with high energy (and thus low surface area), namely minority surfaces, may offer new opportunities. Although minority surfaces often diminish quickly during crystal growth due to their low stability, they can be stabilized by controlling the synthesis conditions, as previously demonstrated in the literature [18-20]. In terms of reactivity, minority surfaces have a large amount of lowly coordinated atoms that can be actively involved in surface reactions, including adsorbing CH4 and stabilizing intermediates [7]. Following this strategy, this work explores the catalysis of copper oxide (CuO), a promising catalyst for CH4 oxidation as identified in the literature [8]. Different from these reports, we focus on the performance of the minority surface (001).

Results and Discussion

Starting with computational calculations, CuO surfaces with low indexes (including (110), (111), (101), (010), (011) and (001)) have been systematically screened under the scheme of density functional theory. The stability of these surfaces has been reported earlier as (010) > (011) > (100) > (101) > (110) > (001) [21], according to which 001 is the most reactive surface, which is consistent with our work as demonstrated below.

Two indicators, namely the adsorption energy (AE) and dissociation energy (DE, energy change from physical adsorption to dissociative adsorption), are employed for the analysis. The surface models are shown in Figure 1a. Given that the catalysts are exposed to abundant oxygen, O or O/Cu-mixed termination is employed in the models. Among them, five are featured with mixed O/Cu surface atoms, except (001) which is fully covered by two-coordinated oxygen (O2c) before it is relaxed. Very recently, O2c has been identified as an active site for CH4 oxidation in the case of Co3O4 whereby CuO(001) offers an ideal opportunity to test this hypothesis [22].


Figure 1: Computational screening. (a) Models for six low-index surfaces (unrelaxed); (b) Calculated values of AE and DE. Cu and O are shown as rose-carmine and red, respectively.

The AE and DE are calculated and presented in Figure 1b, with negative AE (DE) indicating that the adsorption (dissociation) is favorable. Based on the calculated AE, it is found that the physical adsorption of CH4 on (101), (011), (010) and (001) can occur without additional energy input, with an AE between −0.22 and −0.86 eV. The (001) surface, with AE = −0.86 eV, has been identified as the surface that offers the strongest adsorption capacity among all these surfaces. For CH4 oxidation, the dissociation to form CH3 and H is critical and difficult because strong C–H bonds need to be broken; therefore, the calculated DE is indicative of the oxidation difficulty. Interestingly, the (001) surface has been identified again as the most reactive surface for CH4 dissociation, with DE = −2.16 eV, which is much higher than that of the other surfaces. On the basis of the above computational screening, (001) is the optimal surface for CH4 oxidation among these tested surfaces. From the analysis of the surface, this is not surprising because (001) is strongly polarized and shows high reactivity due to the high ratio of lowly coordinated oxygen – a feature that has been employed for gas sensing and Li-ion batteries [21].

Now we turn to the experimental validation, starting with the synthesis of CuO nanowires (NWs) and CuO nanobelts (NBs) comprised of predominantly (001) surfaces, which is performed based on the method reported by Van Tendeloo et al. [23]. For the NWs and NBs synthesized in this work, a high percentage of the surface area can be attributed to (001) surfaces, particularly for the NBs whose (001) surfaces are the predominant surface found, as examined by transmission electron microscopy (TEM). Figure 2a,b shows the NWs which have a diameter of 20–100 nm and length of 1–3 μm, and Figure 2c shows the thin NBs, with a width of 200–300 nm and a length of ≈1 μm. The selected area electron diffraction patterns (SAED), projected from the [1] zone axis of the yellow square area (see the inset in Figure 2c), reveals the monoclinic structure and that the diffraction spots are ascribed to the (110), (−110), and (020) planes. High-resolution TEM images, as shown in Figure 2d, confirm that the exposed surface of the NBs is the (001) facet and the edge is (100). As shown in an early study [21,23], CuO NWs or NBs having predominantly (001) surfaces can be obtained when Cu(OH)2 is employed as a nanowire precursor for decomposition. The mechanism of shape-reserved transformation from Cu(OH)2 to CuO has been previously discussed in the literature [24-26].


Figure 2: CuO catalyst characterization. (a,b) TEM images of CuO NWs; (c) TEM image of CuO NBs (inset is the SAED pattern of the selected yellow square area); (d) HRTEM along the [1] direction; (e,f) TEM images of a CuO nanobelt after catalysis tests at 650 °C.

Prior to the performance tests, the crystal structure of the collected samples was further examined by X-ray diffraction with commercial CuO nanoparticles (NPs, Aldrich 450812) as a reference for comparison. The NP, NW and NB samples show the similar profiles, confirming that they have the same phase (CuO, space group: C2/c2(15), a = 4.685 Å, b = 3.425 Å, c = 5.130 Å), as shown in Figure S1, Supporting Information File 1. However, the NB sample shows a much stronger (002) peak, suggesting a preferred (001) termination. It is also found that the NP, NW and NB samples have a similar surface area of around 1 m2/g as measured by the Brunauer–Emmett–Teller (BET) method from N2 adsorption isotherms at 77 K, suggesting that the performance difference presented below does not come from the difference of the surface area.

We now compare the catalytic performance of different CuO catalysts for CH4 oxidation. We began with catalytic oxidation tests, starting from 150 °C up to the maximum testing temperature, Tmax = 850 °C. After the first cycle of the test (denoted as C1), the catalytic bed was cooled down from 850 to 150 °C followed by the second test cycle (C2). Figure 3a shows the C1-performance of the NP, NW and NB samples where the oxidation activity follows the order: NBs > NWs > NPs. It is particularly notable that the NB performance is even close to that of 1% Pd loaded on Co3O4 [27], which itself shows excellent catalytic capacity. Supermolecular Pd@CeO2 core–shell structures can offer exceptionally high performance for methane oxidation, achieving complete conversion even below 400 °C [6]. Different from Pd catalysts, CuO NBs, as a low-cost metal oxide material, do not have to be loaded on a support and do not use additional dispersion agents, and are thus a more effective catalyst per volume and weight when assembled on the reactor.


Figure 3: CH4 conversion against the temperature. (a) Heating profile (Tmax = 850 °C) for NBs, NWs and NPs, with 1% Pd/Co3O4 as a reference. (b) Heating profile (Tmax = 600 °C) for NBs tested for three cycles, labelled as C1, C2 and C3.

The aggregation of catalyst nanoparticles upon high-temperature calcination is a typical issue for CH4 oxidation, which was also observed in our experiments. All three CuO catalysts demonstrated poor thermal stability leading to significantly deteriorated catalytic performance in C2 compared to that in C1 when the combustion temperature was as high as 850 °C. Therefore, CH4 oxidation catalyzed by NBs at lower temperature (600 °C) was tested, and the results are shown in Figure 3b. These results show that the catalytic performance can be kept stable after three circles, achieving T10 = 375–378 °C, T50 = 468–475 °C, T90 = 544–562 °C and around 97% of CH4 conversion at 600 °C, indicating that the belt shape may be helpful to suppress catalyst aggregation. However, the stability is still poor as the nanobelts tend to aggregate when high temperature treatment is employed (650 °C) as shown in Figure 2e. Moreover, the surface layers show higher crystallization after catalysis tests, as shown in Figure 2f, indicating that additional efforts to improve the thermal stability of these nanostructures is needed.

Although the calculated AE and DE can provide an explanation for the effect of morphology on catalysis performance, we further investigated the mechanism of full CH4 oxidation over CuO(001), which is informative for the further improvement and the design of new catalysts. Generally, Cu does not show strong magnetization in its neutral or fully oxidized forms, but spin-polarization for lowly coordinated Cu on the surface and radicals involved in CH4 oxidation deserves serious consideration. For instance, the difference in calculated adsorption energies with and without spin-polarization can be as high as 0.1–0.2 eV, with geometries showing slight differences too. Therefore, all energies and geometries shown below are based on spin-polarized calculations.

Starting from clean (001), CH4 is firstly adsorbed with AE = −0.86 eV, followed by a spontaneous dissociation with CH3 and H adsorbed on surface oxygen, as depicted in Figure 4a–c. Similar as discussed in an early publication [28], surface oxygen is often actively involved and may cleave H from CHx to form –OH and H2O, generating an oxygen vacancy (OV), which can be filled with reactant O2, leading to its dissociation and further oxidizing CHx intermediates, as shown in Figure 4d–f. With oxygen transferring to bond with carbon, the hydrogen in CHx can shift to surface oxygen again with an energy release of 3.66 eV and 1.46 eV, indicating that such a shift is highly favorable, as shown in Figure 4g–i. Again, an OV is generated and refilled by O2 when H2O is released, and similarly O2 is dissociated to release atomic oxygen after exceeding the small barrier of 0.47 eV, which can oxidize adsorbed CO to form CO2, as outlined in Figure 4i–l.


Figure 4: CH4 oxidation mechanism by computational calculations. (a) Clean (001); (b) CH4 physical adsorption; (c) CH4 dissociative adsorption; (d) CH2* with oxygen vacancy (OV) presented; (e) CH2* with O2 adsorbed; (f) CH2* rotating and interacting with O2*; (g) transition state (TS) state COH2*; (h) CHO* + H*; (i) CO* with OV presented after releasing one H2O; (j) CO* with O2 adsorbed; (k) TS for O transfer to CO*; (l) CO2 physical adsorbed. Cu, O, C and H are shown as rose-carmine, red, grey and white spheres, respectively.

The energy profile for the above full process is given in Figure 5 in units of eV, using the total energy of a clean (001) surface and free gas-phase CH4 and O2 as the reference. According to the results, the early oxidation to release the first H2O (oxygen is from the surface) is exothermic and generates an OV (see Figure 4c). This is followed by O2 dissociation which occurs over the vacancy with a maximum energy barrier of 0.91 eV. This is informative because it indicates that the key role of OV is to activate O2 and release a highly active oxygen atom, although a barrier of 0.91 eV is found for O2 dissociation in the case of CuO(001), but the dehydrogenation from CHx becomes exothermic, confirming the importance of surface oxygen and oxygen vacancies, as suggested by Hu et al. [22] and Jin et al. [28]. According to this understanding, the catalysis performance may be further improved by adding alloy elements or surface doping to reduce the barrier.


Figure 5: Energy profile for CH4 oxidation. The geometries are shown in Figure 4.


In summary, Cu(001) was identified as being the most promising among six low-index surfaces tested for CH4 oxidation based on the criteria of adsorption energy and dissociation energy. These calculations were experimentally examined with the use of CuO NBs comprised of predominantly (001) surfaces, which performed better than CuO NBs and NPs, achieving almost complete oxidation at a temperature of 600 °C. CuO NBs, employed as low-cost catalysts, can be used without additional agents to disperse or support them. They can therefore be loaded with higher concentration in limited space or weight applications, making CuO NBs a promising replacement to expensive Pd-based catalysts. Additional efforts are needed to improve the thermal stability of such nanostructures as they tend to aggregate after high temperature treatment.


Synthesis of CuO nanowires and nanobelts

For a typical sample, 1 g of Cu(NO3)2 was dissolved in 100 mL distilled water and 30 mL ammonia solution (NH3·H2O, 0.15 mol/L) was added under vigorous stirring. Then, NaOH solution (1 mol/L) was added dropwise to the above solution and the pH value was adjusted to 9–10. The resulting blue Cu(OH)2 precipitate was filtered and washed several times with distilled water to obtain a solid product. CuO NWs were prepared by heating one part of the as-obtained solid product at 130 °C for 10 h in an oven. The other part was dissolved in 50 mL distilled water, then transferred to an autoclave and hydrothermally treated at 130 °C for 10 h. The black solid product was washed with deionized water and dried at 60 °C overnight to get CuO NBs [23].

Methane catalytic oxidation test

Methane catalytic oxidation experiments were carried out in a fixed-bed reactor (U-shaped quartz tube) with an inner diameter of 6 mm at atmospheric pressure. 35 mg of the catalysts was loaded into the reactor and supported by quartz wool. A mixed reaction gas containing 0.6 vol % CH4, 19.6 vol % O2, 0.15% CO2 and balance N2 was flowed through the catalyst bed at a flow rate of 20 mL min−1, corresponding to a gas hourly space velocity of 34,000 mL h−1 g−1. Prior to the catalytic tests, the catalyst was pretreated under the reaction atmosphere for 60 min at 250 °C and then cooled down to 150 °C. Once the temperature was stable at 150 °C, CH4 oxidation catalytic performance was evaluated by heating the catalyst bed at 10 °C min−1 to 850 or 600 °C. The composition of the effluent gases were monitored on-line using a quadrupole mass spectrometer (Hiden MS HPR20) with a secondary electron multiplier detector. Methane conversion was defined as: (influent concentration of CH4 − effluent concentration of CH4)/influent concentration of CH4 × 100%.

Theoretical calculations

Spin-polarized DFT calculations were performed under the generalized gradient approximation (GGA) [29] together with the functional by Perdew, Burke, and Ernzerhof [30], which was embedded in the Vienna Ab-Initio Simulation Package [31]. The calculation was carried out with a kinetic cutoff energy of 380 eV, with the use of the projector augmented wave (PAW) method. The k-space was sampled by the gamma point based on our tests. The k-point and cutoff energy were tested with higher computational settings, as 3 × 3 × 1 and 450 eV, leading to the difference of less than 0.1 eV in terms of the adsorption energies. The van der Waals (vdW) interaction was considered with the use of the DFT-D3 method, as developed by Grimme and Jónsson [32,33]. The CuO surfaces were modelled by 2 × 2 supercells, shown as slabs with thicknesses in the range of 10–14 Å, depending on the surface orientation, and a vacuum space of 12 Å was applied over the surface. The transition state (TS) was identified through the dimer method [33], for which the searching is carried out by a series of intermediate states generated among the reaction path towards the formation of the product and further optimized with one static degree of freedom (in our case, one bond length associated with the change from reactant to product). Based on our tests, both spin-polarization and vdW corrections are necessary, especially for the calculation of intermediate radicals involved in CH4 oxidation (e.g., CH2*, CH* and O*).

During the quick screening of surfaces for CH4 adsorption, the adsorption energy (AE) and dissociation energy (DE) from physical adsorption to dissociative adsorption have been employed, which are defined as follows.

AE = E(CH4*) – E(surface) – E(CH4-gas phase)

DE = E(CH3*-H*) – E(CH4*)

To understand the catalysis mechanism, full methane oxidation, CH4 + 2O2 → CO2 + H2O, has been investigated in which the total energy of CH4, CO2 and H2O was calculated as −24.02 eV, −23.64 eV and −14.23 eV, respectively. The total energy of O2 was derived from H2O and H2, giving −9.97 eV. Based on the above, the reaction energy for CH4 oxidation was calculated as −8.14 eV, which is close to the experimental data (ΔH = −8.31 eV at room temperature).

Supporting Information

Supporting Information File 1: X-ray diffraction profile.
Format: PDF Size: 129.1 KB Download


This work is supported by National Natural Science Foundation of China (Grant Nos. 51302231, 11572057), the Australian Research Council through Discover Project (DP130100268, DP140100193, DP150100056, CS & ZC) and Future Fellowship (FT130100076, CS) and CSIRO Energy. The authors thank the National Computational Infrastructure (NCI) for providing the computational resources. We acknowledge the use of facilities within the Monash Centre for Electron Microscopy and ARC funding (LE110100223).


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