Identifying the nature of the active sites in methanol synthesis over Cu/ZnO/Al2O3 catalysts


The heterogeneously catalysed reaction of hydrogen with carbon monoxide and carbon dioxide (syngas) to methanol is nearly 100 years old, and the standard methanol catalyst Cu/ZnO/Al2O3 has been applied for more than 50 years. Still, the nature of the Zn species on the metallic Cu0 particles (interface sites) is heavily debated. Here, we show that these Zn species are not metallic, but have a positively charged nature under industrial methanol synthesis conditions. Our kinetic results are based on a self-built high-pressure pulse unit, which allows us to inject selective reversible poisons into the syngas feed passing through a fixed-bed reactor containing an industrial Cu/ZnO/Al2O3 catalyst under high-pressure conditions. This method allows us to perform surface-sensitive operando investigations as a function of the reaction conditions, demonstrating that the rate of methanol formation is only decreased in CO2-containing syngas mixtures when pulsing NH3 or methylamines as basic probe molecules.


The high consumption of fossil fuels causes the emission of greenhouse gases and enhances global warming. Therefore, it is the aim of current research to find alternative energy sources and renewable raw materials. One possible alternative is methanol, which is used in a wide range of applications as basic chemical, fuel additive as well as energy carrier1,2. It has a high potential to substitute hydrocarbons originating from fossil fuels in many areas3. Nowadays, methanol is still industrially produced by the heterogeneously catalysed conversion of syngas, a gas mixture containing CO, CO2 and H2 obtained from natural gas or coal, over Cu/ZnO/Al2O3 catalysts at elevated temperatures and pressures4. For a methanol production with low CO2 footprint, the mixing of exhaust gases from steel production with sustainably produced H2 from water electrolysis is a promising route to achieve the gas composition of conventional syngas mixtures5. However, many known and unknown impurities in the ppm as well as in the ppb range may be present in such an off-gas-derived syngas, and the effects of most impurities on the catalytic activity, selectivity and stability cannot be predicted with certainty in view of the lack of poisoning studies in literature6,7. These impurities can interact as irreversible poisons, which strongly interact with the active sites, or as reversible poisons, which can be desorbed from the active sites and flushed out of the reactor8,9. In case of reversible poisoning, the poisons can act as selective probe molecules adsorbing on the active sites without irreversible deactivation. Thus, selective poisoning may allow gaining new insight in the nature of the active sites10.

The active site for methanol formation of the industrial Cu/ZnO/Al2O3 catalyst has been under debate over the last decades. Recent models are the Cu0–Zn0 surface alloy proposed by the Nakamura and Chorkendorff groups11,12, Znδ+ species at the defective Cu0 surface claimed by the Schlögl group13, graphitic-like ZnOx layer on the Cu0 particles also suggested by the Schlögl group14, and ZnO on the top layer of the Cu0 particles postulated by the Rodriguez group15. All models are based on strong metal support interactions (SMSI)16 resulting in Cu–Zn interface sites that are essential for a highly active catalyst, but they differ in the nature of the Zn species in close contact with Cu0, which are controversially debated to be metallic or positively charged. The most active site of methanol synthesis is described as metallic Zn species alloyed into defined Cu0 steps13. Furthermore, it is proposed that high coverages of oxygen-containing intermediates like formate only exist under industrially relevant high-pressure conditions and lead to a partial oxidation of the metallic Zn sites due to the oxophilic nature of Zn compared with Cu013. However, there is no characterisation method available for the Cu/ZnO/Al2O3 catalyst typically operated above 200 °C and 50 bar4, which is able to identify this oxidising effect, because the adjustment of both high-temperature and high-pressure conditions and surface sensitivity is technically impossible for typical single-crystal investigations11, transient in situ experiments17,18, adsorption and desorption studies12,19, in situ infrared (IR) spectroscopy11,20, N2O frontal chromatography12,19, X-ray photoelectron spectroscopy (XPS)11,12,15,19, ambient pressure XPS13, neutron scattering13, microcalorimetry21,22, scanning tunnelling microscopy11, in situ IR reflection-absorption spectroscopy11, high-resolution transmission electron microscopy (TEM)14,23, in situ TEM24, electron energy loss spectroscopy14, in situ X-ray absorption spectroscopy16, or operando X-ray diffraction25. To confirm the positive charge of the Zn species in close contact with Cu0, we establish a surface-sensitive operando method, which allows us to inject selective reversible poisons as probe molecules such as NH3 into the syngas feed. By applying this high-pressure pulse unit (HPPU), we are able to identify the nature of the active sites of the working Cu/ZnO/Al2O3 catalyst under industrially relevant conditions. In detail, we perform conventional methanol synthesis over an industrial Cu/ZnO/Al2O3 catalyst with CO/CO2-containing syngas mixtures above 200 °C and at 60 bar. We investigate the reversible poisoning mechanism of NH3 as well as of different types of methylamines and define the corresponding inhibition strength by the non-produced amount of methanol over a defined period of time. Parallel to the reversible poisoning by the amines, we co-feed ethylene into the syngas mixture, which is fast hydrogenated to ethane, we investigate the reversible poisoning mechanism of NO, and we change the syngas mixture from CO2- to CO-free gas mixtures to clearly confirm that the methanol synthesis catalyst exposes both highly active Cu0–Znδ+ sites and metallic Cu0 sites. At the end, the obtained results are discussed in view of the controversial debate on the active site in methanol synthesis demonstrating that the chosen reaction conditions and the time on stream (TOS) control the structure of the catalyst surface.


High-pressure pulse experiment (HPPE)

The self-built HPPU enabled us to inject defined amounts of probe molecules as pulses into the syngas stream under methanol synthesis conditions (210 °C, 60 bar). In this way, a variety of valuable kinetic results can be collected in a short period of time without disturbing the main reaction on the surface sites for a too long period of time to minimize possible irreversible structural transformations. When injecting N-containing compounds acting as reversible poisons, the temporary blocking of active sites only occurs when the poison is present in the feed gas stream, which is exemplarily shown for NH3 in Fig. 1a.

Fig. 1: High-pressure pulse experiments and the determined inhibition strengths.

a Recorded methanol (black curves) and NH3 (blue curves) mole fractions during the injection of pulses with different NH3 partial pressures over the Cu/ZnO/Al2O3 catalyst (conditions: 210 °C, 60 bar, 13.5% CO, 3.5% CO2, 73.5% H2, 9.5% N2). b Correlation of the determined ΔnMeOH (non-produced amount of methanol over a defined period of time) values (Supplementary Note 1) with the injected mole fractions of the investigated N compounds (NH3 red squares and line, NO black points and line, monomethylamine (MMA) blue triangles and line, dimethylamine (DMA) violet stars and line, trimethylamine (TMA) orange diamonds and line). The corresponding pulse experiments are shown in Supplementary Figs. 15. a, the slope of the corresponding linear interpolation, is defined as the inhibition strength.

A typical HPPE consists of three steps: First, steady state with clean syngas has to be established. The second step is the injection of the probe molecule as a pulse passing through the catalyst bed, and in the third step the period of time is determined until the initial rate of methanol formation is recovered. The pulsing of pure N2 (0% NH3 in Fig. 1a) illustrates that the used low mole fractions of reversible poisons as well as the high inert content in the sample loop lead to a temporary dilution of the product stream. This sharp negative pulse present in every HPPE is neglected for the interpretation of the results. The rising partial pressure of NH3 leads to an increasing loss of methanol activity after the temporary dilution and to longer regeneration times. In addition to the methanol mole fraction (black curves), the NH3 mole fractions (blue curves) were also monitored. For the experiment with 0.05% NH3, no NH3 signal was detected, since it is converted to the methylamines monomethylamine (MMA), dimethylamine (DMA) and trimethylamine (TMA) (Supplementary Fig. 10) reacting with oxygen-containing intermediates of methanol synthesis such as formate26,27. This means that the NH3 signal of the 0.5% HPPE represents the part of the injected NH3, which does not interact with the catalyst surface, because the position of the signal is equal to the temporary dilution. Obviously, the adsorbed NH3 species and syngas reactants are part of adsorption equilibria, so that a complete deactivation of methanol synthesis is not possible with a reversible poison in contrast to an irreversible one8,28.

In the same way, MMA (Supplementary Fig. 2), DMA (Supplementary Fig. 3) as well as TMA (Supplementary Fig. 4) were also injected as pulses into the feed gas stream under high-pressure conditions to better understand the reversible poisoning mechanism of NH3. NO was also used (Supplementary Fig. 5), which is hydrogenated to NH3 and H2O (Supplementary Fig. 11). All investigated N compounds act as reversible poisons, and for the comparison of the different poisoning strengths the relevant methanol mole fractions were integrated to obtain the non-produced amount of methanol ΔnMeOH during the required period of regeneration time (Supplementary Note 1, Supplementary Fig. 6). The correlation of the calculated values ΔnMeOH with the different mole fractions of the reversible poisons is shown in Fig. 1b. The ΔnMeOH values for every corresponding poison correlate linearly with the mole fraction of the poison for values below 0.2% under the investigated conditions. Above this mole fraction, the poisoning strength reaches a stationary regime due to the limited deactivation effect of reversible poisons, exemplarily shown for NH3 (injection of 0.4 and 0.5%). The linear trend of the curves in Fig. 1b can be easily predicted with a one-parameter function through the origin. Here, the slope is defined as the inhibition strength a, and the corresponding values are shown in Fig. 1b. When comparing the determined values for the individual inhibition strengths, the following sequence is obtained, in which NH3 is the strongest reversible poison and TMA the weakest:

$${\mathrm{NH}}_{\mathrm{3}}{\mathrm{ > NO > DMA}} \approx {\mathrm{MMA > TMA}}.$$

The consecutive reaction of NH3 to TMA is one reason for this correlation. NH3 requires the highest number of methylation steps until the final product TMA is formed, resulting in the longest blocking of active sites as well as in the highest consumption of oxygen-containing intermediates26,27. In contrast, TMA only blocks the active sites by adsorption, since no further methylation is possible (Supplementary Fig. 10b), leading to the shortest residence time on the surface and the lowest inhibition strength. In principle, MMA should be a stronger poison than DMA, but Fig. 1b shows that the inhibition strength of DMA is only slightly higher. Thus, it can be assumed that the methylation steps are fast and a clear distinction between both methylamines is difficult to identify at 210 °C and not observable at 250 °C (Supplementary Fig. 10b). The inhibition strength of NO should also be higher than that of NH3 due to the additional hydrogenation step, but the poisoning by NH3 and NO proceeds in different ways as explained in Fig. 2.

Fig. 2: Continuous dosing experiments coupled with HPPEs.

a Continuous dosing of 1% of ethylene (blue curve), which is hydrogenated to ethane (green curve) under methanol (black curve) synthesis conditions, coupled with HPPEs with NH3. b Comparison of the continuous dosing of 0.05% NH3 with the continuous dosing of 0.2% NO. The black bars describe the initial methanol mole fraction in pure syngas (yMeOH, initial) and in the presence of the corresponding impurity (yMeOH, poisoned). The red bars describe the dosed mole fraction of NH3 (yNH3, dosed) and mole fraction in the product gas stream (yNH3, effluent). The blue bar (yNO, dosed) stands for the dosed mole fraction of NO. XNH3 describes the corresponding degree of NH3 conversion to the three methylamines: monomethylamine (orange bar), dimethylamine (grey bar) and trimethylamine (violet bar). c Syngas switching experiments from CO/CO2/H2 to CO/H2 and back to CO/CO2/H2 at 210 °C and 60 bar coupled with HPPEs with NH3. Here, the resulting methanol (black curve) and NH3 (green curve) mole fractions in the product gas stream are shown. The images visualize the oxidative effect of CO2 in the syngas mixture and the corresponding interaction of NH3 with the catalyst surface. Orange area = Cu0 sites, blue area = Znδ+/ZnO sites, grey area = Zn0 sites.

Probing the presence of two different active sites

From the first HPPEs, it can be seen that different types of N compounds interact with the active sites of the Cu/ZnO/Al2O3 catalyst resulting in the observed decrease of methanol formation. Therefore, our work was focused on the identification of the nature of these active sites and on answering the question as to whether other surface sites play an important role. For these investigations, only the probe molecules NH3 as reacting N compound (Fig. 2) and TMA as blocking N compound (Supplementary Fig. 12) were considered. The freshly reduced Cu/ZnO/Al2O3 catalyst has various types of Lewis and Brønsted acid sites with different acid strengths. Actually, the Cu/ZnO/Al2O3 catalyst developed for industrial reactors is a multi-site system. According to its composition, three different types of adsorption sites can be present13,29,30: the Cu–Zn interface, unpromoted metallic Cu0 sites, and sites exposed by ZnO. In addition, every type of exposed surface is non-uniform due to the presence of vacancies, steps and kinks13. In general, the Cu:Zn ratio as well as the synthesis route is chosen in such a way that an intimate contact between Cu and ZnO is achieved to maximize the number of Cu–Zn interface sites. A significant influence of pure ZnO sites under the conditions of the low-temperature methanol synthesis can be neglected31, and the absence of acidic OH groups on the structural promoter Al2O3 is also excluded due to the absence of acid-catalysed products such as dimethyl ether (Supplementary Note 3)4. For Al2O3, it is generally accepted that it acts as physical spacer to enhance the lifetime as well as the surface area of the Cu/ZnO catalyst maintaining economical methanol production rates over several years4. No evidence can be found in literature that Al2O3 is involved in the reaction mechanism of methanol formation or in the formation of the active sites32,33.

The hydrogenation of ethylene and NO was analysed in detail (Fig. 2a, b) to identify the presence of different Cu sites, which has already been claimed in several publications13,17,29,30. Figure 2a shows that the continuous dosing of ethylene into the syngas stream leads to its nearly complete hydrogenation to ethane without influencing the rate of methanol formation. Thus, the two reactions are catalysed by two different active sites. Obviously, unpromoted metallic surfaces like Cu0 are highly suitable for the hydrogenation of unsaturated hydrocarbons. It is known from literature that Cu0 can act as adsorption site for ethylene34, and Cu-based catalysts are also applied in other hydrogenation reactions such as the hydrogenation of esters35. Furthermore, the high hydrogen content in the syngas is sufficient to ensure that ethylene hydrogenation can proceed without disturbing the formation of methanol on the Cu–Zn interface sites. Adding 0.05, 0.1 and 0.2% of NH3 as pulses leads to the expected reversible poisoning of methanol formation, but not to a lowering of the produced amount of ethane neglecting the temporary dilution.

The same result is obtained by comparing the continuous dosing of NH3 with the continuous dosing of NO over the Cu/ZnO/Al2O3 catalyst (Fig. 2b). NO is completely hydrogenated to NH3 and H2O, and the produced amount of NH3 further reacts to methylamines (Supplementary Fig. 11). Figure 2b illustrates that a four times higher content of NO and so of the resulting NH3 after hydrogenation compared with the added amount of 0.05% NH3 leads to a degree of NH3 conversion (XNH3), which is nearly four times lower: 5.5% compared with 20%. This observation implies that NO is not hydrogenated on the same site where NH3 reacts, that is, the NO hydrogenation sites are presumably metallic Cu0 as for ethylene. Thus, the observed deactivation of methanol formation by adding NO originates from the re-adsorption of the hydrogenation products NH3 and H2O, which is favoured under the applied high-pressure conditions according to the following consecutive reaction sequence36

$${\mathrm{NO}}\mathop { \to }\limits^{ + {\mathrm{H}}_2} {\mathrm{NH}}_3\mathop { \to }\limits^{ + {\mathrm{CH}}_3{\mathrm{OH}}} {\mathrm{methyl}}\,{\mathrm{amines}}.$$

As a result, it seems that NH3 does not prefer unpromoted metallic Cu0 as adsorption site, which was also the outcome of NH3 adsorption studies on Cu0 single crystals37,38. To confirm this hypothesis, the syngas mixture was switched from CO/CO2/H2 to CO/H2 and back to the CO2-containing feed at constant reaction temperature and pressure, which is shown in Fig. 2c. The absence of CO2 in the syngas mixture results in a strongly reducing atmosphere, which induces the formation of metallic surfaces on the Cu/ZnO/Al2O3 catalyst. Increasing reaction temperatures and longer reaction times are known to result in brass formation16. Here, the lower production rates for methanol originate from a changed mechanism of methanol formation from the formate pathway to the formyl pathway, which is kinetically not preferred on Zn-promoted Cu0 surfaces17. The adsorbates of the formyl mechanism such as COads and HCOads bind through their C atoms to the catalyst surface, and no oxidising effect is induced due to the absence of CO2 and H2O in contrast to the formate pathway. Therefore, the combination of this experiment with HPPEs shows no reversible poisoning and no conversion of NH3 in the CO/H2 mixture. Thus, the composition of the syngas mixture controls the oxidation state of the catalyst surface, which can be changed reversibly under low-temperature conditions as confirmed in many studies11,16,24. In summary, all experiments shown in Fig. 2 indicate that metallic Cu0 or Cu0–Zn0 sites are not the adsorption sites for NH3, implying that the observed reversible NH3 poisoning in the presence of CO2 must selectively proceed on positively charged Cu0–Znδ+ interface sites due to the oxidising effect of the oxygen-containing adsorbates.

The role of CO2

It was already shown that adsorbates like formate or other oxygen-containing species originating from CO2 play not only a crucial role in the methylation of amines, but also in the partial oxidation of Zn species in contact with metallic Cu0 sites12,13. This type of oxidation is favoured for Zn due to its higher oxophilicity compared with Cu13,17. Providing evidence for this hypothesis requires that the corresponding investigations must be performed under high-pressure methanol synthesis conditions to generate the necessary adsorbates on the surface. For methanol synthesis over Cu/ZnO/Al2O3, the high-pressure pulse method combined with selective poisons as probe molecules enables us to analyse the oxidation effect under working conditions. For the investigation of the adsorbate-induced surface oxidation, the CO2 content in the feed gas was increased from 0 (CO hydrogenation) to 100% (CO2 hydrogenation) to generate different coverage degrees of the reaction intermediates, and for every gas mixture the normalized ΔnMeOH values (Supplementary Note 2) were determined by pulsing NH3 and TMA (Fig. 3).

Fig. 3: Influence of CO2 on the methanol productivity and on the oxidation state of the catalyst surface.

Correlation of the methanol productivity (black points and line) and of the normalized ΔnMeOH values (Supplementary Note 2) of NH3 (blue points and line) and TMA (green points and line) as a function of the CO2 content in the syngas from pure CO hydrogenation (0%) to pure CO2 hydrogenation (100%). Illustrations: Metallic Cu0 particles (orange balls), metallic Zn0 species (white balls), positively charged Zn species (blue balls) and formate as adsorbates. The error bars were determined by measuring every point five times.

Adding small amounts of CO2 in the syngas feed results in a strong increase of the methanol production rate, which further increases with rising CO2 content, because CO2 is much faster hydrogenated to methanol than CO17. In general, it is accepted that the highest production rate is achieved at low CO2 mole fractions around 2–4%4. This statement is only valid for high degrees of syngas conversion and high methanol and H2O mole fractions (Supplementary Fig. 13). In the differential kinetic regime, product inhibition effects by H2O are not significant enough to lower the rate of methanol formation strongly17,36.

In addition to the increasing production rate of methanol, Fig. 3 illustrates that the observed poisoning strengths of NH3 and TMA increase linearly as a function of the CO2 content in the syngas mixture. Therefore, higher CO2 mole fractions lead to increasing coverages of the resulting oxygen-containing adsorbates exemplary shown as formate, and these adsorbates create more Cu0–Znδ+ interface sites. In this way, the adsorption capacity of TMA is enhanced, and more NH3 molecules can be adsorbed and further converted.

On the basis of the presented results and of different literature reports, we assume that the initial reduction of the catalyst surface induces the migration of metallic Zn species onto the metallic Cu0 particles forming the Cu0–Zn0 surface alloy11. This state of the surface seems to be stable under the conditions of CO hydrogenation, but not in the presence of CO2, which leads to the oxidation of the metallic Zn species forming Znδ+ species on the Cu0 surface13. It cannot be clarified if all Zn sites in contact with Cu0 are oxidized in the CO2/H2 gas mixture, but the majority of the sites should have a positively charged nature. The models of the active site of the Cu/ZnO/Al2O3 catalyst of the Nakamura and Schlögl groups are rather similar proposing a Cu0–Zn0 surface alloy11 and Cu steps with Zn alloyed into it13, respectively. Behrens et al.13 assumed the partial oxidation of the metallic Zn species, which cannot be neglected under industrially relevant coverage degrees. In contrast, the assumptions of the Nakamura and Chorkendorff groups11,12,19 are mainly based on results obtained under atmospheric pressure or ultra-high vacuum, which result in low degrees of conversion and coverages. Thus, the fraction of oxidized Zn sites compared to the metallic ones is small, and the oxidation effect is hardly observable. For example, most characterization methods like our pulse experiments at 1 bar (Supplementary Fig. 9d) provide an averaged result over the whole Cu surface area, which is mainly metallic. However, the Cu0–Zn0 surface alloy model11 provides a highly suitable description of the catalyst surface after reduction and presumably for methanol synthesis from CO.


We analysed the rate of methanol formation reaction mainly from CO/CO2-containing syngas mixtures over an industrial Cu/ZnO/Al2O3 catalyst, which can be reversibly deactivated by NH3, which initializes the consecutive methylation reactions. The step-by-step methylation with presumably oxygen-containing intermediates like formate seems to be the major factor determining the inhibition strength of the amines, because NH3 is the strongest inhibitor. Both reactions selectively take place on the positively charged Zn species, which are formed by the diffusion of ZnOx species onto the metallic Cu0 particles creating additional interface sites. The unpromoted Cu0 sites act as hydrogenation sites for ethylene as well as NO, and sites exposed by ZnO nanoparticles are not active under the low-temperature conditions. For the hydrogenation products of NO, the re-adsorption of NH3 and H2O is favoured under the high-pressure conditions. In addition, we showed that the CO2 content in the syngas is essential to achieve the optimum oxidation state of the interface sites, which are less active and more metallic in the absence of CO2. The resulting adsorbate-induced oxidation of surface sites by formate and the importance of Lewis acids on metallic Cu0 for the formation of methanol were also observed in recent studies39,40.

Actually, the statement that CO2 is important for the oxidation state of the surface goes back to Klier et al.41, who assumed erroneously that Cu+ is the active site. Figure 4 illustrates that all newer models can be applied to describe the structural evolution of the Cu/ZnO/Al2O3 catalyst as a function of TOS.

Fig. 4: Long-term methanol synthesis over the industrial Cu/ZnO/Al2O3 catalyst at 210 °C and 60 bar.

Recorded degrees of conversion (black points) under differential controlled conditions. The dashed red curve describes the intra- and extrapolation of the experimental data, which was calculated with the MATLAB® software according to the studies of Fichtl et al.18. Illustrations from right to left: Cu0–Zn0 surface alloy according to Nakamura et al.11. Znδ+ species at the defective Cu0 surface according to Behrens et al.13, graphitic-like ZnOx layer on Cu0 according to Lunkenbein et al.14. ZnO layer on Cu0 according to Lunkenbein et al.23 as well as Fichtl et al.18 and ZnO on the top layer of Cu0 according to Kattel et al.15.

The strong loss of ~50% of the initial activity in the first weeks is inevitable for Cu-based catalysts developed for industrial reactors due to thermal sintering and restructuring4. Therefore, the Cu/ZnO/Al2O3 catalyst is a dynamic system with a continuously changing structure, so that true steady state for a couple of days cannot be reached even under industrial timescales as illustrated by the extrapolated curve. We propose the following structural changes as a function of TOS from left to right in Fig. 4: At the beginning, highly reduced ZnOx species migrate onto the metallic Cu0 nanoparticles during reduction forming a finely dispersed Cu0–Zn0 alloy according to Nakamura et al.11. The change to a CO2-containing syngas mixture initializes the formation of different oxygen-containing adsorbates as well as the oxidation of the metallic Zn species to Znδ+ species at the defective Cu0 surface according to Behrens et al.13. The migration of further Zn species results in the formation first of a graphitic-like ZnOx layer on Cu0 according to Lunkenbein et al.14 and then a more crystalline and stable thick ZnO layer or particles according to Kattel et al.15. The formation of thick ZnO layers due to segregation from the metallic Cu0 phase were observed in recent long-term studies18,23 clarifying that the SMSI process is thermodynamically preferred, but kinetically slow. Under industrially relevant conditions our results clearly confirm the presence of highly active Cu0–Znδ+ interface sites embedded in the structurally constantly changing matrix provided by the Cu/ZnO/Al2O3 catalyst Thus, by applying our developed high-pressure pulse method, we were able to identify the nature of these interface sites, which has not been possible by other characterization methods lacking the combination of surface sensitivity and industrially relevant reaction conditions.


Activation and aging of the Cu/ZnO/Al2O3 catalyst

All measurements in this work were performed with the same industrial Cu/ZnO/Al2O3 catalyst provided by Clariant Produkte (Deutschland) GmbH using a standard high-pressure flow set-up including mass flow controllers (MFC, Bronkhorst Deutschland Nord GmbH) for the adjustment of the necessary volume flows, shutdown (Swagelok Company) and multi-port (VICI Valco Instruments) valves, one tubular 1/4-inch stainless-steel reactor mounted in a 1-zone oven (HTM Reetz GmbH) and equipped with an internal thermocouple in order to achieve the desired reaction temperature in the catalyst bed, a back pressure regulator (BPR, Equilibar Precision Pressure Control) connected to a process pressure controller (PC, Bronkhorst Deutschland Nord GmbH) for the reaching of high-pressure conditions (up to 60 bar) in the reactor and a unique self-built HPPU. In addition, all stainless-steel tubes and parts, which were contaminated by the corrosive reversible poisons used in this work, were coated with SilcoNert 2000® provided by SilcoTek GmbH and heated up to 150 °C to minimize any kind of adsorption phenomena. For the quantification of the product gas streams, a combination of a FTIR spectrometer (Nicolet is50, Thermo Fisher Scientific) and a Micro GC device (Micro GC 490, Agilent) was used. The spectrometer contains a transmission gas cell in the sample holder with ZnSe windows, a pathlength of 150 mm and a cell volume of 7.5 ml. In addition, the spectrometer offers two different types of detectors for recording IR spectra: The thermal DTGS (deuterated triglycine sulfate) and the liquid nitrogen cooled MCT (mercury cadmium telluride) detectors. In the case of the Micro GC device, a pump, a micro-machined injector with an injection volume of 5 µl, a Molsieve 5A column and a micro-machined thermal conductivity detector were used for recording the chromatograms. The calibrations of both analytics were validated and the carbon balance (C-balance) of every kinetic experiment performed in this work was in the acceptable range of 100% ± 1%.

$${\mathrm{C}} - {\mathrm{balance}} = \frac{{y_{C,\mathrm{out}}}}{{y_{C,\mathrm{in}}}} = \frac{{y_{\mathrm{CO},\mathrm{out}} + y_{\mathrm{CO2},\mathrm{out}} + y_{\mathrm{MeOH},\mathrm{out}}}}{{y_{\mathrm{CO},\mathrm{in}} + y_{\mathrm{CO2},\mathrm{in}}}}.$$

Here, the ratio between the mole fraction of all carbon-containing compounds (CO, CO2, CH3OH) in the product gas stream yc,out and the mole fraction of all carbon-containing compounds (CO, CO2) in the feed yc,in yields the C-balance.

For the reduction of the catalyst precursor, the temperature was increased to 175 °C with a heating rate of 1 °C min−1 using a gas flow rate of 500 Nml min−1 gcat−1 diluted H2 (2% H2 (99.999%) in N2 (99.999%)) for 15 h. In a second step, the temperature was increased to 240 °C with 1 °C min−1 and held for 30 min. After the second increase of the temperature, the reduced catalyst was ready for methanol synthesis.

To reach steady-state conditions in a relatively short period of time, the catalyst was aged before performing the kinetic experiments. The reaction temperature was increased to 250 °C at 60 bar to establish equilibrium-controlled conditions ensuring a reproducible deactivation by exposing the whole catalyst bed to the same gas composition at high degrees of conversion according to the study by Fichtl et al.18. As standard syngas mixture, the following composition was used: 13.5% CO (99.997%), 3.5% CO2 (99.998%), 73.5% H2 (99.999%) and 9.5% N2 (99.999%). All measurements in this study were performed in the differential regime with the necessary syngas flow rate.

High-pressure pulse experiment (HPPE)

For the HPPE, a self-built HPPU was developed to inject probe molecules as pulses under high-pressure conditions, which is schematically shown in Fig. 5.

Fig. 5: Scheme of the high-pressure pulse unit integrated in the flow set-up.

PI is defined as pressure sensor in the corresponding line. The area in blue describes the flow direction of the syngas mixture, the red area of the injected impurities and the orange area of the reference gas (Ar) for pressure regulation.

The HPPU consists of one 6 port, 2 position valve equipped with a 1 ml sample loop and two identical back pressure regulators (BPR1 and BPR2) coupled with one process PC. BPR2 is integrated in the reactor line between the reactor outlet and the analytics and BPR1 in the pulse line between the sample loop and the exhaust. The method for the injection of a pulse over the catalyst bed in the reactor under high-pressure conditions is as follows: The BPRs consist of two parts, which are separated from each other by a Kapton® membrane. The upper parts are connected with PC and the other parts with the incoming gas flow from the reactor or the sample loop on the inlet sites and on the outlet sites with the analytics or exhaust. The task of the PC is to reach the same pressure level in both back pressure regulators. It consists of two valves and a pressure sensor PI. For the setting of pressure values up to 60 bar, 65 bar of Ar (99.999%) must be connected on the inlet valve. When a pressure value is set in the program of the PC, the inlet as well as outlet valve is opened and closed until the pressure sensor measures the given value. Consequently, the pressure in both upper parts of BPR1 and BPR2 increases and so the membranes are pressed down. At this moment, the gas flows are stopped and the pressure in the reactor line and pulse line builds up until the same pressure level is reached like in the upper parts. Then, the membranes are lifted up to the starting positions and the gas mixtures can flow again. If both pressure sensors PI in the reactor and pulse line show the same pressure value, then the valve can be switched to inject the first pulse into the syngas stream.

The results of the validation are shown in Fig. 6. Here, 200 mg of α-Al2O3 (sieve fraction: 250–355 µm, Südchemie GmbH) were placed in the isothermal zone of the reactor and fixed between two plugs of quartz wool to simulate an inert catalyst bed. One glass rod was placed after the bed to lower the dead volume. Then, 0.3% CH4 (99.995%) in N2 (99.999%) as IR-active, but inert gas was injected as pulses into a 50 Nml min−1 N2 (99.999%) flow passing through the α-Al2O3 bed at 5, 10, 20, 30, 40, 50 and 60 bar. The retention time τ and the pulse area Apulse of the recorded pulses (Fig. 6a) were determined and correlated with the set pressures (Fig. 6b).

Fig. 6: Validation of the self-built high-pressure pulse unit with inert CH4 pulses over α-Al2O3.

a Recorded methane pulses (green curves) injected over α-Al2O3 as inert bed at different pressures from 5 to 60 bar. τ is defined as the retention time of the CH4 pulses. b Correlation of the determined retention times τ (red points and line) and pulse areas Apulse (blue points and line) against the set pressure levels. The error bars were determined by measuring every point 5 times.

The dashed red line in Fig. 6a represents the injection point of the pulses at time 0. Increasing the pressure leads to longer τ and increasing Apulse. In this case, only the blue curve (Apulse) in Fig. 6b goes through the origin and not the red curve (τ). The reason for this is the constant operation of the analytics under atmospheric pressure and so the expansion of the pulses after the BPR2 (Fig. 5). In general, the volume flow \(\dot V\) of gaseous compounds is reduced by increasing the pressure level p according to the ideal gas law (Eq. (4)), since the molar flow \(\dot n\) (due to a constant mass flow provided by the used MFC at every pressure level), the gas constant R and the temperature T (due to small changes in the pressure level) can be seen as constant:

$$p = \frac{{\dot n \cdot R \cdot T}}{{\dot V}} = {\mathrm{const}}. \cdot \frac{1}{{\dot V}}$$
$$\tau = \frac{V}{{\dot V}} = {\mathrm{const}}. \cdot p$$

In contrast, the resulting retention time or residence time τ, which is defined as reactor volume V divided by the volume flow \(\dot V\) of the pulses is proportional to the applied pressure. The corresponding value for the constant in Eq. (5) is equal to the slope m of the lines in Fig. 6b.

The linear behaviour of both functions (Fig. 6b), the absence of steps in the recorded pulses and the acceptable tailing at higher pressures (Fig. 6a) demonstrate a successful validation of the HPPU. Consequently, significant pressure drops and backmixing of the probe molecules can be excluded. In addition, the small error bars (every measurement was repeated five times) in Fig. 6b underline the reproducibility of the pulse method.

For a typical HPPE, 100 mg of the industrial Cu/ZnO/Al2O3 catalyst (sieve fraction 250–355 µm) were placed in the tubular reactor. In the first step, the initial methanol mole fraction in the standard syngas mixture at 210 °C and 60 bar was recorded under differential controlled conditions. Then, the different N compounds were injected as pulses from the corresponding gas cylinder: 0.5% NH3 (99.999%) in N2 (99.999%), 0.2% NO (99.5%) in N2 (99.999%), 0.2% monomethylamine (MMA, 99.5%) in N2 (99.999%), 0.2% dimethylamine (DMA, 99.5%) in N2 (99.999%), 0.2% trimethylamine (TMA, 99.5%) in N2 (99.999%). The mole fraction in the sample loop was set at 0, 0.01, 0.025, 0.05, 0.075, 0.1 and 0.2%. The measurement with 0% corresponds to a pulse with pure inert gas N2 (99.999%). In the case of NH3, additional HPPEs were performed with 0.4 and 0.5%. In addition, 0.05, 0.1 and 0.2% NH3 were injected at 230 and 250 °C at constant 60 bar as well as at 1, 10, 30 and 60 bar at constant 210 °C.

Co-feeding of NH3, NO, MMA, DMA and TMA

The continuous dosing experiments with various N compounds were performed over 200 mg (sieve fraction 250–355 µm) of the industrial methanol catalyst. For the dosing of 0.05% NH3 (from 0.5% NH3 (99.999%) in N2 (99.999%)) and 0.2% NO (from 2% NO (99.5%) in N2 (99.999%)), the reaction temperature and pressure were set at 210 °C and 60 bar. In the case of dosing of 0.051% NH3, 0.0153% MMA (from 0.2% MMA (99.5%) in N2 (99.999%)), 0.0170% DMA (from 0.2% DMA (99.5%) in N2 (99.999%)) and 0.0157% TMA (from 0.2% TMA (99.5%) in N2 (99.999%)), the reaction temperature was increased to 250 °C. After achieving a constant initial methanol mole fraction applying the standard syngas mixture, the corresponding N compound was continuous dosed over the catalyst bed for a defined period of time by replacing the internal standard N2 in the standard syngas mixture. At the end, the gas stream of the N compounds was switched off to measure the methanol activity in pure syngas.

Co-feeding of ethylene coupled with HPPE with NH3/TMA

The combination of methanol synthesis in the presence of ethylene coupled with HPPEs with NH3 and TMA were performed with 100 mg of the industrial Cu/ZnO/Al2O3 catalyst (sieve fraction 250–355 µm) mounted in the tubular reactor. In the first step, the initial methanol mole fraction was determined with the standard syngas mixture at 210 °C and 60 bar. Then, 1% of the internal standard N2 was replaced by ethylene (from 20% ethylene (99.995%) in N2 (99.999%)) and after a defined period of time, the feed was switched back to the standard syngas mixture. During the adding of ethylene, 0.05%, 0.1% and 0.2% of NH3 (from 0.5% NH3 (99.999%) in N2 (99.999%)) and TMA (from 0.2% TMA (99.5%) in N2 (99.999%)) were injected as pulses.

Syngas switching experiments coupled with HPPE with NH3/TMA

The combination of syngas switching experiments under methanol synthesis conditions with HPPEs with NH3 and TMA were carried out over 100 mg of the industrial Cu/ZnO/Al2O3 catalyst (sieve fraction 250–355 µm). Here, the syngas feed was changed from the standard mixture containing CO/CO2 to 17% CO (99.997%), 73.5% H2 (99.999%), 9.5% N2 (99.999%) and back to the standard mixture. At each instant, methanol was produced at 210 °C and 60 bar. In addition, pulses containing 0.2% of NH3 (from 0.5% NH3 (99.999%) in N2 (99.999%)) and TMA (from 0.2% TMA (99.5%) in N2 (99.999%)) were injected into the different feed gas compositions.

CO/CO2 variation experiment coupled with HPPE with NH3/TMA

The combination of CO/CO2 variation experiments under methanol synthesis conditions with HPPEs with NH3 and TMA were performed with 100 mg of the Cu/ZnO/Al2O3 catalyst (sieve fraction 250–355 µm) in the tubular reactor. The reaction temperature and pressure were constant at 210 °C and 60 bar and the CO2 content in the syngas feed was changed from 0 to 17% (0, 0.5, 3.5, 5, 10, 17%) by substituting or adding CO to maintain the carbon mole fraction at constant 17% (CO + CO2). For every new syngas mixture, the methanol productivity was recorded and 0.2% NH3 (from 0.5% NH3 (99.999%) in N2 (99.999%)) as well as TMA (from 0.2% TMA (99.5%) in N2 (99.999%)) were injected as pulses. Every measurement was repeated five times to determine the corresponding error bars.

Long-term measurement

The procedure of the long-term measurement was adapted from Fichtl et al.18. and is shown in Fig. 7.

Fig. 7: Experimental protocol of the long-term measurement adapted from the studies by Fichtl et al.18.

The violet arrow describes the period of time to record the kinetic data point, the red arrow describes the heating rate, the black arrow describes the aging of the catalyst bed under equilibrium conditions and the blue arrow describes the cooling rate.

Three hundred milligrams of the industrial methanol synthesis catalyst (sieve fraction 250–355 µm) were mixed with 1800 mg purified α-Al2O3 (sieve fraction 510–750 µm) and placed in the tubular reactor. The high dilution should prevent the formation of hot spots, so that a homogeneous temperature profile over the entire catalyst bed was obtained. After the standard activation procedure, the gas stream was changed to the standard syngas mixture and the reaction pressure was increased up to 60 bar. The initial activity test was performed at 210 °C for 60 min under kinetically controlled conditions. Then, the catalyst was heated to the aging temperature of 250 °C and the volume flow was reduced to reach the equilibrium conversion. The equilibrium condition was held for 90% of a day. The decrease of the reaction temperature to 210 °C and the increase of the flow rate allowed to measure the next kinetically controlled rate of methanol formation. The continuous change between the two conditions was carried out until a total TOS of 6 weeks was reached. Besides, the recorded experimental curve was interpolated by using the following empirical power-law model (PLM):

$$\frac{{\mathrm{d}a_{\mathrm{rel}}}}{{\mathrm{d}t}} = - k_d \cdot a_{\mathrm{rel}}\left( t \right)^m,$$
$$a_{\mathrm{rel}} = \frac{{X_{\mathrm{CO}x}(\mathrm{TOS})}}{{X_{\mathrm{CO}x}(\mathrm{TOS} = 0)}},$$

arel is defined as the relative activity, the ratio between the time-dependent COx (CO + CO2) conversion (XCOx(TOS)) and the COx conversion of the initial activity (XCOx(TOS = 0)). kd is the deactivation rate constant and m is an empirical factor or the reaction order. For the calculation of the theoretical curve, the MATLAB® software was used and the procedure was adapted from the work of Fichtl et al.18.

Data availability

The data sets generated during and/or analysed during the current study are available from the corresponding author on reasonable request.


  1. 1.

    Sehested, J. Industrial and scientific directions of methanol catalyst development. J. Catal. 371, 368–375 (2019).

    CAS  Article  Google Scholar 

  2. 2.

    Alvarado, M. 4th IMPCA Mississippi Conf. America (New Orleans, 2016).

  3. 3.

    Olah, G. A. et al. Beyond oil and gas. The methanol economy. Angew. Chem. Int. Ed. 45, 5045–5047 (2006).

    Article  Google Scholar 

  4. 4.

    Hansen, J. B. et al. Handbook of Heterogenous Catalysis: Methanol Synthesis Ch. 13.13 (Wiley-VCH, Weinheim, 2008).

  5. 5.

    Schittkowski, J. et al. Methanol synthesis from steel mill exhaust gases. Challenges for the industrial Cu/ZnO/Al2O3 catalyst. Chem. Ing. Tech. 90, 1419–1429 (2018).

    CAS  Article  Google Scholar 

  6. 6.

    Spencer, M. S. et al. Metal catalyst design and preparation in control of deactivation. Annu. Rev. Mater. Res. 35, 427–464 (2005).

    ADS  CAS  Article  Google Scholar 

  7. 7.

    Remus, R. et al. Best Available Techniques (BAT). Reference Document for Iron and Steel Production: Industrial Emissions Directive 2010/75/ EU (Integrated Pollution Prevention and Control). JRC Reference Report, European Commission, Joint Research Centre, Institute for Prospective Technological Studies (Seville, 2013).

  8. 8.

    Bartholomew, C. H. Mechanisms of catalyst deactivation. Appl. Catal. A: Gen. 212, 17–60 (2001).

    CAS  Article  Google Scholar 

  9. 9.

    Moulijn, J. A. et al. Handbook of Heterogenous Catalysis: Deactivation and Regeneration Ch. 7.1 (Wiley-VCH, Weinheim, 2008).

  10. 10.

    Dahl, S. et al. Role of steps in N2 activation on Ru(0001). Phy. Rev. Lett. 83, 1814–1817 (1999).

    ADS  Article  Google Scholar 

  11. 11.

    Nakamura, J. et al. On the issue of the active site and the role of ZnO in Cu/ZnO methanol synthesis catalysts. Top. Catal. 22, 277–285 (2003).

    CAS  Article  Google Scholar 

  12. 12.

    Kuld, S. et al. Quantifying the promotion of Cu catalysts by ZnO for methanol synthesis. Science 352, 969–974 (2016).

    ADS  CAS  Article  Google Scholar 

  13. 13.

    Behrens, M. et al. The active site of methanol synthesis over Cu/ZnO/Al2O3 industrial catalysts. Science 336, 893–897 (2012).

    ADS  CAS  Article  Google Scholar 

  14. 14.

    Lunkenbein, T. et al. Formation of a ZnO overlayer in industrial Cu/ZnO/Al2O3 catalysts induced by strong metal-support interactions. Angew. Chem. 127, 4627–4631 (2015).

    Article  Google Scholar 

  15. 15.

    Kattel, S. et al. Active sites for CO2 hydrogenation to methanol on Cu/ZnO catalysts. Science 355, 1296–1299 (2017).

    ADS  CAS  Article  Google Scholar 

  16. 16.

    Grunwaldt, J.-D. et al. In situ investigations of structural changes in Cu/ZnO catalysts. J. Catal. 194, 452–460 (2000).

    CAS  Article  Google Scholar 

  17. 17.

    Studt, F. et al. The mechanism of CO and CO2 hydrogenation to methanol over Cu-based catalysts. ChemCatChem 7, 1105–1111 (2015).

    ADS  CAS  Article  Google Scholar 

  18. 18.

    Fichtl, M. B. et al. Kinetics of deactivation on Cu/ZnO/Al2O3 methanol synthesis catalysts. Appl. Catal. A: Gen. 502, 262–270 (2015).

    CAS  Article  Google Scholar 

  19. 19.

    Kuld, S. et al. Quantification of zinc atoms in a surface alloy on copper in an industrial-type methanol synthesis catalyst. Angew. Chem. 126, 6051–6055 (2014).

    Article  Google Scholar 

  20. 20.

    Askgaard, T. S. et al. A kinetic model of methanol synthesis. J. Catal. 156, 229–242 (1995).

    CAS  Article  Google Scholar 

  21. 21.

    Naumann d’Alnoncourt, R. et al. The influence of ZnO on the differential heat of adsorption of CO on Cu catalysts: a microcalorimetric study. J. Catal. 220, 249–253 (2003).

    Article  Google Scholar 

  22. 22.

    Naumann d’Alnoncourt, R. et al. The influence of strongly reducing conditions on strong metal–support interactions in Cu/ZnO catalysts used for methanol synthesis. Phys. Chem. Chem. Phys. 8, 1525–1538 (2006).

    Article  Google Scholar 

  23. 23.

    Lunkenbein, T. et al. Bridging the time gap. A copper/zinc oxide/aluminum oxide catalyst for methanol synthesis studied under industrially relevant conditions and time scales. Angew. Chem. Int. Ed. 55, 12708–12712 (2016).

    CAS  Article  Google Scholar 

  24. 24.

    Hansen, P. L. et al. Atom-resolved imaging of dynamic shape changes in supported copper nanocrystals. Science 295, 2053–2055 (2002).

    ADS  CAS  Article  Google Scholar 

  25. 25.

    Martin, O. et al. Operando synchrotron X-ray powder diffraction and modulated-excitation infrared spectroscopy elucidate the CO2 promotion on a commercial methanol synthesis catalyst. Angew. Chem. 128, 11197–11202 (2016).

    Article  Google Scholar 

  26. 26.

    Vedage, G. A. et al. Chemical trapping of surface intermediates in methanol synthesis by amines. J. Catal. 95, 423–434 (1985).

    CAS  Article  Google Scholar 

  27. 27.

    Gredig, S. V. et al. Synthesis of methylamines from carbon dioxide and ammonia. J. Chem. Soc., Chem. Commun. 1, 73–74 (1995).

    Article  Google Scholar 

  28. 28.

    Twigg, M. V. et al. Deactivation of copper metal catalysts for methanol decomposition, methanol steam reforming and methanol. Synth. Top. Catal. 22, 191–203 (2003).

    CAS  Article  Google Scholar 

  29. 29.

    Zander, S. et al. The role of the oxide component in the development of copper composite catalysts for methanol synthesis. Angew. Chem. Int. Ed. 52, 6536–6540 (2013).

    CAS  Article  Google Scholar 

  30. 30.

    Kunkes, E. L. et al. Hydrogenation of CO2 to methanol and CO on Cu/ZnO/Al2O3. Is there a common intermediate or not? J. Catal. 328, 43–48 (2015).

    CAS  Article  Google Scholar 

  31. 31.

    Song, H. et al. Spinel-structured ZnCr2O4 with excess Zn is the active ZnO/Cr2O3 catalyst for high-temperature methanol synthesis. ACS Catal. 7, 7610–7622 (2017).

    CAS  Article  Google Scholar 

  32. 32.

    Saito, M. et al. Development of copper/zinc oxide-based multicomponent catalysts for methanol synthesis from carbon dioxide and hydrogen. Appl. Catal. A: Gen. 138, 311–318 (1996).

    CAS  Article  Google Scholar 

  33. 33.

    Kurtz, M. et al. Deactivation of supported copper catalysts for methanol synthesis. Catal. Lett. 86, 77–80 (2003).

    CAS  Article  Google Scholar 

  34. 34.

    Franken, P. E. et al. Ethylene adsorption on thin films of Ni, Pd, Pt, Cu, Au and Al; work function measurements. Surf. Sci. 53, 341–350 (1975).

    ADS  CAS  Article  Google Scholar 

  35. 35.

    Li, F. et al. Selective hydrogenation of ethylene carbonate to methanol and ethylene glycol over Cu/SiO2 catalysts prepared by ammonia evaporation method. Int. J. Hydrog. Energy 42, 2144–2156 (2017).

    CAS  Article  Google Scholar 

  36. 36.

    Sahibzada, M. et al. Methanol synthesis from CO/CO2/H2 over Cu/ZnO/Al2O3 at differential and finite conversions. J. Catal. 174, 111–118 (1998).

    CAS  Article  Google Scholar 

  37. 37.

    Biemolt, W. et al. The adsorption site of ammonia at copper surfaces. Catal. Today 12, 427–432 (1992).

    CAS  Article  Google Scholar 

  38. 38.

    van de Kerkhof, G. J. et al. Dissociation of ammonia on a copper surface and the effect of oxygen coadsorption: a quantum-chemical study. Surf. Sci. 284, 361–371 (1993).

    ADS  Article  Google Scholar 

  39. 39.

    Matsubu, J. C. et al. Adsorbate-mediated strong metal-support interactions in oxide-supported Rh catalysts. Nat. Chem. 9, 120–127 (2017).

    CAS  Article  Google Scholar 

  40. 40.

    Kim, J. et al. Surface Lewis acidity of periphery oxide species as a general kinetic descriptor for CO2 hydrogenation to methanol on supported copper nanoparticles. ACS Catal. 9, 10409–10417 (2019).

    CAS  Article  Google Scholar 

  41. 41.

    Klier, K. et al. Catalytic synthesis of methanol from COH2: IV. The effects of carbon dioxide. J. Catal. 74, 343–360 (1982).

    CAS  Article  Google Scholar 

Download references


We gratefully appreciate the financial support received from the German Federal Ministry of Education and Research (Bundesministerium für Bildung und Forschung, BMBF, Verbundvorhaben Carbon2Chem®, L2 ProMeOH, FKZ 03EK3039E). The catalyst used in this study was gratefully provided by project partner Clariant Produkte (Deutschland) GmbH.

Author information




M.M. and H.R. conceived the idea. D.L. designed and built the flow set-up with the unique HPPU under the guidance of M.M and H.R., carried out all catalytic tests and pulse experiments, and performed the data analysis. All authors discussed the results and contributed to the manuscript.

Corresponding author

Correspondence to Martin Muhler.

Ethics declarations

Competing interests

The authors declare no competing interests.

Additional information

Peer review information Nature Communications thanks the anonymous reviewer(s) for their contribution to the peer review of this work.

Publisher’s note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Supplementary information

Rights and permissions

Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in a credit line to the material. If material is not included in the article’s Creative Commons license and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this license, visit

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Laudenschleger, D., Ruland, H. & Muhler, M. Identifying the nature of the active sites in methanol synthesis over Cu/ZnO/Al2O3 catalysts. Nat Commun 11, 3898 (2020).

Download citation


By submitting a comment you agree to abide by our Terms and Community Guidelines. If you find something abusive or that does not comply with our terms or guidelines please flag it as inappropriate.


Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing