Catalytic conversion of carbon dioxide into dimethyl carbonate using reduced copper-cerium oxide catalysts as low as 353 K and 1.3 MPa and the reaction mechanism

Introduction

Carbon dioxide is one of major green house gases. The conversion of CO₂ has been widely investigated to reduce the atmospheric concentration of CO₂ (Izumi, 2013). In the viewpoint of global warming, fixation methods of CO₂ and/or converted compounds from CO₂ are also critical. Transferring captured CO₂ to the bottom of the sea in a supercritical state is partially in practical use, but it incurs huge investment costs. The conversion of CO₂ to dimethyl carbonate (DMC) is attractive because DMC can be used as an electrolytic solution of lithium ion battery, methylating reagent, and feedstock for engineering plastics (Ono, 1997).

DMC has been conventionally synthesized starting from phosgene, carbon monoxide, or oxirane, but these materials are toxic and/or explosive. From CO₂ and methanol/acetals, DMC was synthesized using homogeneous Sn catalysts at 10–30 MPa and 353–453 K (Sakakura et al., 1998, 1999, 2000; Kalhor et al., 2011) and using homogeneous Ni catalysts at 353 K and 1.0 MPa (Shi et al., 2013). Catalyst separation was improved for DMC synthesis using heterogeneous CeO₂ (Yoshida et al., 2006), ZrO₂ (Tomishige et al., 1999), solid solution of ZrO₂ and CeO₂ (Tomishige et al., 2001; Zhang et al., 2011b), Ga₂O₃/Ce_0.6Zr_0.4O₂ (Lee et al., 2011), Ce_xZr_0.9–xY_0.1O₂ (Zhang et al., 2011a), SnO₂–ZrO₂/SiO₂ (Ballivet-Tkatchenko et al., 2011), Co_1.5PW₁₂O₄₀ (Aouissi et al., 2010), H₃PW₁₂O₄₀/Ce_xTi_1–xO₂ (La et al., 2007), Cu–KF/MgSiO (Li and Zhong, 2003), Cu–Ni–diatomite (Chen et al., 2012), Cu–Ni–graphite (Bian et al., 2009a), Cu–Ni–V₂O₅–active carbon (Bian et al., 2009b), and Cu–Ni–V₂O₅–SiO₂ (Wu et al., 2006; Wang et al., 2007) at 353–453 K and 0.1–60 MPa. The conversion of methanol to DMC was as much as 7.9% for 24 h (Zhang et al., 2011b). In the viewpoint of global environment and the reduction of CO₂, it is desirable to synthesize DMC from CO₂ under mild reaction conditions.

In this context, the conversion of CO₂ and methanol to DMC under milder conditions was studied and the mechanism was investigated by X-ray absorption near-edge structure (XANES). Methanol could be synthesized photocatalytically from CO₂ ((Ahmed et al., 2011, 2012); Morikawa et al. under review). In future, the DMC synthesis reported in this work could be combined with photocatalysis to synthesize DMC from CO₂ as a single starting material.

Materials and Methods

Preparation of CeO₂

Cerium oxide samples were prepared from cerium nitrate hexahydrate (Wako Pure Chemical, >98.0%). It was dissolved in deionized water (<0.06 μS cm⁻¹) to make the concentration to 0.2 mol L⁻¹. A 5% ammonia aqueous solution (Wako Pure Chemical) was added to the solution to reach the pH 10. Obtained yellow precipitate was filtered using a polytetrafluoroethene-based membrane filter (Omnipore JGWP04700, Millipore) with a pore size of 0.2 μm and washed several times with deionized water. The obtained powder was calcined in air at 673 K for 4 h. Then, the powder was connected to a vacuum system using rotary and diffusion pumps (10⁻⁶ Pa) and the temperature was elevated at a ramping rate of 5 K min⁻¹ from 290 to 673 K and kept at 673 K for 1 h.

A part of freshly-prepared CeO₂ above was reduced under 25 kPa of hydrogen. The temperature was elevated from 290 to 673 K with the ramping rate of 10 K min⁻¹ and maintained at 673 K for 1 h.

Preparation of Cu–−CeO₂

3.8–950 mg of copper nitrate trihydrate (Wako Pure Chemical, >99.9%) was dissolved in 10 mL of deionized water. The Cu²⁺ solution was added to 1.0 g of CeO₂ powder prepared in section Preparation of CeO₂. Then, 25% of ammonia aqueous solution was added to the suspension until the pH reached 9.5. The mixture was reacted at 290 K for 1 h with magnetically stirred at a rate of 300 rpm. The color of precipitate was yellow, yellow green, and dark brown when the Cu content was 0.1, 1, and 20 wt%, respectively. The precipitate was filtered using JGWP04700 membrane and washed by several times with deionized water. The obtained powder was dried at 353 K for 12 h and denoted Cu–CeO₂. The Cu–CeO₂ samples were treated under H₂ (25 kPa). The temperature was elevated from 290 to 673 K with the ramping rate of 10 K min⁻¹, maintained at 673 K for 1 h, and evacuated (10⁻⁶ Pa) at 673 K for 30 min.

Characterization

Nitrogen adsorption isotherm measurements were performed at 77 K within the pressure range 1.0–90 kPa in a vacuum system connected to diffusion and rotary pumps (10⁻⁶ Pa) and equipped with a capacitance manometer (Models CCMT-1000A and GM-2001, ULVAC). The Brunauer-Emmett-Teller (BET) surface area (S_BET) was calculated on the basis of eight-point measurements between 10 and 46 kPa (P/P₀ = 0.10–0.45) on the adsorption isotherm. The sample was evacuated at 423 K for 90 min before the measurements.

The electronic state of cerium in catalysts was investigated by the synchrotron X-ray measurements. The catalyst powder samples were prepared in vacuum (10⁻⁶ Pa) and transferred directly to a Pyrex glass cell equipped with 50 μm-thick Kapton (Dupont) windows on both sides. The samples in N₂ (60 kPa) or CO₂ gas (60 kPa) were sealed with fire and transported to beamline.

Ce L₃-edge X-ray absorption fine structure (XAFS) spectra were measured at 290 K in a transmission mode in the Photon Factory at the High-Energy Accelerator Research Organization (Tsukuba, Japan) on beamline 9C and also in SPring-8 (Sayo, Japan) on beamline 01B1. The X-ray energy was calibrated at the first intense peak top energy (5731.1 eV) for the Ce L₃-edge spectrum of CeO₂. The XAFS data were analyzed with a software package XDAP version 2.2.7 (Vaarkamp et al., 2006).

DMC Synthesis Tests

An autoclave (Taiatsu Glass Kogyo, inner volume 120 mL; Model TVS–N2–120) was used for the DMC synthesis tests using CeO₂ and Cu–CeO₂ catalysts. The inner space of autoclave was purged with argon gas (>99.998%) at a rate of 300 mL min⁻¹. 10 mL of dehydrated methanol (Kanto Chemical, 99.8%) and 100 mg of catalyst were introduced in the autoclave with the flow of Ar, not in contact with air. Next, CO₂ was flowed at a rate of 300 mL min⁻¹ for 15 min. The outlet valve of reactor was closed and the interior pressure was increased to 2.0, 1.0, 0.50, 0.10 MPa at 290 K. Then, the temperature of the reactor was elevated from 290 to 393, 373, or 353 K with the ramping rate of 4 K min⁻¹, and maintained at the destination temperature for 2–6 h. As a comparison, 10 mL of dehydrated methanol, 50 mg of catalyst, and 3.6 MPa of CO₂ were introduced in the autoclave in similar way at 290 K. Then, the temperature of reactor was elevated from 290 to 403 K with the ramping rate of 4 K min⁻¹, and maintained at 403 K for 2 h. The reaction suspension was filtered using a JGWP04700 membrane. The filtrate was analyzed by gas chromatograph equipped with frame ionization detector (Model GC-18A, Shimadzu) equipped with a capillary column Ultra ALLOY-5 (Frontier Laboratories; inner diameter 250 μm, length 30 m). The conversion (%) of methanol to DMC was defined as

$\text{Conversion}(\%)\text{}=\text{}\frac{2\times \text{molar}\text{amount}\text{of}\text{DMC}\text{formed}}{\text{molar}\text{amount}\text{of}\text{methanol}\text{introduced}}\times 100.$

Results

DMC Synthesis from CO₂ and Methanol

Pretreatment effects in H₂

In the test under the 2.8 MPa CO₂ (initial pressure) at 393 K for 6 h, DMC formation rate using incipient CeO₂ catalyst was 0.44 mmol h⁻¹ g⁻¹_cat and that for reduced CeO₂ was 0.70 mmol h⁻¹ g⁻¹_cat (Table 1A). Total initial pressure of CO₂ and methanol was 3.5 MPa at 393 K. By the pretreatment effect in H₂ at 673 K, the synthesis rate increased by a factor of 1.6 times. The conversion (%) of methanol to DMC was improved to 0.33% (Table 1A).

TABLE 1

Table 1. Conditions and results of DMC synthesis from methanol and CO₂ over Ce oxide and Cu–promoted Ce oxide catalysts¹.

Effects of the Cu addition

The DMC synthesis rate using reduced Cu–CeO₂ (0.5 wt% Cu) was compared to that using reduced CeO₂ at 393 K for 2 h. The rates were 1.8 and 1.5 mmol h⁻¹ g⁻¹_cat, respectively (Table 1B). By the inclusion of 0.5 wt% of Cu in the catalyst, the rate increased by a factor of 1.2 times. The conversion of methanol to DMC was improved to 0.32% (Table 1B).

Next, the effects of Cu addition were investigated by progressively changing the Cu content between 0 and 20 wt% under lower initial pressure (0.67 MPa) of CO₂ at 393 K. By the inclusion of 0.1 wt% of Cu in Cu–CeO₂ catalyst, the DMC synthesis rate increased 2.3-fold higher: from 0.41 mmol h⁻¹ g⁻¹_cat (reduced CeO₂) to 0.95 mmol h⁻¹ g⁻¹_cat (Table 1C; Figure 1). However, further increase of Cu content between 0.3 and 1 wt% in Cu–CeO₂ catalysts was not effective compared to the test results for the Cu–CeO₂ catalyst, 0.1 wt% of Cu (Table 1C). When the Cu content was between 1 and 20 wt%, the synthesis rates gradually approached to constant, similar to the one for undoped CeO₂ (0.41 mmol h⁻¹ g⁻¹_cat) (Table 1C; Figure 1).

FIGURE 1

Figure 1. The dependence of DMC synthesis rates on the copper content in reduced Cu–CeO₂ catalysts under total initial pressure of 1.3 MPa at 393 K.

Reaction pressure effects

In the reaction tests at 393 K using reduced Cu–CeO₂ catalyst (0.5 wt% Cu), partial pressure of CO₂ introduced at 290 K was varied between 2.0 and 0.10 MPa. The partial (initial) pressure of CO₂ increased to between 2.8 and 0.13 MPa at reaction temperature of 393 K (Table 1D). The DMC synthesis rates were plotted as a function of initial pressure of CO₂ and initial total pressure of CO₂+ methanol at 393 K (Figure 2). The DMC synthesis was possible under the total pressure of 1.3 MPa, but the amount of produced DMC was below detection limit (3 μmol) under the total pressure of 0.77 MPa at 393 K (Table 1D). The DMC synthesis rates were proportional to partial pressure of CO₂ (Figure 2).

FIGURE 2

Figure 2. The dependence of DMC synthesis rates on the partial pressure of CO₂ and total pressure using Cu–CeO₂ catalyst (0.5 wt% of Cu) at 393 K.

The reaction pressure effects were also tested under severer reaction conditions: at 403 K and 6.6 MPa using Cu–CeO₂ catalysts (0.1 and 0.5 wt% Cu) (Table 1o,p). The synthesis rates (3.1–1.9 mmol h⁻¹ g⁻¹_cat) were higher by a factor of 3.3–3.2 times compared to corresponding test results at 393 K and 1.3 MPa (Table 1C,D). Thus, major reason of relatively low DMC synthesis rates in this paper was mild reaction conditions at 393–353 K and 3.5–1.3 MPa.

Reaction temperature effects

Further, the reaction temperature was varied between 393 and 353 K using reduced Cu–CeO₂ catalyst (0.5 wt% Cu) under the CO₂ partial pressure of 2.0 MPa introduced at 290 K. The CO₂ pressure increased to between 2.8 and 2.5 MPa at reaction temperatures of 393–353 K (Table 1E). Under the total pressure of 2.7 MPa, DMC synthesis was possible as low as 353 K: 0.031 mmol h⁻¹ g⁻¹_cat (Table 1E; Figure 3). The apparent activation energy was estimated to 120 kJ mol⁻¹ based on the Arrhenius plot (Figure 3, inset).

FIGURE 3

Figure 3. DMC synthesis rates over Cu–CeO₂ catalyst (0.5 wt% of Cu) at 393–353 K. Initial partial pressure of CO₂ was 2.0 MPa at 290 K. (Inset) The associated Arrhenius plot and the fit to the equation.

Bet Surface Area and Ce L₃-Edge Xanes

The BET surface area was 78 and 94 m² g⁻¹_cat for Cu–CeO₂ samples consisting of 0.1 and 0.5 wt% Cu, respectively (Table 2).

TABLE 2

Table 2. BET surface area of Cu–promoted Ce oxide catalysts.

Ce L₃-edge XANES spectra taken for Ce–based catalysts and also standard Ce compounds were depicted in Figure 4. Twin peaks appeared at 5731 and 5738 eV in the XANES spectrum for as-synthesized CeO₂ (spectrum a), indicating that valence state of Ce⁴⁺ was predominant (Zhang et al., 2004).

FIGURE 4

Figure 4. (A) Ce L₃-edge XANES for as-synthesized CeO₂ (a), CeO₂ reduced at 673 K (b), Cu–CeO₂ (0.5 wt% Cu) reduced at 673 K (c), Cu–CeO₂ (0.1 wt% Cu) under N₂ after reduction at 673 K (d), Cu–CeO₂ (0.1 wt% Cu) under CO₂ after reduction at 673 K (e), and Ce(NO₃)₃·6H₂O (f). (B) Fits to spectra (b) and (c) with the combination of spectra (a) and (f). Best-fit results were shown by changing the mixing ratio of data (a) and (f).

When the CeO₂ was reduced under hydrogen at 673 K (spectrum b), a shoulder peak gradually grew at 5727 eV, on the lower side of peak at 5731 eV. As an intense whiteline peak appeared at 5726.7 eV in the spectrum for Ce^III(NO₂)₃·6H₂O (Figure 4A-f), the shoulder peak for spectrum b suggested the partial reduction of initial Ce⁴⁺ to Ce³⁺. The partial reduction of CeO₂ is traditionally known to promote electron-donating catalysis, e.g., ammonia synthesis (Izumi et al., 1996; Aika et al., 1997). The spectrum b was fitted with the spectrum a for fresh CeO₂ and spectrum f for Ce(NO₂)₃·6H₂O by changing the mixing ratio of standard spectra (Izumi and Nagamori, 2000; Izumi et al., 2007). Spectra a and f were used as models of Ce⁴⁺ and Ce³⁺ states, respectively. The goodness of fit was evaluated based on the residual-factor (R_f)

$R_f=\frac{{\displaystyle \int {\left|{\chi }^{\text{sample}\text{data}}(k)-{\chi }^{\text{reference}\text{data}}(k)\right|}^2}\text{d}k}{{\displaystyle \int {\left|{\chi }^{\text{sample}\text{data}}(k)\right|}^2}\text{d}k}$

The spectrum b was best fitted with the mixing ratio of Ce⁴⁺:Ce³⁺ = 90:10 (Figure 4B-b).

The shoulder peak at 5727 eV also appeared in the XANES spectrum for reduced Cu–CeO₂ (0.5 wt% Cu; spectrum c), and the intensity was greater than that in spectrum b for reduced CeO₂. The spectrum c was also fitted with the spectrum a (Ce⁴⁺) and spectrum f (Ce³⁺) by changing the mixing ratio. The best fit was realized with the mixing ratio was Ce⁴⁺:Ce³⁺ = 85:15 (Figure 4B-c).

The Ce L₃-edge XANES spectrum for reduced Cu–CeO₂ catalyst (0.1 wt% Cu; spectrum d) was essentially identical with that for reduced CeO₂ catalyst (spectrum b). The best-fit ratio with the mixing standard spectrum component of Ce⁴⁺ and Ce³⁺ was 90 and 10%. However, the shoulder peak at 5727 eV in the spectrum significantly weakened when 60 kPa of CO₂ was introduced to the reduced Cu–CeO₂ (0.1 wt% Cu) at 290 K (spectrum e). The best-fit ratio with the mixing standard spectrum component of Ce⁴⁺ and Ce³⁺ was 95 and 5%. The decrease of shoulder peak intensity at 5727 eV suggested re-oxidation of Ce³⁺ to Ce⁴⁺ by the reaction with CO₂.

Discussion

DMC Synthesis Under Milder Conditions

DMC synthesis from CO₂ and methanol was reported at a synthesis rate of 1.8–5.1 mmol h⁻¹ g⁻¹_cat using CeO₂ at 403 K and 8.7 MPa for 2–4 h (Yoshida et al., 2006). DMC synthesis rate from CO₂ and methanol in this work using reduced CeO₂ at 393 K and 3.5 MPa for 6 h was lower: 0.70 mmol h⁻¹ g⁻¹_cat (Table 1A) due to lower reaction temperature and lower pressure. Because the forward reaction reduces the molar amount of materials in system from three to two and is uphill reaction (Pacheco and Marshall, 1997) (Equation 1), reaction conditions of lower reaction temperature and lower pressure are disadvantageous for the DMC synthesis reaction. The synthesis rate was enhanced by a factor of 1.6 times by the pre-reduction in H₂ for CeO₂ (Table 1A).

$\begin{array}{cc}\begin{array}{l}{\text{CO}}_{\text{2}}+{\text{2CH}}_{\text{3}}\text{OH}\rightleftarrows \text{OC}({\text{OCH}}_{\text{3}}{)}_2+{\text{H}}_{\text{2}}\text{O}\\ \Delta G_{\text{r}}=51.0{\text{kJmol}}^{-1}(373\text{K})\end{array}& (1)\end{array}$

The disadvantage of moderate reaction conditions was compensated by the Cu addition to CeO₂ catalysts. At 393 K and 3.5 MPa for 2 h, the DMC synthesis rates increased to 1.8 mmol h⁻¹ g⁻¹_cat by the addition of 0.5 wt% of Cu (Table 1B).

The effects of Cu addition to the DMC synthesis rates were compared at even milder reaction conditions: at 393 K and 1.3 MPa for 2 h (Table 1C). Under the reaction conditions, the 0.1 wt% of Cu was most effective and it promoted the synthesis rate by a factor of 2.3 times (Figure 1). One of the plausible explanations is that the positive effects to induce the Ce⁴⁺ site reduction to facilitate H₂ dissociation and spillover on the catalyst surface and negative effects to block (cover) the surface active sites for DMC synthesis, e.g., the adsorption/activation sites for methanol, compromised to make a synthesis rate maximum at the Cu amount of 0.1 wt%.

The maximal DMC synthesis rate using Cu–CeO₂ catalyst (0.1 wt% Cu) at 393 K and 1.3 MPa was 0.95 mmol h⁻¹ g⁻¹_cat (Table 1f), but the rate at 403 K and 6.6 MPa was quite higher (3.1 mmol h⁻¹ g⁻¹_cat), nearly equivalent to those in literature using CeO₂ (1.8–5.1 mmol h⁻¹ g⁻¹_cat) at even severe conditions (403 K and 8.7 MPa) (Yoshida et al., 2006), demonstrating the effects of pre-reduction and/or the Cu addition to CeO₂ found in this work. The S_BET values (78–94 m² g⁻¹_cat; Table 2) for Cu–CeO₂ catalysts (0.1–0.5 wt% Cu) were also similar to those for CeO₂ catalyst reported (80 m² g⁻¹_cat) (Yoshida et al., 2006).

The effects of ZrO₂ mixed with CeO₂ (Tomishige et al., 2001; Zhang et al., 2011b) were also interpreted to enhance the redox chemistry between Ce⁴⁺ and Ce³⁺. In this sense, the redox of Cu⁺ and Cu²⁺ may enhance the redox between Ce⁴⁺ and Ce³⁺. We tested Co–CeO₂ catalyst under the reaction condition of Table 1d. The conversion of methanol to DMC was 0.23% (not listed), slightly inferior to Cu–CeO₂ catalyst. Furthermore, in our preliminary results, the conversions to DMC using Fe–CeO₂ and Ni–CeO₂ catalysts were nearly equivalent to that using Co–CeO₂ catalyst. Thus, the effects of hydrogen activation and/or redox of added metal (Fe, Co, Ni, or Cu) to CeO₂ may work in similar way: enhancing effects of mixed metal ions and/or activating effects of hydrogen during pretreatment.

The reactions at lower reaction temperatures were tested (Table 1E). At 2.7 MPa using Cu–CeO₂ catalyst (0.5 wt% of Cu), DMC was formed at as low as 353 K (Table 1E). The temperature dependence of DMC synthesis rates nicely followed the Arrhenius equation to give the apparent activation energy: 120 kJ mol⁻¹ (Figure 3, inset). Similar range of apparent activation energy (107 kJ mol⁻¹) was obtained using homogeneous Sn catalysts in the temperature range of 357–403 K (Kalhor et al., 2011). The dependences of DMC synthesis rates on the CO₂ pressure and total reactant pressure were also investigated at 393 K using Cu–CeO₂ catalyst (0.5 wt% of Cu; Table 1D). DMC was synthesized as low as 1.3 MPa.

The progress of catalysts to synthesize DMC from CO₂ is quite fast, especially under relatively mild conditions (see the Introduction section). The Cu–CeO₂ catalysts in this study are one of the good catalysts to work at relatively mild conditions. The dependence of synthesis rates on pressure and temperature (Table 1) was interpreted based on X-ray spectroscopy in next section by monitoring the oxygen defect sites and Ce³⁺.

Active Sites of DMC Synthesis

The dependence of DMC synthesis on the CO₂ pressure (previous section) was proportional (Figure 2). This fact suggested that the key reaction step of DMC synthesis depended linearly on the CO₂ concentration.

To provide the insight into the surface reaction mechanism, the electronic state and structure for Ce sites were investigated using Ce L₃-edge XANES. 10–15% of the Ce⁴⁺ sites of as-prepared CeO₂ or Cu–CeO₂ (0.5 wt% of Cu) were reduced to Ce³⁺ based on the shoulder peak intensity at 5727 eV (Figure 4b,c). Similarly, 10% of the Ce⁴⁺ sites of as-prepared Cu–CeO₂ (0.1 wt% of Cu) were reduced to Ce³⁺ under H₂ at 673 K, but a half of the Ce³⁺ sites were re-oxidized to Ce⁴⁺ by the introduction of CO₂ at 290 K (Figure 4d,e). These changes in the XANES spectra suggested the adsorption of CO₂ at the surface defect sites over the catalyst and the associated, neighboring Ce³⁺ sites to the defects were re-oxidized to Ce⁴⁺. This reduction and re-oxidation mechanism was already reported on CeO₂ layers grown over Cu(111) surface (Staudt et al., 2010).

The proposed reaction mechanism was shown in Figure 5. Based on the dependence of DMC synthesis rates on the CO₂ pressure and the change of a shoulder peak at 5727 eV in the Ce L₃-edge XANES spectra, O vacancy was assumed as defect site and worked to adsorb CO₂. The population of O vacancy should increase by the reduction in H₂ and/or by the presence of Cu sites in catalysts. In order to synthesize DMC, surface Lewis base sites are required to subtract H atom from methanol (Figure 5). If each H atom was subtracted at the Lewis base site from two methanol molecules, DMC and water molecules are formed to restore an O vacancy site.

FIGURE 5

Figure 5. Proposed reaction mechanism of CO₂ conversion to DMC using partially-reduced Ce oxide surface.

Conclusions

Reduction of CeO₂ and Cu–promoted CeO₂ catalysts in hydrogen at 673 K was effective to enhance the DMC synthesis from CO₂ and methanol by a factor of 1.6–1.2 times. Added Cu worked cooperatively with CeO₂ catalysts as it accelerated the partial reduction of Ce⁴⁺ sites to Ce³⁺. At the same time, doped Cu sites may block surface active sites. As a compromise, the DMC synthesis rate was maximal: 0.95 mmol h⁻¹ g⁻¹_cat at 393 K and 1.3 MPa (total pressure) in 2 h when the Cu amount was 0.1 wt% for reduced Cu–CeO₂ catalyst. The DMC synthesis was possible at the reaction temperature as low as 353 K (2.7 MPa) using the reduced Cu–CeO₂ catalyst. The apparent activation energy was calculated to be 120 kJ mol⁻¹. Based on the Ce L₃-edge XANES, 10% of Ce sites were reduced to Ce³⁺ by the reduction in H₂ for Cu–CeO₂ (0.1 wt% of Cu) while half of them were re-oxidized to Ce⁴⁺ by the introduction of CO₂ at 290 K. A linear rate dependence on CO₂ pressure and the re-oxidation in CO₂ suggest that the adsorption of CO₂ might be the key step in DMC synthesis. H subtraction from methanol needs to occur at the neighboring sites of adsorbed CO₂. Two methoxy groups and adsorbed CO₂ combine then to form DMC and water and restores surface O vacancy (defect site).

Conflict of Interest Statement

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Acknowledgments

The authors are grateful for the financial support received from the Asahi Glass Foundation (2009–2010). The X-ray absorption experiments were performed with the approval of the Photon Factory Review Committee (No. 2012G683, 2011G083, 2011G033) and the grant of the Priority Program for Disaster-Affected Quantum Beam Facilities (2011A1977, 2011A1978, SPring-8 & KEK). The authors also thank Yusuke Yoshida and Yuta Ogura at Chiba University, Graduate School of Science, for the discussion of reaction conditions.

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