# Use of CuNi/YSZ and CuNi/SDC Catalysts for the Reverse Water Gas Shift Reaction

Authors: Maxime Lortie; Rima J. Isaifan
Journal: Journal of Catalysts
 (2015)

---

## Abstract

Cu50Ni50 nanoparticles were synthesized using a modified polyol method and deposited on samarium-doped ceria, SDC, and yttria-stabilized zirconia, YSZ, supports to form reverse water-gas shift, RWGS, catalysts.  The best CO yields, obtained with the Cu50Ni50/SDC catalyst, were about 90% of the equilibrium CO yields.  In contrast CO yields using Pt/SDC catalysts were equal to equilibrium CO yields at 700°C.  Catalyst selectivity to CO was 100% at hydrogen partial pressures equal to CO2 partial pressures, 1 kPa, and decreased as methane was formed when the hydrogen partial pressure was 2 kPa or greater.  The reaction results were explained using a combination of Eley-Rideal and Langmuir-Hinshelwood mechanisms that involved adsorption on the metal surface and the concentration of oxygen vacancies in the support.  Finally the Cu50Ni50/SDC catalyst was found to be thermally stable for 48 hours at 600/700°C.


---

## Body

## 1. Introduction

The emission of carbon dioxide into the environment is viewed by many as a major contributor to global warming [1]. In spite of the current fossil fuel energy prices, the use of fossil fuels continues to increase resulting in more carbon dioxide emissions. Those emissions affect the state of the atmosphere and the state of the oceans.Carbon capture and storage technologies are one means of diminishing CO2 emissions. Unfortunately, storing CO2 in underground caverns is not sustainable because all the caverns will eventually be filled. An alternative to carbon storage would be the reaction of CO2 with another chemical to obtain a useful product.This work describes the reaction of carbon dioxide with hydrogen obtained from a renewable source. By hydrogenating CO2 [2, 3], it is possible to obtain syngas via (1) or alcohols and hydrocarbons (using the Fischer-Tropsch process), via (2):
(1)
CO
2
+
H
2
⟷
CO
+
H
2
O
(2)
x
CO
2
+
2
x
-
z
+
y
2
H
2
⟷
C
x
H
y
O
z
+
2
x
-
z
H
2
OEquation (1) is the reverse water-gas shift reaction (RWGS). Equation (2) is a synthesis reaction that is practiced on an industrial scale, the Fischer-Tropsch process. In (2) when x
=
1, y
=
4, and z
=
0, methane (CH4) is formed. It is a common by-product of the RWGS reaction. When x
=
1, y
=
4, and z
=
1, the product is methanol (CH3OH). When z
=
0 and 5
<
x
<
20, a highly valued liquid hydrocarbon product is obtained.An appropriate catalyst must satisfy several criteria. Because the equilibrium yield of CO from the RWGS reaction increases with temperature, thermal stability of the catalyst is one criterion. Others are rapid kinetics and selectivity to CO rather than to CH4.Noble metals such as platinum (Pt) have been studied and proven to be among the best RWGS catalysts because they have the ability to dissociate H2 [2]. Also, Pt is stable at high temperatures and produces both high CO selectivity and CO2 conversion [4–6]. However, noble metals such as Pt have a high cost.Copper (Cu) and nickel (Ni) transition metals may be promising alternative catalysts to Pt noble metals. One indication is that both of these metals have produced promising results with the water gas shift, WGS, reaction [2, 7] that is shown in the following:
(3)
CO
+
H
2
O
⟷
CO
2
+
H
2Good results were also obtained when they were tested individually on catalyst supports [4–6] using the RWGS reaction.Metallic pure Cu catalysts have shown a tendency to deactivate over time when exposed to high temperatures [8–10]. Stabilizers have been used in an attempt to improve copper’s thermal stability. Chen et al. [11] reported that an iron (Fe) additive stabilized Cu supported on SiO2 at 600°C for up to 120 h. It also increased CO2 conversion by 7%. In contrast, Cu without Fe deactivated after only 5 hours on stream ultimately reaching 0% conversion after 120 h. Other additives include potassium [12] and zinc oxide [9].Chen et al. [13] showed that a Ni catalyst used for the RWGS reaction enhanced the formation of CH4 which is undesirable. They also investigated a Ni catalyst that was promoted with a potassium (K) additive. Although K increased the selectivity toward CO, it also caused the formation of coke.Y. Liu and D. Liu [14] made a bimetallic Ni and Cu catalyst and used it for the RWGS reaction. Their research was aimed at examining the effect of both metals on selectivity for the RWGS reaction. They found that an increase in catalyst Ni content generated greater CH4 yields while increased Cu contents generated greater CO selectivity.Catalysts are often supported on materials such asγ-Al2O3, SiO2, and C. Yttria-stabilized zirconia, YSZ, and samarium-doped ceria, SDC, are two less common supports that have shown potential for the RWGS reaction [15, 16]. Both contain oxygen vacancies.Yttria-stabilized zirconia, Y0.15Zr0.85O1.925, is a combination of 0.15
*
Y
2
O
3 and 0.85 ZrO2. It is a conductive ceramic which has been used in solid oxide fuel cells and sensor technologies [17]. It is also used for the electrochemical promotion of catalysts, EPOC [18]. The purpose for doping ZrO2 with Y2O3 is twofold: (1) Y2O3 stabilizes the cubic fluorite structure eliminating volumetric variations caused by phase transformations, and (2) Y2O3 creates oxygen vacancies within the ZrO2 lattice [19, 20]. Oxygen vacancies are important for all of the YSZ applications mentioned above. In addition oxygen vacancies in ZrO2 have been shown to affect the WGS reaction [7].Similarly, adding dopants to ceria, CeO2, increases the oxygen vacancies within the crystal lattice [8]. Doping with cations having an ionic radius and electronegativity close to CeO2 is considered to be the most appropriate [21]. Samarium showed the greatest resistance to reduction of the CeO2 support [22] among the doping agents investigated. Since the intent of the work was to examine the effect of oxygen vacancies and not the reducibility of the support, samarium was chosen as the dopant. Sm0.2Ce0.8O1.9 (SDC) is a combination of 0.2
*
Sm
2
O
3 and 0.8
*
CeO
2.YSZ and SDC have different oxygen vacancy contents. Samarium-doped ceria, Sm0.2Ce0.8O1.9, has 0.1 oxygen vacancies per cation when compared to CeO2. In contrast, yttria-stabilized zirconia, Y0.15Zr0.85O1.926, has 0.074 oxygen vacancies per cation when compared to ZrO2. Both of these materials have been tested by themselves without the addition of other metals and have demonstrated thermal stability and CO2 conversion [15].In the present work, Cu50Ni50 nanoparticles were synthesized using a modified polyol technique and deposited on SDC and YSZ supports. The SDC and YSZ supported catalysts were compared to catalysts containing Pt nanoparticles deposited on the same supports at the same reaction conditions. The Cu50Ni50 catalyst with the best performance was examined for thermal stability experiments in which the temperature was maintained between 600 and 700°C for 48 h.


## 2. Experimental

### 2.1. Catalyst Preparation

The synthesis of CuNi nanoparticles was achieved using a modified polyol technique. First, 314.5 mg of nickel nitrate (Ni(NO3)2) (hexahydrate 99.999% metal basis, Alfa Aesar) was dissolved in 30 mL of ethylene glycol (anhydrous 99.8%, SigmaAldrich) to obtain a green solution. That solution’s pH was then increased to 11 via the addition of 199 mg of sodium hydroxide (NaOH) pellets (EM Science, ACS grade) to obtain Solution 1. This caused the solution to slightly darken. In a separate beaker, 321.8 mg of copper nitrate (Cu(NO3)2) (hexahydrate 99.999% metal basis, Alfa Aesar) was dissolved in 30 mL of ethylene glycol to obtain a blue solution. Its pH was also increased to 11 using 199 mg of NaOH pellets to obtain Solution 2. Solution 2 also darkened. Following this, Solution 1 was poured into a round bottom flask, refluxed, and stirred at 196°C. Once the temperature reached 196°C, Solution 2, at room temperature, was added to the round bottom flask. The ratio of Solution 1 to Solution 2 was selected to obtain CuNi colloidal particles of 50 wt% Cu/50 wt% Ni (nominally Cu50Ni50). The combined solution was refluxed at 196°C for 30 minutes and then cooled. The combined solution gradually became dark brown in colour. Once cooled, the colloidal particles were stored in the ethylene glycol solution. The final pH of the combined solution was 7.The colloidal particles were then deposited on supports using a wet impregnation technique. A powdered support was placed into a beaker and subsequently an amount of the combined solution was poured unto the powder. The amount of combined solution was chosen to result in nominally 10 wt% of CuNi when deposited on the supports, which corresponds to a Cu50Ni50 metal/support ratio of 1 to 9. The solution/support was sonicated for 1 hour and stirred for 24 hours. The supported metal was then centrifuged and washed with deionized water several times to remove the salts remaining after the synthesis procedure. The supports were yttria-stabilized zirconia (Tosoh, BET surface area 14.8 m2·g−1) and samarium-doped ceria (FCM, BET surface area 31.0 m2·g−1). The catalyst was then dried using a freeze dryer. Prior to any experiments, the catalyst was crushed.Pt nanoparticles were synthesized using a polyol method as described elsewhere [23]. It involved diluting PtCl4 in a 0.06 M NaOH solution of ethylene glycol. The mixture was then refluxed at 160°C for 3 hours. The deposition technique was the same as that for Cu50Ni50 and the same supports were used. After deposition, each support contained 1 wt% of Pt nanoparticles.


### 2.2. Physical Characterization

X-ray diffraction (XRD) measurements were made on the CuNi colloidal particles using a Rigaku Ultima IV diffractometer which used a Cu Kα X-ray (40 ma, 44 kV) operating with focused beam geometry and a divergence slit of 2/3 degree, a scan speed of 0.17 deg min−1, and a scan step of 0.06 degrees were used while operating between 35° and 55°.Characterization of the CuNi metal particles by scanning electron microscopy, SEM, and X-ray photoelectron spectroscopy has been reported previously [24]. Characterization of the Pt metal particles by transmission electron microscopy, TEM, has also been reported previously [25]. The characterization measurements were made with the metal particles supported on carbon, in order to avoid electrostatic charging that would occur when metals are supported on insulating materials.


### 2.3. Catalytic Performance

Catalytic reaction rates were measured on both Cu50Ni50 and Pt supported nanoparticles for the RWGS reaction. First, the dry metal/support catalyst was finely crushed. Then, 50 mg of the metal/support catalyst was placed on top of a fritted quartz bed located within a tubular, 35 mL quartz reactor. A gaseous mixture containing 1 kPa H2 (Grade 4.0, Linde) and 1 kPa CO2 (Grade 3.0, Linde) with the balance being He (Grade 4.7 Linde) flowed through the reactor at a flow rate of 510 mL·min−1. The reaction was performed at a total pressure of 1 atm using three consecutive temperature cycles. Each temperature cycle consisted of a series of experiments over the temperature range from 400°C to 700°C. Before each experiment, the temperature was held constant for 30 min. The same mass of catalyst was used in each experiment, 50 mg, so that the weight hourly space velocity was constant at 612 L/(h g). Nevertheless, the gas hourly space velocity (GHSV) was different because the supports had different bulk densities (1187 g/L for the YSZ support and 1570 g/L for the SDC support). The GHSV values were 716000 h−1 and 960800 h−1, respectively, for CuNi/YSZ and CuNi/SDC catalysts. The effluent was dehumidified by flowing through an adsorbent and was analyzed by flowing through a mass spectrometer (Ametek Proline DM 100) and a nondispersive infrared CO gas analyzer (Horiba VIA-510). Each set of experiments was repeated three times (24 hrs total) in order to examine reproducibility and stability.A schematic of the experimental equipment is shown in Figure1.Figure 1
Schematic of experimental setup used for catalytic testing of the RWGS reaction.The yield of CO was calculated using the following formula:(4)
Yield
of
CO
%
=
CO
out
CO
2
in
×
100
%
The quantitative measurements obtained using the NDIR CO analyzer were used to obtain the concentration of CO coming out of the reactor (CO
out). The mass spectrometer identified any by-products that were formed via side reactions such as CO methanation. The mass spectrometer indicated the presence of gases with a molecular weight of up to 50 atomic units and had a detection limit of 50 ppm.Thermal stability experiments were performed on the Cu50Ni50/SDC catalyst by maintaining the temperature at 700°C for 24 hrs at a total pressure of 1 atm and a total flow rate of 510 mL·min−1. The gas composition was 1 kPa H2 and 1 kPa CO2 with the balance being He. Subsequently, the temperature was decreased to 600°C and maintained constant for another 24 hrs, for a total catalyst time-on-stream of 48 hrs.Thermodynamic equilibrium calculations were performed using UniSim simulation software. A Gibbs reactor calculation was used to determine the equilibrium conversion at the operating conditions. Equilibrium conversions were compared with experimental results.


## 2.1. Catalyst Preparation

The synthesis of CuNi nanoparticles was achieved using a modified polyol technique. First, 314.5 mg of nickel nitrate (Ni(NO3)2) (hexahydrate 99.999% metal basis, Alfa Aesar) was dissolved in 30 mL of ethylene glycol (anhydrous 99.8%, SigmaAldrich) to obtain a green solution. That solution’s pH was then increased to 11 via the addition of 199 mg of sodium hydroxide (NaOH) pellets (EM Science, ACS grade) to obtain Solution 1. This caused the solution to slightly darken. In a separate beaker, 321.8 mg of copper nitrate (Cu(NO3)2) (hexahydrate 99.999% metal basis, Alfa Aesar) was dissolved in 30 mL of ethylene glycol to obtain a blue solution. Its pH was also increased to 11 using 199 mg of NaOH pellets to obtain Solution 2. Solution 2 also darkened. Following this, Solution 1 was poured into a round bottom flask, refluxed, and stirred at 196°C. Once the temperature reached 196°C, Solution 2, at room temperature, was added to the round bottom flask. The ratio of Solution 1 to Solution 2 was selected to obtain CuNi colloidal particles of 50 wt% Cu/50 wt% Ni (nominally Cu50Ni50). The combined solution was refluxed at 196°C for 30 minutes and then cooled. The combined solution gradually became dark brown in colour. Once cooled, the colloidal particles were stored in the ethylene glycol solution. The final pH of the combined solution was 7.The colloidal particles were then deposited on supports using a wet impregnation technique. A powdered support was placed into a beaker and subsequently an amount of the combined solution was poured unto the powder. The amount of combined solution was chosen to result in nominally 10 wt% of CuNi when deposited on the supports, which corresponds to a Cu50Ni50 metal/support ratio of 1 to 9. The solution/support was sonicated for 1 hour and stirred for 24 hours. The supported metal was then centrifuged and washed with deionized water several times to remove the salts remaining after the synthesis procedure. The supports were yttria-stabilized zirconia (Tosoh, BET surface area 14.8 m2·g−1) and samarium-doped ceria (FCM, BET surface area 31.0 m2·g−1). The catalyst was then dried using a freeze dryer. Prior to any experiments, the catalyst was crushed.Pt nanoparticles were synthesized using a polyol method as described elsewhere [23]. It involved diluting PtCl4 in a 0.06 M NaOH solution of ethylene glycol. The mixture was then refluxed at 160°C for 3 hours. The deposition technique was the same as that for Cu50Ni50 and the same supports were used. After deposition, each support contained 1 wt% of Pt nanoparticles.


## 2.2. Physical Characterization

X-ray diffraction (XRD) measurements were made on the CuNi colloidal particles using a Rigaku Ultima IV diffractometer which used a Cu Kα X-ray (40 ma, 44 kV) operating with focused beam geometry and a divergence slit of 2/3 degree, a scan speed of 0.17 deg min−1, and a scan step of 0.06 degrees were used while operating between 35° and 55°.Characterization of the CuNi metal particles by scanning electron microscopy, SEM, and X-ray photoelectron spectroscopy has been reported previously [24]. Characterization of the Pt metal particles by transmission electron microscopy, TEM, has also been reported previously [25]. The characterization measurements were made with the metal particles supported on carbon, in order to avoid electrostatic charging that would occur when metals are supported on insulating materials.


## 2.3. Catalytic Performance

Catalytic reaction rates were measured on both Cu50Ni50 and Pt supported nanoparticles for the RWGS reaction. First, the dry metal/support catalyst was finely crushed. Then, 50 mg of the metal/support catalyst was placed on top of a fritted quartz bed located within a tubular, 35 mL quartz reactor. A gaseous mixture containing 1 kPa H2 (Grade 4.0, Linde) and 1 kPa CO2 (Grade 3.0, Linde) with the balance being He (Grade 4.7 Linde) flowed through the reactor at a flow rate of 510 mL·min−1. The reaction was performed at a total pressure of 1 atm using three consecutive temperature cycles. Each temperature cycle consisted of a series of experiments over the temperature range from 400°C to 700°C. Before each experiment, the temperature was held constant for 30 min. The same mass of catalyst was used in each experiment, 50 mg, so that the weight hourly space velocity was constant at 612 L/(h g). Nevertheless, the gas hourly space velocity (GHSV) was different because the supports had different bulk densities (1187 g/L for the YSZ support and 1570 g/L for the SDC support). The GHSV values were 716000 h−1 and 960800 h−1, respectively, for CuNi/YSZ and CuNi/SDC catalysts. The effluent was dehumidified by flowing through an adsorbent and was analyzed by flowing through a mass spectrometer (Ametek Proline DM 100) and a nondispersive infrared CO gas analyzer (Horiba VIA-510). Each set of experiments was repeated three times (24 hrs total) in order to examine reproducibility and stability.A schematic of the experimental equipment is shown in Figure1.Figure 1
Schematic of experimental setup used for catalytic testing of the RWGS reaction.The yield of CO was calculated using the following formula:(4)
Yield
of
CO
%
=
CO
out
CO
2
in
×
100
%
The quantitative measurements obtained using the NDIR CO analyzer were used to obtain the concentration of CO coming out of the reactor (CO
out). The mass spectrometer identified any by-products that were formed via side reactions such as CO methanation. The mass spectrometer indicated the presence of gases with a molecular weight of up to 50 atomic units and had a detection limit of 50 ppm.Thermal stability experiments were performed on the Cu50Ni50/SDC catalyst by maintaining the temperature at 700°C for 24 hrs at a total pressure of 1 atm and a total flow rate of 510 mL·min−1. The gas composition was 1 kPa H2 and 1 kPa CO2 with the balance being He. Subsequently, the temperature was decreased to 600°C and maintained constant for another 24 hrs, for a total catalyst time-on-stream of 48 hrs.Thermodynamic equilibrium calculations were performed using UniSim simulation software. A Gibbs reactor calculation was used to determine the equilibrium conversion at the operating conditions. Equilibrium conversions were compared with experimental results.


## 3. Results and Discussion

### 3.1. Physical Characterization of Cu50Ni50

X-ray diffraction spectra of Cu50Ni50 nanoparticles are shown in Figure 2. Ni and Cu were the major species and no nitrate salts were present. X-ray diffraction peaks having 2θ values of 43.39° and 44.41° were attributed, respectively, to reflections from the 111 planes of a Cu rich alloy and from the 111 planes of a Ni rich alloy as shown in [24]. The crystalline size was obtained using Scherrer’s formula and gave 20.5 nm for the Cu rich (111) peak and 9.6 nm for the Ni rich (111) peak.Figure 2
XRD of Cu50Ni50 colloidal solution.SEM images were used to measure particle size, shape, and dispersion on a carbon support. A carbon support was used for SEM because carbon would have less electron static charging than YSZ or SDC. Two images are shown in Figure3 for both COMPO, composition, and LEI, lower secondary electron image, settings.SEM of Cu50Ni50/C in (a) LEI mode and (b) COMPO mode.
(a)
(b)Light coloured regions are indicative of Cu50Ni50 particles and the darker coloured background represents the C support. These images show good dispersion of the metal on the support and also indicate agglomeration. Antiagglomerating agents like polyvinylpyrrolidone (PVP) were not used to minimize the cost of the synthesis materials. A typical particle size observed in multiple SEM spectra was 30 nm.


### 3.2. Catalytic Performance

The only observable components in the gas stream entering the mass spectrometer were CO2, H2, CO, trace amounts of H2O, and carrier gas, He. These results indicate that CO was the main product having a typical concentration of 2000 ppm. Other products including CH4 had concentrations of less than the detection limit of the spectrometer, 50 ppm. These results with the CuNi/YSZ and CuNi/SDC catalysts were completely consistent with previous work using CuNi/C and CuNi/Al2O3 catalysts [24].CO and CH4 were the expected products with pure copper catalysts [9, 11, 14, 26] and pure nickel catalysts [14], respectively. The absence of CH4 in this work might have been caused by the enhanced copper concentration on the catalyst surface. XPS analysis reported previously for Cu50Ni50/C catalysts [24] indicated that the surface atomic Cu/Ni was “2,” even though the bulk atomic Cu/Ni rate was “1.” Perhaps any CO formed on Ni atom sites may have “spilled over” to Cu atom sites and desorbed prior to further hydrogenation to CH4.The data in Figure4 were obtained when the RWGS reaction was performed with a catalyst composed of platinum supported on a YSZ support. The CO yields obtained during all of the cycles were similar at 400 and 450°C. In contrast the CO yields at 650 and 700°C for the third cycle were slightly less than those during the first and second cycles.Figure 4
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 716000 h−1, 50 mg of catalyst: Pt/YSZ, 1 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.Figure5 demonstrates the results obtained when the RWGS reaction was performed over a catalyst composed of CuNi nanoparticles supported on a YSZ support. The CO yields obtained during the second and third cycles were similar and were somewhat less than those obtained during the first cycle. It indicates that while some deactivation had occurred, the catalysts became thermally stable after the first cycle. Cu alone is known to be unstable at high temperatures [9, 11, 26]. It may be that the Ni in Cu50Ni50 stabilizes Cu so that the Ni provides the desired thermal stability and the Cu provides the desired CO yields.Figure 5
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 716000 h−1, 50 mg of catalyst: Cu50Ni50/YSZ, 10 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The data in Figure6 shows the results obtained when Pt supported on a samarium-doped ceria support was used for the RWGS reaction. The CO yields obtained during the second and third cycles were superior to those obtained during the first cycle. This might be caused by a reduction of Pt oxide particles on the surface of the catalyst to metal Pt. Once reduced, its catalytic performance appears to be stable. The fact that similar CO yields were obtained during the second and third cycles indicates that no deactivation was apparent. The thermal stability shown by Pt was expected based on previous reports [16, 27–29]. The CO yields obtained with the Pt/SDC catalyst in Figure 6 were superior to those obtained with the Pt/YSZ catalyst in Figure 4.Figure 6
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 960800 h−1, 50 mg of catalyst: Pt/SDC, 1 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The data in Figure7 were obtained when CuNi nanoparticles supported on a samarium-doped ceria support were used for the RWGS reaction. The CO yields obtained during all of the cycles were virtually the same, indicating that the catalyst was thermally stable and that there was no deactivation. The CO yields obtained with the Cu50Ni50/SDC catalyst in Figure 7 were superior to those obtained with the Cu50Ni50/YSZ catalyst in Figure 5.Figure 7
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 960800 h−1, 50 mg of catalyst: Cu50Ni50/SDC, 10 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The average yields of the two Pt catalysts are compared with the equilibrium CO yield in Figure8. The CO yield with the Pt/SDC catalyst is better than that with the Pt/YSZ catalyst at all temperatures. The CO yield with the Pt/YSZ catalyst was always less than the equilibrium CO yield. Although the CO yield with the Pt/SDC catalyst was less than the equilibrium yield at lower temperatures, at 700°C the equilibrium CO yield was attained using the Pt/SDC catalyst.Figure 8
Average yield of CO for the RWGS reaction using Pt supported on SDC and YSZ at 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He. * = equilibrium, ◆ = Pt/SDC, and ■ = Pt/YSZ.The average yields of the two Cu50Ni50 catalysts are compared with the equilibrium yield in Figure 9. The CO yield with the Cu50Ni50/SDC catalyst is better than that with the Cu50Ni50/YSZ catalyst at all temperatures. In addition the CO yields with both catalysts are less than the equilibrium CO yields at all temperatures.Figure 9
Average yield of CO for the RWGS reaction using Cu50Ni50 supported on SDC and YSZ at 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He. * = equilibrium, ⋄ = Cu50Ni50/SDC, and □ = Cu50Ni50/YSZ.For both Pt and Cu50Ni50 catalysts the CO yields were greater with the SDC support than with the YSZ support. This is consistent with data reported by Dow and Huang [19] for SDC and YSZ supports that did not contain Cu50Ni50. [15]. The CO yields may be related to the concentration of bulk phase oxygen vacancies in the two supports, 0.1 for SDC and 0.074 for YSZ.Two supports having no bulk phase oxygen vacancies, C andγ-Al2O3, were investigated in previous work [24]. Their results with Cu50Ni50 nanoparticles were combined with the Cu50Ni50 nanoparticle results on YSZ and SDC supports and are shown in Figure 10. The CO yields in Figure 10 are definitely correlated with the oxygen vacancy content of the support. Other reaction results have also been correlated with oxygen vacancies. For example, the results Pekridis et al. [16] obtained using a solid oxide fuel cell (SOFC) at 650–800°C were explained in terms of oxygen vacancies.Figure 10
CO yield versus bulk phase oxygen content in supports containing Cu50Ni50 nanoparticles at 700°C and 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He.The catalysts containing carbon andγ-Al2O3 supports had measurable CO yields even though they did not contain bulk phase oxygen vacancies. The surfaces of γ-Al2O3 contain oxygen vacancies. During the preparation of γ-Al2O3, hydroxyl groups are formed on the solid surface. When the solid is heated some of the hydroxyl groups combine to form a water molecule that enters the gas phase [30]. An oxygen anion and an oxygen vacancy are left behind on the solid alumina surface. The surfaces of carbon particles contain various oxygen groups including hydroxyls and carboxyls. When hydrogen is present at the reaction conditions of these experiments, water can be formed and enter the gas phase, leaving surface oxygen vacancies on the surface. Although the carbon and γ-Al2O3 supports do not contain bulk phase oxygen vacancies, they do contain surface oxygen vacancies. The presence of surface oxygen vacancies would be consistent with the CO yields they obtained.A diagram illustrating the bifunctional nature of the catalyst is shown in Figure11. A catalytic mechanism can be suggested which involves the adsorption of hydrogen on the CuNi metal phases and the adsorption of carbon dioxide on the support. The amount of H2 adsorbed on pure Ni is known to be five times greater than that adsorbed on pure Cu [31]. The amount of hydrogen adsorbed on CuNi alloys does not vary much with alloy composition and is approximately one-third of that adsorbed on pure Ni [31]. CO2 adsorption on YSZ has been reported as a bicarbonate species [32]. Although we are not aware of any SDC data, CO2 adsorption has also been reported on gallium doped ceria as a bicarbonate species [33].Figure 11
Diagram showing adsorbed species on the surface of a bifunctional catalyst operating through an Eley-Rideal and a Langmuir Hinshelwood mechanism.Based on the above, the adsorption of the reactants can be expressed in the form of equations. CO2 adsorbed on support oxygen vacancies, V
o
x
(
S
), might be represented as shown in the following:
(5)
CO
2
(
g
)
+
V
o
x
(
S
)
=
CO
2
(
ads
)
-Sup
Hydrogen from the gas phase might be dissociatively adsorbed on the surface of the metal, where the electron on a dissociated hydrogen radical is shared with an empty orbital in the conduction band of the metal, □
Me, as shown in the following:
(6)
H
2
(
g
)
+
2
□
Me
=
2
H
(
ads
)
-Me
Eley-Rideal mechanisms might be operative in two ways. Hydrogen from the gas phase might react with adsorbed CO2 as shown in the following:
(7)
1
2
H
2
(
g
)
+
CO
2
(
ads
)
-Sup
=
OCOH
(
ads
)
-Sup
(8)
1
2
H
2
(
g
)
+
OCOH
(
ads
)
-Sup
=
CO
(
g
)
+
H
2
(
g
)
+
V
o
x
(
S
)
Since the CO2 adsorbed on the support reacts with hydrogen in the gas phase, it could reduce CO2 to CO even if the catalyst did not contain metal particles, as was shown in other work reported by Ismail [15]. In his work, he described both YSZ and SDC catalysts that converted CO2 to other products without a metallic component in the catalyst.A second Eley-Rideal mechanism would occur if CO2 in the gas phase reacted with adsorbed H2 as shown in (9). Vesselli et al. [34, 35] have described the occurrence of the Eley-Rideal mechanism in RWGS reactions:
(9)
CO
2
(
g
)
+
2
H
(
ads
)
-Me
=
CO
(
g
)
+
H
2
O
(
g
)
+
2
□
MeA Langmuir-Hinshelwood mechanism might also be possible. The adsorbed hydrogen might react with the adsorbed CO2 at the three-phase (metal-support-gas) boundary, as shown in (10). Alternatively, the hydrogen adsorbed on the metal surface diffuses from the metal surface unto the support surface prior to reacting via (10) (hydrogen spillover). The resulting species, OCOH(ads), might diffuse over a support surface by hopping from one oxygen vacancy to another until two OCOH(ads) species were adjacent to one another:
(10)
H
(
ads
)
-Me
+
CO
2
(
ads
)
-Sup
=
OCOH
(
ads
)
-Sup
+
□
Me
which might yield the reaction via the following:
(11)
2
OCOH
ads
-Sup
=
CO
2
(
ads
)
-Sup
+
V
o
x
(
S
)
+
CO
(
g
)
+
H
2
O
(
g
)
The rate of surface diffusion might be influenced by the concentration of oxygen vacancies on the support surface. In this case the reaction would occur on an extended region of the support surface surrounding the three-phase boundary. Kim et al. [5] proposed a similar Langmuir-Hinshelwood mechanism to explain results obtained with a solid oxide fuel cell.


### 3.3. Stability Measurements

Time-on-stream experiments were performed in order to examine the catalyst’s thermal stability over a 48-hour period, 24 hours at 700°C and subsequently another 24 hours at 600°C without cooling down the catalyst. The results are shown in Figure12. No deactivation was apparent.Figure 12
Stability measurements of Cu50Ni50/SDC for 2 consecutive days of testing at (a) 700°C and (b) 600°C. GHSV = 960800 h−1. Total flow rate of 510 mL·min−1.This is a significant achievement in the use of a Cu catalyst for the RWGS reaction. Previous studies suggested that Cu is inadequate for use at high temperatures because of its tendency to deactivate over time [11, 12]. In fact, Cu/SiO2 began deactivating after 5 hours on stream. After 48 hours, conversion was down to approximately half the initial conversion when the catalyst was used at 600°C [12]. In contrast, the results in Figure 12 demonstrate CO yields that approached the equilibrium CO yield and suggest long-term thermal stability.The favorable results reported here can probably be attributed to Cu being used as a CuNi alloy catalyst. The Ni component is most likely responsible for the thermal stability. Other research has also shown that Ni can stabilize Cu when both metals were deposited on carbon. Specifically, a 16-hour stability period was demonstrated with a Cu50Ni50/C catalyst [24]. The 100% selectivity to CO may be attributed to the CuNi alloy surface having a much greater concentration of Cu than the bulk CuNi alloy. A large surface concentration of Cu diminishes the tendency for CH4 to be formed on Ni.All of the results reported here were obtained at small partial pressures of hydrogen. The experiments performed at H2 partial pressures of 2 kPa and greater showed (with the CO2 partial pressure constant at 2 kPa) that CH4 was formed and that 100% selectivity to CO was not obtained. There may be merit in performing future experiments at greater hydrogen partial pressures with CuNi alloy catalysts that have larger Cu/Ni ratios than the one used in this investigation, since it is known [24] that the surface Cu/Ni ratio increases nonlinearly with the bulk Cu/Ni ratio.


## 3.1. Physical Characterization of Cu50Ni50

X-ray diffraction spectra of Cu50Ni50 nanoparticles are shown in Figure 2. Ni and Cu were the major species and no nitrate salts were present. X-ray diffraction peaks having 2θ values of 43.39° and 44.41° were attributed, respectively, to reflections from the 111 planes of a Cu rich alloy and from the 111 planes of a Ni rich alloy as shown in [24]. The crystalline size was obtained using Scherrer’s formula and gave 20.5 nm for the Cu rich (111) peak and 9.6 nm for the Ni rich (111) peak.Figure 2
XRD of Cu50Ni50 colloidal solution.SEM images were used to measure particle size, shape, and dispersion on a carbon support. A carbon support was used for SEM because carbon would have less electron static charging than YSZ or SDC. Two images are shown in Figure3 for both COMPO, composition, and LEI, lower secondary electron image, settings.SEM of Cu50Ni50/C in (a) LEI mode and (b) COMPO mode.
(a)
(b)Light coloured regions are indicative of Cu50Ni50 particles and the darker coloured background represents the C support. These images show good dispersion of the metal on the support and also indicate agglomeration. Antiagglomerating agents like polyvinylpyrrolidone (PVP) were not used to minimize the cost of the synthesis materials. A typical particle size observed in multiple SEM spectra was 30 nm.


## 3.2. Catalytic Performance

The only observable components in the gas stream entering the mass spectrometer were CO2, H2, CO, trace amounts of H2O, and carrier gas, He. These results indicate that CO was the main product having a typical concentration of 2000 ppm. Other products including CH4 had concentrations of less than the detection limit of the spectrometer, 50 ppm. These results with the CuNi/YSZ and CuNi/SDC catalysts were completely consistent with previous work using CuNi/C and CuNi/Al2O3 catalysts [24].CO and CH4 were the expected products with pure copper catalysts [9, 11, 14, 26] and pure nickel catalysts [14], respectively. The absence of CH4 in this work might have been caused by the enhanced copper concentration on the catalyst surface. XPS analysis reported previously for Cu50Ni50/C catalysts [24] indicated that the surface atomic Cu/Ni was “2,” even though the bulk atomic Cu/Ni rate was “1.” Perhaps any CO formed on Ni atom sites may have “spilled over” to Cu atom sites and desorbed prior to further hydrogenation to CH4.The data in Figure4 were obtained when the RWGS reaction was performed with a catalyst composed of platinum supported on a YSZ support. The CO yields obtained during all of the cycles were similar at 400 and 450°C. In contrast the CO yields at 650 and 700°C for the third cycle were slightly less than those during the first and second cycles.Figure 4
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 716000 h−1, 50 mg of catalyst: Pt/YSZ, 1 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.Figure5 demonstrates the results obtained when the RWGS reaction was performed over a catalyst composed of CuNi nanoparticles supported on a YSZ support. The CO yields obtained during the second and third cycles were similar and were somewhat less than those obtained during the first cycle. It indicates that while some deactivation had occurred, the catalysts became thermally stable after the first cycle. Cu alone is known to be unstable at high temperatures [9, 11, 26]. It may be that the Ni in Cu50Ni50 stabilizes Cu so that the Ni provides the desired thermal stability and the Cu provides the desired CO yields.Figure 5
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 716000 h−1, 50 mg of catalyst: Cu50Ni50/YSZ, 10 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The data in Figure6 shows the results obtained when Pt supported on a samarium-doped ceria support was used for the RWGS reaction. The CO yields obtained during the second and third cycles were superior to those obtained during the first cycle. This might be caused by a reduction of Pt oxide particles on the surface of the catalyst to metal Pt. Once reduced, its catalytic performance appears to be stable. The fact that similar CO yields were obtained during the second and third cycles indicates that no deactivation was apparent. The thermal stability shown by Pt was expected based on previous reports [16, 27–29]. The CO yields obtained with the Pt/SDC catalyst in Figure 6 were superior to those obtained with the Pt/YSZ catalyst in Figure 4.Figure 6
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 960800 h−1, 50 mg of catalyst: Pt/SDC, 1 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The data in Figure7 were obtained when CuNi nanoparticles supported on a samarium-doped ceria support were used for the RWGS reaction. The CO yields obtained during all of the cycles were virtually the same, indicating that the catalyst was thermally stable and that there was no deactivation. The CO yields obtained with the Cu50Ni50/SDC catalyst in Figure 7 were superior to those obtained with the Cu50Ni50/YSZ catalyst in Figure 5.Figure 7
RWGS reaction at 1 atm,P
H
2
=
P
CO
2
=
1 kPa, balance He, GHSV = 960800 h−1, 50 mg of catalyst: Cu50Ni50/SDC, 10 wt% catalyst where ○ = 1st cycle, ▵ = 2nd cycle, and ⋄ = 3rd cycle.The average yields of the two Pt catalysts are compared with the equilibrium CO yield in Figure8. The CO yield with the Pt/SDC catalyst is better than that with the Pt/YSZ catalyst at all temperatures. The CO yield with the Pt/YSZ catalyst was always less than the equilibrium CO yield. Although the CO yield with the Pt/SDC catalyst was less than the equilibrium yield at lower temperatures, at 700°C the equilibrium CO yield was attained using the Pt/SDC catalyst.Figure 8
Average yield of CO for the RWGS reaction using Pt supported on SDC and YSZ at 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He. * = equilibrium, ◆ = Pt/SDC, and ■ = Pt/YSZ.The average yields of the two Cu50Ni50 catalysts are compared with the equilibrium yield in Figure 9. The CO yield with the Cu50Ni50/SDC catalyst is better than that with the Cu50Ni50/YSZ catalyst at all temperatures. In addition the CO yields with both catalysts are less than the equilibrium CO yields at all temperatures.Figure 9
Average yield of CO for the RWGS reaction using Cu50Ni50 supported on SDC and YSZ at 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He. * = equilibrium, ⋄ = Cu50Ni50/SDC, and □ = Cu50Ni50/YSZ.For both Pt and Cu50Ni50 catalysts the CO yields were greater with the SDC support than with the YSZ support. This is consistent with data reported by Dow and Huang [19] for SDC and YSZ supports that did not contain Cu50Ni50. [15]. The CO yields may be related to the concentration of bulk phase oxygen vacancies in the two supports, 0.1 for SDC and 0.074 for YSZ.Two supports having no bulk phase oxygen vacancies, C andγ-Al2O3, were investigated in previous work [24]. Their results with Cu50Ni50 nanoparticles were combined with the Cu50Ni50 nanoparticle results on YSZ and SDC supports and are shown in Figure 10. The CO yields in Figure 10 are definitely correlated with the oxygen vacancy content of the support. Other reaction results have also been correlated with oxygen vacancies. For example, the results Pekridis et al. [16] obtained using a solid oxide fuel cell (SOFC) at 650–800°C were explained in terms of oxygen vacancies.Figure 10
CO yield versus bulk phase oxygen content in supports containing Cu50Ni50 nanoparticles at 700°C and 1 atm. Total flow rate of 510 mL·min−1, P
CO
2
=
P
H
2
=
1 kPa, balance He.The catalysts containing carbon andγ-Al2O3 supports had measurable CO yields even though they did not contain bulk phase oxygen vacancies. The surfaces of γ-Al2O3 contain oxygen vacancies. During the preparation of γ-Al2O3, hydroxyl groups are formed on the solid surface. When the solid is heated some of the hydroxyl groups combine to form a water molecule that enters the gas phase [30]. An oxygen anion and an oxygen vacancy are left behind on the solid alumina surface. The surfaces of carbon particles contain various oxygen groups including hydroxyls and carboxyls. When hydrogen is present at the reaction conditions of these experiments, water can be formed and enter the gas phase, leaving surface oxygen vacancies on the surface. Although the carbon and γ-Al2O3 supports do not contain bulk phase oxygen vacancies, they do contain surface oxygen vacancies. The presence of surface oxygen vacancies would be consistent with the CO yields they obtained.A diagram illustrating the bifunctional nature of the catalyst is shown in Figure11. A catalytic mechanism can be suggested which involves the adsorption of hydrogen on the CuNi metal phases and the adsorption of carbon dioxide on the support. The amount of H2 adsorbed on pure Ni is known to be five times greater than that adsorbed on pure Cu [31]. The amount of hydrogen adsorbed on CuNi alloys does not vary much with alloy composition and is approximately one-third of that adsorbed on pure Ni [31]. CO2 adsorption on YSZ has been reported as a bicarbonate species [32]. Although we are not aware of any SDC data, CO2 adsorption has also been reported on gallium doped ceria as a bicarbonate species [33].Figure 11
Diagram showing adsorbed species on the surface of a bifunctional catalyst operating through an Eley-Rideal and a Langmuir Hinshelwood mechanism.Based on the above, the adsorption of the reactants can be expressed in the form of equations. CO2 adsorbed on support oxygen vacancies, V
o
x
(
S
), might be represented as shown in the following:
(5)
CO
2
(
g
)
+
V
o
x
(
S
)
=
CO
2
(
ads
)
-Sup
Hydrogen from the gas phase might be dissociatively adsorbed on the surface of the metal, where the electron on a dissociated hydrogen radical is shared with an empty orbital in the conduction band of the metal, □
Me, as shown in the following:
(6)
H
2
(
g
)
+
2
□
Me
=
2
H
(
ads
)
-Me
Eley-Rideal mechanisms might be operative in two ways. Hydrogen from the gas phase might react with adsorbed CO2 as shown in the following:
(7)
1
2
H
2
(
g
)
+
CO
2
(
ads
)
-Sup
=
OCOH
(
ads
)
-Sup
(8)
1
2
H
2
(
g
)
+
OCOH
(
ads
)
-Sup
=
CO
(
g
)
+
H
2
(
g
)
+
V
o
x
(
S
)
Since the CO2 adsorbed on the support reacts with hydrogen in the gas phase, it could reduce CO2 to CO even if the catalyst did not contain metal particles, as was shown in other work reported by Ismail [15]. In his work, he described both YSZ and SDC catalysts that converted CO2 to other products without a metallic component in the catalyst.A second Eley-Rideal mechanism would occur if CO2 in the gas phase reacted with adsorbed H2 as shown in (9). Vesselli et al. [34, 35] have described the occurrence of the Eley-Rideal mechanism in RWGS reactions:
(9)
CO
2
(
g
)
+
2
H
(
ads
)
-Me
=
CO
(
g
)
+
H
2
O
(
g
)
+
2
□
MeA Langmuir-Hinshelwood mechanism might also be possible. The adsorbed hydrogen might react with the adsorbed CO2 at the three-phase (metal-support-gas) boundary, as shown in (10). Alternatively, the hydrogen adsorbed on the metal surface diffuses from the metal surface unto the support surface prior to reacting via (10) (hydrogen spillover). The resulting species, OCOH(ads), might diffuse over a support surface by hopping from one oxygen vacancy to another until two OCOH(ads) species were adjacent to one another:
(10)
H
(
ads
)
-Me
+
CO
2
(
ads
)
-Sup
=
OCOH
(
ads
)
-Sup
+
□
Me
which might yield the reaction via the following:
(11)
2
OCOH
ads
-Sup
=
CO
2
(
ads
)
-Sup
+
V
o
x
(
S
)
+
CO
(
g
)
+
H
2
O
(
g
)
The rate of surface diffusion might be influenced by the concentration of oxygen vacancies on the support surface. In this case the reaction would occur on an extended region of the support surface surrounding the three-phase boundary. Kim et al. [5] proposed a similar Langmuir-Hinshelwood mechanism to explain results obtained with a solid oxide fuel cell.


## 3.3. Stability Measurements

Time-on-stream experiments were performed in order to examine the catalyst’s thermal stability over a 48-hour period, 24 hours at 700°C and subsequently another 24 hours at 600°C without cooling down the catalyst. The results are shown in Figure12. No deactivation was apparent.Figure 12
Stability measurements of Cu50Ni50/SDC for 2 consecutive days of testing at (a) 700°C and (b) 600°C. GHSV = 960800 h−1. Total flow rate of 510 mL·min−1.This is a significant achievement in the use of a Cu catalyst for the RWGS reaction. Previous studies suggested that Cu is inadequate for use at high temperatures because of its tendency to deactivate over time [11, 12]. In fact, Cu/SiO2 began deactivating after 5 hours on stream. After 48 hours, conversion was down to approximately half the initial conversion when the catalyst was used at 600°C [12]. In contrast, the results in Figure 12 demonstrate CO yields that approached the equilibrium CO yield and suggest long-term thermal stability.The favorable results reported here can probably be attributed to Cu being used as a CuNi alloy catalyst. The Ni component is most likely responsible for the thermal stability. Other research has also shown that Ni can stabilize Cu when both metals were deposited on carbon. Specifically, a 16-hour stability period was demonstrated with a Cu50Ni50/C catalyst [24]. The 100% selectivity to CO may be attributed to the CuNi alloy surface having a much greater concentration of Cu than the bulk CuNi alloy. A large surface concentration of Cu diminishes the tendency for CH4 to be formed on Ni.All of the results reported here were obtained at small partial pressures of hydrogen. The experiments performed at H2 partial pressures of 2 kPa and greater showed (with the CO2 partial pressure constant at 2 kPa) that CH4 was formed and that 100% selectivity to CO was not obtained. There may be merit in performing future experiments at greater hydrogen partial pressures with CuNi alloy catalysts that have larger Cu/Ni ratios than the one used in this investigation, since it is known [24] that the surface Cu/Ni ratio increases nonlinearly with the bulk Cu/Ni ratio.


## 4. Summary and Conclusion

Cu50Ni50 nanoparticles were successfully synthesized using a modified polyol method that caused both copper and nickel compounds to be reduced simultaneously and thereby form CuNi alloy nanoparticles. CO yields with Pt/SDC catalysts equaled equilibrium CO yields at 650 and 700°C. In contrast CO yields with Cu50Ni50/SDC catalysts were about 90% of the equilibrium CO yields at 650 and 700°C. Catalysts with YSZ supports had CO yields that were approximately 55% of the CO yields obtained with catalysts having SDC supports.The catalyst selectivity to CO was essentially 100% for the experiments performed at a hydrogen partial pressure of 1 kPa. That may have been caused in part by the Cu content of the catalyst surface being substantially greater than that in the bulk catalyst. The reaction results were explained using a combination of Eley-Rideal and Langmuir-Hinshelwood mechanisms that involved adsorption on the metal surface and the concentration of oxygen vacancies in the support. Finally the Cu50Ni50/SDC catalyst was found to be thermally stable for 48 hours at 650/700°C.Because the costs of Cu and Ni are substantially less than that of Pt and because the performance of the Cu50Ni50/SDC catalysts approached the performance of Pt/SDC catalysts more extensive testing of supported CuNi catalysts is warranted.



---

*Source: 601709-2015-02-17.xml*