Qiang
Dong
*,
Shu
Yin
,
Chongshen
Guo
,
Takeshi
Kimura
and
Tsugio
Sato
Institute of Multidisciplinary Research for Advanced Materials, Tohoku University, 2-1-1 Katahira, Aoba-ku Sendai 980-8577, Japan. E-mail: dong@tagen.tohoku.ac.jp; Fax: +81-22-217-5598; Tel: +81-22-217-5599
First published on 18th October 2012
A facile hydrothermal synthesis of tin doped ceria-zirconia (Ce0.5Zr0.43Sn0.07O2) solid solutions was carried out using Ce(NH4)2(NO3)6, Zr(NO3)3·2H2O and SnCl4·5H2O as the starting materials. The synthesized Ce0.5Zr0.43Sn0.07O2 particles were characterized for their oxygen storage capacity (OSC) for automotive catalysis applications. For the characterization, X-ray diffraction, transmission electron microscopy and the Brunauer-Emmet-Teller (BET) technique were employed. The OSC values of all samples were measured using thermogravimetric-differential thermal analysis. Ce0.5Zr0.43Sn0.07O2 solid solutions with a BET surface area of 246 m2 g−1 exhibited a considerably high OSC of 1425 μmol-O g−1. The incorporation of tin ions in the lattice of the ceria based catalyst greatly enhanced the thermal stability and OSC. The influence of cation radius on the thermal stability and OSC was also discussed.
The redox property of CeO2 can be greatly enhanced by incorporating zirconium ions (Zr4+) into the lattice to form a solid solution.9–11 Nagai et al. have suggested that enhancing the homogeneity of Ce and Zr atoms in the CeO2–ZrO2 solid solutions can improve the OSC performance.12 The detailed structure and property of CeO2–ZrO2 solid solutions were reported in review article by Monte and Kašpar.7 This review included the results of reducing performance for a series of samples with gradually elevated Ce contents, and a possible mechanism of structural changes in the reducing process was proposed. Fornasiero et al. have reported that an optimum composition, like Ce0.5Zr0.5O2 (molar ratio of Ce:Zr = 1:1) can exist as a cubic phase, which can have a considerably high redox property.13 Using density functional theory, Wang et al. found that in a series of Ce1−xZrxO2 solutions with a content of 50% ZrO2 possess the lowest formation energy of the O vacancy, therefore, Ce0.5Zr0.5O2 exhibits the best OSC performance.14 Recently, many researchers have paid a lot of attention to preparing Ce0.5Zr0.5O2 solutions with a homogeneous composition, good dispersion of particles, narrow particle size distribution, better crystallinity and high surface area in order to improve OSC and redox properties for catalytic applications.15–20
Although Ce0.5Zr0.5O2 solid solutions have been studied extensively, there are few reports on the preparation of Ce0.5Zr0.5−xMxO2 in the literature. SnO2 has been widely used as an oxidation catalyst as it can reversibly undergo the Sn4+ ⇔ Sn2+ reaction at relatively lower temperatures.21,22 Sasikala et al. have reported the preparation of Ce1−xSnxO2 by a co-precipitation method and they observed low surface area for the as-prepared Ce1−xSnxO2 with low oxidation/reduction temperature.22 Through a single step solution combustion method using tin oxalate precursor, Ce1−xSnxO2 solid solutions have been prepared, which show high oxygen storage capacity compared to Ce1−xZrxO2, however, the Ce0.8Sn0.2O2 solid solution is only stable up to 700 °C in air.23 Considering the smaller cation radius (eight-coordination) of Sn4+ (0.081 nm) than those of Zr4+ (0.084 nm) and Ce4+ (0.097 nm),24 the incorporation of Sn4+ into Ce–Zr solid solutions may enhance the oxygen release reaction to form larger Ce3+.25 In the present work, we describe the preparation and characterization of Ce0.5Zr0.43Sn0.07O2 solid solutions with high surface area via a facile hydrothermal route. Further experimental results show that introducing tin ions enhances the thermal stability and OSC even after calcination at 1000 °C for 20 h. The OSC of CeO2 and Ce0.5Zr0.5O2 prepared via the same method is compared.
Fig. 1 XRD patterns of fresh samples (a) CeO2, (b) Ce0.5Zr0.5O2, (c) Ce0.5Zr0.43Sn0.07O2, and calcined samples (a′) CeO2, (b′) Ce0.5Zr0.5O2 and (c′) Ce0.5Zr0.43Sn0.07O2. |
The morphology and size of the fresh and calcined samples (1000 °C for 20 h) were observed by TEM as shown in Fig. 2. For fresh samples, the particles seem to be partly dispersed and formed small agglomerates (Fig. 2(a)–(c)), and single particles exhibited a spherical-like morphology with diameters of 9–12 nm, 5–8 nm and 3–5 nm for CeO2, Ce0.5Zr0.5O2 and Ce0.5Zr0.43Sn0.07O2, respectively, which are in agreement with the crystallite size calculated from Scherer's formula. The particle size increased after calcination at 1000 °C for 20 h because of aggregation, and the particle sizes were found to increase to 90–100 nm, 50–55 nm and 30–35 nm for the CeO2, Ce0.5Zr0.5O2 and Ce0.5Zr0.43Sn0.07O2 samples as shown in Fig. 2(a′)–(c′), respectively.
Fig. 2 TEM images of fresh samples (a) CeO2, (b) Ce0.5Zr0.5O2, (c) Ce0.5Zr0.43Sn0.07O2, and calcined samples (a′) CeO2, (b′) Ce0.5Zr0.5O2 and (c′) Ce0.5Zr0.43Sn0.07O2. |
BET nitrogen adsorption-desorption analysis was undertaken to measure the specific surface area of all samples. As a result, the fresh sample of Ce0.5Zr0.43Sn0.07O2 showed much higher surface area (246 m2 g−1) than that of CeO2 (119 m2 g−1) and Ce0.5Zr0.5O2 (168 m2 g−1, Fig. 3(a)–(c)). After calcination at 1000 °C for 20 h in air the specific surface areas of CeO2 (3 m2 g−1) and Ce0.5Zr0.5O2 (8 m2 g−1) decreased to less than 10 m2 g−1, but the sample of Ce0.5Zr0.43Sn0.07O2 exhibited a relatively high BET specific surface area of 24 m2 g−1 (Fig. 3(a′)–(c′)).
Fig. 3 BET specific surface areas of fresh samples (a) CeO2, (b) Ce0.5Zr0.5O2, (c) Ce0.5Zr0.43Sn0.07O2, and calcined samples (a′) CeO2, (b′) Ce0.5Zr0.5O2 and (c′) Ce0.5Zr0.43Sn0.07O2. |
The OSC values of fresh samples and the calcined samples were determined at 600 °C with a continuous flow of H2–N2 gas and air alternately.26,27Fig. 4 shows the typical TG profiles of the CeO2, Ce0.5Zr0.5O2 and Ce0.5Zr0.43Sn0.07O2 samples. The TG profile shows the oxygen release/storage performance of the CeO2, Ce0.5Zr0.5O2 and Ce0.5Zr0.43Sn0.07O2 samples at 600 °C with time. As a result, Ce0.5Zr0.43Sn0.07O2 exhibited the higher OSC of 1425 μmol-O g−1, when compared to that of CeO2 (84 μmol-O g−1) and Ce0.5Zr0.5O2 (721 μmol-O g−1) sample (Table 1). It is accepted that the OSC is dependent on the specific surface area, it is obvious that Ce0.5Zr0.43Sn0.07O2 exhibited the highest specific surface area and highest OSC values. Considering platinum pan was used in TG-DTA, the pan could not contribute to OSC even at high temperatures. Therefore, the highest OSC value of 1425 μmol-O g−1 is close to the theoretical maximum value of OSC (1710 μmol-O g−1).
Fig. 4 TG profiles of fresh and calcined samples (1000 °C, 20 h) at 600 °C, which show oxygen release/storage properties. Fresh samples: (a) CeO2, (b) Ce0.5Zr0.5O2 and (c) Ce0.5Zr0.43Sn0.07O2. Calcined samples: (a′) CeO2, (b′) Ce0.5Zr0.5O2 and (c′) Ce0.5Zr0.43Sn0.07O2. |
Chemical composition | OSC of fresh samples (μmol-O g−1) | OSC of calcined samples (μmol-O g−1) |
---|---|---|
CeO2 | 84 | 13 |
Ce0.5Zr0.5O2 | 721 | 449 |
Ce0.5Zr0.43Sn0.07O2 | 1425 | 1067 |
Ce0.5Zr0.4Ti0.1O2 | 906 | 339 |
Ce0.5Zr0.4Fe0.05Nb0.05O2 | 1112 | 654 |
The OSC of the CeO2, Ce0.5Zr0.5O2 and Ce0.5Zr0.43Sn0.07O2 samples decreased after calcination at 1000 °C for 20 h to 13 μmol-O g−1, 449 μmol-O g−1 and 1067 μmol-O g−1 (Table 1), respectively. The decrease in OSC is due to the increase in particle size and decrease in BET surface area because of the sustained high temperature calcination. In order to examine the OSC performance and stability, oxygen release/storage cycles were measured, and Ce0.5Zr0.43Sn0.07O2 retained the same OSC value and the specific surface area (23 m2 g−1) even after 118 cycles (Fig. S1†). These results indicate that Ce0.5Zr0.43Sn0.07O2 has good OSC performance stability. Moreover, compared with Fig. 2(c) and (c′), the size increased to 9–12 nm for the fresh samples of Ce0.5Zr0.43Sn0.07O2 (Fig. S2(a)†), however, calcined samples (1000 °C for 20 h) kept almost the same morphology and size after treating at 600 °C for 20 h (Fig. S2(b)†).
Recently, incorporating tin into CeO2 has been reported to improve the redox property and oxygen storage capacity at low temperatures.28–30 As the cation radius of Sn4+ (0.077 nm) is smaller than both of Zr4+ (0.084 nm) and Ce4+ (0.097 nm), the incorporation of Sn4+ into Ce–Zr solid solutions may enhance the oxygen release reaction to form larger Ce3+. In the present work, higher surface area is exhibited by Ce0.5Zr0.43Sn0.07O2 solid solutions both before calcination and after calcination compared with Ce0.5Zr0.5O2. The experimental results show that the incorporation of tin ions into Ce–Zr solid solutions also enhances the thermal stability. The Ce0.5Zr0.43Sn0.07O2 solid solutions show considerably higher oxygen storage capacity than Ce0.5Zr0.5O2. The enhanced OSC is not only due to the high surface area but also due to the involvement of Ce4+/Ce3+ and Sn4+/Sn2+ redox couples utilized for H2 oxidation.23 It is proposed that SnO2, being easily reducible, gives out its lattice oxygen for the oxidation reaction, which possibly gets rejuvenated by subtracting oxygen from the adjacent CeO2 molecules.22
Other cations, such as Fe3+ (0.078 nm), Nb5+ (0.074 nm) and Ti4+ (0.074 nm), whose radii are also smaller than both of Zr4+ and Ce4+,24 could also enhance the OSC by incorporating into Ce–Zr solid solutions as shown in Fig. 5 and Table 1. Nb has a similar cation radius to that of Fe. It is better to balance the valency by adding Nb compared to the case of Fe3+ only. It is accepted that Fe3+ might be obtained under hydrothermal treatment conditions, because usually hydrothermal reactions provide an oxidative environment.31,32 The relationship between OSC and cation radius is summarized in Fig. 6. It is indicated that incorporating cation with the radius from 0.074 to 0.084 nm into Ce–Zr solid solutions could enhance the OSC. The OSC (Fig. 5) can be greatly improved by incorporating Sn4+ compared to other cations such as Ti4+, Nb5+ and Fe3+. It was found that the samples incorporating Ti4+, Nb5+ and Fe3+ caused phase separation after calcination at 1000 °C for 20 h as shown in Fig. 7, which resulted in low thermal stability. It was indicated that these cations are too small to stabilize the fluorite structure of Ce–Zr solid solutions. The fresh samples exhibited high specific surface areas, however, they decreased to less than 10 m2 g−1 after calcination as shown in Fig. 8. Therefore, the radius of the incorporated cation might be an important factor which affects thermal stability.
Fig. 5 TG profiles after measuring the OSC at 600 °C for fresh and calcined samples (1000 °C, 20 h), which show oxygen release/storage properties. Fresh samples: (a) Ce0.5Zr0.4Ti0.1O2 and (b) Ce0.5Zr0.4Fe0.05Nb0.05O2. Calcined samples: (a′) Ce0.5Zr0.4Ti0.1O2 and (b′) Ce0.5Zr0.4Fe0.05Nb0.05O2. |
Fig. 6 The relationship between OSC and incorporating cation radius. For fresh samples: (a) CeO2, (b) Ce0.5Zr0.5O2, (c) Ce0.5Zr0.43Sn0.07O2, (d) Ce0.5Zr0.4Fe0.05Nb0.05O2 and (e) Ce0.5Zr0.4Ti0.1O2. For calcined samples: (a′) CeO2, (b′) Ce0.5Zr0.5O2, (c′) Ce0.5Zr0.43Sn0.07O2, (d′) Ce0.5Zr0.4Fe0.05Nb0.05O2 and (e′) Ce0.5Zr0.4Ti0.1O2. |
Fig. 7 XRD patterns of fresh samples (a) Ce0.5Zr0.4Ti0.1O2 and (b) Ce0.5Zr0.4 Fe0.05Nb0.05O2, and calcined samples (a′) Ce0.5Zr0.4Ti0.1O2 and (b′) Ce0.5Zr0.4 Fe0.05Nb0.05O2. |
Fig. 8 BET specific surface areas of fresh samples (a) Ce0.5Zr0.4Ti0.1O2 and (b) Ce0.5Zr0.4Fe0.05Nb0.05O2, and calcined samples (a′) Ce0.5Zr0.4Ti0.1O2 and (b′) Ce0.5Zr0.4Fe0.05Nb0.05O2. |
Footnote |
† Electronic supplementary information (ESI) available: See DOI: 10.1039/c2ra21766j |
This journal is © The Royal Society of Chemistry 2012 |