Li Yanga,
Guobin Lia,
Gewu Gaoa,
Ruile Xua,
Shuwei Zhua,
Xinqian Shu*a,
Sujian Wangb,
Zengshe Dengb and
Peng Wangb
aSchool of Chemical & Environmental Engineering, China University of Mining & Technology, Beijing 100083, China. E-mail: sxq@cumtb.edu.cn; Fax: +86-01062331853; Tel: +86-01062331853
bShaanxi Coal and Chemical Industry Group Company, Xi'an, 710065, China
First published on 13th November 2017
The influence mechanism of SO2 on the NOx removal performance of a La0.9Sr0.1Mn0.97Pd0.03O3 catalyst was investigated in this paper using X-ray diffraction, scanning electron microscopy, Fourier transform infrared spectroscopy, and the transient response method. Results show that incorporating the noble metal Pd into the catalyst increases the specific surface area of the original catalyst, creating a suitable place for NOx contact, reducing the ignition temperature of soot and improving the NOx, C3H6 and CO conversion of the catalyst effectively. Although the catalyst La0.9Sr0.1Mn0.97Pd0.03O3 forms a stable and irreversible sulphate after reacting in a high concentration of SO2 (300 ppm) atmosphere, it retains a high removal efficiency of NOx.
Perovskite-type compounds have numerous advantages, such as oxygen vacancy and good thermal conductivity, as well as B-valence ions, which have the advantages of the mixed and abnormal valence states while maintaining the structure. In addition, perovskite-type compounds have a certain conversion capacity of NO under lean-burn conditions. Therefore, the perovskite-type material is expected to become the new generation of automotive exhaust gas purification catalyst.3
At present, four-way combination catalysis has numerous problems, such as high running cost, complicated structure, and substantially occupied space. For example, the catalyst used for soot-NOx oxidation and reduction has low NOx conversion rate, poor selectivity, sulfur poisoning, and other issues.4–6
Mn has a variable d electronic structure and a variety of valence state, which shows good redox properties. La has a large atomic radius and high thermal stability. Therefore, LaMnO3 is a high-temperature stable redox catalyst that has been applied in numerous fields, such as fuel cells, gas sensors, magnetic structures, hydrocarbon oxidation combustion, and so on.7–12 The Mn4+ and oxygen vacancies appear in the La1−xSrxMnO3 system after doping Sr2+ ions at the A-site of LaMnO3. Therefore, the metal oxide catalyst of perovskite-type composite has excellent catalytic activity. The results show that the addition of a small amount of noble metal in the perovskite catalyst can improve the catalytic activity of the sample. The perovskite-type oxide catalyst with a small amount of noble metal Pd has higher catalytic activity even in high-temperature water vapor, as well as sulfide exhaust, which can also possess high catalytic performance for a long period of time.13–15 Our (La1−xSrxMn1−yPdyO3) catalyst has simultaneously excellent redox properties with the alkaline storage centers Sr and catalytically active centers Pd, thereby creating a promising four-way catalyst.
Temperature programmed reaction was conducted with a GSVH of 20000 h−1. The catalysts were directly exposed to reaction gas containing NO (0.1%), C3H6 (0.05%), CO (0.5%), O2 (10%) and SO2 (300 ppm). The composition of the gas mixture produced from the reaction was analyzed by the online A5000 model gas chromatograph.
The ignition temperature of soot (Tig) and the conversion rate of polluted gas (XNO, XCO, XC3H6) were used as the evaluation index of the activity of the catalyst. In the reaction process, the conversion rate of the reaction gas is calculated by the following formula:
![]() | (1) |
![]() | (2) |
![]() | (3) |
![]() | (4) |
![]() | ||
Fig. 1 XRD of the catalyst and its amplification (right) map (a) La0.9Sr0.1MnO3; (b) La0.9Sr0.1Mn0.97Pd0.03O3. |
Doping Pd to the perovskite structure shifted the diffraction peaks to a small angle. When the Mn4+ is replaced by Pd2+, the size of the perovskite cell increased and the diffraction peak position shifted to a small angle because the ionic radius of Pd2+ (0.64 Å) is larger than Mn4+(0.39 Å). The change of unit cell parameters before and after doping is shown in Table 1. After doping, the lattice parameters a, b and c of the crystallite increase and the specific surface area is increased from 8.72 m2 g−1 to 11.04 m2 g−1, which may be related to the distortion of the crystal.16
Composition | Cell parameters (Å) | BET (m2 g−1) | |||
---|---|---|---|---|---|
a | b | c | d | ||
La0.9Sr0.1MnO3 | 5.48 | 3.83 | 9.84 | 109 | 8.72 |
La0.9Sr0.1Pd0.97Mn0.03O3 | 5.55 | 5.43 | 10.12 | 164 | 11.04 |
Fig. 2A and B are SEM photographs of La0.9Sr0.1MnO3 and La0.9Sr0.1Mn0.97Pd0.03O3, respectively, catalyst magnified 5000 times.
The figure shows that the La0.9Sr0.1MnO3 catalyst particles are stacked together like a structure of flocculent, which may be attributed to insufficient uniform dispersion. The scale of La0.9Sr0.1Mn0.97Pd0.03O3 catalyst particles doped with Pd became significantly smaller and the particle size distribution is uniform. Due to the high temperature calcination, the surface of the sample is sintered and some of the channels collapsed together, resulting in a lot of irregular voids. The formation of the pore became abundant, which is conducive to increasing the surface area of the catalyst and further promoting the contact and adsorption effect with pollutants. The conclusion is consistent with the results of the specific surface area been shown in Table 1.
Pd–NO + Pd–O → Pd–NO2 + Pd | (5) |
SrCO3 + 2NO3 → Sr(NO3)2 + CO2 + O2− | (6) |
SrO + 2NO3 → Sr(NO3)2 + O2− | (7) |
![]() | ||
Fig. 3 Comparison of CO, C3H6 and NO conversion before and after Pd doping (a) La0.9Sr0.1MnO3; (b) La0.9Sr0.1Mn0.97Pd0.03O3. |
In summary, the doping of noble metal Pd can effectively improve the performance of the catalyst activation.
Fig. 5 shows the results of the mixture experiment FTIR over La0.9Sr0.1Mn0.97Pd0.03O3 catalyst. Fig. 5 also shows spectral patterns exhibiting peaks at approximately 1624 cm−1, which are assigned to the deformation vibration and stretching vibration of O–H bonds of the adsorbed water. 848 cm−1 and 1468 cm−1 correspond to the characteristic peak of carbonate. In addition, after SO2-containing gases test the minor absorption associated with nitrate species (broad at 1396 cm−1 due to ionic nitrates) and ionic nitrites (1207 cm−1) are evident. This minor absorption can be attributed to the formation of nitrates by NOx adsorbed on the carbonate surface, which corresponds to the transformation from strontium carbonate to strontium nitrate. The characteristic peaks of carbonates disappeared after the SO2-containing gases test and the free ionic nitrates appeared, thereby indicating that the NOx was stored on the carbonate of the catalyst surface. 1128 cm−1 is the characteristic peak of the bulk sulfate species, and the samples after SO2-containing gases test showed a weak vibration peak of sulfate. The absorption peak at 621 cm−1 is the characteristic vibration peak of the perovskite structure. The results show that the perovskite structure of the prepared catalyst is well, and the structure of the sample remained well after the mixed gas experiment. This indicates that SO2 has a slight effect on the structure of the catalyst, which is similarly to the previous XRD results.
Fig. 6 displays the corresponding conversion-temperature profiles of the La0.9Sr0.1Mn0.97Pd0.03O3 catalyst during the SO2-containing gases and non-SO2 gases test. The figure reveals that the with the increase of T, the conversion rate of NO at the low temperature range (100–200 °C) is increased and the yield of NO2 is correspondingly increased, but the yield of N2 does not change too much. The results indicating that the oxidation of NO to NO2 occurs mainly at low temperature range and NO2 stored in the catalyst in the form of nitrate, corresponding to the previous FT-IR results. When the temperature continues rise, the yield of NO2 decreased while the N2 begin to increase, indicating that the NOx reduced to N2 by reducing gas (CO, C3H6). Meanwhile it can be seen that SO2 has little effect on the oxidation reaction of NO–NO2, but it has some influence on the reduction of NOx during the mixture gas test. A competitive adsorption of the SO2 and NOx on the surface of the catalysts occurs which may probably be due to the NO2 storage stage. The sulfate is more stable than the nitrate and the SO2 is occupied by the mixed gas atmosphere containing SO2 because the (p–d) π bond in the sulfate structure is more stable than the delocalized π-bond in the nitrate, resulting in a decrease in the storage capacity of the catalyst for NOx. The result affects the effective progress of the catalyst reduction reaction.
Fig. 7 illustrates different effects of SO2 concentration on the N2 yield and the CO removal rates of the catalyst (La0.9Sr0.1Mn0.97Pd0.03O3), respectively. The figures show the catalyst La0.9Sr0.1Mn0.97Pd0.03O3 has a high catalytic activity without the presence of SO2, 303 °C, the removal rate of CO which has reached more than 80%, the yields of N2 were up to 87%. When the SO2 concentration is lower than 200 ppm, the denitration efficiency of the catalyst has a slight effect. When SO2 concentrations are up to 300 ppm, the catalytic activity significantly decreased. At a temperature of 303 °C, the highest removal rate of CO is only 27%, and the highest conversion rate of C3H6 is 78%. In addition, the soot ignition temperature is 368 °C, which is 15% higher than that of non-SO2 312 °C, indicating that the catalyst possesses some resistance on low concentrations of SO2. SO2 with high concentrations will obviously inhibit the catalytic activity of La0.9Sr0.1Mn0.97Pd0.03O3. When the concentration of sulfur is higher, the storage capacity of NOx is lower, resulting in catalyst poisoning.
This journal is © The Royal Society of Chemistry 2017 |