Next Article in Journal
Catalytic Copyrolysis of Cork Oak and Waste Plastic Films over HBeta
Previous Article in Journal
Photocatalytic Water Disinfection under Solar Irradiation by d-Glucose-Modified Titania
Previous Article in Special Issue
Plasma-Catalytic Mineralization of Toluene Adsorbed on CeO2
Article Menu
Issue 8 (August) cover image

Export Article

Catalysts 2018, 8(8), 317; doi:10.3390/catal8080317

Plasma Oxidation of H2S over Non-stoichiometric LaxMnO3 Perovskite Catalysts in a Dielectric Barrier Discharge Reactor
1,2,3,* , 2
Faculty of Maritime and Transportation, Ningbo University, Ningbo 315211, China
State Key Laboratory of Clean Energy Utilization, Zhejiang University, Hangzhou 310027, China
Department of Electrical Engineering and Electronics, University of Liverpool, Liverpool L69 3GJ, UK
Authors to whom correspondence should be addressed.
Received: 12 July 2018 / Accepted: 23 July 2018 / Published: 2 August 2018


In this work, plasma-catalytic removal of H2S over LaxMnO3 (x = 0.90, 0.95, 1, 1.05 and 1.10) has been studied in a coaxial dielectric barrier discharge (DBD) reactor. The non-stoichiometric effect of the LaxMnO3 catalysts on the removal of H2S and sulfur balance in the plasma-catalytic process has been investigated as a function of specific energy density (SED). The integration of the plasma with the LaxMnO3 catalysts significantly enhanced the reaction performance compared to the process using plasma alone. The highest H2S removal of 96.4% and sulfur balance of 90.5% were achieved over the La0.90MnO3 catalyst, while the major products included SO2 and SO3. The missing sulfur could be ascribed to the sulfur deposited on the catalyst surfaces. The non-stoichiometric LaxMnO3 catalyst exhibited larger specific surface areas and smaller crystallite sizes compared to the LaMnO3 catalyst. The non-stoichiometric effect changed their redox properties as the decreased La/Mn ratio favored the transformation of Mn3+ to Mn4+, which contributed to the generation of oxygen vacancies on the catalyst surfaces. The XPS and H2-TPR results confirmed that the Mn-rich catalysts showed the higher relative concentration of surface adsorbed oxygen (Oads) and lower reduction temperature compared to LaMnO3 catalyst. The reaction performance of the plasma-catalytic oxidation of H2S is closely related to the relative concentration of Oads formed on the catalyst surfaces and the reducibility of the catalysts.
plasmas-catalysis; non-thermal plasmas; perovskite catalysts; nonstoichiometry; H2S oxidation

1. Introduction

The emission of odors from various sources including wastewater treatment and municipal solid waste (MSW) treatment facilities have become a public concern due to their negative effect on air quality and human health, especially on sensitive or sick people [1]. As a result, air quality control in the waste treatment facilities is important to ensure a comfortable environment for the workers and local residents. Great efforts have been devoted to the research and development of odor abatement technologies including wet scrubbing, active carbon adsorption, incineration and biofiltration, etc. [2,3,4]. However, these technologies are not cost-effective when dealing with low concentrations of odors in high-volume waste gas streams. For example, biological treatment is not flexible for the variation of odor loadings and volume of waste gas streams [5].
Recently, non-thermal plasma (NTP) has been regarded as a promising alternative for deodorization due to its unique characteristics of fast reaction, compact system and adaptability towards complex working conditions [6,7]. Typically, air plasma could generate electrons and various chemically reactive species, which could react with the odor molecules, leading to the purification of the odor-containing waste gas streams. Anderson et al. performed an on-site test of a pilot scale plasma reactor to purify a 138 m3·h−1 odor-containing waste gas stream with the main compositions of acetic acid, propanoic acid, trimethylamine and indole, etc. The average odor removal efficiency of 97% could be achieved at an input power of 140.8 W [8]. Kuwahara et al. developed a dielectric barrier discharge (DBD) reactor with a laminated film-electrode for odor control, while the complete removal of 100 ppm odor was achieved at a discharge power of 10 W and a flow rate of 5 L·min−1 [9]. Lu et al. reported the decomposition of ammonia and hydrogen sulfide with self-designed gliding arc plasma reactor, while a removal efficiency of 100% was achieved at the applied voltage of 11 kV and the velocity of 4.72 m·s−1 [10]. Some researcher also performed scale-up studies of plasma technologies in odor control [11]. Dobslaw et al. performed a 35-day-long scale-up test of plasma odor removal in two industrial sites in Germany, while the odor concentration was significantly reduced by 95.9–98.3% [12]. They also used the scale-up plasma units to enhance the performance of a biotrickling filter, the odor removal efficiency of using plasma alone reached up to 93.9% [13]. However, the relative low selectivity towards the desired final products in the NTP process remains the main challenge for the use of NTP-based technologies in environmental clean-up.
In the last three decades, the combination of non-thermal plasma and heterogeneous catalysis, known as “plasma-catalysis” has been demonstrated as a promising emerging process for the removal of low concentration gas pollutants including odors with reduced formation of by-products and enhanced process performance [14,15,16,17]. Although LaMnO3 perovskite type catalysts have been used in thermal catalytic reactions due to their relatively low cost, comparable activity, and thermal stability [18,19,20], the use of these catalysts in plasma chemical reactions for environmental clean-up or the synthesis of fuels and chemicals has been very limited. Hueso et al. found that the combination of lanthanum based perovskite catalysts and a microwave discharge plasma enhanced the conversion of low concentration methane (3600 ppm) by around 30% compared to the plasma process in the absence of a catalyst at a same energy density of 10 W·m−2 [21,22]. Vandenbroucke et al. reported that the removal of trichloroethylene was increased by 13.9% when packing a Pd/LaMnO3 catalyst into a negative DC corona discharge reactor at a specific energy density (SED) of 460 J·L−1 compared to the plasma reaction without a catalyst. They also found that the coupling of the plasma-catalyst coupling significantly reduced the formation of major by-product CHCl3 [23]. It is well recognized that the substitution of A and B sites of the perovskite catalysts could result in a structural non-stoichiometry, which might generate excess oxygen species on the catalyst surfaces and consequently affect the reaction performance [24]. To the best of our knowledge, the use of perovskite catalysts in plasma-catalytic odor control has not been reported yet, while the knowledge about the underlying mechanisms of the non-stoichiometric effect of the perovskite catalyst on the plasma-catalytic oxidation processes are still missing.
In this work, hydrogen sulfide (H2S) is chosen as a model pollutant since it accounts for over 90% of the total mass concentration in the odor emissions [25]. The non-stoichiometric effect of LaxMnO3 catalysts on the plasma-catalytic removal of low concentration H2S was investigated in a DBD plasma reactor in terms of the removal of H2S and sulfur balance. The physicochemical properties of the catalysts were determined using various characterization techniques, including Brunauer-Emmett-Teller (BET) surface measurement, X-ray diffraction (XRD), X-ray photoelectron spectroscopy (XPS) and temperature programmed reduction of H2 (H2-TPR) to understand the structure-activity relationships between the LaxMnO3 catalysts and the plasma-catalytic process and the role of these catalysts in the plasma-catalytic process.

2. Results and Discussions

2.1. Physicochemical Properties of the Catalysts

Table 1 show the results of N2 adsorption-desorption experiments. The non-stoichiometric effect of the LaxMnO3 catalysts enlarged the specific surface areas (SBET) by 5.7% to 23.5% compared to that of the LaMnO3 catalyst (12.3 m2·g−1), while the La0.9MnO3 catalyst had the highest SBET. Figure 1 shows the XRD patterns of the LaxMnO3 catalysts. The formation of the perovskite phase was observed in all the catalysts and no obvious segregated phases of La2O3 and MnOx were found. The stoichiometric LaMnO3 catalyst exhibited a typical cubic perovskite structure (JCPDS 75-0440) of LaMnO3. The cubic structure of the LaxMnO3 catalysts remained unchanged when the La doping amount was decreased, while the orthorhombic structure of LaMnO3 (JCPDS 89-2470) was observed for the La-rich catalysts (x > 1). According to Table 1, the cell volume of the LaxMnO3 catalysts increased with the increase of La/Mn molar ratio. The expansion of unit cell could be attributed to the transformation of Mn4+ into Mn3+ and the incorporation of La3+ into the perovskite lattice of LaxMnO3 considering the larger ion radius of La3+ (1.06 Å) and Mn3+ (0.65 Å) compared to that of Mn4+ (0.54 Å). The characteristic diffraction peak of LaMnO3 (1 2 1) located at around 32.6° was slightly shifted to a lower 2θ value for the La-rich catalysts, while this peak in the XRD pattern of the Mn-rich catalysts (x < 1) was shifted to a higher 2θ value [26]. The non-stoichiometric catalysts had a smaller crystallite size compared to the LaMnO3 catalyst (16.1 nm), while the La0.90MnO3 catalyst had the smallest crystallite size of 15.4 nm.

2.2. Redox Properties of the Catalysts

The chemical states of major elements (Mn 2p and O 1s) in the LaxMnO3 catalysts were examined using XPS, as shown in Figure 2. The binding energies of La 3d5/2 (838.1 eV and 855.0 eV) were observed for all the catalysts (not shown), while those of La 3d3/2 were located at around 834.8 eV and 851.5 eV. The binding energies and the spin-orbit splitting of La 3d were close to those of pure La2O3, indicating that the lanthanum ions were in trivalent state of the LaxMnO3 catalysts [27].
Figure 2a shows the XPS spectra of Mn 2p3/2 of the LaxMnO3 catalysts. The co-existence of Mn2+, Mn3+ and Mn4+ species in the LaMnO3-based perovskite catalysts has been reported [28]. However, in this work, Mn2+ species were unlikely existed due to the missing satellite peaks at around 648.8 eV [29]. The XPS signals of Mn 2p3/2 can be deconvoluted into two major peaks. The XPS peaks at 641.6 eV were assigned to the generation of Mn3+ cations, while the peaks at around 643.0 eV was associated to the formation of Mn4+ cations. The relative concentration of Mn4+ in the LaxMnO3 catalysts, defined as Mn4+/(Mn3++Mn4+), was calculated based on the deconvoluted peaks (Table 1). The relative concentration of Mn4+ of these catalysts varied from 38.2% to 43.2%, and the La0.90MnO3 catalyst showed the highest value of 43.2%. The relative Mn4+ concentration of the catalysts decreased with the increase of nominal La/Mn molar ratio.
The deconvoluted O 1s spectra of the LaxMnO3 perovskites suggested the coexistence of various oxygen species on the catalyst surface (Figure 2b). The peaks located at around 532.9 eV, 531.2 eV and 529.4 eV could be attributed to the formation of oxygen-containing groups: hydroxyl/carbonate species, surface adsorbed oxygen (Oads) and lattice oxygen (Olat), respectively [30]. The non-stoichiometric effect did not significantly change the binding energy of these three major oxygen species. Table 1 presents the relative concentration of Oads of the catalysts, defined as Oads/(Oads + Olat). The La0.90MnO3 catalyst showed the highest relative Oads concentration of 60.7%, while the relative concentration of Oads of the catalysts decreased with the increase of nominal La/Mn molar ratio. Note that the variation of Oads/(Oads + Olat) with the La/Mn molar ratio followed the same trend as Mn4+/(Mn3+ + Mn4+).
The reducibility of the LaxMnO3 catalysts was analyzed using H2-TPR experiment (Figure 3). For all the LaxMnO3 catalysts, two major reduction peaks were observed. The first broad peak located between 200 °C and 500 °C could be divided into three sub-peaks. The shoulder peak centered between 200 °C and 300 °C could be ascribed to the reduction of weakly adsorbed oxygen species, while the second peak locate at around 350 °C was associated to the reduction of Mn4+ to Mn3+ with concomitant of surface adsorbed oxygen species. The third peak indicated the reduction of Mn3+ with coordination-unsaturated compose, while the peaks at higher temperature (above 600 °C) can be attributed to further reduction of Mn3+ to Mn2+ [27,31]. The lowest reduction temperature of the first broad peaks (335 °C and 392 °C) was observed over the La0.90MnO3 catalyst. Increasing the nominal La/Mn molar ratio slightly shifted the reduction peaks to higher temperatures. For example, the reduction temperatures of the LaMnO3 catalyst were 342 °C and 393 °C, while those for La1.10MnO3 were 351 °C and 401 °C, respectively. This phenomenon indicated stronger interactions between La and Mn species, which inhibited the oxygen mobility on the LaxMnO3 catalysts, and consequently decreased the reducibility of the catalysts.

2.3. Plasma-Catalytic Oxidation of H2S

The effect of the LaxMnO3 catalysts on the removal of H2S and the sulfur balance of the plasma-catalytic process was shown in Figure 4. The removal of H2S increased monotonically with the increasing SED regardless of the presence of the catalysts. In the plasma reaction without a catalyst, the H2S removal increased significantly from 10.7% to 41.5% when increasing the SED from 304.8 J·L−1 to 604.0 J·L−1, while the sulfur balance of the plasma process decreased from 98.2% to 74.3%. The input energy in a typical air plasma is mainly used to generate highly energetic electrons and chemically reactive species, including O, OH·, and nitrogen excited states N2(A), which contributed to the decomposition of the H2S through direct electron-impact dissociation of H2S and radical attack [6]. The dissociation of H2S molecules by electrons with sufficient energy forms H· and SH· radicals [32], while the collision of H2S with radicals (e.g., O and OH·) and excited nitrogen species also takes place in the plasma reaction [33]:
e + H2S → e + H· + SH·
N2(A) + H2S → N2 + H· + SH·
O + H2S → OH· + SH·
OH· + H2S → SH· + H2O
The generated H· radicals could be oxidized to form OH· by the oxidative species and participate the consequent plasma-induced reactions [6]. The SH· radicals were unstable in the oxidative environment and could be reacted with O and OH· radicals to form the major reaction product of SO2:
SH· + O· → SO· + H·
SH· + OH· → SO· + H·
SO· + O· → SO2
SO· + OH· → SO2 + H·
The inner energy of the rotational and vibrational excited species, which were insufficient to break chemical bonds of H2S molecules, could be transferred to the electronically excited species and accelerate the plasma-catalytic reactions [34]. NTP generated by the dielectric barrier discharge reactor consisted of numerous micro-discharges in the plasma region. The number of micro-discharges in each discharge period was increased at a higher SED with fixed gas flow rate, which creates more reaction channels for the decomposition of H2S and intermediates, resulting in the enhanced removal of H2S [35,36,37]. It is worth noting that no ozone was detected in this work, which might be consumed by local heating, catalytic effect, or plasma oxidation reactions [38]. The decreased sulfur balance at a higher SED can be ascribed to the formation of sulfur via: (1) electron impact dissociation of SH· radicals, and (2) disproportionation of SH· radical and recombination between SO2 and H2S [14]:
e + SH· → e + S + H·
SH· + SH· → S + H2S
H2S + SO2 → S + H2O
The oxidation of SO2 to SO3 by highly oxidative species present in a plasma was reported by Jarrige et al. [39]:
SO2 + O· → SO3
SO2 + OH· → SO3 + H·
The presence of the LaxMnO3 catalysts in the plasma region significantly enhanced the removal of H2S and the sulfur balance compared to the plasma processing of H2S without a catalyst. Figure 4 shows that the removal of H2S increased from 34.3% to 91.6% in the plasma reaction over the stoichiometric LaMnO3 when increasing the SED from 303.6 J·L−1 to 573.6 J·L−1, while the sulfur balance of the plasma-catalytic process increased from 59.2% to 87.0% under the same operating conditions. The increase of sulfur balance could be attributed to the enhanced oxidation of solid state sulfur to SO2 at a higher SED, whilst the formation of a small amount of SO3 was also observed. However, the formation of SO3 in the plasma process was relatively low in this work (less than 8%), which was comparable to the results reported by Chang [40] and Kim et al. [41]. The non-stoichiometric effect of the LaxMnO3 catalysts imposes a distinct effect on the plasma-catalytic removal of H2S. Coupling the plasma with the La0.90MnO3 catalyst showed the highest H2S removal of 96.4% and highest sulfur balance of 90.5% at a SED of 593.7 J·L−1. The increase of nominal La/Mn molar ratio inhibited the performance of the plasma-catalytic system for H2S removal. The removal of H2S and the sulfur balance follows the order of La0.90MnO3 > La0.95MnO3 > LaMnO3 > La1.05MnO3 > La1.10MnO3 > NTP in the tested SED range, which is the opposite to the order of La/Mn molar ratio. Part of the missing sulfur element was found on the surface of the spent catalysts by XPS, which was also confirmed by a previous work [14].
Clearly, the LaxMnO3 catalysts played a crucial role in the enhancement of the performance of the plasma-catalytic system. The non-stoichiometric effect slightly increased the specific surface area of the LaxMnO3 catalysts by 3.2 to 20.6% compared to pure LaMnO3 catalyst (12.6 m2·g−1), while the crystalline size of the LaxMnO3 catalysts was decreased by 0.9–9.8% (16.1 nm for the LaMnO3 catalyst). The changes in the specific surface area and crystalline size of the catalysts indicated that the non-stoichiometric effect contributed to the strong interactions between the La and Mn species of the catalysts. Larger specific surface area could offer more adsorption sites and active sites in the plasma-catalytic reaction, which prolonged the residence time of H2S and intermediates in the plasma reaction [42]. Previous study also confirmed that smaller crystallite sizes of the catalysts favored the exposures of active sites on the catalyst surface [43]. To sum up, the changes in the physicochemical properties of the LaxMnO3 catalysts would increase the possibilities of effective collisions between the reactive species and the pollutant including H2S and intermediates, which benefited the reaction performance of the plasma-catalysis system.
The XPS spectra confirmed the coexistence of Mn3+ and Mn4+ cations in the LaxMnO3 catalysts. Charge imbalance may occur in the non-stoichiometric LaxMnO3 regarding the change of the nominal La/Mn molar ratio in the perovskite structure [18,44]. Taking the La0.90MnO3 catalyst as an example, the decrease of La3+ content could form La vacancies in the perovskite lattice. The form of La vacancies could be compensated by the conversion of Mn3+ to Mn4+ to maintain the neutrality, which was evidenced by the production of highest relative concentration of Mn4+ of 43.2% in the La0.90MnO3 catalyst. Similar results were reported for the La-rich samples as more Mn3+ can be generated to maintain the electron neutrality in the presence of excess La cations [45]. The redox cycle between Mn3+ and Mn4+ was closely associated with the redox properties of the catalysts. The value of Mn4+/(Mn3+ + Mn4+) decreased from 43.2% to 38.2% when the La/Mn molar ratio increased from 0.90 to 1.10 in this work. The presence of Mn4+ species was also correlated with the formation of oxygen vacancies on the surface of the LaxMnO3 catalysts [46]. Oxygen vacancies acted as the adsorption-desorption centers for the generation of Oads from gas-phase oxygen species including O2 molecules and O radicals in the plasma process. The oxygen species adsorbed on the oxygen vacancies (Oads) played an important role in the plasma-induced surface reactions for the oxidation of H2S and the intermediates due to the higher mobility of Oads compared to the lattice oxygen (Olat) [47]. Thus, perovskite catalysts with abundant oxygen vacancies were more active for the oxidation of pollutants on the catalyst surface in the plasma region. The La0.90MnO3 catalyst possessed the highest Oads/(Oads + Olat) value of 60.7%, while increasing the nominal La/Mn molar ratio reduced the value to 59.9% for LaMnO3 and 55.2% for La1.10MnO3, respectively. Note the decrease of Oads/(Oads + Olat) at higher La/Mn molar ratio was in line with the decreased Mn4+/(Mn3+ + Mn4+).
The reducibility of the LaxMnO3 catalysts was also significantly affected by the non-stoichiometric effect. Figure 3 shows that the reduction temperatures of the Mn-rich catalysts were much lower compared to the La-rich catalysts and LaMnO3, indicating that on the Mn-rich catalysts had a higher oxygen mobility. As mentioned before, the compensation effect of the insufficient or excess La species could promote or inhibit the formation of oxygen vacancies, which could contribute to the formation of surface adsorbed oxygen (Oads) with higher oxygen mobility and consequently contributes to the enhanced oxidation of the adsorbed H2S and intermediates to the final product of H2O, SO2, sulfur and possibly SO3 in the plasma-catalytic system. It is noteworthy that the order of the reduction temperature of these catalysts was in consistent with the sequence of Oads/(Oads + Olat) and Mn4+/(Mn3+ + Mn4+). Combining the results of XPS and H2-TPR of these catalysts, it is clear that the redox properties of the catalysts play a determining role in the reaction performances of the plasma-catalytic removal of H2S, while the non-stoichiometric effect at higher nominal La/Mn ratio inhibited the removal of H2S in the plasma-catalytic system. The possible reaction mechanisms in the plasma-catalytic oxidation of H2S over the LaxMnO3 catalysts have been summarized in Figure 5.

3. Experimental Setup

3.1. Catalyst Preparation

The non-stoichiometric LaxMnO3 (x = 0.9, 0.95, 1, 1.05 and 1.1) perovskite-type catalysts were synthesized using a citric acid method, while lanthanum nitrate hexahydrate and 50 wt % manganese nitrate solution were used as the precursors [1]. All chemicals were analytic reagent and purchased from Aladdin Co. Ltd. (Shanghai, China) The synthesis procedures of the LaxMnO3 catalysts were: (1) weighted amounts of all precursors and deionized water were mixed to obtain 0.1 M solutions; (2) a 50% excess amount of citric acid (comparing to the total amount of the metal cations) was added to the solution obtained in step 1 as the ligand; (3) the solution was thoroughly stirred for 3 h and evaporated in an 80 °C water bath to form viscous gel; (4) the gel was dried in an oven overnight at 110 °C and then calcined at 700 °C for 5 h; (5) the samples was then pressed and sieved to 35–60 meshes for testing.

3.2. Catalyst Characterizations

The specific surface area, average pore size and pore volume of the LaxMnO3 catalysts were measured using N2 adsorption-desorption experiments (Quantachrome Autosorb-1, Boynton Beach, FL, USA) at 77 K. The LaxMnO3 catalyst samples were degassed at 200 °C for 5 h before each test. The specific surface area (SBET) of the LaxMnO3 catalyst was obtained by the Brunauer-Emmett-Teller (BET) equation.
The X-ray diffraction (XRD) measurements were carried out on a Rikagu D/max-2000 X-ray diffractometer (Tokyo, Japan) using Cu-Kα as the radiation source.
The X-ray photoelectron spectroscopy (XPS) experiments were performed with a Thermo ESCALAB 250 spectrometer (Waltham, MA, USA) using an Al Kα X-ray source (hν = 1486.6 eV). The XPS results were calibrated using the C 1s spectra at a binding energy (B.E.) of 284.6 eV.
The hydrogen temperature-programmed reduction (H2-TPR) were performed using a Micrometrics Autochem II 2920 instrument (Ottawa, ON, Canada). For each test, 50 mg LaxMnO3 catalyst samples were loaded and pretreated at 250 °C in a flowing N2 for 1 h to remove the weakly adsorbed impurities and then cooled down to 50 °C. The samples were then heated from room temperature to 800 °C in a 5 vol % H2/Ar flow (40 mL·min−1). The heating rate was constant at 10 °C·min−1. The H2 consumption was calculated based on the H2-TPR profiles.

3.3. Experimental Set-Up

The schematic experimental set-up is shown in Figure 6. The details of the DBD reactor were described elsewhere [26]. The reactor was co-axial type with the discharge length of 60 mm. The inner diameter of the discharge tube was 8 mm, while the outer diameter was 10 mm. The diameter of the stainless high voltage rod was 2 mm. Thus, the total plasma discharge volume was 2.26 mL. The carrier gas (high-purity air) and H2S was generated from gas cylinders purchased from Jingong, Hangzhou, China. All gas streams were regulated by mass flow controllers and mixed prior to the plasma reactor. The total flow rate was 2 L·min−1, while the initial H2S concentration was 100 ppm. In this work, 100 mg LaxMnO3 catalyst was used in each test. The catalysts was held in place by quartz wool, while only quartz wool was packed in the plasma region in the cases using plasma alone. The reactor was energized by an AC power supply (Suman CTP2000-K, Nanjing, China) and the discharge frequency was fixed at 10 kHz. The temperature at the outer wall of the reactor was measured using an infrared thermometer (Omega OS540, Norwalk, CT, USA). During the experiment process, it gradually increased to approximately 80 °C, while the outlet gas temperature was about 30 °C.
The applied voltage across the plasma-catalytic reactor was measured using a Tektronix 4034B digital oscilloscope connected to a Tektronix 6015A voltage probe (1000:1). An external capacitor was connected in series with the grounded electrode across which the voltage was measured using a TPP500 voltage probe (Tektronix, Beaverton, OR, USA). The average discharge power was calculated by integrating the voltage waveforms by Q-U Lissajous method. The specific energy density (SED) of the plasma-catalysis process can be obtained as:
S E D ( J L 1 ) = P ( W ) Q ( L min 1 ) × 60  
where P is the discharge power of plasma-catalytic process and Q is the total gas flow rate.
H2S was measured by using a PTM-400 H2S analyzer (Yiyuntian, Shenzhen, China) with the measuring range of 0–200 ppm and an accuracy of ±2%, while the concentration of formed SO2 was measured by using a Testo 350XL gas analyzer (Lenzkirch, Germany) with an accuracy of ±5%. The concentration of outlet SO3 was measured using a SO3 analyzer (RJ-SO3-M) (Ruijing Tech., Shenzhen, China) based on the US EPA method 8 (specific IPA absorption method for SO3 measurement). The detection range of the SO3 analyzer was 0–200 ppm, while the average measuring error was less than 10% [48]. All data given in this work was the average value of three repeated measurements. The removal of H2S ( η H 2 S ) and sulfur balance of the plasma-catalytic oxidation of H2S can be defined as:
η H 2 S ( % ) = c i n c o u t c i n × 100 %  
S u l f u r   b a l a n c e ( % ) = c S O 2 + c S O 3 c i n c o u t × 100 %  
where c i n and c o u t are the H2S concentration at the inlet and outlet of the reactor, respectively, while c S O 2 and c S O 3 are the outlet SO2 and SO3 concentrations.

4. Conclusions

A series of non-stoichiometric LaxMnO3 catalysts were evaluated in the plasma-catalytic oxidative removal of H2S using a non-thermal plasma DBD reactor in terms of H2S removal and sulfur balance of the plasma process. The coupling of the DBD plasma with the LaxMnO3 catalysts enhanced both H2S removal and sulfur balance compared to the plasma process without using a catalyst. The highest H2S removal of 96.4% was achieved at a SED of 593.7 J·L−1 when placing the La0.90MnO3 catalyst in the DBD plasma reactor. In addition, the combination of the plasma with the La0.90MnO3 catalyst also showed the highest sulfur balance in the plasma-catalytic process. The non-stoichiometric effect of the LaxMnO3 catalysts significantly affected the removal of H2S since the reaction performance of the plasma-catalytic process decreased with the increasing nominal La/Mn molar ratio. Compared to pure LaMnO3 catalyst, the non-stoichiometric LaxMnO3 catalyst showed enhanced specific surface area and smaller crystallite size. The decreased La/Mn molar ratio in the LaxMnO3 catalysts favored the transformation of Mn3+ cations to Mn4+, which contributed to the formation of oxygen vacancies on the catalyst surfaces. The results of XPS and H2-TPR demonstrated that the Mn-rich catalysts possessed higher relative concentration of surface adsorbed oxygen (Oads) and better reducibility (lower reduction temperature) compared to pure LaMnO3, which suggests that the relative concentration of Oads and reducibility of the catalysts played a key role in determining the reaction performance of the plasma-catalytic removal of H2S.

Author Contributions

Conceptualization: X.Z. and X.T.; data curation: K.X., X.Z., and Y.C.; formal analysis: Y.C.; investigation: K.X. and X.Z.; methodology: X.Z. and Y.C.; writing—original draft: X.Z.; writing—review and editing: X.Z. and X.T.


This research was funded by National Natural Science Foundation of China (no. 51606166) and K.C. Wong Magna Fund in Ningbo University, China.

Conflicts of Interest

The authors declare no conflict of interest.


  1. Bogner, J.E.; Chanton, J.P.; Blake, D.; Abichou, T.; Powelson, D. Effectiveness of a florida landfill biocover for reduction of CH4 and nmhc emissions. Environ. Sci. Technol. 2010, 44, 1197–1203. [Google Scholar] [CrossRef] [PubMed]
  2. Burgess, J.E.; Parsons, S.A.; Stuetz, R.M. Developments in odour control and waste gas treatment biotechnology: A review. Biotechnol. Adv. 2001, 19, 35–63. [Google Scholar] [CrossRef]
  3. Schlegelmilch, M.; Streese, J.; Stegmann, R. Odour management and treatment technologies: An overview. Waste Manag. 2005, 25, 928–939. [Google Scholar] [CrossRef] [PubMed]
  4. Zhang, L.; De Schryver, P.; De Gusseme, B.; De Muynck, W.; Boon, N.; Verstraete, W. Chemical and biological technologies for hydrogen sulfide emission control in sewer systems: A review. Water Res. 2008, 42, 1–12. [Google Scholar] [CrossRef] [PubMed]
  5. Chen, L.; Hoff, S.J. Mitigating odors from agricultural facilities: A review of literature concerning biofilters. Appl. Eng. Agric. 2009, 25, 751–766. [Google Scholar] [CrossRef]
  6. Vandenbroucke, A.M.; Morent, R.; De Geyter, N.; Leys, C. Non-thermal plasmas for non-catalytic and catalytic VOC abatement. J. Hazard. Mater. 2011, 195, 30–54. [Google Scholar] [CrossRef] [PubMed]
  7. Van Durme, J.; Dewulf, J.; Leys, C.; Van Langenhove, H. Combining non-thermal plasma with heterogeneous catalysis in waste gas treatment: A review. Appl. Catal. B Environ. 2008, 78, 324–333. [Google Scholar] [CrossRef]
  8. Andersen, K.B.; Feilberg, A.; Beukes, J.A. Abating odour nuisance from pig production units by the use of a non-thermal plasma system. In Proceedings of the International conference on environmental odour monitoring and control (NOSE), Florence, Italy, 22–24 September 2010; pp. 351–356. [Google Scholar]
  9. Kuwahara, T.; Okubo, M.; Kuroki, T.; Kametaka, H.; Yamamoto, T. Odor removal characteristics of a laminated film-electrode packed-bed nonthermal plasma reactor. Sensors 2011, 11, 5529–5542. [Google Scholar] [CrossRef] [PubMed]
  10. Lu, S.Y.; Chen, L.; Huang, Q.X.; Yang, L.Q.; Du, C.M.; Li, X.D.; Yan, J.H. Decomposition of ammonia and hydrogen sulfide in simulated sludge drying waste gas by a novel non-thermal plasma. Chemosphere 2014, 117, 781–785. [Google Scholar] [CrossRef] [PubMed]
  11. Andersen, K.B.; Feilberg, A.; Beukes, J.A. Use of non-thermal plasma and UV-light for removal of odour from sludge treatment. Water Sci. Technol. 2012, 66, 1656. [Google Scholar] [CrossRef] [PubMed]
  12. Dobslaw, D.; Ortlinghaus, O.; Dobslaw, C. A combined process of non-thermal plasma and a low-cost mineral adsorber for VOC removal and odor abatement in emissions of organic waste treatment plants. J. Environ. Chem. Eng. 2018, 6, 2281–2289. [Google Scholar] [CrossRef]
  13. Dobslaw, D.; Schulz, A.; Helbich, S.; Dobslaw, C.; Engesser, K.-H. VOC removal and odor abatement by a low-cost plasma enhanced biotrickling filter process. J. Environ. Chem. Eng. 2017, 5, 5501–5511. [Google Scholar] [CrossRef]
  14. Maxime, G.; Amine, A.A.; Abdelkrim, B.; Dominique, W. Removal of gas-phase ammonia and hydrogen sulfide using photocatalysis, nonthermal plasma, and combined plasma and photocatalysis at pilot scale. Environ. Sci. Pollut. Res. 2014, 21, 13127–13137. [Google Scholar] [CrossRef] [PubMed]
  15. Ragazzi, M.; Tosi, P.; Rada, E.C.; Torretta, V.; Schiavon, M. Effluents from MBT plants: Plasma techniques for the treatment of VOCs. Waste Manag. 2014, 34, 2400–2406. [Google Scholar] [CrossRef] [PubMed]
  16. Ochiai, T.; Ichihashi, E.; Nishida, N.; Machida, T.; Uchida, Y.; Hayashi, Y.; Morito, Y.; Fujishima, A. Field performance test of an air-cleaner with photocatalysis-plasma synergistic reactors for practical and long-term use. Molecules 2014, 19, 17424–17434. [Google Scholar] [CrossRef] [PubMed]
  17. Almarcha, D.; Almarcha, M.; Jimenez-Coloma, E.; Vidal, L.; Puigcercós, M.; Barrutiabengoa, I. Treatment efficiency by means of a nonthermal plasma combined with heterogeneous catalysis of odoriferous volatile organic compounds emissions from the thermal drying of landfill leachates. J. Eng. 2014, 2014, 831584. [Google Scholar] [CrossRef]
  18. Dinh, M.T.N.; Giraudon, J.M.; Lamonier, J.F.; Vandenbroucke, A.; De Geyter, N.; Leys, C.; Morent, R. Plasma-catalysis of low tce concentration in air using LaMnO3+δ as catalyst. Appl. Catal. B Environ. 2014, 147, 904–911. [Google Scholar] [CrossRef]
  19. Nuns, N.; Beaurain, A.; Dinh, M.T.N.; Vandenbroucke, A.; De Geyter, N.; Morent, R.; Leys, C.; Giraudon, J.M.; Lamonier, J.F. A combined tof-sims and Xps study for the elucidation of the role of water in the performances of a post-plasma process using LaMnO3+δ as catalyst in the total oxidation of trichloroethylene. Appl. Surf. Sci. 2014, 320, 154–160. [Google Scholar] [CrossRef]
  20. Shi, C.; Zhang, Z.S.; Crocker, M.; Xu, L.; Wang, C.Y.; Au, C.T.; Zhu, A.M. Non-thermal plasma-assisted NOx storage and reduction on a LaMn0.9Fe0.1O3 perovskite catalyst. Catal. Today 2013, 211, 96–103. [Google Scholar] [CrossRef]
  21. Hueso, J.; Cotrino, J.; Caballero, A.; Espinos, J.; Gonzalezelipe, A. Plasma catalysis with perovskite-type catalysts for the removal of NO and CH4 from combustion exhausts. J. Catal. 2007, 247, 288–297. [Google Scholar] [CrossRef]
  22. Hueso, J.L.; Caballero, A.; Cotrino, J.; González-Elipe, A.R. Plasma catalysis over lanthanum substituted perovskites. Catal. Commun. 2007, 8, 1739–1742. [Google Scholar] [CrossRef]
  23. Vandenbroucke, A.M.; Nguyen Dinh, M.T.; Nuns, N.; Giraudon, J.M.; De Geyter, N.; Leys, C.; Lamonier, J.F.; Morent, R. Combination of non-thermal plasma and Pd/LaMnO3 for dilute trichloroethylene abatement. Chem. Eng. J. 2016, 283, 668–675. [Google Scholar] [CrossRef]
  24. Choi, J.J.; Billinge, S.J. Perovskites at the nanoscale: From fundamentals to applications. Nanoscale 2016, 8, 6206–6208. [Google Scholar] [CrossRef] [PubMed]
  25. Kim, K.-H.; Choi, Y.J.; Jeon, E.C.; Sunwoo, Y. Characterization of malodorous sulfur compounds in landfill gas. Atmos. Environ. 2005, 39, 1103–1112. [Google Scholar] [CrossRef]
  26. Zhu, X.; Gao, X.; Yu, X.; Zheng, C.; Tu, X. Catalyst screening for acetone removal in a single-stage plasma-catalysis system. Catal. Today 2015, 256, 108–114. [Google Scholar] [CrossRef]
  27. Zhang, C.; Wang, C.; Zhan, W.; Guo, Y.; Guo, Y.; Lu, G.; Baylet, A.; Giroir-Fendler, A. Catalytic oxidation of vinyl chloride emission over LaMnO3 and LaB0.2Mn0.8O3 (B = Co, Ni, Fe) catalysts. Appl. Catal. B Environ. 2013, 129, 509–516. [Google Scholar] [CrossRef]
  28. Zhu, X.; Liu, S.; Cai, Y.; Gao, X.; Zhou, J.; Zheng, C.; Tu, X. Post-plasma catalytic removal of methanol over Mn-Ce catalysts in an atmospheric dielectric barrier discharge. Appl. Catal. B Environ. 2016, 183, 124–132. [Google Scholar] [CrossRef]
  29. Hou, Y.-C.; Ding, M.-W.; Liu, S.-K.; Wu, S.-K.; Lin, Y.-C. Ni-substituted LaMnO3 perovskites for ethanol oxidation. RSC Adv. 2014, 4, 5329. [Google Scholar] [CrossRef]
  30. Shen, M.Q.; Zhao, Z.; Chen, J.H.; Su, Y.G.; Wang, J.; Wang, X.Q. Effects of calcium substitute in LaMnO3 perovskites for NO catalytic oxidation. J. Rare Earth. 2013, 31, 119–123. [Google Scholar] [CrossRef]
  31. Quiroz, J.; Giraudon, J.-M.; Gervasini, A.; Dujardin, C.; Lancelot, C.; Trentesaux, M.; Lamonier, J.-F. Total oxidation of formaldehyde over MnOx-CeO2 catalysts: The effect of acid treatment. ACS Catal. 2015, 5, 2260–2269. [Google Scholar] [CrossRef]
  32. Continetti, R.E.; Balko, B.A.; Lee, Y.T. Photodissociation of H2S and the HS radical at 193.3 nm. Chem. Phys. Lett. 1991, 182, 400–405. [Google Scholar] [CrossRef]
  33. Liang, W.-J.; Fang, H.-P.; Li, J.; Zheng, F.; Li, J.-X.; Jin, Y.-Q. Performance of non-thermal DBD plasma reactor during the removal of hydrogen sulfide. J. Electrostat. 2011, 69, 206–213. [Google Scholar] [CrossRef]
  34. Aerts, R.; Martens, T.; Bogaerts, A. Influence of vibrational states on CO2 splitting by dielectric barrier discharges. J. Phys. Chem. C 2012, 116, 23257–23273. [Google Scholar] [CrossRef]
  35. Zheng, C.; Zhu, X.; Gao, X.; Liu, L.; Chang, Q.; Luo, Z.; Cen, K. Experimental study of acetone removal by packed-bed dielectric barrier discharge reactor. J. Ind. Eng. Chem. 2014, 20, 2761–2768. [Google Scholar] [CrossRef]
  36. Aerts, R.; Tu, X.; De Bie, C.; Whitehead, J.C.; Bogaerts, A. An investigation into the dominant reactions for ethylene destruction in non-thermal atmospheric plasmas. Plasma Process. Polym. 2012, 9, 994–1000. [Google Scholar] [CrossRef]
  37. Zhu, X.; Gao, X.; Qin, R.; Zeng, Y.; Qu, R.; Zheng, C.; Tu, X. Plasma-catalytic removal of formaldehyde over Cu-Ce catalysts in a dielectric barrier discharge reactor. Appl. Catal. B Environ. 2015, 170–171, 293–300. [Google Scholar] [CrossRef]
  38. Holzer, F.; Kopinke, F.D.; Roland, U. Influence of ferroelectric materials and catalysts on the performance of non-thermal plasma (NTP) for the removal of air pollutants. Plasma Chem. Plasma Process. 2005, 25, 595–611. [Google Scholar] [CrossRef]
  39. Jarrige, J.; Vervisch, P. Decomposition of gaseous sulfide compounds in air by pulsed corona discharge. Plasma Chem. Plasma Process. 2007, 27, 241–255. [Google Scholar] [CrossRef]
  40. Chang, M.B.; Balbach, J.H.; Rood, M.J.; Kushner, M.J. Removal of SO2 from gas streams using a dielectric barrier discharge and combined plasma photolysis. J. Appl. Phys. 1991, 69, 4409–4417. [Google Scholar] [CrossRef]
  41. Hyun Ha, K.; Wu, C.; Takashima, K.; Mizuno, A. The influence of reaction conditions on SO2 oxidation in a discharge plasma reactor. IEEE Trans. Ind. Appl. 1999, 3, 1478–1482. [Google Scholar]
  42. Neyts, E.C. Plasma-surface interactions in plasma catalysis. Plasma Chem. Plasma Process. 2015, 36, 185–212. [Google Scholar] [CrossRef]
  43. Tu, X.; Whitehead, J.C. Plasma-catalytic dry reforming of methane in an atmospheric dielectric barrier discharge: Understanding the synergistic effect at low temperature. Appl. Catal. B Environ. 2012, 125, 439–448. [Google Scholar] [CrossRef]
  44. Hosseini, S.A.; Salari, D.; Niaei, A.; Oskoui, S.A. Physical-chemical property and activity evaluation of LaB0.5Co0.5O3 (B = Cr, Mn, Cu) and LaMnxCo1−xO3 (x = 0.1, 0.25, 0.5) nano perovskites in VOC combustion. J. Ind. Eng. Chem. 2013, 19, 1903–1909. [Google Scholar] [CrossRef]
  45. Chen, J.; Shen, M.; Wang, X.; Qi, G.; Wang, J.; Li, W. The influence of nonstoichiometry on LaMnO3 perovskite for catalytic NO oxidation. Appl. Catal. B Environ. 2013, 134–135, 251–257. [Google Scholar] [CrossRef]
  46. Dai, Y.; Wang, X.Y.; Li, D.; Dai, Q.G. Catalytic combustion of chlorobenzene over Mn-Ce-La-O mixed oxide catalysts. J. Hazard. Mater. 2011, 188, 132–139. [Google Scholar]
  47. Zhang, Z.; Jiang, Z.; Shangguan, W. Low-temperature catalysis for VOCs removal in technology and application: A state-of-the-art review. Catal. Today 2016, 264, 270–278. [Google Scholar] [CrossRef]
  48. Yang, Z.; Zheng, C.; Zhang, X.; Zhou, H.; Silva, A.A.; Liu, C.; Snyder, B.; Wang, Y.; Gao, X. Challenge of SO3 removal by wet electrostatic precipitator under simulated flue gas with high SO3 concentration. Fuel 2018, 217, 597–604. [Google Scholar] [CrossRef]
Figure 1. XRD patterns of LaxMnO3 catalysts.
Figure 1. XRD patterns of LaxMnO3 catalysts.
Catalysts 08 00317 g001
Figure 2. XPS spectra of LaxMnO3 catalysts: (a) Mn 2p3/2; and (b) O 1s.
Figure 2. XPS spectra of LaxMnO3 catalysts: (a) Mn 2p3/2; and (b) O 1s.
Catalysts 08 00317 g002
Figure 3. H2-TPR profiles of LaxMnO3 catalysts.
Figure 3. H2-TPR profiles of LaxMnO3 catalysts.
Catalysts 08 00317 g003
Figure 4. Effect of SED on plasma-catalytic removal of H2S over LaxMnO3 catalysts: (a) removal efficiency; and (b) sulfur balance of the plasma-catalytic process.
Figure 4. Effect of SED on plasma-catalytic removal of H2S over LaxMnO3 catalysts: (a) removal efficiency; and (b) sulfur balance of the plasma-catalytic process.
Catalysts 08 00317 g004
Figure 5. Reaction mechanisms of plasma-catalytic removal of H2S over the LaxMnO3 catalysts.
Figure 5. Reaction mechanisms of plasma-catalytic removal of H2S over the LaxMnO3 catalysts.
Catalysts 08 00317 g005
Figure 6. Schematic diagram of the experimental setup.
Figure 6. Schematic diagram of the experimental setup.
Catalysts 08 00317 g006
Table 1. Physicochemical properties of LaxMnO3 catalysts.
Table 1. Physicochemical properties of LaxMnO3 catalysts.
SampleSBET (m2·g−1)1 Crystalline Size (nm)Cell Volume (Å3)Mn4+/(Mn3+ + Mn4+) (%)Oads/(Oads + Olat) (%)
La0.90MnO315.215.458.643.2 60.7
La0.95MnO313.015.858.742.2 59.9
LaMnO312.616.158.941.5 58.1
La1.05MnO313.715.9233.240.8 57.6
La1.10MnO314.615.7234.438.2 56.6
1 Calculated from the diffraction peak of LaxMnO3 located at 2θ = 32.6°.

© 2018 by the authors. Licensee MDPI, Basel, Switzerland. This article is an open access article distributed under the terms and conditions of the Creative Commons Attribution (CC BY) license (
Catalysts EISSN 2073-4344 Published by MDPI AG, Basel, Switzerland RSS E-Mail Table of Contents Alert
Back to Top