Performance of Mn-Fe-Ce / GO-x for Catalytic Oxidation of Hg 0 and Selective Catalytic Reduction of NO x in the Same Temperature Range

A series of composites of Mn-Fe-Ce/GO-x have been synthesized by a hydrothermal method. Their performance in simultaneously performing the catalytic oxidation of Hg0 and the selective catalytic reduction of nitrogen oxides (NOx) in the same temperature range were investigated. In order to investigate the physicochemical properties and surface reaction, basic tests, including Brunauer-Emmett-Teller (BET), XRD, scanning electron microscope (SEM) and X-ray photoelectron spectroscopy (XPS) were selected. The results indicate that the active components deposited on graphene play an important role in the removal of mercury and NOx, with different valences. Especially, the catalyst of Mn-Fe-Ce/GO-20% possesses an excellent efficiency in the temperature range of 170 to 250 ◦C. Graphene has a huge specific surface area and good mechanical property; thus, the active components of the Mn-Fe-Ce catalyst can be highly dispersed on the surface of graphene oxide. In addition, the effects of O2, H2O, NO and SO2 on the removal efficiency of Hg0 were examined in flue gas. Furthermore, the regeneration experiments conducted by thermal methods proved to be promising methods.


Introduction
In recent years, the removal of mercury and its derivatives has attracted significant attention due to their toxic effects on ecological safety and human health [1][2][3].Many researchers have explored an effective way to control the emission of mercury from coal-fired power plants.As we know, mercury is released into exhaust gas in the form of elemental mercury (Hg 0 ), oxidized mercury (Hg 2+ ) and particulate bound mercury (Hg p ) [4][5][6].At present, Hg 2 + is water-soluble and can be easily removed by wet flue gas desulfurization, and Hg p attached to fly ash can be captured by electrostatic precipitators and fabric filters.In a word, Hg 2+ and Hg p can easily be controlled by existing air pollution control devices [7][8][9][10][11][12].However, Hg 0 is difficult to capture due to its high volatility and water-insolubility.Therefore, Hg 0 is the main mercury species that is emitted in the stack flue gas from coal-fired utilities.Even more alarming, Hg 0 can circulate in the atmosphere for years, and its toxic effects have a global-scale impact.Consequently, the conversion of Hg 0 to Hg 2+ or Hg p is the main method of removing elemental mercury.In previous explorations, methods of sorbent injection, catalytic oxidation, electrocatalytic oxidation, and photochemical oxidation were carried out to remove Hg 0 [13][14][15][16][17][18].Therein, the catalytic oxidation of Hg 0 is the most promising method due to its high-efficiency.
Besides the difficulties that are associated with mercury removal, reducing the emission of NO x is also difficult.NO x from the exhaust gases of coal-fired power plants is the major source of air pollution.Specifically, NO x causes photochemical smog, acid rain, ozone depletion, and greenhouse effects, etc.So far, the commercial catalyst of V 2 O 5 -WO 3 /TiO 2 is widely used in the field of controlling NO x emission.However, this catalyst is significantly affected by the flue gas temperature and easily loses its catalytic activities at low temperatures.Meanwhile, the addition of chlorine into the boiler is needed in order to realize the activities of Hg 0 oxidation [19][20][21].It is necessary to explore an effective and economical catalyst to remove Hg 0 and NO x in the same temperature range, without the assistance of chlorine.
Besides the V 2 O 5 -WO 3 /TiO 2 catalyst, many transition metal oxides were explored for the oxidation of Hg 0 and the reduction of NO x , such as MnO x , FeO x , CeO x , V 2 O 5 , CuO x and CoO x [22][23][24][25].However, the single metal oxides, as mentioned above, can hardly meet the demand of simultaneously removing Hg 0 and NO x .Hence, researchers tried to dope one or more metal oxides to obtain catalysts with a higher performance.For instance, Mn-Ce/TiO 2 , Mn-Fe spinel and Ce-Fe-O were studied to enhance the performance of a single metal oxide for Hg 0 and NO x removal [26][27][28].Mn-Ce/TiO 2 is highly effective in removing Hg 0 and NO x , for the reason that the Mn oxides exhibit excellent catalytic activities at lower temperatures, and the Ce oxides can provide an amount of trapped oxygen for redox [29][30][31].However, its high performance is inhibited by SO 2 in the flue gas.In order to explore the catalyst that is resistant to SO 2 , Mn-Fe spinel has been explored, which possesses an excellent SO 2 -resistance ability, by doping Mn oxides with Fe oxides.Regrettably, the Hg 0 oxidation ability of Mn-Fe spinel is limited.It is necessary to explore a catalyst that possesses inhibitory effects of SO 2 and a high activity under different flue gas conditions.The above problems motivate us to focus on the design and synthesis of new catalysts with an optimal catalytic performance.To the best of our knowledge, using the three metal oxides, MnO x , CeO x , and FeO x , to synthesize the Fe-Mn-Ce oxide-based catalyst has seldom been reported in the literature for Hg 0 oxidation and NO x reduction [32].Thus, we carried out systematic explorations on the Fe-Mn-Ce oxide-based catalyst.
Moreover, the carrier plays an important role in enhancing the performance of the catalyst.Usually, the metal oxides have a small specific surface area, while the carrier has a big specific surface area.In particular, graphene is a planar sheet that is composed of carbon atoms [33][34][35].Its large surface area (calculated value, 2630 m 2 /g) is convenient for the dispersion of active components.Moreover, the mobility of charge carriers (200,000 cm 2 /Vs) can significantly facilitate electron transfer in an oxidation-reduction reaction [31].According to the literature, graphene can be oxidized by strong acid or other methods to obtain graphene oxide (GO) with many functional groups, which can offer abundant nucleation sites for metal atoms.It is a viable approach to exploring new catalysts, while using GO as a catalyst carrier.
In this work, the Mn-Fe-Ce/GO-x catalysts were synthesized via a hydrothermal method, based on the excellent properties of GO as a catalyst carrier.Moreover, the characterization methods of Brunauer-Emmett-Teller (BET), XRD, scanning electron microscope (SEM), and X-ray photoelectron spectroscopy (XPS) were selected to reveal the physicochemical properties of the Mn-Fe-Ce/GO-x catalysts.The composites were investigated through a fixed-bed reaction system for Hg 0 and NO x removal in the temperature range of 100 to 400 • C.Moreover, the effects of flue gas components, including O 2 , NO, H 2 O and SO 2 , on the oxidation of Hg 0 and reduction of NO x were discussed.The combination of GO sheets and the Mn-Ce-Fe-O particles is advantageous for the application of Mn-Ce-Fe oxides.The outstanding performance was discussed in light of the test results and characterization techniques.

Characterization of Catalysts
The microstructural parameters of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) catalysts were investigated, and the results are listed in Table 1.With the increase of GO content from 0 to 20%, the specific surface area, pore volume and pore diameter of the catalysts correspondingly increased from 2.37 to 109.23 m 2 /g, 0.0089 to 0.0462 cm 3 /g, and 2.321 to 3.426 nm, respectively.However, further increasing the GO content to 30% resulted in a decrease of microstructural parameters due to the aggregation of GO.Therefore, the Ce-Fe-Mn/GO 0.2 with an appropriate carrier of GO is considered to be a candidate with a better catalytic performance.

Samples
BET Surface (m 2 /g) Pore Volume (cm The XRD patterns of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) catalysts are shown in Figure 1.All of the samples show characteristic diffraction peaks of MnO 2 and Mn 3 O 4 in the patterns.Nevertheless, few weak peaks of crystalline Fe and Ce oxides are detected in the XRD patterns, indicating that all the Fe and Ce oxides have a fine grain size and exist in an amorphous form.The characteristic diffraction peaks of graphene, at approximately 20-25 • in the results, are found in Ce-Mn-Fe/GO-x (x = 10%, 20%, 30%), suggesting that the graphene structure was successfully synthesized, and the peak of GO, at approximately 2θ = 13 • , is also detected by a Bruker D2 PHASER diffractometer.
further increasing the GO content to 30% resulted in a decrease of microstructural parameters due to the aggregation of GO.Therefore, the Ce-Fe-Mn/GO0.2with an appropriate carrier of GO is considered to be a candidate with a better catalytic performance.The XRD patterns of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) catalysts are shown in Figure 1.All of the samples show characteristic diffraction peaks of MnO2 and Mn3O4 in the patterns.Nevertheless, few weak peaks of crystalline Fe and Ce oxides are detected in the XRD patterns, indicating that all the Fe and Ce oxides have a fine grain size and exist in an amorphous form.The characteristic diffraction peaks of graphene, at approximately 20-25° in the results, are found in Ce-Mn-Fe/GO-x (x = 10%, 20%, 30%), suggesting that the graphene structure was successfully synthesized, and the peak of GO, at approximately 2θ = 13°, is also detected by a Bruker D2 PHASER diffractometer.In order to further identify the composition and content on the surface of all the samples, the EDS of Ce-Mn-Fe/GO-20% was selected, and the results are shown in Figure 2. Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10% and Ce-Mn-Fe/GO-30% are shown in Figures S1-S3 in the Supporting Information, respectively.It can be seen, from all of these Figures, that the catalysts present the contents of Fe, Ce, Mn and O elements on the GO carrier.That is to say, there were no visible phases of Fe and Ce oxides in the XRD patterns, indicating that all of the Fe and Ce oxides were highly dispersed over the support, with a low content.The EDS proves the existence of Fe and Ce oxides on GO.
The SEM characterization provides a convenient approach to investigating the morphology of the prepared catalysts.Images of microscopic Ce-Mn-Fe/GO-0 and Ce-Mn-Fe/GO-10% morphologies, which are particle-like as well as highly aggregated and disorganized, are shown in Figures S1 and S2.As shown in the image of Ce-Mn-Fe/GO-20% in Figure 2, the metal oxides distributed on the GO structure were more uniform and showed a smaller particle size.Ce-Mn-Fe/GO-30% in Figure S3 indicates that plenty of GO join together to limit the attachment of In order to further identify the composition and content on the surface of all the samples, the EDS of Ce-Mn-Fe/GO-20% was selected, and the results are shown in Figure 2. Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10% and Ce-Mn-Fe/GO-30% are shown in Figures S1-S3 in the Supporting Information, respectively.It can be seen, from all of these Figures, that the catalysts present the contents of Fe, Ce, Mn and O elements on the GO carrier.That is to say, there were no visible phases of Fe and Ce oxides in the XRD patterns, indicating that all of the Fe and Ce oxides were highly dispersed over the support, with a low content.The EDS proves the existence of Fe and Ce oxides on GO.
The SEM characterization provides a convenient approach to investigating the morphology of the prepared catalysts.Images of microscopic Ce-Mn-Fe/GO-0 and Ce-Mn-Fe/GO-10% morphologies, which are particle-like as well as highly aggregated and disorganized, are shown in Figures S1 and  S2.As shown in the image of Ce-Mn-Fe/GO-20% in Figure 2, the metal oxides distributed on the GO structure were more uniform and showed a smaller particle size.Ce-Mn-Fe/GO-30% in Figure S3 indicates that plenty of GO join together to limit the attachment of oxides, and this result is consistent with the BET test.In the catalyst of Ce-Mn-Fe/GO-20%, numerous nanoparticles were inserted into the GO sheets for further analysis, and this result indicates that GO can not only prevent the aggregation of catalytic activity particles, but also the nanoparticles load on GO through functional groups, such as carboxyl, hydroxyl, and epoxy groups [36].Hence, the highly dispersed and uniform nanoscale Ce-Mn-Fe-O particles are embedded in GO.
Catalysts 2018, 8, x FOR PEER REVIEW 4 of 16 numerous nanoparticles were inserted into the GO sheets for further analysis, and this result indicates that GO can not only prevent the aggregation of catalytic activity particles, but also the nanoparticles load on GO through functional groups, such as carboxyl, hydroxyl, and epoxy groups [36].Hence, the highly dispersed and uniform nanoscale Ce-Mn-Fe-O particles are embedded in GO.The XPS spectra of the samples were performed to further illustrate the chemical composition and the valence states of Mn, Ce and Fe.The results are exhibited in Figure 3, the Mn 3d spectra with two main peaks, corresponding to Mn 2p3/2 and Mn 2p1/2, are observed in Figure 3a.The Mn 2p1/2 peak consists of three sub-peaks, the corresponding binding energy of Mn 3+ is 641.8 eV, and the peaks at about 642.4 eV, 641.2 eV, and 640.2 eV are Mn 4+ , Mn 3+ and Mn 2+ , respectively.The rate of (Mn 4+ + Mn 3+ )/Mn 2+ was usually considerable for Hg 0 oxidation, based on article [37].The high valence Mn oxides enhance Hg 0 oxidation efficiency, as Mn 4+ can directly oxidize the adsorbed Hg 0 , and Mn 3+ also has potential activity in Hg 0 oxidation in the presence of O2.Manganese oxides exist at the mixed states of Mn 4+ and Mn 3+ in the four composition catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%).In particular, the Ce-Mn-Fe/GO-20% possesses a higher Hg 0 oxidation efficiency than other catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 30%), and the main reason may be that the highest ratios of (Mn 4+ + Mn 3+ )/Mn 2+ are in the Ce-Mn-Fe/GO-20% sample, which plays an important role in Hg 0 oxidation.In addition, the catalyst has quite a high content of Mn 4+ and Mn 3+ on the surface and it shows good activity in NOx reduction with NH3 at low temperatures [38].
The XPS spectra of Ce3d for these catalysts are presented in Figure 3b.The peaks that were labeled U and V were the corresponding 3d5/2 and 3d3/2 spin-orbit states, respectively [39].The U0, U1, U3, V3, V2, and V0 belonged to the 3d 10 4f 0 state of the Ce 4+ species, and U2 and V1 are assigned to the 3d 10 4f 1 initial electronic state of the Ce 3+ species [40].When comparing with the four catalysts, the Ce-Mn-Fe/GO-10% has the highest ratio of Ce 4+ /Ce 3+ , but the ratio of Ce 4+ /Ce 3+ decreases in the optimal catalyst, Ce-Mn-Fe/GO-20%, and it can be inferred from this result that some reactions take place in the preparation process.Thus, the most possible reaction is as follows [41]: The reaction further explains the reason why the Ce-Mn-Fe/GO-20% has high ratios of (Mn 4+ + Mn 3+ )/Mn 2+ .The ratios of Ce 4+ /Ce 3+ were calculated and are shown in Figure 3b, and it is obvious that The XPS spectra of the samples were performed to further illustrate the chemical composition and the valence states of Mn, Ce and Fe.The results are exhibited in Figure 3, the Mn 3d spectra with two main peaks, corresponding to Mn 2p 3/2 and Mn 2p 1/2 , are observed in Figure 3a.The Mn 2p 1/2 peak consists of three sub-peaks, the corresponding binding energy of Mn 3+ is 641.8 eV, and the peaks at about 642.4 eV, 641.2 eV, and 640.2 eV are Mn 4+ , Mn 3+ and Mn 2+ , respectively.The rate of (Mn 4+ + Mn 3+ )/Mn 2+ was usually considerable for Hg 0 oxidation, based on article [37].The high valence Mn oxides enhance Hg 0 oxidation efficiency, as Mn 4+ can directly oxidize the adsorbed Hg 0 , and Mn 3+ also has potential activity in Hg 0 oxidation in the presence of O 2 .Manganese oxides exist at the mixed states of Mn 4+ and Mn 3+ in the four composition catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%).In particular, the Ce-Mn-Fe/GO-20% possesses a higher Hg 0 oxidation efficiency than other catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 30%), and the main reason may be that the highest ratios of (Mn 4+ + Mn 3+ )/Mn 2+ are in the Ce-Mn-Fe/GO-20% sample, which plays an important role in Hg 0 oxidation.In addition, the catalyst has quite a high content of Mn 4+ and Mn 3+ on the surface and it shows good activity in NO x reduction with NH 3 at low temperatures [38].
The XPS spectra of Ce3d for these catalysts are presented in Figure 3b.The peaks that were labeled U and V were the corresponding 3d 5/2 and 3d 3/2 spin-orbit states, respectively [39].The U 0 , U 1 , U 3 , V 3 , V 2 , and V 0 belonged to the 3d 10 4f 0 state of the Ce 4+ species, and U 2 and V 1 are assigned to the 3d 10 4f 1 initial electronic state of the Ce 3+ species [40].When comparing with the four catalysts, the Ce-Mn-Fe/GO-10% has the highest ratio of Ce 4+ /Ce 3+ , but the ratio of Ce 4+ /Ce 3+ decreases in the optimal catalyst, Ce-Mn-Fe/GO-20%, and it can be inferred from this result that some reactions take place in the preparation process.Thus, the most possible reaction is as follows [41]: The reaction further explains the reason why the Ce-Mn-Fe/GO-20% has high ratios of (Mn 4+ + Mn 3+ )/Mn 2+ .The ratios of Ce 4+ /Ce 3+ were calculated and are shown in Figure 3b, and it is obvious that the majority of the Ce ions are Ce 4+ , which is beneficial for Hg 0 oxidation.Moreover, it has been reported that the Ce 3+ species can not only create charge imbalance, vacancies, and unsaturated chemical bonds, but also enhance Hg 0 oxidation with the chemisorbed oxygen species on the surface of catalyst [42].
The XPS spectra of Fe2p for catalysts are shown in Figure 3c.The peaks appeared at 709.3 eV, which was attributed to Fe 2+ cations [43], and at the 711.42 eV, 713.2 eV, 725.4 eV, which were assigned to Fe 3+ .Different states of iron cations contain a weak oxidation property in relation to Hg 0 , however, they have positive effects on NO x reduction with NH 3 at the ideal temperatures [44].
As shown in Figure 3d, the peaks at low binding energy (about 259.5-25.97eV) could be regarded as lattice oxygen (denoted as O α ), the binding energy peak at 531.0-531.7 eV is attributed to chemisorbed oxygen and C=O groups (denoted as O β ), and the peak at 532.7-533.5 eV was reported to exist in hydroxy (denoted as O r ) [45,46].When comparing GO with Ce-Mn-Fe/GO-0, the peaks at about 532.8-533.5 eV belong to GO, however, the peaks at about 259.5-25.97eV belong to the metal oxide nanocrystals.On the Ce-Mn-Fe/GO-x (10%, 20%, 30%), the peaks at 531.1-531.7 eV may belong to GO and metal oxide.In this study, the concentrations of the three types of O were listed in Table 2.The concentration of O β and O r on the GO is 45.36% and 54.64%, respectively.On the Ce-Mn-Fe/GO-0, the concentration of O α and O β is 60.24% and 30.76%, respectively.With the increasing of GO content from 0.1 to 0.3, the intensity percentage of O β on Ce-Mn-Fe/GO-x (10%, 20%, 30%) is 31.73%,32.16%, and 18.4%, respectively.The catalyst of Ce-Mn-Fe/GO-20% has a higher efficiency of Hg 0 removal than Ce-Mn-Fe/GO-x (20%, 30%), because the O β species are believed to be the most active oxygen for oxidation reactions [47].The XPS spectra of Fe2p for catalysts are shown in Figure 3c.The peaks appeared at 709.3 eV, which was attributed to Fe 2+ cations [43], and at the 711.42 eV, 713.2 eV, 725.4 eV, which were assigned to Fe 3+ .Different states of iron cations contain a weak oxidation property in relation to Hg 0 , however, they have positive effects on NOx reduction with NH3 at the ideal temperatures [44].
As shown in Figure 3d, the peaks at low binding energy (about 259.5-25.97eV) could be regarded as lattice oxygen (denoted as Oα), the binding energy peak at 531.0-531.7 eV is attributed to chemisorbed oxygen and C=O groups (denoted as Oβ), and the peak at 532.7-533.5 eV was reported to exist in hydroxy (denoted as Or) [45,46].When comparing GO with Ce-Mn-Fe/GO-0, the peaks at about 532.8-533.5 eV belong to GO, however, the peaks at about 259.5-25.97eV belong to the metal oxide nanocrystals.On the Ce-Mn-Fe/GO-x (10%, 20%, 30%), the peaks at 531.1-531.7 eV may belong to GO and metal oxide.In this study, the concentrations of the three types of O were listed in Table 2.The concentration of Oβ and Or on the GO is 45.36% and 54.64%, respectively.On the Ce-Mn-Fe/GO-0, the concentration of Oα and Oβ is 60.24% and 30.76%, respectively.With the increasing of GO content from 0.1 to 0.3, the intensity percentage of Oβ on Ce-Mn-Fe/GO-x (10%, 20%, 30%) is 31.73%,32.16%, and 18.4%, respectively.The catalyst of Ce-Mn-Fe/GO-20% has a higher efficiency of Hg 0 removal than Ce-Mn-Fe/GO-x (20%, 30%), because the Oβ species are believed to be the most active oxygen for oxidation reactions [47].As discussed above, the reactive temperatures of Hg 0 shift to a low temperature region when the manganese oxides are involved in the reaction.The cerium has a superior ability to store oxygen, which contributes to Hg 0 oxidation and NOx reduction.The oxidizability of manganese and cerium oxides is stronger than that of iron oxides, and the presence of the iron content can enhance the high As discussed above, the reactive temperatures of Hg 0 shift to a low temperature region when the manganese oxides are involved in the reaction.The cerium has a superior ability to store oxygen, Catalysts 2018, 8, 399 7 of 17 which contributes to Hg 0 oxidation and NO x reduction.The oxidizability of manganese and cerium oxides is stronger than that of iron oxides, and the presence of the iron content can enhance the high valence states of the other two metal oxides [33].As the result, the catalysts that contain the three metals show an effective property for Hg 0 and NO x removal.
The reducibility of the prepared catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) was detected by H 2 -TPR in the temperature range of 100-900 • C, and the results are shown in Figure 4.For Ce-Mn-Fe/GO-0, the peak at around 314 • C can be attributed to the reduction of a highly dispersed MnO 2 to Mn 3 O 4 .In addition, the higher two reduction peaks at 422 and 494 • C are the reductions of Mn 2 O 3 to MnO and Fe 3 O 4 to FeO, respectively [30,48].The peak at 678 • C may be a reduction of CeO 2 to Ce 2 O 3 [49].The peak above 750 • C was assigned to the reduction of surface FeO to Fe [50].The sample of Ce-Mn-Fe/GO-10% shows three apparent peaks in the H 2 -TPR curves, and the reduction When compared with Ce-Mn-Fe/GO-10%, the reduction peaks of Ce-Mn-Fe/GO-20% shift to a lower temperature due to the increase of GO.Furthermore, Ce-Mn-Fe/GO-30% evidently has an increase in GO, and the reduction curves shift gradually towards a higher temperature, the main reason being that amounts of GO join together and lead to a decrease of reducibility of metallic oxides.Above all, the sample of Ce-Mn-Fe/GO-20% has higher redox ability, with moderate GO.valence states of the other two metal oxides [33].As the result, the catalysts that contain the three metals show an effective property for Hg 0 and NOx removal.
The reducibility of the prepared catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) was detected by H2-TPR in the temperature range of 100-900 °C, and the results are shown in Figure 4.For Ce-Mn-Fe/GO-0, the peak at around 314 °C can be attributed to the reduction of a highly dispersed MnO2 to Mn3O4.In addition, the higher two reduction peaks at 422 and 494 °C are the reductions of Mn2O3 to MnO and Fe3O4 to FeO, respectively [30,48].The peak at 678 °C may be a reduction of CeO2 to Ce2O3 [49].The peak above 750 °C was assigned to the reduction of surface FeO to Fe [50].The sample of Ce-Mn-Fe/GO-10% shows three apparent peaks in the H2-TPR curves, and the reduction When compared with Ce-Mn-Fe/GO-10%, the reduction peaks of Ce-Mn-Fe/GO-20% shift to a lower temperature due to the increase of GO.Furthermore, Ce-Mn-Fe/GO-30% evidently has an increase in GO, and the reduction curves shift gradually towards a higher temperature, the main reason being that amounts of GO join together and lead to a decrease of reducibility of metallic oxides.Above all, the sample of Ce-Mn-Fe/GO-20% has higher redox ability, with moderate GO.

The Performance of the Prepared Materials
The Hg 0 oxidation and NOx recondition efficiencies over Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) were studied at reaction temperatures, with a range of 100 to 400 °C, and the results are shown in Figure 5.The catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) exhibit weak Eoxi, which is approximately 30%, 43%, 67%, and 45% at 100 °C, respectively.The efficiency at this temperature is mainly attributed to the physical adsorption and oxidation of Oβ on the surface of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) for Hg 0 oxidation.The Eoxi increases with the increasing of temperature, and over 95% of Eoxi can be obtained at 170 °C for Ce-Mn-Fe/GO-20% and Ce-Mn-Fe/GO-30%.However, the value for Ce-Mn-Fe/GO-30% starts to decrease, when the temperature reaches 200 °C, and it continues to reduce in the range of 200 to 400 °C.Ce-Mn-Fe/GO-20% maintains the highest Eoxi, until the temperature reaches 250 °C, at which point it decreases rapidly until 400 °C.The samples of Ce-Mn-Fe/GO-0 and Ce-Mn-Fe/GO-10% exhibit the highest Eoxi, exceeding 87% at 300 °C and 83% at 220 °C, and the Eoxi decreases to about 62% and 22% at 400 °C, respectively.Comparing the four composites in relation to Eoxi, the sample of Ce-Mn-Fe/GO-20% shows an outstanding efficiency with a low temperature of 170 °C and when the temperature span is 80 °C (see the larger image in Figure 5).The reason is that metallic oxide particles uniformly load on GO with a large specific surface area, which is beneficial for Hg 0 absorption and oxidation.

The Performance of the Prepared Materials
The Hg 0 oxidation and NO x recondition efficiencies over Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) were studied at reaction temperatures, with a range of 100 to 400 • C, and the results are shown in Figure 5.The catalysts of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) exhibit weak E oxi , which is approximately 30%, 43%, 67%, and 45% at 100 • C, respectively.The efficiency at this temperature is mainly attributed to the physical adsorption and oxidation of O β on the surface of Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) for Hg 0 oxidation.The E oxi increases with the increasing of temperature, and over 95% of E oxi can be obtained at 170 • C for Ce-Mn-Fe/GO-20% and Ce-Mn-Fe/GO-30%.However, the value for Ce-Mn-Fe/GO-30% starts to decrease, when the temperature reaches 200 • C, and it continues to reduce in the range of 200 to 400 • C. Ce-Mn-Fe/GO-20% maintains the highest E oxi , until the temperature reaches 250 • C, at which point it decreases rapidly until 400 • C. The samples of Ce-Mn-Fe/GO-0 and Ce-Mn-Fe/GO-10% exhibit the highest E oxi , exceeding 87% at 300 • C and 83% at 220 • C, and the E oxi decreases to about 62% and 22% at 400 • C, respectively.Comparing the four composites in relation to E oxi , the sample of Ce-Mn-Fe/GO-20% shows an outstanding efficiency with a low temperature of 170 • C and when the temperature span is 80 • C (see the larger image in Figure 5).
The reason is that metallic oxide particles uniformly load on GO with a large specific surface area, which is beneficial for Hg 0 absorption and oxidation.
The η of Ce-Mn-Fe/GO-20% at different temperatures with NH3 is shown in Figure 6.At the reaction temperature of 160 to 255 °C (see the larger image in Figure 6), the η is maintained at above 90%, indicating that the catalyst has a rather wide temperature window.Especially, the η reaches 97% at 170 °C.Interestingly, the excellent Eoxi and η of Ce-Mn-Fe/GO-20% is exhibited in the same temperature range of 170-250 °C, and the highest efficiencies that can be achieved are 95% and 97%, respectively.The η over Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10%, and Ce-Mn-Fe/GO-30% catalysts were also investigated, and the results are shown in the Supporting Information for comparison (Figure S4).The N2O output concentration over Ce-Mn-Fe/GO-20% is shown in Figure 7a.This shows that nearly 100% N2 selectivity was obtained in the region of 180-250 °C over the catalysts.However, the The η of Ce-Mn-Fe/GO-20% at different temperatures with NH 3 is shown in Figure 6.At the reaction temperature of 160 to 255 • C (see the larger image in Figure 6), the η is maintained at above 90%, indicating that the catalyst has a rather wide temperature window.Especially, the η reaches 97% at 170 • C. Interestingly, the excellent E oxi and η of Ce-Mn-Fe/GO-20% is exhibited in the same temperature range of 170-250 • C, and the highest efficiencies that can be achieved are 95% and 97%, respectively.The η over Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10%, and Ce-Mn-Fe/GO-30% catalysts were also investigated, and the results are shown in the Supporting Information for comparison (Figure S4).The η of Ce-Mn-Fe/GO-20% at different temperatures with NH3 is shown in Figure 6.At the reaction temperature of 160 to 255 °C (see the larger image in Figure 6), the η is maintained at above 90%, indicating that the catalyst has a rather wide temperature window.Especially, the η reaches 97% at 170 °C.Interestingly, the excellent Eoxi and η of Ce-Mn-Fe/GO-20% is exhibited in the same temperature range of 170-250 °C, and the highest efficiencies that can be achieved are 95% and 97%, respectively.The η over Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10%, and Ce-Mn-Fe/GO-30% catalysts were also investigated, and the results are shown in the Supporting Information for comparison (Figure S4).The N2O output concentration over Ce-Mn-Fe/GO-20% is shown in Figure 7a.This shows that nearly 100% N2 selectivity was obtained in the region of 180-250 °C over the catalysts.However, the The N 2 O output concentration over Ce-Mn-Fe/GO-20% is shown in Figure 7a.This shows that nearly 100% N 2 selectivity was obtained in the region of 180-250 • C over the catalysts.However, the N 2 O output concentration over Ce-Mn-Fe/GO-20% gradually increased with the rising temperature in the region of 280-300 • C, due to the produce of N 2 O, resulting from the gradual oxidation of NH 3 at a high temperature.The changes of NO 2 concentration in the region of 140-300 • C, indicating that there is almost no NO 2 output, as shown in Figure 7b.N2O output concentration over Ce-Mn-Fe/GO-20% gradually increased with the rising temperature in the region of 280-300 °C, due to the produce of N2O, resulting from the gradual oxidation of NH3 at a high temperature.The changes of NO2 concentration in the region of 140-300 °C, indicating that there is almost no NO2 output, as shown in Figure 7b.

Effect of Individual Flue Gas Components
Hg 0 oxidation efficiencies (average value of one hour) over the Ce-Mn-Fe/GO-20% catalyst at 170 °C, under different flue gas components, are shown in Figure 8.

The Effect of O2 on Mercury Oxidation over the Ce-Mn-Fe/GO-20% Catalyst
O2 plays an important role in Hg 0 oxidation and NOx reduction, and the results are presented in Figure 8.In the absence of O2 (pure N2), at first, the Eoxi is 93%, but after a time, the Eoxi decreases.When the O2 concentration increases to 3%, the Hg 0 removal performance is enhanced, and Eoxi is    O 2 plays an important role in Hg 0 oxidation and NO x reduction, and the results are presented in Figure 8.In the absence of O 2 (pure N 2 ), at first, the E oxi is 93%, but after a time, the E oxi decreases.When the O 2 concentration increases to 3%, the Hg 0 removal performance is enhanced, and E oxi is 96%.To further investigate the effect of O 2 on Hg 0 oxidation, 6% O 2 was added in the simulated flue gas, and the E oxi is increased to 98%.A further increase to 12% O 2 makes no sense.Obviously, O 2 is favorable for Hg 0 oxidation, and this is in accordance with previous studies [23].

Effect of Individual Flue Gas Components
2.3.2.The Effect of SO 2 on Mercury Oxidation over the Ce-Mn-Fe/GO-20% Catalyst The effect of SO 2 on E oxi includes inhibition, promotion, and non-response.In our study, different concentrations of SO 2 (300 ppm and 600 ppm SO 2 ) were added into the pure N 2 gas flow, and the result is demonstrated in Figure 8.The E oxi decreases from 93% (pure N 2 ) to 83% and 75%, with an SO 2 concentration gradient of between 300 ppm to 600 ppm.SO 2 has an inhibition effect on mercury removal.Besides, 6% O 2 and 300 ppm SO 2 were added to the mixer, interestingly increasing the E oxi to 97%, and the result changes little when the concentration of SO 2 changes from 300 ppm to 600 ppm.The reason is that the SO 2 may not only directly react with O 2 over the catalyst, but may also react with the lattice oxygen to form SO 3 , which can offer more acid active sites to oxidize the adsorbed Hg 0 [51].

The Effect of NO on Mercury Oxidation over the Ce-Mn-Fe/GO-20% Catalyst
The affecting factor of NO concentration is usually considered in relation to Hg 0 removal.In this study, the selected concentrations of NO were 300 ppm and 800 ppm.As shown in Figure 8, in the absence of NO, pure N 2 was used for comparison, in which the E oxi is 93%.In an atmosphere of 300 ppm and 800 ppm NO, the E oxi is 78% and 70%, respectively, and the NO exhibits an inhibitory effect on Hg 0 removal.In addition, the E oxi increased to 95% and 92% when 6% O 2 was added to 300 ppm and 800 ppm NO.The probable reason for the promotional effect is that NO could be oxidized by the surface oxygen species in order to generate active species, such as NO 2 [52].Therefore, a promotional effect of NO with O 2 on mercury removal in this study was attributed to the production of NO 2 , which can provide acid sites on the catalyst surface.

The Effect of Water Vapor on Mercury Oxidation over the Ce-Mn-Fe/GO-20% Catalyst
Under the simulated flue gas (SFG), the E oxi is 98.6% (0% H 2 O) and the effect of water vapor on Hg 0 oxidation was explored.The result is shown in Figure 8, in which it can be seen that the water vapor exhibits an inhibitory effect on Hg 0 oxidation.The 5% water vapor was added to the simulated flue gas.The E oxi decreases from 98.6% to 81.3%, which is probably due to the existence of water on the active sites available for mercury adsorption [53].Fortunately, the catalyst has better properties of water resistance when compared with others (Ce-Mn-Fe/GO-0, Ce-Mn-Fe/GO-10% and Ce-Mn-Fe/GO-30%).Hence, the catalyst has a potential application in the humid flue gas environment.Besides, the effect of NH 3 on Hg 0 removal was investigated, and adding 800 ppm NH 3 to the SFG caused the E oxi to decrease slightly.NO should be considered because NO reacts with NH 3 over the catalyst, and NH 3 displays a slight inhibitory effect on Hg 0 removal.

Effect of Individual Flue Gas Components on NO
x Removal over the Ce-Mn-Fe/GO-20% Catalyst under NH 3 Additionally, the effects of SO 2 and H 2 O have been explored, under operating conditions, on NO x removal, and the results were demonstrated in Figure 9. SO 2 has an adverse effect on NO x removal when 300 ppm SO 2 is included in the simulated flue gas (SFG), and η decreased from 97% to 83% and further decreased to 78% when the concentration of SO 2 increased to 600 ppm.Then, cutting off SO 2 , the efficiency recovered slightly.The main reason is that the SO 2 can combine with NH 3 to form ammonium sulfate and cover the surface of the catalyst to inhibit the reaction, resulting in a decrease of catalytic activity.Water vapor presented an inhibitive effect on η over Ce-Mn-Fe/GO-20% when 6% of water vapor was added to the simulated flue gas, and η gradually decreased from 97% to 83%.The competitive adsorption between H 2 O and NH 3 on the surface of the catalyst could account for the deactivation [54].It is worth noting that the conversion can recover soon after cutting off the H 2 O injection.Catalysts 2018, 8, x FOR PEER REVIEW 11 of 16 Figure 9.The influence of SO2 and H2O on de-NOx performance over the Ce-Mn-Fe/GO-20% sample.

Proposed Hg 0 Oxidation Mechanism
The adsorption mechanism of Hg 0 can be described by the following reactions [55]: (3) where MxOy can be seen as FexOy, MnxOy, and CexOy.The existence of MxOy−1 in the catalyst implies the formation of oxygen vacancy, which can be the adsorption sites for gas phase oxygen to form active oxygen over the catalyst surface.In this work, MnxOy and CexOy were the active components and played an important role in the adsorption of Hg 0 .In the adsorption process, Hg 0 adsorption on Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) is a dynamic process: First, the Hg 0 (g) forms Hg(ads), and then, MnxOy and CexOy offer lattice oxygen for the oxidation of Hg(ads).

Regeneration
The most outstanding of the above samples is Ce-Mn-Fe/GO-20%.After 6 h, the Hg 0 and NOx removal efficiencies reduced to 54% and 46%, respectively.To explore the active regeneration of the catalyst, the methods of heating to 400 °C in an atmosphere of nitrogen was employed.However, as Figure 10 shows, with the increase of cycling time, the Hg 0 and NOx removal performance decreased slightly.After the third circulation, the regeneration capacity of Hg 0 and NOx removal reached 85%, so that the regeneration capacity of Ce-Mn-Fe/GO-x highlights its potential applications in the future.

Proposed Hg 0 Oxidation Mechanism
The adsorption mechanism of Hg 0 can be described by the following reactions [55]: Hg 0 (g) + Surface → Hg(ad) (2) where M x O y can be seen as Fe x O y , Mn x O y , and Ce x O y .The existence of M x O y−1 in the catalyst implies the formation of oxygen vacancy, which can be the adsorption sites for gas phase oxygen to form active oxygen over the catalyst surface.In this work, Mn x O y and Ce x O y were the active components and played an important role in the adsorption of Hg 0 .In the adsorption process, Hg 0 adsorption on Ce-Mn-Fe/GO-x (x = 0, 10%, 20%, 30%) is a dynamic process: First, the Hg 0 (g) forms Hg(ads), and then, Mn x O y and Ce x O y offer lattice oxygen for the oxidation of Hg(ads).

Regeneration
The most outstanding of the above samples is Ce-Mn-Fe/GO-20%.After 6 h, the Hg 0 and NO x removal efficiencies reduced to 54% and 46%, respectively.To explore the active regeneration of the catalyst, the methods of heating to 400 • C in an atmosphere of nitrogen was employed.However, as Figure 10 shows, with the increase of cycling time, the Hg 0 and NO x removal performance decreased slightly.After the third circulation, the regeneration capacity of Hg 0 and NO x removal reached 85%, so that the regeneration capacity of Ce-Mn-Fe/GO-x highlights its potential applications in the future.

Catalyst Preparation
The title composites of Ce-Mn-Fe/GO-x catalysts were synthesized by a hydrothermal method.The commercially available chemicals are reagent grade, and the GO was purchased from Qingdao Tianhe Graphite, Qingdao, China.A mixture of Ce(NO3)3⋅6H2O, Mn(NO3)2⋅6H2O, and Fe(NO3)3⋅9H2O, with a molar ratio of 1:1:1(0.001mol Ce(NO3)3⋅6H2O, and 0.001 mol Mn(NO3)2⋅6H2O, 0.001 mol Fe(NO3)3⋅9H2O), respectively, was employed.The reagents were dissolved in 70 mL deionized water and placed inside a 100 mL autoclave with 0, 0.1, 0.2, and 0.3 g GO, respectively.Then, the autoclave was heated inside a furnace to 180 °C for 24 h and slowly cooled to room temperature at a rate of 10 °C/h.Further, the precursor was washed using deionized water five times, then calcined at 500 °C under N2 for 3 h.Finally, highly dispersed Ce-Mn-Fe-O nanoparticles were anchored on the surfaces of the GO, and the Ce-Mn-Fe/GO-x (x = 0%, 10%, 20%, 30%, CeOx 0.17 g, MnOx 0.68 g, FeOx 0.15 g) composites were obtained, where x is the mass percentages of GO in the composite.

Material Characterizations
The surface morphology was characterized using a scanning electron microscope (SEM:DESK V, Denton Vacuum, Cherry Hill, NJ, USA).The X-ray diffraction data were obtained while using a Bruker D2 PHASER diffractometer (Bruker Corp, Billerica, MA, USA), equipped with an incident beam monochromator set for Cu Kα radiation (λ = 1.5418Å).Diffraction patterns were taken from 10° to 80° (2θ), with a scan step width of 0.02°, and a fixed counting time of 1 s/step.The surface property was analyzed by X-ray photoelectron spectroscopy (XPS), while using a VG Multilab 2000 X-ray photoelectron spectrometer (Thermo Fisher Scientific, Waltham, MA, USA), with Al Kα as the excitation source.The C1s line at 284.8 eV was taken as a reference for binding energy calibration, and experimental data were fitted with the Gaussian-Lorentzian mixed function, as implemented in the XPS software.The specific surface areas of the catalysts were determined while using the BET method, the pore volume and pore size were calculated by the Brunauer-Emmett-Teller (BET) method (Quantachrome, Boynto Beach, FL, USA).The temperature-programmed reduction (H2-TPR) experiments were tested by Chembet Pulsar TPR/TPD 2139 (Quantachrome, Boynto Beach, FL, USA) to study the reducibility of catalysts.

Hg 0 Removal Test
A lab-scale fixed-bed (the inner diameter, height, and thickness is 25 mm, 300 mm, and 2 mm,

Catalyst Preparation
The title composites of Ce-Mn-Fe/GO-x catalysts were synthesized by a hydrothermal method.The commercially available chemicals are reagent grade, and the GO was purchased from Qingdao Tianhe Graphite, Qingdao, China.A mixture of Ce(NO 3 ) 3 •6H 2 O, Mn(NO 3 ) 2 •6H 2 O, and Fe(NO 3 ) 3 •9H 2 O, with a molar ratio of 1:1:1(0.001mol Ce(NO 3 ) 3 •6H 2 O, and 0.001 mol Mn(NO 3 ) 2 •6H 2 O, 0.001 mol Fe(NO 3 ) 3 •9H 2 O), respectively, was employed.The reagents were dissolved in 70 mL deionized water and placed inside a 100 mL autoclave with 0, 0.1, 0.2, and 0.3 g GO, respectively.Then, the autoclave was heated inside a furnace to 180 • C for 24 h and slowly cooled to room temperature at a rate of 10 • C/h.Further, the precursor was washed using deionized water five times, then calcined at 500 • C under N 2 for 3 h.Finally, highly dispersed Ce-Mn-Fe-O nanoparticles were anchored on the surfaces of the GO, and the Ce-Mn-Fe/GO-x (x = 0%, 10%, 20%, 30%, CeO x 0.17 g, MnO x 0.68 g, FeO x 0.15 g) composites were obtained, where x is the mass percentages of GO in the composite.

Material Characterizations
The surface morphology was characterized using a scanning electron microscope (SEM:DESK V, Denton Vacuum, Cherry Hill, NJ, USA).The X-ray diffraction data were obtained while using a Bruker D2 PHASER diffractometer (Bruker Corp, Billerica, MA, USA), equipped with an incident beam monochromator set for Cu Kα radiation (λ = 1.5418Å).Diffraction patterns were taken from 10 • to 80 • (2θ), with a scan step width of 0.02 • , and a fixed counting time of 1 s/step.The surface property was analyzed by X-ray photoelectron spectroscopy (XPS), while using a VG Multilab 2000 X-ray photoelectron spectrometer (Thermo Fisher Scientific, Waltham, MA, USA), with Al Kα as the excitation source.The C 1s line at 284.8 eV was taken as a reference for binding energy calibration, and experimental data were fitted with the Gaussian-Lorentzian mixed function, as implemented in the XPS software.The specific surface areas of the catalysts were determined while using the BET method, the pore volume and pore size were calculated by the Brunauer-Emmett-Teller (BET) method (Quantachrome, Boynto Beach, FL, USA).The temperature-programmed reduction (H 2 -TPR) experiments were tested by Chembet Pulsar TPR/TPD 2139 (Quantachrome, Boynto Beach, FL, USA) to study the reducibility of catalysts.

Hg 0 Removal Test
A lab-scale fixed-bed (the inner diameter, height, and thickness is 25 mm, 300 mm, and 2 mm, respectively) reaction system was assembled to evaluate the performance of the catalytic oxidation of Hg 0 , as shown in Figure 11.In each test, a 2.4 mL sample with a 40-60 mesh size was loaded in the reactor, which was placed in the center of a temperature-programmable electric furnace.A Hg 0 permeation tube, loaded in a U-shaped glass tube, was used to generate Hg 0 vapor carried by pure N 2 .The concentration of the Hg 0 feed (45 µg•m −3 ) was provided steadily, and the concentration of Hg 0 was measured while using a Thermo Fisher mercury continuous emission monitoring system (Hg 0 CEMS).Other simulated gases, including NO, O 2 , SO 2 , H 2 O, and NH 3 , were introduced into the gas mixer at constant flow rates, controlled by mass flow controllers.The total flow rate was kept at 2 L/min for the accuracy of the experiment, and the calculated space velocity for the tests was 30,000 h −1 .In every test, the mercury inlet gas stream bypassed the reaction bed and passed into the analytical system, until the desired inlet mercury concentration was established, and the reaction temperature was controlled from 100 to 400 C by a temperature-programmed control.The outlet Hg 0 concentration was measured at the condition of the gas flow, which was passed through the reactor.Hence, the Hg 0 removal efficiency (E oxi ) was calculated according to Equation ( 6): where Hg 0 in and Hg 0 out are the inlet and outlet of Hg 0 concentration, respectively, which were measured by CEMS.
Catalysts 2018, 8, x FOR PEER REVIEW 13 of 16 reactor, which was placed in the center of a temperature-programmable electric furnace.A Hg 0 permeation tube, loaded in a U-shaped glass tube, was used to generate Hg 0 vapor carried by pure N2.The concentration of the Hg 0 feed (45 μg•m −3 ) was provided steadily, and the concentration of Hg 0 was measured while using a Thermo Fisher mercury continuous emission monitoring system (Hg 0 CEMS).Other simulated gases, including NO, O2, SO2, H2O, and NH3, were introduced into the gas mixer at constant flow rates, controlled by mass flow controllers.The total flow rate was kept at 2 L/min for the accuracy of the experiment, and the calculated space velocity for the tests was 30,000 h −1 .In every test, the mercury inlet gas stream bypassed the reaction bed and passed into the analytical system, until the desired inlet mercury concentration was established, and the reaction temperature was controlled from 100 to 400 °C by a temperature-programmed control.The outlet Hg 0 concentration was measured at the condition of the gas flow, which was passed through the reactor.Hence, the Hg 0 removal efficiency (Eoxi) was calculated according to Equation ( 6):

NH3-SCR Catalytic Activity Measurement
The NH3-SCR of NOx experiments were performed according to the procedures employed in the Hg 0 oxidation tests (Figure 11).The 2.4 mL sample was placed into the reactor, and the reactant gas typically consisted of 800 ppm NO, 800 ppm NH3, and 6% O2.Moreover, N2 was employed as the balanced atmosphere in the reaction system.The reaction temperature was controllable from 100 to 400 °C at a heating rate of 5 °C/min.An infrared gas analyzer (GASMET DX4000, Temet Instruments Oy, Helsinki, Finland) was used to check for a gas component in the outlet of the flue gas.Conversion was calculated according to Equation (7): where [NOx]in and [NOx]out refer to the inlet and outlet of NOx concentration, respectively.η is the reduction efficiency of NOx.All the concentrations were measured by an infrared gas analyzer.

NH 3 -SCR Catalytic Activity Measurement
The NH 3 -SCR of NO x experiments were performed according to the procedures employed in the Hg 0 oxidation tests (Figure 11).The 2.4 mL sample was placed into the reactor, and the reactant gas typically consisted of 800 ppm NO, 800 ppm NH 3 , and 6% O 2 .Moreover, N 2 was employed as the balanced atmosphere in the reaction system.The reaction temperature was controllable from 100 to 400 • C at a heating rate of 5 • C/min.An infrared gas analyzer (GASMET DX4000, Temet Instruments Oy, Helsinki, Finland) was used to check for a gas component in the outlet of the flue gas.Conversion was calculated according to Equation ( 7):

Figure 2 .
Figure 2. The element contents on the surface of graphene oxide (EDS) and scanning electron microscope (SEM) images of Ce-Mn-Fe/GO-20%.

Figure 2 .
Figure 2. The element contents on the surface of graphene oxide (EDS) and scanning electron microscope (SEM) images of Ce-Mn-Fe/GO-20%.

Figure 8 .
Figure 8.Effect of the flue gas components on Hg 0 removal over the Ce-Mn-Fe/GO-20% sample at 170 °C.
Hg 0 oxidation efficiencies (average value of one hour) over the Ce-Mn-Fe/GO-20% catalyst at 170 • C, under different flue gas components, are shown in Figure 8.

Figure 8 .
Figure 8.Effect of the flue gas components on Hg 0 removal over the Ce-Mn-Fe/GO-20% sample at 170 °C.

Figure 8 .
Figure 8.Effect of the flue gas components on Hg 0 removal over the Ce-Mn-Fe/GO-20% sample at 170 • C.

Figure 9 .
Figure 9.The influence of SO 2 and H 2 O on de-NO x performance over the Ce-Mn-Fe/GO-20% sample.

Figure 10 .
Figure 10.Regeneration performance of the sorbent for Hg 0 and NOx removal efficiency.

Figure 10 .
Figure 10.Regeneration performance of the sorbent for Hg 0 and NO x removal efficiency.

0
Hg out are the inlet and outlet of Hg 0 concentration, respectively, which were measured by CEMS.

Figure 11 .
Figure 11.Schematic diagram of the experimental setup.

Figure 11 .
Figure 11.Schematic diagram of the experimental setup.