In Situ Removal of Benzene as a Biomass Tar Model Compound Employing Hematite Oxygen Carrier

: Tar is an unavoidable biomass gasiﬁcation byproduct. Tar formation reduces gasiﬁcation efﬁciency and limits the further application of biomass gasiﬁcation technology. Hence, efﬁcient tar removal is a major problem to be solved in the formation and application of biomass gasiﬁcation technology. Chemical looping gasiﬁcation (CLG), a novel and promising gasiﬁcation technology has attracted extensive attention owing to its low tar generation. Active oxygen carriers (OCs), the reduced OC in CLG, are considered to be excellent catalysts for tar cracking. In this study, the use of benzene as a typical tar model compound for tar removal using the iron ore OC is investigated. In the blank experiment, where an inert material (SiO 2 ) is used as the carrier, the benzene cracking is relatively low, and the benzene conversion, H 2 yield, and carbon conversion are 53.65%, 6.33%, and 1.24%, respectively. The addition of hematite promotes benzene cracking. A large amount of oxygen-containing gases (CO and CO 2 ) are generated. Additionally, the conversion degrees for benzene, H 2 and carbon are about 67.75%, 21.55%, and 38.39%, respectively. These results indicate that hematite performs both oxidation and catalysis during benzene cracking. The extension of the residence time facilitates benzene removal, owing to the good interaction between the gas phase and solid phase. The addition of water vapor inhibits the benzene conversion and promotes the conversion of carbon deposition. The lattice oxygen reactivity of hematite OC shows an uptrend as the cycle number is increased during the benzene conversion cycle. The experimental results conﬁrm that CLG has a low-tar advantage and that hematite is an effective OC for benzene removal.


Introduction
China's renewable energy source is equivalent to 2.15 billion standard coal, of which over 50% is biomass energy, which is two times as powerful as hydro energy and three and a half times as powerful as wind energy [1]. Biomass offers a significant advantage over fossil fuels in terms of CO 2 emission reduction. For instance, the CO 2 emissions of a biomass-fired plant with a capacity of 25,000 kW are 220 thousand tons less than that of a coal-fired plant. Additionally, biomass is a low-sulfur, low-nitrogen, and low-ash energy source with reduced environmental pollution levels during utilization [2,3]. Owing to the many similarities between biomass and fossil fuel, including molecular structure and utilization route, the industrial system of fossil fuel can be used for biomass conversion with minor adjustments, generating solid, liquid, and gas fuel or industrial raw materials. With the goal of carbon neutrality, it is crucial to advance biomass energy technology.
One of the practical technologies for biomass utilization is gasification, which converts biomass to syngas via thermo-chemical conversion [4]. Syngas mainly includes CO and minor adjustments, generating solid, liquid, and gas fuel or industrial raw materials. With the goal of carbon neutrality, it is crucial to advance biomass energy technology.
One of the practical technologies for biomass utilization is gasification, which converts biomass to syngas via thermo-chemical conversion [4]. Syngas mainly includes CO and H2, which can be used to generate heat and power and as a platform compound for the synthesis of liquid fuels and chemicals [5][6][7]. Biomass gasification has several advantages including high efficiency, low emissions, and simplicity of integration [8]. However, a significant drawback of the conventional gasification process is the high cost of oxygen sources. During gasification, solid fuel is partially oxidized, and air, oxygen, and H2O steam are commonly used as gasified agents [9]. Using air as a gasification medium will result in the low heating value of the gas products because of nitrogen dilution [10]; using oxygen is beneficial for obtaining high heating-value gas products, but the high cost of oxygen separation cannot be ignored [11]; producing H2O steam requires an external boiler, which consumes a lot of energy [12,13]. Additionally, tar, which accounts for 5%~15% of total energy in raw biomass, is a byproduct of gasification [14]. Therefore, it is crucial to design a biomass gasification method that has a low-cost oxygen source, produces less tar, and produces high-heating-value gas products.
Chemical looping gasification (CLG) is an effective solution for the abovementioned biomass gasification technology demand [15][16][17]. As shown in Figure 1, typical gasification is decomposed into two steps in CLG. In the fuel reactor (FR), the metal oxide is used as the oxygen carrier (OC) [18][19][20][21][22][23][24][25], which serves the dual purpose of oxidation and catalysis in the gasification [26]. The OC catalyzes to facilitate biomass gasification as well as a lattice oxygen source to replace molecular oxygen. After reacting with biomass, the OC is reduced, and it is then sent to the air reactor for air calcining to regenerate. Thereafter, the OC reenters the FR and AR cycle, as well as creating a reduction and oxidation loop (chemical looping). CLG does not require high-cost production of pure oxygen or water steam, and the regulation of syngas components can be achieved by introducing CO2/H2O. Additionally, the OC effectively promotes tar conversion, which is a great advantage for the thermo-chemical conversion of highly volatile solid fuels such as biomass. Biomass tar is a complex mixture, which consists of several polycyclic organic compounds. The major compositions of biomass tar are presented in Table 1. Benzene accounts for the highest proportion of tar compositions, and the majority of other compositions are benzene derivatives [27]. The benzene ring is common to see in the molecular structure of tar compounds, and this phenomenon might be attributed to the extreme stability of the benzene ring [28,29]. Both benzene and naphthalene barely decompose below Biomass tar is a complex mixture, which consists of several polycyclic organic compounds. The major compositions of biomass tar are presented in Table 1. Benzene accounts for the highest proportion of tar compositions, and the majority of other compositions are benzene derivatives [27]. The benzene ring is common to see in the molecular structure of tar compounds, and this phenomenon might be attributed to the extreme stability of the benzene ring [28,29]. Both benzene and naphthalene barely decompose below 900 • C, and their decompositions are not significant until 1000 • C. Moreover, the thermal stability of benzene is higher than that of naphthalene [30]. According to certain studies, naphthalene must undergo a complete breakdown at a reaction temperature higher than 1300 • C, while benzene must undergo a complete decomposition at a reaction temperature higher than Catalysts 2022, 12, 1088 3 of 13 1400 • C [31]. It can be inferred that the decomposition of benzene is a key barrier to the complete conversion of biomass tar because benzene is present in large amounts and has nearly the highest thermal stability. Currently, several methods have been suggested for benzene elimination in gasification. These methods include catalytic steam reforming [32,33], photothermal steam reforming [34], steam-oxygen gasification [35,36], microwave-based treatment [37], and plasma technology [38,39]. Only a few studies in the literature report the in situ removal of benzene in CLG. To investigate the effect of CLG operation on the tar conversion, benzene was used as the biomass tar model compound in the CLG experiments to simulate the in situ removal of biomass tar decomposition using a fixed bed reactor, and hematite was employed as the OC. The effects of residence time, steam/carbon ratio, and cycle number on benzene conversion were investigated. The results provide some important references for biomass tar elimination in CLG operation.

Benzene Conversion Characteristics Using Hematite
The characteristics of benzene cracking between inert SiO 2 and hematite were compared to highlight the role of iron ore OC, as shown in Figure 2 and Tables 2-5. The hematite mass, benzene flow, and N 2 flow were set as 0.5 g, 40 mL/min, and 0.05 mL/min, respectively. The total reaction time was 60 min, and each point was collected every 3 min using a sampling bag. In the blank experiment (using SiO2), the gas concentrations were low, the main gas component was H2 (95.40%) and the CH4 (3.91%) and C2Hm (0.69%) contents were low. The oxygenated gases (CO and CO2) were not observed. H2 concentration increased grad-    In the blank experiment (using SiO 2 ), the gas concentrations were low, the main gas component was H 2 (95.40%) and the CH 4 (3.91%) and C 2 H m (0.69%) contents were low. The oxygenated gases (CO and CO 2 ) were not observed. H 2 concentration increased gradually in the first 30 min before stabilizing. Additionally, the benzene conversion, H 2 yield, and carbon deposition were 55.37%, 7.22%, and 1.98%, respectively. These results indicate that the self-cracking performance of benzene at high temperatures was low, since the inert SiO 2 carrier had no oxidation and catalysis ability. During this process, the reaction (R1) played a major role [41]. Although the benzene conversion was 55.37%, the majority of benzene only partially cracked and only a small portion of its C-H/C-C bonds was completely broken. Thus, the H 2 yield (gas product) and carbon deposition (solid product) were very low, and a large amount of benzene series (liquid product) was generated, as shown in (R2). Benzene dehydrogenation mostly generates benzene radicals, which later combine with other radicals to form a new, larger benzene series. The mass of the generated liquid products was 1.20 g and the main component (biphenyl) accounted for 75.83% of that mass.
However, hematite addition accelerated the benzene cracking. Along with the H 2 , CH 4 , and C 2 H m , a large amount of oxygen-containing gases (CO and CO 2 ) was generated. In the initial stage, a small amount of absorbed oxygen reacted with the benzene on the surface of the hematite, which leads to the formation of CO and CO 2 . After 25 min, the CO concentration increased and reached its peak at 33 min, indicating that lattice oxygen was involved in the benzene oxidation. In the final stage, lattice oxygen was absent, making it impossible to meet the oxygen demand of benzene oxidation, but part of the OC was reduced to metal Fe, which catalyzed the benzene cracking. Therefore, CO concentration declined gradually, and the H 2 concentration increased continuously.
Furthermore, compared to the blank experiment, the benzene conversion, H 2 yield and carbon deposition increased to 69.05%, 21.96%, and 39.13%, respectively. Hematite has the dual function of oxidation and catalysis. First, benzene underwent an oxidationreduction reaction with hematite to generate a large amount of oxygen-containing gas, while the hematite was reduced to metallic Fe or Fe 3 C, as shown in (R3). Subsequently, the generated Fe or Fe 3 C acted as a catalyst to catalytically crack the benzene, and large amounts of hydrogen and carbon deposits were generated, as shown in (R4). Additionally, when compared to the blank experiment, 0.55 g of liquid products were generated during the process. This was attributed to the relatively low oxidation and catalytic ability of hematite. Thus, the secondary reaction R5 occurred in the process.
Catalysts 2022, 12, x FOR PEER REVIEW 5 of 14 reduction reaction with hematite to generate a large amount of oxygen-containing gas, while the hematite was reduced to metallic Fe or Fe3C, as shown in R3. Subsequently, the generated Fe or Fe3C acted as a catalyst to catalytically crack the benzene, and large amounts of hydrogen and carbon deposits were generated, as shown in R4. Additionally, when compared to the blank experiment, 0.55 g of liquid products were generated during the process. This was attributed to the relatively low oxidation and catalytic ability of hematite. Thus, the secondary reaction R5 occurred in the process.  Table 3. Distribution of liquid products during benzene cracked by two carriers.

Mass of Liquid Products (g) Biphenyl C12H10
Meta-Terphenyl C18H14  Table 4. Distribution of carbon-containing species in the products.

The Residence Time
This section investigates the effect of residence time on benzene cracking, and the result is shown in Figure 3. The hematite mass and benzene flow were set as 0.5 g and 0.05

The Residence Time
This section investigates the effect of residence time on benzene cracking, and the result is shown in Figure 3. The hematite mass and benzene flow were set as 0.5 g and 0.05 mL/min, respectively. The total reaction time was 60 min. The residence time was adjusted by controlling the N 2 flow(40, 60, 80, 100 mL/min). The benzene conversion degree increased from 63.5% to 78.3% when the residence time increased from 0.032 to 0.08 s. Over 0.053 s, the benzene conversion increased from 78.3% to 81.1%, but at a slower rate. There was a significant positive correlation between the benzene conversion degree and the residence time. Long residence time allows for increased interaction between benzene and hematite, which is beneficial for benzene cracking. The increased conversion degree reduced slightly after 0.053 s, because the benzene-cracking capacity of the OC was close to the saturation at this condition. Carbon deposition and H2 are the typical byproducts of benzene cracking (R1), and their percentage-time curves were similar to that of the benzene conversion degree. The difference was in the period of 0.032 to 0.053 s, which showed a rapid increase in the carbon deposition and H2 yield curves. The restricted amount of lattice oxygen capacity made it increasingly difficult to completely oxidize input benzene. Therefore, there was a rapid increase in both carbon deposition and H2 yield.
The main gas components were H2 and CO. A small amount of CH4 and CO2 was observed when the residence time was above 0.04 s. Over the residence time, the H2 concentration increased from 12.5% to 31.9%, and the CO concentration increased from 1.9% to 4.4%. As the residence time increased, the lattice oxygen was depleted, and the reducing gas content increased. For the benzene cracking process, OC plays a dual role in catalysis and oxidation in the range of 0.04 to 0.053 s, but the oxidation function declines after 0.053 s because lattice oxygen was exhausted, and the reducing gas content subsequently increased. The benzene conversion degree increased from 63.5% to 78.3% when the residence time increased from 0.032 to 0.08 s. Over 0.053 s, the benzene conversion increased from 78.3% to 81.1%, but at a slower rate. There was a significant positive correlation between the benzene conversion degree and the residence time. Long residence time allows for increased interaction between benzene and hematite, which is beneficial for benzene cracking. The increased conversion degree reduced slightly after 0.053 s, because the benzene-cracking capacity of the OC was close to the saturation at this condition. Carbon deposition and H 2 are the typical byproducts of benzene cracking (R1), and their percentage-time curves were similar to that of the benzene conversion degree. The difference was in the period of 0.032 to 0.053 s, which showed a rapid increase in the carbon deposition and H 2 yield curves. The restricted amount of lattice oxygen capacity made it increasingly difficult to completely oxidize input benzene. Therefore, there was a rapid increase in both carbon deposition and H 2 yield.

H2O Steam Content
The main gas components were H 2 and CO. A small amount of CH 4 and CO 2 was observed when the residence time was above 0.04 s. Over the residence time, the H 2 concentration increased from 12.5% to 31.9%, and the CO concentration increased from 1.9% to 4.4%. As the residence time increased, the lattice oxygen was depleted, and the reducing gas content increased. For the benzene cracking process, OC plays a dual role in catalysis and oxidation in the range of 0.04 to 0.053 s, but the oxidation function declines after 0.053 s because lattice oxygen was exhausted, and the reducing gas content subsequently increased.

H 2 O Steam Content
H 2 O steam is usually used as a gasifying agent to promote biomass gasification. The effect of H 2 O steam on benzene conversion degree, H 2 yield, and carbon deposition was investigated, and the Steam/Carbon ratio (S/C) was set in a range of 0.49-1.14. The results are presented in Figure 4. The hematite mass, benzene flow, and N 2 flow were set as 0.5 g, 60 mL/min, and 0.03 mL/min, respectively. The total reaction time was 60 min. The residual solid products were analyzed by X-ray diffraction (XRD, X'Pert Pro MPD) and Cu Kα radiation (λ = 0.1504 nm) at a voltage of 40 kV and a current of 40 mA. The scanning rate was 2 • /min from 2θ = 5 • to 80 • at a step of 0.02 • .  H2O steam inhibited the benzene decomposition, and the benzene conversion degree reduced from 81.8% to 66.8% when the S/C value increased from 0.49 to 1.14. According to R1~R4, benzene was decomposed with the release of H2, as well as carbon deposition. As the benzene conversion degree decreased, H2 yield reduced from 55.5% to 3.7%, while carbon deposition reduced from 35.7% to 0.33%.
There were two possible reasons for the H2O inhabitation of the benzene decomposition. First, in our experimental devices, liquid H2O was pumped into the reactor where it was gasified to H2O steam because of the high internal temperature. The H2O gasification had a significant impact on the gas flow in the reactor, resulting in a higher flow through the quartz tube. Consequently, the residence time of benzene and its decomposition products was shortened leading to a decrease in the benzene conversion degree. Second, the introduction of H2O steam enhanced the oxidation performance of the atmosphere, leading to OC reduction. Thereafter, the catalysis effect, which was dependent on the reduced OC, diminished as a result of the reduced OC formation. C/Fe3C + H2O → CO/CO2+H2+Fe ∆H > 0 (R5) Figure 5 shows the variation in the XRD pattern of the reduced OC when the S/C value increased from 0.49 to 0.81. When the S/C value was set at 0.49, the reduced OC primarily contained metal Fe, carbon, and Fe3C. Carbon and Fe3C vanished as the S/C value was increased to 0.66. Metal Fe was the dominant phase, and its signal intensity was reduced relative to that of the S/C value of 0.49. When the S/C value was increased to 0.81, the signal intensity of metal Fe decreased further, and FeO1-δ was observed in the spectrum. The above phenomenon indicated that H2O first reacted with carbon deposition and Fe3C before oxidizing into FeO1-δ when the carbon was used up. Upon the metal Fe oxidation, the catalysis effect of the OC decreased, resulting in a lower benzene conversion degree. Therefore, the S/C should be set at a level that allows for sufficient elimination for carbon deposition, and little oxidation to the reduced OC, at the same time. When the S/C value reached 0.66, the Fe3C pattern was too weak to be observed, and the OC maintained an almost completed reduced state. Therefore, the S/C value was set at 0.66 for the cyclic experiments. H 2 O steam inhibited the benzene decomposition, and the benzene conversion degree reduced from 81.8% to 66.8% when the S/C value increased from 0.49 to 1.14. According to (R1)~(R4), benzene was decomposed with the release of H 2 , as well as carbon deposition. As the benzene conversion degree decreased, H 2 yield reduced from 55.5% to 3.7%, while carbon deposition reduced from 35.7% to 0.33%.
There were two possible reasons for the H 2 O inhabitation of the benzene decomposition. First, in our experimental devices, liquid H 2 O was pumped into the reactor where it was gasified to H 2 O steam because of the high internal temperature. The H 2 O gasification had a significant impact on the gas flow in the reactor, resulting in a higher flow through the quartz tube. Consequently, the residence time of benzene and its decomposition products was shortened leading to a decrease in the benzene conversion degree. Second, the introduction of H 2 O steam enhanced the oxidation performance of the atmosphere, leading to OC reduction. Thereafter, the catalysis effect, which was dependent on the reduced OC, diminished as a result of the reduced OC formation. C/Fe 3 C + H 2 O → CO/CO 2 + H 2 + Fe ∆H > 0 (R5) Figure 5 shows the variation in the XRD pattern of the reduced OC when the S/C value increased from 0.49 to 0.81. When the S/C value was set at 0.49, the reduced OC primarily contained metal Fe, carbon, and Fe 3 C. Carbon and Fe 3 C vanished as the S/C value was increased to 0.66. Metal Fe was the dominant phase, and its signal intensity was reduced relative to that of the S/C value of 0.49. When the S/C value was increased to 0.81, the signal intensity of metal Fe decreased further, and FeO 1−δ was observed in the spectrum. The above phenomenon indicated that H 2 O first reacted with carbon deposition and Fe 3 C before oxidizing into FeO 1−δ when the carbon was used up. Upon the metal Fe oxidation, the catalysis effect of the OC decreased, resulting in a lower benzene conversion degree. Therefore, the S/C should be set at a level that allows for sufficient elimination for carbon deposition, and little oxidation to the reduced OC, at the same time. When the S/C value reached 0.66, the Fe 3 C pattern was too weak to be observed, and the OC maintained an almost completed reduced state. Therefore, the S/C value was set at 0.66 for the cyclic experiments.   Figure 6a depicts the morphology of the original OC. There were massive blocks distributed in the picture with a few small blocks adhering to the surface. These blocks were made up specifically of the reduced OC particle. After reacting with benzene, the OC particle agglomerated into blocks with a smooth edge, and some tubes, overlapping on the surface of the blocks, crossed over with each other, as shown in Figure 6b. These microtubes had distinct structures from the OC blocks. According to the fixed bed experiments, a large amount of carbon deposition was found in the reduced OC, and these microtubes could be formed from the carbon nanotube polymer, which was generated during the carbon deposition (R1 and R4). Similar results were found in the literature [42]. The carbon microtubes disappeared when H2O steam was introduced into the reaction (R5). Carbon deposition was converted to CO/CO2 when it reacted with H2O. Figure 6c depicted the morphology of the microtube-free OC. After reacting to H2O steam, the OC structure became loose and irregular, and the carbon microtubes were not observed in the image.    Figure 6a depicts the morphology of the original OC. There were massive blocks distributed in the picture with a few small blocks adhering to the surface. These blocks were made up specifically of the reduced OC particle. After reacting with benzene, the OC particle agglomerated into blocks with a smooth edge, and some tubes, overlapping on the surface of the blocks, crossed over with each other, as shown in Figure 6b. These microtubes had distinct structures from the OC blocks. According to the fixed bed experiments, a large amount of carbon deposition was found in the reduced OC, and these microtubes could be formed from the carbon nanotube polymer, which was generated during the carbon deposition ((R1) and (R4)). Similar results were found in the literature [42]. The carbon microtubes disappeared when H 2 O steam was introduced into the reaction (R5). Carbon deposition was converted to CO/CO 2 when it reacted with H 2 O. Figure 6c depicted the morphology of the microtubefree OC. After reacting to H 2 O steam, the OC structure became loose and irregular, and the carbon microtubes were not observed in the image.   Figure 6a depicts the morphology of the original OC. There were massive blocks distributed in the picture with a few small blocks adhering to the surface. These blocks were made up specifically of the reduced OC particle. After reacting with benzene, the OC particle agglomerated into blocks with a smooth edge, and some tubes, overlapping on the surface of the blocks, crossed over with each other, as shown in Figure 6b. These microtubes had distinct structures from the OC blocks. According to the fixed bed experiments, a large amount of carbon deposition was found in the reduced OC, and these microtubes could be formed from the carbon nanotube polymer, which was generated during the carbon deposition (R1 and R4). Similar results were found in the literature [42]. The carbon microtubes disappeared when H2O steam was introduced into the reaction (R5). Carbon deposition was converted to CO/CO2 when it reacted with H2O. Figure 6c depicted the morphology of the microtube-free OC. After reacting to H2O steam, the OC structure became loose and irregular, and the carbon microtubes were not observed in the image.    Figure 7 shows the variations in benzene conversion during 5 chemical looping redox cycles. In the benzene conversion stage, the hematite mass, S/C, benzene flow, and N 2 flow were set as 0.5 g, 0.66, 60 mL/min, and 0.03 mL/min, respectively. The total reaction time was 60 min. In the oxidation stage, the air flow was set as 300 mL/min for 30 min.  Figure 7 shows the variations in benzene conversion during 5 chemical looping redox cycles. In the benzene conversion stage, the hematite mass, S/C, benzene flow, and N2 flow were set as 0.5 g, 0.66, 60 mL/min, and 0.03 mL/min, respectively. The total reaction time was 60 min. In the oxidation stage, the air flow was set as 300 mL/min for 30 min. The benzene conversion degree increased from 63.9% to 74.4% as the cycle number increased. The H2 yield increased from 13.4% to 43.2%, and the carbon deposition increased from 5.8% to 31.0%. This improvement was attributed to the increase in the catalytic effect of OC, which could be observed in the H2 yield and carbon deposition figures.

The Cycle Numbers
The multiple cycles were divided into two stages. In stage I, rapid increases in H2 yield and carbon deposition were observed in the 2nd cycle. The H2 yield and carbon deposition of the 2nd cycle were more than twice those of the 1st cycle. However, compared to that of the 2nd cycle, the benzene conversion degree of the 1st cycle only increased by about 10%. The benzene conversion could not have increased at the same time that H2 yield and carbon deposition were increasing so rapidly. It ought to be related to the further decomposition of medium products generated from the benzene cracking. According to Section 3.3, it could be inferred that the OC was almost reduced to metal Fe. A serious agglomeration would happen to the OC after reduction, resulting in the deactivation of the OC. Lattice oxygen could not be recovered as completely as in the original, and a part of low-valence Fe oxides was exposed to benzene, improving the catalytic effect of the OC. Consequently, the medium products generated from the benzene cracking could be further decomposed by such an OC, leading to a higher H2 yield and a higher carbon deposition. In stage II, the primary effect was eliminated during stage I, and the OC performance was stable. The catalytic effect of the OC gradually increased as the cycle number increased, and the benzene conversion degree also increased. Figure 8 shows the influence of cycle number on relative concentration of gas products and H2/CO ratio. As the cycle number increased from 1 to 4, the H2 concentration increased from 56.6% to 61.2%, and the CO and CO2 concentration decreased from 38.8% to 35.5% and from 4.4% to 3%, respectively. This variation in gas-product relative concentration indicated that the lattice oxygen gradually deactivated after multiple redox cycles. The oxidative performance of the OC was declined, while the catalytic performance was improved. Therefore, the H2 yield, carbon deposition, and H2/CO ratio all increased after multiple redox cycles. The benzene conversion degree increased from 63.9% to 74.4% as the cycle number increased. The H 2 yield increased from 13.4% to 43.2%, and the carbon deposition increased from 5.8% to 31.0%. This improvement was attributed to the increase in the catalytic effect of OC, which could be observed in the H 2 yield and carbon deposition figures.
The multiple cycles were divided into two stages. In stage I, rapid increases in H 2 yield and carbon deposition were observed in the 2nd cycle. The H 2 yield and carbon deposition of the 2nd cycle were more than twice those of the 1st cycle. However, compared to that of the 2nd cycle, the benzene conversion degree of the 1st cycle only increased by about 10%. The benzene conversion could not have increased at the same time that H 2 yield and carbon deposition were increasing so rapidly. It ought to be related to the further decomposition of medium products generated from the benzene cracking. According to Section 3.3, it could be inferred that the OC was almost reduced to metal Fe. A serious agglomeration would happen to the OC after reduction, resulting in the deactivation of the OC. Lattice oxygen could not be recovered as completely as in the original, and a part of low-valence Fe oxides was exposed to benzene, improving the catalytic effect of the OC. Consequently, the medium products generated from the benzene cracking could be further decomposed by such an OC, leading to a higher H 2 yield and a higher carbon deposition. In stage II, the primary effect was eliminated during stage I, and the OC performance was stable. The catalytic effect of the OC gradually increased as the cycle number increased, and the benzene conversion degree also increased. Figure 8 shows the influence of cycle number on relative concentration of gas products and H 2 /CO ratio. As the cycle number increased from 1 to 4, the H 2 concentration increased from 56.6% to 61.2%, and the CO and CO 2 concentration decreased from 38.8% to 35.5% and from 4.4% to 3%, respectively. This variation in gas-product relative concentration indicated that the lattice oxygen gradually deactivated after multiple redox cycles. The oxidative performance of the OC was declined, while the catalytic performance was improved. Therefore, the H 2 yield, carbon deposition, and H 2 /CO ratio all increased after multiple redox cycles.

Hematite
In the experiments, Australian hematite was used as the OC, and its compositions are listed in Table 5. The hematite was heated from room temperature to 1100 ℃ at a heating rate of 10 ℃/min before being maintained at 1100 ℃ for 3 h. Thereafter, the hematite was naturally cooled to room temperature before being ground into a powder and sieved to a diameter less than 0.15 mm.

Fixed Bed Experiment
The fixed bed reactor is shown in Figure 9. Benzene or deionized water was injected into the valve by using a high-pressure infusion pump at a certain flow rate and a pressure of 1 atm, and the N2 or air flow was controlled by using a mass flowmeter. The quartz tube had an outer diameter of 20 mm, and inner diameter of 15 mm, and a length of 800 mm. In the middle of the quartz tube, there was a porous bezel, which carried a certain mass of quartz cotton (about 0.02 g), and the OC was placed on top of it. To avoid condensation of liquid products, a heater (150 °C) was wrapped around the line connecting the quartz tube to the gas collector and the bottom of the quartz tube, which was placed at the center of the reactor. The reaction temperature was set as 850 °C. The exit of the reactor was connected to a gas collector, which contained isopropanol. After the collection, the solution in the collector was stored at 5 °C. The gas product was collected in the sample bag for subsequent analysis. After the benzene conversion experiment, air was used to oxidize the carrier and to eliminate the carbon deposit, and the gas product was collected by using the sample bag. The amount of carbon deposit from the benzene conversion was calculated by measuring the CO and CO2 content in the gas product. The solution in the collector was transferred to a 200 mL volumetric flask. The gas and liquid products were analyzed using the Agilent 7890A gas chromatograph; the split flow was set as 10:1, the FID detector was set at 280 °C, the DB-5HT nonpolar capillary column was equipped with gas chromatograph, and the column was heated from 40 °C to 280 °C at a heating rate of 40 ℃/min.

Hematite
In the experiments, Australian hematite was used as the OC, and its compositions are listed in Table 5. The hematite was heated from room temperature to 1100°C at a heating rate of 10°C/min before being maintained at 1100°C for 3 h. Thereafter, the hematite was naturally cooled to room temperature before being ground into a powder and sieved to a diameter less than 0.15 mm.

Fixed Bed Experiment
The fixed bed reactor is shown in Figure 9. Benzene or deionized water was injected into the valve by using a high-pressure infusion pump at a certain flow rate and a pressure of 1 atm, and the N 2 or air flow was controlled by using a mass flowmeter. The quartz tube had an outer diameter of 20 mm, and inner diameter of 15 mm, and a length of 800 mm. In the middle of the quartz tube, there was a porous bezel, which carried a certain mass of quartz cotton (about 0.02 g), and the OC was placed on top of it. To avoid condensation of liquid products, a heater (150 • C) was wrapped around the line connecting the quartz tube to the gas collector and the bottom of the quartz tube, which was placed at the center of the reactor. The reaction temperature was set as 850 • C. The exit of the reactor was connected to a gas collector, which contained isopropanol. After the collection, the solution in the collector was stored at 5 • C. The gas product was collected in the sample bag for subsequent analysis. After the benzene conversion experiment, air was used to oxidize the carrier and to eliminate the carbon deposit, and the gas product was collected by using the sample bag. The amount of carbon deposit from the benzene conversion was calculated by measuring the CO and CO 2 content in the gas product. The solution in the collector was transferred to a 200 mL volumetric flask. The gas and liquid products were analyzed using the Agilent 7890A gas chromatograph; the split flow was set as 10:1, the FID detector was set at 280 • C, the DB-5HT nonpolar capillary column was equipped with gas chromatograph, and the column was heated from 40 • C to 280 • C at a heating rate of 40°C/min. Catalysts 2022, 12, x FOR PEER REVIEW 11 of 14 Figure 9. A schematic of the fixed bed experiment.

Data Processing
During the experiment, isopropanol was used to absorb the content of benzene (g/L) as part of the non-participating reaction, and the conversion degree of benzene was: In the formula: mt--------Amount of benzene fed during reaction time (g); mo-------Quality of unreacted benzene (g). The total accumulation of gas exports was calculated using the nitrogen balance. The formula was shown in (2).
In the formula: mi--------Amount of benzene fed during reaction time (g); mo-------Quality of unreacted benzene (g); mc-------Carbon mass on the surface of the OC (g), which was calculated by measuring the CO and CO2 content during the OC oxidation.
H2 yield is calculated as follows: Figure 9. A schematic of the fixed bed experiment.

Data Processing
During the experiment, isopropanol was used to absorb the content of benzene (g/L) as part of the non-participating reaction, and the conversion degree of benzene was: In the formula: m t--------Amount of benzene fed during reaction time (g); m 0-------Quality of unreacted benzene (g). The total accumulation of gas exports was calculated using the nitrogen balance. The formula was shown in (2).
In the formula: V in--------Total volume of imported nitrogen (L); V out-------Total volume of gas outlet (L); V n-------The volume fraction of the total volume of the outlet occupied by N 2 in the dry-base state.
Carbon deposition Y c (%): In the formula: m i--------Amount of benzene fed during reaction time (g); m 0-------Quality of unreacted benzene (g); m c-------Carbon mass on the surface of the OC (g), which was calculated by measuring the CO and CO 2 content during the OC oxidation.
H 2 yield is calculated as follows: In the formula: Relative concentration = y k y CO 2 + y CO + y CH 4 + y H 2 × 100% (6) where y gas is the actual concentration of gas products (CO 2 , CO, CH 4 , and H 2 ) detected by GC, and y k is the specific gas product (CO 2 , CO, CH 4 , C 2 H x , or H 2 ). The residence times are calculated as below: The residence time = V OC N 2 f low In the formula: V OC--------The volume of the OC is estimated as 0.053 cm 3 (0.5 g hematite in the quartz tube with an inner diameter of 15 mm); N 2 flow -------The volume flow of N 2 (40, 60, 80, and 100 mL/min).

Conclusions
In this study, fixed-bed reactor tests for benzene conversion using hematite as an OC were performed. In summary, hematite exhibited better benzene conversion than an inert carrier (SiO 2 ). The conclusions are as follows: (1) During benzene conversion, hematite functioned as both an oxidative and a catalytic OC. Hematite also improved the benzene conversion degree by about 20%, going from 55.37% to 69.05%. (2) As the residence time increased from 0.032 s to 0.08 s, the benzene conversion increased from 63.5% to 81.1%. However, the positive influence of the increased residence time declined when the residence time was over 0.053 s. (3) The introduction of H 2 O steam was advantageous for the removal of carbon deposition. As the S/C ratio increased from 0.49 to 1.14, the carbon deposition decreased from 35.7% to 0.33%, and H 2 O inhibited the benzene conversion, resulting in a decrease in H 2 yield. (4) A significant primary effect was observed in the multiple redox cycles. The benzene conversion increased in the 2nd cycle. The agglomeration of hematite deactivated a part of lattice oxygen vacancy, resulting in a decline in the oxidative performance of the hematite after the redox cycle. As the cycle number increased, the benzene conversion improved.