# Abatement of Toluene Using a Sequential Adsorption-Catalytic Oxidation Process: Comparative Study of Potential Adsorbent/Catalytic Materials

Shilpa Sonar, Jean-Marc Giraudon, Savita Kaliya Perumal Veerapandian, Rim Bitar, Karen Leus, Pascal van der Voort, Jean-François Lamonier, Rino Morent, Nathalie de Geyter, Axel Löfberg

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Shilpa Sonar, Jean-Marc Giraudon, Savita Kaliya Perumal Veerapandian, Rim Bitar, Karen Leus, et al.. Abatement of Toluene Using a Sequential Adsorption-Catalytic Oxidation Process: Comparative Study of Potential Adsorbent/Catalytic Materials. Catalysts, 2020, Catalysts, 10 (7), pp.761. 10.3390/catal10070761. [hal-03024480v3](https://hal-univ-lille.fr/hal-03024480v3)

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Article

# Abatement of Toluene Using a Sequential Adsorption-Catalytic Oxidation Process: Comparative Study of Potential Adsorbent/Catalytic Materials

Shilpa Sonar <fnref n="1" />,<fnref n="2" />, Jean-Marc Giraudon <fnref n="1" />, Savita Kaliya Perumal Veerapandian <fnref n="2" />, Rim Bitar <fnref n="2" />, Karen Leus <fnref n="3" />, Pascal Van Der Voort <fnref n="3" />, Jean-François Lamonier <fnref n="1" />, Rino Morent <fnref n="2" />, Nathalie De Geyter <fnref n="2" /> and Axel Löfberg <fnref n="1" />,*

Received: 12 June 2020; Accepted: 30 June 2020; Published: 8 July 2020

<figure><img src="image_2.png" /></figure>

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**Abstract:** A novel strategy for toluene abatement was investigated using a sequential adsorption-regeneration process. Commercial Hopcalite (CuMn₂Oₓ, Purelyst101MD), Ceria nanorods, and UiO-66-SO₃H, a metal-organic framework (MOF), were selected for this study. Toluene was first adsorbed on the material and a mild thermal activation was performed afterwards in order to oxidize toluene into CO₂ and H₂O. The materials were characterized by XRD, N₂ adsorption-desorption analysis, H₂-TPR and TGA/DSC. The best dynamic toluene adsorption capacity was observed for UiO-66-SO₃H due to its hierarchical porosity and high specific surface area. However, in terms of balance between storage and catalytic properties, Hopcalite stands out from others owing to its superior textural/chemical properties promoting irreversible toluene adsorption and outstanding redox properties, allowing a high activity and CO₂ selectivity in toluene oxidation. The high conversion of toluene into CO₂ which easily desorbs from the surface during heating treatment shows that the sequential adsorption-catalytic thermal oxidation can encompass a classical oxidation process in terms of efficiency, CO₂ yield, and energy-cost saving, providing that the bifunctional material displays a good stability in repetitive working conditions.

**Keywords:** adsorption; catalytic oxidation; sequential adsorption-thermal oxidation; toluene abatement; Hopcalite; nanorod Ceria; UiO-66-SO₃H

## 1. Introduction

Volatile organic compounds (VOCs) usually refer to organic compounds with boiling points less than or equal to 250 °C at atmospheric pressure and high vapor pressures (above 0.1 mm Hg) at room temperature [1,2]. Among the different types of VOCs, aromatics play an important role in stratospheric ozone depletion as well as aerosol and smog formations [3] and have adverse effects on human health [3]. Toluene, which is an important representative of aromatic VOCs, is widely

<footnote n="1">¹ Univ. Lille, CNRS, Centrale Lille, Univ. Artois, UMR 8181-UCCS-Unité de Catalyse et Chimie du Solide, F-59000 Lille, France; shilpasonar01@gmail.com (S.S.); jean-marc.giraudon@univ-lille.fr (J.-M.G.); jean-francois.lamonier@univ-lille.fr (J.-F.L.)</footnote>

<footnote n="2">² Research Unit Plasma Technology, Department of Applied Physics, Faculty of Engineering and Architecture, Ghent University, Sint-Pietersnieuwstraat 41 (B4), 9000 Ghent, Belgium; Savita.KaliyaPerumalVeerapandian@ugent.be (S.K.P.V.); Rim.Bitar@UGent.be (R.B.); Rino.Morent@UGent.be (R.M.); Nathalie.DeGeyter@UGent.be (N.D.G.)</footnote>

<footnote n="3">³ Center for Ordered Materials, Organometallics and Catalysis (COMOC), Department of Chemistry, Faculty of Sciences, Ghent University, Krijgslaan 281 (S3), 9000 Ghent, Belgium; Karen.Leus@ugent.be (K.L.); pascal.vandervoort@ugent.be (P.V.D.V.)</footnote>

<footnote>* Correspondence: axel.lofberg@univ-lille.fr</footnote>
found in indoor and outdoor air due to its use as solvent. Owing to stringent legislations on VOC emissions, various technologies, such as adsorption [4,5], absorption [6], photocatalytic degradation [7], catalytic oxidation [5,8], and catalytic combustion [8], have been extensively used to scale down the energy cost [8].

For instance, storage regeneration processes have been proposed and investigated to eliminate low-concentration indoor VOCs such as formaldehyde and benzene [9]. This sequential method implies two steps: (i) first, the VOC is adsorbed on a material and (ii) then a regeneration of the material through VOC oxidation into CO₂ and H₂O is performed. A key issue in this approach is the design of adsorbent/catalytic materials which should possess balanced properties between storage and regeneration. The bifunctional materials used for the storage of VOCs should thus not only possess high and selective VOC storage capacity, but also be easily regenerated without any release of the VOCs or generation of secondary pollutants. To that order, thermal regeneration [9], non-thermal plasma oxidation [10,11], or ozone enabled regeneration [12] have been assessed as regeneration methods.

Regarding adsorption/catalytic regeneration, Guillemot et al. reported on a double adsorbent/catalyst bed for the removal of tetrachloroethylene (PCE) and methyl ethyl ketone (MEK) in a moist gas stream. The VOCs were physically adsorbed on an appropriate adsorbent (zeolites) at room temperature. After that, the VOCs were desorbed from the adsorbent and catalytically oxidized by supported catalysts (Pt, Ag, etc.) at elevated temperature. It appeared that the adsorbent-catalyst couple remains efficient for MEK transformation during several successive adsorption/oxidation cycles [13].

In the present work, the sequential adsorption-catalytic process is proposed for the abatement of toluene as VOC. The implementation of such process requires to identify proper materials that exhibit both sufficient adsorption capacity and good catalytic performances. This can be approached by different ways, for example by adding catalytic functions to well-known adsorbents or by developing the adsorption properties of known catalytic materials. For instance, in this exploratory work, Hopcalite (Purelyst 101MD), nanorod Ceria, and a sulfonic Zr-based metal organic framework (MOF) (UiO-66-SO₃H) have been used for the adsorption-thermal catalytic removal of toluene using a mild thermal activation from 25 °C up to 250 °C.

Hopcalite (CuMnOₓ), a cost-effective catalyst, consists of a mixture of copper and manganese oxides [14]. It is recognized as one of the most efficient catalyst for low-temperature oxidation reactions such as CO oxidation [14], indoor HCHO oxidation [15], and VOC total oxidation. As a consequence, Hopcalite is widely used for respiratory protection systems for various types of applications like military, mining and space devices, etc. [16]. The high catalytic activity in CO oxidation over CuMnOₓ catalyst has been ascribed previously to the redox reaction Cu²⁺ + Mn³⁺ ⇌ Cu⁺ + Mn⁴⁺ and the high adsorption of CO onto Cu²⁺/Mn⁴⁺ and of O₂ onto Cu⁺/Mn³⁺ [14]. It should be noted that the mesoporous Cu–Mn Hopcalite catalyst is generally highly active in the amorphous state, but loses its catalytic activity at high temperature (>500 °C) owing to the generation of crystallized phase [14].

Cerium oxide (CeO₂) is widely investigated as a catalyst or catalyst support for various applications in the field of environmental catalysis, in particular three-way catalysis. Ceria nanoparticles (Ceria NPs) have unique redox properties of easy cycling between the Ce⁴⁺ and Ce³⁺ oxidation states. As a consequence, the high oxygen storage/release capacity makes this material a key ingredient for catalytic oxidation reactions. The enhancement of defects linked to the morphology, size, and shape of cerium oxide is known to promote catalytic activity. In that respect, NPs of CeO₂ nanorods (NR) exposing surface (110) and (100) planes exhibit enhanced catalytic properties in CO oxidation [17].

UiO-66-SO₃H (UiO: University of Oslo) is a metal organic frameworks (MOF) isostructural with UiO-66 and can be synthesized easily via a direct solvothermal approach [18]. MOFs exhibit tunable structures, large surface areas and multifunctional properties which have attracted increasing attention in various applications such as adsorption [19], catalytic oxidation [20,21], and photocatalysis [22]. MOFs might be considered as a potential alternative to zeolites and active carbons in adsorption
technologies. UiO-66-SO3H is an acid MOF used in acid-basic reactions which also shows high performance in terms of CO2 adsorption capacity.

In the present paper, adsorption-desorption/oxidation of gaseous toluene on the two calcined materials (Hopcalite and CeO₂ nanorods) and activated MOF was investigated by breakthrough experiments followed by toluene desorption experiments at ambient temperature to be ended by temperature programmed reactions (TPR). At that stage, the TP reactions were performed either in He to probe the redox properties of the materials or in a He:O₂ (50:50) gaseous mixture to assess the catalytic properties of the materials during this regeneration step. In a complementary approach, the catalytic properties were investigated from light-off curves. Finally, the adsorbent/catalyst performance of the materials was assessed and discussed in accordance with their physico-chemical properties.

**2. Results and Discussion**

**2.1. *Catalyst Characterization***

**2.1.1. Structural Properties**

The X-ray diffraction (XRD) pattern (Figure 1) of Hopcalite shows two low intensity peaks positioned at 36.7° and 66.0° in 2θ originating from some based MnO₂ spacing in line with the amorphous character of the material [23]. The XRD pattern of the as-synthesized CeO₂-NR shows well defined diffraction peaks located at 28.5°, 33.1°, 47.5°, 56.3°, 59.1°, 69.4°, 76.7°, and 79.1° ascribed to the (111), (200), (220), (311), (222), (400), (331), and (420) planes of the face-centered cubic (fcc) CeO₂ fluorite structure (JCPDS 34-0394, space group Fm3m) [24]. Using the Scherrer formula, it was found that mean crystallite size of 8 nm from the (111) peak. The XRD pattern of UiO-66-SO₃H is in good agreement with those reported previously for a crystalline activated UiO-66-SO₃H [18,25-27].

<figure><img src="image_3.png" /><figcaption>**Figure 1.** *Cont.*</figcaption></figure>
<figure><img src="image_4.png" /><figcaption>**Figure 1.** XRD patterns of (a): Hopcalite and CeO₂-NR, (b): UiO-66-SO₃H.</figcaption></figure>

2.1.2. Textural Properties

The N₂ adsorption-desorption isotherms and pore size distribution (PSD; insets) of the three materials are illustrated in Figure 2 and the corresponding textural properties are summarized in Table 1. The crushed and sieved particles of commercial Hopcalite show a type IV isotherm with an H3 hysteresis loop in the relative pressure (P/P₀) range of 0.42–1.0. The formation of two adsorption steps at relative pressures (P/P₀) 0.6–0.8 and 0.9–1.0 due to capillary condensation is indicative of a mesoporous material in line with well-distributed pore diameters at 7.8 nm followed by a broad porosity distribution displaying maximum pore diameters around 80 nm. Additionally, the vertical nitrogen uptake at P/P₀ below 0.05 is characteristic of micropore filling. The specific surface area is 229 m² g⁻¹ and the total pore volume Vp is 0.45 cm³ g⁻¹. The S_BET value is less than the one reported by the supplier (>300 m²/g as pellets).

The isotherm of Ceria-NR shows a Type IV shape with a Type H1 hysteresis loop in the high relative pressure (P/P₀) range of 0.82–1.0. The PSD shows a broad peak centered at 35 nm corresponding to the inter-particle spaces in the scaffold-like assembly of nanorods [28]. The BET surface area of 91 m² g⁻¹ and Vp of 0.63 cm³ g⁻¹ are in accordance with previous results [29,30].

<figure><img src="image_5.png" /><figcaption>**Figure 2.** *Cont.*</figcaption></figure>
<figure><img src="image_6.png" /></figure>

<figure><img src="image_7.png" /><figcaption>**Figure 2.** N₂ adsorption/desorption isotherms and PSD (inserts) of Hopcalite, Ceria-NR and UiO-66-SO₃H.</figcaption></figure>

<table><caption>**Table 1.** Textural and redox properties of the materials.</caption><thead><tr><th>Materials</th><th>S<sub>BET</sub><br>(m<sup>2</sup> g<sup>-1</sup>)</th><th>V<sub>p</sub><sup>a</sup> (cm<sup>3</sup> g<sup>-1</sup>)</th><th>H<sub>2</sub> Consumption (mmol g<sup>-1</sup>)</th></tr></thead><tbody><tr><td>Hopcalite</td><td>229</td><td>0.45</td><td>11.1</td></tr><tr><td>Ceria-NR</td><td>91</td><td>0.63</td><td>0.65</td></tr><tr><td>UiO-66-SO<sub>3</sub>H</td><td>685</td><td>0.82</td><td>0.60</td></tr></tbody></table>

The N₂ sorption isotherm of activated UiO-66-SO₃H is a somewhat mixed type I/IV, with a sharp increase of gas uptake at the low-pressure range and an observable hysteresis between adsorption and desorption branches in the high relative pressure (P/P₀) range of 0.73–1.0. UiO-66-SO₃H is a microporous metal-organic framework. The lattice capillary condensation is due to interparticle porosity. As formic acid acts primarily as a monodentate modulator to compete with bidentate bridging H₂BDC-SO₃H ligands for coordination sites on Zr-oxo clusters, the generation of missing-linker defects can be envisioned via incomplete exchange of the pre-loaded formate ligands on the [Zr₆O₄(OH)₄]¹²⁺ secondary building units [31]. The specific surface area of 685 m² g⁻¹ is in agreement with values generally reported for a rather similar material [18,32,33] although an exceeding value of about

<footnote><sup>a</sup> Total pore volume.</footnote>
1180 m²/g was reported for a sulfonic UiO-66 synthesized via a direct solvothermal approach using a mixture of organic linkers (H₂BDC-SO₃H/ H₂BDC) [34].

To sum up, the textural properties are broadly in line with those expected for commercial Hopcalite, CeO₂-NR and UiO-66-SO₃H taking into account the adopted experimental procedures. UiO-66-SO₃H shows an outstanding S<sub>BET</sub> value as compared to the two other porous materials. Additionally, the three materials differ from their pore size distributions. Indeed, the functionalized UiO66-SO₃H displays a hierarchical porosity while the two other solids are mesoporous with Hopcalite developing smaller pores than CeO₂-NR.

### 2.1.3. Redox Properties

The redox properties of the samples were assessed by means of H₂-TPR experiments. H₂-consumption traces are reported in Figure 3 and H₂ consumption amounts are compiled in Table 1.

<figure><img src="image_8.png" /><figcaption>**Figure 3.** (a) H₂-TPR curves of the samples; (b) zoom of the H₂-TPR curves.</figcaption></figure>

The H₂ consumption trace of commercial Hopcalite is complex and resembles broadly to that reported previously for a CuO-MnO₂ solid [35]. The reduction process starts at 90 °C and ends at approximately 360 °C. Five reduction peaks are observed with maxima located at 147, 209, 239, 273 and 343 °C. The first peak at 110 °C and part of the second one are assigned to the reduction of CuOₓ entities into Cu(0). As soon as Cu(II) is reduced into Cu(0), a spill-over of hydrogen takes place from Cu(0) to Mn(IV) entities. As that stage, the reduction of Mn(IV) species occurs in different steps to give
MnO at the end of the process. This is supported by the quantitative results of the H₂ consumption per gram of catalyst. The H₂ consumption of 11.1 mmol g⁻¹ results to a Mn average oxidation state (AOS) of 3.92, a value close to 4.0, assuming the complete reduction of CuO into Cu(0).

The H₂-TPR trace is very flat for CeO₂-NR attesting of a low H₂ consumption as compared with Hopcalite. Three reduction peaks centered at 221 °C, 488 °C and 830 °C related to surface-adsorbed oxygen, sub-surface oxygen and bulk oxygen can be detected in Figure 3b [36]. The sub-surface oxygen species, which are generally considered as the active oxygen species in the low temperature oxidation reactions, amount to 0.65 mmol/gcat, which is much less than the value of 1.05 mmol/gcat obtained by Z. Hu et al. for Ceria nanorods [17]. The H₂-TPR trace for UiO-66-SO₃H is flat from 20 °C to about 400 °C in line with a non-redox active material.

XPS has been performed on Hopcalite to get information about the composition and chemical states of Cu and Mn. The atomic Cu/Mn ratio is 0.16. The Mn AOS, estimated from BE energy separation of the two Mn 3s peaks [37], is 3.14. The BE of Cu 2p₃/₂ of 933.3 eV is in accordance with Cu(II) oxide related species [38]. Hence, we get a Cu(II)/Mn(III) redox system at the surface of Hopcalite in accordance with literature [39].

### 2.1.4. Thermal Stabilities Properties

The thermal stability of the solids has been assessed through TGA/DSC characterizations performed in dry air (Figure 4).

For the activated UiO-66-SO₃H, the DTG curve shows minima at 185 °C and 520 °C indicative of two main weight loss steps (Figure 4). The first weight loss (≈20 wt%) up to 300 °C can be attributed to the release of volatile impurities and CO₂ trapped in the porous network of the MOF [18]. This assumption is supported by the fact that UiO-66-SO₃H loses 11.6 wt% after being heated at 100 °C under vacuum prior to the N₂ adsorption measurement and that no heat flow is detected for a temperature up to 400 °C. A small weight loss occurs between 300 and 400 °C (≈4 wt%). The second main weight loss in the 400–700 °C temperature range amounting to 41 wt% is due to the decomposition of the MOF. A strong exothermic peak at 520 °C substantiates such a thermal decomposition. The weight loss of 41 wt% is substantially less than the expected one of 65.5 wt% assuming total decomposition of [Zr₆O₄(OH)₄(BDC-SO₃H)₆] into ZrO₂. This can be related to partial substitution of the bridging BDC-SO₃H linkers for formate ligands [40].

Hence it can be stated from TG analysis coupled with DSC that the three samples under study can accommodate a thermal activation at 250 °C without deterioration which is a prerequisite for the intended regeneration process.

<figure><img src="image_9.png" /><figcaption>Figure 4. Cont.</figcaption></figure>
<figure><img src="image_10.png" /><figcaption>**Figure 4.** Weight loss (a,c,d) and heat flow (b,e,f) profiles during TGA-DTG analysis of Hopcalite (a,b), CeO₂-NR (c,d) and UiO-66-SO₃H (e,f).</figcaption></figure>

## 2.2. Catalytic Oxidation of Toluene

The light-off curves for toluene oxidation are shown in Figure 5 and the T₁₀, T₅₀, and T₉₀ (temperatures required to achieve 10%, 50%, and 90% of toluene conversion into CO₂) are given in Table 2. During the light-off curve study, only CO₂ and H₂O products have been observed.

<table><caption>**Table 2.** Catalytic properties of the solids in the toluene oxidation.</caption><thead><tr><th>Catalyst</th><th>T<sub>10</sub>(°C)</th><th>T<sub>50</sub>(°C)</th><th>T<sub>90</sub>(°C)</th></tr></thead><tbody><tr><td>Hopcalite</td><td>157</td><td>185</td><td>291</td></tr><tr><td>Ceria-NR</td><td>232</td><td>321</td><td>-</td></tr><tr><td>UiO-66-SO<sub>3</sub>H</td><td>-</td><td>-</td><td>-</td></tr></tbody></table>

Among the different materials, Hopcalite exhibits the best specific activity in terms of T₁₀, T₅₀ and T₉₀. Such results are in accordance with those reported elsewhere [41]. The textural properties (mesoporosity, amorphous state) coupled to the easy cycling between Mn and Cu different valences account for such a behavior. CeO₂-NR is significantly less active as T₉₀ could not be measured (>330 °C) and the T₅₀ of 321 °C is substantially higher than that of Hopcalite. However, Ceria itself is sufficiently active to catalyze the oxidation of toluene. The numerous defects in Ceria in the form of oxygen vacancies are believed to be responsible for its unique catalytic properties. Indeed, Ceria with NR morphology is generally recognized to promote oxygen vacancies. However, the surface oxygen
amount of 0.65 mmol $g_{cat}^{-1}$ is two times less than the amount found by Hu et al. [17]. As described by López et al. [42], the prevalence of surface oxygen vacancies (linked to a high surface-to-bulk oxygen ratio) promotes the activity of the catalysts. Consequently, the lower amount of surface Ceria may account herein for a $T_{50}$ value higher than reported in the literature for NR Ceria, which are typically in the order of 210–220 °C [42]. As expected, UiO-66-SO$_3$H does not convert toluene due to a lack of redox properties. Taking into account the carbon balance, it is found that toluene is trapped inside the UiO66-SO$_3$H structure.

<figure><img src="image_11.png" /><figcaption>**Figure 5.** Light-off curves obtained in the presence of Hopcalite, Ceria-NR and UiO-66-SO$_3$H for toluene oxidation.</figcaption></figure>

## 2.3. Sequential Adsorption/Thermal Conversion

### 2.3.1. Effect of the Initial Toluene Concentration on Hopcalite

To investigate the dynamic adsorption behavior of toluene over Hopcalite, breakthrough adsorption tests were performed with different initial concentrations of toluene (Figure 6a) ranging from 50 to 500 ppm. The adsorption process consists of three steps. First, toluene is fully adsorbed by Hopcalite and very low concentrations of toluene are detected at the outlet of the reactor. This is generally called the unsaturated zone of the breakthrough curve. Second, the appearance of non-adsorbed toluene in the outlet flow, described as the breakthrough stage, is indicative of a weaker adsorption of toluene and by mass transfer limitations. Finally, the inlet toluene concentration is reached, which indicates the saturation [43] and allows for the evaluation of dynamic toluene adsorption capacity of Hopcalite in the given conditions.

At high concentrations of toluene (200 and 500 ppm), the adsorption of toluene is fast. The time during which total adsorption occurs (unsaturated zone) is very short and does not significantly depend on toluene inlet concentration. The curves mostly differentiate by the slope at which saturation is reached in the breakthrough stage. The total adsorption capacity is very similar, in the range of approximately 380–390 µmol g$^{-1}$ (Table 3). This behavior may be due to the improvement of driving force for mass transfer across the liquid film along with increasing of the adsorption rate which leads to quick saturation of the adsorbent [44]. This is even more enhanced when 100 ppm toluene feed is used for which the unsaturated zone is less well defined and the adsorption process slower. Finally, with 50 ppm toluene feed, the process is radically different as no toluene can be detected for a long period and subsequently the saturation abruptly occurs.

The different behavior during the toluene adsorption step according to inlet concentration also affects the “useful” adsorption capacity of the material. Indeed, in a real abatement process, the outlet toluene concentration would not be allowed to exceed a given threshold value, i.e., the adsorption step would need to be stopped once the threshold is reached. If one arbitrarily sets the threshold at 10 ppm,
the breakthrough curves allow to determine approximately the useful adsorption capacity at 470, 230, 160 and 190 µmol g⁻¹ with initial toluene concentrations of 50, 100, 200, and 500 ppm, respectively. With the exception of 50 ppm conditions, these values are significantly lower than those obtained when the full adsorption capacity is considered (Table 3). This suggests that Hopcalite materials should be used preferentially in abatement processes involving rather low toluene concentrations.

These results suggest a complex adsorption process which could involve a rapid adsorption and condensation in the macropores of Hopcalite at high toluene feed concentration followed by diffusion in the mesopores of the solid (Figure 6a). At lower toluene feed concentration, adsorption can occur directly inside the mesoporous structure. Differences can also be seen in the desorption of toluene both at room temperature (not represented) and during heating (Figure 6b) in helium. Above 200 ppm toluene concentration, considerable amounts of toluene (72–74 µmol g⁻¹) desorb at room temperature, showing that adsorption is strongly reversible. Using 100 ppm, this amount reduces to approx. 38 µmol g⁻¹ but a higher amount of toluene desorbs during the heating indicating stronger interactions between the adsorbent surface and toluene.

<figure><img src="image_12.png" /><figcaption>Figure 6. *Cont.*</figcaption></figure>
<figure><img src="image_13.png" /><figcaption>**Figure 6.** (a) Breakthrough curves of Hopcalite at different initial toluene concentration (dotted line corresponds to the concentration of toluene) (b) TPD profile of toluene (c) TPR profile of CO₂ (circle represent the temperature).</figcaption></figure>

<table><caption>**Table 3.** Adsorption (ADS) and desorption (DES) reaction of toluene on Hopcalite in He atmosphere.</caption><thead><tr><th>Toluene Initial Concentration (ppm)</th><th>Tol. ADS at RT (µmol g<sup>-1</sup>)</th><th>Tol. DES at RT (µmol g<sup>-1</sup>)</th><th>Tol. DES during TPR (µmol g<sup>-1</sup>)</th><th>CO<sub>2</sub> Formed during TPR (µmol g<sup>-1</sup>)</th><th>CO<sub>2</sub> Yield (%)</th></tr></thead><tbody><tr><td>50</td><td>472</td><td>0.0</td><td>0.6</td><td>3306</td><td>99.9</td></tr><tr><td>100</td><td>384</td><td>38</td><td>160</td><td>1300</td><td>48.4</td></tr><tr><td>200</td><td>392</td><td>74</td><td>115</td><td>1421</td><td>51.8</td></tr><tr><td>500</td><td>379</td><td>73</td><td>107</td><td>1392</td><td>52.5</td></tr></tbody></table>

Again, a singular behavior is observed using the lowest toluene concentration for which practically no toluene desorption is observed at room temperature. This indicates a strong interaction between toluene and Hopcalite when adsorption is conducted very slowly which is consistent with the long unsaturated time observed during the breakthrough experiment.

The gas phase analysis based on mass spectrometry reveals the formation of CO₂ (m/z = 44) during the temperature programmed desorption process (Figure 6c). Interestingly, no other by products such as CO and HCHO have been observed which is indicative of a high selectivity of Hopcalite towards total oxidation. It can be seen that CO₂ formation starts at 110–120 °C when the lowest toluene concentration was used (50 ppm) and at approximately 150 °C for the higher toluene concentrations. It should be noted that, in this case, CO₂ is produced by reducing the Hopcalite as no oxygen is provided by the gas flow. The highest amount of CO₂ formation is observed (Table 3) in the case of an initial toluene concentration of 50 ppm which is consistent with the absence of toluene desorption at room temperature or during TPR.

Therefore, it can be seen that the so-called irreversible adsorption of toluene (i.e., which does not desorb at RT or during heating) is favored when a low concentration of toluene is used in the inlet feed. This could be due to a better distribution of toluene species on the surface of Hopcalite, in particular within the mesoporous structure. Another possibility is that the irreversible adsorption is slow.

### 2.3.2. Comparative Study of the Different Materials

In the previous section, the dynamic toluene adsorption capacity of the adsorbent was determined by breakthrough curves. The breakthrough provides interesting information with regards to the adsorption properties of a solid but, as explained, cannot be reached in a real toluene abatement process because this would mean that a significant amount of toluene would still be released during the so-called breakthrough stage of the curve. In a real process, the adsorption would need to be stopped when a given threshold is reached corresponding to an acceptable level of toluene emission.
For these reasons, a comparative study of the three different materials (Hopcalite, UiO-66-SO₃H and Ceria-NR) was performed using 100 ppm toluene in the feed and the process was stopped when a concentration of approximately 10 ppm was reached in the outlet flow. In this way, only the so-called "useful" adsorption capacity was taken into consideration.

To identify the catalytic properties, TPR has been performed in two different conditions: (1) in a pure inert gas, i.e., in a pure helium flow and (2) in an oxidizing atmosphere: He: O₂ = 50:50 with a total flow = 100 mL min⁻¹ in both cases. For each experiment, a fresh sample has been used.

All quantitative data obtained on the three materials in inert or oxidizing atmosphere are summarized in Table 4. The "useful" adsorption capacities follow this order: UiO-66-SO₃H > Hopcalite > Ceria-NR which is consistent with the surface area of the respective solids (Table 1). Slight differences are observed on all samples between adsorption steps followed by TPR in He or in He:O₂ even though the adsorption process in always performed in similar conditions (without O₂). This can be due to the difficulty in precisely evaluating the moment at which a 10-ppm residual toluene concentration is reached.

<table><caption>**Table 4.** Comparison of materials during toluene (100 ppm) adsorption followed by temperature programmed desorption in inert and oxidizing atmosphere.</caption><thead><tr><th>Materials and TP Atmosphere</th><th>Tol. ADS at RT (µmol g<sup>-1</sup>)</th><th>Tol. DES at RT (µmol g<sup>-1</sup>)</th><th>Tol. DES during TPR (µmol g<sup>-1</sup>)</th><th>CO<sub>2</sub> Formed during TPR (µmol g<sup>-1</sup>)</th><th>CO<sub>2</sub> Yield (%)</th></tr></thead><tbody><tr><td>Hopcalite-He</td><td>136</td><td>1.4</td><td>23.8</td><td>780</td><td>81.9</td></tr><tr><td>Hopcalite-He:O<sub>2</sub></td><td>108</td><td>1.8</td><td>6.8</td><td>698</td><td>92.3</td></tr><tr><td>Ceria-He</td><td>73</td><td>8.6</td><td>60.5</td><td>28.0</td><td>5.5</td></tr><tr><td>Ceria-He:O<sub>2</sub></td><td>51</td><td>2.6</td><td>34.8</td><td>53.8</td><td>15.1</td></tr><tr><td>UiO-66-SO<sub>3</sub>H-He</td><td>339</td><td>1.6</td><td>301</td><td>258</td><td>10.9</td></tr><tr><td>UiO-66-SO<sub>3</sub>H-He:O<sub>2</sub></td><td>315</td><td>2.3</td><td>267</td><td>315</td><td>14.3</td></tr></tbody></table>

Figure 7 describes the toluene and CO₂ concentration evolution during TPR which follows the adsorption sequence. First, it can be noted that on Hopcalite the overall process is much more efficient in terms of CO₂ yield when the adsorption process is effectively limited to the useful adsorption capacity. Indeed, at a similar inlet concentration of 100 ppm, the CO₂ yield reaches 81.9% when adsorption is limited to 10 ppm max outlet concentration (Table 4) whereas only 48.4% was obtained when the total adsorption capacity is reached (Table 3). Clearly, the amount of reversibly adsorbed toluene is strongly reduced by limiting to the useful adsorption capacity. Still on Hopcalite, in the absence of O₂, a desorption of toluene is observed from room temperature up to approximately 150 °C. This desorption process appears in the form of two peaks, but this could be due to an irregularity in the rate of temperature increase around 80–100 °C as can be seen for all experiments.

The decrease in toluene desorption corresponds to the appearance of CO₂ (Figure 7a', dark blue curve) due to the reaction between toluene and the lattice oxygen species contained in the catalyst. In the presence of oxygen (red curves), the desorption of toluene is interrupted at lower temperature (T < 100 °C) by a sharp increase of CO₂ production. The maximum CO₂ production is reached at approximately 200 °C and ends before the temperature reaches its maximum of 250 °C contrary to what is observed in the absence of a gaseous oxygen feed. These results are in good agreement with the excellent redox properties of Hopcalite for toluene oxidation as a very high conversion of toluene to CO₂ is also obtained in the absence of oxygen (81.6 vs. 92.0% in absence or presence of O₂, respectively). The catalytic properties of Hopcalite are evidenced by the lowering of reaction temperature and by a better total conversion to CO₂. Interestingly, the maximum conversion of adsorbed toluene to CO₂ is reached at a similar temperature in sequential mode with respect to the co-feed (Figure 5) for which T₅₀ was observed at 185 °C.

A similar behavior is observed for CeO₂-NR (Figure 7b,b') but with the major difference that the amounts of CO₂ produced are considerably lower than for Hopcalite. It is nevertheless interesting
to observe that more CO₂ is produced in the low temperature range (<200 °C) while practically no catalytic activity was observed at such low temperature in the co-feed (Figure 5). At higher temperature, the behavior of Ceria is less affected by the presence of O₂ in the gas phase confirming that mostly subsurface oxygen may be involved.

With the objective to get a more accurate view on the redox properties of the two transition metal oxides, the quantity of extracted oxygen from the solids has been estimated from the amount of CO₂ released during He-TPR after toluene adsorption (Table 4) to be compared with H₂ consumption and thus released oxygen in the H₂-TPR experiments (Table 1). For Hopcalite, the extracted oxygen to global oxygen (O<sub>ext</sub>/O<sub>glo</sub>) atomic ratio estimated from the He-TPR (toluene) is approximately five times lower than the ratio obtained from the H₂-TPR experiment (Table 5). This indicates that only the most reducible species or that a few layers of Hopcalite are involved in the reaction. Regarding CeO₂-NR, it is seen that the amount of extracted oxygen with respect to global oxygen (O<sub>ext</sub>/O<sub>glo</sub>) in the TPR after toluene adsorption is approximately 10 times lower than the ratio extracted during H₂-TPR. This is in good coherence with the H₂-TPR profile (Figure 3) which indicated only a very small hydrogen consumption below 300 °C associated with adsorbed oxygen species. This result suggests that mostly surface and eventually some subsurface oxygen species participate in this oxidation process, which is in accordance with literature [42,45].

<table><caption>Table 5. Determination of extracted oxygen from solids in He atmosphere.</caption><thead><tr><th rowspan="2">Materials</th><th>H<sub>2</sub>-TPR</th><th>He-TPR (Toluene)</th></tr><tr><th>O Consumption (mmol g<sup>-1</sup>)</th><th>O Consumption (mmol g<sup>-1</sup>)</th></tr></thead><tbody><tr><td>Hopcalite</td><td>11.1</td><td>2.00</td></tr><tr><td>CeO<sub>2</sub>-NR</td><td>0.65</td><td>0.07</td></tr></tbody><tfoot><tr><td colspan="3"><sup>a</sup> atomic ratio.</td></tr></tfoot></table>

In the case of UiO-66-SO₃H, most toluene desorbs from the surface of the catalysts without transformation (Figure 7c) and this is unaffected by the presence of O₂ in the gas phase. Interestingly however, such desorption occurs at much higher temperature as the maximum toluene pressure is reached around 150 °C and ends around 200 °C. Indeed, for other materials, such a process would end below 150 °C. This confirms the excellent adsorption capacities of UiO-66-SO₃H. Significant amounts of CO₂ are produced on this material but these are not affected by the presence of O₂ (Figure 7c' and Table 4). This indicates that toluene reacts with oxygen species contained in the solid. As UiO-66-SO₃H is not expected to contain such redox properties, one can suppose that the Zr species at the surface of the MOF are partially oxidized and can provide such redox functionality but no actual catalytic properties. Also, UiO-66-SO₃H MOFs contain a lot of B-OH groups, that could also be involved in the oxidation of toluene [46].

<figure><img src="image_14.png" /><figcaption>Figure 7. *Cont.*</figcaption></figure>
<figure><img src="image_15.png" /><figcaption>**Figure 7.** Toluene (a,b,c) and CO₂ (a',b',c') concentration evolution during temperature programmed reaction on Hopcalite (a,a'), CeO₂-NR (b,b') and UiO-66-SO₃H (c,c').</figcaption></figure>

To sum up the results, during sequential adsorption thermal oxidation Hopcalite possess high catalytic activity and high yield formation in absence and/or presence of oxygen. Interestingly, in presence of oxygen the CO₂ formation is take place at below 200 °C. Moreover, no significant difference has been observed for Ceria-NR and UiO-66-SO₃H in absence and presence of the oxygen. Although only a single adsorption-catalytic combustion sequence was performed in each case, this study shows that the Hopcalite stands as a good candidate due to its adsorption and redox properties. As the reaction takes place at temperatures significantly below that of the calcination, good reproducible cyclic behavior can be expected but will need to be explored in future. In the case of Ceria-NR and UiO-66-SO₃H, future study should be focused on enhancing the catalytic activity by addition of an active phase.

# 3. Materials and Methods

## 3.1. *Catalyst Preparation*

Hopcalite (Purelyst MD101; bulk pellets) was purchased from PureSphere Co., Ltd. The approximate chemical composition of Hopcalite was: CuO > 23 mol%, MnO₂ > 69 mol% with the presence of K and Al. The pellets (diameter of 3 ± 0.5 mm) with a length of 10 mm were crushed and sieved to select the 200–300 µm particle size range. The resulting black powder was calcined at 300 °C for 4 h in flowing dry air (2 °C min⁻¹).

CeO₂-NR was synthesized according to the procedure reported by Du et al. [29]. Typically, 1.74 g of Ce(NO₃)₃·6H₂O (Sigma Aldrich, 99%) and an appropriate amount of NaOH (19.2 g pellets, Sigma Aldrich, >99%) were dissolved separately in 40 mL of distilled water. The solutions were mixed together and kept stirring for 30 min. The slightly purple color slurry was then transferred into a 100 mL Teflon-lined stainless-steel autoclave, heated at 100 °C for 24 h in a laboratory oven and cooled to 25 °C. The resulting precipitate was collected by centrifugation at 600 rpm for 10 min,
washed several times with distilled water and ethanol (30 mL), before being dried at 80 °C for 12 h. The resulting pale-yellow powder was calcined at 400 °C for 5 h in flowing dry air (2 °C min⁻¹).

UiO-66-SO₃H (UiO: University of Oslo) was synthesized according to a method described in literature [18]. A mixture, containing ZrO₂Cl₂·8H₂O (0.31 mmol, acbcr chemical, 98%), terephalic acid (0.31 mmol, Sigma Aldrich, 98%), 2-sulphoterephthalic acid mono sodium salt (H₂DBC-SO₃Na, 0.31 mmol, TCI chemicals, >98%), and formic acid (1.2 mL, 3.18 mmol, Sigma Aldrich, >89–91%), was dissolved in N,N Dimethyl acetamide (DMA, 3 mL, 32.5 mmol, Sigma chemicals, >99%) and the solution was placed in a Pyrex tube (10 mL). The filled sealed Pyrex tube was submitted to solvothermal conditions (150 °C for 24 h) and cooled down naturally to 25 °C. The white precipitate was collected by filtration, washed with acetone and dried in ambient condition overnight. A mild three-step activation procedure was employed in order to remove the guest SO₃H linker molecules encapsulated within the pores of the as-synthesized MOF. At first, the guest molecules were exchanged by stirring the as-synthesized UiO-66-SO₃H (0.3 g) in dimethylformamide (DMF, 20 mL, Fluka chemicals, >99.5%) at ambient conditions for 12 h. In the second step, the DMF-exchanged compound was stirred in methanol (30 mL, Fluka chemicals, >99.5%) for 24 h. In the third step, methanol release was carried out using low temperature heating (65 °C) under dynamic vacuum for 24 h to acquire thermally activated UiO-66-SO₃H.

## 3.2. Characterization of the Materials

XRD patterns were recorded using a D8 Advanced Bruker AXS diffractometer with Ni-filtered Cu-Kα radiation. XRD analysis was performed in the 5–80° 2θ range (step size 0.01°, time per step-1 s). The mean crystallite size for CeO₂ was estimated by the Debye–Scherrer formula according to the following equation:

$$D = \frac{K\lambda}{\beta' \cos \theta} \qquad (1)$$

where λ (1.5406 Å) is the X-ray wavelength, K a particle shape factor, taken as 0.9, β' is defined as the width at half maximum of the peak corrected from apparatus broadening (in radians) and θ the position (angle in radians) of the peak.

The textural properties were determined from the adsorption/desorption isotherms of N₂ at 196 °C using a Micrometrics TriStar II 3020 instrument. Prior to adsorption measurement, Hopcalite, Ceria-NR and UiO-66-SO₃H were degassed at 150 °C for 5 h, 250 °C for 5 h [47] and 100 °C for 24 h under vacuum (P = 0.05 mbar), respectively. The pore size distributions were determined from desorption branches of the isotherms using the Barrett-Joyner-Halanda (BJH) method. Total pore volume (Vp) was estimated from the amount of nitrogen adsorbed at a relative pressure (P/P⁰) of 0.99.

H₂-temperature programmed reduction (H₂-TPR) experiments were performed using a Micrometrics model autochem II 2920 equipped with a quartz U-shaped micro reactor. 50 mg of the samples was exposed to a 5% H₂/Ar gas mixture (50 mL min⁻¹) from 25 °C to 1000 °C at a heating rate of 10 °C min⁻¹.

X-ray photoelectron spectroscopy (XPS) experiments were performed using an AXIS Ultra DLD Kratos spectrometer equipped with a monochromatic aluminum source (Al Kα = 1486.7 eV) and charge compensation gun. The binding energies (BE) were referenced from adventitious C 1s at 284.8 eV.

TGA (thermo gravimetric analysis)/DSC (differential scanning calorimetry) measurements were performed using a TA instrument SDT 2960 DSC-TGA V3.0F. Approximately 10 mg of samples were heated from 25 °C to 800 °C (10 °C min⁻¹) in flowing dry air (50 mL min⁻¹). For UiO-66-SO₃H, approximately 2 mg was used due to strong exothermicity of the decomposition process.

## 3.3. Catalytic Activity Tests

The scheme of the home-made experimental set-up for toluene abatement experiments is displayed in Figure 8. All experiments were carried out using a Pyrex glass reactor (inner diameter
10 mm, wall thickness 1 mm) placed into a coaxial tubular furnace which was temperature regulated (TEMPATRON, PID500). All gas flows were regulated using mass flow controllers (Bronkhorst).

<figure><img src="image_16.png" /><figcaption>Figure 8. Schematic diagram of the experimental set-up used for abatement of toluene by adsorption/catalytic oxidation.</figcaption></figure>

### 3.3.1. Catalytic Oxidation

Typically, 0.2 g of the sample was placed in the fixed bed reactor. Before each test, the solids were treated in flowing dry air (100 mL min⁻¹) at 330 °C for 30 min (2 °C min⁻¹). The catalysts were then exposed to the reactive atmosphere (1000 ppmv of toluene diluted in synthetic air) at a flow rate of 100 mL min⁻¹. The temperature was allowed to decrease from 330 °C to 30 °C (with a decreasing rate of 0.5 °C·min⁻¹ to 150 °C followed by 0.2 °C·min⁻¹ from 150 °C to 30 °C). The off-gases were analyzed on-line using a gas chromatograph (µGC, R3000 Agilent Gas Chromatograph) equipped with a thermal conductivity detector (TCD) using a Stabilwax (10 m) column. The results were expressed in terms of toluene conversion into carbon dioxide:

$$X (\%) = \frac{[CO_2]_{out}}{7 \times [C_7H_8]_{in}} \times 100 \quad (2)$$

where X is the toluene conversion into CO₂ while [CO₂]in and [C₇H₈]out are the CO₂ and C₇H₈ concentrations at the inlet and outlet of the reactor, respectively.

### 3.3.2. Sequential Adsorption/Thermal Oxidation

For the sequential adsorption/regeneration experiment, He was used as a carrier gas while toluene was provided from a premixed gas cylinder (0.1 vol% toluene in argon). The evolution of the gas phase composition was monitored using an online mass spectrometer (Omnistar, Pfeiffer Vacuum, Model GSD 301 02). Approximately 0.3 g of the sample was heated in flowing dry air (100 mL min⁻¹) at 150 °C for 4 h (5 °C·min⁻¹) to clean the surface from absorbed species. The sample was then cooled down to room temperature. Meanwhile, the required flow of He and toluene in the argon flow was set to achieve the desired initial toluene concentration (e.g., for 100 ppm toluene: He = 90 mL min⁻¹; toluene/argon = 10 mL min⁻¹). The toluene containing flow was passed through a by-pass and then switched to the reactor to perform the adsorption of toluene. The amount of adsorbed toluene was calculated comparing the initial and residual toluene concentrations. The toluene/argon flow was then switched off and the helium flow adjusted to 100 mL min⁻¹ in order to assess the amount of toluene reversibly adsorbed on the sample. Finally, the sample was heated up to 250 °C (heating rate 2 °C min⁻¹, hold at 250 °C for 1.5 h) in pure He or in O₂:He (50:50).
The amount of toluene desorbed at room temperature ($q(Tol)_{desRT}$), desorbed during the temperature programmed reaction ($q(Tol)_{desTPR}$), the corresponding amount of $CO_2$ formation ($q(CO_2)_{TPR}$), and the amount of toluene adsorbed ($q(Tol)_{ads}$) were calculated as follows:

$$q(Tol)_{desRT} (\mu mol.g^{-1}) = A \times \sum_{0}^{t} (\frac{P(Tol)_{t} + P(Tol)_{t+1}}{2}) \times \Delta t \quad (3)$$

$$q(Tol)_{desTPR} (\mu mol.g^{-1}) = A \times \sum_{0}^{t} (\frac{P(Tol)_{t} + P(Tol)_{t+1}}{2}) \times \Delta t \quad (4)$$

$$q(CO_2)_{TPR} (\mu mol.g^{-1}) = A \times \sum_{0}^{t} (\frac{P(CO_2)_{t} + P(CO_2)_{t+1}}{2}) \times \Delta t \quad (5)$$

$$q(Tol)_{ads} (\mu mol.g^{-1}) = q(Tol)_{desRT} + q(Tol)_{desTPR} + \frac{q(CO_2)_{TPR}}{7} \quad (6)$$

where $P(Tol)_t$ and $P(CO_2)_t$ are the partial pressures of toluene and $CO_2$ at a given time expressed in atm, $t$ is in min, $A = \frac{10^{+3}}{R \times T} \times \frac{F}{M}$ in which $F$ is the total gas flow in mL min$^{-1}$, $M$ is the mass of the material in g, $T = 293$ K, and $R = 8.0206$ L atm mol$^{-1}$ K$^{-1}$.

The $CO_2$ yield was estimated from the formula given below:

$$CO_2 \text{ Yield (\%)} = \frac{q(CO_2)_{TPR}}{7 \times q(Tol)_{ads}} \times 100 \quad (7)$$

The ($O_{ext}/O_{glo}$) atomic ratio where $O_{ext}$ is the amount of oxygen extracted from the solid and $O_{glo}$ the global oxygen content of the solid was also determined in this study. $O_{ext}$ was estimated from the release amount of $CO_2$ during the He-TPR experiments owing to the O balance as follows:

$$C_7H_8 + 18 O = 7CO_2 + 4H_2O \quad (8)$$

$$n(O_{Ext}) = 2 \times n(CO_2)_{TPR} + n(H_2O)_{TPR} = \frac{18}{7} n(CO_2)_{TPR} \quad (9)$$

## 4. Conclusions

The adsorption capacity and catalytic activity of three different materials have been compared for toluene oxidation in co-feed mode and in a novel sequential mode. Among all studied samples, Hopcalite shows the best toluene oxidation and sequential adsorption-thermal oxidation properties. On this material, it has been shown that the adsorption process can be efficient and that the optimal adsorption capacity can be reached at low (<100 ppm) toluene feed. At higher toluene feed concentration, reversible adsorption takes place which is detrimental for the efficiency of the abatement process. The notion of "useful" adsorption capacity is therefore employed to describe the amount of toluene adsorbed before the residual toluene pressure reaches a given acceptable threshold. For instance, with a 10-ppm threshold, the adsorption is mostly irreversible and good toluene abatement performance is reached. Indeed, at a similar inlet concentration of toluene (100 ppm), the $CO_2$ yield is almost twice as large when adsorption is limited to adsorption capacity as compared to that of the obtained adsorption reaching full capacity. In the toluene oxidation step of the process, Hopcalite exhibits the best catalytic oxidation properties allowing to reach high levels of toluene conversion into $CO_2$ and low pollutant release by desorption.

Although the Ceria-NR possesses some catalytic properties, its reactivity at low temperature is not sufficient to convert adsorbed toluene in a useful temperature range, i.e., below 150 °C. Overall performances are thus insufficient to be considered for such a sequential process unless the catalytic performance is enhanced by the addition of an active catalytic phase. $UiO-66-SO_3H$ on
the other hand is a promising material with respect to its excellent adsorption capacities. However, its catalytic properties also need to be improved in order to be considered for a sequential process.

Generally, this exploratory study allows to identify key criteria for the selection of candidate materials for a sequential adsorption-catalysis process for toluene abatement. This study opens the path for further investigations in the search for innovative materials associating active catalytic properties and high-performance adsorption capacities. These may be constituted by well-known adsorbent materials associated with supported catalytically active phases. Alternatively, bulk materials possessing both adsorption and catalytic requirements can be considered and Hopcalite appears as a good candidate in this purpose. Deeper studies of sequential processes are nevertheless required, in particular with regard to the stability of this material in repetitive working conditions. The influence of water vapor and of other competitive pollutants will also need to be carefully investigated in order to simulate realistic pollution abatement conditions.

**Author Contributions:** Conceptualization, J.-M.G. and A.L.; Funding acquisition, J.-F.L. and R.M.; Investigation, S.S., J.-M.G., S.K.P.V., R.B., and A.L.; Supervision, J.-M.G., N.D.G., and A.L.; Visualization, S.S.; Writing—original draft, S.S.; Writing—review & editing, J.-M.G., S.K.P.V., R.B., K.L., P.V.D.V., J.-F.L., R.M., N.D.G., and A.L. All authors have read and agreed to the published version of the manuscript.

**Funding:** The authors acknowledge the support of the European Union for funding this work through an INTERREG V France-Wallonie-Vlaanderen project "Depollutair". The Fonds Européen de Développement Régional (FEDER), CNRS, Région Hauts-de-France, Ministère de l'Éducation Nationale de l'Enseignement Supérieur et de la Recherche and Chevreul Institut are acknowledged for funding of XPS spectrometers and XRD instruments. This research was carried out in the French-Belgium Associated International Laboratory "Plasma & Catalysis" supported by the Universities of Lille and Ghent.

**Conflicts of Interest:** The authors declare no conflicts of interest.

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