# Formaldehyde total oxidation on manganese-doped hydroxyapatite: the effect of Mn content

Dayan Chlala, Jean-Marc Giraudon, Madona Labaki, Jean-Francois Lamonier

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Dayan Chlala, Jean-Marc Giraudon, Madona Labaki, Jean-Francois Lamonier. Formaldehyde total oxidation on manganese-doped hydroxyapatite: the effect of Mn content. Catalysts, 2020, Catalysts (Basel, Switzerland), 10 (12), pp.1422. 10.3390/catal10121422. hal-03944889v2

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Article

# Formaldehyde Total Oxidation on Manganese-Doped Hydroxyapatite: The Effect of Mn Content

Dayan Chlala<sup>1,2,*</sup> and Jean-Marc Giraudon<sup>1</sup>, Madona Labaki<sup>2</sup> and Jean-François Lamonier<sup>1</sup>

Received: 29 October 2020; Accepted: 25 November 2020; Published: 4 December 2020

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**Abstract:** An aqueous impregnation method using manganese (II) nitrate precursor, followed by calcination at 400 °C, was carried out for the preparation of manganese doped hydroxyapatite catalysts (MnxHap; x = Mn wt.-%: 2.5, 5.0, 10, 20, and 30 based on MnO₂). Methods of characterization including inductively coupled plasma spectroscopy (ICP), N₂ physisorption, X-ray Diffraction (XRD), Fourier-Transform Transmission Infrared (FT-IR), Raman, and Thermal gravimetric analysis (TGA/MS) analysis were used for the identification of Mn species and its surrounding environment. Raman spectroscopy indicated the presence of the ε-MnO₂ phase for Mn20Hap and Mn30Hap in agreement with the XRD results and the presence of β-MnOOH species for Mn5Hap and Mn10Hap. The formaldehyde total oxidation was investigated on these catalysts and it was shown that Mn5Hap was the most active catalyst, achieving a normalized rate of formaldehyde (HCHO) conversion into CO₂ per mole of Mn of 0.042 h⁻<fnref n="1" /> at a temperature of 145 °C. The well dispersed oxidized manganese species on Hap with a medium Mn AOS (average oxidation state) were mainly responsible for this performance. Since HCHO was retained on the surface of all catalysts during the catalytic test, the combined Diffuse Reflectance Infrared Fourier Transform spectroscopy (DRIFT) experiment at room temperature and thermodesorption (TD)-FTIR identified formate species as their oxidation consumed surface OH groups. A stability test and moisture effect study showed that the presence of water vapor has a beneficial effect on the performances of the catalyst.

**Keywords:** hydroxyapatite; formaldehyde; manganese; total oxidation

## 1. Introduction

Formaldehyde that is mainly released from coating and adhesive agents for building materials is of great concern due to the fact that formaldehyde (HCHO) is an irritant and carcinogenic volatile organic compound (VOC). This VOC has very harmful effects on the human body, leading to the well-known sick house syndrome. The removal of formaldehyde from existing buildings is of major concern due to stringent legislation surrounding its removal. Among other methods, catalytic oxidation can be one possible attractive technology for the selective elimination of HCHO [1,2]. Total oxidation of HCHO into CO₂ and H₂O has been reported to take place in the presence of supported noble metal catalysts that are operating at low temperatures (<150 °C) [3,4] and even at room temperature in some cases [5]. However, research investigating less costly active options that do not involve noble metals is of considerable interest from an economic point of view. In this context, both supported and unsupported transition metal oxides have been used for the selective elimination of HCHO due to their acid-base and redox properties [6]. Among them, MnₓOᵧ have been studied by several groups due to

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

<footnote n="2">² Laboratory of Physical Chemistry of Materials (LCPM)/PR2N, Faculty of Sciences, Lebanese University, Fanar, Jdeidet El Metn BP 90656, Lebanon; mlabaki@ul.edu.lb</footnote>

<footnote>* Correspondence: dayan.chlala@ul.edu.lb</footnote>
their low volatility and low toxicity. Manganese oxides adopt a wide range of stoichiometry and crystal phases and show excellent efficiency towards achieving HCHO elimination at low temperatures [7]. The ability to switch easily between different oxidation states and the possibility of accommodating defect formations have been put forward to explain such good catalytic performances [8].

In terms of Mn valence, MnO₂ oxide has been claimed to show a higher activity than that of the mixed Mn³+/²⁺ valence Mn₃O₄ oxide [9]. This was consistent with the works of Quiroz Torres et al. [10] showing an increase of the intrinsic HCHO oxidation rate into CO₂ by a factor of 1.4 over an acid-treated catalyst containing Mn₂O₃/Mn₃O₄/Mn₂O₅ phases. This reactivity improvement was mainly related to the promotion of redox properties due to the presence of manganese species at higher oxidation state taking advantage of the disproportionation of Mn(+III). Based on these works highlighting the potential applications of MnO₂ in HCHO elimination, different strategies were adopted to enhance catalytic activities of such materials. Recently a Top-Down approach [11] was proposed for the preparation of high specific surface area α-MnO₂ (cryptomelane). An “Activated Reactive Synthesis” consisting of a High Energy Ball Mill (HEBM) followed by a Low Energy Ball Mill (LEBM) was applied to a commercial α-MnO₂ oxide. The efficiency of this approach was validated by an 8-fold increase of the specific surface area in the optimized conditions of preparation. Although 100% HCHO can be achieved at 175 °C on the best catalyst, contamination by iron at present precludes activity enhancement.

Another possible way to achieve activity enhancement was to investigate the effect of MnO₂ structures. In this context, the square tunnel dimension of related one-dimensional tunnel MnO₂ oxides was recognized to play a key role in HCHO oxidation. It turned out that cryptomelane having a 2 × 2 square tunnel of 0.46 × 0.46 nm² showed the best performances, achieving 100% CO₂ at 140 °C (HCHO: 400 ppmv; Volume Hourly Space Velocity (VHSV) = 18,000 mL g⁻¹ h⁻¹) [12]. The effect of the morphology upon catalytic HCHO total oxidation was subsequently studied on this material by Tian et al. [12]. The best reactivity toward HCHO removal observed on nanoparticles compared to nanorods was explained by a better accessibility of the channel [13]. In that regard, formation of new flower-like cryptomelane particles were reported to exhibit high activity due to their hierarchical structure, large surface area, and large pore size allowing a better diffusion of the reactants [14]. In a similar way, the flake-type morphology of birnessite material (exhibiting a two-dimensional layer) showed a 100% formaldehyde conversion at 100 °C [15].

In order to increase the dispersion of the active MnOₓ phase, the synthesis and physicochemical characterization of mesoporous silica supported manganese oxide have been reported by Averlant et al. [16]. Different impregnation routes have been carried out. As a result, the conventional aqueous impregnation followed by a calcination at 200 °C was found to obtain the best catalytic performances (100% HCHO achieved at 130 °C, Mn (wt%) = 20). Manganese mainly dispersed as β-MnO₂ on the external surface of SiO₂ accounts for such good performances.

As an attractive alternative, hydroxyapatite (Hap) of ideal formula Ca₁₀(PO₄)₆(OH)₂, in foam, has been previously designed as an inexpensive material with active sites for promoting low-temperature catalytic combustion of formaldehyde in moist air [17]. The authors reported the beneficial role of hydroxyl groups bonded within the channel Ca²⁺ to be responsible for adsorption/activation of HCHO. Although the HCHO conversion rate (≈1400 ppmv in moist air, relative humidity (RH) ≈ 8.0%) into CO₂ amounts to 45% at room temperature, 100% HCHO conversion can only be achieved at a temperature of 280 °C.

For a given metal, the dispersion and nature of metal species on a given support depend, among other things, on the nature of the metal precursor, method of preparation (including ion exchange, co-precipitation, impregnation), and temperature of calcination. However, when considering hydroxyapatite, the flexibility in terms of Ca²⁺, PO₄³⁻, and OH⁻ substitution has to also be considered. Some pioneer works have been carried out by our group in order to highlight the nature and location of manganese species when using a conventional precipitation route on hydroxyapatite followed by calcination at 400 °C. The effect of the counter-anion of the manganese (II) salt was first investigated to be correlated with the performances of the final catalyst in toluene total oxidation [18]. It has been
shown that, after calcination at 400 °C, the nitrate Mn(II) precursor allows for getting well dispersed Mn oxidized species on a Ca²⁺ enriched surface, leading to a good toluene conversion (Mn(wt%) = 10; Temperature at which 50% toluene has been converted (T₅₀) = 203 °C; VHSV = 500 mL g⁻¹ h⁻¹). In a second paper, the effect of Mn loading over hydroxyapatite on Mn speciation was investigated to be correlated to the catalytic performances in toluene oxidation [19].

In this study, aqueous precipitation of manganese (II) nitrate, using different Mn content, on hydroxyapatite followed by calcination at 400 °C have been used for the preparation of MnxHap (x = Mn wt%: 2.5, 5, 10, 20, and 30). Different characterizations were used to identify the nature of manganese species to be correlated with the catalytic performances in HCHO total oxidation.

## 2. Results and Discussion

### 2.1. Textural and Structural Properties

The chemical composition values and textural properties of the calcined materials are shown in Table 1. The experimental Mn contents are of the same order relative to the theoretical ones with the margin of error except the Mn30Hap, which has a lower value than expected.

<table><caption>**Table 1.** Chemical composition (CC) and textural properties of the calcined solids.</caption><thead><tr><th rowspan="2">Solids</th><th>CC</th><th>dc<sup>a</sup></th><th>SSA<sup>c</sup></th><th>Vp<sup>d</sup></th></tr><tr><th>Mn (wt%)</th><th>(nm)</th><th>(m<sup>2</sup> g<sup>-1</sup>)</th><th>(cm<sup>3</sup> g<sup>-1</sup>)</th></tr></thead><tbody><tr><td>Hap</td><td>-</td><td></td><td>94</td><td>0.59</td></tr><tr><td>Mn2.5Hap</td><td>2.9</td><td>-</td><td>84</td><td>0.44</td></tr><tr><td>Mn5Hap</td><td>5.8</td><td>-</td><td>84</td><td>0.44</td></tr><tr><td>Mn10Hap</td><td>11.0</td><td>-</td><td>76</td><td>0.38</td></tr><tr><td>Mn20Hap</td><td>20.1</td><td>9</td><td>70</td><td>0.39</td></tr><tr><td>Mn30Hap</td><td>27.5</td><td>9 (36<sup>b</sup>)</td><td>32</td><td>0.18</td></tr></tbody></table>

Results of N₂ physisorption are presented in Figure S1 and the textural properties are gathered in Table 1. Specific surface area (SSA) and Pore volume (Vp) of Hap support were 94 m² g⁻¹ and 0.59 cm³ g⁻¹, respectively. After Mn addition, these values decreased by about 10–24% up to x = 20, whereas a detrimental decrease (66%) was observed for a higher Mn loading. The nitrogen adsorption-desorption isotherms for Hap and Hap-supported Mn samples display the characteristic hysteresis loop of a Type IV(a) isotherm (IUPAC) lying in the P/P0 range of 0.7–0.99 exhibiting an mesoporous character, as shown in Figure S1.

The X-ray diffraction patterns for MnxHap are gathered in Figure 1 and the different peaks belonging to the structures contributing to the refined X-ray diffraction pattern using the Rietveld method are displayed in Figure S2a–c. The X-ray diffraction patterns of MnxHap (x ≤ 10) appear to be very similar to that of monoclinic Hap (JCPDS file: 01-076-0694) up to Mn 10 wt% in accordance with Mn oxidized species below the detection limit and/or well dispersed and/or amorphous MnOₓ species (Figure 1). The X-ray diffraction pattern of Mn20Hap shows a new peak located at about 37.2° and overlapping peaks in 2θ ranges: 42.5–43.5 and 55–58°. Rietveld analysis indicates that the X-ray pattern given in Figure S2b can be adequately described using hexagonal ε-MnO₂ (Akhtenskite; JCPDS file: 01-089-5171) along Hap. The ε-MnO₂ structure can be described as a NiAs unit cell where the Mn(IV) cations are randomly distributed in half of the octahedral positions of the hexagonal close-packed (hcp) oxygen sub-lattice [20]. This structure is recognized to be similar to that of γ-MnO₂ but exhibiting more structural faults and micro-twinning than γ-MnO₂ [21]. The X-ray pattern of Mn30Hap is consistent with the presence of ε-MnO₂ and rhombohedral calcite CaCO₃ (JCPDS file: 01-085-1108) having mean crystallite sizes of 9 and 36 nm, respectively, without excluding the occurrence of α-Mn₂O₃ (JCPDS file: 01-089-2809) in accordance with a relative increase in peak intensity at 32.9°, which has not been taken in account in the simulation.

<footnote><sup>a</sup> Mean crystallite size of MnOx phase; <sup>b</sup> Mean crystallite size of CaCO₃ phase; <sup>c</sup> Specific surface area; <sup>d</sup> Pore volume.</footnote>
<figure><img src="image_3.png" /><figcaption>**Figure 1.** X-ray diffraction pattern of pure Hap and MnxHap samples.</figcaption></figure>

Figure 2 displays the superposition of the Fourier-Transform Transmission Infrared (FT-IR) spectra of Hap support and MnxHap samples. The broad vibrational band in the 3500–3700 cm⁻¹ range has been ascribed to the presence of adsorbed and constitutive water molecules, as shown in Figure 2a. The small band observed at 3571 cm⁻¹ for the Hap support corresponds to structural hydroxyl groups [22], while the bands at 1030 and 1100 cm⁻¹ are assigned to fundamental vibrational modes of PO₄³⁻ groups in Hap [23,24]. The broad multicomponent contribution observed between 1550–1350 cm⁻¹ is assignable to the presence of carbonate groups, which have been mainly incorporated during the synthesis of the material. Their assignments are still controversial in the literature, probably due to the fact that the conditions of collection of the spectra greatly impact the shape of the spectra, as observed by Diallo-Garcia et al. [25], and mainly affect the method for CO₃²⁻ band assignment due to strong band overlapping [26]. FT-IR spectrum of the hydroxyapatite sample in the 1600–1350 cm⁻¹ range shown in Figure 2b allows for observing bands at 1545 cm⁻¹, 1500 cm⁻¹, 1452 cm⁻¹, and 1415 cm⁻¹. Based on literature data, the apparent maximum at 1452 cm⁻¹ can be viewed as the overlapping of 2 bands at about 1456 and 1445 cm⁻¹ [26]. The bands positioned at 1500 cm⁻¹, 1445 cm⁻¹ and 1415 cm⁻¹ have been previously assigned by Cheng et al. to CO₃²⁻ substituting OH⁻ groups, which thus lead to the formation of A-type apatites [26]. The remaining bands at 1456 cm⁻¹ and 1545 cm⁻¹ have been attributed by the same team to CO₃²⁻ substituting PO₄³⁻ groups, which thus lead to the formation of B-type apatites. The broad vibrational band in the 1350–1550 cm⁻¹ range for the Mn30Hap catalyst Figure 2b can be consistent with the overlapping of these previous bands with those CO₃²⁻ bands that originated from CaCO₃, as confirmed by XRD. The FT-IR spectra thus confirmed the combined A and B-type substitution by CO₃²⁻ groups for all MnxHap samples. Neither band was significantly affected by the introduction of Mn. However, the detection of a sharp band at 1385 cm⁻¹ whose intensity increases with Mn loading, attested to the presence of residual NO₃⁻ species. This shows that despite a temperature of calcination of 400 °C for 4 h, a significant amount of NO₃⁻ still remained on the catalyst. It is noteworthy that FT-IR analysis precludes getting valuable information of MnOₓ phases in the 500–600 cm⁻¹ region (not shown here), as expected bands were obscured by some bands of hydroxyapatite.
<figure><img src="image_4.png" /><figcaption>**Figure 2.** Fourier-Transform Transmission Infrared (FT-IR) spectra of Hap and Hap supported Mn catalysts with different loadings in the (a) 500–3700 cm⁻¹ and (b) 1350–1600 cm⁻¹ window.</figcaption></figure>

Figure 3a–e shows the Raman scattering spectra of MnXHap catalysts. The characteristic peaks of Hap can be observed in Figure 3a [27]. It is noteworthy that there was no significant shift of the band located at 960 cm⁻¹ (ν₁ mode of PO₄³⁻). The typical Raman spectra (RS) of different grains of Mn2.5Hap catalyst are presented in Figure 3a. Some only grains reveal the characteristic RS features of the support, while the RS spectra of few grains additionally exhibit a broad envelope due to overlapping of Raman scattering contributions at 580 (s), 640 (s) cm⁻¹ as well as weak RS contributions located at 435 (w), 510 (w), and 710 (w) cm⁻¹. All these RS features are likely related to Mn oxidized species located in an octahedral environment as impurities [28]. As the XPS Mn average oxidation state (AOS) has been found to have a value close to +2.0, Ca²⁺ ions have been supposed to be substituted for Mn²⁺ ions in the Hap lattice, as reported previously [19,29–31]. However, the exact substitution of Ca²⁺ for Mn²⁺ in site 1 (Ca1: columnar Ca atoms parallel to c axis) or in site 2 (Ca2: triangular Ca sites along the c axis of Hap) remains still challenging. Pon-On et al. [32] reported that Mn²⁺ ions substituted for the nine-fold coordinated Ca1²⁺ ions based on Electron Spin Resonance (ESR) analysis of data. Conversely Lala et al. [33] postulated that the Ca2 vacancy site would be more favorable for Mn substitution due to XRD data analysis but using another synthesis procedure. However, complementary experiments have
to be implemented to assess such an assumption. The Mn related RS features are mainly preserved for Mn5Hap (see Mn5Hap(A) in Figure 3b). However, bands at 495, 553, and 635 cm⁻¹ have been observed for Mn5Hap(B) and peaks at 504, 556 and 636 cm⁻¹ for Mn10Hap(B) Figure 3b,c. These three bands can be attributed to stretching vibrations in octahedral MnO₆ [28]. Although these Raman spectra are consistent with those of layered birnessite-type manganese oxide, the X-ray Photoelectron Spectroscopy (XPS) Mn AOS of +3.0 and +3.1 for Mn5Hap and Mn10Hap, respectively, obtained from our previous work [19], differ from that of birnessite (+3.6 to +3.8) [34]. In accordance with the works of Wang et al. [35], these bands have been ascribed to Feitknechtite β-MnOOH, which has hexagonal layered structure. β-MnOOH has been herein considered as the predominant MnOx component of Mn5Hap and Mn10Hap. One possible reason for the existence of β-MnOOH can be the reduction of some expected MnO₂ phase to be reduced back into MnOOH by Mn²⁺ dissolved in the hydroxyapatite. The Raman Mn30Hap(A) spectrum displays lines at 646, 599, 532 and 470 cm⁻¹ (see Figure 3e) in close agreement with those reported for ε-MnO₂ and corroborate our results of XRD data analysis [36]. The same observation was found for Mn20Hap (Figure 3d). Other grains (Mn30Hap(B)) reveal a broad envelope between 400–800 cm⁻¹ due to overlapping peaks of ε-MnO₂, which is probably in line with smaller particle sizes. Also, the Raman spectrum Mn30Hap(C) of some grains displays additional intense peaks at 326, 775, and 807 cm⁻¹ ascribed respectively to v₂, v₃, and v₁ MnO₄³⁻ vibrational modes [37]. This indicates that some Mn(V) replace P(V) in the phosphate lattice, as already noticed in the literature [37]. However, it is expected that this Mn(V) amount is low due to pre-resonance effects [37]. Additionally, a line at 1050 cm⁻¹ was observed for all samples, which has been ascribed to the v₄ mode of remaining NO₃⁻ [38].

<figure><img src="image_5.png" /><figcaption>Figure 3. *Cont.*</figcaption></figure>
<figure><img src="image_6.png" /><figcaption>**Figure 3.** Raman spectra of (a) Hap and Mn2.5Hap; (b) Mn5Hap; (c) Mn10Hap; (d) Mn20Hap and; (e) Mn30Hap.</figcaption></figure>

To investigate the effect of calcination on MnOx phase transformation and NO₃⁻ removal, in-situ Raman spectra were recorded for the precursor of Mn10Hap in a stream of 20% O₂/He while increasing the temperature from 30 to 500 °C with a heating rate of 5 °C/min and keeping the final temperature for 1 h (see Figure S3a). At 100 °C, the broad envelope in the 400–800 cm⁻¹ range was fitted with lines at 496, 596 and 650 cm⁻¹, suggesting the formation of ε-MnO₂ like species Figure S3b. In the range of 200–1800 cm⁻¹, we also observe that the line at 960 cm⁻¹ was already defined as well as that of NO₃⁻ at 1050 cm⁻¹. When increasing the temperature to 500 °C, new lines appeared at 490 and 560 cm⁻¹ whose intensity increases with time and with a shoulder at about 610 cm⁻¹. No significant changes occurred at 500 °C and when returning to 30 °C. The final Raman spectrum is compared to that at the beginning Figure S3c. It is evident that phase transformation occurs from ε-MnO₂ like species into β-MnOOH. Additionally, this transformation was accompanied by a decrease of the intensity of the line at 960 cm⁻¹. With increasing the temperature, the partial disappearance of the line at 1050 cm⁻¹ also takes place. The line intensity-T plot given in Figure S3d showed NO₃⁻ removal as a two steps process, one from 30 °C to 200 °C and the second one from 280 °C to 400 °C. This can be explained by the initial removal of physisorbed NO₃⁻ and to some possible also by NO₃⁻ ions incorporated in the sub-surface of the hydroxyapatite lattice being more difficult to extract.

## 2.2. Thermal Behavior of MnxHap Samples

Thermal gravimetric analysis (TGA) and differential scanning calorimetry (DSC) traces combining with mass-spectroscopy (MS) of Hap, Mn10Hap, and Mn20Hap carried out in dry air are given in Figure 4a,b and relevant results are collected in Table 2. The TG plot of Hap shows three weight loss steps corresponding to the release of water (2.36%) and water/carbon dioxide (2.45% and 2.73%) in agreement with results of on-line mass spectroscopy (see Figure S4). Three weight loss steps were also observed for Mn10Hap due to the release of water (2.78%), water/carbon dioxide/nitrogen monoxide (13.77%), and water/carbon dioxide (2.85%). In comparison, 4 main losses steps were observed for Mn20Hap, whose total weight loss is 1.8 times higher than that of Mn10Hap. The main contributing release of 35.4% was mainly attributed to the release of adsorbed H₂O and NO (not shown here). In agreement with previous studies [39–41], weight losses below 550 °C were ascribed to H₂O and CO₂ desorption from the Hap surface and those above 600 °C to CO₂ released from the bulk of the material. In addition, in our case, the release of water starting from 900 °C was not negligible compared to the loss of CO₂. Therefore, it is not possible to determine the part of weight loss due to CO₂ departure and hence to evaluate the amount of CO₃²⁻ moles per apatite formula. Conversely, such a calculation was possible in the work of Silvester et al. [39], where the weight loss starting from 900 °C and due to H₂O release was much lower compared to that of CO₂. The release of H₂O was not as low compared to that
of CO₂. Furthermore, upon the addition of Mn, some nitrate decomposition took place, rendering the evaluation of carbonates amount more difficult. The different postulated gas releases were supported by the exothermic effects displayed in the DSC curves in Figure 4b. Additionally, an endothermic effect was observed at 930 °C for Mn20Hap, which may be due to crystallization of the ε-MnO₂.

<figure><img src="image_7.png" /><figcaption>**Figure 4.** (a) TG and DT analysis and (b) DSC analysis for Hap, Mn10Hap, and Mn20Hap.</figcaption></figure>

<table><caption>**Table 2.** Thermogravimetric analysis.</caption><thead><tr><th rowspan="2">Catalysts</th><th colspan="5">Weight Loss<br>Temperature Range/°C<br>(Loss Percentage/%)</th></tr><tr><th>I</th><th>II</th><th>III</th><th>IV</th><th>Total</th></tr></thead><tbody><tr><td>Hap</td><td>30–160<br>(2.36)</td><td>160–400<br>(2.45)</td><td>-</td><td>400–1000<br>(2.73)</td><td>30–1000<br>(7.54)</td></tr><tr><td>Mn10Hap</td><td>30–160<br>(2.78)</td><td>160–550<br>(13.77)</td><td>-</td><td>550–1000<br>(2.85)</td><td>30–1000<br>(19.4)</td></tr><tr><td>Mn20Hap</td><td>30–120<br>(12.37)</td><td>120–200<br>(4.17)</td><td>200–450<br>(15.11)</td><td>500–1000<br>(4.19)</td><td>30–1000<br>(35.84)</td></tr></tbody></table>
## 2.3. HCHO Total Oxidation

Figure 5 compares the formaldehyde conversion into CO₂ as a function of temperature over the MnxHap materials thermally activated at 350 °C. The relevant catalytic activity data are given in Table 3. It is worth mentioning the absence of gaseous by-products in the course of the reaction showing, in that way, the selective transformation of HCHO into CO₂ and H₂O. Formaldehyde conversion into CO₂ based on T₅₀ (°C) (the temperature at which 50% of HCHO has been converted into CO₂) increased as follow: Mn2.5Hap (185) < Mn30Hap (163) ~ Mn5Hap (158) ~ Mn10Hap (158) < Mn20Hap (145). The catalysts could be ranked in a similar order after considering the activity data T₁₀ and T₉₀. We achieved 100% conversion of HCHO to H₂O and CO₂ at a temperature of 248 °C on the most active catalyst. It was found that no clear relationship appears between formaldehyde conversion and Mn loading.

<figure><img src="image_8.png" /><figcaption>Figure 5. Conversion of HCHO into CO₂ over MnxHap catalysts.</figcaption></figure>

<table><caption>Table 3. Catalytic performances of the MnxHap catalysts.</caption><thead><tr><th>Catalysts</th><th>T<sub>10</sub>/°C</th><th>T<sub>50</sub>/°C</th><th>T<sub>90</sub>/°C</th><th>Ea/kcal mol<sup>-1</sup></th><th>r<sup>a</sup>/h<sup>-1</sup></th></tr></thead><tbody><tr><td>Mn2.5Hap</td><td>155</td><td>185</td><td>232</td><td>34.4</td><td>0.013</td></tr><tr><td>Mn5Hap</td><td>122</td><td>158</td><td>202</td><td>28</td><td>0.042</td></tr><tr><td>Mn10Hap</td><td>124</td><td>158</td><td>192</td><td>27.3</td><td>0.021</td></tr><tr><td>Mn20Hap</td><td>112</td><td>145</td><td>184</td><td>17.8</td><td>0.019</td></tr><tr><td>Mn30Hap</td><td>141</td><td>163</td><td>202</td><td>39.6</td><td>0.004</td></tr></tbody></table>

The normalized rate r, expressed in the mole of HCHO transformed into CO₂ per mole of Mn per hour, evaluated at 145 °C as a function of Mn content is given in Figure 6. The activity obeys the shape of a Volcano plot with a Mn5Hap catalyst showing the highest normalized rate of 0.042 h⁻¹, which is twice as active as the Mn10Hap catalyst.

Carbon balance as a function of temperature displayed in Figure 7 in any case shows a convex asymmetric curve having one minimum. This indicates that formaldehyde is retained on the surface of the catalysts. The high temperature part of the curve which corresponds to the progressive decrease of the carbon balance down to the minimum value close to zero can be explained by a progressive retention of formaldehyde, probably as formate, on the catalytic surface [42]. The low temperature branch of the curve is consistent with the detection of HCHO as an off gas whose concentration increases with time.

<footnote>a Expressed in the mole of HCHO transformed into CO₂ per mole of Mn per hour estimated at 145 °C.</footnote>
<figure><img src="image_9.png" /><figcaption>**Figure 6.** Normalized rate as a function of the Mn content (wt%).</figcaption></figure>

<figure><img src="image_10.png" /><figcaption>**Figure 7.** Carbon balance as a function of temperature for MnxHap catalysts.</figcaption></figure>

However, the initial concentration of formaldehyde at low temperature is not retrieved due to physical adsorption of formaldehyde on the catalyst surface. Calculation of the area under the curve by integration allows for estimating the percentage of carbon deficiency, which ranges between 17 and 20%. In order to get additional insight about the thermal behavior of formaldehyde-based species retained by the catalysts, MnxHap samples (x = 5; 10; 30) were subjected to a calcination step after the catalytic test was performed in O₂/He (20/80) from 25 °C to 300 °C, and the pertinent data are given in Table 4. Figure 8 displays the evolution of formaldehyde and CO₂ as a function of temperature over the catalysts. Desorption of formaldehyde is observed on all the catalyst surfaces at 25 °C. It rapidly decreases down to zero at about 140 °C.
<table><caption>**Table 4.** Carbon balance levels.</caption><thead><tr><th>Catalysts</th><th>CB <sup>a</sup>/%</th><th>HCHO/µmol</th><th>CO<sub>2</sub>/µmol</th><th>CB <sup>b</sup>/%</th><th>CO<sub>2</sub>/Mn</th></tr></thead><tbody><tr><td>Mn5Hap</td><td>80</td><td>17</td><td>42</td><td>92</td><td>0.2</td></tr><tr><td>Mn10Hap</td><td>82</td><td>10</td><td>48</td><td>93</td><td>0.12</td></tr><tr><td>Mn30Hap</td><td>83</td><td>2.2</td><td>11</td><td>86</td><td>0.01</td></tr></tbody></table>

<sup>a</sup> Carbon balance owing to Equation (2); <sup>b</sup> Corrected Carbon Balance considering the molar amount of HCHO and CO<sub>2</sub> produced during the calcination performed after the test.

<figure><img src="image_11.png" /><figcaption>**Figure 8.** (a) Amount of desorbed HCHO and (b) CO<sub>2</sub> production as a function of temperature for Mn5Hap catalysts.</figcaption></figure>

Carbon dioxide production occurred in a single broad peak, between 100 °C (140 °C; Mn30Hap) and 250 °C, with a maximum located at 155 °C (Mn10Hap), 160 °C (Mn5Hap) and 175 °C (Mn30Hap). The amount of CO<sub>2</sub> (µmol) released increased as follows: 11 (Mn30Hap) < 42 (Mn5Hap) < 48 (Mn10Hap). The molar ratio of CO<sub>2</sub> produced to Mn content, which is believed to be proportional to the dispersion of the active phase, was determined for the different samples. The CO<sub>2</sub>/Mn estimated to be 0.20 for Mn5Hap solid was about 1.6 times and 20 times higher than those estimated for Mn10Hap and Mn30Hap catalysts.

The apparent activation energy E<sub>a</sub> values for formaldehyde oxidation over the Mn5Hap catalysts were calculated from the Arrhenius plots and are shown in Figure 9. The apparent activation energies are in the range of those found in the literature [43,44]. The E<sub>a</sub> value depends on the Mn loading in the sample taking values of ca. 17.8 kcal mol<sup>-1</sup> for Mn20Hap, 28 kcal mol<sup>-1</sup> for Mn5Hap and Mn10Hap, 34.4 kcal mol<sup>-1</sup> for Mn2.5Hap, and 39.6 kcal mol<sup>-1</sup> for Mn30Hap. Over the Mn20Hap catalyst, the reaction is easier to activate, which may provide evidence that the reaction pathway was changed.

The main reason behind better catalytic performances was the decrease of the activation energy. However, the pre-exponential factor A in the Arrhenius law played also a role. Mn5Hap presents a higher activation energy than Mn20Hap, yet this fact could be compensated for by a higher value of A, which refers to the frequency of collisions. According to the Arrhenius equation, the calculated value of the pre-exponential factor A for the Mn5Hap catalyst is equal to 1.1785 × 10<sup>15</sup> higher than that of Mn20Hap 5.589 × 10<sup>9</sup>; this indicates that Mn5Hap is a better catalyst with a higher Mn dispersion.

The catalytic properties (T<sub>50</sub>(CO<sub>2</sub>)) of the supported MnOx phases in the total oxidation of formaldehyde are listed in Table 5. It could be found that our systems are among the active ones found in the literature.
<figure><img src="image_12.png" /><figcaption>**Figure 9.** Arrhenius plots for HCHO oxidation over MnxCat catalysts.</figcaption></figure>

<table><caption>**Table 5.** Catalytic performances over MnOx based catalysts given in the literature.</caption><thead><tr><th>Catalyst</th><th>Mn (wt%)</th><th>HCHO (ppm)</th><th>GHSV (h<sup>-1</sup>) (VHSV) (L gcat<sup>-1</sup> h<sup>-1</sup>)</th><th>T<sub>50</sub> (CO<sub>2</sub>) (°C)</th><th>Reference</th></tr></thead><tbody><tr><td>Mn20Hap</td><td>20</td><td></td><td></td><td>145</td><td></td></tr><tr><td>Mn10Hap</td><td>11</td><td>120</td><td>(30)</td><td>158</td><td>This work</td></tr><tr><td>Mn5Hap</td><td>5.8</td><td></td><td></td><td>158</td><td></td></tr><tr><td>MnOx/PG-MN<sup>a</sup></td><td>8.9</td><td>1200</td><td>(60)</td><td>162</td><td>[43]</td></tr><tr><td>Mn/γ-Al<sub>2</sub>O<sub>3</sub></td><td>18.2</td><td>5300</td><td>(120)</td><td>205*</td><td>[45]</td></tr><tr><td rowspan="2">MnO<sub>2</sub>/Cellulose fiber</td><td>8.86</td><td rowspan="2">100</td><td rowspan="2">50,000</td><td>88*</td><td rowspan="2">[46]</td></tr><tr><td>3.2</td><td>140</td></tr><tr><td>Mn/Pal<sup>b</sup></td><td>10.3</td><td>1000</td><td>32,500</td><td>231</td><td>[47]</td></tr><tr><td>Mn/PG</td><td>15</td><td>300</td><td>20,000</td><td>162*</td><td>[48]</td></tr><tr><td>Mnx/DM-AO<sup>c</sup></td><td>19.8</td><td>180</td><td>(0.06)</td><td>48.8*</td><td>[49]</td></tr><tr><td>Mnx/DM-MT<sup>c</sup></td><td>18.5</td><td></td><td></td><td>45.5*</td><td>[49]</td></tr><tr><td>MN-MnOx-Halloysite</td><td>7.6</td><td>1500</td><td>(60)</td><td>~210</td><td>[50]</td></tr></tbody></table>

## 2.4. Diffuse Reflectance Infrared Fourier Transform Spectroscopy (DRIFT) Experiment at Room Temperature

DRIFT experiments have been performed in order to determine the nature of the adsorbates formed after reaction. DRIFT experiments have been conducted at room temperature for the used catalyst (Mn10HapU). For a comparison purpose, the fresh catalyst Mn10Hap was also tested. The obtained results are plotted in Figure 10a and the difference between the two spectra are displayed in Figure 10b. Four intense bands related to formate species adsorbed on the catalyst surface at 2858 (ν<sub>CH</sub>), 1593 (asym ν<sub>OCO</sub>), 1382 (δ<sub>CH</sub>), and 1356 cm<sup>-1</sup> (sym ν<sub>OCO</sub>) were observed.

<footnote><sup>a</sup> MnOx/PG-MN: palygorskite supported manganese oxide with manganese nitrate (MN) as precursor;</footnote>

<footnote><sup>b</sup> Pal: palygorskite is a natural nanorod-like clay mineral; <sup>c</sup> Diatomite-supported birnessite-type MnO<sub>2</sub> (δ-MnO<sub>2</sub>) synthesized through an in-situ reduction method by methanol (Mnx/DM-MT) and hydrothermal reduction method by ammonium oxalate (Mnx/DM-AO), respectively; * Conversion of HCHO.</footnote>
<figure><img src="image_13.png" /><figcaption>**Figure 10.** (a) Diffuse Reflectance Infrared Fourier Transform spectroscopy (DRIFT) spectra of Mn10Hap sample before and after the catalytic test (Mn10HapU) and (b) Difference between the two recorded spectra.</figcaption></figure>

## 2.5. TD-FTIR

Original spectra were recorded over the whole range of transparency of the Hap self-supporting pellet (4000–1250 cm⁻¹).

The typical FTIR spectrum of the formaldehyde saturated Mn10HapF sample is presented in Figure 11. In the v(OH) region, the main band was observed at 3571 cm⁻¹. It was assigned to both the contributions of structural OH⁻ groups located inside the channels (bulk OH⁻) and to structural OH⁻ emerging at the surface (surface OH⁻), as can be seen in Figure 11a. The broad multicomponent contribution observed at 1550–1300 cm⁻¹ Figure 11b was assignable to the presence of carbonate groups. The most intense contributions at 1448 and 1415 cm⁻¹, as well as the weak contribution at 1500 cm⁻¹, were assigned to the incorporation of bulk carbonates located in the A sites (corresponding to substitution of the OH⁻ groups inside the channels) during the preparation. Therefore, at low temperature, the production of CO₂ might arise from the CO₂ desorbing from OH⁻ and O²⁻ basic sites, formed from the reversible substitution A-type on the surface. The positions and intensities of the bands relative to the bulk carbonates located in the A sites were not affected upon thermal treatment at up to 500 °C. The C2v formate, which gives two modes, was assigned to the asymmetric and symmetric C–O stretching (peaks asym and sym). The asymmetric C=O stretching mode was predicted at 1617 cm⁻¹ and 1584 cm⁻¹, while the symmetric C=O stretching mode was predicted at 1308 cm⁻¹ and 1313 cm⁻¹ in interactions with the Hap (001), and the water reacted to WR(010) surfaces [51]. An intense broad band was observed at 1593 cm⁻¹ showing an asymmetry on the high frequency side. A de-convolution of the spectral profile was carried out considering two components. The bands were in really good agreement with frequencies calculated for FA_Ca1,Ca3 (1617 cm⁻¹) and for FA-(010)WR species (1583 cm⁻¹), respectively. The bands at 1356 (vs(COO-)), 1382 (δ(CH)), 1593 (vas(COO-)) and 2858 (ν(C-H)) have been previously attributed to adsorbed formate species [10]. Increasing the temperature induced a decrease of the bands of formate species, accompanied by a concomitant decrease of the band at 3571 cm⁻¹, suggesting that the oxidation of formate consumed OH groups. The almost formate bands disappearance at 344 °C coincided with the net increase of CO₂ production in the gas phase Figure S5. A new band was also detected at 260 °C located at 3542 cm⁻¹ Figure 11a resulting from dehydration of part of the material due to the consumption of OH⁻ groups for the benefit of O²⁻, whose intensity increases as the temperature increases.
<figure><img src="image_14.png" /><figcaption>**Figure 11.** IR spectra of the Mn10HapF sample after HCHO adsorption and heating under He (a) in the 1200–4000 cm⁻¹ and (b) 1150–1850 cm⁻¹ window.</figcaption></figure>

## 2.6. Moisture Effect, Regeneration Step and Stability Test

Figure 12 shows the effect of H₂O on HCHO conversion into CO₂ with time on stream at 135 °C over the Mn10Hap catalyst. After an induction period of 4 h, the catalyst reached a conversion of HCHO into CO₂ of 80% in dry air. When adding water (RH = 25%) in the feed, the HCHO conversion increased up to 92% at the early stage before rapidly decreasing to reach 78%. Once water was stopped, we observed a slight linear deactivation with time (67% after 13 h). The new addition of water in the feed (RH = 50%) induced an instantaneous raise in conversion (close to 97%) followed by a rapid decrease before reaching a quasi-stationary state (71% after 4 h). Stopping water induces a lowering activity with a conversion of 63% after 7 h on stream. This shows that the presence of moisture has a beneficial effect on the activity of the catalyst. In fact, water was first adsorbed on the surface of the catalyst enhancing the adsorption of HCHO on the catalyst by forming hydrogen bonding with HCHO (the O atom of HCHO was adsorbed on the H atom of HOH sites) [52,53]. Adsorbed HCHO
would be oxidized by surface active oxygen (hydroxyl groups bonded within the channel Ca²⁺) [17]. The consumed surface OH was then compensated for by water. This process increases and enhances the activity of the catalyst for the HCHO oxidation.

<figure><img src="image_15.png" /><figcaption>**Figure 12.** Effect of H₂O on HCHO conversion over the Mn10Hap catalyst: 135 °C, HCHO = 110 ppm in moist air, RH = 25% and 50%, VHSV = 500 mL gcat⁻¹ h⁻¹.</figcaption></figure>

## Regeneration Step of the Catalyst

After the stability test, a calcination at 350 °C for 2 h and at 135 °C for 5 h was performed on the used Mn10Hap catalyst. In order to check the efficiency of such a treatment, the catalytic performance of the calcined Mn10Hap was assessed based on the amount of time on stream, as can be seen in Figure 13. After an induction period of about 7 h, the activity of the catalyst was retrieved ≈ 80%) and then a slight deactivation was observed on stream.

<figure><img src="image_16.png" /><figcaption>**Figure 13.** (a) Stability test performed for 27 h at 135 °C after the regeneration step and (b) Carbon balance over the Mn10Hap catalyst.</figcaption></figure>

# 3. Materials and Methods

## 3.1. *Synthesis of the Hap Support and Supported Mn Catalysts*

The Hap support material was synthesized according to a previous procedure [39] was calcined at 400 °C for 4 h prior to impregnation. The Hap supported manganese catalysts were prepared using
the wet impregnation method, as was already reported [19]. To sum up, samples loaded with 2.5, 5, 10, 20, and 30 Mn wt.% (using MnO₂ as the basis) were synthesized using Mn(NO₃)₂·4H₂O (Sigma Aldrich, Darmstadt, Germany, purity: 97%) as a Mn precursor. A total of 50 mL of the appropriate aqueous precursor solution (0.16 mol L⁻¹) was added to Hap (3.4 g) and stirred at 60 °C using a rotary evaporator. The water was then removed under reduced pressure. The solids were then dried at 80 °C for 20 h and calcined for 4 h at 400 °C under air flow. The resulting powders were denoted as MnxHap for which x represents the Mn content (x = 2.5, 5, 10, 20, and 30 wt%).

## 3.2. Characterization of the Materials

Mn elemental analysis was performed by using inductively coupled plasma spectroscopy-optical emission spectroscopy (ICP-OES). Analyses were carried out at the REALCAT platform (Lille University) using an Agilent Technologies 700 Series spectrometer (Agilent, Mulgrave, Vic, Australia). For analysis, 20 mg of the samples were dissolved in 50 mL of aqua regia solution.

The textural properties (specific surface area and pore volume) of the solids were determined using the physisorption technique with a Micromeritics Tristar II analyzer (Micromeritics, Merignac, France). Before N₂ adsorption, the materials were outgassed at 200 °C for 4 h under vacuum.

Powder XRD data were recorded using a Bruker AXS D8 Advance diffractometer (Madison, WI, USA) working in a Bragg-Brentano geometry. The instrument was equipped with a Lynx Eye Super Speed detector. Data were collected at room temperature using the Cu Kα line in a 2θ range from 10 to 50° with a step size of 0.02° and a 10 s counting time per step. LaB₆ was used as a standard to derive the instrument resolution. The Fullprof Suite program was used for Rietveld refinement on the Hap and MnxHap samples. Additionally, the mean crystallite size of Mn oxide phase was calculated by using the Scherrer formula (D = λ/βcosθ in which λ is the wavelength, β is the integral breadth, and θ is the peak position).

Fourier-Transform Transmission Infrared (FT-IR) spectra were recorded at room temperature using a Nicolet 460 Fourier transform infrared spectrometer (Thermo Fisher Scientific, Waltham, MA, USA) from 220 cm⁻¹ to 4000 cm⁻¹. The spectral resolution was 4 cm⁻¹. KBr pellets were prepared by mixing intimately 1 mg of powdered sample with 60 mg of dried KBr. All FT-IR spectra are an average of 256 scans.

The Raman spectra of the samples, were recorded at room temperature using a Raman spectrometer (Horiba Jobin Yvon Labram HR800, Villeneuve d'Ascq, France) equipped with a Peltier-cooled detector. The exciting light source was the 488 nm line of an Ar⁺-ion laser and the spectral resolution was ±1.5 cm⁻¹. Laser power was 0.4 mW and acquisition time was about 100 s. The presented spectra are the average of 3 scans. The Raman spectrometer was calibrated using the silicon Raman line at 520.6 cm⁻¹.

Thermo gravimetric analysis (TGA) was performed using a Thermal Analysis instrument (SDT 2960 DSC-TGA X, Paris, France) connected to a mass spectrometer (Omnistar, Pfeiffer Vacuum, Asslar, Karlsruhe, Germany), on 10 mg of sample. The weight loss was recorded under 20 vol.% O₂/He, at a heating rate of 5 °C.min⁻¹ from room temperature to 1000 °C.

## 3.3. Catalytic Oxidation of Formaldehyde

Catalytic tests were performed with 0.200 g of catalyst loaded in a glass tubular reactor (I.D. = 10 mm). The total flow rate was fixed at 100 mL min⁻¹, with 120 ppmv inlet HCHO in air flow, which corresponds to a Volume Hourly Space Velocity (VHSV) of 500 mL g⁻¹ h⁻¹. Generation of formaldehyde in gas flow was performed using a permeation system from VICI Metronics (Dynacalibrator Model 150, Poulsbo, WA, USA), loaded with paraformaldehyde. Gas phase formaldehyde concentration was adjusted through control of the permeation chamber temperature at a selected gas flow rate. Before catalytic reaction, the catalyst was calcined in dry air at 350 °C (5 °C min⁻¹, total flow rate = 100 mL min⁻¹) for 2 h. The catalyst was then submitted to the reactive gas mixture for 1 h at 350 °C to allow the temperature to decrease at a rate of 0.5 °C min⁻¹. Products and reactants were
separated and quantified by using on line gas chromatography (Varian CP4900 Micro-GC, Palo Alto, CA, USA) equipped with a TCD and CP-Sil 5 CB column for separation (8 m). The HCHO conversion into CO₂ (X) and carbon balance (CB) were calculated according to Equations (1) and (2).

$$X (\%) = \frac{[CO_2]_{\text{out}}}{[HCHO]_{\text{in}}} \times 100 \qquad (1)$$

$$CB (\%) = \frac{[CO_2]_{\text{out}} + [HCHO]_{\text{out}}}{[HCHO]_{\text{in}}} \times 100 \qquad (2)$$

$[CO_2]_{\text{out}}$, $[HCHO]_{\text{in}}$, and $[HCHO]_{\text{out}}$ were the CO₂ concentration in the outlet gas and the HCHO concentration in both the inlet and outlet gas, respectively.

The rate of HCHO conversion was calculated using the formula:

$$r = \frac{F \times X}{n_{Mn}}$$

where r was the rate of HCHO transformed into CO₂ expressed in mole of reacted HCHO per mole of manganese and per hour. F was the normalized flow rate (T = 25 °C) of HCHO in mole per hour and n<sub>Mn</sub> was the molar amount of manganese.

The apparent energy of activation (Eₐ) of the catalytic reaction for the different catalysts was estimated for a HCHO conversion into CO₂ below 20% so that differential reaction conditions could be assumed with negligible heat and mass-transfer effects. After assuming that a reaction which was first and zero-order with respect to HCHO and to O₂ (large excess) respectively, the apparent rate constant kₐpp was calculated using the formula kₐpp = -ln(1 - X)/τ (τ: residence time based on the catalyst volume). Eₐ values were obtained by plotting ln(kₐpp) versus 1/T.

### 3.4. DRIFT Experiment at Room Temperature

DRIFT spectra of fresh Mn10Hap (before the catalytic test) and the used one Mn10HapU (after the catalytic test) were recorded in a Nicolet 6700-FTIR (Thermo Electron Corporation, Waltham, MA, USA) equipped with a smart collector and a liquid N₂ cooled MCT/A detector. The samples (about 30 mg) for study were finely grounded and placed in a ceramic crucible. All spectra were measured at room temperature with a resolution of 4 cm⁻¹ and accumulating 256 scans. A background spectrum was subtracted from each spectrum, respectively.

### 3.5. Adsorption of Formaldehyde

The Mn10Hap solid (≈100 mg) was exposed to flowing air (100 mL min⁻¹) at 150 °C for 20 min (10 °C min⁻¹) to remove water and surface impurities. HCHO saturation of the catalyst surface was performed at room temperature and checked using mass spectrometry (Omnistar, GSD 301-Pfeiffer, Pfeiffer Vacuum, Asslar, Germany). The catalyst was then exposed to He (65 mL min⁻¹) for 3 h to remove physically adsorbed HCHO. The sample was labeled as Mn10HapF.

### 3.6. Thermodesorption (TD)-FTIR Study

The Mn10HapF sample (≈ 10 mg) was pressed into a self-supported pellet and placed in an infrared cell reactor. The thermo-desorption experiment was conducted in He atmosphere (12 mL min⁻¹) from 25 °C to 500 °C (10 °C min⁻¹). In line FT-IR measurements were performed using a Nicolet 460 FT-IR spectrometer equipped with a high sensitivity liquid nitrogen cooled mercury-cadmium-telluride (MCT)/A detector. The FTIR spectra as an average of 32 scans were recorded from 4000 to 1200 cm⁻¹ using a nominal resolution of 4 cm⁻¹. Ambient background was subtracted from all spectra.
### 3.7. Moisture Effect and Regeneration Step

The Mn10Hap catalyst was activated at 350 °C (5 °C min⁻¹) in air flow (100 mL min⁻¹) for 2 h before being cooled down to 135 °C (1 °C min⁻¹). After 10 min of temperature stabilization, the catalyst was submitted to 110 ppmv of HCHO diluted alternatively in dry and moist air (100 mL min⁻¹; VHSV = 500 mL min⁻¹ g⁻¹, several hours at each step for a total duration of 30 h). The relative humidity was adjusted by passing dry air through a water bubbler kept in a water bath at 43 °C. After this multi-step experiment, the catalyst was regenerated in flowing air at 350 °C for 2 h before cooling down at 135 °C (0.5 °C min⁻¹) and was left for 5 h under air flow at this temperature. Then the catalytic performance of the regenerated catalyst was investigated under 110 ppmv HCHO/dry air (VHSV = 500 mL min⁻¹ g⁻¹) and on stream for 27 h.

## 4. Conclusions

Mn doped hydroxyapatite catalysts (Mn: 2.5, 5, 10, 20 and 30 wt%) synthesized by wet impregnation and calcined at 400 °C were intensively characterized and tested under HCHO total oxidation. Structural characterizations showed that the nature of Mn species changed significantly with Mn content: β-MnOOH species were predominantly detected in Mn5Hap and Mn10Hap samples while ε-MnO₂ phase was present in Mn20Hap and Mn30Hap samples. The catalytic behavior of Hap supported MnOx strongly depended on the Mn content, which is closely related to the nature and local environment of the manganese species. The Mn5Hap catalyst exhibited the best catalytic performance for HCHO oxidation compared with the other catalysts. It was able to convert formaldehyde completely into CO₂ at 230 °C and showed the highest normalized rate of 0.042 h⁻¹ at a temperature of 145 °C. Characterizations indicated that good activity was associated with well dispersed manganese oxides on Hap with a medium Mn AOS. HCHO was retained on the surface of all the catalysts during the catalytic test and formate species were detected such as their oxidation consumed surface OH groups. A stability test and moisture effect study showed that MnxHap catalysts were active for the complete oxidation of formaldehyde even in the presence of large amount of moisture. However, a slight linear deactivation with time was observed in dry air followed by an enhancement in catalyst activity in humid air. This result indicated that the presence of water vapor has a beneficial effect on the performances of the catalyst. The consumed surface OH (which acts as an active oxygen species in HCHO oxidation) was regenerated by water.

**Supplementary Materials:** The following are available online at http://www.mdpi.com/2073-4344/10/12/1422/s1, Figure S1: Isotherms of the MnxHap samples. Figure S2: XRD patterns of (a) Mn2.5Hap, (b) Mn20Hap and (c) Mn30Hap. Figure S3: (a) In situ Raman spectra as a function of temperature for the precursor of Mn10Hap calcined in 20%O₂/He atmosphere; (b) Experimental and fitted Raman spectrum at 100 °C; (c) Comparison of the starting and ending Raman spectrum; and (d) Monitoring of the intensity of the 1050 cm⁻¹ band as a function of temperature. Figure S4: Evolution of m/z = 18, m/z = 44 and m/z = 30 as a function of temperature and Derived weight curve for the decomposition of (a,b) Hap and (c,d) Mn10Hap. Figure S5: CO₂ production in the gas phase in the 2000–2800 cm⁻¹ window.

**Author Contributions:** D.C. prepared the materials and performed the experiments, including the characterization of the catalysts and their catalyst activity tests. Conceptualization, J.-M.G.; Supervision, J.-M.G. and J.-F.L.; Writing—original draft, D.C. and J.-M.G.; Review & editing, M.L. and J.-F.L. All authors have read and agreed to the published version of the manuscript.

**Funding:** The European Union through an INTERREG V France-Wallonie-Vlaanderen project "DepollutAir", the Chevreul institute (FR 2638), Ministère de l'Enseignement Supérieur et de la Recherche, Région Nord—Pas de Calais, FEDER as well as the ARCUS E2D2 project and the French Ministry of Foreign Affairs are acknowledged for supporting and funding this work.

**Acknowledgments:** This work was supported by a grant from the French-Lebanese project PHC CEDRE 2015 No 32933QE and the Lebanese CNRS 2016–2017 project N° 01-08-15. The authors are grateful to Olivier Gardoll for TGA/MS experiments, Laurence Burylo for XRD measurements, and Elise Bernier for Raman in-situ measurements.

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