**Plasma-Catalysis for Volatile Organic Compounds Decomposition: Complexity of the Reaction Pathways during Acetaldehyde Removal**

### **Arlette Vega-González \* , Xavier Duten and Sonia Sauce**

CNRS, UPR 3407, Laboratoire des Sciences des Procédés et des Matériaux, LSPM, Université Sorbonne Paris Nord, F-93430 Villetaneuse, France; xavier.duten@lspm.cnrs.fr (X.D.); sauce.sonia@gmail.com (S.S.)

**\*** Correspondence: arlette.vega@lspm.cnrs.fr; Tel.: +33-1-49-40-34-31

Received: 4 September 2020; Accepted: 30 September 2020; Published: 3 October 2020

**Abstract:** Acetaldehyde removal was carried out using non-thermal plasma (NTP) at 150 J·L −1 , and plasma-driven catalysis (PDC) using Ag/TiO2/SiO2, at three different input energies—70, 350 and 1150 J·L −1 . For the experimental configuration used, the PDC process showed better results in acetaldehyde (CH3CHO) degradation. At the exit of the reactor, for both processes and for all the used energies, the same intermediates in CH3CHO decomposition were identified, except for acetone which was only produced in the PDC process. In order to contribute to a better understanding of the synergistic effect between the plasma and the catalyst, acetaldehyde/catalyst surface interactions were studied by diffuse-reflectance infrared Fourier transform spectroscopy (DRIFTS). These measurements showed that different species such as acetate, formate, methoxy, ethoxy and formaldehyde are present on the surface, once it has been in contact with the plasma. A reaction pathway for CH3CHO degradation is proposed taking into account all the identified compounds in both the gas phase and the catalyst surface. It is very likely that in CH3CHO degradation the presence of methanol, one of the intermediates, combined with oxygen activation by silver atoms on the surface, are key elements in the performance of the PDC process.

**Keywords:** non-thermal plasma; catalysis; VOC; DRIFTS; acetaldehyde

#### **1. Introduction**

Diphasic processes combining a non-thermal plasma at atmospheric pressure and a catalytic bed have become of major interest for air-pollutant removal, and particularly volatile organic compounds (VOC) [1–3]. Indeed, compared to classical air cleaning techniques (thermal catalysis or photocatalysis), plasma-driven catalysis can lead to similar or better VOC degradation rates with less energy injected into the reactor and without catalyst deactivation issues [4,5]. Moreover, in the case of indoor air cleaning, where low VOC concentrations (in the ppm order) have to be removed, this diphasic process seems to be the most suitable [6]. Reviews dealing with the synergistic effects and mechanism of a non-thermal plasma catalysis system in volatile organic compound removal have recently been published [7–9]. Among the studies dealing with the different aspects of such a complex process, we can mention studies on plasma/pollutant interactions [10], surface charging [11,12], adsorption [13,14] or catalyst activation by non-thermal plasma (NTP) [15].

Given the fact that the induced heterogeneous reactions and the plasma are interdependent due to the plasma's continuous discharge during processing, it is essential to make further progress on identifying the surface species forming on the catalyst under the plasma effect. The in-situ Fourier transformed infrared spectroscopy (FTIR)/diffuse-reflectance infrared Fourier transform spectroscopy (DRIFTS) approach for studying catalysts under working conditions is gaining importance in the

framework of the plasma-driven catalysis (PDC) process. To our knowledge, the first of these studies was carried out on isopropanol conversion on γ-Al2O<sup>3</sup> [16]. The authors used a dielectric barrier discharge (DBD) plasma reactor, under static conditions, coupled to in-situ FTIR spectroscopy. They were able to show that unlike the thermal catalysis pathway, with the DBD process the first reaction intermediate is acetone. Plasma-assisted hydrocarbon selective catalytic reduction [17], catalytic steam-reforming of methane [18], reverse water–gas [19]/water–gas shift [20] and plasma-assisted CO<sup>2</sup> hydrogenation [21] processes have also been studied using in-situ DRIFTS. These works pointed out the fact that NTP is able to activate some of the species present either in the gas phase or on the surface, thus improving the performance of the PDC process. Indeed, the role of oxygen in the PDC process has been investigated via isotopically-labeled molecular oxygen (18O2); the results showed that oxygen was fixed onto the surface of the catalyst by the action of the NTP discharge, and was able to survive in such a state for about 30 min [22]. What is more, this same study demonstrated that when using Ag nanoparticles supported on catalysts, they served as oxygen reservoirs. As for VOC removal with non-thermal plasma-assisted catalysis, isopropanol [23,24], toluene [24,25] and acetone removal [26] have been studied using an FTIR in-situ technique. This approach allowed the identification of reaction intermediates, and the following of the evolution of secondary compounds arising from the VOC oxidation.

In a previous work [27] we have showed that, by combining a DBD generated at atmospheric pressure and a silver-supported nanostructured catalyst, acetaldehyde can be removed up to 98% with the production of mainly CO, CO<sup>2</sup> and O3. In addition, we have also studied acetaldehyde adsorption and ozonation over the same silver-based catalyst, and the obtained results support the fact that PDC is a rather complex process in which homogeneous and heterogeneous chemistry are closely interconnected [28]. In the present study we analyse the changes that occurred on an Ag/TiO2/SiO<sup>2</sup> catalyst, used for acetaldehyde removal, after plasma exposure. We investigate which intermediate species were formed on the surface after acetaldehyde adsorption and discharge-assisted conversion by using DRIFT spectroscopy. Gaseous by-products resulting from this process were monitored and quantified, with the aim to contribute to a better understanding of the mechanism of acetaldehyde oxidation. Essentially based on the reactor outlet analysis, the surface composition and literature data, an acetaldehyde removal pathway is proposed considering both the homogeneous and heterogeneous chemistry of the process.

#### **2. Results**

The results obtained when studying acetaldehyde removal using non-thermal plasma, NTP-plasma driven catalysis or just a catalyst will be briefly presented. In addition, we have previously shown that VOC adsorption and heterogeneous NTP-induced chemistry have to be taken into account when associating NTP in air with a catalyst. These results, discussed in more detail in previous works [27–29], were obtained at ambient temperature and atmospheric pressure, but in different configurations of the plasma discharge (i.e., corona or DBD discharge, diameter of the catalyst support, mass of catalyst, energy injected).

#### *2.1. Acetaldehyde Decomposition Using the Plasma-Driven Catalysis Process*

The results obtained for acetaldehyde decomposition with the single stage plasma-driven catalysis, and the plasma-alone processes are presented in Table 1. It is worth noting that the degradation of acetaldehyde by the catalyst alone in the DBD reactor was also studied at room temperature and atmospheric pressure. In this case, neither any degradation of acetaldehyde nor by-product formation is observed.

As can be seen from the results presented in the table above, at atmospheric pressure and ambient temperature the catalyst is not active for acetaldehyde removal. With the plasma-alone process acetaldehyde can be removed up to 55% with an energy consumption of 150 J·L −1 (~250 mW power consumption). As soon as the silver nanostructured catalyst is introduced into the discharge zone, acetaldehyde removal increases, already allowing, at 70 J·L −1 (~120 mW), 33% to be obtained and up to 98% at 1150 J·L −1 (~2 mW). Acetaldehyde removal (%) 0 55 33 87 98

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**Table 1.** Acetaldehyde removal obtained using the plasma-driven catalysis and the non-thermal plasma (NTP) processes. As can be seen from the results presented in the table above, at atmospheric pressure and ambient temperature the catalyst is not active for acetaldehyde removal. With the plasma-alone


The main gaseous by-products at the exit of the DBD reactor are CO and CO2, but other organic by-products have also been identified: methanol (Me), acetic acid (AcA), acetone (Ace), methyl formate (MeF), methyl acetate (MeA), 1,2-ethanediol monoformate (EmF), 1,2-ethanediol diformate (EdF), nitromethane (Nm), methyl nitrate (MN) and 2-ethoxyethanol (Eet). Their distribution at the DBD reactor exit is presented in Figure 1, except for the ones present in trace amounts (Eet), or those that could not be quantified (MN). Among these organic products we recognize compounds belonging to different functional groups such as hydroxyl, carboxyl, carbonyl, carboalkoxy and nitro compounds, reflecting the complexity of the chemistry involved in such processes. by-products have also been identified: methanol (Me), acetic acid (AcA), acetone (Ace), methyl formate (MeF), methyl acetate (MeA), 1,2-ethanediol monoformate (EmF), 1,2-ethanediol diformate (EdF), nitromethane (Nm), methyl nitrate (MN) and 2-ethoxyethanol (Eet). Their distribution at the DBD reactor exit is presented in Figure 1, except for the ones present in trace amounts (Eet), or those that could not be quantified (MN). Among these organic products we recognize compounds belonging to different functional groups such as hydroxyl, carboxyl, carbonyl, carboalkoxy and nitro compounds, reflecting the complexity of the chemistry involved in such processes.

**Figure 1.** Comparison of the composition of the dielectric barrier discharge (DBD) reactor effluent obtained with the plasma-alone and the plasma-driven catalysis process, as a function of SIE. **Figure 1.** Comparison of the composition of the dielectric barrier discharge (DBD) reactor effluent obtained with the plasma-alone and the plasma-driven catalysis process, as a function of SIE.

From the obtained results we can say that with the plasma-alone process neither acetone nor nitromethane are produced at 150 J∙L-1; and compared with the PDC process, more acetic acid and methanol are formed. With the PDC process at 70 J∙L, aside from methyl formate and the emergence of acetone, all the other by-products are produced in lower amounts compared with NTP alone, which is certainly due to the lower acetaldehyde conversion. The by-products' formation is promoted as soon as the specific input energy (SIE) increases. Between 70 and 350 J∙L-1, there is a significant rise in each by-product concentration, 150% being the lowest increase observed. Between 350 and 1150 J∙L-1, an almost constant production of CO2, methanol, acetone, methyl formate and nitromethane is observed; whereas an increase between 70/80% in CO, MeA, AcA and EdF, and of 108% in EmF is still observed. Even if the amount of MN could not be quantified, the analyses of the DBD reactor effluent have shown that it is formed in higher quantities in the PDC process, and its production increases with SIE. Furthermore, introducing a catalyst in the discharge zone induces an increase in COx selectivity. In fact, NTP at 150 J∙L-1 has a COx selectivity of 35% while in the PDC process this From the obtained results we can say that with the plasma-alone process neither acetone nor nitromethane are produced at 150 J·L −1 ; and compared with the PDC process, more acetic acid and methanol are formed. With the PDC process at 70 J·L, aside from methyl formate and the emergence of acetone, all the other by-products are produced in lower amounts compared with NTP alone, which is certainly due to the lower acetaldehyde conversion. The by-products' formation is promoted as soon as the specific input energy (SIE) increases. Between 70 and 350 J·L −1 , there is a significant rise in each by-product concentration, 150% being the lowest increase observed. Between 350 and 1150 J·L −1 , an almost constant production of CO2, methanol, acetone, methyl formate and nitromethane is observed; whereas an increase between 70/80% in CO, MeA, AcA and EdF, and of 108% in EmF is still observed. Even if the amount of MN could not be quantified, the analyses of the DBD reactor effluent have shown that it is formed in higher quantities in the PDC process, and its production increases with SIE. Furthermore, introducing a catalyst in the discharge zone induces an increase in CO<sup>x</sup> selectivity. In fact, NTP at 150 J·L <sup>−</sup><sup>1</sup> has a CO<sup>x</sup> selectivity of 35% while in the PDC process this selectivity is equal to 36, 50 and 60% for 70, 350 and 1150 J·L −1 , respectively.

selectivity is equal to 36, 50 and 60% for 70, 350 and 1150 J∙L-1, respectively.

#### *2.2. Acetaldehyde Adsorption on Ag*/*TiO2*/*SiO<sup>2</sup> 2.2. Acetaldehyde Adsorption on Ag/TiO2/SiO<sup>2</sup>*

In order to characterize the catalyst surface before turning the plasma on, in-situ DRIFTS was used to monitor the Ag/TiO2/SiO<sup>2</sup> surface during acetaldehyde adsorption. The adsorption capacity of the catalyst, at the experimental conditions used, was evaluated to be 698 <sup>±</sup> <sup>3</sup> <sup>µ</sup>mol/gcatalyst. In order to characterize the catalyst surface before turning the plasma on, in-situ DRIFTS was used to monitor the Ag/TiO2/SiO2 surface during acetaldehyde adsorption. The adsorption capacity of the catalyst, at the experimental conditions used, was evaluated to be 698 ± 3 mol/gcatalyst.

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Figure 2 shows the infrared spectra of the silver-based catalyst surface after 1 and 30 min of exposition to 1000 ppmC of CH3CHO at 298 K and atmospheric pressure. Acetaldehyde shows peaks in the 3000–2600 cm−<sup>1</sup> region and 1800–1500 cm−<sup>1</sup> region, as shown in the figure. After 1 min acetaldehyde adsorption, bands at 2936, 2922, 2866, 2770, 2748, 1759, 1713, 1555 and 1242 cm−<sup>1</sup> are observed. Once the saturation is attained, after 30 min, the previously mentioned absorption bands increase, and a new band appears at 2974 cm−<sup>1</sup> . In addition, broadband absorption features, associated with the peaks at 1713, 1555 and 1242 cm−<sup>1</sup> are observed. The first broadband presents peaks at 1720 and 1713 cm−<sup>1</sup> ; a small shoulder at 1697 cm−<sup>1</sup> , and a large shoulder in the 1690–1650 cm−<sup>1</sup> range. The second broadband still showing a maximum at 1555 cm−<sup>1</sup> , and many smaller peaks in the 1590–1500 cm−<sup>1</sup> range are visible after saturation of the surface with acetaldehyde. The last broadband also presents smaller peaks in the 1280–1210 cm−<sup>1</sup> range. Figure 2 shows the infrared spectra of the silver-based catalyst surface after 1 and 30 min of exposition to 1000 ppmC of CH3CHO at 298 K and atmospheric pressure. Acetaldehyde shows peaks in the 3000–2600 cm−1 region and 1800–1500 cm−1 region, as shown in the figure. After 1 min acetaldehyde adsorption, bands at 2936, 2922, 2866, 2770, 2748, 1759, 1713, 1555 and 1242 cm−1 are observed. Once the saturation is attained, after 30 min, the previously mentioned absorption bands increase, and a new band appears at 2974 cm−1. In addition, broadband absorption features, associated with the peaks at 1713, 1555 and 1242 cm−1 are observed. The first broadband presents peaks at 1720 and 1713 cm−1; a small shoulder at 1697 cm−1, and a large shoulder in the 1690–1650 cm−1 range. The second broadband still showing a maximum at 1555 cm−1, and many smaller peaks in the 1590–1500 cm−1 range are visible after saturation of the surface with acetaldehyde. The last broadband also presents smaller peaks in the 1280–1210 cm−1 range.

**Figure 2. D**iffuse-reflectance infrared Fourier transform spectroscopy (DRIFTS) spectra recorded after **Figure 2.** Diffuse-reflectance infrared Fourier transform spectroscopy (DRIFTS) spectra recorded after 1 and 30 min of acetaldehyde adsorption on Ag/TiO<sup>2</sup> /SiO<sup>2</sup> at 298 K and atmospheric pressure.

1 and 30 min of acetaldehyde adsorption on Ag/TiO2/SiO2 at 298 K and atmospheric pressure. **Table 1.** Adsorbed acetaldehyde: observed bands and their assignments. Peak assignments are presented in Table 2. In both spectra, bands in the 3000–2800 cm−<sup>1</sup> region, the CH stretching region, can be assigned to symmetric and asymmetric ν(CH3) and ν(CH2) modes [30] and bands in the 1700–1680 cm−<sup>1</sup> region can be assigned to ν(C=O) mode [31].


**Vibrational mode gas phase Reference CH3CHO adsorbed on Table 2.** Adsorbed acetaldehyde: observed bands and their assignments.

**Vibrational assignments (cm−1)** 

the CH stretching region, can be assigned to symmetric and asymmetric (CH3) and (CH2) modes [30] and bands in the 1700–1680 cm−1 region can be assigned to (C=O) mode [31]. From the literature, most of the bands in the CH stretching region could be assigned to adsorbed From the literature, most of the bands in the CH stretching region could be assigned to adsorbed acetaldehyde [32–34]. However significant overlap of much of this region exists between acetaldehyde

region.

and the products of its heterogeneous reactions on oxide surfaces. Indeed, the bands at 2922, 2830 and 2748 cm−<sup>1</sup> could be assigned to crotonaldehyde [33] whereas the band at 2936 cm−<sup>1</sup> may also be assigned to other condensation products derived from surface reactions [31], or to acetate species [32]. The formation of crotonaldehyde is supported by the presence of the peak at 1720 cm−<sup>1</sup> and the broad shoulder at 1690–1650 cm−<sup>1</sup> [31,33,37–39] and the formation of acetate species is in agreement with the emergence of the broadband centered at 1555 cm−<sup>1</sup> [36]. The dominant spectral feature in the ν(C=O) region, at 1713 cm−<sup>1</sup> , which is assigned to adsorbed acetaldehyde, shifts to lower wavenumbers with respect to the same band of CH3CHO in the gas phase. This indicates that acetaldehyde is bound to the surface TiO<sup>2</sup> through its carbonyl group by H-bridge bonding [37,38,40]. In addition, the growth of other infrared spectral features in this region points out the probable formation of other products such as acetone (1697 cm−<sup>1</sup> [41]) or formaldehyde. Indeed, the band at 1242 cm−<sup>1</sup> can be assigned to molecularly adsorbed formaldehyde [42,43], which has also been reported to present bands at 2913, 2863, 2759, 1648 and 1413 cm−<sup>1</sup> [42,44], supporting the presence of formaldehyde on the silver-based catalyst surface after acetaldehyde adsorption. acetaldehyde and the products of its heterogeneous reactions on oxide surfaces. Indeed, the bands at 2922, 2830 and 2748 cm−1 could be assigned to crotonaldehyde [33] whereas the band at 2936 cm−1 may also be assigned to other condensation products derived from surface reactions [31], or to acetate species [32]. The formation of crotonaldehyde is supported by the presence of the peak at 1720 cm−1 and the broad shoulder at 1690–1650 cm−1 [31,33,37–39] and the formation of acetate species is in agreement with the emergence of the broadband centered at 1555 cm−1 [36]. The dominant spectral feature in the (C=O) region, at 1713 cm−1, which is assigned to adsorbed acetaldehyde, shifts to lower wavenumbers with respect to the same band of CH3CHO in the gas phase. This indicates that acetaldehyde is bound to the surface TiO2 through its carbonyl group by H-bridge bonding [37,38,40]. In addition, the growth of other infrared spectral features in this region points out the probable formation of other products such as acetone (1697 cm−1 [41]) or formaldehyde. Indeed, the band at 1242 cm−1 can be assigned to molecularly adsorbed formaldehyde [42,43], which has also been reported to present bands at 2913, 2863, 2759, 1648 and 1413 cm−1 [42,44], supporting the presence of formaldehyde on the silver-based catalyst surface after acetaldehyde adsorption.

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Although at the end of the adsorption step the Ag/TiO2/SiO<sup>2</sup> catalyst surface is mainly covered with adsorbed acetaldehyde, the other species which are also present have to be considered in order to better understand the acetaldehyde degradation mechanism in the following step of the process. Although at the end of the adsorption step the Ag/TiO2/SiO2 catalyst surface is mainly covered with adsorbed acetaldehyde, the other species which are also present have to be considered in order to better understand the acetaldehyde degradation mechanism in the following step of the process.

#### *2.3. Surface Species Formed during the PDC Process 2.3. Surface Species Formed During the PDC Process*

Once saturated with acetaldehyde, the Ag/TiO2/SiO<sup>2</sup> catalyst is used in order to decompose the VOC with the PDC process. Three different energies were used—70, 350 and 1150 J·<sup>L</sup> −1 . Figure 3 shows the surface spectra of the catalyst before and after being exposed to the DBD discharge for 30 min. It is clear that the surface species present on the surface after the adsorption process take part in different surface reactions while the plasma is on, leading to the modification of the surface composition as can be seen from the FTIR band features. Once saturated with acetaldehyde, the Ag/TiO2/SiO2 catalyst is used in order to decompose the VOC with the PDC process. Three different energies were used—70, 350 and 1150 J∙L-1. Figure 3 shows the surface spectra of the catalyst before and after being exposed to the DBD discharge for 30 min. It is clear that the surface species present on the surface after the adsorption process take part in different surface reactions while the plasma is on, leading to the modification of the surface composition as can be seen from the FTIR band features.

**Figure 3.** Ag/TiO2/SiO2 catalyst surface DRIFTS spectra after saturation with CH3CHO; and NTP effect on surface species at different plasma discharge energies: (**a**) C-H stretching region; (**b**) bending **Figure 3.** Ag/TiO<sup>2</sup> /SiO<sup>2</sup> catalyst surface DRIFTS spectra after saturation with CH3CHO; and NTP effect on surface species at different plasma discharge energies: (**a**) C-H stretching region; (**b**) bending region.

From Figure 3a it is clear that, after the PDC process, some of the bands disappear (2974 and 2770 cm−1) or almost disappear (2748 cm−1). The relative intensity of the bands in the 2970–2900 cm−1 region has clearly changed, with visible peaks at 2946, 2955 and 2964 cm−1; the band in the 2900–2800 cm−1 region decreases significantly; and a new broad band with peaks at 2600 and 2581 cm−1 appears. From Figure 3a it is clear that, after the PDC process, some of the bands disappear (2974 and 2770 cm−<sup>1</sup> ) or almost disappear (2748 cm−<sup>1</sup> ). The relative intensity of the bands in the 2970–2900 cm−<sup>1</sup> region has clearly changed, with visible peaks at 2946, 2955 and 2964 cm−<sup>1</sup> ; the band in the 2900–2800 cm−<sup>1</sup> region decreases significantly; and a new broad band with peaks at 2600 and 2581 cm−<sup>1</sup> appears. Figure 3b shows an evident broadening of the bands centered at 1713, 1555 and

Figure 3b shows an evident broadening of the bands centered at 1713, 1555 and 1242 cm−1 in the

1242 cm−<sup>1</sup> in the acetaldehyde-saturated surface. As the plasma input energy increases, the maximum of the <sup>ν</sup>(C=O) band is redshifted and its intensity decreases for an SIE higher than 70 J·L −1 . At the same time, a band with increasing intensity develops in the 1300–1000 cm−<sup>1</sup> region.

The loss of the bands at 2974 and 2770 cm−<sup>1</sup> (assigned to adsorbed acetaldehyde), along with an intensity decrease of the peaks at 2866 and 1713 cm−<sup>1</sup> indicates a gradual depletion of acetaldehyde surface species once the catalyst is in contact with the plasma. Likewise, the loss in intensity of the bands at 2922, 2830, 2748 and 1720 cm−<sup>1</sup> indicates that less crotonaldehyde is present on the surface. Under the plasma effect, the 2950–2900 cm−<sup>1</sup> band broadens, and presents different small peaks and shoulders with maximum intensities at 2946 and 2936 cm−<sup>1</sup> . The former peak may be assigned to surface methoxy [45]; indeed, along with the peak at 2946 cm−<sup>1</sup> , the presence of a small shoulder at 2924 cm−<sup>1</sup> and a peak at 2855 cm−<sup>1</sup> supports the possibility of the formation of surface methoxy [45–47]. Concerning the peak at 2936 cm−<sup>1</sup> , its attribution is less straightforward as it can be related to different surface species such as formate, ethoxy or acetate species [32,44,45]. On the one hand, the infrared features at 2964, 2955, 2936, 2924, 2866 and 2735 cm−<sup>1</sup> bring out the formation of surface formate [45,48]. On the other hand, the peaks at 2964, 2936, 2866 and 2855 cm−<sup>1</sup> have also been assigned to ethoxy species formed on a TiO<sup>2</sup> surface [37,44,49]. Furthermore, the peaks at 2964 and 2936 cm−<sup>1</sup> have also been assigned to methyl acetate [35], whereas the one at 2936 cm−<sup>1</sup> is also assigned to acetic acid [50]. The broad band between 2650 and 2550 cm−<sup>1</sup> that appears after the plasma catalysis process supports the formation of formate species as it has been attributed to formic acid [51]. As the energy increases up to 350 J/L, the 2900–2800 cm−<sup>1</sup> band loses intensity, the loss being more pronounced for the peak at 2936 cm−<sup>1</sup> ; whereas the peaks at 2964 and 2955 cm−<sup>1</sup> , as well as a new peak at 2914 cm−<sup>1</sup> become more visible. This latter peak may be attributed either to acetaldehyde [36], or to an intermediate formed from formaldehyde oxidation or disproportionation to give formate or methoxide, respectively [52,53].

These attributions can be backed by the infrared features in the 2000–950 cm−<sup>1</sup> region. Significant overlapping of the peaks in this wavelength range complicates precise identification of surface species but, based on litterature data, the bands generated on the plasma-exposed surface can be related to distinct vibrational modes of acetate, formate, methoxy, ethoxy, carbonate and formaldehyde species adsorbed on the surface of the Ag/TiO2/SiO<sup>2</sup> catalyst. Thus, we may assign some of the bands as presented in Table 3.


**Table 3.** Infrared (IR) bands assignment of the major surface species formed during the PDC process, in the 2000–950 cm−<sup>1</sup> region.

The change in the vibrational spectrum of the catalyst surface following its exposure to NTP suggests a modification of its composition, which is directly related to the acetaldehyde decomposition mechanism.

#### **3. Discussion**

In this section we will propose a reaction pathway that takes into account acetaldehyde adsorption and its degradation on the surface with the PDC process. On the basis of the DBD reactor effluent analysis, and the infrared spectroscopic measurements carried out on the catalyst surface, it is evident that acetaldehyde undergoes a rather complex chemistry during the process. For this reason, a detailed description of the acetaldehyde decomposition mechanism is out-of-reach at this point. Alternatively, we propose a series of simplified adsorption/degradation routes in order to account for the key aspects of surface activity that lead to the formation of the different identified surface species, and a subsequent increase in acetaldehyde degradation, which results in an increase in the amount of gaseous by-products.

#### *3.1. Acetaldehyde Adsorption Mechanism*

In different studies concerning the photocatalytic degradation pathway of acetaldehyde on a TiO<sup>2</sup> surface, it has been noticed that, upon adsorption of acetaldehyde, different species are already formed without illuminating the catalyst. Two compounds, 3-hydroxybutanal and crotonaldehyde, are formed through an aldol condensation, while bidentate acetate species have been detected to be formed by an oxidation process occurring on the TiO<sup>2</sup> surface [40].

As suggested from the spectra analysis of the saturated surface, when acetaldehyde is brought into contact with the nanostructured TiO2, it will certainly bind to the surface through the oxygen atom of its carbonyl group. Then, two acetaldehyde molecules adsorbed on neighboring sites can react through a β-aldolization reaction to give crotonaldehyde, CH3(CH)2CHO [28,31,33,64–66]. It has been shown that acetaldehyde undergoes aldol condensation forming 3-hydroxybutanal (CH3CH(OH)CH2CHO) which, upon dehydration forms crotonaldehyde [31,34,40]:

$$\text{CH}\_3\text{CHO}\_{\text{ads}} + \text{CH}\_3\text{CHO}\_{\text{ads}} \rightarrow \text{CH}\_3-\text{CH}=\text{CH}-\text{CHO}\_{\text{ads}} + \text{H}\_2\text{O} \tag{1}$$

Formation of acetate species can result from the direct oxidation on the surface of acetaldehyde [30, 32,46,66], and to a lesser extent of crotonaldehyde [40], through a surface oxygen (Os):

$$\text{CH}\_3\text{CHO}\_{\text{ads}} + \text{O}\_{\text{s}} \rightarrow \text{CH}\_3\text{COO}\_{\text{ads}}^- + \text{H}\_{\text{ads}}^+\tag{2}$$

Besides, a Cannizzaro disproportionation of two acetaldehyde molecules involving a vacancy (VO) and surface oxygen would result in the formation of acetate and ethoxy groups. This pathway has been proposed for acetaldehyde adsorption on rutile TiO<sup>2</sup> [33]:

$$2\text{CH}\_3\text{CHO}\_{\text{ads}} + \text{V}\_\text{O}/\text{O}\_\text{s} \to \text{CH}\_3\text{COO}\_{\text{ads}}^- + \text{CH}\_3\text{CH}\_2\text{O}\_{\text{ads}}^-\tag{3}$$

Despite the fact that it is difficult to ascertain the presence of ethoxy species from the spectra in Figure 2, their presence at much smaller levels than acetates cannot be completely ruled out.

Concerning acetone formation on oxide surfaces from aldehydes, two pathways are mainly known. The first is via a two-step reaction: oxidation to carboxylates followed by the coupling of two carboxylates to form one molecule of ketone. The second pathway is through the reaction of an adsorbed acyl group, RC=O, with an alkyl group [32]. Examples of acetone formation from acetaldehyde via these two pathways have been reported, but they concern studies carried out at temperatures well above the ambient temperature [32,67–69]. Another possibility is acetone formation through 3-hydroxybutanal. Indeed, at ambient temperature this compound is very reactive and, either it undergoes fast dehydration on the surface to form crotonaldehyde; or it can be converted via intramolecular H transfer to 4-hydroxybutan-2-al (CH3C(O)CH2CH2OH). The latter can be further transferred into acetone (CH3C(O)CH3) and formaldehyde (HC(O)H) via reverse reaction to aldol condensation [34]:

$$\text{C}2\text{CH}\_3\text{CHO}\_{\text{ads}} \rightarrow \text{CH}\_3\text{CH}(\text{OH})\text{CH}\_2\text{CHO}\_{\text{ads}} \leftrightarrow \text{CH}\_3\text{C}(\text{O})\text{CH}\_2\text{CH}\_2\text{OH} \rightarrow \text{HC}(\text{O})\text{H} + \text{CH}\_3\text{C}(\text{O})\text{CH}\_3 \tag{4}$$

This mechanism is a very plausible one, as it explains acetone and formaldehyde formation after acetaldehyde adsorption at ambient temperature.

#### *3.2. Surface Species Formed during the PDC Process: Formation Mechanism*

Before turning the plasma on, the catalyst surface is mainly composed of adsorbed acetaldehyde. Part of this acetaldehyde yields crotonaldehyde (Reaction (1)); acetate (Reactions (2) and (3)), acetone and formaldehyde (Reaction (4)). DRIFTS measurements carried out on the catalyst exposed to the plasma reveal that acetaldehyde degradation proceeds with the formation of different surface compounds such as acetate, methoxy, ethoxy, formate and carbonate species, as well as formaldehyde and formic and acetic acid. It should be noted that, despite being referred to as formic acid and acetic acid, it is most likely formate and acetate species on the surface [40]. Indeed, previous studies have shown that photocatalytic oxidation of acetaldehyde could yield acetic and formic acid that remain adsorbed on the surface in a dissociated form, i.e., as acetate and formate, respectively (degradation routes Reactions (5) and (6)) [55,69].

$$\text{CH}\_3\text{CHO}\_\text{a} \rightarrow \text{CH}\_3\text{COO}\_\text{a}^- + \text{H}\_\text{a}^+ \tag{5}$$

$$\text{CH}\_3\text{CHO}\_3 \rightarrow \text{HCHO}\_3 \rightarrow \text{HCOO}\_3^- + \text{H}\_4^+ \tag{6}$$

The formation of acetate species on the catalyst surface has already been presented in the previous section. Nevertheless, once the plasma is turned on, two more routes may be considered. One route involves the acetyl radical resulting from adsorbed acetaldehyde decomposition by the plasma; which in turn can react with gas-phase oxygen to form acetate species (Reaction (7)) [56]. The other one is the reaction of gaseous acetaldehyde with an activated surface oxygen (Reaction (8)) [70]—indeed, it has been shown that the presence of silver atoms enhances the adsorption of oxygen on the catalyst and promotes its activation [22,71]. *above above above*

−−−−−−−−−−−−−→ *below below below*

$$\mathrm{CH\_3CHO\_a} \rightarrow \mathrm{CH\_3CO\_a} + \mathrm{H\_a} \xrightarrow{+\mathrm{O\_2}} \mathrm{CH\_3COO\_a^-} \tag{7}$$

$$\rm{CH\_3OH\_8^- + O\_a \to CH\_3COO\_a^- + H\_a^+} \tag{8}$$

Regarding formate species, its formation through oxidation of different compounds such as acetone (Reaction (9)) [55], acetate species (Reactions (10) and (11)) [46,55], formaldehyde (Reaction (12)) [55,72–74] and crotonaldehyde (Reaction (13)) [64] should be considered.

$$2\text{ CH}\_3\text{C(O)CH}\_3 \xrightarrow{\text{O}\_2} 2\text{HCOO}\_3^- + \text{H}\_a^+ + \text{CO}\_2 \tag{9}$$

$$\rm{CH\_3COO\_4^- + H^+ \to HCOO\_4^- + H\_a^+} \tag{10}$$

$$\rm CH\_3COO\_a^- \rightarrow CH\_3O\_a \rightarrow CH\_2O\_a \rightarrow HCOO\_a^- \tag{11}$$

$$\rm{HCHO} + \rm{O\_{a}} \rightarrow \rm{HCOO\_{a}^{-}} \tag{12}$$

$$\rm CH\_3(CH)\_2CHO\_a \to \rm HCOO\_a^- + H\_a^+ \tag{13}$$

Methoxy species may be formed following different routes, one of which involves methanol, a by-product of acetaldehyde decomposition by NTP. The proposed routes are direct oxidation of surface acetate species (Reaction (14)) [46], and dissociative adsorption of methanol (Reaction (15)) [75,76]. Indeed, on the basis of reaction mechanisms derived from model studies carried out under ultrahigh vacuum conditions on noble metal surfaces, methanol is activated by surface oxygen so that adsorbed methoxy species can form [77].

$$\rm{CH\_3COO\_4^-} \rightarrow \rm{CH\_3O\_4 + CO\_2} \tag{14}$$

$$\rm{CH\_3OH\_g} + \rm{S} \rightarrow \rm{CH\_3O\_a} + \rm{H\_a^+} \tag{15}$$

where S is a site on the oxide surface.

Concerning ethoxy species, one possible pathway has already been proposed through the Reaction (3) route. Moreover, it has been shown that TiO2-supported catalysts may significantly promote the reaction of acetaldehyde with adsorbed hydrogen formed in previous steps to form ethoxy species [54,66] (Reaction (16)).

$$\text{CH}\_3\text{CHO}\_4 + \text{H}\_4^+ \rightarrow \text{CH}\_3\text{CH}\_2\text{O}\_4^- \tag{16}$$

As for carbonate species, they may be produced from acetates (Reactions (17) and (18)) [56,67,70]. Furthermore, an investigation carried out using supported TiO<sup>2</sup> catalysts in the presence of H2O<sup>2</sup> [58] has shown that formate species interaction with the surface can lead to carbonate and acetone formation (Reaction (19)). This latter possibility should be considered in our case, as NTP is able to generate H2O2.

$$\rm{CH\_3COO\_3^-} + \rm{OH\_s} \rightarrow \rm{CO\_3^{2-}} + \rm{CH\_4} \tag{17}$$

$$\rm{2CH\_3COO\_3^-} \rightarrow \rm{CH\_3C(O)CH\_3\, a + CO\_3^{2-}} \tag{18}$$

$$\rm{HCOO\_{3}^{-}} \xrightarrow{H\_{2}O\_{2}} \rm{CO\_{3}^{2-}} \tag{19}$$

Regarding formaldehyde formation, in addition to Reaction (4) route, other routes may also be allowed for. These include formation of formaldehyde from acetaldehyde on TiO<sup>2</sup> surfaces, either directly or through an acetate intermediary (Reaction (20)) [55], from acetaldehyde oxidation by surface oxygen (Reaction (21)) [54], from surface ethoxy and methoxy species oxidation (Reactions (22) and (23)) [44,46,57] and as an intermediate in methanol oxidation (Reaction (24)) [74].

$$\text{CH}\_3\text{CHO}\_\text{a} \xrightarrow{\text{(CH}\_3\text{COO}\_3^-)} \text{HCHO}\_\text{a} + \text{HCOOH}\_\text{a} \tag{20}$$

$$\text{CH}\_3\text{CHO}\_4 + 2\text{O}\_8 \rightarrow \text{HCHO}\_4 + \text{HCOOH}\_4 \tag{21}$$

$$\rm CH\_3CH\_2O\_a^- \rightarrow \rm HCHO\_a \tag{22}$$

$$\rm{CH\_3O\_a} \rightarrow \rm{HCHO\_a} + \frac{1}{2} \rm{H\_2}\_{\rm g} \tag{23}$$

$$\text{CH}\_3\text{OH} \rightarrow \text{HCHO}\_4 + \text{H}\_2\text{ads} \tag{24}$$

It can be seen that routes through Reactions (20) and (21) are not only a possible source of formaldehyde, but also of formic acid.

Some authors working with photocatalytic degradation of acetaldehyde have also observed that the initially formed species, 3-hydroxybutanal and crotonaldehyde, are converted to other intermediates upon illumination of the catalyst. Among the main intermediates, they have identified formic acid, acetic acid and formaldehyde, and this is in accordance with our results [40,64].

It is important to bear in mind that some of the species identified on the catalyst surface after the PDC process can also be formed directly in the gas phase. Indeed, gas-phase acetaldehyde decomposition by NTP can lead to the formation of methoxy radical, as well as acetone, acetic acid and formaldehyde [78], which can subsequently adsorb on the surface.

#### *3.3. Proposed Simplified Mechanism for Acetaldehyde Decomposition Using the Plasma*/*Catalysis Process*

From the identified gaseous by-products, surface IRbands' assignment and proposed adsorption/ degradation routes—a schematic diagram of the possible pathways for acetaldehyde degradation over Ag/TiO2/SiO<sup>2</sup> in the PDC process is presented in Figure 4. It is worth noting that we have not detected formaldehyde at the exit of the DBD reactor whereas it has been detected on the catalyst surface. There are two reasons for this: formaldehyde is a short-lived species [77] and it is strongly adsorbed onto silver catalyst [79].

*Catalysts* **2020**, *10*, x FOR PEER REVIEW 10 of 16

selectivity is dependent on the O3:HCHO ratio and the relative humidity (RH). In this work, for a O3:HCHO ratio of 5 (best ratio) and 20% RH, 90% of HCHO removal and a CO/CO2 ratio of 1.5 were

**Figure 4.** Schematic diagram of the proposed reaction pathway of the PDC degradation of acetaldehyde on Ag/TiO2/SiO2. The line patterns (solid line, dotted line, dashed line) represent, respectively, either direct routes or routes involving reactions with simple radicals/atoms/sites on the surface (H/OH/O/VO/S), routes involving two surface species and routes leading to the formation of by-products observed only at high energy. Blue color compounds: not detected/identified. **Figure 4.** Schematic diagram of the proposed reaction pathway of the PDC degradation of acetaldehyde on Ag/TiO<sup>2</sup> /SiO<sup>2</sup> . The line patterns (solid line, dotted line, dashed line) represent, respectively, either direct routes or routes involving reactions with simple radicals/atoms/sites on the surface (H/OH/O/VO/S), routes involving two surface species and routes leading to the formation of by-products observed only at high energy. Blue color compounds: not detected/identified.

As presented in Section 2.1, except from Ace and the fraction corresponding to the unknown compounds, the same by-products are obtained with the NTP and PDC processes. This fact allows the drawing of an initial conclusion concerning Ace and MeF formation. Indeed, at the experimental conditions used, Ace seems to be generated only on the surface, and most certainly through the ketonization of acetic acid/acetate species. In addition, with NTP at 150 J∙L-1 there is no formation of MeF, whereas with the PDC process it is already formed at 70 J∙L-1, and in equivalent amounts to the other acetate/formate compounds. Thus, it is clear that the catalyst surface promotes MeF formation. As mentioned earlier, Me can be activated by surface oxygen. In a study on methanol oxidation over silver catalysts, the authors reported that the catalytic oxidative reaction of methanol to methyl formate is related to a synergic process concerning oxygen species on the silver surface. The It is very likely that EdF and EmF are formed through the esterification of ethylene glycol (EG) and formic acid, even if there is no evidence of the presence of EG either on the effluent or on the surface. However, it is well-known that silver catalysts are commonly used in the manufacturing process for the direct oxidation of ethylene to ethylene oxide (EO) [80], and EO is a precursor of EG [81,82]. Besides, ethylene and EO can be formed from acetaldehyde decomposition on the surface [83–86]. Thus, EdF and EmF formation through an EG pathway is very plausible in the PDC process. In addition, low-energy, electron-induced processes on Me have been proven to induce the formation of methoxy (CH3O) and hydroxymethyl (CH2OH) radicals via electron impact excitation, which, followed by radical–radical coupling, can lead to EG and formic acid formation [87], therefore explaining EmF and EdF production with NTP alone.

mechanism proposed in this Os-Me system starts with methanol dehydrogenation to form adsorbed formaldehyde and methoxy; thereafter, formaldehyde reacts with adsorbed OH or O to form adsorbed formate, that reacts with methoxy and forms methyl formate [79,90]. Thus, Me formed as a by-product of acetaldehyde decomposition can be the precursor of MeF, with formaldehyde and CH3O as intermediates. In addition, as presented in Figure 1, NTP at 150 J∙L-1 produces more Me and AcA than the PDC process. Thus, we can suggest that the lower amount of Me is related to its decomposition into formaldehyde and CH3O, that will in turn produce MeF; and the lower amount of AcA is probably related to the preferential decomposition of acetate through other routes than the one at its origin. From spectra in Figure 3 we have seen that bands corresponding to methoxy, acetate and formaldehyde are present at 70 J∙L-1, which stresses the feasibility of the proposed mechanisms for Ace and MeF formation. Increasing SIE from 70 to 350 J∙L-1 increases acetaldehyde degradation from 33% to 87%, which leads to an important rise in the concentration of all the identified by-products. CO concentration increases 8-fold, whereas the other compounds experience a 2.5- to 4-fold increase. This result confirms the fact that acetaldehyde degradation follows a pathway favoring CO formation. In this diagram we did not include the pathways leading to CO<sup>2</sup> and CO formation as there are many possibilities. The different routes to CO<sup>x</sup> can involve many of the different adsorbed species or gaseous organic compounds. Nevertheless, it is worth noting that increasing the energy in the PDC process also increases the selectivity towards CO. In order to explain this result, we have proposed in a previous work a decarbonylation process of acetaldehyde on the silver-based catalyst [27]. However, this higher CO selectivity can also be the result of the by-products' decomposition pathways. According to a study on the mechanism of the heterogeneously-catalyzed oxidation of organic molecules on metal oxides, it has been stated that formate ions rather easily decompose to CO over metal oxides [88]. Furthermore, an experimental study of ozone catalytic oxidation of gaseous formaldehyde using a TiO2-supported catalyst at room temperature has shown that CO<sup>x</sup> selectivity is dependent on the O3:HCHO ratio and the relative humidity (RH). In this work, for a O3:HCHO ratio of 5 (best ratio) and 20% RH, 90% of HCHO removal and a CO/CO<sup>2</sup> ratio of 1.5 were achieved, making CO the major product [89]. Similar results regarding higher conversion towards CO than CO<sup>2</sup> where obtained when using TiO2-supported catalysts for ethanol oxidation; and it is well-known that acetaldehyde is one of the major intermediate species in ethanol decomposition [70].

Concerning the catalyst surface composition, in Figure 3b we can see the emergence of a peak at 2914 As presented in Section 2.1, except from Ace and the fraction corresponding to the unknown compounds, the same by-products are obtained with the NTP and PDC processes. This fact allows the drawing of an initial conclusion concerning Ace and MeF formation. Indeed, at the experimental conditions used, Ace seems to be generated only on the surface, and most certainly through the

ketonization of acetic acid/acetate species. In addition, with NTP at 150 J·L −1 there is no formation of MeF, whereas with the PDC process it is already formed at 70 J·L −1 , and in equivalent amounts to the other acetate/formate compounds. Thus, it is clear that the catalyst surface promotes MeF formation. As mentioned earlier, Me can be activated by surface oxygen. In a study on methanol oxidation over silver catalysts, the authors reported that the catalytic oxidative reaction of methanol to methyl formate is related to a synergic process concerning oxygen species on the silver surface. The mechanism proposed in this Os-Me system starts with methanol dehydrogenation to form adsorbed formaldehyde and methoxy; thereafter, formaldehyde reacts with adsorbed OH or O to form adsorbed formate, that reacts with methoxy and forms methyl formate [79,90]. Thus, Me formed as a by-product of acetaldehyde decomposition can be the precursor of MeF, with formaldehyde and CH3O as intermediates. In addition, as presented in Figure 1, NTP at 150 J·L <sup>−</sup><sup>1</sup> produces more Me and AcA than the PDC process. Thus, we can suggest that the lower amount of Me is related to its decomposition into formaldehyde and CH3O, that will in turn produce MeF; and the lower amount of AcA is probably related to the preferential decomposition of acetate through other routes than the one at its origin. From spectra in Figure 3 we have seen that bands corresponding to methoxy, acetate and formaldehyde are present at 70 J·L −1 , which stresses the feasibility of the proposed mechanisms for Ace and MeF formation.

Increasing SIE from 70 to 350 J·L −1 increases acetaldehyde degradation from 33% to 87%, which leads to an important rise in the concentration of all the identified by-products. CO concentration increases 8-fold, whereas the other compounds experience a 2.5- to 4-fold increase. This result confirms the fact that acetaldehyde degradation follows a pathway favoring CO formation. Concerning the catalyst surface composition, in Figure 3b we can see the emergence of a peak at 2914 cm−<sup>1</sup> , which has been assigned in Section 2.3 either to adsorbed acetaldehyde or to an intermediate formed from formaldehyde oxidation or disproportionation. Considering all the above, this peak could rather be assigned to the intermediate formed from formaldehyde oxidation to formate species, that will subsequently lead to the formation of the different formate compounds. This is supported by the loss of the band centered at 1870 cm−<sup>1</sup> , attributed to formate species, for which desorption from the surface may be favored at this energy. Similarly, the growth of a rather broad band in the 1300–950 cm−<sup>1</sup> region observed in Figure 3a should rather be assigned to methoxy species that can also promote formate species formation.

When increasing SIE to 1150 J·L −1 , two different behaviors among the by-products were observed: (i) those whose concentration remains rather constant (CO2, MeO, MeF and Ace), (ii) those whose concentration almost doubled (CO, MeA, EdF, EmF and AcA). Therefore, it seems that once formate/ formaldehyde are formed, the path that would be favored is the one towards formic acid and then EmF and EdF. Additionally, acetates will be transformed into AcA and MeA rather than into Ace.

#### **4. Materials and Methods**

#### *4.1. Catalyst Preparation*

Silver nanoparticles deposition was performed following the method presented in a previous study [91]. In this same study, atomic forcemicroscopy (AFM, Veeco, Munich, Germany), scanning electron microscopy (SEM, Supra 40 VP, Zeiss, France) and transmission electron microscopy (TEM, 200 kV JEM 2011, JEOL, France) measurements showing a homogeneous dispersion of silver nanoclusters on the TiO<sup>2</sup> monolayer can be found. The silver nanoparticles were deposited on 150-µm-diameter SiO<sup>2</sup> pellets (Sigma-Aldrich silica gel, St. Louis, MO, USA). The pellets were first covered by a size-selected titanium oxo-alkoxy (TOA, Sigma-Aldrich, St. Louis, MO, USA, 99.999% purity)) nanoparticles monolayer synthesized in a rapid micromixing sol-gel reactor. Then, the silver nanoclusters (10 nm mean diameter) were grown on the TOA monolayer by photocatalytic reduction of an Ag<sup>+</sup> aqueous solution (AgNO3, Prolabo, Prolabo, Paris, France, 99.8% purity), under ultraviolet (UV) irradiation (Philips, Haarlem, The Netherlands, operating at 362 ± 10 nm, 8W). Finally, the pellets were washed in distilled water and

dried at 80 ◦C for 4 h. A 303 m2g <sup>−</sup><sup>1</sup> BET (Brunauer–Emmet–Teller) (Beckman Coulter, Brea, CA, USA, SATM 3100) specific surface area was measured.

#### *4.2. Plasma*/*Catalysis Process*

A DBD reactor previously described [27], was used for acetaldehyde removal at room temperature and atmospheric pressure. The DBD reactor is composed of a quartz cylinder externally covered by a grounded stainless steel. A sinusoidal high voltage is applied to a stainless steel cylindrical center electrode through a 5-mm gap. This high voltage is obtained using a voltage amplifier (TREK, 20/20 C, France), coupled to a frequency generator. Different values of the specific input energy (SIE in J·<sup>L</sup> −1 ), defined as the ratio of the discharge power (W) over the flow rate (L·s −1 ), were obtained by changing the frequency of the signal. When using the PDC process, the Ag/TiO2/SiO<sup>2</sup> nanostructured catalyst was placed in the plasma discharge zone.

The pollutant mixture was composed of acetaldehyde (1000 ppmC), oxygen (20%) and nitrogen (balance) (Air Liquide AlphagazTM 1), and the flow rate was set to 100 mL·min−<sup>1</sup> (Bronkhorst El-Flow® Select). The gas was admitted at the bottom of the DBD reactor and flowed upward through the fluidized bed. At the exit, it was sent to a set of analyzers: gas chromatography (Shimadzu GC-2110, Shimadzu, Noisiel, France), for quantitative analysis of residual acetaldehyde; gas chromatography coupled to mass spectrometry, for identification of the gaseous by-products (Shimadzu 2110-GC coupled to a QP2010S-MS, Shimadzu, Noisiel, France); and an infrared multigas analyzer (MIR 9000, Environment SA, France), for CO<sup>2</sup> and CO quantification. The plasma-catalysis experiments were carried out in two stages: (i) the catalyst surface was saturated by acetaldehyde at room temperature and atmospheric pressure, and (ii) the plasma discharge was switched on for 30 min to induce acetaldehyde removal on the surface in the same temperature and pressure conditions. The surface was then characterized by DRIFTS analysis.

#### *4.3. DRIFTS Measurements*

DRIFTS analyses were performed with a Shimadzu IRPrestige-21 spectrophotometer (DLATGS detector, 100 scans accumulation, and 4 cm−<sup>1</sup> resolution, Shimadzu, France). A Pike DiffusIRTM accessory (Pike, Eurolabo, France) containing a chamber equipped with a KBr window was adapted on the FTIR spectrophotometer. This chamber can contain a cup with approximately 10 mg of catalyst. All DRIFTS spectra presented were acquired in transmittance mode.

#### **5. Conclusions**

In summary, we used DRIFT spectroscopy to identify the adsorbed species formed on an Ag/TiO2/SiO<sup>2</sup> surface during acetaldehyde adsorption and degradation with a PDC process. The measurements showed that different species such as acetate, formate, methoxy, ethoxy and formaldehyde are present on the surface, once it has been in contact with the plasma.

A pathway that considers the formation of these intermediates via the interaction of adsorbed acetaldehyde, and the plasma-generated species and/or by-products of acetaldehyde decomposition in the gas phase is proposed. The main carbonaceous intermediates identified allowed more detailed mechanism for acetaldehyde degradation to be given, as well as the formation of most of the identified by-products detected in the gas phase leaving the reactor to be explained.

Further investigations are needed to include nitrogenous species detected in the gas phase in the mechanism of acetaldehyde degradation with the PDC process. It is very likely that in CH3CHO degradation the presence of methanol, one of the intermediate by-products in CH3CHO oxidation, combined with oxygen activation by silver atoms on the surface, are key elements in the performance of the PDC process.

**Author Contributions:** Conceptualization, A.V.-G., X.D. and S.S.; Formal analysis, A.V.-G., X.D. and S.S.; Funding acquisition, X.D.; Investigation, A.V.-G., X.D. and S.S.; Methodology, A.V.-G., X.D. and S.S.; Supervision, A.V.-G. and X.D.; Validation, A.V.-G. and X.D.; Writing—original draft, A.V.-G. All authors have read and agreed to the published version of the manuscript.

**Funding:** This research was funded by the ANR Programme Blanc grant ANR-08-BLAN-015–01 à 04)) and Region Ile de France grant IF-110005975 and 10005961).

**Acknowledgments:** The authors wish to thank Nicolas Fagnon for the Labview program used for the automated data acquisition during the DRIFTS experiments.

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

#### **References**


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