Sammy W.
Verbruggen†
ab,
Kasper
Masschaele†
b,
Elke
Moortgat
b,
Tamas E.
Korany
b,
Birger
Hauchecorne
a,
Johan A.
Martens
*b and
Silvia
Lenaerts
*a
aFaculty of Science, Department of Bioscience Engineering, Research unit Sustainable Energy and Air Purification, University of Antwerp, Groenenborgerlaan 171, B-2020 Antwerp, Belgium. E-mail: silvia.lenaerts@ua.ac.be
bFaculty of Bio-engineering, Department of Microbial and Molecular Systems, Kasteelpark 23, 3001 Heverlee (Leuven), Belgium. E-mail: Johan.Martens@biw.kuleuven.be
First published on 13th June 2012
The photocatalytic activity of two commercial titanium dioxide powders (Cristal Global, Millennium PC500 and Evonik, P25) is compared towards acetaldehyde degradation in the gas phase. In contrast to the extensive literature available, we found a higher activity for the PC500 than for the P25 coating. Here, we present a comprehensive characterization of the bulk and surface properties of both powders. Our comparison shows that the material properties that dominate the overall photocatalytic activity in gas phase differ from those required for the photodegradation of water-borne pollutants.
Recently, the large potential of gas phase photocatalysis for environmental applications has been postulated since a wide range of air contaminants including alkanes,5 alkenes,6 halocarbons,7 alcohols,8 aldehydes,9 nitrogen-containing compounds,10 and ketones11 can be partially or completely degraded with the TiO2-assisted UV irradiation. In addition, TiO2 based semiconductors have been used for the photocatalytic degradation of chlorinated organics, pesticides and herbicides, surfactants, dyes, and destruction of bacteria, viruses, and molds in water.3 In this context it is worthwhile pointing out that photocatalytic methods of decontamination are ideal since they operate at near ambient conditions using only light as the source of energy. Thus, photocatalysis has emerged as an advanced oxidation process (AOP). Although some success has been realized in the complete oxidation of several organics at the laboratory scale, photocatalysis using TiO2 still suffers from relatively low quantum efficiency.
Here, the photocatalytic degradation of acetaldehyde into CO2 and H2O is studied on two titanium dioxide catalysts. The goal of our study is to determine the required material properties to obtain an optimal photocatalytic activity. Previous reports have discussed the photocatalytic degradation of acetaldehyde in detail,12–17 but in addition it has been recognized that acetaldehyde is encountered as an intermediate in the photocatalytic degradation of ethanol.18,19
In this work, we study photocatalytic degradation of acetaldehyde in the gas phase using two commercial TiO2 nanopowders (Millennium PC500 and Degussa P25). In contrast to many earlier reports and especially water-borne applications, we observed better activity for the PC500 than for the P25 powder.20–23 The aim of this work is to get a fundamental understanding of the parameters that determine the photocatalytic activity of a photocatalyst for gas phase purification. A comprehensive characterization of both materials enables us to distinguish the important bulk and surface parameters. More specifically, the operating principles in the gas and water phase performance are of major interest.
The concentration of the reagents and products was monitored in time by on-line FTIR spectroscopy of the outlet gas flow. The absorbance peak heights of vibrations of molecules of interest were plotted as a function of time by recording four to five FTIR spectra per minute and analyzing the peaks with the MacrosBasic software (Thermo Fisher). In particular, for acetaldehyde, CO2 and CO the peak heights were recorded at wavenumbers of 2728 cm−1, 2360 cm−1 and 2179 cm−1 respectively. These positions were selected because they do not interfere with other vibrations in the spectrum. The automation of the test set-up is described in more detail by Tytgat et al.25
UV-VIS absorption spectra were collected in the range of 300–700 nm using a Shimadzu UV-2501PC double beam spectrophotometer equipped with a 60 mm BaSO4 coated integrating sphere and a Photomultiplier R-446U detector.
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Fig. 1 Concentration profiles of acetaldehyde and CO2 over P25 (solid line) and PC500 (dashed line) in the outlet gas stream during one experiment. The acetaldehyde inlet concentration is 100 ppmv in air at a total flow rate of 2000 cm3 min−1. Red: CO2, blue: H2O, black: acetaldehyde. |
When UV illumination is switched on in step III, the FTIR signal reveals an immediate decrease in the acetaldehyde concentration in the outlet gas-stream, and additionally CO2 is formed. The decreased acetaldehyde concentration in combination with the formation of CO2 indicates photo-induced degradation of acetaldehyde. When the reactor was loaded with uncoated glass beads no acetaldehyde conversion was found, indicating the absence of photolysis.
Probing the acetaldehyde concentration in the outlet gas-stream it is suggested that for the P25, an equilibrium is established after approximately 10 minutes and a steady-state conversion of 93 ± 1% is observed. The PC500 material shows steady state behavior after more than 30 minutes and shows nearly 100% conversion. The steady-state concentrations of CO2 monitored by FTIR peak height are consistent with the trend observed from the acetaldehyde levels during degradation, with more acetaldehyde degradation at PC500 coated beads compared to P25 coated ones. Initially, the excessive conversion on PC500 is significant compared to the P25 powder, as can be verified from Fig. 1, step III. The observed overshoot in the produced CO2 concentration for PC500 is reproducible (data not shown) and the height of the overshoot is determined by the acetaldehyde loading concentration. For an increasing inlet concentration of acetaldehyde the overshoot gradually decreased and finally disappeared completely. The P25 samples on the other hand succeeded in a degradation of 76% of the introduced acetaldehyde in a 170 ppmv flow, in contrast to a conversion of 99% for the PC500 coated beads (data not shown). For a 100 ppmv inlet stream the turnover frequency (TOF) of acetaldehyde on PC500 and P25 equals 0.7 mol per mol TiO2 per hour, and 0.54 mol per mol TiO2 per hour, respectively. Furthermore, for the P25 the absolute amount of acetaldehyde degraded was independent of the inlet concentration (for concentrations exceeding 170 ppmv). This suggests that the degradation rate is kinetically determined (light absorption or charge transfer) and mass transfer issues can be neglected in this case.
The steady state conversion remains constant for long times which convinces us that adsorbed intermediates do not affect the activity of the photocatalyst, nor the absence of additional humidity becomes the rate limiting step. Fouling or poisoning of the catalyst would result in a gradual decrease in activity because all active sites are occupied and no further conversion is observed. Absence of water near the surface could result in a lower rate of OH radical formation during illumination. In any case, initially the photocatalysts contain an appreciable amount of physically and chemically adsorbed water. Furthermore, water is formed during the photocatalytic degradation of acetaldehyde as shown in Fig. 1 and previously reported by us.17 Long term measurements for 30 hours showed that there was no observable decrease in acetaldehyde degradation or CO2 formation (data not shown).
In the following we characterize the PC500 and P25 powders and distinguish the important material properties:
1. Surface properties
2. Bulk properties
3. Morphology
The bulk properties will determine the photon-to-electrical conversion in the form of electron–hole pairs (quantum efficiency). Ideally the bulk properties support charge separation of the photo-generated holes and electrons, resulting in good apparent quantum efficiency. Secondly, the surface properties will determine to a great extent the activity of the catalyst. A high concentration of reactive species and optimal adsorption behavior are preferred. Finally, the morphology is important because of possible diffusion limitations and effective available surface area. Therefore, the thickness, porosity and crystal structure of the coatings need to be optimized.27
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Fig. 2 (a) DRS UV-VIS and XRD (b) scans for titanium dioxide powders P25 and PC500. Anatase: A, rutile: R. |
Using the Kubelka–Munk function, the bandgap energies of P25 and PC500 are calculated to be 3.08 and 3.20 eV respectively. The bandgap of PC500 corresponds to that of pure TiO2 anatase, whereas the lower bandgap of P25 can be explained by the presence of 20% rutile. Although, the absorption spectra reveal the photoresponse, the photocatalytic behavior is determined by measuring the generated photocurrents upon illumination in different electrolyte solutions.28 To this extent, transparent electrodes of P25 and PC500 were coated on ITO glass slides and subsequently illuminated under a bias of +0.2 V vs. Ag/AgCl. When an electrolyte containing 1 M NaOH was used, the photocurrent generated on the P25 electrodes was found to be much higher than for the PC500 electrode, as shown in Fig. 3. However, when methanol (15 vol%) was added to the electrolyte the P25 electrode gave higher photocurrents compared to the pure water system (an increase from 950 to 1900 μA), but the PC500 electrode showed an increase in the photocurrent by a factor of 200 (from 4 to 730 μA).
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Fig. 3 Average photocurrents measured over P25 (a) and PC500 (b) electrodes. The first bar is the average photocurrent measured in water only, the second bar is the average photocurrent measured in water with methanol added. |
These results enable a direct distinction between pure bulk and surface behavior. In a pristine 1 M NaOH electrolyte the generated photoholes are consumed by OH-groups, while dissolved oxygen is reduced by the photo-electrons. When methanol is added, on the other hand, methanol oxidation is preferred over water splitting. It has been shown that the TiO2 hole transfer to methanol is an ultrafast process and can proceed with a time constant of ≈300 ps, while for water it can be as high as 2 ms.29 By overcoming the limitations of the hole transfer step with sacrificial donors (methanol), it is possible to boost the lifetime of electrons.30 Use of alcohols such as methanol31 as sacrificial donors has also been found to be favorable in doubling the photocurrent generation in photoelectrochemical cells since the alkoxy radicals formed upon hole oxidation are capable of delivering electrons to the semiconductor electrode.32 By adding methanol to the electrolyte we have eliminated to a certain extent the effect of the surface properties that enables us to conclude that more bulk recombination occurs in the PC500 catalyst compared to the P25 (approximately a factor of 2–3). For two materials having a similar surface concentration of surface hydroxyls, but different quantum efficiency (photon-to-exciton conversion), the material with the highest quantum efficiency will yield a higher number of hydroxyl radicals per unit surface area.
The improved quantum efficiency of P25 is attributed to the crystalline structure with crystallites of 30 nm and an anatase/rutile ratio of approximately 4/1, as can be seen in Fig. 2(b). Although the mechanism remains speculative, it is expected that the interface between the rutile and anatase crystals favors charge separation for longer time periods.33 The PC500 on the other hand was found to be 75% anatase with a primary particle size of approximately 5–10 nanometers and 25% amorphous titanium dioxide which favors bulk recombination resulting in a lower overall conversion of photons in photo-generated charge carriers. Although the photocurrent measurements give direct evidence for a lower photon conversion per unit of surface area on the PC500, some additional sources for recombination are introduced in the latter experiments. The photogenerated electrons need to travel towards the ITO substrate. The amorphous nature of PC500 and the small primary particle size create many possible trapping sites and thus an enhanced recombination of photo-generated charge carriers, lowering the observed photocurrents. In the original gasphase experiments the electrons have to diffuse only to small distances before they reach the electrolyte and reduce the adsorbed oxygen.
CH3CHO + 3H2O + 10h+ → 2CO2 + 10H+ | (1) |
CH3CHO + H2O + 2h+ → CH3COOH + 2H+ | (2) |
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Fig. 4 (a) Adsorption/desorption isotherms of P25 and PC500 and (b) pore volume distribution plot of P25 and PC500. A logarithmic scale for the pore width was used for clarity purposes. |
The effective surface area available for acetaldehyde adsorption on PC-500 was found to be 3.5 times higher compared to the P25, as determined from Fig. 5. Integration of the area in zone I, and in zones I + II, provides estimates of the amount of adsorbed acetaldehyde on the P25 and PC500, respectively. The total surface area of PC500, as determined from BET, was six times larger than that of P25, but the effective surface area for acetaldehyde adsorption is found to be much smaller. A study of the surface chemistry of both powders should indicate the origin of this difference.
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Fig. 5 Outlet concentration of acetaldehyde after adsorption on P25 and PC500 in function of time. |
1. the surface hydroxyl concentration
2. the surface cation concentration
3. the presence of adsorbed intermediates, oxygen, surface groups. It is commonly acknowledged that hydroxyl groups play a major role in the photo-oxidation of organic compounds. Here, we will investigate the total number of surface hydroxyls and the surface density of hydroxyls on both materials. Secondly, Fourier Transformed Infrared spectra enable us to study the interactions between acetaldehyde molecules and the surface hydroxyl groups. A first estimate of the physically and chemically bonded water or hydroxyls is given by thermogravimetric measurements (TGA). Most of the physically bound water is expected to evaporate at temperatures around 170–200 °C. At higher temperatures, the chemically bound hydroxyls are released, and at temperatures exceeding 400 °C phase transformation can be expected. For the P25, the total mass loss at 400 °C is approximately 2.5%. The total mass of the PC500 decreases rapidly up to temperatures of 400 °C, and then levels off. At a steady temperature increase of 10 °C min−1 almost 17% mass loss was found for the PC500 at 400 °C. If only the mass loss between 170 °C and 400 °C is considered, a simple estimation yields values of 2.7 OH per nm2 for PC500 and 5 OH per nm2 for P25, which is in good agreement with suppliers info. FTIR analysis of the OH stretching region (4000–3500 cm−1) on both materials was in agreement with the spectrum earlier reported in the literature.34
The FTIR spectra of P25 and PC500 when brought into contact with acetaldehyde discern differences in acetaldehyde adsorption. Fig. 6 shows the spectra after equilibrating the reactor for 10 min with acetaldehyde in air. The FTIR spectrum of acetaldehyde in the gas phase is shown in Fig. 6(a), and the typical peaks for the carbonyl group are present at 1761, 1746, and 1734 cm−1. When the acetaldehyde is adsorbed, the carbonyl bands are redshifted towards lower wavenumbers, indicating a significant interaction between the acetaldehyde molecules and the TiO2 surface. In the case of P25 (see Fig. 6(b)), it is found that acetaldehyde adsorbs in two different ways on the TiO2 surface. A H-bridge can be formed with a surface hydroxyl group (CH3CHO⋯HO–Ti), resulting in a redshift of the IR band to 1714 cm−1. The second mode results in an IR band at 1693 cm−1 and is assigned to the carbonyl bonding with a cation Ti4+-surface group (CH3CH
O⋯Ti4+).35 For the adsorption on PC500 (see Fig. 6(c)) on the other hand, only at 1714 cm−1 an IR absorption peak was found, indicating that the acetaldehyde dominantly binds with a surface hydroxyl of the PC500 surface. The presence of high amounts of water that preferentially bind to the cations might be a possible explanation. The peak absorbed at 1633 cm−1 is attributed to Ti4+ coordinated water, and that at 1621 cm−1 to water coordinated through hydrogen bonds.36 Overall, bands near 1630 cm−1 are assigned to adsorbed water.
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Fig. 6 IR spectra at RT of (a) acetaldehyde in the gas phase; (b) acetaldehyde after 10 min adsorption on P25; (c) acetaldehyde after 10 min adsorption on PC500. Wavenumbers are summarized in Table 1. |
Species [1] | Mode [1] | Gas | P25 | PC500 |
---|---|---|---|---|
CH3CHOg |
ν(C![]() |
1761 | ||
CH3CHOg |
ν(C![]() |
1746 | ||
CH3CHOg |
ν(C![]() |
1734 | ||
CH3CHOad |
ν(C![]() |
1714 | 1714 | |
CH3CHOad |
ν(C![]() |
1693 | ||
Ti–OH2 | δ(OH) | 1633 | ||
Ti–OH2 | δ(OH) | 1621 | ||
CH3COOad− | ν as(COO) | 1568 | ||
CH3COOad− | ν as(COO) | 1532 | ||
CH3COOad− | ν s(COO) | 1453 | ||
CH3CHOg | δ as(CH3) | 1436 | ||
CH3CHOad | δ(CH3) | 1400 | ||
CH3CHOg | δ s(CH3) | 1395 | ||
CH3CHOad | δ(CH3) | 1377 | ||
CH3CHOg | δ(CH) | 1352 | ||
CH3CHOad | δ(CH) | 1353 | 1344 |
Broad bands near 1550 cm−1 and 1444 and 1400 cm−1 were observed only for the PC500, which are attributed to acetic acid and acetate νas and νs vibrations respectively.37 Although acetic acid adsorbed on titanium dioxide is expected to induce absorption peaks at 1415 cm−1 and 1540 cm−1, the peak at 1400 cm−1 is intriguing. The coordination of adsorbed acetic acid or acetate by adsorbed or dissociated water may reduce possible vibration modes. The band at 1540 and 1400 cm−1 persisted upon heating of the PC500 sample, where the 1541 and 1414 cm−1 peaks remained even up to 400 °C, which may indicate strong adsorption of the acetic acid on the TiO2 surface.37
In Table 2 a brief overview of the studied parameters is given. The high surface area of PC500 is found to be an enormous advantage for the gas phase degradation of acetaldehyde. The adsorbed amount of acetaldehyde agrees with the total number of OH groups on the PC500 surface, and thus exceeds the adsorbed quantity on P25 by a factor of 3.5 (ratio equals 0.28). If acetaldehyde adsorption would only occur through interaction with surface hydroxyls, a factor of 4 would be expected, but from FTIR analysis it was found that on P25 adsorption occurs also on Ti4+ cations. The improved activity (TOF) of PC500 in comparison with P25 is thus rationalized by considering the high surface area, absolute amount of surface hydroxyls, adsorption and the possible reaction paths which can be determined by the photo-absorption efficiency, as discussed in Section 3.3. Considering surface properties alone, the TOF on P25 would be approximately 0.25 of that on PC500. In our experiments, however, the TOF on P25 is 0.77 of that on PC500, which is believed to be attributed to the bulk properties. Indeed the high crystallinity of P25 compared to PC500 is confirmed by XRD in Fig. 2 and the larger bandgap for PC500 implies a lower quantum efficiency for PC500 compared to P25. Unfortunately, current data do not provide enough information to quantitatively determine the major losses. Recombination losses due to the high fraction of amorphous titanium dioxide are believed to further decrease the quantum efficiency on PC500, eventually resulting in a ratio of the TOF of 0.77.
Property | Ratio P25/PC500 |
---|---|
TOF | 0.77 |
Total surface area | 0.15 |
OH surface density | 2 |
OH total amount | 0.25 |
Acetaldehyde adsorbed | 0.28 |
In summary, in the specific case of acetaldehyde oxidation in the gasphase the high surface area of PC500 can be fully exploited. Although the low hydroxyl concentration per unit area and the inferior quantum efficiency will limit the available hydroxyl radicals during illumination, the PC500 material is found to have a higher TOF than P25.
Our results confirm that for photocatalytic degradation of VOC in the gas phase a high surface area is beneficial. Earlier reports, however, indicate that the photodegradation of water-borne organic dyes or organic pollutants occurs better on P25 compared to PC500. The reason is believed to be two-fold. First, the experiments are performed at slightly acidic pH, due to dissolved CO2 in DI or RO water. The isoelectric points (IEP) of P25 and PC500 are 7.0 and 6.2, respectively,38 meaning that a P25 surface will have a net positive charge, while the PC500 is slightly negative, in slightly acidic media. Most targeted pollutants in water purification applications, like (azo-)dyes, have a negative charge, due to a relatively low pKa value.39 Electrostatic repulsions between pollutants and the PC500 catalyst surface inhibit adsorption and prevent facile charge transfer. The positive Ti4+ groups on the P25 surface on the other hand attract the anionic pollutants and promote subsequent adsorption. For very acid solutions, where the PC500 surface also carries a net positive charge, it has been shown that PC500 shows a higher activity compared to P25.3 Secondly, the effective available surface for PC500 is expected to be much smaller due to the complex structure of the pores, and the full potential of the PC500 surface cannot be exploited. The adsorbed and bulk water in the nanopores is believed to hinder an easy diffusion of molecules. On the other hand, the absence of bulk water in gas phase experiments is expected to complicate desorption of intermediates.40 The accumulation of intermediates on the catalysts surface is expected to result in a gradual decrease in activity, which was not observed in the experiments presented here.
Finally, based on our work we conclude with suggestions for an optimized photocatalyst. A first possible route is the improvement of the degree of crystallinity of PC500, while maintaining the high surface area, by decoupling morphological and functional effects of annealed nanostructured porous coatings. Prior to a 550 °C annealing, the PC500 coating is encapsulated by a SiO2 scaffold to convert all amorphous titanium dioxide into highly crystalline anatase.41 Subsequently, the silica is dissolved in a 2 M NaOH solution. In this way, the high surface area is retained, and the degree of crystallinity increases. Secondly, the surface density of the hydroxyls can be increased by a hydrothermal treatment,42 enhancing the activity.
Footnote |
† These authors contributed equally to this work. |
This journal is © The Royal Society of Chemistry 2012 |