In-Situ FTIR Study of Heterogeneous Oxidation of SOA Tracers by Ozone

Introduction

Organic tracers have been used widely for source apportionment of organic aerosols under the assumption that they are not reactive in the atmosphere (Katrib et al., 2005; Kleindienst et al., 2007; Ding et al., 2012; Lai et al., 2014). However, previous studies have indicated that some of those tracers may not remain stable, which leads to the inaccurate estimation of source contributions (And and Smith, 2004; Weitkamp et al., 2008a; Hoffmann et al., 2010; Lambe et al., 2012; Wang et al., 2020). Weitkamp et al. studied the ozone oxidation of primary organic tracers of cooking oil emission (oleic acid, palmitoleic acid, and cholesterol etc.) through a series of chamber experiments. The results showed that the rate constant of ozone heterogeneous oxidation of oleic acid was 1.5 × 10⁻¹¹ cm³ molec⁻¹ sec⁻¹, which was ten times of cholesterol and four times of palmitoleic acid (Weitkamp et al., 2008b). Lambe et al. studied the effective reaction rate of oxidation reaction of norhopane, an organic tracer of motor oil by hydroxyl radical, and the rate constant of norhopane was 8.4 × 10⁻¹² cm³ molec⁻¹ s⁻¹ (Lambe et al., 2009). The study of Hennigan et al. indicated that rate constant of levoglucosan was 1.1 × 10⁻¹¹ cm³ molecule⁻¹s⁻¹ when biomass burning particles were exposed to 1 × 10⁶ molecules cm⁻³ of OH (Hennigan et al., 2010).

The above studies were focused on the heterogeneous oxidation of primary organic tracers, while such investigations on the secondary organic tracers have seldom been reported. And there is no clear conclusion about the complexity of heterogeneous oxidation of secondary tracers. Kessler et al. used the erythritol as a surrogate for 2-methyltetrols and studied heterogeneous oxidation of pure erythritol particles by gas-phase OH radicals with an effective OH uptake coefficient, γ_eff, of 0.77 ± 0.1 and a corresponding chemical lifetime of ∼13.8 ± 1.4 days at a relative humidity (RH) of 30 % (Kessler et al., 2010). However, Xu et al. investigated the heterogeneous OH oxidation of pure erythritol aerosols that contained erythritol and ammonium sulfate (AS) at different dry inorganic-to-organic mass ratios (IOR) in an aerosol flow tube reactor at a high relative humidity of 85 %. Their kinetic data would suggest that 2-methyltetrols in atmospheric particles were likely chemically stable against heterogeneous OH oxidation under humid conditions (Xu et al., 2020).

The laboratory studies on atmospheric heterogeneous oxidation reactions, using Knudsen cell (Seisel et al., 2006; Zhou and Wang, 2014), flow tube reactor (Lelièvre et al., 2004; Kessler et al., 2010), FTIR (Zeng et al., 2013; He et al., 2016), smog chamber (Lee et al., 2004; Hartz et al., 2007; Weitkamp et al., 2007; Ge et al., 2016), have developed rapidly in the determination of kinetic constants of trace gases and adsorption reactions on particle surfaces (Lee and Harris, 2006; Goldstein et al., 2008; Nieto et al., 2008; He and Zhang, 2019). In recent years, in-situ FTIR technology has been widely used in heterogeneous oxidation studies of various compounds by monitoring functional group transformation as reactions progressed (Zeng et al., 2013; He et al., 2016; Gao et al., 2019). The evolution of the FTIR absorption peak with time is generally used to estimate the uptake coefficient, which refers to the fraction of gaseous oxidants irreversibly reacted in the surface of compounds after collision (Hudson et al., 2001; Smith et al., 2002; Hung et al., 2005). It is an important physicochemical parameter to characterize the heterogeneous reaction in the atmosphere, and an important quantitative index for the surface uptake ability of atmospheric particles (Moise and Rudich, 2002; Thornberry and Abbatt, 2004; Ziemann, 2005; Hung and Tang, 2010). The heterogeneous reaction rate between gaseous oxides and the condensed compounds can be calculated based on a pseudo-first-order rate equation with the corresponding uptake coefficient (Worsnop et al., 2002). Gao et al. studied the heterogeneous reactions of ozone with oleic acid via a flow system combined with ATR-FTIR, and reported the uptake coefficient γ of ozone on oleic acid was (4.6 ± 1.0) × 10⁻⁴ (Gao et al., 2019). The uptake coefficients of ozone on oleic acid in previous studies ranged from (7.8 ± 2) × 10⁻³ to (1.9 ± 0.6) × 10⁻⁵ (Hartz et al., 2007; Hearn and Smith, 2004; Nash et al., 2006; Smith et al., 2002; Rosen et al., 2008).

In this paper, in order to study the ozone heterogeneous oxidations of Erythritol, Analogue of 2-Methyl Erythritol (AME) and 2, 3-Dihydroxy-4-oxopentanoic Acid (DHOPA) which are secondary organic tracers of the largest natural source of non-methane hydrocarbons (isoprene) and the representative precursor of anthropogenic SOA (toluene) respectively, an in-situ FTIR was used to analyze the chemical structure changes of AME and DHOPA, when exposed to high concentrations of ozone for short periods. The uptake coefficients of ozone on the surface of AME and DHOPA were measured and the pseudo-first-order reaction rate constant of AME and DHOPA were estimated.

Materials and Methods

Materials and Instruments

All chemicals used for this study had purity levels greater than 99%. -AME was supplied by Aladdin, and DHOPA was supplied by TRC. Ozone was generated photolytically using a Xonics ozone generator (Jelight Model 600, Irvine, CA) and the ozone concentration was measured with a photometric ozone detector (2BTechnologies Model 106L). The experiment was carried out at room temperature, in that low constant temperature water baths (DHC-0505-A, qiwei), which controlled the temperature of ambient chamber at 25°C. Analyses of heterogeneous oxidation of the AME and DHOPA were carried out in an in-situ FTIR (Is-50FT-IR, Thermo). The in-situ FTIR was composed of a reaction chamber and a Harrick Praying Mantis. The reaction chamber consisted of an ambient chamber and a dome which equipped with two round KBr observation windows. The external facilities of the Harrick Praying Mantis included observation windows, purge door and purge line fitting, as well as two tilted mirrors and four horizontal mirrors in the Praying Mantis.

Figure 1 showed the experimental setup for measuring the uptake coefficients of ozone on the surface of AME or DHOPA solid powder using in-situ FTIR. The general procedures of the experiments were briefly outlined below: Firstly, a transmittance spectrum with the Praying Mantis in the sample compartment was collected when the wavenumber at 2,500 cm⁻¹ reached the maximum value. Then, dry air was blown for 5 min, and the background was collected. Finally, 1 mg AME/DHOPA solid powders were spread out evenly at the bottom of the sample cup of the ambient chamber, and 20 ppm ozone was injected for 30 min continuously. The characteristic infrared absorption peaks of surface of solid powder during the process of the ozone oxidation of AME or DHOPA were monitored online under the FTIR operational conditions of the infrared resolution of 4 cm⁻¹, the background scanning of 64 times, the series sample scanning of 32 times, the sample interval of 41.27 s, and the scanning range of 4,000–400 cm⁻¹. After each experiment completed, the residual ozone in the ambient chamber was removed by blowing dry air through the outlet.

FIGURE 1

FIGURE 1. in-situ FTIR experimental setup.

Calculation of Uptake Coefficient

The method used to measure the uptake coefficients in this work was similar to that used in previous studies on ozone oxidations of oleic acid and linoleic acid (Jaoui et al., 2004; Hung et al., 2005; Engelke et al., 2010). Zeng et al. studied the heterogeneous reaction of linoleic acid with ozone. It was confirmed that the rate constant of linoleic acid oxidation was in accordance with the pseudo-first-order reaction rate constant. When the sample was exposed to 250 ppb ozone concentration at 30% RH, k_app was 5.98 × 10⁻⁴ s⁻¹ and the uptake coefficient was 5.79 × 10⁻⁴ (Zeng et al., 2013).

In our experiments, the molar ratio of ozone to AME or DHOPA remained at more than three orders of magnitude. Under such pseudo-first order reaction, the second-order reaction of ozone (as A in Eq. 1) and AME or DHOPA (as B in Eq. 1) can be considered as the pseudo-first-order reaction, the rate constant for which can be calculated by Eq. 2 (Gao et al., 2019).

$\mathrm{A+B}\to \mathrm{P}(1)$

$\frac{d\left[B\right]}{dt}={\text{k}}_{\text{app}}\left[B\right]\text{ when }{k}_{app}\left[\text{B}\right]=k\left[A\right]\left[B\right](2)$

$k_{app}$——Pseudo-first-order rate constant (s⁻¹);

k——Second order rate constant (cm³·molecule⁻¹·s⁻¹);

The uptake coefficient γ was calculated using the change rate of the integral area of characteristic absorption peaks at specific wavelengths of AME or DHOPA based on Eq. 3 (Worsnop et al., 2002; Gao et al., 2019).

$\frac{d\left[C_i^a\right]}{dt}=-\text{γ}\left({\mathrm{N}}_A\frac{{\mathrm{P}}_{{\mathrm{O}}_3}\overline{\mathrm{c}}}{4\mathrm{R}\mathrm{T}}\right)\frac{{\mathrm{S}}_{\mathrm{A}}}{\mathrm{V}}(3)$

[$C_i^a$]—— the initial concentration of i (molecules·cm⁻³);

$\frac{d\left[C_i^a\right]}{\text{dt}}$—— the rate of molecular change of i (molecules·cm⁻³·s⁻¹);

$\overline{\text{c}}$—— average rate of ozone in the gas phase (cm·s⁻¹);

N_A—— Avogadro’s number (6.02 × 10²³ molecules·mol⁻¹);

$P_{{\text{O}}_3}$—— atmospheric pressure of ozone (Pa = kg·m⁻¹·s⁻²);

R—— gas constant or proportionality constant (8.314 J mol⁻¹ K⁻¹);

T—— temperature (K);

$\frac{S_A}{V}$—— the specific surface area of i (cm⁻¹).

In this study, the surface area of the reaction chamber (20 cm⁻¹) was assumed as the specific surface area for collision. However, the collision area corresponds to the sample preparation methods and affects the uptake coefficient. In order to distinguish the changes of FTIR absorption peaks during the process of the oxidation reactions, enough amounts of samples was used, resulting in the formation of pores within the solid powder for ozone to permeate. As a result, our experiments measured the upper bounds of the uptake coefficients of AME and DHOPA.

Results and Discussion

Ozone Oxidation of AME

Figure 2 showed the infrared spectrum of AME at a room temperature of 25°C and 30% RH.

FIGURE 2

FIGURE 2. Infrared spectrum of AME at room temperature.

To resolve the broad O–H stretching band of carboxyl groups that was superimposed on the peaks of interest between 3,700 and 2,500 cm⁻¹, the six superimposed peaks were separated by 8.5 origin Gaussian fitting, including the stretching bands of -OH at 3,180 cm⁻¹ and 3,480 cm⁻¹, -CH₂ antisymmetric stretching at 2,910 cm⁻¹, -CH stretching at 2,823 cm⁻¹, -CH₂ symmetric stretching at 2,718 cm⁻¹, and -CH stretching at 2,663 cm⁻¹, as shown in Figure 3 (Injae et al., 1998; Luo et al., 2003; Branca et al., 2016). The detailed assignment of spectral bands for AME was summarized in Table 1.

FIGURE 3

FIGURE 3. Gaussian fitting results of AME in the 3,700–2500cm⁻¹ region.

TABLE 1

TABLE 1. IR frequencies and assignments for functional groups in AME.

The heterogeneous oxidation of ozone on AME was carried out in a reaction chamber of FTIR under the same ambient conditions. The FTIR spectra of the AME were recorded as a function of time. Figure 4A showed that the area of the absorption peak at wavenumber 3480 cm⁻¹ (-OH stretching) decreased with time when exposed to ozone. In addition, a small absorption peak at 1700 cm⁻¹ appeared and the area of this peak increased with time, as shown in Figure 4B. It was likely the infrared absorption caused by the C=O stretching of the reaction product. Changes in AME absorption peaks at 3,480 cm⁻¹ and at 1700 cm⁻¹ during the experiments indicated that–OH at the end chain of AME was oxidized to C=O bond by ozone. Based on the changes in the absorption peak area at 3,480 and 1700 cm⁻¹, the change rates of peak areas were calculated as −0.00134 int. abs/s and 0.00117 int. abs/s, respectively.

FIGURE 4

FIGURE 4. Changes of the AME absorption peak at 3,480 and 1700 cm⁻¹ in the course of reactions. (A) 3,480 cm⁻¹ (B) 1700 cm⁻¹.

Ozone Oxidation of DHOPA

The infrared spectrum of DHOPA at a room temperature of 25°C and 30% relative humidity was presented in Figure 5. To resolve the broad O–H stretching band of alcohol OH and carboxylic acid -OH that were superimposed on the peaks of interest between 4,000 and 3,000 cm⁻¹, as well as the peaks between 1800 and 1,600 cm⁻¹, 8.5 origin Gaussian fitting was used for peak separation. The resolved peaks, included the stretching bands of -OH at 3,540 and 3,340 cm⁻¹, C=O of carboxylic acid (COOH) and of ketone at 1730 and 1,640 cm⁻¹ respectively as shown in Figure 6. A comprehensive interpretation of FTIR spectra was tabulated in Table 2, which summarized the detailed assignment of spectral bands for DHOPA.

FIGURE 5

FIGURE 5. Infrared absorption spectrum of DHOPA at room temperature.

FIGURE 6

FIGURE 6. Gaussian fitting results of DHOPA in the 4,000–3,000 and 1800–1,600 cm⁻¹ region.

TABLE 2

TABLE 2. IR frequencies and assignments for functional groups in DHOPA.

The heterogeneous oxidations of DHOPA and ozone were carried out in a reaction chamber of FTIR. The FTIR spectra of the DHOPA were monitored with time as the reactions processed. The results showed that the area of the absorption peak at wavenumber 1640 cm⁻¹ (C=O stretching) decreased with time when exposed to ozone, as shown in Figure 7A. Furthermore, the appearance of a small absorption peak at 3,340 cm⁻¹ and the increase of this peak area with time were observed, as shown in Figure 7B. It was likely the infrared absorption caused by the O–H stretching of the reaction products. Changes in DHOPA absorption peaks at 1,640 cm⁻¹ and at 3,340 cm⁻¹ during the experiments indicated that C=O of DHOPA was oxidized to CO–OH by ozone. Because COOH is more stable than C=O, the most reasonable product is 2, 3, 4-trihydroxyvaleric acid. Based on the evolution in the absorption peak area at 1,640 and 3,340 cm⁻¹ with time, the change rates of peak areas were calculated as −0.00191 int.abs/s and 0.00218 int.abs/s, respectively.

FIGURE 7

FIGURE 7. Changes of the DHOPA absorption peak at 1,640 and 3,340 cm⁻¹ in the course of reactions. (A) 1,640 cm⁻¹ (B) 3,340 cm⁻¹.

Determination of Uptake Coefficient and Reaction Rate

Figure 8 showed the standard curve of the number of AME molecules vs. the characteristic absorption peak area of AME at 3,480 cm⁻¹. The equation was y = 6.95 × 10¹⁶ x = 2.57 × 10¹⁹ with the correlation coefficient of 0.9805. Figure 9 showed the standard curve of the number of DHOPA molecules vs. the characteristic absorption peak area of DHOPA at 1,640 cm⁻¹. The equation was y = 4.51 × 10¹⁶ x = 5.33 × 10¹⁸, and the correlation coefficient was 0.9783.

FIGURE 8

FIGURE 8. Standard curve of number of AME molecules vs. absorption peak area at 3,480 cm⁻¹.

FIGURE 9

FIGURE 9. Standard curve of number of DHOPA molecules vs. absorption peak area at 1,640 cm⁻¹.

Based on the change rate of the absorption peak area (−0.00134 int.abs/s at 3,480 cm⁻¹) obtained in Ozone Oxidation of AME, the calculated change rate of number of AME molecules was −9.313 × 10¹³ molecules·s⁻¹ according to the standard curve shown in Figure 8. In the same way, with the change rate of DHOPA peak area at 1,640 cm⁻¹ (−0.00191 int.abs/s), the calculated change rate of number of DHOPA molecules was −8.614 × 10¹³ molecules·s⁻¹. Under the pseudo-first order reaction of this study, the uptake coefficients γ and the pseudo-first-order reaction rate constants k_app could be calculated using the change rates of the absorption peak areas at 3,480 cm⁻¹ of AME and 1,640 cm⁻¹ of DHOPA based on Eqs 2, 3, using the surface area of the reaction chamber of 20 cm⁻¹ as the specific surface area for collision, the concentration of ozone of 20 ppm and the average rate of ozone of 115 ml/min. The pseudo-first-order reaction rate constant k_app were 1.89 × 10⁻⁸ s⁻¹ and 2.12 × 10⁻⁷ s⁻¹, and the uptake coefficients of ozone on the surface of AME and DHOPA were (1.3 ± 0.8) × 10⁻⁸ and (4.5 ± 2.7) × 10⁻⁸, respectively.

This experiment is the first time to study the uptake coefficient of AME and DHOPA, so we find the data of ozone heterogeneous oxidation of some other organic substances for comparison. Table 3 summarized the uptake coefficients of ozone on the surface of organic compounds reported in the literature and obtained in this study. It clearly showed that the uptake coefficients of ozone on AME and DHOPA were quite different from other organic compounds, which were 2-5 orders of magnitude lower than those of oleic acid, linoleic acid, and cholesterol, as well as no significant correlation with ozone concentration.

TABLE 3

TABLE 3. Uptake coefficients of ozone on surface of organic matters.

Conclusion

In this study, in-situ FTIR was utilized to study the heterogeneous oxidations of two secondary organic tracers (AME and DHOPA) by ozone. Under the condition of 20 ppm ozone exposure for 30 min, the heterogeneous oxidations of AME and DHOPA by ozone were carried out in a reaction chamber of FTIR at a room temperature of 25°C and 30% relative humidity. The results showed that the AME absorption peak area at 3,480 cm⁻¹ (-OH stretching) decreased while a small absorption peak area increased at 1700 cm⁻¹ during ozone passing over the AME solid powder. Such changes indicated that–OH, at the end chain of AME, was oxidized to C=O bond by ozone. For DHOPA, the absorption peak area at 1,640 cm⁻¹ (Carbonyl C=O stretching) decreased while a small absorption peak area increased at 3,340 cm⁻¹ during the ozone oxidation. It was likely the infrared absorption caused by the O–H stretching of the reaction products. Based on the changes in the absorption peak area at 3,480 and 1700 cm⁻¹ of AME, as well as the changes at 1,640 and 3,340 cm⁻¹ of DHOPA, the change rates of peak areas were calculated as -0.00134 and 0.00117 int.abs/s for AME, as well as −0.00191 and 0.00218 int.abs/s for DHOPA, respectively. The pseudo-first-order reaction rate constant k_app were 1.89 × 10⁻⁸ s⁻¹ and 2.12 × 10⁻⁷ s⁻¹, and the uptake coefficients of ozone on the surface of AME and DHOPA were (1.3 ± 0.8) × 10⁻⁸ and (4.5 ± 2.7) × 10⁻⁸, respectively.

The oxidation rates of AME and DHOPA were found to be relatively slow compared with those of the primary organic tracers reported in previous literature, even exposed to relative high ozone concentrations. It indicates that AME and DHOPA could be reactive, but the oxidation processes would be so slow that the changes of AME and DHOPA due to ozone oxidation are negligible. Therefore, under the atmospheric conditions with ozone as the main oxidant, AME and DHOPA, the secondary organic tracers of isoprene and toluene respectively, can be considered the source contribution estimated on the basis of the tracer methods are reliable. In this paper, the heterogeneous oxidation of secondary organic tracers in ozone environment was discussed. The heterogeneous oxidation of organic tracers by different oxidants needs to be studied more comprehensively in the future.

Data Availability Statement

The original contributions presented in the study are included in the article/Supplementary Material, further inquiries can be directed to the corresponding author.

Author Contributions

RW Participate in experiments and write this paper YH Participate in experiments QH Participate in experiments GC Support and guide experiments RZ Guide experiments.

Funding

This study was financially supported by the National Natural Science Foundation of China (21876036) and the Fund for the Research and Development of Science and Technology in Shenzhen (JCYJ20150625142543472, ZDSYS201603301417588).

Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Publisher’s Note

All claims expressed in this article are solely those of the authors and do not necessarily represent those of their affiliated organizations, or those of the publisher, the editors and the reviewers. Any product that may be evaluated in this article, or claim that may be made by its manufacturer, is not guaranteed or endorsed by the publisher.

References

And, J., and Smith, G. D. (2004). Kinetics and Product Studies for Ozonolysis Reactions of Organic Particles Using Aerosol CIMS [J]. The J. Phys. Chem. A 108 (445), 10019–10029.

Google Scholar

Branca, C., D'Angelo, G., Crupi, C., Khouzami, K., Rifici, S., Ruello, G., et al. (2016). Role of the OH and NH Vibrational Groups in Polysaccharide-Nanocomposite Interactions: A FTIR-ATR Study on Chitosan and Chitosan/clay Films. Polymer 99, 614–622. doi:10.1016/j.polymer.2016.07.086

CrossRef Full Text | Google Scholar

Ding, X., Wang, X. M., and Gao, B. (2012). Tracer-Based Estimation of Secondary Organic Carbon in the Pearl River Delta, South China [J]. J. Geophys. Res. Atmospheres 117 (D5), 313. doi:10.1029/2011jd016596

CrossRef Full Text | Google Scholar

Dreyfus, M. A., Tolocka, M. P., Dodds, S. M., Dykins, J., and Johnston, M. V. (2005). Cholesterol Ozonolysis: Kinetics, Mechanism, and Oligomer Products. J. Phys. Chem. A. 109 (28), 6242–6248. doi:10.1021/jp050606f

CrossRef Full Text | Google Scholar

Engelke, U. F. H., Zijlstra, F. S. M., Mochel, F., Valayannopoulos, V., Rabier, D., Kluijtmans, L. A. J., et al. (2010). Mitochondrial Involvement and Erythronic Acid as a Novel Biomarker in Transaldolase Deficiency. Biochim. Biophys. Acta (Bba) - Mol. Basis Dis. 1802 (11), 1028–1035. doi:10.1016/j.bbadis.2010.06.007

CrossRef Full Text | Google Scholar

Gao, X., Leng, C., Zeng, G., Fu, D., Zhang, Y., and Liu, Y. (2019). Ozone Initiated Heterogeneous Oxidation of Unsaturated Carboxylic Acids by ATR-FTIR Spectroscopy. Spectrochimica Acta A: Mol. Biomol. Spectrosc. 214, 177–183. doi:10.1016/j.saa.2019.02.025

PubMed Abstract | CrossRef Full Text | Google Scholar

Ge, S., Xu, Y., and Jia, L. (2016). Secondary Organic Aerosol Formation from Ethyne in the Presence of NaCl in a Smog Chamber. Environ. Chem. 13 (4), 699–710. doi:10.1071/en15155

CrossRef Full Text | Google Scholar

Goldstein, D. N., Mccormick, J. A., and George, S. M. (2008). Al2O3 Atomic Layer Deposition with Trimethylaluminum and Ozone Studied by In Situ Transmission FTIR Spectroscopy and Quadrupole Mass Spectrometry. J. Phys. Chem. C 112 (49), 19530–19539. doi:10.1021/jp804296a

CrossRef Full Text | Google Scholar

Hartz, K., Weitkamp, E. A., Sage, A. M., Donahue, N. M., and Robinson, A. L. (2007). Laboratory Measurements of the Oxidation Kinetics of Organic Aerosol Mixtures Using a Relative Rate Constants Approach[J]. J. Geophys. Res. 112 (D4), 204. doi:10.1029/2006jd007526

CrossRef Full Text | Google Scholar

He, X., Leng, C. B., and Zhang, Y. H. (2016). A Comparison of Heterogeneous Reaction Kinetics of Oleic Acid Thin Film and Oleic Acid Coated Flyash with Ozone Using Vacuum FTIR. Guang Pu Xue Yu Guang Pu Fen Xi 36 (5), 1576–1580.

PubMed Abstract | Google Scholar

He, X., and Zhang, Y.-H. (2019). Influence of Relative Humidity on SO2 Oxidation by O3 and NO2 on the Surface of TiO2 Particles: Potential for Formation of Secondary Sulfate Aerosol. Spectrochimica Acta Part A: Mol. Biomol. Spectrosc. 219, 121–128. doi:10.1016/j.saa.2019.04.046

PubMed Abstract | CrossRef Full Text | Google Scholar

Hearn, J. D., and Smith, G. D. (2004). Kinetics and Product Studies for Ozonolysis Reactions of Organic Particles Using Aerosol CIMS. J. Phys.Chem. A. 108, 10,019–10,029. doi:10.1021/jp0404145

CrossRef Full Text | Google Scholar

Hennigan, C. J., Sullivan, A. P., Collett, J., and Robinson, A. L. (2010). Levoglucosan Stability in Biomass Burning Particles Exposed to Hydroxyl Radicals [J]. Geophys. Res. Lett. 37 (L09), 806. doi:10.1029/2010gl043088

CrossRef Full Text | Google Scholar

Hoffmann, D., Tilgner, A., Iinuma, Y., and Herrmann, H. (2010). Atmospheric Stability of Levoglucosan: A Detailed Laboratory and Modeling Study. Environ. Sci. Technol. 44, 694–699. doi:10.1021/es902476f

PubMed Abstract | CrossRef Full Text | Google Scholar

Hudson, P. K., Foster, K. L., Tolbert, M. A., George, S. M., Carlo, S. R., and Grassian, V. H. (2001). HBr Uptake on Ice: Uptake Coefficient, H2O/HBr Hydrate Formation, and H2O Desorption Kinetics. J. Phys. Chem. A. 105 (4), 694–702. doi:10.1021/jp002700w

CrossRef Full Text | Google Scholar

Hung, H.-M., Katrib, Y., and Martin, S. T. (2005). Products and Mechanisms of the Reaction of Oleic Acid with Ozone and Nitrate Radical. J. Phys. Chem. A. 109 (20), 4517–4530. doi:10.1021/jp0500900

CrossRef Full Text | Google Scholar

Hung, H.-M., and Tang, C.-W. (2010). Effects of Temperature and Physical State on Heterogeneous Oxidation of Oleic Acid Droplets with Ozone. J. Phys. Chem. A. 114 (50), 13104–13112. doi:10.1021/jp105042w

CrossRef Full Text | Google Scholar

Injae, K., Hong, J., Chung, Y., Jeongchil, S., Dongyoung, K., Dongyoon, S., et al. (1998). Statistical Analysis on Deviation of Radial Composition by Measuring FTIR for Hg1-xCdxTe [J]. Ungyong Mulli 11 (1), S38–S42.

Google Scholar

Jaoui, M., Kleindienst, T. E., Lewandowski, M., and Edney, E. O. (2004). Identification and Quantification of Aerosol Polar Oxygenated Compounds Bearing Carboxylic or Hydroxyl Groups. 1. Method Development. Anal. Chem. 76 (16), 4765–4778. doi:10.1021/ac049919h

PubMed Abstract | CrossRef Full Text | Google Scholar

Katrib, Y., Biskos, G., Buseck, P. R., Davidovits, P., Jayne, J. T., Mochida, M., et al. (2005). Ozonolysis of Mixed Oleic-Acid/Stearic-Acid Particles: Reaction Kinetics and Chemical Morphology. J. Phys. Chem. A. 109 (48), 10910–10919. doi:10.1021/jp054714d

CrossRef Full Text | Google Scholar

Kessler, S. H., Smith, J. D., Che, D. L., Worsnop, D. R., Wilson, K. R., and Kroll, J. H. (2010). Chemical Sinks of Organic Aerosol: Kinetics and Products of the Heterogeneous Oxidation of Erythritol and Levoglucosan. Environ. Sci. Technol. 44 (18), 7005–7010. doi:10.1021/es101465m

PubMed Abstract | CrossRef Full Text | Google Scholar

Kleindienst, T. E., Jaoui, M., Lewandowski, M., Offenberg, J. H., Lewis, C. W., Bhave, P. V., et al. (2007). Estimates of the Contributions of Biogenic and Anthropogenic Hydrocarbons to Secondary Organic Aerosol at a southeastern US Location. Atmos. Environ. 41 (37), 8288–8300. doi:10.1016/j.atmosenv.2007.06.045

CrossRef Full Text | Google Scholar

Lai, C., Liu, Y., Ma, J., Ma, Q., and He, H. (2014). Degradation Kinetics of Levoglucosan Initiated by Hydroxyl Radical under Different Environmental Conditions. Atmos. Environ. 91 (054), 32–39. doi:10.1016/j.atmosenv.2014.03.054

CrossRef Full Text | Google Scholar

Lambe, A. T., Miracolo, M. A., Hennigan, C. J., Robinson, A. L., and Donahue, N. M. (2009). Effective Rate Constants and Uptake Coefficients for the Reactions of Organic Molecular Markers (N-Alkanes, Hopanes, and Steranes) in Motor Oil and Diesel Primary Organic Aerosols with Hydroxyl Radicals. Environ. Sci. Technol. 43 (23), 8794–8800. doi:10.1021/es901745h

PubMed Abstract | CrossRef Full Text | Google Scholar

Lambe, A. T., Onasch, T. B., Croasdale, D. R., Wright, J. P., Martin, A. T., Franklin, J. P., et al. (2012). Transitions from Functionalization to Fragmentation Reactions of Laboratory Secondary Organic Aerosol (SOA) Generated from the OH Oxidation of Alkane Precursors. Environ. Sci. Technol. 46 (10), 5430–5437. doi:10.1021/es300274t

PubMed Abstract | CrossRef Full Text | Google Scholar

Lee, S.-Y., and Harris, M. T. (2006). Surface Modification of Magnetic Nanoparticles Capped by Oleic Acids: Characterization and Colloidal Stability in Polar Solvents. J. Colloid Interf. Sci. 293 (2), 401–408. doi:10.1016/j.jcis.2005.06.062

CrossRef Full Text | Google Scholar

Lee, S., Jang, M., and Kamens, R. M. (2004). SOA Formation from the Photooxidation of α-pinene in the Presence of Freshly Emitted Diesel Soot Exhaust. Atmos. Environ. 38 (16), 2597–2605. doi:10.1016/j.atmosenv.2003.12.041

CrossRef Full Text | Google Scholar

Lelièvre, S., Bedjanian, Y., Pouvesle, N., Delfau, J.-L., Vovelle, C., and Le Bras, G. (2004). Heterogeneous Reaction of Ozone with Hydrocarbon Flame Soot. Phys. Chem. Chem. Phys. 6 (6), 1181–1191. doi:10.1039/b316895f

CrossRef Full Text | Google Scholar

Luo, Z., Lin, X. Y., Lin, S. H., Yu, C. H., Lin, K. X., Yu, Y. P., et al. (2003). Infrared Analysis on Hydrogen Content and Si-H Bonding Configurations of Hydrogenated Amorphous Silicon Films. Acta Physica Sinica 52 (1), 169–174. doi:10.7498/aps.52.169

CrossRef Full Text | Google Scholar

Moise, T., and Rudich, Y. (2002). Reactive Uptake of Ozone by Aerosol-Associated Unsaturated Fatty Acids: Kinetics, Mechanism, and Products. J. Phys. Chem. A. 106 (27), 6469–6476. doi:10.1021/jp025597e

CrossRef Full Text | Google Scholar

Nash, D. G., Tolocka, M. P., and Baer, T. (2006). The Uptake of O3by Myristic Acid-Oleic Acid Mixed Particles: Evidence for Solid Surface Layers. Phys. Chem. Chem. Phys. 8 (38), 4468–4475. doi:10.1039/b609855j

PubMed Abstract | CrossRef Full Text | Google Scholar

Nieto-Gligorovski, L., Net, S., Gligorovski, S., Zetzsch, C., Jammoul, A., D’Anna, B., et al. (2008). Interactions of Ozone with Organic Surface Films in the Presence of Simulated Sunlight: Impact on Wettability of Aerosols. Phys. Chem. Chem. Phys. 10 (20), 2964–2971. doi:10.1039/b717993f

PubMed Abstract | CrossRef Full Text | Google Scholar

Rosen, E. P., Garland, E. R., and Baer, T. (2008). Ozonolysis of Oleic Acid Adsorbed to Polar and Nonpolar Aerosol Particles. J. Phys. Chem. A. 112 (41), 10315–10324. doi:10.1021/jp8045802

CrossRef Full Text | Google Scholar

Seisel, S., Keil, T., Lian, Y., and Zellner, R. (2006). Kinetics of the Uptake of SO2 on mineral Oxides: Improved Initial Uptake Coefficients at 298 K from Pulsed Knudsen Cell Experiments. Int. J. Chem. Kinet. 38 (4), 242–249. doi:10.1002/kin.20148

CrossRef Full Text | Google Scholar

Smith, G. D., Woods, E., Deforest, C. L., Baer, T., and Miller, R. E. (2002). Reactive Uptake of Ozone by Oleic Acid Aerosol Particles: Application of Single-Particle Mass Spectrometry to Heterogeneous Reaction Kinetics. J. Phys. Chem. A. 106 (35), 8085–8095. doi:10.1021/jp020527t

CrossRef Full Text | Google Scholar

Thornberry, T., and Abbatt, J. P. D. (2004). Heterogeneous Reaction of Ozone with Liquid Unsaturated Fatty Acids: Detailed Kinetics and Gas-phase Product Studies. Phys. Chem. Chem. Phys. 6 (1), 84–93. doi:10.1039/b310149e

CrossRef Full Text | Google Scholar

Wang, R. H., Huang, Y. J., and Cao, G. (2020). Heterogeneous Oxidation of Isoprene SOA and Toluene SOA Tracers by Ozone. Chemosphere 249, 126258.

PubMed Abstract | CrossRef Full Text | Google Scholar

Weitkamp, E. A., Hartz, K. E. H., Sage, A. M., Donahue, N. M., and Robinson, A. L. (2008a). Laboratory Measurements of the Heterogeneous Oxidation of Condensed-phase Organic Molecular Makers for Meat Cooking Emissions. Environ. Sci. Technol. 42 (14), 5177–5182. doi:10.1021/es800181b

PubMed Abstract | CrossRef Full Text | Google Scholar

Weitkamp, E. A., Lambe, A. T., Donahue, N. M., and Robinson, A. L. (2008b). Laboratory Measurements of the Heterogeneous Oxidation of Condensed-phase Organic Molecular Makers for Motor Vehicle Exhaust. Environ. Sci. Technol. 42 (21), 7950–7956. doi:10.1021/es800745x

PubMed Abstract | CrossRef Full Text | Google Scholar

Weitkamp, E. A., Sage, A. M., Pierce, J. R., Donahue, N. M., and Robinson, A. L. (2007). Organic Aerosol Formation from Photochemical Oxidation of Diesel Exhaust in a Smog Chamber. Environ. Sci. Technol. 41 (20), 6969–6975. doi:10.1021/es070193r

PubMed Abstract | CrossRef Full Text | Google Scholar

Worsnop, D. R., Morris, J. W., Shi, Q., Davidovits, P., and Kolb, C. A. (2002). A Chemical Kinetic Model for Reactive Transformations of Aerosol Particles [J]. Geophys. Res. Lett. 29 (20), 571–574. doi:10.1029/2002gl015542

CrossRef Full Text | Google Scholar

Xu, R., Lam, H. K., Wilson, K. R., Davies, J. F., Song, M., Li, W., et al. (2020). Effect of Inorganic-To-Organic Mass Ratio on the Heterogeneous OH Reaction Rates of Erythritol: Implications for Atmospheric Chemical Stability of 2-methyltetrols. Atmos. Chem. Phys. 20 (6), 3879–3893. doi:10.5194/acp-20-3879-2020

CrossRef Full Text | Google Scholar

Zeng, G., Holladay, S., Langlois, D., Zhang, Y., and Liu, Y. (2013). Kinetics of Heterogeneous Reaction of Ozone with Linoleic Acid and its Dependence on Temperature, Physical State, RH, and Ozone Concentration. J. Phys. Chem. A. 117 (9), 1963–1974. doi:10.1021/jp308304n

CrossRef Full Text | Google Scholar

Zhou, L., Wang, W., Gai, Y., and Ge, M. (2014). Knudsen Cell and Smog Chamber Study of the Heterogeneous Uptake of Sulfur Dioxide on Chinese mineral Dust. JOURNAL ENVIRONMENTAL SCIENCES 26 (12), 2423–2433. doi:10.1016/j.jes.2014.04.005

PubMed Abstract | CrossRef Full Text | Google Scholar

Ziemann, P. J. (2005). Aerosol Products, Mechanisms, and Kinetics of Heterogeneous Reactions of Ozone with Oleic Acid in Pure and Mixed Particles. Faraday Discuss. 130, 469–490. doi:10.1039/b417502f

PubMed Abstract | CrossRef Full Text | Google Scholar