Phsicochemical Treatment of Hazardous Wastes - Chapter 8 pps

8 Ultraviolet/Ozone 8.1 Introduction Three dominant reactions during ultraviolet (UV)/ozone (O 3 ) treatment processes that effectively decompose organic pollutants are photolysis, ozonation, and reactions of hydroxyl radicals. The generation of hydroxyl radicals is essential in this oxidation process as it is the reaction between these radicals and organic compounds that can ultimately destroy organic pollutants. Physical parameters, such as temperature, pH, initial compound and ozone concentrations, UV intensity, and ozone partial pressure will also have considerable effects on the kinetic rate constants and removal efficiency of any compound. The UV/ozone process is commonly used to degrade toxic organic compounds often found in surface and groundwater. Many of these compounds originate from the chemical, petrochemical, pesticide, and herbicide indus- tries. The molecular structure of organic pollutants to be oxidized has a significant impact on kinetic rate constants and the removal efficiency of the compound. Parent compounds can be partially oxidized to form by-products during oxidation treatment. These intermediates can further react with hydroxyl radicals, creating a “scavenging” effect that often reduces the degradation rates of parent compounds. 8.2 Decomposition Kinetics of UV/Ozone in Aqueous Solution Ozonation processes are rather complex, due to the high instability of ozone in aqueous solutions. Ozone absorbs UV photons with the maximal absorption at 253.7 nm. The decomposition of ozone under UV radiation typically occurs through three reactions: direct photolysis, direct ozonation, and reactions between hydroxyl radicals and hydrogen peroxide as shown in the following reactions: TX69272_C08.fm Page 283 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 284 Physicochemical Treatment of Hazardous Wastes Photolysis (slow): (8.1) (8.2) Ozonation: HO 2 – + O 3 Æ HO 2 • + O 3 – (8.3) Hydroxyl radical reactions: H 2 O 2 + OH • Æ HO 2 • + H 2 O (8.4) HO 2 – + OH • Æ HO 2 • + OH – (8.5) In a gaseous phase enriched with water vapor, the mechanism of photolysis involves the release of a molecule of oxygen and an atom of oxygen ( 1 D). The latter may react with water to produce hydroxyl radicals: O 3 + h n Æ O 2 + O ( 1 D) (8.6) O ( 1 D) + H 2 O Æ HO ª + HO • (8.7) where the kinetic rate constants for Equation (8.6) and Equation (8.7) are 2.7 ¥ 10 7 and 7.5 ¥ 10 9 M –1 s –1 , respectively (Beltran et al., 1994); however, if two hydroxyl radicals are prevented from escaping the solvent cage, they may recombine in solution to form hydrogen peroxide. The overall photolysis of ozone in solution is therefore likely to be represented by the following reaction: (8.8) Prousek (1996) showed that hydrogen peroxide is in fact the primary product of ozone photolysis and also summarized the chemistry involved in the generation of HO ∑ radicals by the UV/ozone process as follows: (8.9) O 3 – + H + Æ HO 3 Æ HO + O 2 (8.10) OHOHOO 32 222 +Æ + hn H O 2OH 22 • Æ hn O H O [2HO ] O H O O 32 • 22 +Æ +Æ + h cage n 22 HO HO – O HOO O – 22 2 3 • 3 ´Æ + TX69272_C08.fm Page 284 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC Ultraviolet/Ozone 285 O 3 – + H 2 O Æ HO • + HO – + O 2 (8.11) HO • + RH Æ R – Æ ROO • (8.12) Reactions of ozone can be initiated by HO • or HOO • or by photolysis of hydrogen peroxide. Ozone can also be decomposed through the following reaction pathways: O 3 – Æ O 2 + O – (8.13) O – + H 2 O Æ HO • + HO – (8.14) Decomposition rates of ozone can be influenced by pH, UV irradiation, and the presence of free-radical scavengers generated from anion species (Ku et al., 1996a). For example, anions such as chloride, carbonate, and nitrate in aqueous solutions tend to scavenge hydroxyl radicals produced during UV/ozone oxidation processes, subsequently reducing the decomposition rates of ozone. An increase in alkalinity will rapidly increase the decomposition rate of ozone, due to hydroxyl radicals being consistently formed by the reaction between ozone and hydroxide ions. UV irradiation also assists in increasing the decomposition rate of ozone. The rates of reaction expressed by second-order kinetics achieved by hydroxyl radicals are typically 10 6 to 10 9 times faster than the corresponding rates by molecular ozone, as shown in Table 8.1. The rate constants are useful in estimating HO • -induced oxidation rates of organic compounds in a variety of aqueous systems, including atmospheric water droplets, sunlit surface waters, and room-temperature radical oxidation processes. TABLE 8.1 Reaction Rates of Ozone and Hydroxyl Radicals with Classes of Organic Compounds Compound k ( M –1 s –1 ) O 3 HO • Olefins S-containing organics Phenols N-containing organics Aromatics Acetylenes Aldehydes Ketones Alcohols Alkanes Carboxylic acids 1–450 ¥ 10 3 10–1.6 ¥ 10 3 10 3 10–10 2 1–10 2 50 10 1 10 –2 –1 10 –2 10 –3 –10 –2 10 9 –10 11 10 9 –10 10 10 9 10 8 –10 10 10 8 –10 10 10 8 –10 9 10 9 10 9 –10 10 10 8 –10 9 10 6 –10 9 10 7 –10 9 TX69272_C08.fm Page 285 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 286 Physicochemical Treatment of Hazardous Wastes According to Hayashi et al. (1993), refractory compounds, such as saturated alcohols and carboxylic acids are built up in the system after a certain amount of ozonation. Kusakabe (1990, 1991) applied UV irradiation to the preozonation of humic acid and found that the UV/ozone process accelerated the decomposition of volatile organic compound (VOC) and nonvolatile organic carbon (NVOC) precursors. Vollmuth and Niessner (1997) argued that, if organic compounds in dilute aqueous solutions are oxidized only by a direct reaction with ozone, the accelerated decomposition of ozone should retard the oxidation rate. This is not the case at a pH greater than 7, when decomposition of ozone actually accelerates the degradation of organic pollutants. Benitez et al. (1997), Glaze et al. (1982), and Peyton and Glaze (1988) have argued that a synergistic effect must exist between ozone and UV photons that cannot be accounted for as shown in Figure 8.1. Yue (1993) suggested a mechanism of destruction of an organic pollutant that begins with photolysis of ozone in the solution, which produces hydrogen peroxide. The deprotonated peroxide reacts with ozone to produce ozonide and hydroxyl radicals that attack the organic substrate to form an organic carbon-centered radical, which reacts quickly with oxygen to form a peroxyl radical, which decomposes to produce superoxide or hydrogen peroxide. The cyclic reaction pathway is completed with the superoxide reacting with ozone to produce ozonide. Chemical reactions in UV/ozone process are a series of slow and fast reactions. The reaction time is determined by the time taken to complete the sequence of reactions. In the presence of OH ∑ radical scavengers, the oxida- tive efficiency of OH ∑ radicals will be reduced. For example, bicarbonate and carbonate ions usually play a dominant role as OH ∑ radical scavengers, because they present at concentrations of several millimoles per liter and react with OH ∑ radicals with rate constants as high as 1.1 ¥ 10 7 L/mol/cm and 3.9 ¥ 10 8 L/mol/cm for bicarbonate and carbonate, respectively. FIGURE 8.1 Comparison of the oxidation power of the different oxidants used on syringic acid degradation. T = 20°C, pH = 7, pressure = 0.43 kPa. (From Benitez F.J. et al., Indust. Eng. Chem. Res. , 33, 1264–1270, 1997. With permission.) 0 20 40 60 80 100 0204060 t, min C, concentration ppm UV Ozone Ozone + UV TX69272_C08.fm Page 286 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC Ultraviolet/Ozone 287 Mokrini et al. (1997) proposed that the photolytic ozonation kinetics of substrates is a linear combination of purging, ozonation, photolysis, and photolytic ozonation: d[ S ]/d t = k purge [ S ] + k photo I a [ S ] b + k ozon [O 3 ] l c [ S ] d + k po I e D f [ S ] g (8.15) where I is the flux of radiation input into a reactor; D is the dose rate of ozone; [O 3 ] l is the concentration of ozone in the liquid phase; and [ S ] is the substrate concentration (Figure 8.2). Four major factors influence the oxidation rate of organic pollutants: (1) pH, (2) relative concentration of oxidants (O 3 /H 2 O 2 ), (3) photon flux in the UV/O 3 system, and (4) radical scavenger concentration. 8.2.1 pH Effect Beltran et al. (1998) reported that the oxidation kinetics of nitroaromatic hydrocarbons at different pH levels (between 2 and 12) was similar to those found in O 3 /H 2 O 2 oxidation — for example, the positive effect of pH on removal rate between pH 2 and 7 and partial inhibition at pH 12. The ozone efficiency increased with pH, from 30 to 40% (pH = 4) to 95% (pH 9 or 11). At pH 4, about a 10% difference was observed between the ozone efficiencies obtained during UV/ozone radiation oxidation and ozonation alone, while no difference was observed at pH 9 or 11. Figure 8.3 shows this effect for the degradation of vanillic acid, as reported by Benitez et al. (1997). FIGURE 8.2 Ozone decomposition process by photolysis at 253.7 nm. (From Peyton, R. and Glaze, W., Environ. Sci. Technol. , 22, 761–767, 1988. With permission.) H 2 O 2 hν hν HO 2 O 3 O 3 - HO 3 H + OH O 2 MH O 2 MH O 2 - HO 2 MH + O 2 HMH TX69272_C08.fm Page 287 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 288 Physicochemical Treatment of Hazardous Wastes 8.2.2 Concentration of Oxidants In UV/ozone processes, the increase of ozone feed rate leads to an increase of oxidation rate at a given time. This increase of ozone feed rate leads to an increase of the ozone partial pressure and hence to an increase of ozone driving force and thus the ozone absorption rate. When ozone is combined with UV radiation, dinitrotoluene (DNT) is removed at a faster rate than by ozonation alone; therefore, a synergism exists between ozone and UV radiation (Beltran et al., 1998). Shen and Young (1997) reported that the addition of ozone slightly improved (4 to 6%) on the removal rate of trichloroethylene (TCE) until the dosage reached 480 ppmv, at which point further addition of ozone decreased the removal of TCE. Bhowmick and Semmens (1994) concluded that the absorption of UV photons by ozone increased significantly with ozone concentration and thus inhibited photolysis. The chlorinated intermediates generated from the decomposition of TCE by the UV/ ozone process were found to be much fewer than for direct photolysis, indicating that hydroxyl radicals could significantly promote the decomposition of chlorinated intermediates. The optimum ozone dosage was found to be 480 ppmv; however, excessive ozone would reduce the treatment efficiency of TCE by the UV/ozone process. 8.2.3 Effect of Photon Flux in the UV/Ozone System The effect of UV light intensity on the decomposition of organics by the UV/ ozone process was studied by Ku and Shen (1999). The removal efficiency of three chloroethenes increased with increasing light intensity and could be as high as 95%. The treatment efficiency of chloroethenes by the UV/ozone process was found to be much higher than for direct photolysis under var- ious UV light intensities. FIGURE 8.3 UV/ozone: influence of pH on the degradation of vanillic acid. T = 20°C, pressure = 0.43 kP a . (From Benitez, F.J. et al., Indust. Eng. Chem. Res. , 33, 1264–1270, 1997. With permission.) 0 10 20 30 40 50 60 70 80 90 100 110 0204060 t, min. C, concentration ppm pH 2 pH 5 pH 7 pH 9 TX69272_C08.fm Page 288 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC Ultraviolet/Ozone 289 8.2.4 Radical Scavengers Inhibitors of free-radical reactions are compounds capable of consuming OH radicals without regenerating the superoxide anion O 2 – . Some of the common inhibitors include bicarbonate and carbonate ions, alkyl groups, tertiary alcohols, and humic substances. Natural waters contain varying concentrations of numerous organic and inorganic natural compounds. These compounds are present in dissolved and suspended forms. In the presence of algae and degraded animal and vegetable residues, physical, chemical, and biological reactions in water and soil will produce natural organic matter. The main organic constituents in natural water are a collection of polymer- ized organic acids called humic acids . The inhibitive reactions of bicarbonate and carbonate ions with hydroxyl radicals are similar to those described in Chapter 7. During the oxidation of atrazine, UV light accelerates the decomposition of dissolved ozone in aqueous solutions (Ku et al., 1996a). Furthermore, in solutions of pH greater than 3, the decomposition rates of ozone are usually constant. UV light causes the consumption rates of ozone ( r c ) to increase, while an increase in solution pH value reduces the degree to which UV irradiation affects ozone consumption rates. UV irradiation will not significantly affect the consumption rate of hydroxide ions ( ). Decomposition rates generally increase linearly as UV light intensity increases, regardless of pH. The main contribution of ozone decomposition in acidic solutions would be UV photolysis, because the decomposition of ozone was found to be at a minimum at a pH of 2 without the influence of UV irradiation (Ku et al., 1996a). The overall decomposition rate equation of ozone in the presence of UV light in a range of solution pH of 2 to 10 is given as follows: –d[O 3 ]/d t = 23.47 [O 3 ] 1.5 [OH – ] 0.395 + 0.1414[O 3 ] 1.5 [OH – ] 0.064 [ I ] 0.9 (8.16) where I is the UV light intensity (W/m 2 ). The UV light required to decompose ozone decreases with increasing solution pH values, indicating that the decomposition of ozone by OH – could be the major reaction in alkaline solutions. Photolysis is the main reaction pathway in acidic solutions in the presence of UV light (Ku et al., 1996a). The presence of anion species did not significantly change the decomposition rates of ozone ( r c ) or hydroxide ions ( ). However, hydroxide ion consumption increased considerably under UV irradiation; ozone decomposition increased only slightly under UV light. Cl – and NO 3 – ions were found to be very weak scavengers of hydroxyl radicals and had only a minimal effect on the decomposition of ozone. With the presence of CO 3 2– , the consumption of hydroxide ions was not detected during the decomposition of ozone without UV irradiation, possibly due to the carbonate-buffer effect; however, carbonate is the most effective scavenger among the three anions studied. r OH – r OH – TX69272_C08.fm Page 289 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 290 Physicochemical Treatment of Hazardous Wastes Changes in pH value and UV irradiation intensity usually have the greatest effect on ozone decomposition rates, while the selected anion species such as chloride, carbonate, and nitrate have virtually no influence on the decomposition rates. UV irradiation decomposes chemicals through photolysis, where photons in the far UV region are capable of breaking down hydrogen peroxide to form hydroxyl radicals, which oxidize organic pollutants (Esplu- gas et al., 1994). Ozone itself can be decomposed to oxygen radicals by its reaction with hydroperoxide ions (HO 2 – ). However, the effect of the combination of the two treatments is often synergistic, with a subsequent increase in the rate of hydroxyl radical formation. The radicals produced from these reactions are responsible for the complete degradation of organic pollutants. The rate at which ozone decomposes during photolysis can be given by the following equation: –r = d[O 3 ]/dt = k I ([O 3 ] m ¥ [COMP] n ) (8.17) where –r is the decomposition rate of ozone; k is the kinetic rate constant; I is UV irradiation intensity; [O 3 ] and [COMP] are initial ozone and compound concentrations, respectively; and m and n are the rate orders, which can be found according to mathematical models defined by Benitez et al. (1996). In the model, UV intensity is directly proportional to the ozone decomposition rate. Both ozone and compound initial concentrations are also proportional to degradation rate r. The actual amount of any particular compound destroyed during UV/ozone oxidation is known as the removal percentage or efficiency. This efficiency is dependent upon the kinetic rate constant, k. The amount of compound that must be removed during UV/ozone oxidation depends upon actual standards, advisory concentrations, or toxicity levels for a given organic pollutant. The degradation kinetic rate constants are often dependent upon four factors: physical parameters, pH, scavengers, and molecular structure of the organic pollutant to be oxidized. Operating conditions, such as temperature, pH, and ozone partial pressure, are directly proportional to kinetic rates and removal efficiency. For example, low pH tends to lower removal efficiency and reaction rate constants because molecular ozone is the dominant species. At pH greater than 7, hydroxyl radicals are the dominant species; therefore, a high pH is required to achieve high removal efficiency. However, scavenger formation tends to develop more readily in alkaline solutions, which will reduce the removal rates, so optimum removal efficiency and highest kinetic rate constants usually occur when pH is near or slightly higher than neutral, which is consistent with what would be expected theoretically. The formation of scavenger substances can also retard removal efficiency and kinetic reaction rates. Scavengers are ions such as bicarbonate, carbonate, chloride, and humic acid, etc. These scavengers subsequently react with hydroxyl radicals produced during the degradation process. Therefore, the removal efficiency will be reduced significantly. In the presence of scaveng- TX69272_C08.fm Page 290 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC Ultraviolet/Ozone 291 ing substances, 100% removal of organic pollutants from an influent stream is often impossible. It is important to note that the molecular structure of organic compounds has a determined effect on the oxidation rate constants. For example, if a compound is “saturated” with four chlorine atoms per carbon atom such as tetrachloroalkane, its reactivity rate with hydroxyl radicals is expected to be significantly lower than that of an “unsaturated” compound with only two or three chlorine atoms such as di- and trichloroalkanes. 8.3 Degradation Kinetics of Organic Pollutants The kinetic rate of an organic pollutant, k, is a function of the decomposition rate of ozone, UV irradiation intensity, pH, and initial ozone concentration. The removal efficiency usually increases with kinetic rate constants, while physical parameters, such as temperature, pH, UV intensity, and ozone partial pressure have significant influences on these rates. For most organic pollutants, the optimum solution pH is near or slightly higher than neutral pH. UV intensity, temperature, and ozone partial pressure are all usually directly proportional to kinetic rate constants and removal efficiencies; however, removal efficiency has generally been found to be inversely proportional to scavengers generated during degradation processes. Kinetic rate constants can be used to determine whether the UV/ozone process is suitable for treating a particular organic pollutant. For example, if the rate constant for a certain compound were high, then, theoretically, more of the compound would be removed from the influent in less time. This would be a major advantage, because less operating time would reduce operating costs at the treatment plant. Another advantage is that most organic contaminants will respond to UV/ozone treatment, and usually to an appreciable extent. How- ever, a significant disadvantage is that many compounds have special requirements in order for their degradation to occur. High UV intensities and initial ozone concentrations, for example, may be necessary to achieve the desired results, which will increase operating costs. This is because the generation and storage of ozone can be very expensive because ozone is unstable and highly reactive. 8.3.1 Atrazine Ozone combined with ultraviolet radiation (l = 254 nm) has been shown to oxidize atrazine in water. The process can be used to oxidize different organic compounds such as volatile organochlorine substances (e.g., pesticides). Mass transfer and kinetic data have been applied to the mass balance equations of atrazine to obtain corresponding concentrations under varying TX69272_C08.fm Page 291 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 292 Physicochemical Treatment of Hazardous Wastes physical conditions (Beltran et al., 1994). Increasing the pH leads to an increase of the oxidation rate of atrazine. This is due to radical reactions involving ozone and hydrogen peroxide rather than to direct photolysis or ozonation (Beltran et al., 1994). If pH decreases, a higher concentration of dissolved ozone will be required. The increase in ozone concentration reaches a maximum value followed by a gradual decrease in ozone concentration required. This pattern is due to the competition between atrazine and ozone for hydroxyl radicals (Beltran et al., 1994). Hydrogen peroxide is a product typically formed during direct photolysis of ozone (Beltran et al., 1994). During the first 5 min of oxidation, Beltran et al. (1994) found that the concentrations of hydrogen peroxide at pH 2 and 7 remained constant. After 5 min, the H 2 O 2 at pH 7 tended to level off, while the H 2 O 2 concentration at pH 2 continued to increase. This difference was due to the fact that hydrogen peroxide (pK = 11.7) remains in its non- dissociating form at pH 2, which cannot directly react with ozone (Beltran et al., 1994). Beltran et al. (1994) reported that the higher the temperature at any given time, the greater the elimination rate of atrazine will be. The mass balance equation for atrazine is as follows: –dC A/ dt = k C A C O3 – I A + k OH,A C A C OH (8.18) where I A is the degradation rate of atrazine due to direct photolysis, which is given as (Beltran et al., 1994): I A = –j A I 0 f A [1 – exp (–2.3L Âe I C i )] (8.19) where j A is the quantum yield of atrazine; I 0 is the effective intensity of incident radiation in the water; f A is the fraction of radiation absorbed by atrazine; L is the effective path of radiation; and e i and C i are the extinction coefficient and concentration of species present in water, respectively. At pH less than 3, the reaction will occur slowly enough for kinetic models to be true. Thus, a pH 2 or 7 can be utilized for the slow kinetics of atrazine oxidation by UV/ozone processes, while rapid reactions will take place at pH 12. All of the three reaction mechanisms will be affected by other vari- ables such as temperature, pH, and bicarbonate ion concentrations. 8.3.2 Humic Acids Chlorinated organic compounds present in water, due to their carcinogenic nature, have become a great concern with respect to human health. Such substances are formed when humic acids react with chlorine in disinfection processes. Ozonation alone is generally not suited for the complete oxidation of chlorinated compounds because scavenger compounds such as acetic acid, formic acid, and oxalic acid can form and accumulate as by-products in the TX69272_C08.fm Page 292 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC [...]... TX69272_C 08. fm Page 315 Tuesday, November 11, 2003 12:09 PM Ultraviolet/Ozone 315 y = -5 4.018x - 20.26 2 R = 0.9996 Kinetic Rate Constant (sec ^-1 ) 0.350 y = -5 3.699x - 20.122 2 0.300 0.250 R = 0.9992 y = -4 0.434x - 15. 083 2 R = 1 0.200 17 mg/L 0.150 0.100 28 mg/L 38 mg/L Linear (17 mg/L) 0.050 Linear ( 28 mg/L) 0.000 -0 . 381 0 -0 . 380 0 -0 .3790 -0 .3 780 -0 .3770 -0 .3760 Linear ( 38 mg/L) -0 .3750 E HOMO FIGURE 8. 16... 0.9039 y = 0.6198x + 0.2097 Kinetic Rate Constant (sec ^-1 ) R 0.03 2 2 R 0.025 = 0.2 785 y = 1.0 087 x + 0.3441 = 0.972 y = 1. 184 x + 0.4026 R 2 = 0.974 y = 1.1439x + 0. 388 8 0.02 0.015 2 R = 0.9726 37 ppmv 159 ppmv 360 ppmv 0.01 779 ppmv 1174 ppmv 0.005 1 589 ppmv Linear (37 ppmv) Linear (159 ppmv) 0 -0 .3340 -0 .3320 -0 .3300 -0 .3 280 -0 .3260 -0 .3240 -0 .3220 -0 .3200 -0 .3 180 -0 .3160 -0 .3140 -0 .3120 E HOMO Linear... 0.0226 8. 4.6 Slope Ultraviolet Intensity (W/m2) 0.222 0.311 0.413 0.519 0.604 0.697 0. 083 0.116 0.154 0.194 0.226 0.26 68 87 105 117 1 28 141 68 87 105 117 1 28 141 Correlation Coefficient 0.9467 0.9119 0 .89 21 0 .87 84 0 .88 4 0 .88 1 0.9394 0.90 28 0 .88 2 0 .86 8 0 .87 3 0 .87 15 Chlorinated Alkanes and Alkenes Kinetic rate constants, EHOMO, and Hammett’s constants can be correlated with reaction rate constants Table 8. 6... 0.200 Linear (80 watts) 0.150 0.100 0.050 0.000 -0 . 381 -0 . 380 -0 . 380 -0 .379 -0 .379 -0 .3 78 -0 .3 78 -0 .377 -0 .377 -0 .376 -0 .376 -0 .375 0 5 0 5 0 5 0 5 0 5 0 5 E HOMO FIGURE 8. 15 Correlation between kinetic rate constant vs EHOMO for different UV intensities for triazin herbicides Experimental conditions: T = 25°C, pH = 7 .8, ozone concentration = 38 mg/L (Data from Zweiner, C et al., Vorm Wasser, 84 , 47–60,... Chemosphere, 35, 283 7– 284 7, 1997.) © 2004 by CRC Press LLC TX69272_C 08. fm Page 311 Tuesday, November 11, 2003 12:09 PM Ultraviolet/Ozone 311 Kinetic Rate Constant (ppm.min ^-1 ) -0 .5000 120.0 y = 1006.5x + 465.53 R2 = 0.9 981 100.0 80 .0 60.0 40.0 20.0 -0 . 480 0 -0 .4600 -0 .4400 -0 .4200 -0 .4000 -0 . 380 0 -0 .3600 0.0 -0 .3400 E HOMO FIGURE 8. 11 Correlation between kinetic rate constant and EHOMO for a mixture of alkanes... EHOMO – 1 .83 89 –4.2024 UV = 68 W/m2 0.7451 k = –5.9265 EHOMO – 2.5951 –5.9265 UV = 87 W/m2 0 .82 11 k = –7. 387 2 EHOMO – 3.2354 –7. 387 2 UV = 105 W/m2 0 .84 09 k = 8. 794 EHOMO – 3 .85 14 8. 794 UV = 117 W/m2 0 .84 61 –11.32 UV = 1 28 W/m2 0 .87 17 –13.21 2 0 .87 42 k = –11.32 EHOMO – 4.9611 k = –13.21 EHOMO – 5.7911 k = 0.163 ELUMO – 0.02 08 0.163 UV = 141 W/m [O3] = 37 ppmv 0 .87 53 k = 0.23 ELUMO – 0.0 286 0.23 [O3]... Bader, H., Proc of the International Ozone Association Symposium, International Ozone Association, Toronto, 1977, p 16 With permission y = -2 6 .85 x - 10. 086 R 50 Watts Kinetic Rate Constant (sec ^-1 ) 2 = 0.9992 y = -4 5.952x - 17.2 78 60 watts R 0.350 70 watts 2 = 0.9 58 y = -5 2.108x - 19. 587 80 watts R 0.300 Linear (50 Watts) Linear (60 watts) Linear (70 watts) 2 = 0.9302 y = -6 3.003x - 23. 686 0.250 R 2 =... 35, 283 7– 284 7, 1997.) TABLE 8. 5 QSAR Models for Chlorophenols QSAR Model k k k k = = = = -1 4 08 EHOMO –440.39 –764.44 ELUMO +102.62 22.153sres – 0.7456 0.0003 log P + 1 ¥ 10–5 Slope –14 08 –764.44 22.153 0.0003 Correlation Coefficient 0 .80 37 0 .82 56 0 .86 89 0 .86 9 Dataset: 2-Chlorophenol, 4-chlorophenol, 2,4-dichlorophenol, 2,4,5-trichlorophenol, 2,4,6-trichlorophenol © 2004 by CRC Press LLC TX69272_C 08. fm... diffusion-controlled limits © 2004 by CRC Press LLC TX69272_C 08. fm Page 307 Tuesday, November 11, 2003 12:09 PM Ultraviolet/Ozone 307 y = 0.2229x + 0.1042 R 2 = 0.9467 y = 0.3114x + 0.1459 Kinetic Rate Constant sec ^-1 0.025 2 R = 0.9119 y = 0.4133x + 0.19 38 R 2 = 0 .89 21 y = 0.5197x + 0.24 38 0.020 R 2 = 0 .87 84 y = 0.6042x + 0. 283 9 R 2 = 0 .88 38 0.015 y = 0.6974x + 0.3276 R 2 = 0 .88 18 68 Watts/m 2 0.010 87 ... Constant vs E HOMO (Herbicides-Amines) 4.E+09 y = 1E+11x + 6E+10 R2 = 0.9122 4.E+09 3.E+09 3.E+09 2.E+09 2.E+09 1.E+09 5.E+ 08 -0 . 380 0 -0 .3 780 -0 .3760 -0 .3740 -0 .3720 -0 .3700 -0 .3 680 0.E+00 -0 .3660 -0 .3640 E (HOMO) FIGURE 8. 4 Correlation between EHOMO and kinetic rate constant of amine herbicides Experimental conditions: T = 20°C, pH = 7.5 (Data from De Laat, J et al., J Water Sci., 8, 23–42, 1995.) © 2004 . reactions: TX69272_C 08. fm Page 283 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC 284 Physicochemical Treatment of Hazardous Wastes Photolysis (slow): (8. 1) (8. 2) Ozonation: . Press LLC 288 Physicochemical Treatment of Hazardous Wastes 8. 2.2 Concentration of Oxidants In UV/ozone processes, the increase of ozone feed rate leads to an increase of oxidation rate. TX69272_C 08. fm Page 288 Tuesday, November 11, 2003 12:09 PM © 2004 by CRC Press LLC Ultraviolet/Ozone 289 8. 2.4 Radical Scavengers Inhibitors of free-radical reactions are compounds capable of