2002_J.perkowski_Decomposition of Anthraquinone Dye in the Aqueous Solution by Ozone, Hydrogen...

8/10/2019 2002_J.perkowski_Decomposition of Anthraquinone Dye in the Aqueous Solution by Ozone, Hydrogen Peroxide or …

http://slidepdf.com/reader/full/2002jperkowskidecomposition-of-anthraquinone-dye-in-the-aqueous-solution 1/6

72 FIBRES & TEXTILES in Eastern Europe July/September 2002

Decomposition of Anthraquinone Dyein the Aqueous Solution by Ozone,

Hydrogen Peroxide or UV Radiation

Jan Perkowski,Stanisław Ledakowicz*

Technical University of £ódŸ,

Institute of Applied Radiation Chemistry

*Technical University of £ódŸ

Faculty of Process

and Environmental Engineering,

Department of Bioprocess Engineering

ul. Wólczañska 213, 92-005 £ódŸ, Poland

Abstract

The results into investigations of the decomposition of an anthraquinone dye (polan blue E2R) in anaqueous solution induced by ozone, hydrogen peroxide and UV radiation are discussed in the paper.The effect of the ozone dose and concentration, as well as the temperature on decolouration at differentinitial dye concentrations, were investigated. Low ozone concentrations enabled its better utilisationin the reaction with the dye, although the process rate was slow. An increase of gas flow rate and ozoneconcentration at the reactor inlet caused a decrease of ozone consumption from 80% to 49%. Thehydrogen peroxide concentration from 0.05 to 0.1 mol/dm3 allowed us to obtain a 45% decolourationdegree after 48 hours, with the process proceeding most quickly in the first 2 hours. It was found that

the yield of anthraquinone dye photolysis in the aqueous solution was affected by both the power of theUV lamp and the character of the light which it emitted. It appeared most advantageous to use mono-energetic radiation in the UV range below 310 nm.

Key words: decolouration, ozone, hydrogen peroxide, UV radiation, hydroxyl radicals,anthraquinone dye.

■ Introduction

Dyes are a class of compounds thathave been used extensively in various

branches of industry, in particular inthe textile and clothing industries. The

industrial revolution of the 18th centu-ry caused an abrupt increase indemand for various goods and semi-finished products, including dyes, andhence natural dyes were replaced bysynthetic ones. The first synthetic dyewas produced by Natanson aroundthe year 1855. The production of dyesin Poland was started by JanŚniechowski, the founder of the'Boruta' dye factory in Zgierz, which isstill in operation.

In the initial period of production no

attention was paid to environmentalpollution. As the dye industry devel-oped and the volume of production,product range and applicabilityincreased, dye neutralisation and

especially the treatment of wastewatercoming from both chemical plants pro-ducing dyes and textile factories whichused them have gained importance.

A specific feature of wastewater contain-ing dyes is a strong colouration at lowconcentrations which is revealed by

small values of such parameters aschemical oxygen demand (COD), bio-logical oxygen demand (BOD5) and totalorganic carbon (TOC), at high values ofthe colour threshold number (CT).

Textile wastewater is the main sourceof all types of surface water pollutionconnected with drastic colour changes.Beside strong colour, this wastewateris characterised by a high content ofsurfactants, various auxiliary agentsand strong mineralisation (mainlychloride and sodium carbonate).Despite the relatively small content ofdyes in the wastewater, their varietyand stability hampers or even preventstreatment. In the case of the textileindustry, reactive or direct dyes pre-vail; there is also a large percentage ofdispersed dyes (pigments) as well as

basic and acid dyes. The dyes used atpresent are usually non-toxic tohumans, although the infiltration ofcoloured dyes into surface water pre-vents its recreational or economic use.The dyes in the water strongly absorbsunlight, which decreases the intensityof its assimilation by water plants and

phytoplankton and reduces the self-purification capacity of water reser-voirs. Additionally, dyes used in thetextile industry may be toxic to organ-isms living in the surface water, and

can be resistant to natural biologicaldegradation.

The treatment of coloured wastewater,including that from textiles, is a diffi-cult and costly task because of itsquantity and composition. Usually it isnecessary to apply a three-stage treat-

ment technique, which includesmechanical, biological, physico-chemi-cal and chemical processes.

On the basis of theoretical data, themost advantageous method for waste-water decolouration appeared to bechemical oxidation, and next, ifrequired, the elimination of decompo-sition products from water by biologi-cal methods. First, studies on dye oxi-dation were carried out using chlorineand potassium permanganate. In thefirst case, a very negative feature wasthe formation of carcinogenic low-molecular chlorine compounds solublein water; in the other, the obtainedresults were not encouraging as far as

both the final effect and total cost ofthe method were concerned. Recently,there are firstly the processes of oxida-tion based on ozone, hydrogen perox-ide and oxidation combined with UVirradiation, and also all types of combi-nation of these processes. Low selec-tivity, high capacity and the rate of theprocess, as well as the lack of by-prod-ucts, are the main features that encour-age further detailed studies and work

on pilot-plant and semi-commercialscale installations.

A brief review of the application ofozone for textile wastewater treatment



73FIBRES & TEXTILES in Eastern Europe July/September 2002

should make the reader realise howadvanced works in this field are andhow competitive they are in relation tothe classical methods [1,2].

The first wastewater decolourationsystem was installed in Nagahama

Plants (Kanebo, Japan) in 1974. In thatsystem, a combined action of activatedcarbon and ozone (a so-called GAC)was used. Coloured wastewater wassupplied to a 600 m3 tank. The amountof ozone fed to the tank was 7.2 kg/h.The tank in the form of a column wasfilled with granulated activated car-

bon. As a result of the processes thattook place in the column, the waste-water was decoloured and oxidised.The values of COD and BOD5decreased by about 60-80%.

Beside the installation presented above,

in Japan there are at least seven systemsthat use ozone for wastewater treat-ment in the textile industry. Themethod they employ is mainly the GACtechnique. The biggest of these systemswas built in 1978. Its capacity was12,000 m3 of textile wastewater per day.

Textile wastewater ozonation was usedalso on an industrial scale in Leek, GreatBritain. The installation reached fullcapacity in June 1992. Beside coagulationand biological treatment it was necessaryto apply ozonation as well. Capacity of

the installation was 17,424 m3

/day at anozone consumption of 6.6 kg/h.

Studies on wastewater decolourationtechnologies by means of ozone have

been carried out in Spain and Canada.They concern the wastewater fromplants producing azo dyes, while inCanada they cover dispersed dyes.

Ozonation of wastewater from threedyehouses of textile factories was car-ried out in Taiwan. In a laboratory-scale system ozonation, coagulation,sedimentation and purification with

active sludge were applied. In the full-scale installation design the capacity of5400 tons/day was assumed. Labora-tory-scale investigations in this fieldwere also carried out in Germany andthe United States.

As for a separate application of hydro-gen peroxide or UV radiation in thedecolouration or treatment of textilewastewater, besides bench-scale inves-tigations there has been no informa-tion on the use of these factors on alarger scale.

The UV radiation itself may be usedfor water disinfection, especially inswimming pools where it is appliedinstead of chlorination. Hydrogen per-

oxide is used mainly in the textileindustry for bleaching. Recently, thegrowing applicability of H2O2 has

been observed in the Fenton processapplied to the purification of industri-al wastewater and leachates [3,4].

■ MaterialThe investigation covered ananthraquinone dye, polan blue E2R(Acid Blue 62, C.I. 62045). Because oftheir chemical structure, theanthraquinone dyes are often the sub-

ject of studies on decolouration inwater solutions [5-9]. In the textileindustry it is applied in dyeing polyamide fibres and wool. Its chemi-cal structure is presented below:

■ Experimental Procedure■ and Analytical Methods

The system in which experiments ondye decomposition in water solutionsusing ozone, hydrogen peroxide andUV radiation were conducted has

been presented in our previous studiesdedicated to advanced oxidation

processes [10,11].Dye oxidation processes were carriedout in a Sovirel glass reactor 1.5 dm3 involume, equipped with a thermostat-ing jacket. In the centre of the reactorthere was a quartz tube with lightsources. The mixture of oxygen andozone flowing to the reactor was sup-plied to the solution by means of aporous plate which enabled fine gas

bubbling.

The solutions were analysed by a spec-trophotometric method using aHewlett Packard HP8452A device. Thespectra were collected in the rangefrom 190 to 800 nm. For quantitativedeterminations, absorption data at 620nm with the maximum of the dye spec-trum in the visible range were used.Because of the intensity of solutioncolouration, the length of optical pathwas 1 mm. Dye solutions of the con-centrations 100 and 200 mg/dm3 (0.25and 0.5 mmol/dm3) were tested. Theinitial pH value was natural (pH=3.8).The solution volume was 1.2 dm3.

The experimental procedure was asfollows:1. In the case of ozonation, the oxygen

flow rate ranged from 3 to 40 dm3 /h,and the ozone concentration in the

gas at the reactor inlet was withinthe range from 6 to 36 mg O3 /dm3.The process time usually did notexceed 60 minutes; samples foranalysis were taken every 5 minutes.The temperature applied rangedfrom 288 to 333 K (15-60°C).

2. The treatment with hydrogen per-oxide consisted in adding 5 or 10cm3 of 30% H2O2 solution (perhy-drol) to 1 dm3 of dye solution at theconcentration of 100 mg/dm3. Totalhydrogen peroxide was added atthe beginning of the reaction. Thetreatment time was 48 hours. Thesolution was mixed by oxygen flow-ing at the rate of 20 dm3 /h. Theprocess temperature was 298 K (25°C).

3. In the case of UV irradiation ofwastewater, the reaction time wasup to 5 hours. Oxygen passed

through the orifice at a rate of 17dm3 /h. The following lamps wereused: a low-pressure mercury-dis-charge lamp TNN 15/32 of 15 Wpower, medium-pressure lamp oftype TQ150 of 150 W electric power,and a high-pressure Q-400 burner(Hanau, Germany) of 400 W power.The experiments were carried out atthe dye concentration of 100mg/dm3; the volume of solution was1 dm3 and the temperature 298 K (25°C).

Actinometric measurements weremade in order to set oxidised UV dosessupplied to wastewater samples and tocalculate the quantum yields of pollu-tant decomposition.

To determine light intensity, a uranyl-oxalate actinometer was used. Thiswas an aqueous solution of uranyl sul-phate at the concentration of 0.01mol/dm3 and oxalate acid at the con-centration of 0.05 mol/dm3. The actin-ometer was sensitive to the wave-lengths from 208 nm to 436 nm. Lightacting on the actinometric solution

caused decomposition of the oxalicacid sensibilised with uranyl ion.

The reaction was measured by deter-mining the losses of oxalate acid atspecified time intervals by means oftitrating the samples with potassiumpermanganate at the concentration of0.2 mol/dm3. Analyses were made inan acid medium and at an elevatedtemperature (~310 K).

The aqueous dye solutions were treat-ed with ozone, hydrogen peroxide and

UV radiation. All these processes wereused to decolour the water solutions.The results obtained can be also usedin comparison with other versions ofoxidation, particularly advanced oxi-




dation with a simultaneous use ofthese two or three oxidising agents.More attention was given to theprocess of ozonation, which was con-sidered efficient, simple and economi-cal.

OzonationThe polan dye decomposition withozone was tested with respect to onthe flow rate of the oxygen-ozone mix-ture, ozone concentration in the gas,the process temperature and dye con-centration.

The effect of ozone concentration at theinlet to the reactor was investigated forozone concentrations equal to 6, 17, 20and 36 mg O3 /dm3 gas, at the flow rateof the oxygen-ozone mixture of 17dm3 /h, which gave ozone doses 85,240, 283 and 510 mg O

3 /h×dm3 solu-

tion respectively. The initial dyeconcentration in the solution was 100mg/dm3. The volume of the solutionwas 1.2 dm3 at the process tempera-ture of 298 K (25°C). The changes inthe dye concentration during ozona-tion are shown in Figure 1.

The process of decolouration dependsclearly on the ozone concentration inthe gas at the inlet to the reactor. At aconstant flow rate, this corresponds tothe amount of ozone supplied to thereaction mixture (dosing rate of O3). At

determined parameters of ozonetransfer to the aqueous solution, ozoneself-degradation rate and reaction withthe dye, the rate of ozone consump-tion during the decolouration of polan

blue can be defined.

With an increase of the reaction timeand ozone dose, a growing degree ofsolution decolouration is observed. Asexpected, the process rate is the fastestfor the highest ozone concentrationapplied, equal to 36 mg O3 /dm3. Forthe lowest ozone concentration, i.e. 6

mg O3 /dm3, there was an inductionperiod of about 5 minutes connectedwith setting up the reaction parame-ters (mainly saturating the solutionwith ozone). At concentrations 17 and20 mg O3 /dm3 the induction period isvery short, while at 36 mg O3 /dm3 itdoes not occur in practice.

Distinct induction periods areobserved when dye decompositioncurves are presented not as a functionof time but as a dose of reacted ozone.The ozone dose corresponding to the

induction period is from 10 to 25 mg O3 /dm3 solution, and increases withan increase in ozone concentration inthe gas (this corresponds to time from7 to 3 minutes).

A decrease of dye concentration in thesolution depending on the ozone con-tent in the gas mixture supplied to thereaction for three reaction times isillustrated in the inset in Figure 1. Anevident increase may be observed indye decomposition yield with a grow-

ing ozone concentration, especially forthe reaction times of 15 and 30 min-utes.

These relationships undoubtedlyderive from the applicability of ozonesupplied to the reactor in thedecolouration process. Low ozoneconcentrations in the gas phase ensure

better use of the ozone, while at highozone content in the gas its penetra-tion to the solution and participationin the decolouration reaction are muchworse. Unfortunately, if we wish to useozone in the most efficient way, the

reaction time is prolonged significant-ly and the economic efficiency of theprocess decreases. In our system, theamount of unreacted ozone increasedin time from about 20% to 60% in thegas exit.

The effect of gas mixture flow rate wasinvestigated in the range from 10 to 40dm3 /h at a constant ozone concentra-tion in the gas equal to 16 mg O3 /dm3

and the dye concentration of 100mg/dm3. The process temperature was298 K (25°C) and the reaction time was

60 minutes. A diagram of colourchanges in time is shown in Figure 2. Itis seen that with an increase of theflow rate (ozone dose supplied), thedegree of solution decolourationincreases. The relations illustrated inthe inset (Figure 2, inset) show thiseffect even more distinctly. For thegiven reaction times (15, 30 and 45min) there is a sudden decrease of dyeconcentration in the solution with anincrease of gas flow rate.

If the dye concentration is presentednot versus reaction time but versus the

doses of reacted ozone, the kineticcurves for different gas mixture flowrates will not overlap. Thus, there is animpact of gas flow rate, with the worstresults of the solution decolouration inthe experimental conditions appearing at 30 dm3 /h. This can be explained bythe fact that there are at least twoeffects in different directions. On theone hand, with an increase of the gasflow rate, the time of contact decreasesand hence the conditions of ozonepenetration to the solution deteriorate;on the other hand, mixing is more

intensive, which has a favourableeffect on the reaction rate. As a result,there is a relationship between gasflow rate and decolouration yield at aconstant dose of the reacted ozone.

The amount of unreacted ozone in theprocess conditions increases (with anincrease in the gas flow rate) fromabout 24% to 70%.

The effect of temperature on dyedecomposition during ozonation was

investigated for the gas flow rate of 17dm3 /h and at a low ozone concentra-tion in the gas of 6 mg O3 /dm3. A slighteffect of temperature on the process ofdecolouration was found. The bestresults were obtained at 318 K (45°C).The dye decomposition rate close tooptimum was obtained at 323 K (60°C).A slightly slower rate was reported at288 and 203 K (15 and 30°C) (Figure 3).It is well known that gas solubility inliquid (ozone in water) decreases withtemperature growth, while the rate ofozone decomposition in water andthat of reaction with the dye increases.The latter effect probably prevails, as isreflected by the results obtained. Thisdependence is clearly visible in theinset in Figure 3, where the decoloura-tion degree depends only slightly ontemperature for the three selectedreaction times of 20, 30 and 45 min.

In the case of elevated temperature,the amount of unreacted ozone in theoutlet gas decreased to 8.3% at 318 K (45°C) and 5.3% at 333 K (60°C). This isundoubtedly related not so much to itsreaction with the dye particles as to the

process of ozone self-degradation.

When increasing the dye concentrationup to 200 mg/dm3, a decrease in per-centage yield of the dye decomposi-tion was observed, as expected. Thiseffect is visible when dye degradationis considered with respect to the react-ed ozone dose (Figure 4). The absolutereaction rate increases with an increasein the dye concentration.

Summing up the process of polan bluedecomposition in the water solution

by means of ozone, it is concluded thatthe choice of optimum process para-meters would require a decision con-cerning optimisation criteria. Weshould decide whether the main crite-rion should be the process duration orthe dose of reacted ozone (mostadvantageous in the decolourationprocess). In both cases the results will

be different. In technological condi-tions a compromise should be made

between these two parameters, because both are very important forthe process' economy. A decrease in

the ozone supply rate reduces thedirect costs of ozone (electrical energyand exploitation costs), but prolongsthe process duration, thus increasing the residence time of the wastewater




and the installation capacity (invest-ment costs).

The application of hydrogen peroxideThe conditions and technique of carry-ing out the decomposition of theanthraquinone dye by means of

hydrogen peroxide have been dis-cussed earlier. In this study, high con-centrations of hydrogen peroxide wereused bearing in mind the poor resultsof colour reduction at low concentra-tions obtained in our previous investi-gations on the decomposition of non-ionic detergents, Tritons and Tergitols[12-14] and textile wastewater - both ina model and in reality [15,16].

Figure 5 shows the decolourationdegree in time up to 48 hours for twodifferent initial concentrations ofH

2O

2. In this time (48h), hydrogen

peroxide in the solution at tempera-ture of 298 K is wholly degraded. Inthe first case the amount of H2O2added to the solution was 5 cm3 /dm3,which corresponded to the peroxideconcentration equal to 0.049 mol/dm3,while in the second case the concen-tration was twice as high and amount-ed to 0.098 mol/dm3.

It follows from the relationshipsobtained that the main course of thereaction takes place in the first 2 hourswhen the decolouration degree

increases linearly. This may beexplained by the assumption of a con-stant concentration of hydroxyl radi-cals, products of hydrogen peroxidedecomposition in the first phase of thereaction course, when the H2O2 con-centration is high enough. The secondstage, in which decolouration of thesolution is much slower, is probablyrelated to secondary processes involv-ing colour products of polan blue oxi-dation. Processes leading to the recon-struction of dye molecules are alsopossible [17-19]. The yield of

decolouration does not depend strictlyon the initial concentration of hydro-gen peroxide, because when it is dou-

bled, the decolouration degree increas-es from 5.8% to 7.8% after 45 minutesand from 17.4% to 20.1% after 130 min-utes. Hence, even a doubled concen-tration of H2O2 caused only a slight(ca. 4%) increase in the polan dye'sdegree of degradation.

Photochemical processThe decomposition of polan blue E2Rin the aqueous solution by means of

UV radiation (photolysis) was carriedout using three types of lamps. Theydiffered both in the type of emittedspectrum and in their power. The max-imum photo-reaction time was 5

Figure 1. The effect of ozonation time on changes in dye concentration (solution colouration) for different ozone concentrations (6, 17, 20 and 36 mg O3 /dm3 ) in the oxygen-ozone mixture. Temperature25°C. Flow rate of the gas mixture 17 dm3 /h. Dye concentration in water 100 mg/dm3. Inset:Dependence of dye concentration on ozone concentration in the oxygen-ozone mixture for three reac-

tion times 15, 30 and 45 min.

Figure 2. The effect of ozonation time on changes in dye concentration (solution colouration) for different gas mixture flow rates (10, 17, 30 and 40 dm3 /h). Ozone concentration in the oxygen-ozonemixture 17 mg O3 /dm3. Temperature 25°C, dye concentration 100 mg/dm3. Inset: Dependence of dyeconcentration on gas mixture flow rate for three reaction times 15, 30 and 45 min.

Figure 3. The effect of ozonation time on changes in the dye concentration (solution colouration) fordifferent temperatures of the solutions (15, 30, 45 and 60°C). Gas flow rate 17 dm3 /h, ozone concen-tration in the oxygen-ozone mixture 6 mg O3 /dm3 , dye concentration in the solution 100 mg/dm3.Inset: Dependence of dye concentration on the solution temperature for three reaction times 20, 30and 45 min.




Figure 4. Decomposition of alizarin blue in theaqueous solution for two initial concentrations

100 and 200 mg/dm3

depending on ozone dose.

Figure 5. Dependence of decolouration degree of the solution on reactiontime for two doses of hydrogen peroxide added (5 cm 3 and 10 cm3

H 2O2 /dm3 solution). Initial dye concentration 100 mg/dm3 , temperature25°C.

Figure 6. Kinetics of alizarin blue photolysis depending on the absorbeddose of radiation for three different radiation sources: low-pressure lamp 15W, medium-pressure lamp 150 W and Q-400 quartz burner. Initial dyeconcentration 100 mg/dm3 , temperature 25°C.

hours. The relevant data are given inTable 1.

For instance, a low-pressure mercury-discharge lamp TNN 15/32 of 15 Wpower emitted light of intensity1.97·1022 quantum/dm3h, which corre-sponded to 3.27·10-2 Einstein/dm3h.75.9% of the quanta were radiation atλ <310 nm with maximum at λ =254nm. The number of quanta is given pertime unit and volume unit of the reac-tor in which experiments were carriedout. The quantum yield of the decom-position is calculated on the assump-tion that the whole colour change inthe solution is related to the decompo-sition of dye molecules. Photochemicalcapacity is the amount of decomposedmolecules per 100 eV of absorbed lightenergy. The power emitted by the

lamp in the form of light was 3.33W/dm3.

When comparing the applied lampsand taking into account light emission

below 310 nm only, the most efficientappeared to be the TQ150 (2.61·10-2

Einstein/dm3

h) and TNN15/32 (2.48·10-

2 Einstein/dm3h) lamps, while the Q-400 burner was about 3 times less effi-cient (7.4·10-3 Einstein/dm3h).

The results of polan dye decomposi-tion by photolysis have no direct con-nection with the determined intensityof light emitted by particular lamps.The 15 W lamp, emitting the mostmonoergetic light in the UV range(λ =254 nm), gives very good results ofdecomposition both in the aspect oftime and quanta absorbed. On theother hand, the medium-pressure

mercury-discharge lamp, (despite its10 times higher electric power) with asimilar number of quanta in the UVrange, gives much worse results of dyedecomposition both in time and whenanalysing decolouration as a functionof the absorbed quanta.

It is interesting that the quantum yieldof polan blue decomposition is almostidentical for the TQ150 lamp and theQ-400 burner, despite significant dif-ferences in the emission spectrum of

both light sources.

The character of decomposition curvesreveals that in the aqueous solutionthe dye is degraded as a result of pho-tolysis and photo-oxidation when UVradiation is used. The UV radiationthat is emitted with light impedes pho-todegradation. The significant contri-

bution of UV radiation to the processmay lead to a serious hampering of the

reaction, whose rate is then at least 10times lower than when monoenergeticradiation from the UV range is used.

■ Conclusions

The experiments revealed the highsusceptibility of polan blue E2R todegradation by ozone, hydrogen per-oxide and photolysis. The best resultsof decolouration were obtained using ozone as an oxidant. The degradationrate was affected by ozone dose andconcentration in the gas mixture, itsflow rate through the solution, and bytemperature.

The process may be optimised by tak-ing into account the dose of reactedozone or the time of reaction. Highdegrees of ozone utilisation and lowdoses of the reacted ozone required a

slow gas flow rate and a low ozoneconcentration therein.

This in turn caused the reaction timeto be longer, which as a consequencerequired a larger reactor volume. Inindustrial conditions, a compromiseis necessary and the decolorisationshould be optimised, taking intoaccount the process' economy.

The use of hydrogen peroxide as anoxidant, or to carry out dye photolysisin the presence of oxygen, does not

bring about satisfactory results. Re-action times are long, and the requiredlight intensity or H2O2 concentration ishigh. From the economic point ofview, these two factors have no practi-cal importance.

In the case of industrial coloured solu-tions, which do not require very accu-rate treatment but only a complete




QuantityLow-pressure lamp

15 W

Medium-pressure

lamp 150 WQ-400 quartz burner

Amount of quanta emitted per time

unit for the whole UV-VIS range

1.47 ·1022

quantum/dm3 h

0.975 ·1023

quantum/ dm3 h

5.52 ·1022

quantum/dm3 h

Quantum yield calculated for total

absorbed light

1.72 ·10-3

molecules/quantum

1.29 ·10-4

molecules/quantum

9.68 ·10-5

molecules/quantum

Amount of quanta emitted per time

unit for light at λ <310 nm

2.244 ·1020

quantum/min

2.107 ·1020

quantum/min

8.94 ·1019

quantum/min

Quantum yield calculated for

light at λ <310 nm

2.27 ·10-3

molecules/quantum

1.19 ·10-3

molecules/quantum

1.19 ·10-3

molecules/quantum

Power of light emitted in the whole

UV-VIS range3.33 W 15.52 W 8.35 W

Photochemical quantum yield calcu-

lated for the whole absorbed light

4.07·10-2

molecules/100eV

4.34·10-3

molecules/100eV

3.32·10-3

molecules/100eV

Power of light emitted in the range

of λ <310 nm2.92 W 2.48 W 1.00 W

Photochemical quantum yield

calculated for light at λ <310 nm

4.64·10-2

molecules/100eV

2.71·10-2

molecules/100eV

2.77 ·10-2

molecules/100eV

Table 1. Comparison of parameters and results of photochemical decomposition of anthraquinone dyeby light emitted by different lamp types.

decolouration which would enabletheir re-use in the technologicalprocess, one-stage processes of chemi-cal oxidation through ozonation can

be used successfully.

❏

References

1. R.G. Rice, “Applications of ozone for industrial wastewater treatment - a review”, OzoneScience & Engineering 18, 477-515 (1997).

2. R.G. Rice, “Applications and current status of ozone for municipal and industrial wastewater treatment: A literature review”, The Role of Ozone in Wastewater Treatment, Proceedingsof a Seminar held at the Centre for Environ-

mental Control & Waste Managemant, Imperial College of Science, Technology & Medicine,

London SW7 2BU UK.3. E. Oliveros, O. Legrini, M. Hohl, T. Muller, A.M.

Braun, “Industrial waste water treatment: large scale development of a light-enhanced Fenton reaction”, Chemical Engineering and Pro-

cessing 36, 397-405 (1997). 4. S. H. Gau, F.S. Chang, "Improved Fenton me-thod to remove recalcitrant organics in landfill

leachate", Wat. Sci. Tech. 34, 7-8, 455-462(1996).

5. M. Matsui, H. Nakabayashi, K. Shibata, Y.Takase, “Ozonization of triphenylmethanedyes”, Bull. Chem. Soc. Japan., 57, 11, 3312-3316 (1984).

6. J. P. Gould, K. A. Groff, “The kinetics of ozonol- ysis of synthetics dyes”, Ozone Science & Engineering, vol. 9, pp. 153-164, 1987.

7. T. Kono, S. Nakamoto, Y. Shimada, “Dye efflu-ent treatment with ozone”, 13th Ozone World Congress, Kyoto, Japan, 1997, pp. 283-288.

8. R. Tosik, K. Janio, “Kinetic aspects and ozoneconsumption in the decolouration process of dyes”, Proceedings of the IOA PAG ANNUALCONFERENCE, 1997, The International Ozone

Association, Pan American Group, 369-377.

9. K. Honda, Y. Wada, “Ozonation of dyestuff man-ufactory waste water”, 13th Ozone World Congress, Kyoto, Japan, 1997, pp. 41-44.

10. L. Kos, J. Perkowski, S. Ledakowicz, “Advanc-ed oxidation of textile wasteater from polyester dyeing process”, Environment. Protec. Eng.,

25, (4) 21-29 (1999).11. J. Perkowski, L . Kos, S. Ledakowicz, “Ad-

vanced oxidation of textile wastewaters”,Ozone Sci. & Eng., 22, 5, 535-550 (2000).

12. J. Perkowski, S. Ledakowicz, “Ozonation of Tergitol TMN6 in water solutions (in Polish)”,Ochrona Œrodowiska, 4 (79), 9-14, 2000 (in

Polish).13. S. Ledakowicz, J. Perkowski, “Kinetics of

ozonation of non-ionic detergent in aqueous solutions”, Proc. of the 13th Ozone World Congress, Vol.1, Kyoto 1997, pp. 343-348.

14. S. Ledakowicz, J. Perkowski, “Destruction kinetic of the Triton X-100 under influence of ozone”, In¿ynieria Chemiczna i Procesowa, 19,1, 205-216 (1998).

15. J. Perkowski, L. Kos, S. Ledakowicz, “Appli-cation of ozone in textile wastewater treat-

ment”, Ozone Sci. & Eng., 18, 73-85 (1996).16. J. Perkowski, L. Kos, S. Ledakowicz, “Appli-cation of ozone in textile wastewater treat-

ment”, Proc. Int. Ozone Symp. Application of ozone in wastewater treatment, A.K. Biñ, Ed.Warsaw 1994, pp. 327-335.

17. J. Perkowski, J. L. Gêbicki, R. £ubis, J. Mayer,“Pulse radiolysis of antraquinone dye aqueous

solution”, Radiat. Phys. Chem., 33, 2103-108(1989).

18. J. Perkowski, J. Mayer, “Gamma radiolysis of anthraquinone dye aqueous solution”, J. Radioanal. Nucl. Chem., Articles, 132, 269-280(1989).

19. J. Perkowski, J. Mayer, “Gamma radiolysis of an aqueous anthraquinone dye solution in the presence of oxygen”, J. Radioanal. Nucl.Chem., Articles, 172, 19-27 (1993).

❏ Received 28.11.2001 Reviewed: 23.05.2002

Date post:	02-Jun-2018
Category:	Documents
Upload:	pablocolindres
View:	218 times
Download:	0 times

2002_J.perkowski_Decomposition of Anthraquinone Dye in the Aqueous Solution by Ozone, Hydrogen...

Documents