ABSTRACT
This book is based on the Mid-Atlantic Industrial and Hazardous Waste Conference to bring together professionals interested in the advancement and application of technologies and methods for managing industrial and hazardous wastes.
TABLE OF CONTENTS
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good engineers.
MANNERS Manners are the social mores of our society. Within each society we agree on what are good and bad manners. In many societies, when someone holds open a door for us, for example, we respond with a "thank you", acknowledging an unselfish deed. Manners is what the African-
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not adhere to a adhere to the admonition will make them better engineers. moral statement is that engineering involves the public and not keeping up must do to continue to be part of the engineering community. The can result in harm to both the engineer and the public.
admonitions statement in a Code of Ethics will not get engineers in trouble, but to For example, in the ASCE Code of Ethics, Guideline 7a reads: 7a. Engineers should keep current in their specialty field by engaging in professional practice, participating in continuing
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act in such a act in a manner that we would not necessarily
way. That is, if we find that having bad manners, or acting immorally, or even breaking a law is advantageous to us individually, why we, at any given moment, ought not to want others to emulate. The obvious answer to that question is that we don’t want to get
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know we are behaving badly and eventually regret
such actions. But if, by telling lies, I become a scoundrel, why would I believe this to be an undesirable result? If I ran an engineering practice where I made it a habit of telling lies to clients (e.g. "The report is in the mail" when in fact it is still being prepared), why is this detrimental? Why will telling lies
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good engineer. Lying: Moral Choice in Public and Private Life On Being Responsible University Press of
Bok, Sissela (1978) Pantheon, New York Pritchard, Michael S. (1991) Kansas, Lawrence KS
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Abstra ct for Mid-Atlantic Industrial and Hazardous Waste Conference
P’ A 2 P: P , A 2
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To bet ter compare the reaction rates observed for various iron particles, it is essential to quantify the reactivity per unit metal surface area. The rate of transformation for a chlorinated organic compound in a batch system can be described by the following equation [4]: pseudo-first-order kinetics. Best-fit values of KSA are 5.31X1 O'4 for nanoscale iron and 1.0x1 O'4 for the Aldrich iron, respectively. Several factors may contribute to the difference in reactivity. Laboratory synthesized nanoscale iron surface may have “fresher” metal surface due to less surface oxidation or surface contamination. Mass transfer resistance was also less significant for the nanoscale iron batch system. The metal to solution ratio for the Aldrich iron experiment (10 g/20 mL) was 40 times of that for the nanoscale iron experiment (0.25 g/20 mL). However, the two batch systems had similar mixing intensity (mixed on a rotary shaker at 30 rpm). It was observed that most of the Aldrich iron particles were settled at the bottom of the bottle while Figure 2. Reactions of commercial grade iron particles (Aldrich, <10 pm) with CT. Initial CT concentration was 0.103 mM (15.9 mg/L). Metal to solution ratio was 10 g/20 mL.
Where C is the concentration of organic compound in the aqueous phase (mg/L), KSA is the surface-area-normalized rate coefficient (L/h/m2), as is the specific surface area of metal (m2/g), pm is the mass concentration of metal (g/L), and t is time (h). For a specific system, KSA, as and pm are constants. The above equation therefore represents a
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PO LLUTION PREVENTION IN A PHARMACEUTICAL FACILITY INTRODUCTION
ALAN F. YEN, Ph.D., P.E., DEE AFY, Inc. 504 Harvard Avenue Swarthmore, PA 19081 EDWARD G. HELMIG
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METHODOLOGY
In order to characterize the spent blast material and to study the variability among samples, ten actual ABM samples were collected from Atlantic Marine Corporation, and respective metal concentrations were measured using two EPA standard methods i.e. the toxicity characteristic leachate procedure and total
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RESULTS
its compressive strength, that is, its behavior under load. To understand the behavior of hardened concrete with blast material and to study the variability in samples from one operation to another ten different samples (moisture content 0- 9.5 % and finenes of modulus 1.23-3.6) were used. Four samples per blast
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______________ _________ l og(Kp) = 1,071og(Kow) - 2.34; = 0.9764
Sorbent: Dover DGSL
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REFERENCES
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REFERENCES Groundwater Models—Scientific and
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MODELING ASPECTS OF CONTAMINANT TRANSPORT STUDIES USING A GEOTECHNICAL CENTRIFUGE δ"1 St. 8th St. INTRODUCTION
THOMAS F. ZIMMIE Civil Engineering Department Rensselaer Polytechnic Institute
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GEOTECHNICAL CENTRIFUGE TYPES ]. The small
In general, the two commonly used geotechnical centrifuges are the balanced-arm type and the drum type. The balanced-arm centrifuge consists of the centrifuge arm, centrifuge platform that holds the model, balancing counterweight, various fluid and signal connections for data acquisition and mechanism signaling, and the driving mechanism. This centrifuge will typically
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,200 g-tons centrifuge at the U.S. CENTRIFUGE MODELING PRINCIPLES Modeling of Models Scaling Relations
Army Corps of Engineers Waterways Experiment Station in Vicksburg, Mississippi. The use of a centrifuge is advantageous for studying phenomena dominated by the earth’s gravity such as saturated groundwater flow. The basic idea is to
chapter 100|1 pages
times greater than that of ,000 times longer than that of the Pi Numbers
corresponding model distance. An example is shown in Figure 1 for a simple flow problem where a 1/N scale centrifuge model experiment was run for one day, using g = 100. As is shown, the prototype seepage velocity is 1/100 that of the model while the corresponding distance is the model. Under these modeling conditions the time for a fluid particle to
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represents the transition zone between laminar and turbulent flow for flow g, however, for sands the R<. is 1 at about 50 g for g for a medium to fine sand. 0, mechanical dispersion will CENTRIFUGE MODELING AS A PREDICTIVE TOOL
through porous media [13]. Thus it is important that Rc remain below 1, so that flow remains laminar in both the model and prototype. Under this condition, Darcy’s law is valid. Under normal circumstances, turbulent flow through most soils is rare. It should be noted that Rc in the model and prototype will not be equal (i.e., no similitude of Reynold’s numbers) since the fluid flow velocity in
chapter 2|2 pages
[15] which is Radioactive Contaminant Transport g-ton geotechnical centrifuge [6]. The Using the finite was injected into the soil at position GM 2, traveled through the soil, the radioactive count rates were traveled through the soil. The time of 115 minutes does not
basically a small test pad. This type of testing in the laboratory, under 1 g conditions, is unlikely and if attempted, very time consuming. Analytical and numerical solutions are often used for most studies on contaminant transport. Analytical solutions are more common since they are simple to use. However, in general, analytical solutions tend to be highly
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CONCLUSIONS REFERENCES
The following conclusions can be made pertaining to the centrifuge modeling of contaminant transport processes: 1. Centrifuge model tests have the ability to accelerate the transport processes (by a factor of N2) in flow problems and provide stress levels similar to prototype stresses.
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Figure 2 - Results of batch removal of arsenic [As(V)] with Connelly-GPM iron and calcareous sand (initial concentrations 50 to 22,000 μg/L) 500 j ................................................... O ppb As(V)..................... “Šk 400 Flow = 1.0 mL/mìn « 200 HRT = 6.0 minutes І 100 O V · — *
------------1------------l·-^ 0 200 400 600 800 1000 e Volumes Figure 3 - Results of laboratory column arsenic [As(V)] retention experiment. pH 6.3 and I.S.=0.01 M
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and the presence o
f non volatile transformation intermediates. Incorporation o f radiolabelled carbon into biomass was not determined. These and similar data were evaluated to determine the maximum rates o f naphthalene mineralization for the three sorbents and four aging periods (Figure 2). Figure 1. Distribution o f 14"C-components during biodegradation o f
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A NEW ION-EXCHANGE PROCESS FOR CHROMATE REMOVAL Dongye Zhao, Arup K. SenGuota and Lori Stewart Environmental Engineering Program 13 E. Packer Avenue Lehigh University Bethlehem, PA 18015 INTRODUCTION
Cr(VI) concentration. Understandably, polymeric anion exchangers in fixed-bed column configuration have been widely used both at laboratory and commercial- scale levels for chromate removals from contaminated waters (7-10). Previous
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COD is reduced (the COD removal is 49%) for 25,000 mg/1 hydrogen peroxide and 2,000 mg/1 ferrous ion applied. The wastewater pH is reduced to 1.38. Fig. 3 shows variations of the residual hydrogen peroxide in the wastewater treated with hydrogen peroxide and Fenton's reagent. For the oxidation process using hydrogen peroxide only, the hydrogen peroxide applied is decomposed about 40%. Using Fenton's reagent, a higher percentage (80%) of hydrogen peroxide is decomposed. The reaction between hydrogen peroxide and ferrous ion results in the production of hydroxyl radicals (see eq.l) which are effective to oxidize the organic chemicals that are difficult to oxidize with ordinary oxidants. Thus, the decomposition rate of hydrogen peroxide and COD removal rate for Fenton oxidation are higher than for hydrogen peroxide oxidation. ( 1 )
The variation of hydrogen peroxide is an important parameter for the Fenton oxidation process. Fig. 4 shows the COD removal at different concentrations of hydrogen peroxide. More COD is removed at higher hydrogen peroxide concentrations with 44% of COD removed with 25,000 mg/1 hydrogen peroxide applied.
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Re sults of the Kinetic Experiment Table II provides data for the twelve experimental runs. When initial PCP concentration was 100 mg/1, the best removal occurred with an initial hydrogen peroxide concentration of 0.1M to reduce PCP to 0.03 mg/1 in 120 minutes. With an initial PCP concentration of 10 mg/1, 0.01 M of hydrogen peroxide reduced PCP concentration to 0.03 mg/1 in 15 minutes and to below detectable limits in less than 30 minutes. Finally, the best removal for 1 mg/1 of PCP occurred with 0.001 M of hydrogen peroxide reducing PCP concentration to 0.01 mg/1 in 5 minutes and to below detectable limits in less than 15 minutes. Therefore, the optimum concentration of hydrogen peroxide decreased with decreasing initial PCP concentration. Since all experimental runs were described by the first order reaction kinetics, the removal of PCP generally follows first order reaction kinetics. Models The independent variables of the kinetic experiments were time, and
where ki = First order rate constant; kmax = constant to determine maximum height of the curve; h = constant that determines the spread of the curve; and Oopt = concentration of hydrogen peroxide at which ki is maximum.
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The equa tion is modified as follows to account for the influence of (3) where a,b,c,d = constants. The model was applied to the data, resulting in 99 .115 % of the variance being explained, an R of 0.996 and a final loss of 0.00437. The determined constants were as follows: a = 1.693, b = 0.688, c = 396.056, d= 0.862, h = 0.301, and kmin = 0.0195. That is, the model is good for the range of PCPj from 1 mg/1 to 100 mg/1 and from 1 M to 0.001 M. Therefore, the model is only good for
the rate constant for benzene oxidation by both hydrogen peroxide and UV light the benzene concentration, μΜ; and the hydrogen peroxide concentration, μΜ. a, b, and c are reaction orders Again, the data was applied to the above model. It was found that this
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ERWIN M. COHEN INTRODUCTION
EMCO Testing & Engineering 159 Sachem Street Norwich, CT 06360 In what has become known as the "Quiet Corner" of
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Un fortunately, the State's acid rain testing program was stopped in 1990. But unpublished data collected by the author in recent years, and reports from New York State strongly suggest that the acidity of rain has not significantly improved. ORIGINS AND EFFECTS OF ACID RAIN
Sulfur dioxide and nitric oxide are the two main factors in the formation of acid rain. When high sulfur coal is burned in Midwestern and other coal producing areas, the combustion gas vented through tall stacks travel with the normal west to east winds to
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and soils. They also do not have the problem of acid wells. Therefore, it should be recognized that the acidity of Southeastern Connecticut's ground water is due to a combination of acid rain and the native rock and soil properties. Figure 2 is a picture taken in the Norwich area, at Exit 81 on Interstate 395. This outcrop shows the typical bedrock of the county. Figure 2 Typical Granitic Rock Outcrop in Norwich Conclusions and Recommendations
Federal and state environmental agencies need to recognize that acid rain is contributing to the acidity of both well waters and surface waters. Both are
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th at originates in neighboring countries has been recognized as a cause of well water problems. The Swedish government has alerted home owners to the danger, and even subsidized the purchase of home water treatment systems [5]. In New York, where the Adirondack lakes continue to be affected by acid rain. Long Island Lighting Company (LILCO) announced it will no longer sell its pollution rights to Midwestern or Southeastern power companies [6]. Recently many states, including Connecticut, have passed electric deregulation bills. This encourages large scale users to purchase the cheapest power available. Some citizens are concerned this will increase the burning of coal in plants without pollution controls and lead to more acid rain. Perhaps the only recourse for citizens will be to come together and initiate Federal court actions to prevent downwind environmental damage. References
1. "Annual Air Quality Survey for 1986." Department of Environmental Protection, State of Connecticut. 2. "Environmental Quality in Connecticut, 1996 Annual Report." Council of Environmental Quality. 3. Rogers, John. 1985. "Bedrock and Geological Map of
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FACTORS AFFECTING THE OXIDATION OF DICHLORVOS INSECTICIDE BY FENTON’S REAGENT
Department of Environmental Engineering and Health Chia Nan College of Pharmacy and Science Tainan 717. Taiwan, R.O.C.
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(9) the oxidation rate of organic compounds is fast when large amount of ferrous ions are present because large amount of hydroxyl radicals are produced. However, the Fenton reaction may slow down due to the slow ferrous ion production. In previous studies, the photocatalytic degradation of dichlorvos (DDVP. an insecticide) on glass supported titanium dioxide was investigated. Results indicate that photocatalysis can be an effective process for the degradation of dichlorvos [3]. The mineralization of dichlorvos and the reduction of toxicity were investigated via the photocatalytic reaction [4]. This study uses Fenton’s reagent, ferrous ions/hydrogen peroxide, to oxidize dichlorvos with an attempt to explore the behavior of dichlorvos oxidation and how factors such as pH, [H O ],
The reaction rate in Equ. 6 is much slower than that in Equ. 1. It is derived that ferrous ions are exhausted quickly, but reproduced slowly [2]. Consequently,
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INDEX
Accidental Release, 395 W. A., 310 Activated Sludge, 197 Brownfields, 111, 133 P, 339 E., 522 Adsorption, 288, 717 R., 155 Advanced Oxidation Processes, 106, B. L., 585
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IN DICES FOR 25тн, 26тн, 27тн, 28тн & 29тн INDUSTRIAL WASTE CONFERENCES
Abandoned Mine Lands, XXV 468 Aeration, XXVIII, 531 Abandoned Mine Lands, XXIX, 553 Aerobic, XXIX, 54, 414, 434 Abandoned Wastes, XXV 305 Aerobic Biodegradation, XXVIII, 15, Abatement Costs, XXVI, 380 109, 326, 537
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ХХү 330
Phytoremediation, XXIX, 605 D., XXVII, 528 Pilot Scale, XXVIII, 611, 619 J. C., XXVI, 285 W O., XXVII, 274 Pentachlorophenol, XXY 209 Plant Survey, ΧΧΥ 159 Pentachlorophenol, XXVI, 637 Plastics, XXVI, 557 Pentachlorophenol, XXVIII, 655 Platinized Titanium Dioxide, XXIX,
