Catalytic Destruction of Gas-Phase PCE and TCE in Groundwater and Soils - Laboratory Study & Field Investigation Departments of Atmospheric Sciences & Chemical and Environmental Engineering, The University of Arizona, Tucson, AZ 85721 Song Gao , Erik Rupp, Marty Willinger, Theresa Foley, Erik Rupp, Marty Willinger, Theresa Foley, Suzanne Bell, Brian Barbaris, Robert Arnold, Suzanne Bell, Brian Barbaris, Robert Arnold, Eduardo Sáez, Eric Betterton Eduardo Sáez, Eric Betterton Desert Remedial Action Technologies Workshop - Phoenix October 3, 2007
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Catalytic Destruction of Gas-Phase PCE and TCE in Groundwater and Soils -
Laboratory Study & Field Investigation Departments of Atmospheric Sciences & Chemical and Environmental
Engineering, The University of Arizona, Tucson, AZ 85721
Song Gao, Erik Rupp, Marty Willinger, Theresa Foley, Suzanne Bell, Erik Rupp, Marty Willinger, Theresa Foley, Suzanne Bell, Brian Barbaris, Robert Arnold, Eduardo Sáez, Eric BettertonBrian Barbaris, Robert Arnold, Eduardo Sáez, Eric Betterton
• Demonstrate the validity of a new remediation method to destroy chlorinated solvents: Redox Catalysis.
• Explore reaction mechanisms and kinetics involved.
• Describe the successful application of this method in a pilot field study at a State Superfund site in Tucson.
• Estimate treatment costs and illustrate the potential of this method for low-cost, large-scale remediation.
Paper in PressPaper in Press: Applied Catalysis B: Environmental, 2007: Applied Catalysis B: Environmental, 2007
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at bench scale; in a fixed-bed reactor
Chlorinated Solvents are Widespread Contaminants in Soils and Groundwater in the US
• PCE & TCE are among the top 31 CERCLA (Superfund) Priority List of Hazardous Substances.
• PCE and TCE are the 1st and 3rd most frequently detected solvents in groundwater at concentrations greater than their respective MCLs.
Moran et al. 2007
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Also, PCE and TCE are the most frequently occurring mixture of solvents in goundwater. They are often found as mixtures due to their co-use in industrial processes or their degradation from one to another.
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Samples of groundwater taken from more than 5000 wells thourhgout the US, by US Geological Survey.
Widespread Contamination by Chlorinated Solvents
• Regional level:
Are primary contaminants at 29 out of 33 of Arizona’s WQARF (“State Superfund”) sites &
at 13 out of the 14 National Superfund sites.
• Local Level:
The Park-Euclid site in Tucson is contaminated by PCE and TCE that are derived from long-defunct dry cleaning operations and
PCE concentration PCE concentration in groundwater in groundwater
from 100 ppb to 1 from 100 ppb to 1 ppb.ppb.
1 ppb
10 ppb
100 ppb
1000 ft
Harmful Health Effects ofPCE & TCE
• Can cause cancers in animals.• Are probably human carcinogens (DHHS).
Necessity to develop efficient & economic remediation technologies to destroy chlorinated solvents.
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Of the 50 remediation technologies identified by NRC (majority are physical containment or biological in nature), only 5 chemical reaction technologieds were listed. This shortage of alternative remediation technologies is having the undesirable effects of limiting remediation efforts to only those sites that post an immediate health risk. There is also mounting pressure to relax standards at other sites because there is no cost-effective alternatives.
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Chlorinated solvents have been implicated in skin, liver and kidney cancers, nervous system dysfuction, and fetal heart defects.
Previous Methodologies
• Incineration (oxidation)- air pollution; formation of toxic substances
• Solidification- not destructive in nature
• Pump and Treat (for groundwater)- high cost; contaminant rebound
• Soil Vapor Extraction (SVE)- high cost; not destructive in nature; further treatment
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When semi-volatile contaminants are present in an extensive vadose zone, SVE is frequently selected to recover pollutants.SVE applications yield contaminated gas streams that are frequently cleaned up via carbon adsorption before release to the atmosphere - unadsorbed hydrocarbons may still post a threat. The cost of such operations can be heavily influenced by carbon recovery or replacement costs, particularly when spent carbon must be treated off site as hazardous waste.
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Pump and treat is more expensive than SVE, since pressure driven gas recovery (SVE) is more economical than water recovery from porous media (p&t).
SVE followed by Activated Carbon Adsorption
• The cost of such operations can be heavily influenced by carbon recovery or replacement costs, particularly when spent carbon must be treated off site as a hazardous waste.Ground Water
Contaminant Plume
VaporVadose Zone
GAC
Column
Released into atmosphere
Catalytic Destruction - Oxidation
• C2Cl4 + 2O2 2CO2+ 2Cl2
• 4HCl + O2 2H2O + 2Cl2
metal catalyst
metal catalyst
• Catalyst categories:
- supported noble metals (e.g. Pt, Pd); base metal oxides (e.g., Cu,
- Deactivation through chlorine poisoning (blocking active sites)
- Production of furans and dioxins (incomplete oxidation)
• C2Cl4 + 5H2 C2H6 + 4HCl
• Cl2 + H2 2HCl
metal catalyst
metal catalyst
• Catalyst categories:- Supported and unsupported noble metals
• Issues - Rapid deactivation through coking
- High cost of H2
Catalytic Destruction – Reduction
• Hypothesis
- Simultaneous reducing and oxidizing (“redox”) conditions may overcome the issues arising from reduction or oxidation alone?
• Lab study of redox catalysis- Reaction temperatures low enough?
- Efficient destruction of PCE and TCE?
- Catalyst deactivation avoided?
- Good alternatives for H2 as the reductant?
• Field study- Explore feasibility of redox method in field operations
- Estimate treatment costs
Objectives
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This is an example of how intuition can lead to surprising, and surprisingly wonderful, discoveries.
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Do we have an edge over other technologies, not only in terms of effectiveness of treatment, but economics of treatment?
Lab Process Flow Diagram
• 1” Diameter• 1” Length
Catalyst
• Cut from an automobile catalytic converter (cylindrical: 1” diameter x 1” length)
• Pt/Rh are supported (3:1) on a monolithic honeycomb
• Honeycomb is composed of cordierite (90%) and washcoat (10%), containing alumina, cerium, zirconium and other trace constituents
• Cross section of catalyst’s channels: 2mm x 2mm
Reactor System
Water Bath
PCE filled U TubeMFC
MFC (Mass Flow Controller )
N2
H2
O2
Waste
Tube Furnace
Reactor
GCwaste
Honeycomb
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The honeycomb is ~ 20cm from the upstream of furnace (38cm in length). This gives the gas enough residence time to warm up to the furnace T before it enters the honeycomb. This is verified by an independent measurment.
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First describe reactor; then describe PCE generation, naturally leadning to next slide - gas measurements.
Analytical Measurements
• HP 5890 Gas Chromatograph
• Measure chlorinated and de-chlorinated hydrocarbons:
A 0.53μm wide-bore capillary column with a
flame ionization detector (FID)
• Measure CO2, H2 and O2:
A Supleco packed column with a
thermal conductivity detector (TCD)
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He used as carrier gas. Injector and detector T were typically 200C and 250C, respectively.
Experiments
• Initial furnace temperature was 75°C.• Furnace temperature was ramped to the desired final
temperature at 2°C/min. • T change was slow enough to assume steady state
reactions at any given T.• Influent and effluent gas streams were periodically
sampled and analyzed for composition.• At end of each experiment, all gas streams were turned
off except for O2, and the furnace T was held at 450°C for 8 hours in order to clean the catalyst surface.
This regeneration process proves to be effective in maintaining catalyst activity for over two years!
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mild and convenient!
Multiple Reduction & Oxidation Reactions in a Redox System
• Major reactions leading to end products
C2Cl4 + 5H2 C2H6 + 4HCl
C2Cl4 + 2O2 2CO2 + 2Cl2
C2H6 + 3.5O2 2CO2 + 3H2O
2 H2 + O2 2H2O
• Additional reactions (involving intermediates)
2C2Cl4 + 7H2 2C + 8HCl + C2H6
C + O2 CO2
4HCl + O2 2Cl2 + 2H2O
H2 + Cl2 2HCl
PCE Conversion under Redox and O2-only Conditions
0%
10%
20%
30%
40%
50%
60%
70%
80%
90%
100%
50 100 150 200 250 300 350 400 450 500
Catalyst Temperature (oC)
PCE Conversion
a
H2/O2 2.15H2/O2 1.18H2/O2 0.67H2/O2 0.26H2/O2 0.0
• 0.5 Lpm Flow
Rate • 5% O2 (vol)
•Varying H2
•N2 Remainder
•0.7 s Residence Time (400 °C)
•800 ppmv PCE
Effects of H2/O2 ratio and T
• PCE conversion increases with both H2/O2 ratio and T.
• Under O2-only condition, PCE conversion does not take off until 350°C.
• Under redox condition, there is substantial conversion (≥ 50%) at relatively low temperatures (≥ 300°C).
• Optimum condition (PCE conversion ≥ 90%):
H2/O2 ≥ 2.2 and T ≥ 400 °C.
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In Figure 3's experiments, as long as H2/O2 > 1.2, PCE conversion is above 50% at just above 300C.
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We did experiments with H2/O2 ratios larger tahn 2.2. Results show that eventually at the operating T (400 C), the conversion remains the same as in H2/O2 = 2.2 case.
PCE Conversion ~ Catalyst Deactivation:Role of Reaction Condition!
T = 180°C T = 280°C T=380°C T = 450°C H2-only (6%) Conversion
decreased from 15% to zero in 30 min.
Conversion decreased from 98% to 38% in 1 h 50 min.
O2-only (5%) Conversion was ~ 30% for 4 h.
Conversion was ~ 30% for 4 h.
Redox (6% H 2, 3% O 2)
Conversion was steady at 67% for 5 h 30 min.
Conversion was steady at 72% for 2 h.
Conversion was steady at 84% for 30 h.
PCE = 800ppmv, Residence Time ~ 1.5 s (25 °C), ~ 0.7 s (400°C)
Catalyst Poisoning is Minimized by the Simultaneous Presence of H2 and O2
• Low-T (< 300 °C) conversions were mainly due to reduction.
• Declines in conv. (130 ~200 °C)
indicated poisoning;
• Recovery of conv. (> 200 °C): “self-cleaning” due to Redox!
• Conv. rose steadily (H2/O2≥2.2): heat prevents coke deposition and catalyst poisoning entirely!
0
10
20
30
40
50
60
70
80
90
100
75 125 175 225 275 325 375 425 475
Catalyst Surface Temperature (°C)
% PCE Conversion
a
H2/O2 = 2.2
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H2O/O2 reactions were not the primary cause, according to our experiments. The conversions at low T, from PCE/O2/H2O, were much lower than those in this figure.
Catalyst Surface T ~ Furnace T
0
50
100
150
200
250
300
350
400
450
500
0 100 200 300 400 500Furnace Temperature (°C)
Catalyst Surface Temperature (°C)
.
H2/O2 = 2.2
Homologous Alkanes as Alternative Reductants Replacing H2
Oxidation Reaction C-H Bond Dissociation
Energy (kJ/mol)
Methane CH4 + 2O2 CO2 + 2H2O 439.3 +/- 0.4
Ethane C2H6 + 3.5O2 2CO2 + 3H2O 420.5 +/- 1.3
Propane C3H8 + 5O2 3CO2 + 4H2O 410.5 +/- 2.9
n-Butane C4H10 + 6.5O2 4CO2 + 5H2O 400.4 +/- 2.9
* CRC Handbook of Chemistry & Physics, 86th edition (2005-2006)
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Obviously there are other reactions in addition to alkane oxidation. But following H2/O2, alkane/O2 is probably the main heat provider for the reaction system. And as we have seen before, the stoichiometric ratio of alkane/O2 is a good indicator of how much alkane we should use for optimum PCE conversion.
Experimental and Modeling Results of PCE Conversion under O2/alkane Conditions
Temperature (°C) vs Fraction of PCE Removed
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1
150 250 350 450 550 650 750
Temperature (°C)
Fraction of PCE Removed
Methane Model
Methane Experimental
Ethane Model
Ethane Experimental
Propane Model
Propane Experimental
Butane Model
Butane Experimental
175-200 ppm PCE
1 L/min total flow
Resid. Time ~ 0.5 sec
Assume first-order reaction rate with respect to PCE;
Assume activation energy is a linear function of alkane’s BDE;
Three-parameter fits eventually yield conversions reproducing experimental data reasonably well.
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Plug flow reactor.
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assume E(a) = aE(D) + b, assume there exist a and b applying to all alkanes, then k = k(0)exp(-(aE(D) + B)/RT).At each T, calculate k with a three-parameter fit (k(0), a, b) and compare with k from experim. When k(exp) and k(mod) have the least deviations (minimum square approach), the optimum parameters are found.Turns out this simple assumption can model the PCE conversion very well, meaning the BDE of alkane used in the reaction plays a major, even decisive. role in PCE reaction rate.
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Alkanes were at half the stoichiometric ratio to O2 (21%).
0.0%
10.0%
20.0%
30.0%
40.0%
50.0%
60.0%
70.0%
80.0%
340.0 360.0 380.0 400.0 420.0 440.0 460.0 480.0
Catalyst Temperature (0C)
PCE Conversion
a
0% C3H80.4% C3H80.6% C3H81.0% C3H8
• 1 Lpm Flow Rate • 5% O2 (vol)
•Varying Propane
•N2 Remainder
•0.25 s Resid. Time
•800 ppmv PCE
Lab (Redox): Use of Propane as Reductant
Field (Redox): Use of Propane as Reductant Park-Euclid Site, SBIR Phase I
Propane
SVE pump
Catalytic converters
Effluent stream
Heater control
Catalytic converters
Scrubber tower
Effluent stream
100 L/min through each reactor (3.5 cfm)100 L/min through each reactor (3.5 cfm)
300 L/min (10 cfm)300 L/min (10 cfm)
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Hydro Geo Chem Inc. in collaboration
• 2 Alumina supported Pt/Rh catalysts– 2" long x 4.7" major axis; 3.15" minor axis
(Siemens Water Technologies, Sept. 2006) $7/lb PCE absorbed (increaseincrease with [PCE])
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Propane consumption is independent of PCE concentration (always at 2% of total SVE gas volume). 2% propane is always in 1/2 stoichiometric ratio to O2 (1:10), optimum for conversion.Therefore, the higher PCE concentration is to be treated, the lower the cost/lb PCE is!
PCE Treatment Cost ~ Soil Vapor [PCE] (ppmv)
0.0
5.0
10.0
15.0
20.0
25.0
0 100 200 300 400 500 600 700
SVE PCE conc (ppmv)
PC
E t
rea
tme
nt
co
st
($/l
b)
Redox catalysis
GAC
Conclusions
• Redox catalysis is highly efficient in destroying chlorinated solvents at moderate temperatures.
• Catalyst activity can be maintained for extended periods using mild, convenient regeneration procedures.
• Alkanes can replace H2 as the reductant in the redox system for efficient removal of target compounds.
• PCE reaction rate appears to be directly related to the C-H bond dissociation energy of the alkane used.
• We achieved success in applying this method in a pilot field study.
• Redox catalysis holds potential for low-cost, large-scale field operation as an alternative remediation technology.
Future Work
• Lab– Further determine reaction mechanisms– Examine adsorption behaviors of reactants and products– Quantify reaction rates and model the processes– Optimize operating conditions
• Field– Carry out a larger-scale field project (Phoenix area)– Improved scrubber design; larger flow rates; other target
compounds (Freons)?
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So far from lab work, the best we have gleaned about the reaction mechanisms is that reduction steps probably precede oxidation ones and the importance of oxidation lies in its elimination of intermediates that would otherwise lead to rapid catalyst poisoning.
Acknowledgements
• National Institute of Environmental Health Sciences, NIH
• U of A Superfund Basic Research Program
Extra
Hydrodechlorination (reduction by H2) General Reaction Mechanisms
• Sequential/serial mechanism
H2 + 2 * ↔ 2 H*
RClx + * ↔ RClx*
RClx* + H* ↔ RHClx-1* + Cl*
RHClx-1* ↔ RHClx-1 + * (etc.)
H*+ Cl* ↔ HCl + 2 *
• Concerted/parallel mechanism
RClx* + x H*→ RHx + x Cl*
* refers to an active site on the catalyst surface; or an adsorbed species that is activated.
After displaying all Redox reactions possible, state that “it would seem to be a mess that we are in – ok, what reaction
happen, to what extent, and what converts to what…”
• Well, all this is under way to being fully understood through doing detailed and systematic experiments, but phenomenologically, we can focus on observing two things to meet our initial purposes, i.e.,