Abstract:
Advanced oxidation process namely ozonation and Fenton&#39;s (hydrogen peroxide/Fe: 2+ ) were utilized to degrade kinetic hydrate inhibitor (KHI). The oxidized solution after scavenging oxygen can be successfully disposed to the injection well. This facilitates use of KHI more frequently and in higher concentrations for future projects oil &amp; gas operations. It also offers an alternative that competes efficiently with thermodynamic hydrate inhibitor (THI) or complements THI.

Description:
CROSS-REFERENCE TO RELATED APPLICATIONS 
     This application is a non-provisional application which claims benefit under 35 USC §119(e) to U.S. Provisional Application Ser. No. 61/466,686 filed Mar. 23, 2011, entitled “ADVANCED OXIDATION OF KINETIC HYDRATE INHIBITORS,” which is incorporated herein in its entirety. 
     STATEMENT REGARDING FEDERALLY SPONSORED RESEARCH 
     None. 
     FIELD OF THE INVENTION 
     This invention relates to a process of treating process water, produced water and industrial waste water to remove contaminants including kinetic hydrate inhibitors (KHI). 
     BACKGROUND OF THE INVENTION 
     Treatment of water and disposal during the production of oil and gas can play a major role in the viability and cost of oil and gas projects. In many locations water is expensive or difficult to obtain. Water may have to be transported to the site or purchased in order to complete a project. Water used during the project is frequently reused as much as possible, and after production the water must be disposed of. In order to recycle or disposal of wastewater, contaminants in the water must be degraded, processed, and/or removed to ensure that the clean environment is not harmed and chemicals are not released. 
     Hydrates are crystalline solids that can be formed in a fluid whether the fluid is flowing or stationary. Hydrates form crystalline ice-like solids when water under the certain pressures and temperatures in the presence of low molecular weight hydrocarbon gases including methane, ethane, propane, butanes, pentanes, hexanes, H 2 S, CO 2 , and other small gases. Although hydrates are most problematic in fluids that are conveyed through pipe, they may form solid under a variety of conditions and block the surface of the pipe, which can lead to catastrophe. Hydrates can also be abrasive and deteriorate the pipe wall. Changes in pressure and temperature may cause hydrates to expand releasing explosive gases and increasing pressures to dangerous levels. There is a need, therefore, for improved and cost effective methods for inhibiting hydrate formation without permanently contaminating water produced or used during the production and transportation of hydrocarbons, including natural gas, crude oil, bitumen, tar sands, and other hydrocarbon sources. 
     There are two broad techniques to control hydrate formation in hydrocarbons, namely thermodynamic and kinetic inhibitors. Thermodynamic inhibitors include water removal, increasing temperature, decreasing pressure, addition of “antifreeze” to the fluid and combinations of these methods. The kinetic approach generally prevents/delays the smaller hydrocarbon hydrate crystals from agglomerating into larger ones (known in the industry as an anti-agglomerate and abbreviated AA), they also may inhibit, retard and prevent initial hydrocarbon hydrate crystal nucleation or crystal growth (known in the industry as a kinetic hydrate inhibitor and abbreviated KHI). Additionally, films that protect the inside of the pipelines, tubing, valves and such prevent both hydrate crystallization and corrosion of the materials. Thermodynamic inhibitors, kinetic hydrate inhibitors and anti-agglomerate were used to reduce or prevent hydrate formation. 
     In U.S. Pat. No. 6,646,082 and US2003063998, Ghosh, used oligomeric and polymeric compositions as fluid additives in aqueous systems which are effective corrosion inhibitors over a wide range of pH and render metals passive to repeated attack by oxidants and oxidizing biocides. Dahlman, U.S. Pat. No. 7,435,845, and Leinweber, U.S. Pat. No. 7,615,102, replace hazardous thermodynamic hydrate inhibitors with corrosion inhibitors and gas hydrate inhibitors having improved film persistence and good biodegradability. Talley and Colle, US20080312478, discovered the synergistic effects of the thermodynamic hydrate inhibitors and kinetic hydrate inhibitors are additive and therefore, significantly reduce hydrate formation in a fluid. 
     Ozonation has been shown to effectively remove surfactants, biological contaminants, and other materials from wastewater for municipal and commercial production services (Klasson et al, 2002). Suzuki and associates (1976 a&amp;b) found  P. aeruginosa  PEG-K utilized ethylene glycol, diethylene glycol, and triethylene glycol produced by ozone degradation of high molecular PEG followed by treatment with H 2 O 2 . Narkis and associates (Narkis and Schneider-Rotel, 1980; Narkis and Schneider-Rotel, 1985; Narkis, et al. 1987) improved biodegradability of non-ionic surfactants caused by ozonation through changes in molecular structure. Delanghe, et al., (1991) reviewed the aqueous ozonation reactions of surfactants including the degree of reaction and ozonation byproduct identity. Homg, et al., (1998) investigated surfactant wastewater treatment by electro-chemical oxidation with or without hydrogen peroxide. Da Pozzo, et al., (2005) described electro-Fenton treatment of a solution containing phosphorus compounds using graphite electrodes. Urbans, (2006) describes the use of peroxide as a water treatment method. Agladze, et al., (2007) optimized cell design and current efficiencies for cathodic reduction of oxygen at gas-diffusion electrodes in membrane cells. Peralta-Hernández, et al., (2009) summarize and analyze the results of electro-Fenton (EF) and photoelectro-Fenton (PEF) methods. Petrucci, et al., (2009) presented enhancement of electro-Fenton treatment, performed by employing a PTFE-bonded gas diffusion cathode. Rosales, et al., (2009) describes the use of the electro-Fenton process to clean soil or clay contaminated by organic compounds. Brillas provides an overview of current oxidation technologies (Oturan and Brillas, 2009; Brillas, 2009; Oturan, et al., 2009). Unfortunately, waste water produced from natural gas, SAGD, LNG, and other hydrocarbon processes contains contaminants not present in other commercial processes. Additionally, KHI materials are becoming more complex, KHI concentrations are increasing, and there is a greater volume of produced water, so systems used to process KHI containing water must work more rapidly on a larger scale than previously available. Processes that involve heating, incineration or other attempts simply produce more waste, use more equipment, or are too expensive to be implemented at the variety of hydrocarbon processing locations around the world under a variety of different environmental conditions. 
     An efficient KHI removal process is required not only to remove KHI in production and transportations systems today, but that will allow production from more extreme areas, such as deep water and arctic reservoirs where increased pressures and lower temperatures will contribute to hydrate formation. Improved KHI removal will allow higher concentrations of KHI to be used in these more extreme environments. Additionally, KHIs may be used in systems with other more complex contaminants. An efficient and inexpensive method of KHI removal must be developed to remove kinetic hydrate inhibitors from wastewater and process water that allows the water to be either re-injected into the subterranean formation or further processed without producing solid wastes and/or generating toxic by-products that are difficult to dispose of or damaging to the environment. 
     BRIEF SUMMARY OF THE DISCLOSURE 
     A robust oxidation system is desired that degrades significant amounts of KHI at lower temperatures, because oxidations reactions improve with increasing temperatures, produced water with KHI will be readily oxidized at higher temperatures if the reaction functions well at low temperatures. Processing the KHI containing solutions at produced water temperature without heating or cooling, reduces the cost of processing, decreases the amount of equipment required, and provides a smaller footprint within the limited confines of the production area. 
     The invention more particularly includes a process for treating kinetic hydrate inhibitor contaminated solutions by mixing one or more kinetic hydrate inhibitor (KHI) containing aqueous solutions with a KHI degrading oxygen containing molecule, including Fenton&#39;s Process (adding hydrogen peroxide then adding iron (Fe2+)) and/or bubbling with ozone; separating precipitates from the KHI degraded solution; and obtaining clean water. 
     In another embodiment, a process for treating KHI contaminated solutions is described where one or more KHI containing aqueous solutions is mixed with Fenton&#39;s solution (adding hydrogen peroxide then adding iron (Fe2+)), separating precipitates from the KHI degraded solution; and obtaining clean water. 
     Additionally, a process for treating KHI contaminated solutions is described where one or more KHI containing aqueous solutions is bubbled with ozone; and clean water is obtained. 
     The processes may be conducted in a tank, sediment pond, or other water storage container. The process may use one or more columns in a continuous process. The process may include ozonation and Fenton&#39;s process simultaneously. The process may include ozonation followed by Fenton&#39;s process. The process may include Fenton&#39;s process followed by ozonation. 
     One or more KHIs may include vinyl caprolactam, ester amides, polyester pyroglutamate, N-acylalkylene imines, 2-alkyl-2-oxazolines, PMeOx, PEtOx, PnPrOx, PiBuOx, PnBuOx, N-vinyl-N-methyl acetamide, vinylpyrrolidone, PVP, tetrabutylammonium bromide, PDMAEMA, homopolymers, copolymers, linear, branched, highly branched monomers, polymers and mixed polymers thereof. Oxygenated KHIs may include a highly branched methoxylate, ethoxylate, propoxylate, butoxylate, pentoxylate, hexoxylate, carboxylate, ester, or other oxygenated KHI. 
    
    
     
       BRIEF DESCRIPTION OF THE DRAWINGS 
       A more complete understanding of the present invention and benefits thereof may be acquired by referring to the follow description taken in conjunction with the accompanying drawings in which: 
         FIG. 1 : Ozone Bubble column system.  FIG. 1A  is a diagram of an ozone bubble column for KHI removal,  FIG. 1B  is the schematics of the ozone bubble column showing the ozone generator, feed ozone detector, bubble column, dehumidifier, off gas ozone detector and heated catalyst. 
         FIG. 2 : Degradation of KHI in field Brine:  FIG. 2A  demonstrates KHI oxidation of field brine by ozone as function of time.  FIG. 2B  demonstrates relative KHI concentration of field brine by ozonation as function of time. 
         FIG. 3 : Oxidation and Cloud Point of 1.5% KHI solutions in synthetic brine. (1.5%)  FIG. 3A  demonstrate KHI oxidation and cloud point as function of time.  FIG. 3B  demonstrates relative KHI concentration of synthetic brine by ozonation as function of time. 
         FIG. 4 : Fenton&#39;s Process. 
         FIG. 5 : Ozone degradation of KHI. 
         FIG. 6 : KHI Oxidation at pH 3.5 and pH 9.0.  FIG. 6A  demonstrates KHI oxidation in synthetic brine by ozone at pH 3.5 and pH 9.0.  FIG. 6B  demonstrates relative KHI concentration during the ozonation at pH 3.5 and pH 9.0. 
         FIG. 7 : Simultaneous ozonation and Fenton process treatment. 
         FIG. 8 : Sequential ozonation then Fenton process treatment. 
         FIG. 9 : Sequential Fenton process treatment then ozonation. 
         FIG. 10 : Ozone contactors including (A) a baffled chamber diffuser, (B) a turbine diffuser contactor, and (C) a side stream ozone system. 
     
    
    
     DETAILED DESCRIPTION 
     Turning now to the detailed description of the preferred arrangement or arrangements of the present invention, it should be understood that the inventive features and concepts may be manifested in other arrangements and that the scope of the invention is not limited to the embodiments described or illustrated. The scope of the invention is intended only to be limited by the scope of the claims that follow. 
     Abbreviations include: kinetic hydrate inhibitor (KHI); thermal hydrate inhibitor (THI); low dosage hydrate inhibitor (LDHI); normal liters per minute (Nit/min); grams per normal cubic meter (g/Nm 3 ); parts per million (ppm); monoethylene glycol (MEG), diethylene glycol (DEG), triethylene glycol (TEG), poly(2-methyl-2-oxazoline) (PMeOx); poly(2-ethyl-2-oxazoline) (PEtOx); poly(2-n-propyl-2-oxazoline) (PnPrOx); poly(2-isobutyl-2-oxazoline) (PiBuOx); poly(2-n-butyl-2-oxazoline) (PnBuOx); poly-N-vinylcaprolactam (PVCap); polydimethylaminoethylmethacrylate (PDMAEMA); poly vinylpyrrolidone (PVP); high pressure liquid chromatography (HPLC); advanced oxidation processes (AOPs), and wet humid oxidation process (OHP®). 
     As used herein, hydrocarbons may include natural gas, petroleum, crude oil, bitumen, tarsands, pitch, and other hydrocarbon containing materials as well as processed hydrocarbon materials including methane, ethane, butane, LNG, syngas, gasoline, fuel oil, diesel, kerosene, and the like. Hydrocarbons being recovered, processed and transported may have KHIs added to prevent hydrate formation. 
     Hydrates, as used herein, refers to ice-like structures in which water molecules, under pressure, form structures composed of polyhedral cages surrounding “guest” molecules including salts, methane, ethane or other molecules. 
     Kinetic hydrate inhibitors (KHIs) include, but are not limited to: vinyl caprolactam, ester amides, polyester pyroglutamate, N-acylalkylene imines, 2-alkyl-2-oxazolines including PMeOx, PEtOx, PnPrOx, PiBuOx, PnBuOx and the like; N-vinyl-N-methyl acetamide; vinylpyrrolidone; PVP; tetrabutylammonium bromide; PDMAEMA; as well as homopolymers, copolymers, and mixed polymers thereof, including linear, branched and highly branched monomers and polymers. Proprietary KHIs are available from NALCO®, and include FREEFLOW® LDHI, among others. 
     Thermodynamic inhibitors (THIs) include methanol, ethanol, glycol, ethylene glycol, MEG, DEG, TEG, salts, NaCl, CaCl 2 , KCl, and the like. 
     Oxidants for KHI degradation include ozone, Fenton process, OHP® process, ClO 2 , peroxide, and other oxidants weak or strong depending upon the application and concentration of KHI to be removed. Oxidants may be used individually, in series, or during the same oxidation reaction if applicable. Ozone and chlorine dioxide have the highest oxidation potential as shown in Table 1. Ozone and chlorine dioxide produce hydroxyl radicals, whereas Fenton process requires Fe ion to react with hydrogen peroxide at pH 3-5 to produce hydroxyl radicals. Other oxidizers are available that may be adapted to one or more processes. Selection of oxidizing agent will depend upon the kinetic inhibitors used and the concentration of the kinetic inhibitors. Additionally, oxidation can be improved in the presence of electrolysis, sonic cavitation, or other processes. In one example the OzoNix® system which uses cavitation to increase solution temperature during cavitation using electrolysis and sonic cavitation. 
     
       
         
               
             
               
               
               
             
           
               
                 TABLE 1 
               
             
             
               
                   
               
               
                 Oxidation Potential 
               
             
          
           
               
                   
                 Oxidizing agent 
                 Oxidation potential 
               
               
                   
                   
               
               
                   
                 Fluoride 
                 3.06 V 
               
               
                   
                 Hydroxyl radical OH −   
                 2.80 V 
               
               
                   
                 Atomic Oxygen 
                 2.42 V 
               
               
                   
                 Ozone 
                 2.07 V 
               
               
                   
                 Hydrogen peroxide 
                 1.77 V 
               
               
                   
                 Permagnate Ion 
                 1.67 V 
               
               
                   
                 Chlorine di oxide 
                 1.50 V 
               
               
                   
                 Chlorine 
                 1.36 V 
               
               
                   
                   
               
             
          
         
       
     
     Brine solution may be any aqueous solution with a mixture of salts, including inorganic salts such as carbonates and sulfates of various metals, i.e. calcium, strontium and barium as well as complex salts of iron such as sulfides, hydrous oxides and carbonates. Although salt compositions may vary, some typical ions dissolved in brine include sodium (Na), potassium (K), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), iron (Fe), chloride (Cl), bromide (Br), sulfate (SO 4 ), bicarbonate (CO 3 ). Brines from a variety of locations, including various production wells and ocean water are shown in Table 2. Brine solution composition will vary greatly dependent upon the reservoir being produced and the treatment being applied to the reservoir, additionally conditions will vary over time. 
     
       
         
               
             
               
               
               
               
               
               
               
               
               
               
             
               
               
               
               
               
               
               
               
               
               
             
           
               
                 TABLE 2 
               
             
             
               
                   
               
               
                 A variety of Brine Solutions 
               
             
          
           
               
                   
                   
                   
                   
                   
                   
                 Prudhoe 
                 North 
                 BRINE 
                 BRINE 
               
               
                 ION 
                 Well 1 
                 Well 2 
                 Well 3 
                 Well 4 
                 Well 5 
                 Bay 
                 Sea 
                 “A” 
                 “E” 
               
               
                   
               
             
          
           
               
                 Sodium 
                 7805 
                 29370 
                 56723 
                 28100 
                 52225 
                 8000 
                 11010 
                 72000 
                 81600 
               
               
                 Potassium 
                 200 
                 372 
                 1525 
                 1630 
                 3507 
                 83 
                 460 
                 6300 
                 8000 
               
               
                 Magnesium 
                 25 
                 504 
                 1250 
                 113 
                 2249 
                 84 
                 1368 
                 4000 
                 2500 
               
               
                 Calcium 
                 70 
                 2808 
                 16075 
                 615 
                 34675 
                 180 
                 428 
                 48000 
                 20000 
               
               
                 Strontium 
                 20 
                 574 
                 938 
                 65 
                 1157 
                 24 
                 8 
                 1000 
                 2000 
               
               
                 Barium 
                 70 
                 252 
                 23 
                 770 
                 91 
                 4 
                 &lt;1 
                 1200 
                 3700 
               
               
                 Iron 
                 &lt;1 
                 &lt;1 
                 60 
                 &lt;1 
                 107 
                 — 
                 &lt;1 
                 — 
                 — 
               
               
                 Chloride 
                 11500 
                 52360 
                 121600 
                 46050 
                 153025 
                 11500 
                 19700 
                 21000 
                 174000 
               
               
                 Sulfate 
                 0 
                 11 
                 220 
                 4 
                 44 
                 10 
                 2960 
                 0 
                 0 
               
               
                 Bicarbonate 
                 1650 
                 496 
                 100-300 
                 1655 
                 134 
                 2222 
                 124 
                 — 
                 — 
               
               
                 Total 
                 21350 
                 86747 
                 198614 
                 79003 
                 247214 
                 22107 
                 36058 
                 N/A 
                 N/A 
               
               
                 Dissolved 
               
               
                 Solids 
               
               
                 Ionic 
                 0.359 
                 1.58 
                 3.90 
                 1.35 
                 5.28 
                   
                 0.712 
               
               
                 Strength 
               
               
                   
               
             
          
         
       
     
     As used herein a diffuser is used to ensure contact time between the KHI in solution and the ozone or other gases applied to the solution. Diffusers may include baffled chamber diffusers, turbine diffusers, side stream ozone contactor, and other diffusers some of which are shown in  FIG. 10 . In one embodiment, baffled chamber diffusers are designed to degrade KHI at a rate sufficient to remove all of the KHI even at or above capacity. The number of chambers, the geometry, the diffuser systems, and operation may be adjusted to degrade KHI at an appropriate rate. In one example, the ozone contactor has several compartments in series with bubble diffusers at the bottom. In the first compartment the water flows downward against the rising bubbles, and in the second compartment the water flows upward. The chambers are covered to prevent the escape of ozone and to increase the partial pressure of the ozone in the contactor. Additional chambers follow to guarantee a contact time between the ozone and the water. Each of the chambers has sampling ports so that the ozone concentration in each chamber can be determined. This is needed to calculate the product of concentration and retention time required to ensure contact time value. 
     In one embodiment, a synthetic brine was prepared by dissolving 1.68 g NaCl, 5.475 g CaCl.2H 2 O, 3.120 g MgCl 2 .5H 2 O, 19.5 ml of 0.1 M KCl, 0.111 g Na 2 SO 4 , 0.135 g NH 4 Cl, 0.1125 g SrCl 2 .6H 2 O and 1.2 g NaC 2 H 3 O 2  (Sodium Acetate) per 1.5 liters total of aqueous solution. The solution was adjusted to pH 9.0. In another embodiment, commercial brine from ADMA-OPCO is available with the following ionic concentrations: 3,300 mg/L Cl − , 350 mg/ml acetate, 50 mg/L SO 4   −2 , 10 mg/L Br − , 600 mg/L Na + , 50 mg/L K + , 250 mg/L Mg +2 , 1000 mg/L Ca +2 , 30 mg/L NH 4   + , and 25 mg/L Sr +2 . Although this example uses multiple salts in various concentrations, brine solutions may contain only one type of salt, i.e. a sodium chloride brine or potassium sulfate brine for example. In another embodiment, the brine concentration varies as the water is produced and may be adjusted to achieve a specific ionic strength by adding de-ionized water, fresh water, or purified water to reduce ionic strength; or by adding recycled water, salts, or other additives to increase ionic strength. The pH may also be monitored as it will fluctuate during production and may be adjusted by adding buffer, acid or base as appropriate. 
     Normal conditions are 0° C. and 1 atm pressure unless otherwise stated. The temperature may change during production and processing and may vary depending upon the type of production, the location of the water and the stage of water production. Waste water produced during transportation, i.e. to and from the wellhead or platform may be at 0-4° C. Water produced to and from various LNG processes may be at or below 0° C. and may even go down to about −40° C. or lower dependent upon the pressures and salt concentrations, while water produced during distillation processes may be at or near boiling. Similarly, wastewater from a SAGD production may be at or near boiling while wastewater produced from offshore marine platforms may be at or near 0° C. Pressure may also vary and is completely dependent upon the conditions under which the water is produced, although the wastewater or production water can be brought to atmospheric pressure for processing. 
     Ozonation equipment demonstrated in  FIG. 1A  and as show in detail in  FIG. 1B , includes an oxygen source, an oxygen flow meter (i.e. an MMF oxygen flow meter), an ozone generator (i.e. a BMT ozone generator), an inlet ozone detector (i.e. a BMT 964 2bara ozone detector), a bubble column, a dehumidifier, an outlet ozone detector (i.e. a BMT 964 2bara ozone detector), and a heated catalyst to break down any excess ozone and other by-products. 
     A variety of oxygen flow meters are available from a variety of commercial sources. The MMF flow meter described above is available from DWYER® Instruments, Dakota Mass, PVL, Fox Instruments, and many other commercial suppliers. The oxygen flow meter may measure oxygen content, temperature, flow rate, and other parameters depending upon the model and rate of oxygen flow. 
     The ozone generator is selected to produce above a minimum level of ozone required per hour and ozone generation is monitored using an ozone detector that can measure at a minimum ozone concentration. Numerous ozone generators and detectors are available from BMT Messtechnik GmbH, Berlin, Germany. Ozone generators are also commercially available from Ozone Generator USA,  O 3 OZONE  Generators, DEL® Ozone Generators, PROZONE® Commercial Systems, and other commercial sources. Ozone detectors are available from BMT, ChemLogic, IN USA, Inc., as well as other ozone analyzers including various UV/Vis systems. Numerous chemistry suppliers can provide commercial or custom made column bubblers including those available from P YREX ®, C HEMGLASS ®, VWR Labshop, N OVA T ECH ® International, and other suppliers. A bubble column may also be assembled from one or more columns, including mixing columns with filters at the base and/or along the length of the column. In one embodiment a supply tube is placed below a borosilicate frit at the base of a 1 liter column, ozone is bubbled through the frit into the treated solution. A frit at the top of the column prevents foaming solution from escaping the top of the column and entering the gas outlet to the dehumidifier. 
     Mixing may be achieved by bubbling, with paddles or mixers, by pumping, or by aeration with ozone, air, or other gas. The reaction processes described herein may be conducted in a column, mixing column, reactor, tank, mixing tank, storage tank, storage pond, or other means of storage used in the industry for water, wastewater or production water. Where applicable, reactions may be carried out in batch, semi-batch processes, or continuous operations depending upon the amount of aqueous solution, concentration of hydrate inhibitor, and strength of oxidant used. Mixing may be achieved in one or more column and columns may be assembled in series with multiple ozonation columns each with a unique concentration of ozone. 
     The following examples of certain embodiments of the invention are given. Each example is provided by way of explanation of the invention, one of many embodiments of the invention, and the following examples should not be read to limit, or define, the scope of the invention. 
     Example 1 
     Ozonation 
     Ozonation can remove up to 94% of the KHI present in wastewater ( FIG. 5 ). In one embodiment KHI was removed from a mixed brine solution containing 1.5% KHI by bubbling ozone through the solution. A synthetic brine solution was made with 1.5% KHI, a hyper branched polymer with ethoxy functional group The solution contained 2.2715 g NaCl, 7.3128 g CaCl 2 .2H 2 O, 4.1762 g MgCl 2 .6H 2 O, 26.0295 g of 0.1M KCl, 0.1493 NaSO 4 , 0.1800 g NH 4 Cl; 0.1591 g SrCl 2 .6H 2 O, 1.6081 g NaC 2 H 3 O 2 , and 30.0117 g of hyper branched KHI, pH was adjusted to 8.83 in 2 L aqueous solution. This synthetic brine is similar to brine separated from sludge catcher of crude oil/LNG production at several facilities. 
     Ozonation was first run through the synthetic brine without KHI as previously described. 1 liter of water with oxygen flow at 0.4 lt/min was run through an ozone bubbling column (see  FIG. 1 ) with DI water. Inlet ozone was approximately 194.9 gN/m 3  to 195.1 g/Nm 3  and the outlet ozone concentration was monitored with time to reach steady state value. The residual ozone concentration in water changes with temperature. It was found around 20 ppm 
     Next, ozone was bubbled through synthetic brine with 1.5% KHI at 0.07 lt/min. Inlet ozone concentration was approximately 183.4 gN/m 3  and outlet ozone concentration varied time. The experiment was carried for more than 4 hours until a steady state outlet concentration was achieved. Initial and final KHI concentration were around 16,000 mg/l and 285 mg/l, which reflected 96-98% removal. 
     Field brine was obtained from a crude oil production. The brine was spiked with KHI to a final concentration of 1.5% KHI. The brine pH with KHI addition was about pH 4.1. 250 ml of KHI spiked brine was bubbled for 3.5 hours with 0.07 NIt/min oxygen, inlet ozone concentration and ozone mass flow rate were 180 g/Nm 3  and 0.73 g/h respectively. Samples were taken at 15, 30, 45, 60, 90, 120, 150, 180 and 210 minutes (see  FIGS. 2A  and B). KHI concentration decreased from 16,787 mg/l initially to 3564 mg/L after ozone treatment. The solution pH decreased from pH 4.1 to 2.2. This demonstrates that ozonation can remove 78% of the KHI from field brine. 
     This batch system of degrading KHI in a concentrated brine solution demonstrates that ozone can sufficiently degrade KHI and the treated brine may then be re-injected into the well or be used in other applications. 
     In another embodiment, a solution of 1.5% KHI in OPCO Brine at a pH of 3.6 was bubbled with ozone for 4 hours. Over 80% of the KHI in solution was degraded and cloud point was reduced dramatically. A total volume of 250 ml of 1.5% KHI was bubbled with ozone at 0.07 NIt/min. The average inlet ozone concentration after 12 minutes was 180 g/Nm3 (gas phase). The system at this scale was exposed to an ozone dosage of 0.73 g/h. 3 ml samples were taken at 15, 30 and 45 minutes after the start up of the experiment and 10 ml samples were taken at 60, 90, 120, 150, 180, 210 and 240 minutes for cloud point analysis. After 240 minutes, the solution was purged with oxygen to remove the remaining ozone gas. 
     
       
         
               
             
               
               
               
               
             
               
               
               
               
             
           
               
                 TABLE 3 
               
             
             
               
                   
               
               
                 Ozonation of 1.5% KHI in OPCO brine. 
               
             
          
           
               
                   
                 Cloud Point Temp 
                 KHI Conc. 
                   
               
               
                 Sample 
                 (° C.) 
                 (mg/ml) 
                 KHI Oxidized (%) 
               
               
                   
               
             
          
           
               
                 Initial 
                 37 
                 14943 
                   
               
               
                 Final 
                 64 
                 2532 
                 83% 
               
               
                   
               
             
          
         
       
     
     As shown in Table 3 and  FIGS. 3A  &amp; B, ozonation degraded 1.5% KHI reducing KHI concentration by up to 83% and increasing cloud point temperature to approximately 65° C. Feed and treated samples were centrifuged at 2000 rpm for 30 minutes; the supernatant was filtered through a 0.45 μm filter, and cloud point of the supernatant measured (note that any initial haziness was removed by centrifugation). The supernatant solution was heated up to 64° C., haziness was observed, the solution never became opaque, even at temperatures above 75° C. KHI solutions with higher cloud points dramatically reduces pore plugging in deep reservoir as well as prevent scaling and fouling of equipment used for additional processing. 
     Example 2 
     pH Effects 
     Synthetic brine was mixed with KHI to produce an initial solution with 0.25% KHI (mixed for at least one hour). The pH in two separate brine solutions was adjusted to pH 3.5 and pH 9.0. 
     Ozone was bubbled for one hour with the following parameters: 250 ml of synthetic brine with 0.25% KHI, mixed for greater than one hour, was treated by ozonation with an oxygen flow rate of 0.075 Nit/min, 4.5 PSI, generating 180 gN/m 3  ozone at the inlet with ozone mass flow rate of 0.78 g/h ozonation. Samples (4 ml) were taken at 5, 10, 20, 30, 45 and 60 minutes. After 60 minutes, the solution was purged with oxygen to remove the remaining ozone gas. 
     synthetic brine with 0.25% KHI at pH 3.5 had 2524 mg/L KHI and an initial cloud point of 42° C. and was completely opaque at 53° C. OPCO Brine with 0.25% KHI at pH 9.0 had 2431 mg/L KHI and an initial cloud point of 42° C. and was completely opaque at 53° C. After bubbling in ozone for 60 minutes, the solutions had dramatic reductions in the total KHI concentration. The pH 3.5 solution had a final KHI concentration of 782 mg/L KHI, an approximately 69% drop in KHI concentration. The pH 9.0 solutions had a final KHI concentration of 517 mg/L KHI, an approximately 79% drop in KHI concentration. The ozonated KHI solutions, both pH 3.5 and pH 9.0, were heated over 80° C., but did not cloud significantly. The solutions were never opaque. 
     Example 3 
     Fenton Process 
     The Fenton process was conducted by mixing hydrogen peroxide (H 2 O 2 ) with the KHI solution and adding ammonium ferrous sulfate hexahydrate (NH 4 FeSO 4 .6H 2 O). Mixing the H 2 O 2  with NH 4 FeSO 4 .6H 2 O releases oxygen radicals producing hydroxyl ions and hydroxyl radicals, that may then react with reactive groups in the KHI ( FIG. 4 ). In one embodiment, a 0.25% KHI brine solution was treated using the Fenton Process to remove KHI. In a 500 ml volumetric flask, 100 ml concentrated 5 fold concentrated synthetic brine was mixed with 100 ml of 12.5 mg/ml KHI for 1 hour. Next, 157 ml of 6% H2O2 was added along with 100 ml 66.3 mg/ml NH 4 FeSO 4 .6H2O. The flask was filled to 500 ml with deionized water for a final volume of 500 ml. After stirring, the solution was allowed to settle. The solution color goes from transparent to light orange to opaque dark orange. After several hours, the iron oxides precipitated to the bottom of the flask and the solution returned to a transparent light orange color. The clarified solution had a KHI concentration of 401 mg/L. This process resulted in approximately 84% KHI removal. 
     Example 4 
     Fenton Process and Ozonation 
     Several individual processes were shown to remove a majority of the KHI from a simulated wastewater stream. Individually, ozonation or the Fenton process could remove up to 95% of the KHI from a 0.25% KHI Brine solution. This is sufficient in most cases to either re-inject the water solution or use the water for other processes. If the water must be further processed or if the KHI concentrations are higher due to extreme conditions, the processes may be used simultaneously or sequentially to achieve degradation of more KHI. Additionally, a method is developed to incorporate KHI removal in a continuous process. In  FIG. 7 , KHI is treated with ozonation and the Fenton process simultaneously. A wastewater stream containing KHI is mixed with concentrated H 2 O 2  and fed into a column (either vertical or horizontal), an iron (Fe 2− ) containing solution is added either at the top of the column or at intervals along the column then ozone may be added either at the top of the column or along the length of the column, clean water is centrifuged, filtered or otherwise separated from the iron precipitate, to generate purified water for re-injection or other use. If the column is vertical, KHI containing wastewater mixed with concentrated peroxide may be fed into the top of the column with an iron (Fe 2+ ) containing solution and ozone bubbled from the bottom of the column. After the process is complete, the waste is centrifuged to remove precipitates. 
     The processes may also be run in series where the KHI contaminated brine is treated with ozonation then the Fenton Process. The process may be conducted vertically with the ozone and brine fed at one end of the column and gases removed from the other. Alternatively, as shown in  FIG. 8 , the KHI contaminated water is fed into the top of a bubble column and ozone is fed from the bottom. As the KHI contaminated water flows down the column, the ozone concentration will increase and the KHI concentration decrease, thus producing treated water at the end of the column. Column flow rate is dictated by the initial concentration of KHI, rate of ozone production, length of the bubble column, and final concentration of KHI desired. In one embodiment, the water from the treated column may then mixed with peroxide and fed with iron (Fe2+) into an adjacent column. After sufficient reaction time, the clean water is centrifuged or filtered to remove particulates and the clean water is produced. 
     The process may also be run where the KHI contaminated brine is treated by the Fenton process then ozonation. A sequential process is shown in  FIG. 9 , with Fenton Process and then Ozonation occurring in adjacent columns. Centrifugation may be done after a Fenton process or after ozonation, dependent upon reactor design and the amount of precipitate produced during the Fenton process. Although “columns” are used to demonstrate the process these columns may be any diffuser, mixer or contact system including baffle diffusers, turbine diffusers, a side stream contactor with Fenton&#39;s reagents, ozonation, wet oxidation or other AOP fed at the beginning of the diffuser/mixer or along the length of the diffuser/mixer. Alternatively, Fenton&#39;s process and ozonation may be carried out in one or more columns, diffusers, tanks, batch fed tanks, including sedimentation tanks or ponds, to achieve a similar level of water treatment. 
     In one embodiment Fenton&#39;s process is conducted in a sedimentation tank containing KHI contaminated brine. A peroxide solution is added to achieve approximately 7.5:1 molar ratio of peroxide to KHI. After stirring or mixing to achieve a uniform distribution an iron (Fe 2+ ) solution is added to achieve a 1:10 ratio for iron to peroxide. The solution is again mixed to achieve a uniform distribution. The solution is allowed to settle before ozone is bubbled in the tank. Once sufficient KHI has been degraded the clean water is removed and the process is repeated. When excess precipitate builds up, the precipitate can be removed and either recycled, sold as raw ferric oxide, or otherwise disposed of. The process may be done at atmospheric pressure and ambient temperature, or the container may be closed and pressurized to prevent bubbling during ozonation. Additionally, an anti-foaming agent may be added to reduce or prevent foaming. 
     Experimental results have proven large amount of KHI can be degraded using either an ozonation or Fenton process. Cloud point determination demonstrated that clean water is produced that can be either re-injected or used for other processes. This technology can be used to clean large quantities of produced water from a variety of processes where KHI can be used to prevent or slow hydrate formation. This is essential as production and transportation of crude oil, bitumen, tar sands, LNG, and other petrochemicals move to more difficult environments that increase the chance of hydrate formation, hydrate inhibitors will be used more frequently at higher concentrations. KHI inhibitors become more viable and less problematic now that this disposal system, using ozonation, Fenton&#39;s process, or combinations to remove KHI. Preventing hydrates is essential to prevent clogging with hydrates and to prevent dangerous gas pressure fluctuations caused by rapid hydrate dissociation. 
     Example 5 
     Pilot Scale and Full Scale Production Process 
     In another embodiment, the process may be used to process produced water from a subterranean formation. Rates and conditions vary from formation to formation and the oxidation process may be scaled to a variety of production rates as shown in Table 4. 
     
       
         
               
             
               
               
             
               
               
               
               
               
               
               
               
             
               
               
               
               
               
               
               
               
             
           
               
                 TABLE 4 
               
             
             
               
                   
               
               
                 Production flow rate and ozone requirement. 
               
             
          
           
               
                   
                 Flow Rate (m 3 /hr) 
               
             
          
           
               
                   
                 5 
                 10 
                 20 
                 30 
                 50 
                 75 
                 100 
               
               
                   
                   
               
             
          
           
               
                 KHI (kg/d) 
                 1800 
                 3600 
                 7200 
                 10800 
                 18000 
                 27000 
                 36000 
               
               
                 Ozone use 
                 1025 
                 2049 
                 4099 
                 6148 
                 10247 
                 15370 
                 20493 
               
               
                 (kg/d) 
               
               
                   
               
             
          
         
       
     
     Although scaling may be accomplished by simply increasing contact time with additional ozone, other methods of increasing contact time include increasing the size and length of the diffuser, increasing the number of diffusers, and adding one or more additional oxidizing agents. In one embodiment ClO 2  is added prior to ozonation in a diffuser or column. 
     In closing, it should be noted that the discussion of any reference is not an admission that it is prior art to the present invention, especially any reference that may have a publication date after the priority date of this application. At the same time, each and every claim below is hereby incorporated into this detailed description or specification as additional embodiments of the present invention. 
     Although the systems and processes described herein have been described in detail, it should be understood that various changes, substitutions, and alterations can be made without departing from the spirit and scope of the invention as defined by the following claims. Those skilled in the art may be able to study the preferred embodiments and identify other ways to practice the invention that are not exactly as described herein. It is the intent of the inventors that variations and equivalents of the invention are within the scope of the claims while the description, abstract and drawings are not to be used to limit the scope of the invention. The invention is specifically intended to be as broad as the claims below and their equivalents. 
     REFERENCES 
     All of the references cited herein are expressly incorporated by reference. The discussion of any reference is not an admission that it is prior art to the present invention, especially any reference that may have a publication date after the priority date of this application. Incorporated references are listed again here for convenience:
     1. U.S. Pat. No. 6,646,082, US2003065116, “Rohm &amp; Haas (Ghosh) Priority: Sep. 4, 2001.   2. U.S. Pat. No. 7,435,845, US2005101495, “Corrosion and gas hydrate inhibitors having improved water solubility and increased biodegradability” Clariant (Dahlman) Priority: Feb. 24, 2003.   3. U.S. Pat. No. 7,615,102, US20090173663, WO2006040013, Clariant (Leinweber), Priority: Oct. 7, 2004.   4. US2003063998, Rohm &amp; Haas (Ghosh), Priority: Sep. 4, 2001   5. US20080312478, WO2006110192, Exxonmobil Upstream Research Co. (Talley), Priority: Apr. 7, 2005.   6. US 20090173663 “Corrosion and gas hydrate inhibitors with an increased biological degradability and a reduced toxicity” (2009).   7. “Peroxone (Ozone/Hydrogen Peroxide),” EPA Guidance Manual Alternative Disinfectants and Oxidants (1999).   8. Agladze, et al., “Comparative study of hydrogen peroxide electro-generation on gas-diffusion electrodes in undivided and membrane cells.” J. Appl. Ellectrochem. 37:375-83 (2007).   9. Benner and Terner, “Ozonation of Propranolol: Formation of Oxidation products,” Environmental Science Technology 43:5086-93 (2009).   10. Brillas, et al., “Electro-Fenton Process and Related Electrochemical Technologies Based on Fenton&#39;s Reaction Chemistry.” Chem. Rev. 109:6570-631 (2009).   11. Da Pozzo, et al., “Oxidation efficiency in the electro-Fenton process.” J. Appl. Electrochem. 35:391-8 (2005).   12. Delanghe, et al., “Aqueous Ozonation of Surfactants: A Review.” Ozone Sci. Eng. 13:639-73 (1991).   13. Homg, et al., “Enhanced electrochemical oxidation of anionic surfactants.” J. Environ. Sci. Health, part A 33:681-99 (1998).   14. Huber, et al., “Oxydation of pharmaceuticals during ozonation of municipal waste water effluents: A pilot study,” Environmental Science Technology 39:4290-9 (2005).   15. Klasson, et al., “Ozone treatment of soluble organics in produced water, Petroleum Environment,” Research Forum Project 98-04, Oak Ridge National Laboratory, (2002).   16. Loraine, “Oxidation of polyvinylpyrrolidone and an ethoxylate surfactant in phase inversion waste water,” Water Environment Research, 4: 373-9 (2008).   17. Masten and Davies, “The use of ozonation to degrade organic contaminants in waste waters,” Environmental Science Technology 28:180A-185A (1994).   18. Narkis and Schneider-Rotel, “Ozone-Induced Biodegradability of a Non-ionic Surfactant.” Water Res. 14:1225-32 (1980).   19. Narkis and Schneider-Rotel, “Ozonation of Non-ionic Surfactants in Aqueous Solutions.” Water Sci. Tech. 17:1069-80 (1985).   20. Narkis, et al., “Non-Ionic Surfactants Interactions with Ozone.” Tenside Sufactants Detergents 24:200-6 (1987).   21. Oturan and Brillas, “Advanced Oxidation Processes for Wastewater Treatment: 2. Wastewater Treatment by Electro-Fenton Process.” J. Environ. Eng. Manage., 19:233-4 (2009).   22. Oturan, et al., “Degradation Of Pesticides In Aqueous Medium By Electro-Fenton And Related Methods. A Review.” J. Environ. Eng. Manage., 19 (5), 235-55 (2009).   23. Peralta-Hernández, et al., “Recent Advances in the Application of Electro-Fenton and Photoelectro-Fenton Process for Removal of Synthetic Dyes in Wastewater Treatment,” J. Environ. Eng. Manage., 19:257-65 (2009).   24. Petrucci, et al., “Effect of Carbon Material on the Performance of a Gas Diffusion Electrode in Electro-Fenton Process,” J. Environ. Eng. Manage., 19:299-305 (2009).   25. Rosales, et al., “Influence of operational parameters on electro-Fenton degradation of organic pollutants from soil.” J. Env. Sci. Health Part A, 44:1104-10 (2009).   26. Shanbag, et al., “Membrane based ozonation of organic compounds,” Ind. Eng. Chem. Res. 37:4388-4398 (1998).   27. Stemmler and Gonten, “OH radical initiated oxidation of organic compounds in atmospheric water phases: part 1. Reaction of peroxyl radicals derived from 2-butoxyethanol in water, Atmospheric Environment 34:4241-52 (2000).   28. Stemmler and Gonten, “OH radical initiated oxidation of organic compounds in atmospheric water phases: part 2. Reaction of peroxy radicals derived with transition metals,” Atmospheric Environment 34:4253-64 (2000).   29. Suzuki, “Study on Ozone Treatment of Water-Soluble Polymers. I. Ozone Degredation of Polyethylene Glycol in Water.” J. Appl. Polymer Sci. 20:2791-7 (1976).   30. Suzuki, et al., “Study on Ozone Treatment of Water-Soluble Polymers. II. Utilization of Ozonized Polyethylene Glycol by Bacteria.” J. Appl. Polymer Sci. 20:2791-7 (1976).   31. Urbans, “Practical Application of Peroxide for Iron &amp; Hydrogen Sulfide.” Res-Kem Corp., Media, Pa. 1-5 (2006).   32. Villano, et al., Class of Kinetic hydrate inhibitor with good biodegradability, Energy &amp; Fuels, 22:3143-9 (2008).   33. Villano, et al., A study of the Kinetic Hydrate Inhibition performance and sea water biodegradability of a series of Poly(2-alkyl-2-oxazoline)s, Energy &amp; Fuels, 23:3665-73 (2009).