Abstract:
A process utilizing nitric acid and oxygen as co-oxidants to oxidize aldehydes, alcohols, polyols, preferably carbohydrates, specifically reducing sugars to produce the corresponding carboxylic acids.

Description:
RELATED APPLICATION INFORMATION 
     This claims priority to U.S. Patent Application No. 61/780,472, filed on Mar. 13, 2013, the entire contents of which are incorporated herein by reference. 
    
    
     FIELD OF THE INVENTION 
     This invention describes an improved process utilizing nitric acid and oxygen as co-oxidants to oxidize aldehydes, alcohols and/or polyols, preferably carbohydrates to produce the corresponding carboxylic acids. The improved process described herein can be used as a batch process or as a continuous process. 
     BACKGROUND OF THE INVENTION 
     Hydroxycarboxylic acids, and in particular carbohydrate diacids (aldaric acids) offer significant economic potential as carbon based chemical building blocks for the chemical industry, as safe additives or components of products used in pharmaceutical preparations and food products, and as structural components of biodegradable polymers, if they can be effectively produced on an industrial scale. Glucaric acid, for example, is produced through the oxidation of glucose and in salt form is currently in use as a nutraceutical for preventing cancer. The price of this material however is high, approximately $100/lb. Industrial scale production of aldaric acids would also provide sufficient materials for the production of other useful compounds, that include environmentally degradable polyamides with varying properties and applications, which are otherwise not commercially available. 
     Carbohydrate diacids are produced a number of ways from reducing sugars using a variety of oxidizing agents, including nitric acid. An example of a nitric acid oxidation of a carbohydrate is that of D-glucose to give D-glucaric acid, typically isolated as its mono potassium salt (See, W. N. Haworth and W. G. M. Jones, J. Chem. Soc., 65-76 (1944), C. L. Mehltretter and C. E. Rist, Agric. and Food Chem., 1, 779-783 (1953) and C. L. Mehltretter, “D-Glucaric Acid”, in Methods in Carbohydrate Chemistry, R. L. Whistler, M. L. Wolfrom, Eds; Academic Press, New York, 1962, Vol. II, pp 46-48). Alternatively, D-glucaric acid can be isolated from nitric acid oxidation of D-glucose as a disodium salt (See, D. E. Kiely, A. Carter and D. P. Shrout, U.S. Pat. No. 5,599,977, Feb. 4, 1997) or as the 1,4:6,3-dilactone (See, D. E. Kiely and G. Ponder, U.S. Pat. No. 6,049,004, Apr. 11, 2000). Routes have been described showing synthesis of diacids through catalytic oxidation with oxygen over a noble metal catalyst (See, C. L. Mehltretter, U.S. Pat. No. 2,472,168, Jun. 7, 1949). An additional route of synthesis exists by use of oxoammonium salts in combination with hypophalites as the terminal oxidants. For example, Merbough and coworkers describe oxidation of D-glucose, D-mannose and D-galactose to their corresponding diacids using 4-acetylamino-2,2,4,6-tetamethyl-1-piperidinyloxy (4-AcNH-TEMPO) with hypohalites as the oxidizing medium (See, N. Merbough, J. M. Bobbitt and C. Bruckner, J. Carbohydr. Chem., 21, 66-77 (2002) and Merbouh, J M. Bobbitt, and C. Bruckner, U.S. Pat. No. 6,498,269, Dec. 24, 2002). A microbial oxidation of myo-inositol to glucuronic acid which is then oxidized enzymatically or by catalytic oxidation to glucaric acid has also been recently described (See, W. A. Schroeder, P. M. Hicks, S. McFarlan, and T. W. Abraham, U.S. Patent Application, 20040185562, Sep. 24, 2004). 
     A variety of different processes for the oxidation of carbohydrates using nitric acid are known. For example, U.S. Pat. No. 2,380,196 (the &#39;196 patent) describes the nitric acid oxidation of carbohydrates to dibasic acids, particularly tartaric acid. The &#39;196 patent describes a cyclic process in which in each cycle, fresh carbohydrate and residue from a previous oxidation is oxidized with nitric acid. A catalyst, such as vanadium, manganese, iron and molybdenum, is employed to increase the yield of tartaric acid. According to the &#39;196 patent, good yields are obtained when the molar ratio of nitric acid to glucose is 5:7.5, preferably 6:7.5. The &#39;196 patent also describes that when mixing the ingredients, the temperature should be maintained at 20° C. or lower. Following mixing, the temperature is raised gradually or allowed to rise spontaneously to about 30° C. to 35° C. (this is the induction or heating-up stage). When the temperature reaches 30° C. to 35° C., an autocatalytic strong exothermic reaction called the “blow” sets in. The “blow” stage is maintained at a temperature of about 50° C. to 75° C., preferably 65-70° C. for anywhere from 45 to 120 minutes. The final temperature stage of the oxidation is the “fume-off” stage at which the last of the nitric acid is reacted and passed off as lower nitrogen oxides. During the “fume-off” stage, the reaction mixture is maintained at a high temperature somewhat below the boiling point of the mixture, at approximately 90° C. to 95° C. until nitrogen oxide is no longer detectable by the fumes. Oxalic and tartaric acids are recovered from the oxidized reaction mixture by direct precipitation and crystallization. 
     U.S. Pat. No. 2,436,659 (the &#39;659 patent) discloses an improved and economical process for the production of  D -saccharic acid. Specifically, the &#39;659 patent discloses a process that produces higher yields of  D -saccharic acid in a shorter period of time, is more convenient while not employing the use of metal oxidation catalysts. According to the &#39;659 patent, crystalline  D -glucose, in anhydrous or monohydrate form, is added to a solution of nitric acid at a rate that allows control of the temperature of the reaction between 55° C. to 90° C. The mole ratio of glucose to nitric acid used in the process is 1:4. However, the &#39;659 patent notes that a mole ratio of glucose to nitric acid of 1:3 lowers the yield of  D -saccharic acid while a ratio of 1:8 increases this yield. The &#39;659 patent also discloses that when 60 to 70 percent nitric acid is used it is preferred to use reaction temperatures of 55° C. to 70° C. and that when lower concentrations of nitric acid are employed higher reaction temperatures are preferred. When the process is performed in this manner, it is quite rapid, with maximum yields of  D -saccharic acid being obtained in a one-hour period of oxidation. 
     U.S. Pat. No. 3,242,207 (the &#39;207 patent) discloses a continuous process for the oxidation of  D -glucose with nitric acid at elevated temperatures. Specifically, the process described in the &#39;207 patent is performed as follows: (1) to an initial reaction mixture prepared by oxidizing an aqueous solution of  D -glucose with concentrated nitric acids, an aqueous  D -glucose solution and concentrated nitric acid in the molecular ratio of 1:3 to 1:3.5 is simultaneously and continuously added at a temperature of about 40° C. to 70° C.; (2) continuously withdrawing from the reaction vessel an apportion of the reaction mixture corresponding to the volume of the fed-in liquids; and (3) isolating the product formed. 
     U.S. Pat. No. 7,692,041 (the &#39;041 patent) discloses an improved method for oxidizing water soluble compounds using nitric acid oxidation. The method involves (1) preparing an aqueous solution of an organic compound suitable for nitric acid oxidation; (2) combining, over time, employing a controlled process, in a closed reaction vessel, under positive pressure of oxygen, the aqueous solution of the organic compound and an aqueous solution of nitric acid to oxidize the organic compound to a mixture of organic acids; (3) maintaining controlled, moderate temperatures of from about 25° C. to about 50° C., controlled positive pressure of oxygen, and controlled agitation of the organic compound and nitric acid reaction mixture during the oxidation reaction; and (4) removing a portion of the nitric acid from the combined aqueous solution to give a mixture of organic acids suitable for further processing. 
     There is a need in the art for improved oxidation process that is safe, economical and efficient for converting organic compounds into their corresponding acids. 
     SUMMARY OF THE INVENTION 
     In one aspect, the present invention relates to a method of synthesizing a mixture of organic acids, the method comprising the steps of: 
     (a) combining, over time, in one or more closed reaction vessels, under a positive pressure of oxygen and with continuous mixing, an organic compound suitable for nitric acid oxidation and an aqueous solution of nitric acid to form a first reaction mixture, wherein the organic compound and the aqueous solution of nitric acid are introduced into the one or more closed reaction vessels; 
     (b) flowing said first reaction mixture through the one or more reaction vessels while maintaining a controlled temperature of from about 5° C. to about 105° C. and controlled positive pressure of oxygen of from about 0 bar g to about 1000 bar g for a time period suitable to oxidize the organic compound to a subsequent reaction mixture comprising a mixture of organic acid products and nitrogen oxides; 
     (c) recirculating the subsequent reaction mixture into the reaction vessel vapor space headspace; and 
     (d) recovering nitric acid from the subsequent reaction mixture. 
     In the above method, the one or more closed reaction vessels comprise one or more reactors. More specifically, the one or more closed reaction vessels are in series (continuous) or in parallel with one another (batch). For example, the reactor can be a continuously stirred tank reactor (CSTRs), falling film reactors or tubular type plug flow reactor almost any type reactor that mixes, controls temperature and pressure and has a liquid and gas phase (not hydraulically full). 
     The above method can be a continuous process. Alternatively, the above method can be a batch process. 
     In the above method, the organic compound comprises a single organic material or a mixture of organic materials suitable for nitric acid oxidation. 
     In another aspect, the above method further comprises the step of removing a significant portion of the nitric acid from the subsequent reaction mixture. 
     In the above method, the removal of the nitric acid is accomplished by an evaporation, distillation, nanofiltration, diffusion dialysis or alcohol or ether precipitation. 
     The above method further comprises the step of making basic the subsequent reaction mixture from which most of the nitric acid has been removed to convert residual nitric acid to inorganic nitrate and the mixture of organic acids to a mixture of organic acid salts. 
     In the above method, organic compound suitable for nitric acid oxidation is selected from the group consisting of monohydric alcohols, diols, polyols, aldehydes, ketones, carbohydrates, hydroxyacids, cellulose, starch and combinations thereof. For example, the carbohydrates are selected from the group consisting of monosaccharides, disaccharides, oligosaccharides, aldonic acids, aldonic acid esters, aldonic acid salts, aluronic acids, alduronic acid esters, alduronic acid salts, alditols, cyclitols, corn syrups with different dextrose equivalent values, and monosaccharides, disaccharides, oligosaccharides and polysaccharides derived from plants, microorganisms or biomass sources. 
     In the above method, the nitrogen oxides are N 2 O 3 , N 2 O 4 , NO, NO 2  and N 2 O. 
     In another aspect, the present invention relates to a method of synthesizing a mixture of organic acids, the method comprising the steps of: 
     (a) combining, over time, in one or more closed reaction vessels, under a positive pressure of oxygen and with continuous stirring mixing an organic compound suitable for nitric acid oxidation and an aqueous solution of nitric acid to form a reaction mixture, wherein the organic compound and the aqueous solution of nitric acid are concurrently introduced into the one or more closed reaction vessels; 
     (b) flowing said reaction mixture through the one or more closed reaction vessels while (i) maintaining a controlled temperature of from about 5° C. to about 105° C. in a portion of the reaction vessel, (ii) maintaining a reaction vessel headspace temperature of from about 80° C. to about −42° C.; and (iii) a controlled positive pressure of oxygen of from about 0 bar g to about 1000 bar g for a time period suitable to oxidize the organic compound to a subsequent reaction mixture comprising a mixture of organic acid products and nitrogen oxides; and 
     (c) removing most of nitric acid from the subsequent reaction mixture to give a final reaction mixture of organic acids suitable for further processing. 
     In the above method, the one or more closed reaction vessels comprise one or more reactors. More specifically, the one or more closed reaction vessels are in series (continuous) or in parallel with one another (batch). For example, the reactor can be a continuously stirred tank reactor (CSTRs), falling film reactor or a tubular type plug flow reactor or almost any type reactor that can mix, controls temperature and pressure and has a liquid and gas phase (not hydraulically full). The above method can be a continuous process. Alternatively, the above method can be a batch process. 
     In the above method, the organic compound comprises a single organic material or a mixture of organic materials suitable for nitric acid oxidation. 
     In another aspect, the above method further comprises the step of removing a significant portion of the nitric acid from the subsequent reaction mixture. 
     In the above method, the removal of the nitric acid is accomplished by an evaporation, distillation, nanofiltration, diffusion dialysis or alcohol or ether precipitation. 
     The above method further comprises the step of making basic the subsequent reaction mixture from which most of the nitric acid has been removed to convert residual nitric acid to inorganic nitrate and the mixture of organic acids to a mixture of organic acid salts. 
     In the above method, organic compound suitable for nitric acid oxidation is selected from the group consisting of monohydric alcohols, diols, polyols, aldehydes, ketones, carbohydrates, hydroxyacids, cellulose, starch and combinations thereof. For example, the carbohydrates are selected from the group consisting of monosaccharides, disaccharides, oligosaccharides, aldonic acids, aldonic acid esters, aldonic acid salts, aluronic acids, alduronic acid esters, alduronic acid salts, alditols, cyclitols, corn syrups with different dextrose equivalent values, and monosaccharides, disaccharides, oligosaccharides and polysaccharides derived from plants, microorganisms or biomass sources. 
     In the above method, the nitrogen oxides are N 2 O 3 , N 2 O 4 , NO, NO 2  and N 2 O. 
    
    
     DETAILED DESCRIPTION OF THE INVENTION 
     The present invention relates to a safe, efficient and economical oxidation process for oxidizing organic compounds into their corresponding organic acid products. Specifically, this invention relates to an improved method for regenerating nitric acid in situ during the oxidation reaction while also improving the safety and quality of the final product. Effective regeneration of nitric acid reduces the amount of nitric acid required to accomplish the oxidation and allows subsequent recovery and recycling of the nitric acid thus improving the efficiency and economy of the process. However, increasing the amount of nitric acid during the reaction can also lead to run away oxidation rates and over oxidation of the organic substrate. Other patents have disclosed methods for regenerating nitric acid in situ during the oxidation process. U.S. Pat. No. 7,692,041 (the &#39;041 patent) discloses an improved method for oxidizing water soluble compounds using nitric acid oxidation whereby a positive pressure of oxygen is introduced during the reaction to convert gaseous oxides of nitrogen (NOx), by-products from the oxidation, back to nitric acid. The process described in the &#39;041 patent uses a sealed vessel, pressurized with oxygen to re-oxidize NOx in the headspace back to nitric acid, thereby improving reaction rates by increasing the nitric acid concentration in the liquid reaction phase. The &#39;041 patent does not describe alternative methods of improving nitric acid regeneration or oxidation reaction rates. One skilled in the art would expect that increasing the temperature in the headspace would improve nitric acid regeneration by increasing the oxidation rate of NOx back to nitric acid. One skilled in the art would also expect that improving mass transfer of the gas phase back into the liquid phase would increase oxidation rates of the organic substrate. 
     To better understand the effects of headspace temperature, the inventors used a reactor capable of independently heating and cooling the gas and liquid. The &#39;041 patent does not disclose using a reactor having a separate control over headspace and liquid temperatures. Surprisingly, the inventors found that cooling, instead of heating, the headspace below the temperature of the liquid phase improved the overall rate of nitric acid regeneration. Increasing the rate of nitric acid regeneration allows the oxidation process in this invention to use less nitric acid than previously described to achieve the same degree of oxidation. 
     Additionally, in another aspect, while trying to improve nitric acid regeneration by increasing mass transfer of the gas phase into the liquid phase by recirculating the liquid reaction mixture into the gaseous headspace the inventors surprisingly discovered that the oxidation reaction rates did not increase and in fact, the oxidation was quenched and conversion of the organic substrate into organic acid products was stopped. This surprising result may be used to control the energetic oxidation reaction, particularly in preventing over oxidation of the organic substrate once the desired level of oxidation has been reached. This is particularly effective when combined with improved nitric acid regeneration through cooling of the headspace which leads to faster oxidation rates and makes control over the degree of oxidation difficult to control. 
     The oxidation process described herein can be performed as a batch-type process or as a continuous process. The first step of the process of the present invention involves combining an organic compound suitable for nitric acid oxidation with an aqueous solution of nitric acid to form an initial or first reaction mixture, whereby the organic compound is oxidized to form a reaction mixture of organic acids (which constitute part of the liquid phase during the reaction). It should also be noted that during the oxidation that gaseous oxides of nitrogen (gaseous oxides of nitrogen are also referred to herein as “nitrogen oxides” and include N 2 O 3 , N 2 O 4 , NO, NO 2  and N 2 O) are produced in the reaction mixture (which constitute part of the gas or gaseous phase). In one aspect, the organic compound and aqueous solution of nitric acid can be injected simultaneously or sequentially, in any order, into one or more closed reaction vessels that comprise a reaction vessel train. 
     The organic compounds that can be used in the process of the present invention can generally be described to include monohydric alcohols, diols, polyols, aldehydes, ketones, carbohydrates, and mixtures thereof. Non-limiting examples of carbohydrates that may be used in the processes of the current invention include, but are not limited to, monosaccharides, such as the common monosaccharides D-glucose, D-mannose, D-xylose, L-arabinose, D-arabinose, D-galactose, D-arabinose, D-ribose, D-fructose; disaccharides, such as the common disaccharides maltose, sucrose, isomaltose, cellobiose and lactose; oligosaccharides, for example, maltotriose and maltotetrose; aldonic acids such as D-gluconic acid, D-ribonic acid, and D-galactonic acid; aldonic acid esters, lactones and salts that include, but are not limited to, those derived from D-gluconic acid, D-ribonic acid and D-galactonic acid; alduronic acids, for example, D-glucuronic acid and L-iduronic acid; alduronic esters, lactones and salts that include, but are not limited to, those derived from D-glucuronic acid and L-iduronic acid; alditols that include glycerol, threitol, erythritol, xylitol, D-glucitol; alditols with more than six carbon atoms; cyclitols, for example common cyclitols such as myo-inositol and scyllitol; corn syrups with different dextrose equivalent values; other aldonic acids and salts thereof, such as, glucoheptonic acids, glycerbionic acids, erythrobionic acids, threobionic acids, ribobionic acids, arabinobionic acids, xylobionic acids, lyxobionic acids, allobionic acids, altrobionic acids, glucobionic acids, mannobionic acids, gulobionic acids, idobionic acids, galactobionic acids, talobionic acids, alloheptobionic acids, altroheptobionic acids, glucoheptobionic acids, mannoheptobionic acids, guloheptobionic acids, idoheptobionic acids, galactoheptobionic acids and taloheptobionic acids; glycols such as ethylene glycol, diethylene glycols, triethylene glycols or mixtures thereof; mixtures of carbohydrates from different biomass, plant or microorganism sources; polysaccharides from biomass, plant or microorganism sources (such as starch, celluloses, etc.) and of varying structures, saccharide units and molecular weights. The organic compound may also comprise a combination of one or more of the organic compounds. The organic compound may be added neat (namely, as pure substance as a solid or liquid (namely, aqueous)), depending on the desired properties of the reaction mixture. In one aspect, the organic compound is provided as an aqueous solution. 
     As mentioned previously herein, the organic compound is combined with an aqueous solution of nitric acid to form the initial or first reaction mixture. The concentration of nitric acid used in the process of the present invention is not critical. For example, the nitric acid used can be 60% nitric acid, 70% nitric acid, etc. It will be understood by one skilled in the art that the ratio of aqueous nitric acid to organic compound used in the process of the present invention can vary depending on the desired oxidation product composition. The molar ratio is calculated at the beginning of the reaction if all reactants are added at the beginning of the reaction in batch (all together) or in a continuous flow reactor system (all together in the first reactor of the reactor system). The molar ratio is calculated at the end of the reaction step if a fed batch is used (the phrase “fed batch” means starting with one of the reactants (such as an organic compound or nitric acid) in a reaction vessel and then adding the other reactants as the reaction progresses to completion) or if a continuous series of reaction vessels are used and one of the reactants is added at different locations through the reactor train (an amount is added to each reactor vessel in the reactor train). In one aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.1:1 to approximately 2:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.8:1. In still yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.7:1. In still yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.6:1. In still yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.5:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.4:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.3:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1.2:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.25:1 to approximately 1:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1 to approximately 0.9:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1 to approximately 0.8:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1 to approximately 0.75:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1 to approximately 0.65:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.8:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.7:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.6:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.5:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.4:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.3:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1.2:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.4:1 to approximately 1:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.4:1 to approximately 0.9:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.4:1 to approximately 0.8:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.4:1 to approximately 0.75:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.4:1 to approximately 0.65:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.8:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.7:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.6:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.5:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.4:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.3:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1.2:1. In yet another aspect, the molar ratio of aqueous nitric acid to organic compound ranges from approximately 0.5:1 to approximately 1:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1 to approximately 0.9:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1 to approximately 0.8:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1 to approximately 0.75:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1 to approximately 0.65:1. In another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1 to approximately 0.65:1. In a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.5:1. In a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.6:1. In a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.7:1. In a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.8:1. In a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.9:1. In yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.1:2. In still yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.1:1.5. In still yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.1:1. In yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:3. In still yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1.5. In still yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.25:1. In yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.50:2. In still yet a further aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 0.50:1.5. In still yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 1.5:1. In still yet another aspect, the molar ratio of aqueous nitric acid to organic compound is approximately 2:1. 
     Optionally, inorganic nitrate can be added into the reaction mixture at any time during the oxidation process. Generally, the inorganic nitrite will be added at the beginning during the period of time that the first reaction mixture is being formed. Generally, once the oxidation reaction has begun, it may no longer be necessary to add any additional nitrate. 
     The initial reaction mixture is prepared (in one or more reaction vessels) at a temperature that generally ranges from about 5° C. to about 105° C. For example, the temperature ranges may be from about 10° C. to about 105° C., about 15° C. to about 105° C., about 20° C. to about 105° C., about 25° C. to about 105° C., about 30° C. to about 105° C., about 35° C. to about 105° C., about 40° C. to about 105° C., about 45° C. to about 105° C., about 50° C. to about 105° C., about 55° C. to about 105° C., about 60° C. to about 105° C., about 5° C. to about 100° C., about 10° C. to about 100° C., about 15° C. to about 100° C., about 20° C. to about 100° C., about 25° C. to about 100° C., about 30° C. to about 100° C., about 35° C. to about 100° C., about 40° C. to about 100° C., about 45° C. to about 100° C., about 50° C. to about 100° C., about 55° C. to about 100° C., about 60° C. to about 100° C., about 5° C. to about 95° C., about 10° C. to about 95° C., about 15° C. to about 95° C., about 20° C. to about 95° C., about 25° C. to about 95° C., about 30° C. to about 95° C., about 35° C. to about 95° C., about 40° C. to about 95° C., about 45° C. to about 95° C., about 50° C. to about 95° C., about 55° C. to about 95° C., about 60° C. to about 95° C., about 5° C. to about 90° C., about 10° C. to about 90° C., about 15° C. to about 90° C., about 20° C. to about 90° C., about 25° C. to about 90° C., about 30° C. to about 90° C., about 35° C. to about 90° C., about 40° C. to about 90° C., about 45° C. to about 90° C., about 50° C. to about 90° C., about 55° C. to about 90° C., about 60° C. to about 90° C., about 5° C. to about 85° C., about 10° C. to about 85° C., about 15° C. to about 85° C., about 20° C. to about 85° C., about 25° C. to about 85° C., about 30° C. to about 85° C., about 35° C. to about 85° C., about 40° C. to about 85° C., about 45° C. to about 85° C., about 50° C. to about 85° C., about 55° C. to about 85° C., about 60° C. to about 85° C., about 5° C. to about 80° C., about 10° C. to about 80° C., about 15° C. to about 80° C., about 20° C. to about 80° C., about 25° C. to about 80° C., about 30° C. to about 80° C., about 35° C. to about 80° C., about 40° C. to about 80° C., about 45° C. to about 80° C., about 50° C. to about 80° C., about 55° C. to about 80° C., about 60° C. to about 80° C., about 5° C. to about 70° C., about 10° C. to about 70° C., about 15° C. to about 70° C., about 20° C. to about 70° C., about 25° C. to about 70° C., about 30° C. to about 70° C., about 35° C. to about 70° C., about 40° C. to about 70° C., about 45° C. to about 70° C., about 50° C. to about 70° C., about 55° C. to about 70° C., about 60° C. to about 70° C., about 55° C. to about 105° C., about 60° C. to about 105° C., about 65° C. to about 105° C., about 70° C. to about 105° C., about 75° C. to about 105° C., about 80° C. to about 105° C., about 85° C. to about 105° C., about 90° C. to about 105° C., about 55° C. to about 100° C., about 60° C. to about 100° C., about 65° C. to about 100° C., about 70° C. to about 100° C., about 75° C. to about 100° C., about 80° C. to about 100° C., about 85° C. to about 100° C., about 90° C. to about 100° C., about 55° C. to about 95° C., about 60° C. to about 95° C., about 65° C. to about 95° C., about 70° C. to about 95° C., about 75° C. to about 95° C., about 80° C. to about 95° C., about 85° C. to about 95° C., about 90° C. to about 95° C., about 55° C. to about 90° C., about 60° C. to about 90° C., about 65° C. to about 90° C., about 70° C. to about 90° C., about 75° C. to about 90° C., about 80° C. to about 90° C., about 85° C. to about 90° C., about 25° C. to about 55° C., or about 25° C. to about 50° C. 
     As mentioned previously, the reaction mixture is contained within one or more closed reaction vessels that are capable of carrying out the oxidation process. For example, any type of reaction vessel that allows for the gas and liquid phases to have a high mass transfer during the oxidation reaction can be used. In one aspect, the reactor is capable of independently heating and cooling the gas and liquid phases. Examples of reactor vessels that can be used include one or more continuously stirred tank reactors (CSTRs), plug flow reactors, spinning disc reactors, or tubular type plug flow reactors. Additionally, the reaction vessel can contain heat transfer systems such as coils, jackets, loops, etc. Furthermore, when one or more reaction vessels are used, any combination of different types and kinds of reaction vessels can be use. For example, the reaction train can contain a combination of one or more CSTRs, one or more tubular type plug flow reactors, and/or one or more evaporators. The reaction train contain one reaction vessel, two reaction vessels, three reaction vessels, four reaction vessels, five reaction vessels, six reaction vessels, seven reaction vessels, eight reaction vessels, nine reaction vessels or ten reaction vessels. If one or more reaction vessels are used, the reaction vessels can be connected in series with one another or one (such as in a continuous process) or one or more reaction vessels can be used in parallel (such as in a batch process). 
     The reaction vessel can be described as a container or vessel that is insulated from the external environment, such that the reaction mixture contained within the tank reactor is not exposed to ambient air. Additionally, the reaction vessel can comprise one or more mixing elements that are capable of continuously stirring and providing controlled agitation of the reaction mixture within the vessel. The one or more mixing elements may include, but are not limited to magnetic stirrers, propeller stirrers, turbine stirrers, anchor stirrers, kneading stirrers, centrifugal stirrers, paddle stirrers and combinations thereof. Generally, the mixing element is electronically controlled such that the spinning velocity of the mixing element may be altered as needed. 
     The reaction vessel typically maintains a vapor or head space wherein the gaseous phase (gaseous oxides of nitrogen) exists in addition to the liquid phase. The vapor or head space is created by filing the tank reactor with a volume of the reaction mixture that is less than 100% of the volume of the tank. Generally, the reaction vessel is filled with a volume that ranges from approximately 1% of the reaction vessel volume to approximately 99% of the reaction vessel volume. In certain aspects of the current invention, the reaction mixture comprises a volume of the reaction vessel that is not greater than 95%, not greater than 90%, not greater than 85%, not greater than 80%, not greater than 75%, not greater than 70%, not greater than 65%, not greater than 60%, not greater than 55%, not greater than 50%, not greater than 45%, not greater than 40%, not greater than 35%, not greater than 30%, not greater than 25%, not greater than 20%, not greater than 15%, not greater than 10%, and not greater than 5%. 
     In one aspect, the vapor or head space of one or more reaction vessels may be maintained at a temperature of from about 80° C. to about −42° C. For example, the temperature of the vapor (gas phase) or head space can be from about 80° C. to about −41° C., about 80° C. to about −40° C., about 80° C. to about −35° C., about 80° C. to about −30° C., about 80° C. to about −20° C., about 80° C. to about −15° C., about 80° C. to about −10° C., about 70° C. to about −42° C., about 70° C. to about −41° C., about 70° C. to about −40° C., about 70° C. to about −35° C., about 70° C. to about −30° C., about 70° C. to about −20° C., about 70° C. to about −15° C., about 70° C. to about −10° C., about 60° C. to about −42° C., about 60° C. to about −41° C., about 60° C. to about −40° C., about 60° C. to about −35° C., about 60° C. to about −30° C., about 60° C. to about −20° C., about 60° C. to about −15° C., about 60° C. to about −10° C., about 50° C. to about −42° C., about 50° C. to about −41° C., about 50° C. to about −40° C., about 50° C. to about −35° C., about 50° C. to about −30° C., about 50° C. to about −20° C., about 50° C. to about −15° C., about 50° C. to about −10° C., 40° C. to about −42° C., about 40° C. to about −41° C., about 40° C. to about −40° C., about 40° C. to about −35° C., about 40° C. to about −30° C., about 40° C. to about −20° C., about 40° C. to about −15° C., about 40° C. to about −10° C., about 30° C. to about −42° C., about 30° C. to about −41° C., about 30° C. to about −40° C., about 30° C. to about −35° C., about 30° C. to about −30° C., about 30° C. to about −20° C., about 30° C. to about −15° C., about 30° C. to about −10° C., about 20° C. to about −42° C., about 20° C. to about −41° C., about 20° C. to about −40° C., about 20° C. to about −35° C., about 20° C. to about −30° C., about 20° C. to about −20° C., about 20° C. to about −15° C., about 20° C. to about −10° C., about 10° C. to about −42° C., about 10° C. to about −41° C., about 10° C. to about −40° C., about 10° C. to about −35° C., about 10° C. to about −30° C., about 10° C. to about −20° C., about 10° C. to about −15° C., about 10° C. to about −10° C., about 5° C. to about −42° C., about 5° C. to about −41° C., about 5° C. to about −40° C., about 5° C. to about −35° C., about 5° C. to about −30° C., about 5° C. to about −20° C., about 5° C. to about −15° C. or about 5° C. to about −10° C. While the vapor or head space of one or more reaction vessels may be maintained at a temperature of from about 80° C. to about −42° C., the liquid phase of the one or more reaction vessels may be maintained at a temperature of 5° C. to about 105° C. In one aspect, the vapor or head space is maintained at a lower temperature than the temperature of the liquid phase in the reaction vessel. For example, the vapor or head space is at least 1° C., 5° C., 10° C., 15° C., 20° C., 25° C., 30° C., 35° C., 40° C., 45° C., 50° C., 55° C., 60° C., 65° C., 70° C., 75° C., 80° C., 85° C., 90° C., 95° C. or 100° C. cooler than the liquid phase. 
     By specifically controlling the head space to temperature and pressure, the inventors of the present invention found that this results in an improvement in the rate of conversion of nitrogen oxides to nitric acid in the vapor space. Specifically, the inventors found that cooling the headspace below the temperature of the liquid phase improved the overall rate of nitric acid regeneration. Increasing the rate of nitric acid regeneration allows the oxidation process in this invention to use less nitric acid than previously described to achieve the same degree of oxidation. In addition, the process of the present invention is more economical because less nitric acid is lost during pressure control venting of the reaction and during the recovery steps of the process discussed later herein. In other words, the method of the present invention results in a “low waste” oxidation process which has not existed previously. As used herein, the term “low waste” means that less than 1%, less than 0.9%, less than 0.8%, less than 0.7%, less than 0.6%, less than 0.5%, less than 0.4%, less than 0.3%, less than 0.2%, less than 0.1% of nitric acid is lost during the process of the present invention during pressure control venting of the reaction and during the recovery steps. 
     The process of the present invention requires exposing the first reaction mixture to the positive pressure of oxygen. Therefore, oxygen is added at point at time and at some location in the one or more reaction vessels. The addition of oxygen and the location of its addition may be during the formation of the initial or first reaction mixture. Alternatively, in another aspect, oxygen can be added in the last reactor or only reactor (if only a single reactor comprises the reaction train). Still further alternatively, oxygen may be added at a selected reactor in the reaction vessel train. Still further alternatively, oxygen can be to each individual reaction vessel comprising the reaction vessel train. The oxygen may be introduced into the first reaction mixture by any means known in the art, including bubbling gaseous oxygen through the reaction mixture. The oxygen added to the reaction vessel train can be added cocurrently or countercurrently or both cocurrently and countercurrently. The pressure within the reaction vessel generally ranges from above about 0 bar g to about 1000 bar g. In one aspect, the pressure can range from about 1 bar g to about 1000 bar g, about 5 bar g to about 1000 bar g, about 10 bar g to about 1000 bar g, 20 bar g to about 1000 bar g, about 30 bar g to about 1000 bar g, about 40 bar g to about 1000 bar g, 50 bar g to about 1000 bar g, about 60 bar g to about 1000 bar g, about 70 bar g to about 1000 bar g, about 80 bar g to about 1000 bar g, about 90 bar g to about 1000 bar g, about 100 bar g to about 1000 bar g, about 200 bar g to about 1000 bar g, about 300 bar g to about 1000 bar g, about 400 bar g to about 1000 bar g, about 50 bar g to about 1000 bar g, 0 bar g to about 900 bar g, 1 bar g to about 900 bar g, about 5 bar g to about 900 bar g, about 10 bar g to about 900 bar g, 20 bar g to about 900 bar g, about 30 bar g to about 900 bar g, about 40 bar g to about 900 bar g, 50 bar g to about 900 bar g, about 60 bar g to about 900 bar g, about 70 bar g to about 900 bar g, about 80 bar g to about 900 bar g, about 90 bar g to about 900 bar g, about 100 bar g to about 900 bar g, about 200 bar g to about 900 bar g, about 300 bar g to about 900 bar g, about 400 bar g to about 900 bar g, about 50 bar g to about 900 bar g, 0 bar g to about 800 bar g, 1 bar g to about 800 bar g, about 5 bar g to about 800 bar g, about 10 bar g to about 800 bar g, 20 bar g to about 800 bar g, about 30 bar g to about 800 bar g, about 40 bar g to about 800 bar g, 50 bar g to about 800 bar g, about 60 bar g to about 800 bar g, about 70 bar g to about 800 bar g, about 80 bar g to about 800 bar g, about 90 bar g to about 800 bar g, about 100 bar g to about 800 bar g, about 200 bar g to about 800 bar g, about 300 bar g to about 800 bar g, about 400 bar g to about 800 bar g, about 50 bar g to about 800 bar g, 0 bar g to about 700 bar g, 1 bar g to about 700 bar g, about 5 bar g to about 700 bar g, about 10 bar g to about 700 bar g, 20 bar g to about 700 bar g, about 30 bar g to about 700 bar g, about 40 bar g to about 700 bar g, 50 bar g to about 700 bar g, about 60 bar g to about 700 bar g, about 70 bar g to about 700 bar g, about 80 bar g to about 700 bar g, about 90 bar g to about 700 bar g, about 100 bar g to about 700 bar g, about 200 bar g to about 700 bar g, about 300 bar g to about 700 bar g, about 400 bar g to about 700 bar g, about 50 bar g to about 700 bar g, 0 bar g to about 600 bar g, 1 bar g to about 600 bar g, about 5 bar g to about 600 bar g, about 10 bar g to about 600 bar g, 20 bar g to about 600 bar g, about 30 bar g to about 600 bar g, about 40 bar g to about 600 bar g, 50 bar g to about 600 bar g, about 60 bar g to about 600 bar g, about 70 bar g to about 600 bar g, about 80 bar g to about 600 bar g, about 90 bar g to about 600 bar g, about 100 bar g to about 600 bar g, about 200 bar g to about 600 bar g, about 300 bar g to about 600 bar g, about 400 bar g to about 600 bar g or about 50 bar g to about 600 bar g. In still another aspect, the pressure can range from about 1 bar g to about 200 bar g, about 5 bar g to about 200 bar g, about 10 bar g to about 200 bar g, about 20 bar g to about 200 bar g, about 30 bar g to about 200 bar g, about 40 bar g to about 200 bar g, about 50 bar g to about 200 bar g, 1 bar g to about 100 bar g, about 5 bar g to about 100 bar g, about 10 bar g to about 100 bar g, about 20 bar g to about 100 bar g, about 30 bar g to about 100 bar g, about 40 bar g to about 100 bar g, about 50 bar g to about 100 bar g, 1 bar g to about 50 bar g, about 5 bar g to about 50 bar g, about 10 bar g to about 50 bar g, about 20 bar g to about 50 bar g, about 30 bar g to about 50 bar g, or about 40 bar g to about 50 bar g. 
     The first reaction mixture flows through the one or more reaction vessels or reaction vessel train under the controlled temperature and controlled positive pressure of oxygen as described previously herein (namely, a controlled temperature of from about 5° C. to about 105° C. and a controlled positive pressure of oxygen from about 0 bar g to about 1000 bar g) for a period of time suitable to oxidize the organic compounds in the first reaction mixture to form a subsequent (or second) reaction mixture that comprises a mixture of organic acid products and nitrogen oxides (namely, N 2 O 3 , N 2 O 4 , NO, NO 2  and N 2 O). 
     Once this subsequent (final) reaction mixture is formed, it is contacted with, delivered or recirculated to the vapor or headspace of one or more reaction vessels. If multiple reaction vessels are used, the subsequent (final) reaction mixture can be contacted, delivered or recirculated in any of the reaction vessels that contain the subsequent (final) reaction mixture. For example, recirculation may occur in the last or second to last reaction vessel comprising the reaction train. 
     The step of contacting, delivering or recirculating is important in the process of the present invention. Specifically, the contacting, delivery or recirculation step is used convert or recycle the nitrogen oxides contained in the subsequent (final) reaction mixture and gases back to nitric acid (HNO 3 ). This “converted” or “recycled” nitric acid can be reused in the oxidation process through methods described herein. 
     The contacting, delivering or recirculating can be conducted using any technique known in the art provided that a means is used that provides for a high surface area of contact between the gas and liquid phases contained in the subsequent final reaction mixture thereby allowing the nitrogen oxides to be converted or recycled back to nitric acid. The most important aspect is that some means is used to increase the surface area. Basically, any means for creating a high surface area of contact between the gas and liquid phases contained in a reaction vessel can be used in the process of the present invention. For example, the reaction vessel can comprise a pump at the bottom and a spray nozzle at the top. The pump transports the subsequent (final) reaction mixture to the top of the reaction vessel to one or more spray nozzles which spray the reaction mixture into the reaction vessel thereby creating a high surface area of contact. Alternatively, a falling film contactor or packed bed (such as a random, structured, or anything that can cause high surface area contact as known by those skilled in the art), where liquid is pumped from the bottom to the top of a device that creates high surface area as the liquid drops through the tubes of a heat exchanger or a high surface area bed can be used. Alternatively, a high surface area of contact between the gas and liquid phases contained in the subsequent (final) reaction mixture can be created by employing an agitator which can be used to create a high rate of agitation (either horizontal or vertical) in one or more reaction vessels thereby resulting in the reaction mixture being thrown or pushed into the vapor space above the liquid. High rates of agitation using an agitator in one or more reaction vessels employed in the process of the present invention can be determined using routine techniques known to those skilled in the art. 
     While conducting an experiment to understand if improving the mass transfer between the gas and liquid phases the reaction would speed up the reaction, the inventors surprisingly the inventors surprisingly discovered that the oxidation reaction rates did not increase and in fact, the oxidation was quenched and conversion of the organic substrate into organic acid products was stopped. Specifically, the inventors found that when the subsequent (final) reaction mixture was sprayed from one or more spray nozzles at the top of the reaction vessel during this contacting, delivering or recirculating step, that the oxidation reaction immediately terminated, which was immediately identified/recognized by reduced cooling load and the colors of the NOX gas and liquids changing from dark to clear relatively quickly. This surprising result may be used to control the energetic oxidation reaction, particularly in preventing over oxidation of the organic substrate once the desired level of oxidation has been reached. This is particularly effective when combined with improved nitric acid regeneration (discussed more in the next paragraph below) through cooling of the headspace which leads to faster oxidation rates and makes control over the degree of oxidation difficult to control. 
     Additionally, the inventors also discovered that the contacting, delivering or recirculating step allowed for the more efficient recovery of nitric acid as the nitric compounds were more quickly converted to nitric acid due to the efficient contact of the vapor and liquid The inventors believe that the reason the reaction is terminated with this step is that the nitrogen oxides contained in both the headspace and the subsequent (final) reaction mixture are converted back to nitric acid. Once the contacting, delivering or recirculating (recirculation) step is completed and the nitrogen oxides converted to nitric acid, then the nitric acid can be recovered or removed from the subsequent (final) reaction mixture to give a final reaction mixture of organic acids that are suitable for further processing. The nitric acid can be recovered or removed from the subsequent reaction mixture using any technique known in the art. For example, evaporation, distillation, nanofiltration, diffusion dialysis or alcohol or ether precipitation can be used. Regardless of the technique used, a significant portion of the nitric acid is removed from the subsequent (final) reaction mixture. In one aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 65% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 70% of the nitric acid is removed from the subsequent (final) reaction mixture. In still yet another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 75% of the nitric acid is removed from the subsequent (final) reaction mixture. In still yet another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 80% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 85% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 90% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 95% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that at least 99% of the nitric acid is removed from the subsequent (final) reaction mixture. In another aspect, the term “significant” when used in connection with removal of nitric acid from the subsequent (final) reaction mixture means that 99.9% of the nitric acid is removed from the subsequent (final) reaction mixture. For example if the nitric acid is to be removed by evaporation, any evaporator known in the art can be used. Examples of evaporators that can be used in the process of the present invention include, but are not limited to, vertical-pipe, horizontal-pipe, slanting-pipe, rotor or thin-layer, centrifugal, worm and falling-film evaporators, tube-bundle evaporators, basket evaporators, high viscosity evaporators, evaporators with one or more scrubbers, evaporators with one or more boilers, evaporators with one or more distillation columns, evaporators with external return pipe and forced circulation, evaporators with external heating elements and forced circulation and other evaporators known to those skilled in the art. In one aspect, the method of evaporation comprises the use of at least one wiped film evaporator. In an alternative aspect, the method of evaporation comprises the use of at least two wiped film evaporators. In yet another aspect, the method of evaporation comprises the use of a wiped film evaporator and another type of evaporator such as a vertical-pipe evaporator, a horizontal-pipe evaporator, a basket evaporator, etc. In one aspect, more than one evaporator is used in the reaction train. In one aspect, more than two evaporators are used in the reaction train. In another aspect, more than three evaporators are used in the reaction train. In yet another aspect, more than four evaporators are used in the reaction train. In still another aspect, more than one evaporator is used in the reaction train in which at least one evaporator contains a scrubber, condenser or a distillation column. In still another aspect, more than two evaporators are used in the reaction train in which at least one evaporator contains a scrubber, condenser or a distillation column. In still another aspect, more than three evaporators are used in the reaction train in which at least one evaporator contains a scrubber, condenser or a distillation column. In still another aspect, more than four evaporators are used in the reaction train in which at least one evaporator contains a scrubber, condenser or a distillation column. 
     Alternatively, as mentioned previously, the nitric acid can be removed from the subsequent (final) reaction mixture using diffusion dialysis. Diffusion dialysis can be used to remove nitric acid from the reaction mixture instead of or in conjunction with an evaporator. This process is typically used for the separation of common inorganic acids such as hydrochloric acid, sulfuric acid, or nitric acid from multivalent metal cations such as Cu 2+  or Zn 2+ . The aqueous acid feedstock of the inorganic acid and metal salt(s) and a separate water stream are routed through a diffusion dialysis system consisting of low pressure pumps and an appropriate membrane system. Two aqueous exit streams are generated, an acid recovery stream comprised primarily of inorganic acid with some metal salt(s), and a product recovery stream comprised of primarily metal salt(s) with some inorganic acid. The separate streams can be subjected to further diffusion dialysis as needed to give a stream with higher inorganic acid concentration and lower metal salt concentrations, and a stream with higher metal salt concentration and lower inorganic acid concentration. This separation technique was applied to nitric acid oxidation reaction mixtures as prepared by the described methods herein, and was found to perform in the same manner as used in separation of inorganic acids from metal salts. The bulk of the nitric acid with some organic acid products, was in the acid recovery stream, and the bulk of the organic acid products with some of the nitric acid, was in the organic product recovery stream. The use of this technology to separate nitric acid from the organic acid products produced from the oxidation process described here is a very low energy process, operates at ambient temperature, and can be run continuously. It offers an additional advantage over direct evaporation/distillation of nitric acid from the reaction mixture in that in the latter process, additional oxidative processes can occur generating additional nitrogen oxide gases that have to be contained, removed and/or converted to oxides of nitrogen that are convertible to nitric acid. In contrast, the diffusion dialysis process operates at dilute concentrations and the recovered nitric acid stream from the diffusion dialysis process is low in carbohydrate product content and evaporation/distillation of the recovered nitric acid is achieved with minimal oxidation and nitrogen oxide formation occurring during nitric acid recovery. 
     It is recognized that the final reaction mixture from which nitric acid has been removed may be made basic to convert any residual or remaining nitric acid to inorganic nitrate, and converting the organic acids to a mixture of organic acid salts. Neutralization to a pH greater than 7 with inorganic base, without removal of nitric acid, requires base for all of the nitric acid plus the organic acids and the nitric acid is not directly recovered for further use. In contrast, partial recovery of the nitric acid for reuse by vacuum distillation is advantageous because the recovered nitric acid can be used again for oxidation purposes, although it is difficult to remove all the residual nitric acid from the syrupy concentrate with ease. 
     Depending upon the starting organic compounds, the specific reaction conditions employed, and the target products, this solution can be treated accordingly to give the organic acids in one or more forms. Organic acids can be obtained in free acid forms, as disalts, mono salts, acid lactones, and/or dilactones, or as mixtures of various salt forms, and/or acid and/or acid lactone forms. Acids generated from oligosaccharides and other higher molecular weight carbohydrates are mixtures which can contain some of the above aldonic and aldaric acids plus higher molecular weight acids derived from higher molecular weight carbohydrates. These acids can be also be obtained in various acid, lactone and salt forms. 
     Additionally, when oxidation products are obtained from direct concentration of the reaction mixture that removes most of the nitric acid, or by subjecting the oxidation reaction mixture to diffusion dialysis followed by removal of the bulk of the remaining nitric acid by an evaporation/distillation step, residual nitric acid can be removed as nitrate and recovered by a membrane filtration method. When the resultant syrupy product/residual nitric acid mixture is treated with an inorganic base to a pH greater than 7, the resulting solution contains inorganic nitrate and the salt(s) of the product organic acids. This solution is then subjected to filtration, typically nanofiltration, with the bulk of inorganic nitrate passing through the membrane and into the permeate, and the bulk of the organic product remaining in the retentate. The prior art has reported removal of inorganic nitrate from organic acid salts after nitric acid oxidation using ion retardation chromatography (See, D. E. Kiely and G. Ponder, U.S. Pat. No. 6,049,004, Apr. 11, 2000). However, ion retardation chromatography is not as fast, not as applicable on a large scale, and not as efficient as the filtration methods described herein. In the oxidation processes of the current invention, the remaining retentate contains the organic acid salt forms with minimal inorganic salt content. The presence of only small amounts of inorganic nitrate in the organic acid salt products renders purification and/or isolation of the organic acid salt products or non-salt products greatly improved over previously reported methods. 
     In an alternative aspect, the current invention also comprises a mixture of one or more organic acids, produced by the oxidation methods described herein. The mixture of one or more organic acids may be the result of the oxidation of a variety of organic compounds. The mixture of one or more organic acids generally includes the oxidation products of monohydric alcohols, diols, polyols, aldehydes, ketones, carbohydrates, and mixtures thereof. Non-limiting examples of carbohydrates suitable for oxidation by the processes of the current invention include, but are not limited to, monosaccharides, such as the common monosaccharides D-glucose, D-mannose, D-xylose, L-arabinose, D-arabinose, D-galactose, D-arabinose, D-ribose, D-fructose; disaccharides, such as the common disaccharides maltose, sucrose, isomaltose, and lactose; oligosaccharides, for example, maltotriose and maltotetrose; aldonic acids such as D-gluconic acid, D-ribonic acid, and D-galactonic acid; glucoheptonic acid; aldonic acid esters, lactones and salts that include but are not limited to those derived from D-gluconic acid, D-ribonic acid, glucoheptonic acid, and D-galactonic acid; alduronic acids, for example, D-glucuronic acid and L-iduronic acid; alduronic esters, lactones and salts that include but are not limited to those derived from D-glucuronic acid and L-iduronic acid; alditols that include glycerol, threitol, erythritol, xylitol, D-glucitol; alditols with more than six carbon atoms; cyclitols, for example common cyclitols such as myo-inositol and scyllitol; corn syrups with different dextrose equivalent values; other aldonic acids and salts thereof, such as, glucoheptonic acids, glycerbionic acids, erythrobionic acids, threobionic acids, ribobionic acids, arabinobionic acids, xylobionic acids, lyxobionic acids, allobionic acids, altrobionic acids, glucobionic acids, mannobionic acids, gulobionic acids, idobionic acids, galactobionic acids, talobionic acids, alloheptobionic acids, altroheptobionic acids, glucoheptobionic acids, mannoheptobionic acids, guloheptobionic acids, idoheptobionic acids, galactoheptobionic acids and taloheptobionic acids; glycols such as ethylene glycol, diethylene glycols, triethylene glycols or mixtures thereof; mixtures of carbohydrates from different biomass, plant or microorganism sources; polysaccharides from biomass, plant or microorganism sources (such as starch or celluloses) and of varying structures, saccharide units and molecular weights. 
     Additionally, the mixture of one or more organic acids may include the acid or salt forms of the oxidized organic compound. Suitable examples of organic acid salts include, but are not limited to sodium hydrogen glucarate, potassium hydrogen glucarate, lithium hydrogen glucarate, disodium glucarate, sodium potassium glucarate, dipotassium glucarate, dilithium glucarate, lithium sodium glucarate, lithium potassium glucarate, zinc glucarate, calcium glucarate, sodium hydrogen xylarate, potassium hydrogen xylarate, lithium hydrogen xylarate, disodium xylarate, sodium potassium xylarate, dipotassium xylarate, dilithium xylarate, lithium sodium xylarate, lithium potassium xylarate, zinc xylarate, calcium xylarate, sodium gluconate, potassium gluconate, lithium gluconate, disodium gluconate, sodium potassium gluconate, dipotassium gluconate, dilithium gluconate, lithium sodium gluconate, lithium potassium gluconate, zinc gluconate, calcium gluconate, sodium galactarate, potassium galactarate, lithium galactarate, disodium galactarate, sodium potassium galactarate, dipotassium galactarate, dilithium galactarate, lithium sodium galactarate, lithium potassium galactarate, zinc galactarate, calcium galactarate, sodium hydrogen tartarate, potassium tartarate, lithium hydrogen tartarate, disodium tartarate, sodium potassium tartarate, dipotassium tartarate, dilithium tartarate, lithium sodium tartarate, lithium potassium tartarate, zinc tartarate, sodium hydrogen tartronate, potassium hydrogen tartronate, lithium hydrogen tartronate, disodium tartronate, sodium potassium tartronate, dipotassium tartronate, dilithium tartronate, lithium sodium tartronate, lithium potassium tartronate, zinc tartronate, calcium tartronate, sodium hydrogen oxalate, potassium hydrogen oxalate, lithium hydrogen oxalate, disodium oxalate, sodium potassium oxalate, dipotassium oxalate, dilithium oxalate, lithium sodium oxalate, lithium potassium oxalate, zinc oxalate, calcium oxalate, sodium glycolate, potassium glycolate, lithium glycolate, disodium glycolate, sodium potassium glycolate, dipotassium glycolate, dilithium glycolate, lithium sodium glycolate, lithium potassium glycolate, zinc glycolate, calcium glycolate, sodium glycerate, potassium glycerate, lithium glycerate, zinc glycerate, calcium glycerate, and combinations thereof. In another aspect, the hydroxycarboxylic acid may include, but is not limited to, disodium glucarate, sodium potassium glucarate, dipotassium glucarate, zinc glucarate, disodium xylarate, sodium potassium xylarate, dipotassium xylarate, zinc xylarate, disodium galactarate, sodium potassium galactarate, dipotassium galactarate, zinc galactarate, and combinations thereof. 
     EXAMPLES 
     Example 1 
     General Methods for High Surface Area Contact for Examples 2-4 
     Oxidations were carried out in a Metler Toledo Labmax reactor which is designed to operate under computer control. The Labmax was fitted with an overhead agitation motor that drove a stir shaft fitted with an anchor style agitation paddle. The reactor was made of glass and had a silicon oil filled jacket for cooling and heating. In addition, the Labmax was fitted with an overhead balance in communication with a metering pump for controlled dosing of reactants into the reactor, and resistance temperature detector (“RTD”) temperature probes to measure the temperature of both the reactor contents and the reactor jacket oil. A Mettler Toledo LMPress 60 with a pressure transducer and internal proportional-integral derivative (“PID”) loop processing was used to maintain oxygen pressure of 1.0 barg+/−0.04 barg within the reactor. A pressure manifold fitted with a pressure relief valve, a rupture disc, and a pressure gauge was added to the head of the reactor. The Labmax was controlled using iControlLabmax software version 4.0 which allows the user to specify reaction parameters, measures and logs data, and uses PID loop processing to maintain stable material temperatures during a reaction and dose reactants into the reactor at a given rate. 
     Example 2 
     Static Oxidation 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 40° C. 411 g (4.5 moles) of concentrated nitric acid was then added to the reactor and the iControl software was used to maintain a reaction temperature of 25° C. and an agitation speed of 200 RPM for the duration of the reaction Immediately after the nitric acid was added 0.31 g (4.5 millimoles) of sodium nitrite was added to the reactor and the reactor was sealed and pressurized with 1 barg oxygen. The 62.5% D-glucose solution was dosed into the reactor at a rate of 2.88 g/min until 432.4 g (1.5 moles) had been added (150 min). After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature having to run at colder and colder temperatures to maintain the material temperature of 25° C. After 25 minutes, the jacket was running at 12° C. and brown NO x  gasses began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. After 35 minutes, the jacket temperature was running at 4.5° C. to maintain a reaction temperature of 25° C. The headspace filled with dark brown NO x  gas and the liquid mixture turned dark green. At this time, the reaction began to slowly subside taking about 6 hours for the jacket temperature to rise to 20° C. to maintain a reaction temperature of 25° C. The headspace continued to be filled with dark brown gasses and the liquid mixture continued to be dark green in color until the reaction was fully quenched/terminated by adding a liter of cold water to the reactor. The exothermicity, gas production, and green liquid color observations were shown to be typical of all nitric acid oxidations performed in a closed vessel under oxygen pressure regardless of molar ratio or batch size. 
     Example 3 
     Recirculated Oxidation 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 40° C. 411 g (4.5 moles) of concentrated nitric acid was added to the reactor and the iControl software was used to maintain a reaction temperature of 25° C. and an agitation speed of 200 RPM for the duration of the reaction. 0.31 g (4.5 millimoles) of sodium nitrite was added to the reactor and the reactor was sealed and pressurized with 1 barg oxygen. The 62.5% D-glucose solution was dosed into the reactor at a rate of 2.88 g/min until 432.4 g (1.5 moles) had been added (150 min). After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature having to run at colder and colder temperatures to maintain the material temperature of 25° C. After 25 minutes, the jacket was running at 13.8° C. brown NO x  gases began to fill the headspace of the reactor turning dark brown and the liquid contents of the reactor turned emerald green in color. At this time, slow recirculation of the reaction material was started and allowed to continue for the duration of the reaction. The material was recirculated slowly through a spray nozzle so that the material was removed from the bottom of the reactor and sprayed through the headspace of the reactor and back onto the liquid surface. Immediately, the reaction began consuming oxygen indicated by the LM Press 60 having to work harder in order to maintain the 1 barg pressure, and the brown NO x  gasses in the headspace began to dissipate resulting in a colorless headspace and the emerald green color in the liquid lightened up. Within a few minutes, the reaction rate had slowed down enough that the jacket temperature could be run at 17° C. and the reaction temperature maintained at 25° C. The green color in the liquid began to fade to pale yellow and after 1 hour, and the jacket temperature was running at 20° C. to maintain a reaction temperature of 25° C. The early consumption of oxygen, and the reduction in exothermicity, gas production, and green liquid color were shown to be typical effects of recirculation during all nitric acid oxidations performed in a closed vessel under oxygen pressure regardless of molar ratio or batch size. 
     Example 4 
     Recirculated Oxidation 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 40° C. 205.5 g (2.25 moles) of concentrated nitric acid was added to the reactor and the iControl software was used to maintain a reaction temperature of 25° C. and an agitation speed of 200 RPM for the duration of the reaction. 0.46 g (6.7 millimoles) of sodium nitrite was added to the reactor and the reactor was sealed and pressurized with 1 barg oxygen. The 62.5% D-glucose solution was dosed into the reactor at a rate of 2.88 g/min until 648.6 g (2.25 moles) had been added (225 min). After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature having to run at colder and colder temperatures to maintain the material temperature of 25° C. After 18 minutes, the jacket was running at 11.5° C. and brown NO x  gases began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. At this time, slow recirculation of the reaction material was started and allowed to continue for the duration of the reaction. The material was recirculated slowly through a spray nozzle so that the material was removed from the bottom of the reactor and sprayed through the headspace of the reactor and back onto the liquid. surface Immediately, the reaction began consuming oxygen indicated by the LM Press 60 having to work harder in order to maintain the 1 barg pressure, and the brown NO x  gasses in the headspace began to dissipate resulting in a colorless headspace. Within a few minutes, the reaction rate had slowed down enough that the jacket temperature could be run at 23° C. and the reaction temperature maintained at 25° C. The green color in the liquid began to fade to pale yellow and after 1 hour, and the jacket temperature was still running at 23° C. to maintain a reaction temperature of 25° C. The early consumption of oxygen, and the reduction in exothermicity, gas production, and green liquid color were shown to be typical effects of recirculation during all nitric acid oxidations performed in a closed vessel under oxygen pressure regardless of molar ratio or batch size. 
     Example 5 
     General Methods for Examples 6-9 
     Oxidations were carried out in a Metler Toledo Labmax reactor which is designed to operate under computer control. The Labmax was fitted with an overhead agitation motor that drove a stir shaft fitted with four propeller type agitation paddles spaced equally throughout the height of the reactor. The reactor was made of glass and had a siliconoil filled jacket for cooling and heating. In addition, the Labmax was fitted with an overhead balance in communication with a metering pump for controlled dosing of reactants into the reactor, and RTD temperature probes to measure the temperature of both the reactor contents and the reactor jacket oil and a type K thermocouple was used to measure the temperature of the headspace. A Mettler Toledo LMPress 60 with a pressure transducer and internal PID loop processing was used to maintain oxygen pressure of 1.0 barg+/−0.04 barg within the reactor. A pressure manifold fitted with a pressure relief valve, a rupture disc and a pressure gauge was added to the head of the reactor. The reactor was equipped with a stainless steel condenser coil that extended inside the reactor from the top to about half way down the reactor. This condenser coil could be used to cool the top portion of the reactor independently of the oil jacket. The Labmax was controlled using iControl Labmax software version 4.0 which allows the user to specify reaction parameters, measures and logs data, and uses PID loop processing to maintain stable material temperatures during a reaction and dose reactants into the reactor at a given rate. The headspace of the reactor was plumbed into an external FT-IR gas cell with valves allowing gas samples to be removed from the headspace of the reactor. The gas cell was fitted into a Thermo Scientific Antaris Industrial Gas System (IGS) which could be used to take FT-IR spectra of the gas samples in real time. All spectra were obtained using the average of 8 scans from 700-3900 wavenumbers (i.e., inverse centimeters) and a resolution of 0.5 wavenumbers. The IGS was calibrated using certified gas standards. The gas standards were diluted with nitrogen using an Environics 4040 Diluter which allows the user to flow standard gas and nitrogen through the cell at predetermined flow rates in order to achieve desired gas concentrations. A 10-point calibration curve was generated for each gas analyzed. Due to the equilibrium relationship of NO 2  and its dimer N 2 O 4 , the concentrations of both species are expressed in terms of total NO 2  units where total NO 2  units equals the concentration of NO 2  plus two times the concentration of N 2 O 4 . 
     Example 6 
     No Cooling in Headspace 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 40° C. 1238.9 g (13.5 moles) of concentrated nitric acid was added to the reactor and the iControl software was used to maintain a reaction temperature of 25° C. for 3 hours and 25 minutes then increase to 30° C. for 45 min then increase again to 35° C. for 75 min. An agitation speed of 100 RPM was used for the duration of the reaction. 0.93 g (13.5 millimoles) of sodium nitrite was added to the reactor and the reactor was sealed and pressurized with 1 barg oxygen. The 62.5% D-glucose solution was dosed into the reactor at a variable rate starting at 3.12 g/min and gradually increasing to 14.9 g/min until 1297.2 g (7.20 moles) had been added (205 min) After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature needing to run at colder and colder temperatures to maintain the material temperature of 25° C. Gas samples were taken from the reactor every 20 minutes and analyzed with FT-IR for composition and quantification. After 25 minutes, brown NO x  gasses began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. After 4.5 hours the total NO 2  units concentration had built to 70% in the headspace of the reactor then slowly decreased to about 59% at the end of the oxidation. Despite the liquid temperature being maintained at 25° C.-35° C. the temperature of the headspace slowly built to a maximum of 40° C. reaching this maximum at the same time the total NO 2  units concentration reached a max of 70%. This temperature build was due to the exothermic reaction 2NO+O 2             2NO 2 .
     Example 7 
     Cooling in Headspace 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 40° C. 1238.9 g (13.5 moles) of concentrated nitric acid was added to the reactor and the iControl software was used to maintain a reaction temperature of 25° C. for 3 hours and 25 minutes then increase to 30° C. for 45 min then increase again to 35° C. for 75 min. An agitation speed of 100 RPM was used for the duration of the reaction. The headspace condenser was then activated and allowed to run at −12° C. for the duration of the reaction. 0.93 g (13.5 millimoles) of sodium nitrite was added to the reactor and the reactor was sealed and pressurized with 1 barg oxygen. The 62.5% D-glucose solution was dosed into the reactor at a variable rate starting at 3.12 g/min and gradually increasing to 14.9 g/min until 1297.2 g (7.20 moles) had been added (205 min) After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature needing to run at colder and colder temperatures to maintain the material temperature of 25° C. Gas samples were taken from the reactor every 20 minutes and analyzed with FT-IR for composition and quantification. After 25 minutes, brown NO x  gasses began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. After 4.5 hours the total NO 2  units concentration had built to 55% in the headspace of the reactor then slowly decreased to about 50% at the end of the oxidation. The headspace condenser was able to keep the temperature of the headspace below 20° C. despite the exothermic reaction 2NO+O 2             2NO 2 . This lower temperature shifts the equilibrium of the dimerization of NO 2  to N 2 O 4  allowing for more N 2 O 4  to form then enables N 2 O 4  to condense into the liquid phase. Once in the liquid phase the N 2 O 4  can react with water to make HNO 3  and HNO 2  according to the reaction N 2 O 4 +H 2 0         HNO 2 +HNO 3 . The higher concentration of nitric acid in the liquid phase was indicated by the lower concentration of total NO 2  units in the gas phase. At the end of the oxidation, the jacket temperature of the reactor was adjusted so that the headspace could be cooled to 5° C. This resulted in the total NO 2  units concentration in the headspace gradually diminishing to 18% over a 60 min period allowing for more nitric acid recovery.
     Example 8 
     No Cooling in Headspace 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 30° C. 1110 g (12.2 moles) of concentrated nitric acid was added to the reactor. Then 1.1 g (15.9 millimoles) of sodium nitrite and 1753 g of the above dextrose solution (6.1 moles) were added to the reactor and the iControl software was used to maintain a reaction temperature of 35° C. and an agitation speed of 300 RPM was used for the duration of the reaction. The reactor was then sealed and pressurized with 1 barg oxygen. After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature needing to run at colder and colder temperatures to maintain the material temperature of 25° C. Gas samples were taken from the reactor periodically and analyzed with FT-IR for composition and quantification. After about 30 minutes, brown NO x  gasses began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. After 3.9 hours the total NO 2  units concentration had built to 57% in the headspace of the reactor then slowly decreased to about 46% at the end of the oxidation. 
     Example 9 
     Cooling in Headspace 
     A 62.5% (wt/wt) D-glucose solution was prepared by adding solid anhydrous D-glucose to deionized water in a screw-capped flask containing a stir bar. Next, the solution was heated to 65° C. with stirring. Once the glucose was adequately dissolved, the solution was cooled to 30° C. 1110 g (12.2 moles) of concentrated nitric acid was added to the reactor. Then 1.1 g (15.9 millimoles) of sodium nitrite and 1753 g of the above dextrose solution (6.1 moles) were added to the reactor and the iControl software was used to maintain a reaction temperature of 35° C. and an agitation speed of 300 RPM was used for the duration of the reaction. The reactor was then sealed and pressurized with 1 barg oxygen. After a short induction period, the mixture began to react exothermically as indicated by the jacket temperature needing to run at colder and colder temperatures to maintain the material temperature of 25° C. Gas samples were taken from the reactor periodically and analyzed with FT-IR for composition and quantification. After about 30 minutes, brown NO x  gasses began to fill the headspace of the reactor and the liquid contents of the reactor turned emerald green in color. After 3.9 hours the total NO 2  units concentration had built to 50.0% in the headspace of the reactor then slowly decreased to about 40% at the end of the oxidation. The headspace condenser was able to keep the temperature of the headspace below 20° C. despite the exothermic reaction 2NO+O 2             2NO 2 . This lower temperature shifts the equilibrium of the dimerization of NO 2  to N 2 O 4  allowing for more N 2 O 4  to form then enables N 2 O 4  to condense into the liquid phase. Once in the liquid phase the N 2 O 4  can react with water to make HNO 3  and HNO 2  according to the reaction N 2 O 4 +H 2 0         HNO 2 +HNO 3 . The higher concentration of nitric acid in the liquid phase was indicated by the lower concentration of total NO 2  units in the gas phase. The total NO 2  units concentration was consistently 5%-8% lower in this experiment then in the previous example (which was identical in every way except headspace temperature). At the end of the oxidation, the jacket temperature of the reactor was adjusted so that the headspace could be cooled to −8° C. This resulted in the total NO 2  units concentration in the headspace gradually diminishing to 13% over a 60 min period allowing for more nitric acid recovery.
     It is understood that the foregoing examples are merely illustrative of the present invention. Certain modifications of the articles and/or methods may be made and still achieve the objectives of the invention. Such modifications are contemplated as within the scope of the claimed invention.