CL IM OF PRIORITY

The present Applications claims benefit of priority from U.S. Provisional Application No. 61/719,53?, filed on 29 October 2012, the contents of which are herein incorporated.

FIELD OF INVEN TION

The present invention relates to a chemical process for preparing esters from organic acids. In particular, the invention pertains to reactions of carboxyiic acids with carbonates in a solvent to produce esters.

BACKGROUND

Esters are an important class of compounds that are encountered in various roles in all areas of synthetic organic chemistry. General methods of preparing esters start, from carboxyisc acids which ate directly condensed with alcohol using acid catalysis (Fischer esterification}. These prior esteritlcation methods, in spite of their utility, sutler from several environmental drawbacks. Fischer esterification is an equilibrium process typically catalyzed by strong, corrosive, mineral acids (e.g., pKa 0). ^' The water generated in the reaction has to be continuously removed by azeotroping or by use of a dehydrative agent or its role countered by use of a large excess of alcohol. Commonly used alcohols, such as methanol and ethanol, can generate gene-toxic afkyi sulphates. Acylation and alkylatio-a are inherently polluting because of salt generation, the use of toxic catalysts and reagents and use of chlorinated solvents.

In .recent years chemists have looked to other ester preparation approaches that can be less polluting and more environmentally friendly. Dimetirylcarbonate (DMC) .has gained prominence as a "green ^{5 "} reagent in. either acid- or base-catalyzed methyiation or methoxyearbonyiauon of anilines, phenols, active methylene compounds and carboxyiic acids. The attraction of DMC lies in the tact that it is non-toxic and gives rise only to C<¾ and methanol (recoverable) as the byproducts.

Several groups have proposed different approaches of using DMC in base-catalyzed methyiation or methoxyeatbonylation of anilines, phenols, active methylene compounds and carboxyiic acids. Others have proposed, a chemosekctive process for the esterification of carbox iic acids under mild i-~80~90*C) and solvent-free conditions using DMC and diethylcarbonate (DEC) under acid catalysis. (See, Vamsi V. Rekha ei /., "A Simple, ^' Efficient, Green, Cost Effective and Chemosekctive Process for the Esterification of Carboxyiic Acids ^* ORGANIC PROCESS RBSEARCJ I & ^■ DEV ELOPMENT, Vol. 13, No.4, 769-773 (2009). ) The process requires the use of strong acids (i.e., pK.a ø} such as FbSO. _i; or.p oluenes ifb.nic acid tPTSA), or mild acids such as m-toiuic acid (MTA), which requires a downstream neutralisation step prior to purification. .Another issue with current esterifieation reactions of organic acids with DMC is thai they are often performed in ditnethyHormamide CDMF). which can be troublesome in post-synthesis downstream processing and purification, because of DMF ^' s high boding point (e.g. , - [ 53 ^C C) a«d propensity to decompose over lime, which can lead to formation of highly toxic and reactive dimethylamme. This contamination of the desired ester products can be costly and harmful.

in view of the foregoing disadvantages a new process of esterifieation is needed, that, can eliminate or minimize the issues associated with esterifieation reactions that depend on an extrinsic catalyst.

SUMMARY Of THE INVENTION

The present invention provides a method of preparing esters. The method involves the reaction of an organic acid with a diakyieat honate in the presence of an alcohol-containing solvent and without either an extrinsic acidic or basic catalyst species. The method further comprises isolating the corresponding esters. The organic acid is a mono-, di-. tri-carboxy!ic acid or combination of such organic acids. The solvent is composed of an alcohol, a mixture of different alcohols, or a combination of an alcohol and a non-alcoholic species. The alcohol functions as a mediating agent in the reaction between the diaikylcarhonate and organic acid. Absent are an extrinsic acid or a base catalyst, as the inherent nueleophilicity of the alcohol drives the ester synthesis. Depending on the reaction species, one can. produce monoesters, d testers, or triesters separately, or mixtures thereof in various combinations.

In another aspect the present invention relates to an ester compound formed from a reaction of a car boxy lie acid with a carbonate in an alcohol-containing solven without the presence of either as? acid or base catalyst.

Additional features and advantages of the present methods will be disclosed in the following detailed description. It is understood that both the foregoing summary and the following detailed description and examples are merely representati ve of the invention, and are intended to provide an overview for understanding the invention as claimed,

BRIEF DESCRIPTION OF FIGURES FIG. I is an illustration of an esterifieation reaction according to an iteration of the present process.

FIG. 2 is an illustration of a rate-limiting step for in-siiu carbonate metathesis ^,

FIG. 3 shows a set of esterifieation reactions in which various earhoxylic acids are reacted with methyfearbonate in methanol, according to an embodiment of the present invention ^,

FIG, 4 shows a set of esterifieation reactions in which various carboxyhc acids are reacted with diethylcarbonate in ethano!, according to an embodiment of the present invention. FIG. 5 shows a comparative set of ester; fication reactions in which ievulinic acid is reacted in neat carbonates without an alcoholic solvent.

DETAILED DESCRIPTION OF THE INVENTION

Section I - Description

In the present disclosure, we describe a facile, effective method of preparing esters from organic acids using environmentally friendly or so-called gr etC non-toxic dial ky icarbonates {e.g., dimethyl or dicthytcarbonates) in an alcoholic solvent {e.g., methanol or ethanol). ^' The process ol ^: ester synthesis involves an alcohol-mediated reaction between an organic acid and a carbonate without the presence of either an extrinsic acid or base catalyst, conducted over relatively short reaction times. This approach is unprecedented in that no additional extrinsic acid or base catalysts are necessary to effect the esterification. Bsterification of an organic acid with a diaiky!carbonate according to the present process results in high conversion rates (e.g., >. 50%) of the organic acid into its corresponding organic acid alkyi esters in relatively high yield (e.g., >. 35%). The alkyi esters can be easily isolated from the reaction mixture without need for neutralization, such as by means of at least fractional distillation, chromatography, or both. This process is achieved with a minimal amount of side products.

Although not. bound by theory, Figure ] presents an illustration of a proposed, non-limiting mechanism for the present esterification reaction. In the proposed mechanism, the organic acid serves a dual role in the reaction. The organic acid itself serves, first, to activates the carbonate, and second, as a chemical reactant. Self catalysis by the organic acid circumvents the need for an external catalyst. Additionally, the mechanism shows that an alcohol solvent/eo-solvent serves as a reagent in the irreversible step of decomposition of the putative anhydride structure resulting in the formation of the product and CC½.

In general, the present esterification reactions take advantage of soivoiysis, in which the solvent serves as a reagent, driving the reaction forward by virtue of its great excess. For the esterification to proceed according to the present process, the solvent in the reaction is an alcohol. Solvoiytic reactions entail nucleophiiic substitutions (i.e., reactions in which an atom or a group of atoms in a molecule is replaced by another atom or group of atoms), where the electron rich solvents act as nacleophiles that add to then force the elimination of small molecules or group from the substrate.

Unlike conventional esterification reactions, in the present method the alcohol-containing solvent does not function according to traditional nuc!eophile substitution mechanisms, in which the R-suhsfituent of the alcohol directly displaces a leaving group. Not to be bound by theory. Figure 2 illustrates a putative rate-limiting step of the present esterification reaction, which involves an in-sU generation of alkyi carbonates front dialkylcarbonates via a metathesis process, in which an anhydride ester Is formed. This transient intermediate species in an intermo!ecu!ar conversion rapidly decomposes in the presence of alcohol to a corresponding alky I. es er with the release of€<¼ and a m la equivalent of alcohol. The soiveni- etathesized carbonate is the statistically favored product.

This result suggests that the alcohol species drives the ester formation through the decomposition of the anhydride intermediate, not the carbonate itself as whatever carbonate one may start with will be altered depending on which kind of alcohol is used. In general, when carhoxyiic acids are reacted with a dlalkyloarfxmate in a corresponding a!ky! alcohol the aikyi-gronp of the alcohol appears to control which ester species is generated. For instance, when the aikyl-group of the dialkyiearhonate is different from that of the alcohol (e.g., DMC with ethane;) the resulting ester will predominately have alkyi groups similar to that of the alcohol ( \ diethyl-ester). Hence, the presence of an alcohol-containing solvent is important, for this process. The esterifieation reaction can be driven by an alcohol solvent alone or a mixed solvent containing an alcohol and a non-alcoholic species, and requires no extrinsic acid or base catalysts.

it appears that a greater amount of alcohol in excess of the amount of carbonate in a reaction will help drive the esteri fieation to completion. Hence, in certain embodiments the amount of alcohol present is about 1.5- to 3-foid excess of the stoichiometric amount of carbonate, in other

embodiments the amount of alcohol used is about 2- to 4-fold, or desirably about to 7- or 10-fold excess of the stoichiometric amount of carbonate.

The stoichiometric amount of carbonate used in the reaction should be in excess e uivalents of the number of carboxyl groups of the organic acid. At minimum the carbonate should be about 1.5 or 2 equivalents per carboxyl group. Typically, the amount of carbonate Is about 2.5 equivalents or more, more typically about 3 to about 5 or 7 equivalents per carboxyl group.

The present esterifieation reaction of carhoxyiic acid with dialkylearbonate is performed typically in the liquid phase, in an alcohol-containing solvent. The particular amount of alcohol and species of alcohol may vary. The solvent may be composed entirely (i.e., 100%) of an alcohol or a mixture of different alcohols, or may comprise a mixture of an alcohol and a non-alcoholic species ί e.g., an alcohol and C<¾ or carbonate mixture, which can generate in situ an active reagent). A certain amount of alcohol species in the solvent is required to perpetuate higher yields of the corresponding d rnono-esters. The alcohol concentration in the solvent should be at least about 5% to about 10% by vvt. of the solution.

A mixed solvent of alcohol and non-alcoholic species can produce a good yield of esters. The non-alcoholic component of the solvent can include an organic solvent, such as: cartx ate C0 ₂ , dimethyl formamide ( DMF). dimethyl sulfoxide (DMSO). acetomtrile, tetrahydrofuran ( THF ?, acetone, N~mcthyi-2-pyrrolidone ( P), chloroform, ethyl acetate, provided that the organic acids are at least partially soluble within them at the temperatures of the reaction.

For instance, when a mixed-solvent or blended system of DMP/aieohol, such as methanol is used in a 1 : 1 ratio, such as in Examples 7 and 20 of Table 3, the mixed solvent blend can help enhance substrate solubility for carbonate species that have a high molecular weight. is another example, a reaction mixture is prepared with COj and methanol with a heterogeneous catalyst to generate a reaction product containing DMC and methanol. This reaction product, can be part or a cost efficient and self-sustaining reagent system, and allows one to avoid the need to synthesis pure DMC. (for more detail about this process of converting CO and methanol to DMC, see: Michael A. Paoheco, el if ., ^" Review of Dimethyl Carbortaie (DMC) Ma factitre and Its Characteristics a Fuel Additive. " ENERGY & FURLS 1 997, I f 2-1 9; Masayoshi Honda, e al, "Catalytic Synthesis of Diaikyl Carbonate from low Pressure C<¼ ana Alcohols Combined with Ac tonitrite Hydration Catalyzed by CeO>< " CATALYSIS A; GENERAL 384 (2010} 1 5- 170; or Masayoshi Honda, ei h, "CerkhCafafyzed Conversion of Carbon Dioxide into Dimethyl Carbonate with 2-Cy opyridim. " CHEMSUSCHKM, V.6. issue 8, pp. 1341 - 134 Aug. 2013, the contents of each are incorporated herein by reference. }

ny liquid alcohol with R-groups having one to 12 carbons, or more, can serve as the solvent (reagent). The R-groups can be saturated, unsaturated, or aromatic. Alcohols such as methanol, ethanol, propanol, or butanol are more typical in view of their common availability, inexpensiveness, and mechanistic simplicit in the ester; fication. reaction. Table 1 shows non-limiting examples of some unsaturated and aromatic alcohols, which represent alternative species including their various permutations and derivatives. These alkene, alkyne, and aromatic alcohols are commercially available and relatively inexpensive.

TABLE L - ;»sa£urau¾i *¾ romafe Al ohols

The particular choice of alcohol species can determine the kind of ester spec ies generated ^, in certain embodiments, the alcohol may have an R-group different front that of the alk l group in the d alkylcarbonate. For instance, when the alkyl group in the diakylcarbonate is a methyl group and the alcohol is an ethyl group. Alternatively, the alcohol species can have an R- group wit an identical number of carbon atoms as that of the diaklyiearbon&te, such as ethanol reacting with

dtethylcarhonate. Various aikylearbonaic species car: be used in the ester? fkation reaction according to the present process. I he alky! group in the dialkyicarbonate may have any number of carbon atoms, for instance, from 1 or 2 to 1 8 or 20 carbon atoms, typically between 1 and 1 S carbon atoms, more typically between 1 and 10 carbon atoms. Preferably, the alkyl group has 1 to 6 carbon atoms. The alkyl group may, for example, be methyl, ethyl, n-propyl, isopropyl a-butyi, iso- butyl peo yl, isopentyi, hexyi, or isohexyi. Preferably, the alkyl is methyl or ethyl Table 2 provides non-1 imitsng examples of common dialkyl carbonate species, such as dl etirvlcarbonate (D C L ά ietby lcar bonate (DEC), dipropylcarbonate (DPC), or dibutykarbonate (DBC), and their respective molecular weights and boiling points. For reasons of cost, common availability and ease of handling, dimethylcarbonate or diethylcarbon&te are the carbonate species employed typically, but other dialkyicarbonate species as ay also be used.

TABLK 2. - Carb ssates

One can use a variety of different organic acids, for example, selected, from; a)

monoc&rhoxylic acids: formic acid, acetic acid, propionic acid , lactic acid, butyric acid, isobufyric acid, valeric acid, hexanoic acid, beptanoic acid, decanoic acid, lauric acid., myristio acid, and C 14- C 1 fatty acids; b s dkarboxylic acids: 2,5-furandscarboxyUc acid i ^' PDCA), funiark acid, itaeonie acid, malic acid, succinic acid, ma ie acid, ma ionic acid, giotaric acid, glacarie acid, oxalic acid, adipic acid, pimeiie acid, suberic acid, azelaic acid, seback acid, dodecanedioic acid, glutaconic acid, oriho-phihalk acid, isophthalk acid, ferephthalic acid; or c) tricarboxylic acids: citric acid, isocitric acid, aco itic acid, rricarbailylic acid, and triraesic acid. Desirably, the organic acid is a dkarboxylic or tricarboxylic acid. In certain preferred embodiments, the carboxylk acid can be selected from one or more of the following: succinic acid, malic acid, citric acid, ievulinic acid, or adipk acid. As used herein an organic acid may be either a carboxylk acid or an amino acid.

The amount of reagents used in each reaction is adjusted to meet the requirements of the different organic acids. In other words, a mono-acid will need one equivalent of reageots, while a di~ acid will use two equivalents, and a tri-acid will use three equivalents. Typically, the reactions are performed within a time period not exceeding about 24 hours, often not exceeding about i O or 12 hours, or preferably within about 6 or 8 hours, and snore preferably within about 4 or 5 hour*;. For about each hour of increase in the duration of the reaction, the amount yield of ester product can improve about 5-10%.

The temperatures at which the estenfication reaction is conducted may vary considerably, but usually the reaction temperature is in a range from about 1 30°C to about 230 C, depending on the species of organic acid and diaikylcarbonate used in the reaction, in an inert atmosphere such as Typically, the temperature is in a range from about ;40 ^'~: C or 150°C to about 213°€ or 220 ^':' C, In certain embodiments the carboxyiic acid and carbonate are reacted at a temperature between about 15I C or \ 60°C to about 208°C or 215°C. Particular examples involve reactions at a temperature between about 165°C or ! 68 C to about 205 ^'; C or 212 ^' . in other examples, the temperature is in a rringe from about 1 ?0°C or ! 75°C to about 200 ^' 'C o 2 s G ^¾ C; particularly, front about 18 X or 185°C to about l.90°C or 1 5X.

Since the temperatures required to obtain good results in reasonable reaction times from an industrial point of view are generally higher than. 120X, and since the dia!k learhonate (e.g. _t DMC, DEC. DPC, DBC) boils under such temperature ranges, the alkylation reactions are executed in an apparatus capable of bearing the required pressures.

T he pressures at which the reaction is conducted are similarly susceptible to variation.

Atmospheric and super-atmospheric pressures are generally applied, depending on the vapor pressure of the particular solvent at a particular temperature In the operative temperature range. Typically, the pressure is in a range from about 145 psi to about 950 psi; more typically from about .150 psi or 155 pel to about 900 psi or 920 psi (gauge). In certain examples the pressure is between about 160 psi and about 650 psi, or about. } 8 psi to about 620 psi. For instance, the vapor pressure of methanol is about 293.9 psi or 587.8 psi. respectively, at about I 6?.8 ^V € or 203.5°C. FShaool. for example, has a vapor pressure of about 295 psi and 580 psi, respectively, at about ] 85°C and 212 ^:: C

According io the present process, one is able to achieve at least 50% conversion of a particular carboxyiic acid to its corresponding mono-, di-, or tri-esters. Typically, the acid conversion rate is at least about 55%. More typically, the acid conversion rate is between about 60% and about 100%, Desirably, one is able to achieve at least 70% conversion. In some reactions, at leas- 50% of the organic acid is converted to a combined yield of monoesters and di-esters. Usually, the combined monoester and cli-ester conversion rate is about 65% or greater. With optimization, complete conversions of carboxyiic acids to their corresponding mono- and/or di -esters can be accomplished under the reaction conditions. The reaction can be performed in either a batch or continuous reaction process,

A principal advantage of the present method of esferiilcation derives from the circumvention of added catalyst to effect complete acid or ester conversions. A corollary to this benefit is the simplification of downstream separation process for the reaction products in comparison to conventional techniques. One can eliminate a conventionally necessary d wn tream step of pH adjustment ρπΌϊ to purification. Moreover, the avoidance of either as extrinsic acidic or alkaline catalyst with the present synthesis process, one need not worry about the effects that acids or bases present in the distillation columns and one can recycle the distillation, bottoms product back into the reaction.

The different organic acid esters produced in the esterificsb ^' on reaction can be isolated from the reaction mixture using various techniques such as by means of distillation or acid-base extraction. For instance, one can separate the mono and diesvers, which tend to have boil ing point of about 2 0°C or greater, from lower boiling solvents by means of simple distillation, or use an acid-base extraction to precipitate the carboxylate, and then regenerate the organic acid with a strong acid < p a < , e.g.. 1-ICI s.

Section it -· Examples

According to the present esterifseation process, it is probable that in reactions involving diaeids formation of monoesters would dominate during the initial stages of the reaction primarily due to statistics. Equation { 1 > represents an example of this mechanism involving a reaction of succinic acid with a diethyicarbonate in ethanol. According to the mechanism, if one di- acid molecule collides with two molecules of the carbonate, the di-ester would form. Statistically, however, it would be more likely that one molecule of the di-aeid collides with one molecule of the carbonate, thus generating the monoester. Over time, the monoester would convert to corresponding di-esters.

The ratio of mortoesiers to diesters produced can vary depending on the duration and temperature of the esterifi cat ton reaction. Early in the reaction (i.e., 0- 1. hours), the ratio significantly favors the monoester species (e.g., about 95:0.5). The ratio is about 4: 1 after about 3-4 hours, and about 1 : 1 - i :2. S ( depending on the acid and conditions) after 5 hours. This ratio would be about 1 :3 or :4 alter about 6-7 hours and about 0.5:95 after about 8- 10 hours. Repeating these reactions will generate the di-ester or id-ester of the corresponding di- or tri-acids.

I able 3 summarizes a number of comparative examples and inventive examples. In

Comparative Examples I and 2, when an organic acid (e.g., succinic acid or levuiinic acid) is reacted with an alcohol solvent alone, virtually no ester is produced, and the acid remains largely nreactive . When the organic acid is reacted with a dialkyi carbonate in D F solvent, as in Comparat ive Examples 3 and 4, the acid was again largely unreactive and generated a yield from about 0 wt.% to about 1 7 wt.% of estei.

When the esterification reaction is run without the presence of an alcohol, we observe vers.'

Utile to no conversion of the carboxyiie acid to its corresponding mono-ester, di -ester, tri-ester, or polyester, in the comparative examples, esterification reactions conducted neat in carbonate solvent resulted in negl igible conversions of add to ester product, such as in Comparative Examples 5 and 6 (i .e., levul tic acid -10% wl, methyl eateriilcation with DMC; - C l ¾ wt. ethyl esterification with DEC). Hence, alcohols appear to be an important reagent m the reaction so as to obtain a high- yiekimg esterification process (e.g., d tester yield of > 35%).

In contrast, the present esterification method can work well with a variety of different organic acids. in the examples conducted according to the present esterification reactions, we demonstrate that one can produce mono--, di- or tri -esters by means of reacting a corresponding carboxyiie acid and dialkyi carbonate in an alcoholic, solvent. Reacting five different carboxyiie acids (i.e., mono-, dt- and tri-ackis: ievulinie, succinic, malic, adipie, and citric acids) and a combination of dialkyi carbonate species, the examples show that esters front each acid and carbonate combination can he prepared in relatively good yields (e.g., > 45% or 50%) and with specificity (e.g., up to about -79% ·.*.- 3% dteste-r). The amount of ester produced and conversion of ^" the acid are significantly greater than.. e.g., 90% - 100% conversion, up to about 80% yield vis- ~ that of the comparative examples.

Depending on particular reaction parameters, such as the temperature, pressure and duration of the esterification reaction, esters were produced with yields between about 43% or 45% and 75% or 80% by weight {e.g., 50% or 60% by vet.). ith optimization of the process one can achieve even snore favorable conversation rates and yields (e.g., about 90%, 95%, 97%, or 98% by weigh ⁾ .

E 3. - &pertneat»! Resal s with Various Acid Species

9 Malic DEC Eihanoi Diethyirfialate 69.4 0.0

Hi Malic i:mc Ethane} Diethylmakte 77.6 0.0

\ i Levaiinie DMC dhanoi Meihyiievu!m&te 70.5 29.3

12 l . vaCac- DEC Bihanoi Ethylkviilinaie 46.8 50.8

1 Levaiiiik: DP€ Ρ· !;;·η<:; Et ylkvuHisaic 45.6 54.7

I S Citric DMC Methanol Tr nethY!c Urate 7 1 .3 0.0

16 Citric DEC Ethane! Trtethvlc irate ^■ 45,6 0 0

17 Citric DMC Et aaol Tne&yicitrate 55.8 0.0

18 Adipie DMC Methanol D!raethyiadlp&ie 39.8 0.0

19 Adspi DEC Ethanol Diethyiadipate 35.1 0.0

20 Adipie DMC Methano!/DMF Dinxahyladlpate 13.5 0.0

DMC Disisc iyiesi- opat

DEC ----- Dic;hy!c3rhof;;si.c

DPC -·-·· OlpropyJcat oiSHtc

C P ----- Dimetbjiformamakte

Reaction eoisdiiii!jss: 20 . acxd. 5 molar cquiv-i!enis UMa Ci'DPC (2.5 molar cq. in ease onevirtinfc: acid). 500 g.

soiveui -. -^d at i&rC, 5 }:,. 3 0 f.«! ■

The following describe the preparation and reaction of some of the comparative and inventive cxaosples in Table 3 in greater detail

Example A; Synthesis of Diethyiadipate from Adipie Acid, Die y!carbonate, and Ethanol

H)0% cooversiofs 35% Cd 6S% yield

Twnty grams adipie acid, 83 mL of diethy (carbonate, and 300 g of ethanol were charged to a stainless steel, 1.1, Parr reactor body. While stirring .mechanically at 1 00 rpm, the internal headspace was pressurized to 200 psi _: , and heated to 1 WC for 5h. After this time, the reactor body was cooled in a water bath until reaching room temperature and pressure released. The homogeneous solution was poured into a storage flask and a sample of this quantitatively analyzed for

diethyladipate, mono-methyiadipate and adipie acid.

Example B: Synthesis of Dimethyimalate from Malic Acid, Dimethykarbonate, and Methanol

100% conversion ?9% yield ^' Twenty grams malic acid, 63 roL of diroethy lcarbonate, and .300 g of methanol were charged to a stainless steel, I L Parr reactor body. While stirring mechanically at 1 100 s in, the internal head pace was pressurized to 200 psi ₂ and heated to 1 ffiC for 5b. After this time, the reactor body was cooled in a water bath until reaching room temperature and pressure released. The homogeneous solution was poured into a storage flask and a sample of this quantitatively analyzed for

dsmeihylmalate and malic acid. Based on findings with adipie acid, the absence of malic acid in the product mixture and 79% yield of diester adduces the remaining 21 % of product mixture as the vorrespou ding mono-ester.

Example Synthesis of ethyiievuhnate from Levuiinie acid and Dimethy!carbonafc

100% conversion -i

Twenty grams levuiinie acid and 300 g dimetftyiearbonate were charged to a stainless steel, I L Parr reactor body. While stirring mechanically at 1 100 rpm, the internal headspace was pressurised to 200 psi ; and heated to 180 ^¾ C for Sh. After this time, the reactor body was cooled in a water bath until reaching room temperature and pressure released. The homogeneous solution was poured into a storage flask and a sample of this quantitatively analyzed for methylievulinate and levuiinie acid,

EmmpU- 0: Synthesis of Dimethylsuccinate from Succinic acid. imeihylcarbonaie, and

Dimethyitbrmamide

48%% conversion 16% yield

Twenty grams succinic acid, 72 mL dimethylcarbonaie and 300 g of DMF were charged to a stainless steel, 1 L Parr reactor body. While stirring mechanically at. 1 100 rpm. the internal headspace was pressurised to 200 psi N ₂ and heated to . S0"C for 5h. After this time, the reactor body was cooled in a water bath until reaching room temperature and pressure released. The homogeneous solution -was poured into a storage flask and a sample of this quantitatively analyzed for dimethylsuccinate and succinic acid.

The accompanying Tables 4-7 summarise examples of the synthesis of di -esters from dimethyl carbonate and diethyl carbonate using succinic acid and either methanol or ethanol solvent. in Table 4, succinic acid is rea ted w th diroethyicarbonate in etbanol at a temperature of about ! 80"€ in an inert nitrogen atmosphere at a pressure of 500 psig. The di-ester product is predominately diethyfsuccinate at about 56.5% yield with minimal dimethylsuccinate at 0.1 % yield. A small amount of succinic acid remained unreacted. In contrast, in Table 5, succinic acid is reacted with

5 diethyicarbonate and methanol at 1 0°€ under s nlar conditions. The di-ester product is

overw helmingly d imethy Isuccinate at about 57.64% yield, with minimal diethylsuccinate at 0,0% yield. Table 6 presents a .reaction of succinic acid with diethyicarbonate in etbanol at I 90°C for 5 hours, which produced diethylsuccinate at about 52.5% conversion. T able 7 summarizes the results of a reaction between citric acid and diethyicarbonate in etbanol at a temperature of I 0 ^':; C for about 5

10 hours irt an inert atmosphere at a pressure of about 500 psig. The reaction produced triethyleitr&te at. about 38% conversion. Ail of the citric acid was consumed. As the examples show in these tables, este ification conducted under mild conditions according to the present process produces various kinds di-esters and tri -esters front different organic acids at relatively good conversion rates. The ester yields will improve with adjustments to increase the reaction time and/or temperatures for

I S optimal results.

Figure 3 presents a series of methyl esterification reactions using various kinds ofcarboxylic acids with diroethyicarbonate in methanol. Each reaction used 20 g. carboxylic acid, 5 molar equivalents of dimethylcarbonate (DMC (2.5 equivalents for levulinic acid), 300 g. of absolute methanol, at. 1 8<fC. 5h, 200 psi >½. All acids, except levulinic acid, completely converted in the

20 reaction. Each exh ibited high selectivity (e.g., 40%) of the fully esters iied target (d lesser) species.

Figures 3A and 38 represent ester; fication of succinic acid and malic acid, respectively, which produced about a yield of about 60% and 79%, respectively, oft.be corresponding di-esters. in Figure 3C, about 71 % of levulinic acid was consumed in the reaction to produce about 70% yield of the ester. The esterification reaction with adipie acid produced a mixed product of the corresponding

25 mono-ester and di-ester, respectively, at about 60% and 40¾ yield.

Similar to the reactions in Figure 3, Figure 4 presents a number of reactions in which different ethyl esters o carboxylic acids are prepared with diethyicarbonate in etbanol. The each of the reactions was performed with 20 g. carboxylic acid, S molar equivalents of diethyicarbonate (DEC) (2.S e uivalents for levulinic acid. 300 g. ethanol, at. 1 H(fC, 5h, 200 psi N ₂ . Again all acids, except

30 levulinic acid, manifested complete conversion during the respective reactions. The selectivity for each of the esterified targets was very good, at about 35% or greater. Figure 4A shows the esterification of succinic acid, which produced a yield of about 54% of the corresponding di-ester. In Figure 4B, .malic acid is also completely consumed and produced a yield of about 69% of the corresponding di-ester. In Figure 40, about 50% of the levulinic acid is consumed to yield about. 47%

35 of the corresponding ester, in Figure 4D, citric acid completely converted to produce about 46% of the tri -ester. Figure 4E shows the reaction of adipie acid to make a mixed product of the corresponding monoester and di-ester, about 65% and 35%, respectively. The remaining product in each ease, excepting levulinic acid, presumably is the mono-ester.

Figures 5 A and S B illustrate comparative examples (entries 5 and 6 of Table 3) in which levulinic acid is reacted, respectively, with diethyjearbona e and diroethylcarbonate without any other solvent being added. The reactions were performed with 50 g. carboxy!ic acid, 300 g. of

diethylcarbonate (DEC) / diroethylcarbonate (D C) (respectively 5.9, 7.7 molar equivalents), at 180*€, 5h, 200 psi Nj. The reactions .in the comparative examples both exhibited relatively high conversion (-80%) of the organic acid, but low yield of ester, which indicates an ineffective method ofesterification. The reactions generated a very small amount of ester (-1%) when using DEC. and made a slightly better but still minor amount of ester (<10%) when using DMC. The difference in yield obtained between the reactions that employed DMC versus ^' DEC is likely a result ofsteric hindrance to the bimoieeular substitution in the reaction.

The present invention has beet- described in general and in detail by way of examples.

Persons of skill in the art understand that the invention is not limited necessarily to the embodiments specifically disclosed, but that modifications and variations may be made without departing from the scope of the invention as defined by the following claims or their equivalents, including other equivalent components presently known, or to be developed, which may be used within the scope of the present invention. Therefore, unless changes otherwise depart from the scope of the invention, the changes should be construed as being included herein.

 TABLE 5 - Esteri ication of Succinic Acid with Dtethyicarhcmaie n Met a ol

1

Mass of Succinic Acid (gk 20

Molecular weigh* succinic acid (g/rn i) 118.04

Moles of Succinic Acid 0.169

Moiar equivalents of Dieihyicarbonaie S

ass of Dietnyi ;jf hnnate fgi 100.31

Molecular weight of diethyicarbenate g/moi 118.13

Moles of Diethyicarbonate 0.847

Density of Dsethyicarbonate (g/ml) 0.975

Volume of Diethyicarbonate (ml.) 103

Mass of Methano (g) 300

Density of Methanol {g/mLJ 0792

Volume >f nol {mQ 378,79 i

Total Voiurne (ml) "481.79 i i

Total Mass (g) 420.31 i 1

Reaction Temperature c) SO ;

Reaction Time i h) S ; ί

Initial Wj Pressure (psig) 200 ; j

; Pressure at ISi C ipsig; 500 i

Molecular weight diethyl succinat ig/moi) 174.1.9 1

Molecular weigh! dimethyl succinate {g/wo 145.14

Results are in g L Qiethylsuccimite {g L} Mass diethyl succinate {gj Moles diethyl succinate % Conversion

0.00 0,0014 ^■ 3.0000 0.0%

Results are in g/l. Dimethylsoccinate (g/U Mass dim thyfsucclnaie (g) Moies din¾ethyi succinate %Yield

29.40 14.1.646 0.0969 57.64%

Results are in g/kg Su cinic Acid Remaining Mass Succinic Acid (g) Moles Succinic Acid % Succinic Acid

Remaining

4.27 i. r - ; 0.0150 8.9%

