TREATMENT OF QUARRY LIQUID EFFLUENT

Abstract

Disclosed is a method for preparing a solid material including manganese, the method including the following steps: a. bringing into contact an aqueous effluent including manganese, for example at least 5 mg/L, typically at least 5 to 50 mg/L, and preferably 7 to 25 mg/L of manganese, with an oxidizing agent, manganese, preferably at a temperature between 10 C. and 50 C., and obtaining an oxidized aqueous solution; b. adding a base to the oxidized aqueous solution obtained at the end of step a) until a pH of between 8 and 12, preferably greater than 9, and preferably from 9 to 10.5, and obtaining a solution including a precipitate; c. filtration of the solution obtained at the end of step b); and d. obtaining a solid material including manganese, and especially manganese (IV) and/or Mn (III).

Claims

1. Method for the preparation of a solid material comprising manganese, said method comprising the following steps: a. bringing into contact an aqueous effluent comprising manganese, for example at least 5 mg/L, typically at least 5 to 50 mg/L with an manganese oxidizing agent, and obtaining an oxidized aqueous solution; b. adding to the oxidized aqueous solution obtained at the end of step a) of a base until a pH of between 8 and 12, and obtaining a solution comprising a precipitate; c. filtration of the solution obtained at the end of step b); and d. obtaining a solid material comprising manganese.

2. Method according to claim 1, wherein the solid material obtained at the end of step d) comprises oxides of manganese.

3. Method for the depollution of an aqueous effluent comprising manganese, for example at least 5 mg/L, typically at least 5 to 50 mg/L, preferably 7 to 25 mg/manganese, and comprising the following steps: a. bringing into contact the aqueous effluent with a manganese oxidizing agent, and obtaining an oxidized aqueous solution; b. adding a base to the oxidized aqueous solution obtained at the end of step a) until a pH of between 8 and 12, and obtaining a solution comprising a precipitate; c. filtration of the solution obtained at the end of step b); and d. obtaining an aqueous effluent comprising less than 1 ppm of manganese.

4. Method according to claim 1, wherein the oxidizing agent is chosen from hydrogen peroxide, dioxygen or sodium percarbonate.

5. Method according to claim 1, wherein the oxidizing agent is added in a concentration of between 0.015 mL/L and 2 mL/L.

6. Method according to claim 1 wherein the base is selected from potassium hydroxide, sodium hydroxide, calcium carbonate, sodium carbonate and calcium hydroxide.

7. Method according to claim 1 wherein in step b) the base is added until a pH of at least 9.5.

8. Method according to claim 1 wherein the effluent further comprises one or more of the elements selected from aluminum, calcium, copper, iron, potassium, magnesium, sodium, zinc, nickel, arsenic and silicon.

9. Solid material comprising manganese obtainable by a method as defined according to claim 1.

10. Method of carrying out an organic synthesis reaction comprising the following steps: iii) preparing a compound comprising manganese according to claim 1; iv) carrying out an organic synthesis reaction by contacting the compound obtained at the end of stage i) as a catalyst with a reaction medium.

11. Method according to claim 10, in which the organic synthesis reaction is chosen from the oxidation reactions; the oxidative cleavage reactions; and the epoxidation reactions of alkenes.

12. Method according to claim 11 wherein the organic synthesis reaction is carried out in the presence of a catalyst oxidizing agent.

13. The method of claim 1, wherein: the step of bringing into contact the aqueous effluent comprising manganese uses at least 5 mg/L of manganese, with an manganese oxidizing agent, at a temperature between 10 C. and 50 C.; the step of adding to the oxidized aqueous solution a base is performed until a pH greater than 9 is achieved; and the solid material obtained is manganese (IV) and/or Mn (III).

14. The method of claim 3, wherein: the step of bringing into contact the aqueous effluent with the manganese oxidizing agent is performed at a temperature between 10 C. and 50 C.; the step of adding the base to the oxidized aqueous solution is performed until a pH of greater than 9 is achieved; and the aqueous effluent obtained is less than 0.4 ppm of manganese.

15. Method according to claim 1, wherein the oxidizing agent is hydrogen peroxide.

16. Method according to claim 1 wherein the base is sodium hydroxide.

17. Method according to claim 1 wherein in step b) the base is added until a pH 9.5 is obtained.

18. Method according to claim 1 wherein the effluent further comprises one or more of the elements selected from aluminum, calcium, copper, iron, potassium, magnesium and sodium.

19. Solid material comprising manganese (IV) and/or Mn (III), obtainable by a method as defined according to claim 1.

20. Method according to claim 10, in which the organic synthesis reaction is chosen from the reactions for the oxidation of alcohols to aldehydes or ketones, of alcohols in alpha of an aromatic ring, including heterocyclic, in alpha of a double bond, aliphatic alcohols, for example oxidation of benzyl alcohol to benzaldehyde and selective oxidation of hydroxymethyl furfural to diformyl furan; the oxidative cleavage reactions of diols, of alpha hydroxy acids, of alpha hydroxylated carbonyl derivatives, of dicarbonyl derivatives; and the epoxidation reactions of mono, di-, tri or tetrasubstituted alkenes.

Description

DESCRIPTION OF THE FIGURES

[0045] FIG. 1 shows the composition of the effluents according to the pH of precipitation of metals established by MP-AES

[0046] FIG. 2 shows the composition of the catalysts as a function of the precipitation pH established by MP-AES

DESCRIPTION OF THE PREFERRED EMBODIMENTS

Example 1: Analysis of Effluents from Quarries of Pyrite

[0047]

TABLE-US-00001 TABLE 1 MP-AES analyses of different effluents from pyrite quarries (values in ppm) Al Ca Cu Fe K Mg Mn Na Effluent 1 5.2 71.4 0.4 5.1 6.6 63.2 13.4 31.8 Effluent 2 4.3 65.3 0.5 1.8 6.3 58.2 12.3 31.8 Effluent 3 3 55.2 0.7 2.2 5.3 36.9 9.1 26.4 Effluent 4 56.8 243.5 0.05 6.4 5.3 153.2 14.1 20.8 Effluent 5 154 280 <1 3.4 5.0 227 25.2 24.0

[0048] The effluents come from different pyrite quarries located in Brittany and Normandy. The effluent tested in the examples below is the effluent 3.

[0049] These analyses show that the effluents tested are characterized by a high content of manganese.

Example 2: Preparation of Compounds from Effluents

[0050] The effluent 3 (850 L) was stirred with H.sub.2O.sub.2 (30%, 70 eq) at room temperature. After 30 min, NaOH (2 M) was added dropwise until the desired pH was reached. A black and then yellow precipitate appeared progressively as NaOH was added. The solution was stirred at room temperature for 1 night. The precipitated solid was filtered and washed with demineralized water (3 times) and then with absolute ethanol (3 times). The resulting solid, black (pH9.5), dark brown (pH10.5) or light brown (pH>11), was then dried at 140 C. for 24 hours.

[0051] The metal contents were measured by MP-AES and are presented in the following table.

TABLE-US-00002 TABLE 2 MP-AES analysis of Eco-PS2 formed at different precipitation pH. Mn Fe Ca Mg Na Al K Precipitation (wt (wt (wt (wt (wt (wt (wt Compound pH %) %) %) %) %) %) %) 1 9.5 12.6 4.8 2.1 2.7 0.1 4.3 0. 2 11 3.7 1.1 6.9 13.2 0.1 1.15 0.1 3 14 2.8 0.3 14.4 13.2 0 1.0 0 (comparative)

[0052] The precipitation pH (step b) has a strong influence on the metal content in the final solid obtained after filtration.

[0053] Spectroscopic analysis (transmission electron microscopy) has shown that compounds 1 and 2 have a structure comprising crumpled stars without rods, whereas commercial compounds such as MnO.sub.2 have a rod structure.

[0054] In addition, the XPS analyses suggest that the oxides of manganese (IV) present in the compounds 1 and 2 are associated with oxides of manganese (III). The presence of Mn.sub.2O3 seems to be more plausible than that of manganite (-MnOOH). The XPS spectra of compounds 1 and 2 have a peak Mn 2p3/2 at 642.4 eV and a peak Mn 2p1/2 at 654.4 eV. The XPS analyses were carried out via a spectrophotometer ESCALAB 250 (Thermo Electron Corporation), equipped with a monochromatic Al K X-ray source (1486.6 eV).

[0055] XRD analyses show that only calcium sulphate is crystalline, while Mn oxides are amorphous, as the most active form of MnO.sub.2. The XRD analyses were carried out via a BRUKER diffractometer (D8 advance, with a CuK radiation =1.54086 A) equipped with a LynxEye detector.

[0056] Finally, the BET analyses show that the compound 1 is characterized by a specific surface area equal to 319 m.sup.2/g and an average pore diameter equal to 130 , while the compound 2 is characterized by a specific surface area equal to 154 m.sup.2/g and an average diameter of pores equal to 130 . Finally, BET analyses (Brunauer-Emmett-Teller method are established as follows: pore volume and average pore sizes are estimated from the Barrett-Joyner-Helenda method with the Kruk-Jaroniec-Sayari equation (BJH/KJS).

[0057] The addition of soda ash in the effluents is intended not only to neutralize the acidity of the water but also to precipitate all the metals present. Nevertheless, an excess of NaOH (up to pH=14). When the precipitation pH is 14, almost all of the calcium and magnesium contained in the effluents precipitates and the catalysts formed are then predominantly composed of the corresponding hydroxides. The latter can therefore modulate the activity of the compound, but also retain the reagents and/or products on the surface of the mineral matrix of the compound.

[0058] While calcium can have an activating effect on manganese, on the contrary, magnesium is described in the literature as having an antagonistic effect. It is therefore preferable to control the precipitation pH in order to selectively precipitate the metals.

[0059] The MP-AES analyses presented in FIG. 1 indicate that the manganese concentration in the effluents after metal precipitation is less than 1.8 ppm as soon as the pH reaches 9.

[0060] Therefore, in order to meet the imposed industry standards, it is preferable that the precipitation pH be greater than 9. Then, the MP-AES analyses (FIG. 2) of the solids formed by varying the precipitation pH show that the highest manganese content is achieved for a pH of about 9.5, reaching about 13 wt %. Moreover, it should be noted that, in this case, the Mn/Ca molar ratio is very close to that of the natural cluster (Mn.sub.4, Ca) derived from photosystem 2.

Example 3: Organic Synthesis Reaction

[0061] To test the activity of the materials of the invention, the oxidation of benzyl alcohol to benzaldehyde was taken as a model reaction.

##STR00001##

The procedure adopted was as follows: the reagent (100 mmol.Math.L.sup.1) was brought into contact with the solid prepared in Example 2 in anhydrous toluene and the solution was heated to 110 C. for 5 h. The reaction mixture was then analyzed by GC-MS to determine conversion and selectivity using dodecane as an internal standard.

[0062] The results obtained are presented in the following Table (the pH corresponds to the pH obtained during the precipitation of the compound).

TABLE-US-00003 TABLE 3 Comparison of the precipitation pH on oxidative catalytic activity of solids during the oxidation of benzyl alcohol to benzaldehyde. Conversion.sup.b Yield.sup.b Selectivity.sup.b,c Entry pH Eq. Mn (%) (%) (%) 1 9.5 1 70 69 >99 2.sup.d 9.5 0.3 22 21 >99 3 10 1 <93.sup.e >54.sup.e 4.sup.d 10 0.1 8 7 >99 5.sup.d 10.5 0.3 73 72 >99 6 11 1. <86.sup.e >44.sup.e 7.sup.d 11 0.3 79 78 >99 8 (comparative) 14 1 <45.sup.e >16.sup.e 9.sup.d (comparative) 14 0.3 10 9 >99.sup.e .sup.aReaction conditions: benzyl alcohol 1 (100 mmol.L.sup.1) catalyst, anhydrous toluene reflux at 110 C., 5 h. .sup.bConversion, yield and selectivity were determined by GC-MS, using dodecane as an internal standard. .sup.cRatio of GC-MS to aldehyde yield on conversion. .sup.dReaction performed with bubbling air. e Loss of reagents on the catalyst matrix.

[0063] The first reactions involving the compounds prepared via the method of the invention (pH=9.5) and benzyl alcohol in a stoichiometric amount show a yield of 70% benzaldehyde with excellent selectivity after 5 hours of reaction. In addition, no loss of reagent or product by retention on the mineral matrix of the compound is observed, contrary to what is observed for compounds formed at higher pH.

[0064] However, when the compounds prepared via the method of the invention (pH=9.5) are used in a catalytic amount (0.3 eq) with bubbling air to re-oxidize the catalyst using oxygen, the reaction only occurs in a stoichiometric quantity (20% conversion). The oxygen contained in the air does not allow the re-oxidation of the solids prepared at pH=9.5, 10 and 14.

[0065] On the contrary, a re-oxidation of the compounds (pH=10.5) and solid (pH=11) by the dioxygen of the air is observed. When the compounds are engaged in a catalytic amount (0.3 eq), a conversion of 73% and 79% respectively is obtained in 5 hours of reaction with a total selectivity of benzaldehyde. A 100% yield is obtained after 7 hours of reaction.

[0066] Therefore, the modification of the precipitation pH allows the synthesis of manganese oxide compounds with oxidative power much higher than that observed with compounds prepared with a precipitation pH of 14. The compounds prepared by the method of the invention shows excellent selectivity to benzaldehyde, without over-oxidation to benzoic acid. The compounds prepared at pH=11 and pH=10.5 have the particularity of being re-oxidized by oxygen in the air.

Example 4: Comparison of Activity with Synthetic and Commercial Catalysts

[0067] In order to determine the origin of the activity of the compounds prepared via the method of the invention, synthetic catalysts were prepared. Since precipitation pH influences the activity and re-oxidation of compounds through air oxygen, it is expected that calcium and/or magnesium, the main elements affected by pH change in the range 9-12, play a role in the activity of the catalysts formed.

[0068] Various synthetic catalysts have been prepared from manganese, calcium and magnesium salts.

[0069] The preparation of these catalysts was identical to that followed to synthesize the solids of the invention prepared at a pH=11 from the effluent 3. The synthetic catalysts are derived from commercial products MnSO.sub.4, CaSO.sub.4, MgSO.sub.4. Catalysts 3, 4 and 5 of Table 4 are reconstituted so as to respect the Mn, Mg and Ca ratios of the solid of the invention obtained from effluent 3.

[0070] The concentrations of committed salts are identical to those of the effluents, except in the case of Mn-synthetic catalysts where the concentration of MnSO.sub.4.H.sub.2O has been multiplied by 4 with respect to the concentration of manganese sulphate in the effluents so as to obtain more material to work on.

[0071] The catalytic activity of these catalysts was tested under the same conditions as for the compounds of the invention, by taking the oxidation of benzyl alcohol to benzaldehyde as a model reaction. The results are shown in Table 4.

TABLE-US-00004 TABLE 4 Comparison of the oxidative catalytic activity of the solids of the invention (pH = 11) with that of synthetic and commercial catalysts during the oxidation of benzyl alcohol to benzaldehyde. Eq. Conversion.sup.b Yield.sup.b Selectivity Entry Catalyst Mn (%) (%) (%) 1 Solid according to the 0.3 79% 78% >99% invention prepared at pH = 11 2 Mn-synthetic 0.3 100% 99% >99% 3 MnCa-synthetic 0.3 100% 99% >99% 4 MnMg-synthetic 0.3 67% 66% >99% 5 MnCaMg-synthetic 0.3 90% 89% >99% 6 MnO.sub.2 commercially 1 89% 88% >99% activated.sup.d 7 MnO.sub.2 commercially 0.3 38% 37% >99% activated Reaction conditions: benzyl alcohol 1 (100 mmol.L.sup.1), catalyst, anhydrous toluene, bubbling with air, reflux at 110 C., 5 h. .sup.bConversion, yield and selectivity were determined by GC-MS, using dodecane as an internal standard. .sup.cRatio of GC-MS to aldehyde yield on conversion. .sup.dReaction performed without bubbling air.

[0072] The conversion to benzaldehyde is 100% in cases where the manganese is not coupled to any other metal as well as in the presence of calcium (Table 4, entries 2-3). The method of the invention thus makes it possible to obtain an activated manganese (IV) oxide, more active than MnO.sub.2, including activated MnO.sub.2. These results do not allow one to know whether the presence of calcium within the catalyst has a positive or neutral effect on its reactivity. In contrast, the presence of magnesium appears to reduce the activity of the catalyst, since the GC-MS yield decreases to 66% and 89% for the MnMg-synthetic and MnCaMg-synthetic catalysts, respectively.

[0073] In comparison, the oxidation reaction of benzyl alcohol was also tested under the same conditions with commercially activated MnO.sub.2. Introduced in stoichiometric amount, the reactivity is similar to that of the compounds of the invention, with an 88% yield of benzaldehyde (Table 4, entry 6). However, when introduced in a catalytic amount, the commercially activated MnO.sub.2 is not (or very little) reoxidized by the dioxygen of air, since the yield is only 37% (Table 4), entry 7). These results are in agreement with the literature data that commercially activated MnO.sub.2 must be introduced in excess to effect the oxidation of organic substrates.

[0074] In conclusion, with respect to the oxidation of benzyl alcohol to benzaldehyde, the compounds of the invention (prepared at pH=11) have an oxidizing catalytic activity greater than that of commercially activated MnO.sub.2. This reactivity seems intrinsic to the implemented synthetic procedure, since the Mn-synthetic catalysts show an activity greater than that of the solids of the invention (pH=11). As expected, magnesium has an antagonistic effect on the reactivity of the catalysts, but the experiments carried out do not allow one to conclude as to the effect of synergy between manganese and calcium. Therefore, the procedure employed makes it possible to form an activated manganese (IV) oxide with a high oxidizing power.

[0075] Finally, it is important to take into consideration the environmental footprint that the synthesis of Mn-synthetic catalysts involves compared to that of the compounds of the invention. In fact, the manganese sulphate used to synthesize the Mn-synthetic catalysts is generally prepared by treating MnO.sub.2 with sulfur dioxide or by reacting potassium permanganate with sodium hydrogen sulphate and hydrogen peroxide. In addition to the catalytic performances, it is important to take into account the life cycle analysis (LCA) of catalysts formed so that the synthesis method is part of a sustainable development approach.

Example 5: Use of the Solids of the Invention in the Selective Oxidation of HMF (HydroxyMethylFurfural) to DFF (DiFormyl Furane)

[0076] The compounds of the invention (pH=11) were used as an oxidizing catalyst in the selective oxidation reaction of HMF to DFF.

##STR00002##

HMF (126 mg, HMF DFF 1 mmol) was dissolved in methoxycyclopentane (2 mL), the catalyst (0.3 mol eq Mn) and 10 mL of dry toluene were placed in a container. The solution was stirred and refluxed at 110 C. in the presence of bubbling air for 5 h. The solution was then acidified with an aqueous solution of sulfuric acid at pH=3.3 (10 mL). Ethyl acetate (10 mL) was added and the solution was stirred for 15 minutes. The solution was filtered and the solid was washed three times with 10 mL of ethyl acetate. The aqueous phase was extracted with three times 10 mL of ethyl acetate. The various organic phases were combined and the solvent was evaporated. An orange-yellow solid was obtained. Conversion and selectivity were determined by GC-MS, using biphenyl as the internal standard. The results are shown in Table 5.

TABLE-US-00005 TABLE 5 Conversion to HMF and selectivity to DFF obtained with Eco-PS2 as catalysts. Conversion b Selectivity b, Entry Catalyst Eq. Mn (%) c (%) 1 Solid according to the 1 50% 75% invention prepared at pH = 11 3 Solid according to the 0.3 45% 71% invention prepared at pH = 11 3 Solid according to the 1 60% 77% invention prepared at pH = 9.5 .sup.aReaction conditions: HMF 3 (100 mmol.L.sup.1) dissolved in CPME, catalyst, anhydrous toluene, bubbling with air, reflux at 110 C., 5 h. .sup.bConversion, yield, and selectivity were determined by GC-MS, using biphenyl as an internal standard. .sup.cRatio of GC-MS to aldehyde yield on conversion.

[0077] GC-MS analyses show no other products besides HMF and DFF. The use of the compounds of the invention (pH=11) in stoichiometric or catalytic amounts gives the same results in terms of conversion and selectivity (Table 5, entry 1-2). In both cases, the conversion is close to 50%.

[0078] The conversion and the yield obtained with the solids of the invention (pH=9.5) are slightly higher than those obtained with the solids of the invention (pH=11), with 60% conversion (Table 5, entry 3). In all cases, the selectivity in DFF is close to 75%. In order to determine the presence or absence of carboxylic acids, IR and LC MS analyses confirmed the formation of HMF and DFF.

[0079] N,O-bis(trimethylsilyl) trifluoroacetamide was used as silylating agent. GC-MS analysis of the silylation products indicates the presence of no other compounds than DFF and silylated HMF. The selectivity of the reaction is therefore very high and superior to the methods of the literature which describe the formation of mono and diacids.

Example 6: Oxidation Reactions

[0080] The method of the invention has been implemented in several oxidation reactions using the catalyst from effluent 2. The results are shown in Table 6.

TABLE-US-00006 TABLE 6 Oxidation reactions Entry Alcohol Aldehyde Conversion (%) 1 [00003] [00004] 100 2 [00005] [00006] 98 3 [00007] [00008] 61 5 [00009] [00010] 49 6 [00011] [00012] 94 (54% yield)

[0081] The oxidation is compatible with the OH group of phenol. The primary alcohol is oxidized without touching the phenolic nucleus (entry 3). This reaction makes it possible to obtain vanillin, the product highly sought after in the food, cosmetics, perfume and other industries.

[0082] Oxidation does not degrade the furan nucleus (entries 4 and 5). The reaction stops at the dialdehyde. No trace of acid or diacid is observed either in GC/MS or after treatment of the medium with an inorganic acid followed by extraction. Dialdehyde is a very interesting biosourced building block (see J. Ma, Z. Du, J. Xu, Q Chu, Y. Pang ChemSusChem, 2011, 4, 51-54, A. Gandini, Green Chem., 2011, 13, 1061-1083).

[0083] Cinnamic alcohol is almost completely oxidized to the corresponding aldehyde (entry 6). The aldehyde product is isolated with 54% yield and 40% condensation product is obtained as a reaction by-product. Cinnamic aldehyde is a highly sought-after product in the food, cosmetics, perfume and other industries. The advantages of this method over existing methods are as follows: [0084] the reaction is effected at atmospheric pressure [0085] it is not necessary to bubble pure oxygen or to make the reaction under pressure of O.sub.2. Our method works either in air or by bubbling the air into the reaction medium. [0086] the amount of manganese used in the reaction is from 10 mol % to 50 mol % in Mn, which is much lower than the existing methods.

Example 7: Oxidative Cleavage

[0087] The method may also be extended to the oxidative cleavage of -diols, -hydroxyketones, -hydroxyacids. The results are shown in Table 8.

TABLE-US-00007 TABLE 8 Oxidative cleavage using the catalyst from effluent 2 Entry Alcohol % Benzaldehyde Conversion 1 [00013] 100% 100% 2 [00014] 84% 100% 3 [00015] >95 >95%

[0088] The advantages of this method are as follows: [0089] the preparation of the catalyst requires a small amount of sodium hydroxide or other base. [0090] no base used during the reaction [0091] no need to bubble pure oxygen or make the reaction under pressure in the pure oxygen atmosphere. Our method works either in air or by bubbling air into the reaction medium [0092] the reaction is carried out at atmospheric pressure and with small amounts of Mn

Example 8: Epoxidation of Alkenes

[0093] The epoxidation of the alkenes may also be easily carried out from the industrial effluent in the presence of a co-oxidant such as hydrogen peroxide. The method may be advantageously compared to the methods of the literature.

[0094] General Procedure for the Epoxidation Reaction:

[0095] NaHCO.sub.3 (0.007 g, 0.09 mol, 5 eq), effluent 2 (0.26 mL (pH=3.5, Mn=12 ppm), 0.001 eq relative to Mn), t-BuOH or DMF (0.263 mL) and alkene (0.02 mol, 1 eq) at 30 C. in air. After stirring for 10 minutes, 30% H.sub.2O.sub.2 (0.016 mL, 0.17 mol, 10 eq) is added to the reaction mixture at 30 C. in air. The evolution of gas is observed after one minute. Stirring is continued for another four hours and then the reaction is cooled to room temperature. The product is extracted with dichloromethane and analyzed by GC MS.

[0096] The conversions are shown in Table 8.

TABLE-US-00008 TABLE 8 Epoxidation of alkenes Eco-PS2/ Eco- EcoMn** Substrate tBuOH PS2/DMF (DMF) literature Styrene 91% 91% Cyclooctene 81% 55% Cyclohexene 86% 89% Isoeugenol 0% 50%* Oxidative cleavage Pinene traces 100% 75% 40% (Qi, B. J. Mol. Cat. A 2010, 322, 73) Limonene traces 92% 43% Linalool traces 95% 63% Nopol traces 45% 74% *In the case of isoeugenol, GC-MS indicates the formation of a family of isoeugenol self-condensation products. The majority product appears to be Licarine A. **Eco-Mn derived from Mn accumulators of the genus Grevillea

[0097] The Eco-PS2 solids represent the catalysts prepared via the method of the invention.