WO2018222642A1 - Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène - Google Patents

Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène Download PDF

Info

Publication number
WO2018222642A1
WO2018222642A1 PCT/US2018/035010 US2018035010W WO2018222642A1 WO 2018222642 A1 WO2018222642 A1 WO 2018222642A1 US 2018035010 W US2018035010 W US 2018035010W WO 2018222642 A1 WO2018222642 A1 WO 2018222642A1
Authority
WO
WIPO (PCT)
Prior art keywords
dcp
pch
metal
oxidation state
reactor
Prior art date
Application number
PCT/US2018/035010
Other languages
English (en)
Inventor
Kyle Self
Michael Joseph WEISS
Ryan J. Gilliam
Thomas A. Albrecht
Original Assignee
Calera Corporation
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Calera Corporation filed Critical Calera Corporation
Priority to CN201880036582.5A priority Critical patent/CN110753679A/zh
Priority to EP18809606.9A priority patent/EP3630709A4/fr
Publication of WO2018222642A1 publication Critical patent/WO2018222642A1/fr

Links

Classifications

    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B3/00—Electrolytic production of organic compounds
    • C25B3/20—Processes
    • C25B3/27—Halogenation
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B15/00—Operating or servicing cells
    • C25B15/08—Supplying or removing reactants or electrolytes; Regeneration of electrolytes
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C17/00—Preparation of halogenated hydrocarbons
    • C07C17/013—Preparation of halogenated hydrocarbons by addition of halogens
    • C07C17/02—Preparation of halogenated hydrocarbons by addition of halogens to unsaturated hydrocarbons
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C29/00—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring
    • C07C29/09—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by hydrolysis
    • C07C29/12—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by hydrolysis of esters of mineral acids
    • C07C29/124—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by hydrolysis of esters of mineral acids of halides
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C29/00—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring
    • C07C29/64—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by simultaneous introduction of -OH groups and halogens
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C29/00—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring
    • C07C29/74—Separation; Purification; Use of additives, e.g. for stabilisation
    • C07C29/76—Separation; Purification; Use of additives, e.g. for stabilisation by physical treatment
    • C07C29/86—Separation; Purification; Use of additives, e.g. for stabilisation by physical treatment by liquid-liquid treatment
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/24—Halogens or compounds thereof
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/24—Halogens or compounds thereof
    • C25B1/26—Chlorine; Compounds thereof
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
    • C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
    • C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
    • C25B11/051—Electrodes formed of electrocatalysts on a substrate or carrier
    • C25B11/055—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the substrate or carrier material
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B3/00—Electrolytic production of organic compounds
    • C25B3/20—Processes
    • C25B3/23—Oxidation

Definitions

  • Polyurethane production remains one of the environmentally challenging manufacturing processes in industrial polymerization. Formed from addition reactions of di- isocyanates and polyols, polyurethanes may have a significant embedded environmental footprint because of the challenges associated with both feedstocks. Polyols are themselves polymerization derivatives which use propylene oxide as raw materials. Traditionally, propylene oxide (PO) may be synthesized from a chlorinated intermediate, propylene chlorohydrin. However, an environmentally acceptable process for the economic production of propylene oxide remains elusive. High costs of chlorine and significant waste water production (approximately 40 tonnes of waste water per tonne of PO) has caused
  • PCH propylene chlorohydrin
  • PO propylene oxide
  • methods to form PCH comprising:
  • methods to form PCH comprising:
  • methods to form PCH comprising:
  • methods to form PCH comprising:
  • the DCP as the extraction solvent is the DCP separated and recirculated from the same process and/or is DCP from other sources.
  • the amount of the DCP in the hydrolysis is between about 10-95% by volume.
  • the hydrolysis is catalyzed by presence of a nobel metal selected from ruthenium, rhodium, palladium, silver, osmium, iridium, platinum, gold, mercury, rhenium, titanium, niobium, tantalum, and combinations thereof.
  • a nobel metal selected from ruthenium, rhodium, palladium, silver, osmium, iridium, platinum, gold, mercury, rhenium, titanium, niobium, tantalum, and combinations thereof.
  • the hydrolysis is carried out in presence of metal hydroxychloride species of stoichiometry M x n+ Cl y (OH) (nx-y) , such as, for example only, Cu x Cl y (OH)(2 X - y ).
  • the method further comprises after extraction, transferring aqueous medium comprising the metal chloride with metal ions in the higher oxidation state and the lower oxidation state to the oxychlorination reaction and oxidizing the metal ion of the metal chloride from the lower oxidation state to the higher oxidation state in presence of the oxidant.
  • the oxidant is HCl and oxygen or hydrogen peroxide (or any other oxidant as described herein).
  • the method further comprises forming HCl by the hydrolysis of the DCP to the PCH; separating the HCl; and transferring the HCl to the oxychlorination reaction; and/or adding other HCl to the oxychlorination reaction.
  • the "other HCl" has been described herein.
  • the method further comprises recirculating the metal chloride with the metal ion in the higher oxidation state back to the chlorination reaction and/or the electrochemical reaction.
  • the method further comprises after extraction, transferring aqueous medium comprising the metal chloride with metal ion in the higher oxidation state and the lower oxidation state to the hydrolysis reaction.
  • the PCH is formed with selectivity of between about 20-100% by wt and/or more than 0.01 STY.
  • the method further comprises after hydrolysis, transferring organic medium comprising PCH and DCP to epoxidation; and epoxidizing the PCH with a base to form PO in presence of the DCP.
  • the base is selected from alkali metal hydroxide, alkali metal oxide, alkaline earth metal hydroxide, or alkaline earth metal oxide.
  • the base is a metal hydroxychloride species, such as copper hydroxychloride species of stoichiometry Cu x Cl y (OH)(2x- y) .
  • metal in the metal hydroxychloride is same as metal in the metal chloride.
  • the method further comprises forming the metal hydroxychloride by oxychlorinating the metal chloride with the metal ion in the lower oxidation state to the higher oxidation state in presence of water and oxygen.
  • the base is between about 5-38 wt%.
  • the reaction forms between about 5-42 or 5-40 tonnes of brine per tonne of PO.
  • the saltwater comprises alkali metal chloride or alkaline earth metal chloride.
  • metal ion in the metal chloride is selected from the group consisting of iron, chromium, copper, tin, silver, cobalt, uranium, lead, mercury, vanadium, bismuth, titanium, ruthenium, osmium, europium, zinc, cadmium, gold, nickel, palladium, platinum, rhodium, iridium, manganese, technetium, rhenium, molybdenum, tungsten, niobium, tantalum, zirconium, hafnium, and combination thereof.
  • the metal chloride is copper chloride.
  • the method further comprises adding other DCP to the chlorination; to the hydrolysis; and/or to the epoxidation for the extraction.
  • the other DCP is obtained from a traditional chlorohydrin process and/or from direct chlorination of propylene with chlorine.
  • the one or more products further comprise isopropanol and/or isopropyl chloride.
  • the method further comprises converting the isopropanol and/or the isopropyl chloride back to the propylene, DCP, and/or PCH.
  • systems to form PO comprising:
  • an electrochemical cell comprising an anode chamber comprising an anode and an anode electrolyte wherein the anode electrolyte comprises metal chloride and saltwater and the anode is configured to oxidize the metal chloride with metal ion in a lower oxidation state to a higher oxidation state; a cathode chamber comprising a cathode and a cathode electrolyte; and a voltage source configured to apply voltage to the anode and the cathode;
  • electrochemical cell and configured to obtain the anode electrolyte and chlorinate propylene with the anode electrolyte comprising the metal chloride with the metal ion in the higher oxidation state in the saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state;
  • a hydrolysis reactor operably connected to the chlorination reactor and configured to obtain the one or more products comprising DCP from the chlorination reactor with or without the saltwater comprising metal chloride and configured to hydrolyze the DCP to PCH;
  • an epoxidation reactor operably connected to the hydrolysis reactor and configured to obtain the solution comprising DCP and PCH and epoxidize the PCH to PO in presence of a base.
  • systems to form PO comprising:
  • an oxychlorination reactor configured to oxidize metal chloride with metal ion in lower oxidation state to higher oxidation state using an oxidant (oxidants have been described herein);
  • a chlorination reactor operably connected to the oxychlorination reactor and configured to obtain the metal chloride with the metal ion in the higher oxidation state and chlorinate propylene with the metal chloride with the metal ion in the higher oxidation state in the saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state;
  • a hydrolysis reactor operably connected to the chlorination reactor and configured to obtain the one or more products comprising DCP from the chlorination reactor with or without the saltwater comprising metal chloride and configured to hydrolyze the DCP to PCH; and
  • an epoxidation reactor operably connected to the hydrolysis reactor and configured to obtain the solution comprising DCP and PCH and epoxidize the PCH to PO in presence of a base.
  • systems to form PO comprising:
  • a chlorination reactor configured to chlorinate propylene with chlorine to result in one or more products comprising DCP
  • a hydrolysis reactor operably connected to the chlorination reactor and configured to obtain the one or more products comprising DCP from the chlorination reactor and configured to hydrolyze the DCP to PCH;
  • an epoxidation reactor operably connected to the hydrolysis reactor and configured to obtain the solution comprising DCP and PCH and epoxidize the PCH to PO in presence of a base.
  • system further comprises an oxychlorination reactor
  • oxidant comprising the HC1 and oxygen, or hydrogen peroxide (or any other oxidant known in the art).
  • the system further comprises the chlorination reactor and/or the hydrolysis reactor operably connected to a traditional chlorohydrin system and/or to another chlorination reactor chlorinating propylene with chlorine, and configured to obtain other DCP from the traditional chlorohydrin system and/or from the another chlorination reactor chlorinating propylene with chlorine.
  • a method to form propylene chlorohydrin comprising: chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt to result in one or more products comprising propylene chlorohydrin (PCH), and the metal chloride with the metal ion in lower oxidation state.
  • the one or more products further comprise 1,2-dichloropropane (DCP).
  • the method further comprises separating DCP from the aqueous medium and converting the DCP to the PCH.
  • the method further comprises hydro lyzing the DCP to the PCH in situ.
  • the method further comprises adding platinum or palladium to the aqueous medium to form PCH in yield of between about 10-100%.
  • the platinum or palladium is in concentration of between about 0.001-0.1M.
  • the method further comprises chlorinating propylene in presence of oxygen.
  • reaction conditions for the chlorination reaction comprise temperature between 20-150°C, pressure between 125- 350psig, or combination thereof.
  • the one or more products further comprise isopropanol and/or isopropyl chloride.
  • the method further comprises converting the isopropanol and/or the isopropyl chloride back to the propylene.
  • the one or more products further comprise hydrochloric acid (HC1).
  • the method further comprises after the chlorinating step,
  • the method further comprises recirculating the metal chloride in the higher oxidation state back to the chlorinating step.
  • the method further comprises reacting the PCH with a base to form propylene oxide (PO).
  • PO propylene oxide
  • the base is an alkali metal or alkaline earth metal hydroxide. In some embodiments of the foregoing aspect and embodiments, the base is metal hydroxychloride. In some embodiments of the foregoing aspect and embodiments, the base is an alkali metal or alkaline earth metal hydroxide. In some embodiments of the foregoing aspect and embodiments, the base is metal hydroxychloride. In some embodiments of the foregoing aspect and embodiments, the base is an alkali metal or alkaline earth metal hydroxide. In some embodiments of the foregoing aspect and embodiments, the base is metal hydroxychloride. In some embodiments of the foregoing aspect and
  • metal in the metal hydroxychloride is same as metal in the metal chloride.
  • the method further comprises forming the metal hydroxychloride by oxychlorinating the metal chloride with the metal ion in the lower oxidation state to the higher oxidation state in presence of water and oxygen.
  • the reaction further forms brine in water. In some embodiments of the foregoing aspect and embodiments, the reaction forms between about 5-45 or 5-42 tonnes of brine per tonne of PO.
  • a method to form propylene oxide (PO), comprising chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt to result in one or more products comprising between about 5- 99.9 wt% propylene chlorohydrin (PCH), and the metal chloride with the metal ion in lower oxidation state; and reacting the PCH with a base to form propylene oxide (PO) and brine in water, wherein the reaction forms between about 5-45 or 5-42 or 5-40 tonnes of brine per tonne of PO.
  • the base is between about 5-38 wt% or between about 5-35 wt% or between about 8-15 wt% sodium hydroxide or calcium hydroxide or calcium oxide (or any other base as described herein).
  • the method further comprises transferring the aqueous medium comprising the metal chloride with the metal ion in the lower oxidation state and the salt to an anode electrolyte in contact with an anode in an electrochemical cell and oxidizing the metal ion from the lower oxidation state to the higher oxidation state at the anode.
  • the method further comprises transferring the aqueous medium comprising the metal chloride with the metal ion in the lower oxidation state and the salt to an oxychlorination reaction and oxidizing the metal ion from the lower oxidation state to the higher oxidation state in the presence of HC1 and oxygen.
  • the salt comprises alkali metal chloride or alkaline earth metal chloride.
  • total amount of chloride content in the aqueous medium is between 3-15M or between 3-5M or between 3- 4M.
  • salt comprises sodium chloride
  • the metal chloride in the higher oxidation state is in range of 0.1-8M or between about 0.1-3 or between about 0.1-2.5M
  • the metal chloride in the lower oxidation state is in range of 0.1-2M
  • the sodium chloride is in range of 0.1-5M or between about 0.1-3M.
  • metal ion in the metal chloride is selected from the group consisting of iron, chromium, copper, tin, silver, cobalt, uranium, lead, mercury, vanadium, bismuth, titanium, ruthenium, osmium, europium, zinc, cadmium, gold, nickel, palladium, platinum, rhodium, iridium, manganese, technetium, rhenium, molybdenum, tungsten, niobium, tantalum, zirconium, hafnium, and combination thereof.
  • the metal chloride is copper chloride.
  • Fig. 1A is an illustration of some embodiments related to the methods and systems provided herein to form the PCH and the PO.
  • Fig. IB is an illustration of some embodiments related to the methods and systems provided herein to form the PCH and the PO.
  • Fig. 2 is an illustration of some embodiments related to the formation of products from chlorination of propylene.
  • FIG. 3 is an illustration of some embodiments related to the methods and systems provided herein to form the PCH and the PO.
  • FIG. 4 is an illustration of some embodiments related to the methods and systems provided herein to form the PCH and the PO.
  • Fig. 5 is an illustration of some embodiments related to the methods and systems provided herein to form the PCH and the PO.
  • [60] There are provided methods and systems that relate to the chlorination of propylene for the generation of one or more products comprising dichloropropane or 1,2- dichloropropane (DCP) and/or propylene chlorohydrin (PCH); hydrolysis of the DCP to the PCH; and further reaction of the PCH to form propylene oxide (PO).
  • the chlorination is done using metal chloride solution with metal ions in higher oxidation state.
  • separation/purification of the products from the metal ion solution regeneration of the metal chloride with metal ions in the higher oxidation state; recycling of the metal ion solution back to the chlorination reaction; and recycling of other side products.
  • Applicants have devised methods and systems to form the PCH and/or DCP in high yields and high selectivity where either the side products are not formed, or are formed in low yields, or are converted to the PCH, DCP, and/or propylene. Applicants have also devised methods and systems to convert the side products back either to the propylene or to the PCH such that the PCH is formed in high yield and with selectivity. Further Applicants have devised methods and systems to form the PO from the PCH in high yield and with high selectivity. Applicants have devised methods and systems to form the PO with reduced waste water, resulting in economical and environmentally friendly methods to form the PO.
  • FIG. 1A Illustrated in Fig. 1A is the block flow diagram for the formation of the PO from the propylene.
  • block 3 is shown an electrochemical reaction/cell where the metal ions of the metal halide in the lower oxidation state and the higher oxidation state are illustrated as CuCl x (a mixture of CuCl and CuCl 2 ).
  • Metal ions are oxidized from the lower oxidation state to the higher oxidation state at the anode where cathode reaction includes formation of sodium hydroxide.
  • cathode reaction are also possible and are explained in detail in US Patent Application No. 15/963,637, filed April 26, 2018, which is incorporated herein by reference in its entirety.
  • the cathode electrolyte comprises water and the cathode is an oxygen depolarizing cathode that reduces oxygen and water to hydroxide ions;
  • the cathode electrolyte comprises water and the cathode is a hydrogen gas producing cathode that reduces water to hydrogen gas and hydroxide ions;
  • the cathode electrolyte comprises hydrochloric acid and the cathode is a hydrogen gas producing cathode that reduces hydrochloric acid to hydrogen gas; or the cathode electrolyte comprises hydrochloric acid and the cathode is an oxygen depolarizing cathode that reacts hydrochloric acid and oxygen gas to form water.
  • metal ion or “metal” or “metal ion in the metal chloride” or “metal ion in the metal halide” as used herein, includes any metal ion capable of being converted from lower oxidation state to higher oxidation state and vice versa.
  • metal ions in the metal halide include, but are not limited to, iron, chromium, copper, tin, silver, cobalt, uranium, lead, mercury, vanadium, bismuth, titanium, ruthenium, osmium, europium, zinc, cadmium, gold, nickel, palladium, platinum, rhodium, iridium, manganese, technetium, rhenium, molybdenum, tungsten, niobium, tantalum, zirconium, hafnium, and combination thereof.
  • the metal ions include, but are not limited to, iron, copper, tin, chromium, or combination thereof.
  • the metal ion is copper. In some embodiments, the metal ion is tin. In some embodiments, the metal ion is iron. In some embodiments, the metal ion is chromium. In some embodiments, the metal ion is platinum.
  • metal halide includes metal chlorides such as, but not limited to, copper chloride (CuCl with Cu in the lower oxidation state of 1 and CuCl 2 with Cu in the higher oxidation state of 2).
  • the "salt” or “saltwater” includes salt or salt in water where salt can be any alkali metal chloride or alkaline earth metal chloride, including but not limited to, sodium chloride, potassium chloride, lithium chloride, calcium chloride, magnesium chloride etc.
  • the metal chloride with the metal ion in the lower oxidation state and the metal chloride with the metal ion in the higher oxidation state are both present in the aqueous medium in the electrochemical reaction/cell and the chlorination reaction/reactor. Owing to the reduction of the metal chloride from the higher oxidation state to the lower oxidation state in the chlorination reaction, the ratio of the metal chloride in the lower and the higher oxidation state are different in the aqueous medium entering the chlorination reaction and exiting the chlorination reaction. Suitable concentrations of the metal ions in the lower and higher oxidation state in the aqueous medium have been described herein.
  • Some examples of the metal chlorides that may be used in the systems and methods include, but are not limited to, copper chloride, iron chloride, tin chloride, chromium chloride, zinc chloride, etc.
  • PCH polypropylene chlorohydrin
  • PCH in its isomeric form, such as, l-chloro-2-propanol, 2-chloro-l-propanol, or both.
  • both isomers may be formed and both may be subsequently converted to the PO.
  • the explicit declaration of one isomer may not be construed as the absence of the other.
  • some of the Cu(I) produced in block 1 is regenerated using chemical oxidation in oxychlorination reaction/reactor using oxidants such as, but not limited to, X 2 gas alone; or HX gas and/or HX solution in combination with gas comprising oxygen or ozone; or hydrogen peroxide; or HXO or salt thereof; or HXO 3 or salt thereof; or HXO 4 or salt thereof; or combinations thereof, wherein each X independently is a halogen selected from fluorine, chlorine, iodine, and bromine.
  • chlorine gas may be used to oxidize the metal halide from the lower to the higher oxidation state.
  • CuCl may be oxidized to CuCl 2 in the presence of chlorine gas as follows:
  • the oxidant is HCl gas and/or HCl solution in combination with gas comprising oxygen.
  • An example is as follows:
  • the oxidant is HX gas and/or HX solution in combination with hydrogen peroxide, wherein X is a halogen.
  • HX gas and/or HX solution in combination with hydrogen peroxide wherein X is a halogen.
  • X is a halogen.
  • HCl Hydrochloric acid
  • the methods and systems provided herein can leverage the HCl in the oxychlorination step as a mechanism to provide additional copper oxidation.
  • the HCl can also be sourced from other reactions and is labeled as "other HCl" in figures.
  • the incorporation of HCl from chlorination reaction or other reactions may lead to additional PO production by upgrading these streams to more valuable products.
  • the reuse of the HCl in oxychlorination process allows for the reduction of the base consumption to neutralize the acid which may improve overall economics, especially in cases where the base could otherwise be sold.
  • electrochemical reaction, chlorination reaction, and the oxychlorination reaction may each be individually carried out or may be in combination with one or more other processes.
  • the electrochemically generated CuCl 2 may be used in one reactor for the chlorination of the propylene to the PCH and/or the DCP and the chemically generated CuCl 2 (via oxychlorination) may be used in another propylene chlorination reactor each with the option of making the PCH directly or making the DCP with subsequent conversion to the PCH, all such configurations are within the scope of the present disclosure.
  • the oxychlorination reaction/reactor oxidizes the metal ion of the metal chloride in the lower oxidation state to the higher oxidation state in the presence of the oxidant (and in the absence of any electrochemical reaction/cell) and then the metal chloride with the metal ion in the higher oxidation state is then transferred to the chlorination reaction/reactor to chlorinate propylene, as illustrated in Fig. IB.
  • block 2 is shown an oxychlorination reaction/reactor where the metal ions of the metal halide in the lower oxidation state and the higher oxidation state are illustrated as CuCl x (a mixture of CuCl and CuCl 2 ).
  • Metal ions are oxidized from the lower oxidation state to the higher oxidation state in the oxychlorination reaction/reactor.
  • reaction/reactor containing CuCl x is then transferred to the chlorination reaction/reactor shown in block 1.
  • the propylene C 3 H 6 is converted into the DCP and/or the PCH using copper chloride (II), simultaneously reducing two Cu(II) ions to Cu(I).
  • II copper chloride
  • the electrochemical reaction/cell and the oxychlorination reaction/reactor may independently be carried out for the oxidation of the metal chloride (such as Fig. IB for the oxychlorination reaction/reactor) or may be carried out in combination (such as Fig. 1A).
  • methods that include chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt under reaction conditions to result in one or more products comprising PCH, and the metal chloride with the metal ion in lower oxidation state.
  • the chlorination reaction may take place after the electrochemical reaction and/or the oxychlorination reaction.
  • methods that include (i) contacting an anode with an anode electrolyte in an electrochemical cell wherein the anode electrolyte comprises metal chloride and saltwater; contacting a cathode with a cathode electrolyte in the electrochemical cell; applying voltage to the anode and the cathode and oxidizing the metal chloride with metal ion in a lower oxidation state to a higher oxidation state at the anode; and (ii) withdrawing the anode electrolyte from the electrochemical cell and chlorinating propylene with the anode electrolyte comprising the metal chloride with the metal ion in the higher oxidation state in the saltwater under reaction conditions to result in one or more products comprising PCH and the metal chloride with the metal ion in the lower oxidation state.
  • methods that include (i) oxidizing metal chloride with metal ion in a lower oxidation state to a higher oxidation state in presence of an oxidant in an oxychlorination reaction; and (ii) withdrawing the metal chloride with metal ion in the higher oxidation state from the oxychlorination reaction and chlorinating propylene with the metal chloride with the metal ion in the higher oxidation state in saltwater under reaction conditions to result in one or more products comprising PCH and the metal chloride with the metal ion in the lower oxidation state.
  • the methods further include (iii) epoxidizing the PCH with a base to form PO.
  • the propylene may be supplied under pressure in the liquid phase and/or the gas phase and the metal chloride, for example only, copper (II) chloride (also containing copper (I) chloride) is supplied in an aqueous solution such as saltwater.
  • the reaction may occur in the liquid phase where the dissolved propylene reacts with the copper (II) chloride.
  • the chlorination of the propylene in the presence of the metal chloride with the metal ion in the higher oxidation state e.g.
  • CuCl 2 may result in one or more products such as, but not limited to, PCH, DCP, isopropanol, and isopropyl chloride.
  • Applicants have found that in order to form the PCH in high space time yield (to minimize reactor costs) with high selectivity (to minimize propylene costs) certain reactions conditions may be controlled and used.
  • reaction conditions include, but are not limited to, temperature and pressure in the chlorination reaction; use of the other DCP; use of metal hydroxychloride; amount of salt; amount of total chloride content; residence time of the chlorination mixture; presence of a noble metal; etc.
  • the PCH is formed with selectivity of between about 20-100%; or between about 20-90%; or between about 20-80%; or between about 20-70%; or between about 20-60%; or between about 20- 50%; or between about 20-40%; or between about 30-100%; or between about 30-90%; or between about 30-80%; or between about 30-70%; or between about 30-60%; or between about 30-50%; or between about 30-40%; or between about 40-100%; or between about 40- 90%; or between about 40-80%; or between about 40-70%; or between about 40-60%; or between about 40-50%; or between about 75-100%; or between about 75-90%; or between about 75-80%; or between about 90-100%; or between about 90-99%; or between about 90- 95%.
  • the above noted selectivity is in wt%.
  • the STY (space time yield) of the one or more products from propylene and/or DCP e.g. the STY of PCH is 0.01, or 0.05, or less than 0.1, or more than 0.1, or more than 0.5, or is 1, or more than 1, or more than 2, or more than 3, or more than 4, or between 0.01-0.05, or between 0.01-0.1, or between 0.1-3, or between 0.5-3, or between 0.5-2, or between 0.5-1, or between 3-5.
  • the STY is yield per time unit per reactor volume.
  • the yield of product may be expressed in mol, the time unit in hour and the volume in liter.
  • the volume may be the nominal volume of the reactor, e.g.
  • the STY may also be expressed as STY based on the amount of propylene consumed and/or based on amount of the DCP consumed to form the product.
  • the STY of the PCH product may be deduced from the amount of propylene consumed and/or based on amount of the DCP consumed during the reaction.
  • the selectivity may be the mol of product, e.g. PCH/mol of the propylene consumed and/or PCH/mol of the DCP consumed.
  • the yield may be the amount of the product isolated.
  • the purity may be the amount of the product/total amount of all products (e.g., amount of PCH/all the organic products formed).
  • the "other DCP” or “other sources of DCP” as mentioned herein (and illustrated in figures) includes DCP formed as a by-product of other processes.
  • the other processes or sources include, but are not limited to, the traditional chlorohydrin route to the PO or the DCP formed by the chlorination of the propylene with chlorine.
  • This stream is labeled as "other DCP” in figures, which illustrates the various locations in the process where this stream may be incorporated into the process.
  • the incorporation of this other DCP can lead to additional PCH and PO production by upgrading these streams to more valuable products.
  • the PCH may be formed through the addition of hypochlorous acid (HOC1) to the propylene.
  • HOC1 may itself be formed by the addition of chlorine (Cl 2 ) to water, a reaction which co-produces a stoichiometric amount of hydrochloric acid (HC1).
  • the reactor may be operated under very dilute concentrations of HOC1 and with an equivalent of base (in the form of NaOH or CaO) to neutralize the HC1. Even under these conditions, the formation of unwanted DCP can be significant, representing a propylene selectivity loss on the order of 10%. This unwanted DCP can be used as the other DCP in the methods described herein and provide an economic use of a waste stream.
  • Another source of DCP is the production of the DCP through the direct addition of chlorine to the propylene.
  • New or existing sources of chlorine such as, but not limited to, Deacon process and the chlor-alkali process
  • This DCP formed via direct chlorination may then be converted to the PCH using methods provided herein and ultimately form the PO.
  • the HC1 formed as a by-product from the conversion to the PCH would then be captured and reused.
  • Such methods and systems for other sources of DCP may be integrated with the methods and systems provided herein to hydro lyze the DCP formed as a major product or as a waste stream to the PCH and then to the PO.
  • reaction conditions for the chlorination reaction comprise temperature between 100-150°C, pressure between 125-350 psig, or combination thereof.
  • the methods to form PCH comprise reaction conditions, such as, but not limited to, use of metal hydroxychloride.
  • metal chloride may react with water and oxygen to form metal hydroxychloride species of stoichiometry M x n+ Cl y (OH) (nx-y) , M x Cl y (OH) (2x-y) , M x Cl y (OH) (3x-y) or M x Cl y (OH) (4x-y) , where M is the metal ion.
  • An illustration of the reaction is as shown below (VII) taking copper chloride as an example:
  • CuClOH species represents one of many possible copper hydroxychloride species of stoichiometry Cu x Cl y (OH) (2x-y) . If in reaction with the propylene, the CuCl 2 is replaced (e.g. at least partially) by a hydroxychloride, the following reaction (VIII) may take place:
  • This reaction may allow for improved selectivity for the PCH vs. the other products the DCP.
  • the reaction with the oxygen to form the metal hydroxychloride species of stoichiometries as noted above, may occur in a reactor separate from the chlorination reactor or may occur in the chlorination reactor during the chlorination of the propylene.
  • Other examples of the metal hydroxychloride without limitation include, MoCl(OH)3,
  • the reaction conditions in the methods to form the PCH comprise chlorinating in between about l-30wt% salt.
  • the salt may be between l-30wt%; or between 5-30wt% salt; or between about 8- 30wt%; or between 10-30wt%; or between 15-30wt%; r between 20-30wt%; or between 5- 10wt%.
  • Salt as used herein includes its conventional sense to refer to a number of different types of salts including, but not limited to, alkali metal chlorides such as, sodium chloride, potassium chloride, lithium chloride, cesium chloride, etc.; alkaline earth metal chlorides such as, calcium chloride, strontium chloride, magnesium chloride, barium chloride, etc; or ammonium chloride.
  • alkali metal chlorides such as, sodium chloride, potassium chloride, lithium chloride, cesium chloride, etc.
  • alkaline earth metal chlorides such as, calcium chloride, strontium chloride, magnesium chloride, barium chloride, etc; or ammonium chloride.
  • the salt comprises alkali metal chloride or alkaline earth metal chloride.
  • the salt (for example only, sodium chloride or calcium chloride) in the chlorination includes between about l-30wt% salt; or between l-25wt% salt; or between l-20wt% salt; or between l-10wt% salt; or between 5-30wt% salt; or between 5-20wt% salt; or between 5-10wt% salt; or between about 8-30wt% salt; or between about 8-25wt% salt; or between about 8-20wt% salt; or between about 8-15wt% salt; or between about 10-30wt% salt; or between about 10- 25wt% salt; or between about 10-20wt% salt; or between about 10-15wt% salt; or between about 15-30wt% salt; or between about 15-25wt% salt; or between about 15-20wt% salt; or between about 20-30wt% salt; or between about 20-25wt% salt.
  • the aqueous medium for the chlorination reaction may contain between 5-50%; or 5-40%; or 5-30%; or 5-20%; or 5-10%; or 50-75%; or 50-70%; or 50- 65%; or 50-60% by weight of water in the aqueous medium depending on the amount of salt and the metal halide.
  • the reaction conditions in the methods to form the PCH comprise chlorinating in aquoeus medium with total chloride content of between about 10-30 wt%.
  • the total chloride content is a combination of chloride from the metal chloride as well as the chloride from the salt.
  • the reaction conditions in the methods to form the PCH comprise varying the incubation time or residence time or mean residence time of the chlorination mixture.
  • the "incubation time” or “residence time” or “mean residence time” as used herein includes the time period for which the chlorination mixture is left in the reactor at the above noted temperatures before being taken out for the separation of the product.
  • the residence time for the chlorination mixture is few seconds or between about lsec-lhour; or lsec-lOhours; or lOmin-lOhours or more depending on the temperature of the chlorination mixture.
  • This residence time may be in combination with other reaction conditions such as, e.g. the temperature ranges and/or total chloride concentrations provided herein.
  • the residence time for the chlorination mixture is between about lsec-3hour; or between about lsec-2.5hour; or between about lsec-2hour; or between about lsec-1.5hour; or between about lsec-lhour; or 10min-3hour; or between about lOmin- 2.5hour; or between about 10min-2hour; or between about 10min-1.5hour; or between about lOmin-lhour; or between about 10min-30min; or between about 20min-3hour; or between about 20min-2hour; or between about 20min-lhour; or between about 30min-3hour; or between about 30min-2hour; or between about 30min-lhour; or between about lhour-2hour; or between about lhour-3hour; or between about 2hour-3hour, to form the PCH as noted herein.
  • the reaction conditions in the methods to form the PCH include carrying out the chlorination in the presence of a noble metal.
  • the "noble metal" as used herein includes metals that are resistant to corrosion in moist conditions.
  • the noble metals are selected from ruthenium, rhodium, palladium, silver, osmium, iridium, platinum, gold, mercury, rhenium, titanium, niobium, tantalum, and combinations thereof.
  • the noble metal is selected from rhodium, palladium, silver, platinum, gold, titanium, niobium, tantalum, and combinations thereof.
  • the noble metal is palladium, platinum, titanium, niobium, tantalum, or combinations thereof.
  • the foregoing noble metals may be present in 0, +2 or +4 oxidation states as appropriate.
  • platinum or palladium may be present as metal or as a metal over carbon or may be present as PtCl 2 or PdCl 2 etc.
  • the foregoing noble metal is supported on a solid. Examples of solid support include, without limitation, carbon, zeolite, titanium dioxide, alumina, silica, and the like.
  • the foregoing noble metal is supported on carbon.
  • the catalyst is palladium or palladium over carbon.
  • the amount of nobel metal used in the chlorination reaction is between 0.001M to 2M; or between 0.001-1.5M; or between about 0.001- 1M; or between about 0.001-0.5M; or between about 0.001-0.05M; or between 0.01- 2M; or between 0.01-1.5M; or between 0.01- 1M; or between 0.01-0.5M; or between 0.1-2M; or between 0.1-1.5M; or between 0.1- 1M; or between 0.1-0.5M; or between 1-2M.
  • the method to form the PCH further comprises adding platinum or palladium to the aqueous medium.
  • the platinum or palladium is in concentration of between about 0.001-0.1M.
  • total amount of chloride content in the aqueous medium is between 4-15M or 4-10M.
  • the aqueous medium in the chlorination reaction comprises the metal chloride in the higher oxidation state in range of 0.1-5M or 1-5M, or 1.5- 5M, the metal chloride in the lower oxidation state in range of 0.1 -2M, and the sodium chloride in range of 0.1-5M or 1-5M.
  • DCP may be another product formed after the chlorination of propylene.
  • the "1,2-dichloropropane” or “dichloropropane” or “propylene dichloride” or “DCP” or “PDC” can be used interchangeably.
  • the DCP may be formed as a major product and in one aspect, there are provided methods and systems to convert the DCP to the PCH in the same or a separate reactor.
  • methods that include chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt under reaction conditions to result in one or more products comprising DCP, and the metal chloride with the metal ion in lower oxidation state; and hydrolyzing the DCP to PCH.
  • the one or more products further comprise PCH.
  • the method comprises one or more of (A) hydrolyzing the DCP to the PCH in situ; (B) separating the DCP from the aqueous medium and/or from the PCH (when both DCP and PCH are formed in the chlorination reaction) and hydrolyzing the DCP to the PCH; and/or (C) hydrolyzing the DCP to the PCH without the separation of the DCP from the PCH and/or from the aqueous medium, to increase the yield of the PCH.
  • the electrochemical reaction/cell, the chlorination reaction/reactor, the oxychlorination reaction/reactor, the hydrolysis reaction/reactor, and the epoxidation reaction/reactor are all illustrated in Fig. 3.
  • the chlorination reaction may take place after the electrochemical reaction and/or the oxychlorination reaction.
  • methods that include (i) contacting an anode with an anode electrolyte in an electrochemical cell wherein the anode electrolyte comprises metal chloride and saltwater; contacting a cathode with a cathode electrolyte in the electrochemical cell; applying voltage to the anode and the cathode and oxidizing the metal chloride with metal ion in a lower oxidation state to a higher oxidation state at the anode; (ii) withdrawing the anode electrolyte from the electrochemical cell and chlorinating propylene with the anode electrolyte comprising the metal chloride with the metal ion in the higher oxidation state in the saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state; and (iii) hydrolyzing the DCP
  • methods that include (i) oxidizing metal chloride with metal ion in a lower oxidation state to a higher oxidation state in presence of an oxidant in an oxychlorination reaction; (ii) withdrawing the metal chloride with metal ion in the higher oxidation state from the oxychlorination reaction and chlorinating propylene with the metal chloride with metal ion in the higher oxidation state in saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state; and (iii) hydrolyzing the DCP to the PCH.
  • the one or more products further comprise PCH.
  • the method further comprises one or more of (A) hydrolyzing the DCP to the PCH in situ; (B) separating the DCP from the aqueous medium and/or from the PCH and then hydrolyzing the DCP to the PCH; and/or (C) hydrolyzing the DCP to the PCH without the separation of the DCP from the PCH and/or the aqueous medium, to increase the yield of the PCH.
  • the methods further include (iv) epoxidizing the PCH with a base to form PO.
  • a system comprising (i) an electrochemical cell comprising an anode chamber comprising an anode and an anode electrolyte wherein the anode electrolyte comprises metal chloride and saltwater and anode is configured to oxidize metal chloride with metal ion in a lower oxidation state to a higher oxidation state; a cathode chamber comprising a cathode and a cathode electrolyte; and a voltage source configured to apply voltage to the anode and the cathode; (ii) a chlorination reactor operably connected to the anode chamber of the electrochemical cell and configured to obtain the anode electrolyte and chlorinate propylene with the anode electrolyte comprising the metal chloride with the metal ion in the higher oxidation state in the saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state; (iii) a
  • the system further comprises an oxychlorination reactor operably connected to the chlorination reactor and/or the electrochemical cell, and the hydrolysis reactor and configured to obtain aqueous medium from the chlorination reactor and/or the electrochemical cell comprising the metal chloride with metal ion in the lower oxidation state and the higher oxidation state and obtain HC1 produced in the hydrolysis reactor and configured to oxidize the metal chloride with metal ion in the lower oxidation state to the higher oxidation state using an oxidant comprising the HC1 and oxygen, or hydrogen peroxide (or any other oxidant as described herein).
  • an oxychlorination reactor operably connected to the chlorination reactor and/or the electrochemical cell, and the hydrolysis reactor and configured to obtain aqueous medium from the chlorination reactor and/or the electrochemical cell comprising the metal chloride with metal ion in the lower oxidation state and the higher oxidation state and obtain HC1 produced in the hydrolysis reactor and configured to oxidize the metal chloride with metal
  • the oxychlorination reactor is used independent of the electrochemical cell.
  • a system comprising (i) oxychlorination reactor configured to oxidize metal chloride with metal ion in lower oxidation state to higher oxidation state using an oxidant comprising HC1 and oxygen, or hydrogen peroxide (or any other oxidant as described herein); (ii) a chlorination reactor operably connected to the oxychlorination reactor and configured to obtain the metal chloride with the metal ion in the higher oxidation state and chlorinate propylene with the metal chloride with the metal ion in the higher oxidation state in saltwater to result in one or more products comprising DCP and the metal chloride with the metal ion in the lower oxidation state; (iii) a hydrolysis reactor operably connected to the chlorination reactor and configured to obtain the one or more products comprising DCP from the chlorination reactor with or without the saltwater comprising metal chloride and configured to hydro
  • the oxychlorination reactor is also operably connected to the chlorination reactor and the hydrolysis reactor and is configured to obtain the aqueous medium from the chlorination reactor comprising the metal chloride with metal ion in the lower oxidation state and the higher oxidation state and is configured to obtain HC1 produced in the hydrolysis reactor.
  • the conversion of the DCP to the PCH is a hydrolysis reaction:
  • the reaction conditions listed in the foregoing section also aid in (A) the hydrolysis of the DCP to the PCH in situ (e.g. during chlorination reaction in the chlorination reactor).
  • the DCP may be hydrolyzed to the PCH in situ by increasing the available free water during the reaction. Because water is a reactant in the hydrolysis of the DCP to the PCH, the presence of free water may lead to the conversion of the DCP to the PCH.
  • the DCP may be formed in high yield and may then be hydrolyzed to the PCH (B and C above).
  • some amount of PCH may be formed in the chlorination reaction which may or may not be separated from the DCP.
  • the high concentrations of salt may be accomplished through the addition of the copper chloride salts (such as CuCl 2 , CuCl or in combination) or through other salts such as NaCl.
  • There are also a number of process conditions which can be optimized to provide higher STY and better selectivity for the DCP production including temperature, pressure (e.g. pressures under which the propylene may form a liquid or supercritical phase), and residence time.
  • the conversion of the DCP to the PCH may be executed in a second reaction step downstream (in a separate reactor) of the propylene chlorination, illustrated as the hydrolysis reactor in Fig. 3.
  • the DCP may be hydrolyzed to the PCH by (B) separating the DCP from the aqueous medium and/or from the PCH (when both DCP and PCH are formed in the chlorination reaction) and then hydrolyzing the DCP to the PCH; and/or (C) hydro lyzing the DCP to the PCH without the separation of the DCP from the PCH and/or the aqueous medium, to increase the yield of the PCH.
  • the hydrolysis of the DCP to the PCH may utilize the aqueous stream leaving the chlorination reaction/reactor (containing the aqueous metal chloride, e.g. aqueous copper chloride) as part of a circulating loop (embodiment C above related to hydrolysis without the separation of the DCP from the aqueous medium).
  • Illustrated in Fig. 3 is the aspect where the DCP is converted to the PCH in a hydrolysis reaction/reactor after the chlorination reaction/reactor.
  • Fig. 3 illustrates that the chlorination is divided among two reaction blocks.
  • Block 1 effects propylene chlorination to one or more products comprising the DCP (and optionally the PCH too).
  • Block 5 in Fig. 3 uses the aqueous copper chloride stream from block 1 and hydrolyzes the DCP to the PCH.
  • the process may recover at least some of the HC1 byproduct from the hydrolysis of the DCP to the PCH (equations IX and X above).
  • This HC1 can be reused in a traditional oxychlorination reaction for the production of ethylene dichloride (EDC) or used in the oxychlorination unit 2 within the process to generate additional PO.
  • EDC ethylene dichloride
  • the method comprises (B) separating the DCP from the aqueous medium and/or from the PCH and then hydro lyzing the DCP to the PCH.
  • a separation step takes place between the chlorination and the hydrolysis.
  • methods to form PCH comprising: (i) contacting an anode with an anode electrolyte in an electrochemical cell wherein the anode electrolyte comprises metal chloride and saltwater; contacting a cathode with a cathode electrolyte in the electrochemical cell; applying voltage to the anode and the cathode and oxidizing the metal chloride with metal ion in a lower oxidation state to a higher oxidation state at the anode; (ii) withdrawing the anode electrolyte from the electrochemical cell and chlorinating propylene in the anode electrolyte comprising metal chloride with metal ion in higher oxidation state and the saltwater to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) separating the PCH from the aqueous medium; and (iv) treating the aqueous medium comprising the metal chloride with
  • methods to form PCH comprising: (i) oxidizing metal chloride with metal ion in a lower oxidation state to a higher oxidation state in presence of an oxidant in an oxychlorination reaction; (ii) withdrawing the metal chloride with metal ion in the higher oxidation state from the oxychlorination reaction and chlorinating propylene with the metal chloride with the metal ion in the higher oxidation state in saltwater under reaction conditions to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) separating the PCH from the aqueous medium; and (iv) treating the aqueous medium comprising the metal chloride with metal ions in the higher oxidation state and the lower oxidation state and the DCP with water to hydrolyze the DCP to the PCH.
  • the methods further include (v) epoxidizing the PCH with a base to form propylene oxide (PO).
  • the PCH may be separated from the aqueous stream using various separation techniques, including, but not limited to, reactive separation, distillation, molecular sieve, membrane, etc.
  • both the DCP and the PCH are separated from the aqueous stream and the DCP is hydrolyzed to the PCH in the absence of the metal salts used in the chlorination of the propylene (e.g. metal chlorides used in the chlorination of propylene).
  • the metal salts used in the chlorination of the propylene e.g. metal chlorides used in the chlorination of propylene.
  • methods to form PCH comprising: (i) contacting an anode with an anode electrolyte in an electrochemical cell wherein the anode electrolyte comprises metal chloride and saltwater; contacting a cathode with a cathode electrolyte in the electrochemical cell; applying voltage to the anode and the cathode and oxidizing the metal chloride with metal ion in a lower oxidation state to a higher oxidation state at the anode; (ii) withdrawing the anode electrolyte from the electrochemical cell and chlorinating propylene in the anode electrolyte comprising metal chloride with metal ion in higher oxidation state to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) separating organics comprising the PCH and the DCP from the aqueous medium comprising the metal chloride with metal ions in the higher
  • methods to form PCH comprising: (i) oxidizing metal chloride with metal ion in a lower oxidation state to a higher oxidation state in presence of an oxidant in an oxychlorination reaction; (ii) withdrawing the metal chloride with metal ion in the higher oxidation state from the oxychlorination reaction and chlorinating propylene with the metal chloride with the metal ion in the higher oxidation state in saltwater under reaction conditions to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) separating organics comprising the PCH and the DCP from the aqueous medium comprising the metal chloride with metal ions in the higher oxidation state and the lower oxidation state; and (iv) hydro lyzing the DCP (also containing PCH) with water to form the PCH.
  • the DCP is separated from the PCH before the hydrolysis step.
  • the method further includes (v) epoxidizing the PCH with a base to form propylene oxide (PO).
  • the hydrolysis step forms HC1 and the method further comprises recirculating the HC1 to the oxychlorination step (illustrated in Fig. 3) where the metal chloride with the metal ion in the lower oxidation state is converted to the metal chloride with the metal ion in the higher oxidation state in presence of the HC1 and oxygen, or hydrogen peroxide, or any other oxidant described herein.
  • the chlorination reaction may be run in reaction conditions, such as, at elevated temperatures and at lower metal chloride concentration.
  • both the PCH and the DCP may be separated from the aqueous medium comprising metal chloride as stated above.
  • the step of separating the one or more products comprising DCP from the chlorination reaction comprises any separation method known in the art.
  • the one or more products comprising DCP and optionally the PCH may be separated from the chlorination reaction as a vapor stream.
  • the separated vapors may be cooled and/or compressed and subjected to the hydrolysis reaction.
  • Other separation methods include, without limitation, distillation and/or flash distillation using the distillation column or flash distillation column.
  • the remaining one or more products comprising DCP and optionally the PCH in the aqueous medium may be further separated using methods such as, decantation, extraction, or combination thereof.
  • Various examples of the separation methods are described in detail in US Patent Application No. 14/446,791, filed July 30, 2014, which is incorporated herein by reference in its entirety.
  • the DCP may be used as an extraction solvent that extracts DCP and the PCH from the aqueous stream from the chlorination reaction/reactor.
  • the DCP used as the extraction solvent can be DCP from the same process that has been separated and recirculated and/or is the other DCP.
  • the "other DCP" has been described herein.
  • the extraction solvent can be any organic solvent that removes DCP and/or the PCH from the aqueous metal ion solution.
  • the use of DCP as the extraction solvent may ensure that the hydrolysis reaction, which occurs in an aqueous solution with metal chlorides (aspect above) or without metal chlorides (another aspect above), can have the maximum rate as the aqueous medium can be saturated with the DCP.
  • the DCP may be present in excess amount in order to facilitate efficient hydrolysis.
  • the mol% of the DCP is equal to or greater than the mol% of the PCH.
  • the DCP may be as high as 10-95% by volume; or 10-90% by volume; or 10-80% by volume; or 10-70% by volume; or 10-60% by volume; or 10-50% by volume; or 10-40% by volume; or 10-30% by volume; or 10-20% by volume, of the total solution volume.
  • the DCP can form a second organic phase which may help ensure that a soluble concentration of DCP remains in the aqueous phase.
  • further degradation of the PCH into other products such as, but not limited to, acetone and/or propylene glycol
  • the PCH may be removed from the reactor in the organic phase with the un-reacted DCP. This last advantage may alleviate the need to separate the PCH from the aqueous solution by other techniques such as distillation.
  • the PCH can be removed from the chlorination reactor by removing the DCP layer that is phase- separated from the aqueous layer.
  • Fig. 4 illustrates an example of the use of the DCP as an extracting solvent.
  • the recirculating DCP stream serves to extract the PCH both from the propylene chlorination reactor (block 1) and the hydrolysis reactor (block 5).
  • the PCH recovered from these reactors along with the DCP may be then sent to epoxidation, where the PCH is converted to the PO and the DCP stream is recirculated.
  • any DCP made in the propylene chlorination reactor may be balanced by conversion to the PCH in the hydrolysis reactor.
  • the extracting solvent as shown in Fig. 4 can flow either clockwise or counterclockwise. The order of operations may be determined by process economics.
  • the epoxidation of the PCH to the PO in the presence of the DCP has been described below in detail.
  • the DCP as the extraction solvent is the DCP separated and recirculated from the same process (as illustrated in Fig. 4) and/or is other DCP from other sources.
  • the process using the other DCP is as illustrated in Fig. 5.
  • new or existing sources of chlorine to make the DCP via direct chlorination of propylene shown as block 7 in Fig. 5, is connected to the chlorination reactor and/or the hydrolysis reactor for the DCP to be converted to the PCH and ultimately to the PO.
  • the HC1 formed as a byproduct from the conversion to the PCH would then be captured and reused.
  • the direct chlorination reactor such as traditional chlorohydrin process and/or direct chlorination of propylene with chlorine may replace or supplement the electrochemical and/or the oxychlorination processes provided herein (oxychlorination shown as block 2 in Fig. 5).
  • methods to form PCH comprising: (i) contacting an anode with an anode electrolyte in an electrochemical cell wherein the anode electrolyte comprises metal chloride and saltwater; contacting a cathode with a cathode electrolyte in the electrochemical cell; applying voltage to the anode and the cathode and oxidizing the metal chloride with metal ion in a lower oxidation state to a higher oxidation state at the anode; (ii) withdrawing the anode electrolyte from the electrochemical cell and chlorinating propylene in the anode electrolyte comprising metal chloride with metal ion in higher oxidation state to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) extracting the one or more products comprising PCH and DCP from the aqueous medium by extracting with DCP as an extraction
  • methods to form PCH comprising: (i) oxidizing metal chloride with metal ion in a lower oxidation state to a higher oxidation state in presence of an oxidant in an oxychlorination reaction; (ii) withdrawing the metal chloride with metal ion in the higher oxidation state from the oxychlorination reaction and chlorinating propylene with the metal chloride with the metal ion in the higher oxidation state in saltwater under reaction conditions to result in one or more products comprising PCH and DCP, and the metal chloride with the metal ion in lower oxidation state; (iii) extracting the one or more products comprising PCH and DCP from the aqueous medium by extracting with DCP as an extraction solvent; and (iv) hydrolyzing the DCP with water to form the PCH.
  • the anode electrolyte withdrawn from the electrochemical cell and/or the metal chloride with metal ion in the higher oxidation state withdrawn from the oxychlorination reaction comprise both the metal chloride with the metal ion in the lower oxidation state as well as the metal chloride with the metal ion in the higher oxidation state (e.g. CuCl x ).
  • the method further includes after extraction, transferring aqueous medium comprising the metal chloride with metal ions in the higher oxidation state and the lower oxidation state to the oxychlorinating reaction/reactor; to the hydrolysis reaction/reactor; to the chlorination reaction/reactor; and/or to the electrochemical reaction/cell.
  • the temperature and the residence time in the hydrolysis reaction/reactor may be different from the one in the chlorination reaction/reactor.
  • the hydrolysis reaction may be run at a lower temperature than the chlorination reaction.
  • the residence time in the hydrolysis reaction may be longer than that in the chlorination reaction.
  • the extraction method may be such that once the one or more products comprising DCP and PCH are extracted from the aqueous medium using the DCP as an extraction solvent, the organics are transferred to the hydrolysis reaction; the aqueous stream comprising metal chloride with metal ions in the higher oxidation state and the lower oxidation state is added back to the hydrolysis reaction; and the reaction is run at lower temperature and longer residence time so that the DCP is hydrolyzed to the PCH. This may avoid more DCP being formed and/or more PCH decomposing to form other side products in the chlorination reaction.
  • the method further includes (v) transferring the organic medium comprising PCH and DCP (remaining if any, after the hydro lyis) from the hydro lyzing step to epoxidation; and (vi) epoxidizing the PCH with a base to form PO in the presence of the DCP (described in detail further herein below).
  • the methods further comprise extracting the PCH formed after the hydrolysis step from the aqueous medium using the DCP as an extraction solvent.
  • the DCP may be separated from the PCH and the separated DCP may be recirculated to the separation reaction/reactor and/or to the hydrolysis reaction/reactor.
  • the one or more products further comprise isopropanol and/or isopropyl chloride.
  • the method further comprises converting the isopropanol and/or the isopropyl chloride back to the propylene, DCP, and/or PCH.
  • other isopropanol and/or other isopropyl chloride may be used in this process and are converted to more valuable propylene, DCP, and/or PCH.
  • a recirculating stream of the DCP hydro lyzes to the PCH in the hydrolysis reactor by addition of reactants and removal of products.
  • Some reaction conditions such as, but not limited to, low temperature and longer residence time have been described above.
  • the hydrolysis reactor runs at different pressure and temperature conditions than the chlorination reactor and that drives the hydrolysis reaction. For example, in some embodiments, since there is no propylene in the hydrolysis reactor, it can be run at a lower pressure and/or longer residence time than the chlorination reactor, thereby expediting the hydrolysis reaction.
  • the temperature of the hydrolysis reaction/reactor is between 20°C-200°C or between 90°C-160°C.
  • the residence time in the hydrolysis reaction/reactor is less than two hrs; or less than one hr; or between lsec-2hrs; or between lmin-lhr.
  • the hydrolysis of the DCP to the PCH in the hydrolysis reactor may be catalyzed by the presence of a heterogenous catalyst, such as, but not limited to, a noble metal.
  • a heterogenous catalyst such as, but not limited to, a noble metal.
  • the noble metals have been described herein for the formation of the PCH and can be used in the hydrolysis of the DCP to the PCH as well.
  • both the DCP and the water may be minimally soluble in one another and as a result the hydrolysis reactor may contain one or two liquid phases. If the reactor contains both liquid phases, the reaction can proceed in both phases, i.e. both the DCP which is soluble in the water-rich phase and the water which is soluble in the DCP-rich phase, may react. In the hydrolysis reactor, a single liquid phase or both the DCP rich phase (with dissolved water) and the water rich phase (with dissolved DCP) are contemplated.
  • the hydrolysis of the DCP to the PCH comprises
  • concentration of the metal chloride with metal ion in the higher oxidation state for example only CuCl 2 .
  • the hydrolysis of the DCP to the PCH may be carried out in presence of copper hydroxychloride species of stoichiometry Cu x Cl y (OH) (2x-y) .
  • CuCl copper chloride
  • CuCl 2 copper chloride with metal ions in the higher oxidation state
  • the hydrolysis of the DCP to the PCH may be carried out in presence of copper hydroxychloride species of stoichiometry Cu x Cl y (OH) (2x-y) .
  • the formation of the copper hydroxychloride species of stoichiometry Cu x Cl y (OH) (2x-y) via the oxychlorination reaction has been described above.
  • the copper hydroxychloride species of stoichiometry Cu x Cl y (OH) (2x-y) can serve as a base consuming HC1 via:
  • the Cu(OH)Cl may serve as an active site to form the PCH directly from the DCP as shown in reaction (XII) below:
  • the methods further comprise reacting the PCH with a base to form the PO.
  • a base to form the PO.
  • the conversion of the PCH to the PO is a ring-closing reaction whereby the chlorohydrin molecule may be combined in a near stoichiometric ratio with a base such as e.g. sodium hydroxide (NaOH) or lime (CaO).
  • a base such as sodium hydroxide (NaOH) or lime (CaO).
  • the products are PO, the chloride salt of the base (e.g. NaCl or CaCl 2 respectively) and water.
  • the PO may be a reactive molecule, it may need to be removed from the reaction media quickly.
  • the short residence time requirement may be achieved by steam stripping the PO as it is formed in the reactor.
  • the PCH feeding the reactor may be diluted with a large excess of water due to upstream reaction selectivity considerations (described further herein below), the steam demand for PO stripping may be very high.
  • methods and systems comprising reacting the PCH with a base to form PO in presence of DCP or the methods and systems comprise reacting the solution of the PCH and the DCP with a base to form PO.
  • the DCP is not separated from the PCH after hydrolysis and the solution is directly subjected to epoxidation.
  • the separation of the DCP and the PCH step may be combined with the epoxidation step such that when the base is added into the epoxidation reactor, the base reacts with the PCH to form the PO, which may leave the reactor as a vapor.
  • some DCP may be converted to the PCH which would also form the PO.
  • the residual levels of un- reacted PCH may leave the reactor in the DCP extraction solvent (DCP as an extraction solvent has been described before) and return to the process where appropriate.
  • the methods and systems provided herein for converting the PCH to the PO in the presence of the DCP (where the mol% of the DCP may be equal to or greater than the mol% of the PCH) has a number of advantages. First, it may obviate the need for separation of the PCH from the DCP prior to the epoxidation. To maintain high selectivity of the PCH during the hydrolysis reaction, the DCP level may be in excess relative to the converted amount of the DCP as described above. The PCH may be separated from the DCP via a typical separation operation. If PCH were the lighter (lower boiling) component, distillation would be an option.
  • the reactor may not require steam stripping inside the reactor.
  • the PO can be removed from the reactor in the DCP phase if desired and separated downstream.
  • additional side reactions may be minimized because PO may react much more slowly in the organic (DCP) phase.
  • the total waste water demand may be significantly reduced because the water leaving the reactor would primarily be that which came in with the caustic (and low levels of soluble water with the organic phase).
  • the resulting aqueous solution may be concentrated enough in NaCl to merit removing the waste organics and using the brine back in the electrochemical cell.
  • the conversion of the PCH to the PO in the presence of DCP may also allow for process options that minimize by-product losses, such as, a single aqueous phase reactor that contains both reactants and products; minimizing by-product formation by running the reactor with a short residence time; step-wise addition of the NaOH; and recycling of the product stream back to the reactor.
  • the step- wise addition of NaOH e.g. along a length of pipe if the reaction is done in a continuous system
  • the recycling of the aqueous product stream back to the reactor inlet may also minimize the NaOH concentration in the aqueous phase.
  • the recycling option has other advantages too.
  • the recycle stream may return salt-rich brine to the reactor.
  • the presence of the salt may minimize the solubility of the PO in the aqueous phase which may improve reactor selectivity.
  • the highly concentrated salt may be advantageous because the resulting brine stream exiting the epoxidation unit may serve as a feedstock for electrolysis cells after removal of the residual, soluble organics.
  • the recycle of reactor outlet may allow the reactor to run in such a way as to produce a high salt concentration outlet stream without having to feed a high concentration NaOH stream directly to the reactor.
  • the other advantages of the high salt concentration outlet stream have also been described further herein.
  • the base is an alkali metal hydroxide, such as e.g. NaOH or alkali metal oxide; alkaline earth metal hydroxide or oxide, such as e.g. Ca(OH) 2 or CaO; or metal hydroxide chloride (for example only, M x n Cl y (OH) (nx-y) ).
  • metal in the metal hydroxychloride is same as metal in the metal chloride.
  • the method further comprises forming the metal hydroxychloride by oxychlorinating the metal chloride with the metal ion in the lower oxidation state to the higher oxidation state in presence of water and oxygen (as explained above).
  • the NaOH may be combined and reacted with an approximately 4-5 wt% solution of propylene chlorohydrins.
  • the propylene chlorohydrins are a mix of l-chloro-2-propanol
  • Propylene oxide may be rapidly stripped from the solution in either a vacuum stripper or steam stripper.
  • a primary disadvantage of the process may be the generation of a dilute NaCl brine stream with about 3-6 wt% NaCl with flow rate exceeding 40-45 tonnes of brine per tonne of propylene oxide.
  • the large amount of dilute brine may result in large amount of waste water.
  • the reason for the large volume of water may be that the reactor producing the propylene chlorohydrins must operate at dilute concentrations of about 4-5 wt% propylene chlorohydrin in order to achieve high selectivity.
  • the amount of dilute brine generated after the PO formation can be substantially reduced.
  • the reaction forms between about 5-40 tonnes of brine per tonne of PO which is substantially less brine compared to the brine generated in a typical PO reaction.
  • a method to form propylene oxide (PO), comprising chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt to result in one or more products comprising between about 5- 99.9 wt% PCH, and the metal chloride with the metal ion in lower oxidation state; and reacting the PCH with a base to form PO and brine in water, wherein the reaction forms between about 5-42 tonnes of brine per tonne of PO.
  • a method to form propylene oxide (PO), comprising chlorinating propylene in an aqueous medium comprising metal chloride with metal ion in higher oxidation state and salt to result in one or more products comprising DCP and PCH, and the metal chloride with the metal ion in lower oxidation state; extracting the DCP and the PCH with re-circulating DCP from the same process and/or the other DCP; hydro lyzing the DCP in the mixture of the DCP and the PCH to the PCH; and reacting the PCH in presence of remaining DCP with a base to form PO and brine in water.
  • P propylene oxide
  • the reaction forms between about 5-42 or about 5-40 tonnes of brine per tonne of PO.
  • the selectivity of the PCH formed is between about 10-99.9 wt%.
  • the base is between about 5-35 wt% or between about 8-15 wt%.
  • the bases have been described herein and include without limitation, the alkali metal hydroxide e.g. sodium hydroxide or potassium hydroxide; alkaline earth metal hydroxide e.g. calcium hydroxide or oxide e.g. CaO or MgO; or metal hydroxide chloride.
  • the PO formation has been illustrated in Figs. 1-5.
  • the PO formed is between about 5-50 wt%; or between about 5-40 wt%; or between about 5-30 wt%; or between about 5-20 wt%; or between about 5-10 wt%; or between about 10-50 wt%; or between about 10-40 wt%; or between about 10-30 wt%; or between about 10-20 wt%; or between about 20-50 wt%; or between about 20-40 wt%; or between about 20-30 wt%; or between about 30-50 wt%; or between about 30-40 wt%; or between about 40-50 wt%.
  • the PO formed is between about 1-25 wt%; or between about 2-20 wt%; or between about 3-15 wt%.
  • the reaction forms between about 5-42 tonnes of brine per tonne of PO; or between about 5-40 tonnes of brine per tonne of PO; or between about 5-35 tonnes of brine per tonne of PO; or between about 5-30 tonnes of brine per tonne of PO; or between about 5-25 tonnes of brine per tonne of PO; or between about 5-20 tonnes of brine per tonne of PO; or between about 5-10 tonnes of brine per tonne of PO.
  • the reaction forms between about 3-40 tonnes of brine per tonne of PO; or between about 4-20 tonnes of brine per tonne of PO; or between about 4-12 tonnes of brine per tonne of PO.
  • the base is between about 5-50 wt%; or between about 5-40 wt%; or between about 5-30 wt%; or between about 5-20 wt%; or between about 5-10 wt%; or between about 10-50 wt%; or between about 10-40 wt%; or between about 10-30 wt%; or between about 10-20 wt%; or between about 20-50 wt%; or between about 20-40 wt%; or between about 20-30 wt%; or between about 30-50 wt%; or between about 30-40 wt%; or between about 40-50 wt%; or between about 8-15 wt%; or between about 10-15 wt%; or between about 12-15 wt%; or between about 14-15 wt%; or between about 8-10 wt%; or between about 8-12 wt%. In some embodiments of the aspect and embodiments provided herein, the base is between about 5-38 wt%; or
  • the method further comprises transferring aqueous medium comprising the metal chloride with the metal ion in the lower oxidation state and the salt to an anode electrolyte in contact with an anode in an electrochemical cell and oxidizing the metal ion from the lower oxidation state to the higher oxidation state at the anode.
  • the method further comprises transferring the aqueous medium comprising the metal chloride with the metal ion in the lower oxidation state and the salt to an oxychlorination reaction and oxidizing the metal ion from the lower oxidation state to the higher oxidation state in the presence of the oxidant.
  • the one or more products further comprise hydrochloric acid (HC1).
  • the method further comprises after the chlorinating step, oxychlorinating the metal chloride with the metal ion in the lower oxidation state to the metal ion in the higher oxidation state in presence of the HC1 and oxygen, or hydrogen peroxide.
  • the method further comprises recirculating the metal chloride in the higher oxidation state back to the chlorinating step.
  • the separation and/or purification may include one or more of the separation and purification of the organic products from the metal ion solution and/or the separation and purification of the organic products from each other, to improve the overall yield of the PCH, improve selectivity of the PCH, improve purity of the PCH, improve efficiency of the systems, improve ease of use of the solutions in the overall process, improve reuse of the metal solution, and/or to improve the overall economics of the process.
  • the solution containing the one or more products and the metal chloride may be subjected to a washing step which may include rinsing with an organic solvent or passing the organic product through a column to remove the metal ions.
  • the organic products may be purified by distillation.
  • the systems provided herein include one or more reactors that carry out the chlorination reaction; the hydrolysis reaction; the oxychlorination reaction; and the epoxidation reaction.
  • the "reactor” as used herein is any vessel or unit in which the reaction provided herein is carried out.
  • the chlorination reactor is configured to contact the metal chloride solution with the propylene to form the one or more products comprising DCP and/or PCH.
  • the reactor may be any means for contacting the metal chloride with the propylene.
  • Such means or such reactor are well known in the art and include, but not limited to, pipe, column, duct, tank, series of tanks, container, tower, conduit, and the like.
  • the reactor may be equipped with one or more of controllers to control temperature sensor, pressure sensor, control mechanisms, inert gas injector, etc. to monitor, control, and/or facilitate the reaction.
  • the reactor system may be a series of reactors connected to each other.
  • the chlorination mixture may be kept either in the same reaction vessel (or reactor), or in a second reaction vessel (hydrolysis reactor) that does not contain additional propylene.
  • a second reaction vessel may be a stirred tank. The stirring may increase the mass transfer rate of the PCH and/or the DCP into the aqueous medium accelerating the reaction to the PCH.
  • the reactor configuration includes, but is not limited to, design parameters of the reactor such as, e.g. length/diameter ratio, flow rates of the liquid(s) and gas(es), material of construction, packing material and type of reactor such as, packed column, bubble column, or trickle-bed reactor, or combinations thereof.
  • the systems may include one reactor or a series of multiple reactors connected to each other or operating separately.
  • the reactor may be a packed bed such as, but not limited to, a hollow tube, pipe, column or other vessel filled with packing material.
  • the reactor may be a spray reactor.
  • the reactor may be a trickle-bed reactor.
  • the reactor may be a bubble column.
  • the packed bed reactor includes a reactor configured such that the aqueous medium containing the metal ions and the propylene flow counter-currently in the reactor or includes the reactor where the aqueous medium containing the metal ions flows in from the top of the reactor and the propylene gas is pressured in from the bottom.
  • the propylene may be fed in such a way that only when the propylene gets consumed, that more propylene flows into the reactor.
  • the trickle-bed reactor includes a reactor where the aqueous medium containing the metal ions and the propylene flow co- currently in the reactor.
  • the reactor may be configured for both the reaction and separation of the products.
  • the processes and systems described herein may be batch processes or systems or continuous flow processes or systems.
  • the salt solutions comprised CuCl 2 , CuCl, and NaCl.
  • the salts were weighed into 10ml vials with water added to bring the solution volume to approximately 4ml. 50 ⁇ of DCP was added to each vial and then a stir bar was also added.
  • the vials were closed with a split- septa cap and placed inside an 8 well high throughput reactor. The entire system was heated to 150°C for 30 minutes, during which time the vials were all stirred at 600 rpm.
  • the organics were extracted using 4ml of ethyl acetate and the resulting solutions were measured by GC-MS. Using the peak areas from the GC-MS, the following conversions were obtained shown in Table I:
  • Experiment 2 An aqueous solution of CuCl 2 (1.0 mol/kg), CuCl (1.0 mol/kg), and NaCl (1.0 mol/kg) was heated in a Parr reactor under propylene pressure to 140°C for 30 minutes. The reactor was depressurized into a bubbler trap at 0°C to capture volatile compounds. When the reactor was opened, the solution was extracted three times with an organic solvent, e.g. ethyl acetate or dichloromethane, which was analyzed with a gas chromatograph equipped with a mass spectrometer. A total of 15 umol DCP and 88 umol PCH were measured. The amounts of recyclable products measured were 917 umol isopropanol, 4 umol acetone, and 35 umol isopropyl chloride.
  • organic solvent e.g. ethyl acetate or dichloromethane
  • a 40 wt% solution of propylene chlorohydrin is combined with a 10 wt% solution of sodium hydroxide and brine.
  • the use of the more concentrated PCH reduces the brine effluent from 46.2 to 10.1 tonnes per tonne of propylene oxide resulting in significant cost savings for the handling of this stream.
  • feeding a solution of PCH in DCP may lower the total water discharged to around 7 tonnes per tonne PO, which is due to the amount of water contained in the added NaOH solution.
  • a glass vial was loaded with 5 mL of 0.1 N NaOH and 100 ul of PCH (70% 1- chloro-2-propanol and 30% 2-chloro-l-propanol). The vial was stirred with a magnetic stir bar for 20 hours. Afterward, a 1 ml aliquot was extracted with 2 ml of ethyl acetate that was subsequently analyzed by gas chromatography with a mass spectrometer detector. Propylene oxide as well as both isomers of PCH was observed, as determined by their fragmentation patterns.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Engineering & Computer Science (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Inorganic Chemistry (AREA)
  • Epoxy Compounds (AREA)

Abstract

L'invention concerne des procédés et des systèmes pour former de la chlorhydrine de propylène par hydrolyse de 1,2-dichloropropane et pour former en outre de l'oxyde de propylène à partir de la chlorhydrine de propylène.
PCT/US2018/035010 2017-05-31 2018-05-30 Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène WO2018222642A1 (fr)

Priority Applications (2)

Application Number Priority Date Filing Date Title
CN201880036582.5A CN110753679A (zh) 2017-05-31 2018-05-30 形成氯丙醇和环氧丙烷的方法和系统
EP18809606.9A EP3630709A4 (fr) 2017-05-31 2018-05-30 Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène

Applications Claiming Priority (6)

Application Number Priority Date Filing Date Title
US201762512900P 2017-05-31 2017-05-31
US62/512,900 2017-05-31
US201762531669P 2017-07-12 2017-07-12
US62/531,669 2017-07-12
US201762596215P 2017-12-08 2017-12-08
US62/596,215 2017-12-08

Publications (1)

Publication Number Publication Date
WO2018222642A1 true WO2018222642A1 (fr) 2018-12-06

Family

ID=64456156

Family Applications (1)

Application Number Title Priority Date Filing Date
PCT/US2018/035010 WO2018222642A1 (fr) 2017-05-31 2018-05-30 Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène

Country Status (4)

Country Link
US (1) US20180347056A1 (fr)
EP (1) EP3630709A4 (fr)
CN (1) CN110753679A (fr)
WO (1) WO2018222642A1 (fr)

Families Citing this family (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US10619254B2 (en) 2016-10-28 2020-04-14 Calera Corporation Electrochemical, chlorination, and oxychlorination systems and methods to form propylene oxide or ethylene oxide
US10590054B2 (en) 2018-05-30 2020-03-17 Calera Corporation Methods and systems to form propylene chlorohydrin from dichloropropane using Lewis acid
CN111253254B (zh) * 2020-03-05 2021-03-16 苏州大学 可见光催化的脂肪族烯烃的双氯加成产物的制备方法
CN116354908B (zh) * 2023-05-25 2023-09-19 山东联欣环保科技有限公司 一种全生物基环氧丙烷的制备方法及其应用

Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4008133A (en) * 1974-09-20 1977-02-15 The Lummus Company Production of epoxy compounds from olefinic compounds
US4126526A (en) * 1977-11-16 1978-11-21 The Lummus Company Cyclic process for production of alkylene oxide using electrolysis of brine
US4277405A (en) * 1979-05-03 1981-07-07 The Lummus Company Production of epoxy compounds from olefinic compounds
US20170073823A1 (en) * 2011-05-19 2017-03-16 Calera Corporation Electrochemical hydroxide systems and methods using metal oxidation
US20170121832A1 (en) * 2015-10-28 2017-05-04 Calera Corporation Electrochemical, halogenation, and oxyhalogenation systems and methods

Family Cites Families (2)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
GB1553819A (en) * 1975-07-25 1979-10-10 Ici Ltd Hydrolysis of propylene dichloride
EP3615709A4 (fr) * 2017-04-27 2021-01-20 Calera Corporation Systèmes et procédés électrochimiques, de chloration et d'oxychloration destinés à former de l'oxyde de propylène ou de l'oxyde d'éthylène

Patent Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4008133A (en) * 1974-09-20 1977-02-15 The Lummus Company Production of epoxy compounds from olefinic compounds
US4126526A (en) * 1977-11-16 1978-11-21 The Lummus Company Cyclic process for production of alkylene oxide using electrolysis of brine
US4277405A (en) * 1979-05-03 1981-07-07 The Lummus Company Production of epoxy compounds from olefinic compounds
US20170073823A1 (en) * 2011-05-19 2017-03-16 Calera Corporation Electrochemical hydroxide systems and methods using metal oxidation
US20170121832A1 (en) * 2015-10-28 2017-05-04 Calera Corporation Electrochemical, halogenation, and oxyhalogenation systems and methods

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See also references of EP3630709A4 *

Also Published As

Publication number Publication date
EP3630709A1 (fr) 2020-04-08
EP3630709A4 (fr) 2021-03-03
CN110753679A (zh) 2020-02-04
US20180347056A1 (en) 2018-12-06

Similar Documents

Publication Publication Date Title
WO2018222642A1 (fr) Procédés et systèmes pour former de la chlorhydrine de propylène et de l'oxyde de propylène
US5246551A (en) Electrochemical methods for production of alkali metal hydroxides without the co-production of chlorine
EP3149228B1 (fr) Procédé pour la réduction électrochimique de dioxyde de carbone au moyen d'une électrode à diffusion gazeuse
JP5508278B2 (ja) ジアリールカーボネートの製造方法
FI71354C (fi) Foerfarande foer framstaellning av natriumklorat
US4169773A (en) Removal of chlorate from electrolytic cell anolyte
TW200835682A (en) Processes for the production of diaryl carbonates and treatment of alkalichloride solutions resulting therefrom
WO1994025643A1 (fr) Recuperation du brome et preparation d'acide hypobromeux a partir d'une solution de bromure
WO2008152043A1 (fr) Composition aqueuse contenant un sel, procédé de fabrication et utilisation
US20200240025A1 (en) Electrochemical, chlorination, and oxychlorination systems and methods to form propylene oxide or ethylene oxide
US20190017183A1 (en) System and Method for the Co-Production of Oxalic Acid and Acetic Acid
KR20150056627A (ko) 이산화탄소로부터 카복실산을 생산하기 위한 통합 공정
EP3157897B1 (fr) Procédé intégré de co-production d'acides carboxyliques et de produits d'halogène à partir de dioxyde de carbone
CA1214429A (fr) Separation du chromate de la solution saline d'une pile electrolytique
CN110573659A (zh) 电化学、氯化和氧氯化系统及形成环氧丙烷或环氧乙烷的方法
US10807927B2 (en) Methods and systems to form propylene chlorohydrin from dichloropropane using lewis acid
US3455797A (en) Procedure for the preparation of olefin oxides
CN109721573B (zh) 一种环氧氯丙烷合成方法
US20200115809A1 (en) Systems and methods using lanthanide halide
CN109721570B (zh) 一种生产环氧氯丙烷的方法
US9527753B1 (en) Production of zinc chloride and zinc sulfate from geothermal brines
US20190119186A1 (en) Systems and methods using lanthanide halide
JPH0238573B2 (fr)
WO2010114144A1 (fr) Oxyde de trichloro-trifluoro-propylène et son procédé de production
CN109721572B (zh) 一种环氧氯丙烷制备方法

Legal Events

Date Code Title Description
121 Ep: the epo has been informed by wipo that ep was designated in this application

Ref document number: 18809606

Country of ref document: EP

Kind code of ref document: A1

NENP Non-entry into the national phase

Ref country code: DE

WWE Wipo information: entry into national phase

Ref document number: 2018809606

Country of ref document: EP

ENP Entry into the national phase

Ref document number: 2018809606

Country of ref document: EP

Effective date: 20200102