OXYGEN GENERATOR AND METHOD OF CONTROLLING THE OXYGEN PRODUCTION RATE OF AN OXYGEN GENERATOR

Abstract

An oxygen generator has a composition for generating oxygen and an acidic compound and/or a basic compound. The composition for generating oxygen includes an oxygen source, an ionic liquid, a metal oxide compound and/or a metal salt, and optionally a basic compound. The oxygen source is a peroxide compound, the ionic liquid is in the liquid state at least in a temperature range from 10 C. to +50 C., the metal oxide compound is an oxide of a single metal or of two or more different metals selected from the metals of groups 2 to 14 of the periodic table of the elements. The metal salt has a single metal or two or more different metals, and an organic and/or an inorganic anion. There is also described a method for controlling the oxygen production rate of the oxygen generator, and a device for generating oxygen in a controlled manner.

Claims

1. (canceled)

2. The oxygen generator according to claim 16, wherein the oxygen source is selected from the group consisting of alkali metal percarbonates, alkali metal perborates, urea hydrogen peroxide, and mixtures thereof.

3. The oxygen generator according to claim 16, wherein the ionic liquid is at least one salt having a cation and an anion, wherein the cation is selected from the group consisting of imidazolium, pyrrolidinium, ammonium, pyridinium, pyrazolium, piperidinium, phosphonium, and sulfonium cations and/or wherein the anion is selected from the group consisting of dimethylphosphate, methylsulfate, ethylsulfate, trifluoromethylsulfonate, bis(trifluoromethylsulfonyl)imide, chloride, bromide, iodide, tetrafluoroborate, hexafluorophosphate, acetate, and but-3-enoate.

4. The oxygen generator according to claim 16, wherein the metal oxide compound is selected from the group consisting of MnO.sub.2, Co.sub.3O.sub.4, CrO.sub.3, Ag.sub.2O, CuO, Fe.sub.3O.sub.4 and PbO.sub.2, or is selected from the group consisting of mixed cobalt iron oxides, mixed copper iron oxides, mixed nickel iron oxides, mixed manganese iron oxides, mixed copper manganese oxides, mixed cobalt manganese oxides, mixed nickel manganese oxides, mixed nickel cobalt oxides, mixed lanthanum iron nickel oxides, mixed lanthanum strontium manganese oxides, and mixtures thereof.

5. The oxygen generator according to claim 16, wherein the metal salt comprises at least one cation selected from the group consisting of vanadium, chromium, manganese, iron, cobalt, copper, molybdenum, ruthenium, iridium, and lead.

6. The oxygen generator according to claim 16, wherein the acidic compound is selected from the group consisting of inorganic acids, organic acids, acidic salts, and ionic liquids having acidic functionality.

7. The oxygen generator according to claim 16, wherein the acidic compound is selected from the group consisting of hydrochloric acid, sulphuric acid, nitric acid, phosphoric acid, acetic acid, succinic acid, citric acid, benzoic acid, sodium hydrogen sulfate, monopotassium phosphate, 1-ethyl-3-methylimidazolium hydrogen sulfate, trimethylammonium propanesulfonic acid hydrogen sulfate, 1-(4-sulfobutyl)-3-methylimidazolium hydrogen sulfate, and diethylmethylammonium methanesulfonate.

8. The oxygen generator according to claim 16, wherein the basic compound is selected from the group consisting of hydroxides, basic oxides, basic salts, and ionic liquids having basic properties.

9. The oxygen generator according to claim 16, wherein the basic compound is selected from the group consisting of sodium hydroxide, potassium hydroxide, potassium phosphate, sodium acetate, sodium percarbonate, potassium carbonate, calcium hydroxide, calcium oxide, 1-ethyl-3-methylimidazolium acetate, tetrabutylammonium arginine, and tetraethyl-ammonium but-3-enoate.

10. The oxygen generator according to claim 16, wherein the acidic compound is provided in a form selected from the group consisting of a solid form, the form of a solution or dispersion, and the form of a pure liquid substance, and/or wherein the basic compound or the further basic compound is provided in a form selected from the group consisting of a solid form, the form of a solution or dispersion, and the form of a pure liquid substance.

11. A method for controlling the oxygen production rate of an oxygen generating composition, the method comprising: providing an oxygen source, providing an ionic liquid, and providing a metal oxide compound and/or a metal salt; generating oxygen by contacting the oxygen source, the ionic liquid and the metal oxide compound and/or the metal salt; and modifying the oxygen production rate by selectively adding an acidic compound and/or a basic compound to the oxygen source, the ionic liquid, and the metal oxide compound and/or the metal salt; or, if the ionic liquid is an acidic compound or contains an acidic compound: providing an oxygen source, providing the ionic liquid, providing a metal oxide compound and/or a metal salt, and providing a basic compound; generating oxygen by contacting the oxygen source, the ionic liquid, the metal oxide compound and/or the metal salt and the basic compound and, optionally, modifying the oxygen production rate by adding a further acidic compound and/or a further basic compound to the oxygen source, the ionic liquid, the metal oxide compound and/or the metal salt, and the basic compound; wherein the oxygen source comprises a peroxide compound; the ionic liquid is in the liquid state at least in a temperature range from 10 C. to +50 C.; the metal oxide compound is an oxide of a single metal or of two or more different metals selected from the metals of groups 2 to 14 of the periodic table of the elements; and the metal salt has a single metal or two or more different metals, and one or both of an organic anion and/or an inorganic anion.

12. The method according to claim 11, wherein the step of modifying the oxygen production rate comprises decelerating or stopping the oxygen production by adding an acidic compound or a further acidic compound, once or multiple times.

13. The method according to claim 11, wherein the step of modifying the oxygen production rate comprises accelerating or restarting the oxygen production by adding a basic compound or a further basic compound, once or multiple times.

14. The method according to claim 11, wherein the step of modifying the oxygen production rate comprises decelerating or interrupting the oxygen production by adding an acidic compound or a further acidic compound and, after a desired time interval, accelerating or restarting the oxygen production by adding a basic compound or a further basic compound, once or multiple times.

15. (canceled)

16. An oxygen generator, comprising: an oxygen source, an ionic liquid, and a metal oxide compound and/or a metal salt; said oxygen source, said ionic liquid, said metal oxide compound or metal salt, upon coming into contact with one another, forming a composition for generating oxygen; an acidic compound for selectively decreasing a rate of reaction of the composition for generating oxygen and a basic compound for selectively initiating or increasing the rate of reaction for generating oxygen; wherein: the oxygen source is a peroxide compound; the ionic liquid is in the liquid state in a temperature range from 10 C. to +50 C.; the metal oxide compound is an oxide of a single metal or of two or more different metals selected from the metals of groups 2 to 14 of the periodic table of the elements; and the metal salt includes a single metal or two or more different metals, and one or both of an organic anion and an inorganic anion.

17. An oxygen generator, comprising: an oxygen source, an ionic liquid, a metal oxide compound and/or a metal salt, and a basic compound, and, optionally, an acidic compound; the oxygen source, the ionic liquid, the metal oxide compound or metal salt, and the optional acidic compound, upon coming into contact with one another, forming a composition for generating oxygen; wherein: the ionic liquid is an acidic compound or contains an acidic compound; the oxygen source is a peroxide compound; the ionic liquid is in the liquid state in a temperature range from 10 C. to +50 C.; the metal oxide compound is an oxide of a single metal or of two or more different metals selected from the metals of groups 2 to 14 of the periodic table of the elements; and the metal salt includes a single metal or two or more different metals, and one or both of an organic anion and an inorganic anion.

18. The oxygen generator according to claim 17, wherein the oxygen source is selected from the group consisting of alkali metal percarbonates, alkali metal perborates, urea hydrogen peroxide, and mixtures thereof.

19. The oxygen generator according to claim 17, wherein the ionic liquid is at least one salt having a cation and an anion, wherein the cation is selected from the group consisting of imidazolium, pyrrolidinium, ammonium, pyridinium, pyrazolium, piperidinium, phosphonium, and sulfonium cations and/or wherein the anion is selected from the group consisting of dimethylphosphate, methylsulfate, ethylsulfate, trifluoromethylsulfonate, bis(trifluoromethylsulfonyl)imide, chloride, bromide, iodide, tetrafluoroborate, hexafluorophosphate, acetate, and but-3-enoate.

20. The oxygen generator according to claim 17, wherein the metal oxide compound is selected from the group consisting of MnO.sub.2, Co.sub.3O.sub.4, CrO.sub.3, Ag.sub.2O, CuO, Fe.sub.3O.sub.4 and PbO.sub.2, or is selected from the group consisting of mixed cobalt iron oxides, mixed copper iron oxides, mixed nickel iron oxides, mixed manganese iron oxides, mixed copper manganese oxides, mixed cobalt manganese oxides, mixed nickel manganese oxides, mixed nickel cobalt oxides, mixed lanthanum iron nickel oxides, mixed lanthanum strontium manganese oxides, and mixtures thereof.

21. The oxygen generator according to claim 17, wherein the metal salt comprises at least one cation selected from the group consisting of vanadium, chromium, manganese, iron, cobalt, copper, molybdenum, ruthenium, iridium, and lead.

22. The oxygen generator according to claim 17, wherein the acidic compound is selected from the group consisting of inorganic acids, organic acids, acidic salts, and ionic liquids having acidic functionality.

23. The oxygen generator according to claim 17, wherein the acidic compound is selected from the group consisting of hydrochloric acid, sulphuric acid, nitric acid, phosphoric acid, acetic acid, succinic acid, citric acid, benzoic acid, sodium hydrogen sulfate, monopotassium phosphate, 1-ethyl-3-methylimidazolium hydrogen sulfate, trimethylammonium propanesulfonic acid hydrogen sulfate, 1-(4-sulfobutyl)-3-methylimidazolium hydrogen sulfate, and diethylmethylammonium methanesulfonate.

24. The oxygen generator according to claim 17, wherein the basic compound is selected from the group consisting of hydroxides, basic oxides, basic salts, and ionic liquids having basic properties.

25. The oxygen generator according to claim 17, wherein the basic compound is selected from the group consisting of sodium hydroxide, potassium hydroxide, potassium phosphate, sodium acetate, sodium percarbonate, potassium carbonate, calcium hydroxide, calcium oxide, 1-ethyl-3-methylimidazolium acetate, tetrabutylammonium arginine, and tetraethyl-ammonium but-3-enoate.

26. The oxygen generator according to claim 17, wherein the acidic compound is provided in a form selected from the group consisting of a solid form, the form of a solution or dispersion, and the form of a pure liquid substance, and/or wherein the basic compound or the further basic compound is provided in a form selected from the group consisting of a solid form, the form of a solution or dispersion, and the form of a pure liquid substance.

Description

BRIEF DESCRIPTION OF THE SEVERAL VIEWS OF THE DRAWING

[0150] FIGS. 1-13 are graphs illustrating decomposition of UHP (urea hydrogen peroxide), catalyzed be dissolved catalysts, termination of the decomposition reactions by addition of liquid acid solutions, and restart of the decomposition reactions by addition of basic solutions,

[0151] FIGS. 14-25 are graphs illustrating decomposition of UHP, catalyzed by dispersed solid catalysts, termination of the decomposition reactions by addition of liquid acid solutions, and restart of the decomposition reactions by addition of basic solutions,

[0152] FIG. 26 is a graph illustrating decomposition of UHP, catalyzed by a dissolved catalyst, termination of the decomposition reaction by addition of a liquid acid solution, and restart of the decomposition reaction by addition of a potassium phosphate solution,

[0153] FIG. 27 is a graph illustrating start of the decomposition reaction of UHP contained in an acidic ionic liquid having catalysts dissolved therein,

[0154] FIGS. 28 and 29 are graphs illustrating decomposition of UHP, catalyzed by dissolved or dispersed catalysts, and repeated termination and restart of the decomposition reactions by addition of liquid acid solutions and sodium hydroxide solutions, respectively,

[0155] FIGS. 30 and 31 are graphs illustrating decomposition of mixtures of UHP and SPC (sodium percarbonate), and of UHP and SPB (sodium perborate), respectively, catalyzed by dispersed solid catalysts, termination of the decomposition reactions by addition of sulfuric acid, and restart of the decomposition reactions by addition of sodium hydroxide solutions,

[0156] FIGS. 32 to 39 are graphs illustrating decomposition of UHP, catalyzed by dissolved or dispersed catalysts, termination of the decomposition reactions by addition of solid acids, and restart of the decomposition reactions by addition of solid or dissolved bases,

[0157] FIGS. 40 to 44 are graphs illustrating decomposition of UHP, catalyzed by dissolved lead acetate, termination of the decomposition reactions by addition of solid acids, and restart of the decomposition reactions by addition of sodium hydroxide solutions,

[0158] FIGS. 45 to 49 are graphs illustrating decomposition of UHP, catalyzed by dissolved or dispersed catalysts, termination of the decomposition reactions by addition of solid acids or liquid acids, and restart of the decomposition reactions by addition of solid bases,

[0159] FIGS. 50 to 55 are graphs illustrating decomposition of UHP, catalyzed by dissolved or dispersed catalysts, termination of the decomposition reactions by addition of ionic liquids with acidic functionality, and restart of the decomposition reactions by addition of sodium hydroxide solutions,

[0160] FIGS. 56 to 59 are graphs illustrating decomposition of UHP, catalyzed by dissolved or dispersed catalysts, termination of the decomposition reactions by addition of liquid acids, and restart of the decomposition reactions by ionic liquids with basic functionality,

[0161] FIG. 60 is a sectional view of an embodiment of a device for generating oxygen according to this invention, and

[0162] FIG. 61 is a sectional view of another embodiment of a device for generating oxygen according to this invention.

DETAILED DESCRIPTION OF THE INVENTION

[0163] Referring now to the figures of the drawing in detail, all of the graphs illustrating oxygen release, the oxygen flow rate and the volume are plotted against run time, wherein run time is the time which starts running at the time point of contacting the oxygen source, the ionic liquid and the catalyst, or at the time point of contacting the oxygen source, the ionic liquid, the metal oxide compound and/or the metal salt with a basic compound. Volume is the oxygen volume released in total. Oxygen flow rate (I/h) and volume released (I) by each decomposition reaction where measured with a drum gas meter in each of the experiments of examples 1 to 14, throughout the experiments.

[0164] In the following examples acids were used in order to stop running peroxide decomposition reactions, and bases were used in order to restart the decomposition reactions. Amounts of acids were chosen to provide about 3 mmol to 6 mmol H+ ions/g ionic liquid, and amounts of bases were chosen to at least neutralize the acids. It is, however, believed that in most cases lower amounts of acid would have been sufficient for bringing the peroxide decomposition to a halt. In addition, it would have been possible to use more base than required for acid neutralization, thus speeding up the decomposition reaction.

Example 1

[0165] Example 1 comprises experiments 1 to 5. In each experiment, an ionic liquid having catalysts dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time, an aqueous solution of NaOH was added into the flask.

[0166] Type and amount of the compounds used in each experiment, as well as the time of addition (in minutes after start of the run time) of acids and bases are listed in table 1. Table 1 also shows in which figure each particular experiment is illustrated.

TABLE-US-00001 TABLE 1 peroxide acid base Figure/ Catalyst adduct ionic liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 1 Pb(OAc).sub.23H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] HOAc NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (2.5 min) (17.8 min) 2 CoSO.sub.47H.sub.2O UHP [EMIM][OAc] HNO.sub.3 NaOH.sub.(aq.) (14.9 mg) (20 g) (10 g) (1.7 min) (20.3 min) 3 FeCl.sub.36H.sub.2O UHP [EMIM][OAc] H.sub.2SO.sub.4 NaOH.sub.(aq.) (14.4 mg) (20 g) (10 g) (1.1 min) (12.1 min) 4 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] H.sub.3PO.sub.4 NaOH.sub.(aq.) (367.9 mg) (20 g) (10 g) (4.0 min) (10.5 min) 5 CuCl.sub.22H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (18.1 mg) (10 g) (5 g) (1.1 min) (15.2 min)

[0167] In each of FIGS. 1-5, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rate, and line 5 indicates the oxygen volume released in total from UHP by the respective catalyst in the respective ionic liquid.

[0168] FIGS. 1-5 show that the peroxide decomposition reaction starts nearly without delay after contacting the peroxide compound, the ionic liquid and the catalyst. Adding an acidic compound stops the peroxide decomposition reaction promptly, and adding a basic compound restarts the decomposition reaction with a reaction rate comparable to the reaction rate before interruption of the decomposition reaction.

[0169] Example 1 proves that the peroxide decomposition reaction can be stopped by different liquid acids (aqueous acid solutions) independent of the catalyst used.

Example 2

[0170] Example 2 comprises experiments 6 to 10. In each experiment, an ionic liquid having catalysts dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time, an aqueous solution of NaOH was added into the flask.

[0171] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the run time) of acids and bases are listed in table 2. Table 2 also shows in which figure each particular experiment is illustrated.

TABLE-US-00002 TABLE 2 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 6 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] H.sub.3PO.sub.4 NaOH.sub.(aq.) (367.9 mg) (20 g) (10 g) (4.0 min) (10.5 min) 7 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] NaHSO.sub.4(aq.) NaOH.sub.(aq.) (367.9 mg) (20 g) (10 g) (3.4 min) (7.9 min) 8 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] HCl.sub.(aq.) NaOH.sub.(aq.) (735.7 mg) (40 g) (30 g) (8.9 min) (23.5 min) 9 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] HOAc NaOH.sub.(aq.) (735.7 mg) (40 g) (30 g) (8.3 min) (59.1 min) 10 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] Bernsteinsaure NaOH.sub.(aq.) (367.9 mg) (20 g) (10 g) in (21.3 min) [EMIM][OAc] (4.0 min)

[0172] In each of FIGS. 6-10, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP by the catalyst in the ionic liquid.

[0173] FIGS. 6-10 show that the peroxide decomposition reaction starts nearly without delay after contacting the peroxide compound, the ionic liquid and the catalyst. Adding a liquid acid stops the peroxide decomposition reaction promptly, and adding a liquid base restarts the decomposition reaction, the reaction rate being comparable to the reaction rate before interruption of the decomposition reaction.

[0174] Example 2 proves that the decomposition of a peroxide compound can be started by a catalyst which is dissolved in an ionic liquid. The decomposition reaction can be stopped by adding various liquid acids.

Example 3

[0175] Example 3 comprises experiments 11 to 13. In each experiment, an ionic liquid having catalysts dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous nitric acid) was added into the flask, and after a further predetermined period of time, an aqueous solution of NaOH was added into the flask.

[0176] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 3. Table 3 also shows in which figure each particular experiment is illustrated.

TABLE-US-00003 TABLE 3 Peroxide Ionic acid Figure/ catalyst adduct liquid (time of base experiment (mass) (mass) (mass) addition) (time of addition) 11 Co(OAc).sub.24H.sub.2O UHP [EMIM][OAc] HNO.sub.3(aq.) NaOH.sub.(aq.) (13.2 mg) (20 g) (10 g) (0.8 min) (20.6 min) 12 CoCl.sub.26H.sub.2O UHP [EMIM][OAc] HNO.sub.3(aq.) NaOH.sub.(aq.) (12.6 mg) (20 g) (10 g) (0.8 min) (20.1 min) 13 CoSO.sub.47H.sub.2O UHP) [EMIM][OAc] HNO.sub.3(aq.) NaOH.sub.(aq.) (14.9 mg) (20 g) (10 g) (1.7 min) (20.3 min)

[0177] In each of FIGS. 11-13, line 1 indicates the time of addition of nitric acid, line 2 indicates the time of addition of the aqueous solution of sodium hydroxide, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP by the respective catalysts.

[0178] FIGS. 11-13 show that the peroxide decomposition reaction starts nearly without delay after contacting the peroxide compound with the ionic liquid and the catalyst. Adding an aqueous acid solution stops the peroxide decomposition reaction promptly, and adding an aqueous base solution restarts the decomposition reaction.

[0179] Example 3 proves that the peroxide decomposition reaction, catalyzed by a metal salt which has been dissolved in an ionic liquid, can be stopped by adding a liquid acid. Different catalyst anions are equally effective.

Example 4

[0180] Example 4 comprises experiments 14-17. In each experiment, an ionic liquid having catalysts dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time, an aqueous solution of sodium hydroxide was added into the flask.

[0181] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 4. Table 4 also shows in which figure each particular experiment is illustrated.

TABLE-US-00004 TABLE 4 Peroxide Ionic acid Figure/ catalyst adduct liquid (time of base experiment (mass) (mass) (mass) addition) (time of addition) 14 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] H.sub.2SO.sub.4(aq.) NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (5.2 min) (29.8 min) 15 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] H.sub.3PO.sub.4(aq.) NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (4.3 min) (23.0 min) 16 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] HNO.sub.3(aq.) NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (3.2 min) (27.5 min) 17 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (1478.0 mg) (40 g) (25 g) (2.5 min) (19.6 min)

[0182] In each of FIGS. 14-17, line 1 indicates the time of addition of the liquid acid, line 2 indicates the time of addition of the sodium hydroxide solution, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP by manganese dioxide dispersed in an ionic liquid.

[0183] FIGS. 14-17 show that the peroxide decomposition reaction starts without delay after contacting the peroxide with the ionic liquid and the catalyst. Adding an acid stops the peroxide composition reaction promptly, and adding a basic solution restarts the decomposition reaction with a high reaction rate.

[0184] Example 4 proves that the peroxide decomposition reaction, catalyzed by a solid metal oxide dispersed in a ionic liquid, can be stopped by adding different liquid acids.

Example 5

[0185] Example 5 comprises experiments 18-20. In each experiment, an ionic liquid having catalysts dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time, an aqueous solution of NaOH was added into the flask.

[0186] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 5. Table 5 also shows in which figure each particular experiment is illustrated.

TABLE-US-00005 TABLE 5 Peroxide Ionic acid Figure/ catalyst adduct liquid (time of base experiment (mass) (mass) (mass) addition) (time of addition) 18 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (1478.0 mg) (40 g) (25 g) (2.5 min) (19.6 min) 19 PbO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (127.0 mg) (20 g) (10 g) (9.9 min) (37.2 min) 20 CoFe.sub.2O.sub.4 UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (1372.0 mg) (20 g) (10 g) (25.3 min) (49.9 min)

[0187] In each of FIGS. 18-20, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP by the respective catalyst dispersed in the ionic liquid.

[0188] FIGS. 18-20 shows that the peroxide decomposition reaction starts with some delay in the case of lead oxide and in the case of mixed cobalt iron oxide, and can be stopped immediately by adding an aqueous acid solution. Adding a basic compound restarts the decomposition reaction with a high reaction rate.

[0189] Example 5 proves that the peroxide decomposition reaction, catalyzed by different metal oxides dispersed in an ionic liquid, can be stopped by adding a liquid acid.

Example 6

[0190] Example 6 comprises experiments 21-24. In each experiment, an ionic liquid having catalyst (MnO.sub.2) dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous H.sub.2SO.sub.4), was added into the flask, and after a further predetermined period of time, a liquid base (aqueous solution of NaOH or [EMIM][OAc]) was added into the flask.

[0191] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 6. Table 6 also shows in which figure each particular experiment is illustrated.

TABLE-US-00006 TABLE 6 Peroxide Ionic acid base Figure/ catalyst adduct liquid (time of (time of Experiment (mass) (mass) (mass) addition) addition) 21 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] H.sub.2SO.sub.4(aq.) NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (5.3 min) (29.8 min) 22 MnO.sub.2 UHP [EMIM][EtSO.sub.4] H.sub.2SO.sub.4(aq.) [EMIM][OAc] (1108.8 mg) (40 g) (25 g) (1.6 min) (20.0 min) 23 MnO.sub.2 UHP 1-Butylpyridinium H.sub.2SO.sub.4(aq.) NaOH.sub.(aq.) (554.4 mg) (20 g) tetrafluoroborat (1.0 min) (13.8 min) (10 g) 24 MnO.sub.2 UHP Diethylmethylammonium H.sub.2SO.sub.4(aq.) NaOH.sub.(aq.) (554.4 mg) (20 g) methanesulfonat (1.0 min) (15.6 min) (10 g)

[0192] In each of FIGS. 21-24, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP by MnO.sub.2 in the respective ionic liquid.

[0193] FIGS. 21-24 show that the peroxide decomposition reaction is stopped promptly upon addition of aqueous H.sub.2So.sub.4, and is restarted promptly upon addition of an aqueous solution of NaOH or [EMIM][OAc].

[0194] Example 6 proves that it is possible in different ionic liquids to stop the peroxide decomposition by adding an acid, and to restart the decomposition reaction by adding a base.

Example 7

[0195] Example 7 comprises experiments 25-27. In experiment 25, an ionic liquid having catalyst dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time, a liquid base (aqueous solution of NaOH) was added into the flask.

[0196] In experiment 26, an ionic liquid having catalyst dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous acid solution) was added into the flask, and after a further predetermined period of time a first portion of a liquid base (aqueous base solution) was added into the flask, and after a still further predetermined period of time, a second portion of the same liquid base was added into the flask.

[0197] In experiment 27, an ionic liquid with acidic properties having catalyst dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid base (aqueous base solution) was added into the flask.

[0198] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in Table 7. Table 7 also shows in which figure each particular experiment is illustrated.

TABLE-US-00007 TABLE 7 Peroxide Ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 25 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] H.sub.2SO.sub.4 NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (5.3 min) (29.8 min) 26 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] H.sub.3PO.sub.4 K.sub.3PO.sub.4(aq.) (367.9 mg) (20 g) (10 g) (3.0 min) (25.9 min; 30.7 min) 27 CoSO.sub.47H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] / K.sub.2CO.sub.3(aq.) (149.4 mg) (20 g) (10 g) (22.7 min)

[0199] In FIG. 25, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0200] In FIG. 26, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the first portion of the base, line 6 indicates the time of addition of the second portion of the base, lines 3, 4 and 7 indicate the oxygen flow rates (with line 4 indicating the oxygen flow rate after addition of the first base portion, and line 7 indicating the oxygen flow rate after addition of the second base portion), and line 5 indicates the oxygen volume released in total from UHP.

[0201] In FIG. 27, line 2 indicates the time of addition of the base, line 4 indicates the oxygen flow rate, and line 5 indicates the oxygen volume released in total from UHP.

[0202] Example 7 proves that different liquid bases (aqueous base solutions) can be used for starting the peroxide decomposition reaction. Example 7 (see FIG. 26) also proves that the oxygen of a peroxide compound can be released in several steps by adding a base in several steps. Example 7 still further proves (see FIG. 27) that a peroxide decomposition catalyst does not catalyse the peroxide decomposition reaction when the catalyst and the peroxide are contained in an ionic liquid having acidic properties, i.e. the catalyst is inactive in the acidic medium. Upon addition of a base, however, the peroxide decomposition starts.

Example 8

[0203] Example 8 comprises experiments 28 and 29. In each experiment, an ionic liquid having catalyst dissolved or dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. Then, liquid acids (aqueous acid solutions) and liquid bases (aqueous base solutions) were added into the flask in an alternating manner. Specifically, in experiment 28, phosphoric acid was added after a runtime of 9.1 minutes and of 30.9 minutes, and an aqueous solution of sodium hydroxide was added after a runtime of 26.8 minutes and of 44.1 minutes. In experiment 29, hydrochloric acid was added after a runtime of 4.4 minutes, of 16.3 minutes, and of 21.3 minutes, and an aqueous solution of sodium hydroxide was added after a runtime of 13.8 minutes, of 19.1 minutes, and of 24.2 minutes.

[0204] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 8. Table 8 also shows in which figure each particular experiment is illustrated.

TABLE-US-00008 TABLE 8 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 28 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] H.sub.3PO.sub.4 NaOH.sub.(aq.) (1379.6 mg) (100 g) (75 g) (9.1 min; (26.8 min; 30.9 min) 44.1 min) 29 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] HCl.sub.(aq.) NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (4.4 min; (13.8 min; 16.3 min; 19.1 min; 21.3 min) 24.2 min)

[0205] In FIG. 28, lines 1 and 6 indicate the time points of addition of the acid, lines 2 and 7 indicate the time points of addition of the base, lines 3, 4 and 8 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0206] In FIG. 29, lines 1, 6 and 9 indicate the time points of addition of the acid, lines 2, 7 and 10 indicate the time points of addition of the base, lines 3, 4, 8 and 11 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0207] Example 8 proves that the peroxide decomposition reaction can be stopped and restarted several times whenever termination of the oxygen production and restart of the oxygen production is desired until the complete supply of oxygen source has been decomposed.

Example 9

[0208] Example 9 comprises experiments 30 and 31. In each experiment, an ionic liquid having catalyst (MnO.sub.2) dispersed therein was added to a mixture of UHP and SPC (sodium percarbonate), and to a mixture of UHP and SPB (sodium perborate) contained in a glass flask. After a predetermined period of time, a liquid acid (aqueous H.sub.2SO.sub.4) was added into a flask, and after a further predetermined period of time, a liquid base (aqueous solution of sodium hydroxide) was added into the flask.

[0209] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 9. Table 9 also shows in which figure each particular experiment is illustrated.

TABLE-US-00009 TABLE 9 peroxide ionic acid Figure/ catalyst adduct liquid (time of base experiment (mass) (mass) (mass) addition) (time of addition) 30 MnO.sub.2 UHP (25 g) [MMIM]PO.sub.4Me.sub.2] H.sub.2SO.sub.4 NaOH (1108.8 mg) SPC (15 g) (25 g) (2.0 min) (13.4 min) 31 MnO.sub.2 UHP (25 g) [MMIM]PO.sub.4Me.sub.2] H.sub.2SO.sub.4 NaOH (1108.8 mg) SPB (15 g) (25 g) (1.4 min) (7.9 min)

[0210] In FIGS. 30 and 31, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from the oxygen source.

[0211] Example 9 proves that the procedure of interrupting the decomposition process of a peroxide compound, and of restarting the peroxide decomposition process, is not limited to hydrogen peroxide adduct compounds such as UHP, but rather is applicable to compounds having peroxo groups in general, such as e.g. sodium percarbonate and sodium perborate.

Example 10

[0212] Example 10 comprises experiments 32 to 39. In each experiment, an ionic liquid having catalyst dissolved or dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a solid acid was added into the flask, and after a further predetermined period of time, a base was added into the flask.

[0213] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 10. Table 10 also shows in which figure each particular experiment is illustrated.

TABLE-US-00010 TABLE 10 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 32 Pb(OAc).sub.23H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] citric acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (2.5 min) (21.6 min) 33 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] KH.sub.2PO.sub.4(s) KOH.sub.(s) (367.9 mg) (20 g) (10 g) (3.0 min) (27.5 min) 34 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] NaHSO.sub.4(s) K.sub.2CO.sub.3(s) (1109 mg) (40 g) (25 g) (4.3 min) (30.4 min) 35 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] citric acid NaOH.sub.(aq.) (1109 mg) (40 g) (25 g) (2.7 min) (73.4 min) 36 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] succinic acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.3 min) (6.7 min) 37 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] benzoic acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.3 min) (5.2 min) 38 FeCl.sub.36H.sub.2O UHP [EMIM][OAc] NaHSO.sub.4(s) NaOH.sub.(aq.) (14.4 mg) (20 g) (10 g) (0.1 min) (5.0 min) 39 CoSO.sub.47H.sub.2O UHP) [EMIM][OAc] NaHSO.sub.4(s) NaOH.sub.(aq.) (14.9 mg) (20 g) (10 g) (0.8 min; 3.0 min) (7.4 min)

[0214] In each of FIGS. 32 to 38, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0215] FIGS. 32 to 38 show that the peroxide decomposition reaction is stopped promptly upon addition of a solid acid, and is restarted promptly upon addition of a base.

[0216] In FIG. 39, lines 1 and 6 indicate the time of addition of an acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP. FIG. 39 shows that the addition of an acid to the oxygen producing composition does not necessarily stop the peroxide decomposition reaction completely. Rather, the decomposition reaction may be only decelerated, depending from the type and amount of acid added to the oxygen generating composition. In experiment 39, the peroxide decomposition reaction is decelerated after addition of a first amount of solid sodium hydrogen sulfate (see line 3), and is completely stopped after addition of a second amount of solid sodium hydrogen sulfate.

[0217] Example 10 proves that the peroxide decomposition reaction can be stopped, or alternatively decelerated, by adding different solid acids. The decomposition reaction can be restarted, or alternatively accelerated, by adding a basic compound. The phenomenon is not limited to particular compounds or combinations of compounds, but is widely applicable to different catalysts, ionic liquids, acids and bases.

Example 11

[0218] Example 11 comprises experiments 40 to 44. In each experiment, an ionic liquid having catalyst (lead acetate) dissolved therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a solid acid was added into the flask, and after a further predetermined period of time, a liquid base (aqueous solution of sodium hydroxide) was added into the flask.

[0219] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 11. Table 11 also shows in which figure each particular experiment is illustrated.

TABLE-US-00011 TABLE 11 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 40 Pb(OAc).sub.23H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] citric acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (2.5 min) (21.6 min) 41 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] KH.sub.2PO.sub.4 NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.4 min) (6.5 min) 42 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] NaHSO.sub.4 NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.3 min) (4.3 min) 43 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] succinic acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.3 min) (6.7 min) 44 Pb(OAc).sub.23H.sub.2O UHP [EMIM][OAc] benzoic acid NaOH.sub.(aq.) (1008 mg) (20 g) (10 g) (0.3 min) (5.2 min)

[0220] In each of FIGS. 40-44, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0221] FIGS. 40-44 show that the peroxide decomposition reaction is stopped promptly upon addition of a solid acid, and is restarted promptly upon addition of an aqueous base solution.

[0222] Example 11 proves that the peroxide decomposition reaction can be stopped by addition of different solid acids.

Example 12

[0223] Example 12 comprises experiments 45 to 49. In each experiment, an ionic liquid having catalyst dissolved or dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a solid or liquid acid was added into the flask, and after a further predetermined period of time, a solid base was added into the flask.

[0224] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 12. Table 12 also shows in which figure each particular experiment is illustrated.

TABLE-US-00012 TABLE 12 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 45 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] NaHSO.sub.4(s) K.sub.2CO.sub.3(s) (1109 mg) (40 g) (25 g) (4.3 min) (30.4 min) 46 Mn(OAc).sub.24H.sub.2O UHP [BMIM][OAc] KH.sub.2PO.sub.4(s) KOH.sub.(s) (367.9 mg) (20 g) (10 g) (3.0 min) (27.5 min) 47 Mn(OAc).sub.24H.sub.2O UHP) [EMIM][OAc] HCl.sub.(aq.) CaO.sub.(s) (367.9 mg) (20 g) (10 g) (1.2 min) (10.1 min) 48 Mn(OAc).sub.24H.sub.2O UHP [EMIM][OAc] H.sub.2SO.sub.4(aq.) sodium (367.9 mg) (20 g) (10 g) (1.1 min) percarbonate(s) (20.0 min) 49 FeCl.sub.36H.sub.2O UHP [EMIM][OAc] HNO.sub.3(aq.) K.sub.3PO.sub.4(s) (57.4 mg) (20 g) (10 g) (0.1 min) (20.0 min)

[0225] In each of FIGS. 45-49, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total from UHP.

[0226] FIGS. 45-49 show that the peroxide decomposition reaction is stopped promptly upon addition of a liquid or solid acid, and is restarted promptly upon addition of a solid base.

[0227] Example 12 proves that the decomposition of a peroxide compound in an ionic liquid can be stopped by adding an acid, and can be restarted by addition of solid bases. The phenomenon is not limited to particular acids, bases, catalysts, etc., but rather the concept is widely applicable to different combinations of catalysts, ionic liquids, peroxides, acids, and bases.

Example 13

[0228] Example 13 comprises experiments 50-54. In each experiment, an ionic liquid having catalyst dissolved or dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, an ionic liquid having acidic functionality was added into the flask, and after a further predetermined period of time, a liquid base (aqueous solution of sodium hydroxide) was added into the flask.

[0229] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 13. Table 13 also shows in which figure each particular experiment is illustrated.

TABLE-US-00013 TABLE 13 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 50 Mn(OAc).sub.24H.sub.2O UHP [EMIM][OAc] [EMIM][HSO.sub.4] NaOH.sub.(aq.) (367.9 mg) (20 g) (10 g) (1.6 min) (26.4 min) 51 Pb(OAc).sub.23H.sub.2O UHP [EMIM][EtSO.sub.4] [EMIM][HSO.sub.4] NaOH.sub.(aq.) (1008.0 mg) (20 g) (10 g) (0.1 min) (26.4 min) 52 MnO.sub.2 UHP [MMIM][PO.sub.4Me.sub.2] [EMIM][HSO.sub.4] NaOH.sub.(aq.) (1108.8 mg) (40 g) (25 g) (2.2 min) (60.1 min) 53 CoSO.sub.47H.sub.2O UHP [EMIM][OAc] [EMIM][HSO.sub.4] NaOH.sub.(aq.) (14.9 mg) (20 g) (10 g) (1.2 min) (19.2 min) 54 FeCl.sub.36H.sub.2O UHP [EMIM][OAc] [EMIM][HSO.sub.4] NaOH.sub.(aq.) (14.4 mg) (20 g) (10 g) (0.4 min) (30.0 min)

[0230] In each of FIGS. 50-55, line 1 indicates the time of addition of the ionic liquid with acidic functionality, line 2 indicates the time of addition of the base, lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total.

[0231] FIGS. 50-54 show that the peroxide composition reaction is stopped promptly upon addition of an ionic liquid having acidic functionality, and is restarted promptly upon addition of a liquid base.

[0232] Thus, example 13 proves that the peroxide decomposition reaction in ionic liquids can be stopped by adding an additional ionic liquid having acidic functionality. Termination of the decomposition reaction by acidic ionic liquids is not limited to particular decomposition catalysts.

Example 14

[0233] Example 14 comprises experiments 55-59. In each experiment, an ionic liquid having catalyst dissolved or dispersed therein was added to a peroxide compound (UHP) contained in a glass flask. After a predetermined period of time, a liquid acid was added into the flask, and after a further predetermined period of time, an ionic liquid having basic functionality was added into the flask.

[0234] Types and amounts of the compounds used in each experiment, as well as the time of addition (in minutes after start of the runtime) of acids and bases are listed in table 14. Table 14 also shows in which figure each particular experiment is illustrated.

TABLE-US-00014 TABLE 14 peroxide ionic acid base Figure/ catalyst adduct liquid (time of (time of experiment (mass) (mass) (mass) addition) addition) 55 Mn(OAc).sub.24H.sub.2O UHP [EMIM][OAc] [EMIM][HSO.sub.4] [EMIM][OAc] (367.9 mg) (20 g) (10 g) (1.0 min) (16.1 min) 56 MnO.sub.2 UHP [EMIM][EtSO.sub.4] H.sub.2SO.sub.4(aq.) [EMIM][OAc] (1108.8 mg) (40 g) (25 g) (1.6 min) (20.2 min) 57 FeCl.sub.36H.sub.2O UHP [EMIM][OAc] H.sub.2SO.sub.4(aq.) [EMIM][OAc] (14.4 mg) (20 g) (10 g) (0.3 min) (7.8 min) 58 CoSO.sub.47H.sub.2O UHP [EMIM][OAc] H.sub.2SO.sub.4(aq.) [EMIM][OAc] (14.9 mg) (20 g) (10 g) (1.3 min) (6.0 min) 59 CuCl.sub.22H.sub.2O UHP [MMIM][PO.sub.4Me.sub.2] H.sub.2SO.sub.4(aq.) [EMIM][OAc] (18.1 mg) (20 g) (5 g) (2.9 min) (15.4 min)

[0235] In each of FIGS. 55-59, line 1 indicates the time of addition of the acid, line 2 indicates the time of addition of the base (additional ionic liquid having basic functionality), lines 3 and 4 indicate the oxygen flow rates, and line 5 indicates the oxygen volume released in total.

[0236] FIGS. 55-59 show that the peroxide decomposition reaction can be stopped or decelerated by adding a liquid acid. In the reaction shown in FIG. 58 the amount of added sulfuric acid was not sufficient to achieve a complete termination of the decomposition reaction promptly. FIGS. 55-59 also show that the peroxide decomposition reaction can be restarted by adding ionic liquids having basic functionality.

[0237] Thus, example 14 proves that ionic liquids having basic properties can restart interrupted peroxide decomposition reactions. This phenomenon is not limited to particular oxygen generating compositions, but rather the concept is widely applicable to different catalysts, peroxide compounds and ionic liquids.

[0238] FIG. 60 illustrates an exemplary device 1 for generating oxygen in a controlled manner, the device having one single reaction chamber 2 for storing the composition for generating oxygen. In such a single reaction chamber 2 at least one of the constituents of the composition for generating oxygen can be enclosed in a receptacle in order to avoid contact with the remaining constituents of the composition contained in the reaction chamber 2. The device is particularly suitable for use with neutral and basic ionic liquids. In the embodiment shown in FIG. 60, two receptacles 5, 6 are arranged in the reaction chamber. Receptacle 5 contains an intimate mixture of the oxygen source 7 and the decomposition catalyst 9, for example in powder form or compressed into pellets, in a thoroughly dried condition. Receptacle 6 contains the ionic liquid 8.

[0239] Alternatively, there may be only one receptacle for enclosing the peroxide/catalyst mixture, while the ionic liquid is free within reaction chamber 2, or ionic liquid 8 may be enclosed within a receptacle, while the peroxide/catalyst mixture is not enclosed in a separate receptacle. Further alternatively, the catalyst may be dissolved (soluble metal salts) or partly dissolved (partly soluble metal salts) or dispersed (insoluble metals salts or metal oxide compounds) in the ionic liquid. This alternative is particularly advantageous. It is, in principle, also possible to enclose only the catalyst within a separate receptacle, while the ionic liquid and the peroxide are not enclosed. It is only necessary to avoid contact between all three constituents during storage of the device for generating oxygen.

[0240] It is desirable to store the peroxide 7, the ionic liquid 8 and the catalyst 9 within the reaction chamber 2 in such an arrangement that all constituents will be able to get intimately mixed once oxygen generation is required. When, for example, an insoluble or only partly soluble metal salt is used as a catalyst, and this catalyst and the ionic liquid are provided in one receptacle, and the peroxide in another receptacle, the catalyst may settle within the ionic liquid during storage. In such a case proper mixing with the peroxide may be inhibited. Quick and perfect mixing of all constituents can be achieved when the peroxide and the soluble or insoluble catalyst are intimately mixed in advance in a dry condition, optionally compacted into moulds, and filled either into the reaction chamber 2 or into a separate receptacle 5 to be placed within the reaction chamber 2, and the ionic liquid is provided in a separate receptacle 6. Quick and perfect mixing can also be achieved when the catalyst is soluble in the ionic liquid, and is essentially dissolved therein. Placing the ionic liquid (or the ionic liquid and the catalyst) in a separate receptacle, although this is not absolutely necessary in a case where peroxide and catalyst (or the peroxide alone) are placed in a receptacle 5, constitutes an advantageous precautionary measure against accidental mixing of the constituents in case of receptacle 5 leakage or breakage. Care must be taken, when UHP and catalyst are mixed, because UHP is highly hygroscopic.

[0241] In a situation where oxygen shall be generated, receptacle 5, or receptacles 5 and 6, respectively, are destroyed by a breaking device 18. In FIG. 60, breaking device 18 has the form of a plate, however, means for destroying the receptacle(s) are not limited to plates, and other means are known to persons skilled in the art, for example firing pins or grids. Movement of plate 18 can be achieved by a spring 19 or another activation mechanism. During storage of the device for generating oxygen, spring 19 is under tension and holds plate 18 at a position distant from receptacles 5, 6. Once the tension is released by a suitable trigger mechanism (not shown), spring 19 moves plate 18 towards receptacles 5, 6, and plate 18 destroys receptacles 5, 6. Such a trigger may be, for example, pulling an oxygen mask towards a passenger in an airplane.

[0242] Another exemplary trigger mechanism is an oxygen sensor sensing a low oxygen condition.

[0243] Receptacles 5, 6, and plate 18 are made from materials which guarantee that receptacles 5, 6 will be broken or ruptured when hit by plate 18. Exemplary materials are plastic foils or glass for receptacles 5, 6, and thicker plastic material or metal for plate 18.

[0244] Destruction of receptacles 5, 6 causes mixing of peroxide, ionic liquid, and catalyst, and initiates oxygen generation. In order to allow that the oxygen exits reaction chamber 2, reaction chamber 2 has an opening. In the illustrated embodiment, the opening is sealed with a gas permeable membrane 16. The opening may be at a different position than shown in FIG. 60, or there may be more than one opening.

[0245] In exemplary embodiments, the oxygen generated in the device described herein may be passed through a filter or other purification means as known in the art. The device may be equipped with such means.

[0246] The oxygen generating reaction is an only slightly exothermic process, and proceeds at low temperature, i.e. below 150 C., or even below 120 C. or below 100 C. Therefore, reaction chamber 2 does not need to resist high temperatures, and may be made from lightweight, low melting materials such as plastics. In addition, any bulky insulation is not required. This is particularly advantageous in all cases where weight must be saved and/or space is limited, for example in the case of oxygen masks which shall be installed in an aircraft.

[0247] The exemplary device illustrated in FIG. 60 is equipped with two injection devices 11, 11, for examples syringes or other dosing devices. Openings 17, 17 fluidly connect the interior spaces of reaction chamber 2 and of injection devices 11, 11 respectively.

[0248] The injection device 11 comprises a receptacle 12, a slide bar 13 and a spike 14. The injection device 11 comprises a receptacle 12, a slide bar 13 and a spike 14. Spikes 14, 14 are held in place by fixtures 15, 15. Receptacles 12, 12 are made from a material which can easily be ruptured, for example bags made from plastic foils. Receptacle 12 contains an acidic compound and receptacle 12 contains a basic compound.

[0249] In the exemplary embodiment illustrated in FIG. 60, slide bars 13, 13 can be actuated in an analogous manner as the braking device 18. Once actuated, slide bar 13 pushes receptacle 12 towards spike 14, receptacle 12 is ruptured and acid is injected through opening 17 into reaction chamber 2. Similarly, once actuated, slide bar 13 pushes receptacle 12 towards spike 14, receptacle 12 is ruptured and base is injected through opening 17 into reaction chamber 2.

[0250] Actuation of braking device 18 starts the peroxide decomposition reaction in reaction chamber 2. Without interference, the decomposition reaction proceeds until all peroxide compound has been decomposed. The device illustrated in FIG. 60 allows a user to stop the peroxide decomposition reaction by actuating slide bar 13, and to save the peroxide not yet decomposed for later use. Whenever oxygen is needed again, the user may actuate slide bar 13, thus starting the peroxide decomposition reaction again.

[0251] The device illustrated in FIG. 60 has only one injection device 11 containing an acidic compound, and one injection device 11 containing a basic compound. Such a device allows to stop and to restart the peroxide composition reaction only once. Providing reaction chamber 2 with several injection devices containing an acid, and with several injection devices containing a base allows to stop and to restart the peroxide decomposition several times. For example, a device 1 for generating oxygen having three injection devices containing acidic compounds and having three injection devices containing basic compounds, allows a user to interrupt and to restart the oxygen production three times, or at least until all of the oxygen source has been decomposed.

[0252] If desired, a device as illustrated in FIG. 60 can be also used for reducing or increasing the oxygen flow rate by injecting an acidic compound or a basic compound, respectively into reaction chamber 2, for example when leveling out increasing or decreasing or fluctuating oxygen flow rates shall be achieved.

[0253] It is also possible to provide only injection devices filled with acid, or only injection devices filled with base. In such a case, oxygen generating device 1 will only allow to reduce the oxygen flow rate, or to increase the oxygen flow rate, respectively.

[0254] An alternative exemplary device for generating oxygen in a controlled manner is illustrated in FIG. 61. In FIG. 61 the same reference numerals as in FIG. 60 are used for designating components which correspond to components already illustrated in FIG. 60.

[0255] The device illustrated in FIG. 61 is suitable for use with acidic ionic liquids. In the illustrated embodiment, reaction chamber 2 contains a mixture of acidic ionic liquid 8, oxygen source 7 and decomposition catalyst 9, for example pellets comprising a peroxide/catalyst mixture dispersed within the ionic liquid. Of course, the acidic ionic liquid, the oxygen source and the catalyst may be provided in any different manner, for example in the form of a dispersion of oxygen source powder in a solution of the catalyst within the ionic liquid.

[0256] The exemplary device illustrated in FIG. 61 is equipped with two injection devices 11, 11, which are identical to the injection devices 11, 11 of the device illustrated in FIG. 60. Injection device 11 contains an acidic compound, and injection device 11 contains a basic compound. Injection device 11 may be omitted. An oxygen generating device 1 having only injection device 11 allows to start the peroxide decomposition reaction by destroying receptacle 12 and injecting the basic compound through opening 17 into reaction chamber 2. The peroxide decomposition reaction will then proceed until all peroxide compound has been decomposed, and the oxygen generated by the composition reaction will leave reaction chamber 2 through gas permeable membrane 16.

[0257] A device for generating oxygen in a controlled manner needs at least one further injection device, for example injection device 11 containing an acidic compound, as illustrated in FIG. 61. Injecting the acidic compound contained in injection device 11 into reaction chamber 2 allows to decelerate the peroxide decomposition reaction and to reduce a too high oxygen flow rate.

[0258] In alternative embodiments, the oxygen generating device illustrated in FIG. 61 may be provided with one or more additional injection devices containing basic compounds and/or with one or more additional injection devices containing acidic compounds. Such additional injection devices allow to increase or decrease the oxygen production rate, respectively, or to stop and restart the oxygen production several times.

[0259] The oxygen produced according to this invention is pure and at a low temperature and, therefore, ideal for applications in airplanes, in self-rescuers and in rebreathers for human breathing. However, the use for technical purposes such as in portable welding devices in mining and submarine applications, and in spaceflight, e.g. in control nozzles is also contemplated.

[0260] While the invention has been described with reference to exemplary embodiments, it will be understood by those skilled in the art that various changes may be made and equivalents may be substituted for elements thereof without departing from the scope of the invention. In addition, many modifications may be made to adapt a particular situation or material to the teachings of the invention without departing from the essential scope thereof. Therefore, it is intended that the invention not be limited to the particular embodiment disclosed, but that the invention will include all embodiments falling within the scope of the appended claims.