COMPOSITION FOR GENERATING OXYGEN, OXYGEN GENERATOR, AND METHOD OF GENERATING OXYGEN

Abstract

A composition for generating oxygen includes the following constituents. Potassium superoxide forming an oxygen source. An ionic liquid, which is a salt with at least one cation and at most 100 cations and with at least one anion and at most 100 anions. The composition additionally has a water-containing solution or a water-containing mixture. The water-containing solution contains such an amount of a further salt or such an amount of a further salt together with such an amount of an antifreeze or the water-containing mixture contains such an amount of an antifreeze, that the freezing point of the solution or of the mixture is lowered by at least 10° C. compared to the freezing point of the water.

Claims

1. A composition for generating oxygen, comprising: an oxygen source, said oxygen source being potassium superoxide; an ionic liquid, said ionic liquid being a salt consisting of at least one cation and at most 100 cations, and at least one anion and at most 100 anions; a water-containing solution or a water-containing mixture, said water-containing solution containing a given amount of a further salt or a given amount of the further salt together with a given amount of an antifreeze, or the water-containing mixture contains a given amount of an antifreeze, to effectively lower a freezing point of said water-containing solution or of said water-containing mixture by at least 10° C. compared with a freezing point of the water; said further salt of said water-containing solution being an alkali metal hydroxide, an alkali metal hydroxide hydrate, an alkali metal chloride, an alkali metal chloride hydrate, a hydroxide with an organic cation, a hydrate of a hydroxide with an organic cation, or a mixture of at least two compounds selected from the group consisting of an alkali metal hydroxide, an alkali metal hydroxide hydrate, an alkali metal chloride, an alkali metal chloride hydrate, a hydroxide with an organic cation, and a hydrate of a hydroxide with an organic cation; and said antifreeze includes an alcohol or consists of an alcohol.

2. The composition according to claim 1, consisting of said oxygen source, said ionic liquid, and said water-containing mixture or said water-containing solution.

3. The composition according to claim 1, wherein: said cation or one of said cations of said ionic liquid is an ammonium ion, a substituted ammonium ion, a phosphonium ion, a substituted phosphonium ion, an N-monosubstituted or an N-disubstituted pyrrolidinium ion, an N-monosubstituted or an N′,N-disubstituted imidazolium ion or an N-monosubstituted pyridinium ion; and/or said anion or one of said anions of said ionic liquid is a halide ion, a tetrafluoroborate ion, a hexafluorophosphate ion, a cyanoborate ion, a substituted cyanoborate ion, a sulfonate ion, a bisperfluoroalkylimide ion, a borate ion, a substituted borate ion, a phosphate ion, or a substituted phosphate ion.

4. The composition according to claim 3, wherein: said substituted ammonium ion is a tetraalkylammonium ion, said substituted phosphonium ion is a tetraalkylphosphonium ion, said substituted cyanoborate ion is a perfluoroalkylcyanoborate ion, said sulfonate ion is a perfluoroalkylsulfonate ion, said substituted borate ion is a perfluoroalkylborate ion, said substituted phosphate ion is a perfluoroalkylphosphate ion or a perfluoroalkylfluorophosphate ion.

5. The composition according to claim 3, wherein a substituent of the N-monosubstituted pyrrolidinium ion, of the N-monosubstituted imidazolium ion and of the N-monosubstituted pyridinium ion, and at least one substituent of the N′,N-disubstituted imidazolium ion, and at least one substituent of the N-disubstituted pyrrolidinium ion, is independently selected from alkyl, in particular methyl, ethyl, propyl or butyl, benzyl and aryl.

6. The composition according to claim 1, wherein said ionic liquid is an ionic liquid that is liquid in a temperature range from −60° C. to +150° C.

7. The composition according to claim 6, wherein said ionic liquid is liquid in a temperature range from −40° C. to +110° C.

8. The composition according to claim 1, wherein said antifreeze comprises or consists of a monohydric alcohol, a dihydric alcohol, a trihydric alcohol, or a mixture of at least two alcohols selected from the group consisting of a monohydric alcohol, a dihydric alcohol, and a trihydric alcohol.

9. The composition according to claim 8, wherein the monohydric alcohol is ethanol or octanol, the dihydric alcohol is propylene glycol or ethylene glycol, and the trihydric alcohol is glycerol.

10. The composition according to claim 1, wherein the alkali metal hydroxide is potassium hydroxide or sodium hydroxide, the alkali metal hydroxide hydrate is a hydrate of potassium hydroxide or a hydrate of sodium hydroxide, the alkali metal chloride is sodium chloride, the alkali metal chloride hydrate is a hydrate of lithium chloride, the hydroxide with the organic cation is a tetraalkylammonium hydroxide, and the hydrate of the hydroxide with the organic cation is a hydrate of a tetraalkylammonium hydroxide.

11. The composition according to claim 10, wherein the tetraalkylammonium hydroxide is a tetrabutylammonium hydroxide and the hydrate of the tetraalkylammonium hydroxide is a hydrate of tetrabutylammonium hydroxide.

12. The composition according to claim 1, wherein a total weight of the further salt or a total weight of the further salt together with the total weight of the antifreeze in the water-containing solution relative to a total weight of the water-containing solution or wherein a total weight of the antifreeze in the water-containing mixture relative to a total weight of the water-containing mixture is at least 25% by weight.

13. The composition according to claim 12, wherein the total weight is at least 30% by weight, or at least 35% by weight, or at least 40% by weight.

14. The composition according to claim 1, further comprising, as a further constituent, at least one additive independently selected from sodium dihydrogenphosphate or potassium hydroxide, an additional substance and an antifoam.

15. The composition according to claim 14, wherein the additional substance is a phyllosilicate or fumed silica.

16. The composition according to claim 12, wherein the antifoam comprises or consists of octanol, paraffin wax or a polysiloxane.

17. An oxygen generator, comprising: a first and a second compartment, an opening for releasing or a conduit for discharging oxygen formed in the oxygen generator, and the composition according to claim 1; said oxygen source and said ionic liquid being disposed in said first compartment and said water-containing solution or water-containing mixture being disposed in said second compartment; a physical barrier configured to separate said first compartment from said second compartment and a device for selectively overcoming said physical barrier, wherein said physical barrier is arranged to enable said oxygen source, said ionic liquid and said water-containing solution or water-containing mixture, after overcoming said physical barrier, to come into contact with one another to release oxygen; and said opening or conduit being arranged to allow the oxygen being formed to exit through said opening or through said conduit.

18. The oxygen generator according to claim 17, further comprising at least one delaying device disposed and configured to allow a total amount of said water-containing solution present in the oxygen generator or a total amount of said water-containing mixture present in the oxygen generator, after overcoming said physical barrier, to come into contact only gradually with a total amount of said oxygen source present in the oxygen generator.

19. A method of generating oxygen, the method which comprises providing the composition according to claim 1 and bringing the oxygen source, the ionic liquid, and the water-containing solution or the water-containing mixture of the composition, and optionally an additive, an additional substance or an antifoam, into contact with one another.

20. The method according to claim 19, wherein the step of bringing into contact with one another is effected at a temperature in a range from −70° C. to +110° C.

Description

BRIEF DESCRIPTION OF THE FIGURES

[0067] FIG. 1 shows a graphical representation of the decomposition of potassium superoxide in ambient air as a function of the formulation and the reaction time;

[0068] FIG. 2 shows a schematic experimental setup for determining the decomposition;

[0069] FIG. 3 shows a .sup.19F NMR spectrum of the ionic liquid prior to and after the release of oxygen from potassium superoxide;

[0070] FIG. 4 shows an .sup.11B NMR spectrum of the ionic liquid prior to and after the release of oxygen from potassium superoxide;

[0071] FIG. 5 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen with and without ionic liquid, as a function of the reaction time;

[0072] FIG. 6 shows a graphical representation of the oxygen flow rates as a function of the reaction time during reactions for releasing oxygen with and without ionic liquid;

[0073] FIG. 7 shows a graphical representation of the volume of oxygen released during the reaction for releasing oxygen as a function of the reaction time;

[0074] FIG. 8 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the aqueous solution and of the reaction time;

[0075] FIG. 9 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the ambient temperature and of the reaction time;

[0076] FIG. 10 shows a graphical representation of the oxygen flow rates as a function of the ambient temperature and of the reaction time during reactions for releasing oxygen;

[0077] FIG. 11 shows a further graphical representation of the volume of oxygen released during the reactions for releasing oxygen with and without ionic liquid, as a function of the reaction time;

[0078] FIG. 12 shows a further graphical representation of the oxygen flow rates as a function of the reaction time during reactions for releasing oxygen with and without ionic liquid;

[0079] FIG. 13 shows a further graphical representation of the volume of oxygen released during the reaction for releasing oxygen as a function of the reaction time;

[0080] FIG. 14 shows a further graphical representation of the oxygen flow rate as a function of the reaction time during the reaction for releasing oxygen;

[0081] FIG. 15 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the ionic liquid and of the reaction time; and

[0082] FIG. 16 shows a graphical representation of the oxygen flow rates as a function of the ionic liquid and of the reaction time during reactions for releasing oxygen.

[0083] The acronym “IL” used in the figures and in the text below stands for “ionic liquid.”

DETAILED DESCRIPTION OF THE INVENTION

First Exemplary Embodiment

[0084] Two sealed reaction vessels were each adjusted to a temperature of 19.5° C. and each filled with 2 mL of distilled water. Then, either 3 g of pulverulent potassium superoxide or 6 g of a paste consisting of 3 g of potassium superoxide and 3 g of ionic liquid [BMIm][BF(CN).sub.3] were added to one each of the reaction vessels such that they were not in contact with the distilled water. The reaction vessels were each incubated at 19.5° C. for 24 hours. The amount of gas released was determined in each case with a bubble counter. The ionic liquid was analysed prior to and after the reaction by means of .sup.19F NMR spectroscopy and .sup.11B NMR spectroscopy. The results are presented in FIGS. 1, 3 and 4 and in Table 1. A schematic experimental setup is presented in FIG. 2.

TABLE-US-00001 TABLE 1 O.sub.2 evolution O.sub.2 evolution detected after KO.sub.2 conversion Oxygen source detected after [h] 24 h [mL] after 24 h [%] KO.sub.2 powder 1 670 89 KO.sub.2/IL paste 2.5 410 54

[0085] It is apparent from FIG. 1 and Table 1 that in the case of potassium superoxide as a powder the decomposition of the potassium superoxide begins after one hour. It is additionally apparent that after 24 hours of incubation time, 89% by weight of the employed potassium superoxide has decomposed. The decomposition of the potassium superoxide in the paste begins after 2.5 hours. It is additionally apparent that after 24 hours of incubation time, 54% by weight of the employed potassium superoxide in the paste has decomposed. A paste consisting of potassium superoxide and ionic liquid increases the stability of the potassium superoxide in a humid atmosphere.

[0086] It is apparent from FIGS. 3 and 4 that there are no differences in the .sup.19F and .sup.11B NMR spectra of the ionic liquid [BMIm][BF(CN).sub.3] prior to and after the above decomposition reaction. The ionic liquid does not take part in the reaction for releasing oxygen and is not chemically altered by this reaction.

Second Exemplary Embodiment

[0087] 10 g in each case of pulverulent potassium superoxide were initially charged as oxygen source into four cylindrical reaction vessels having an internal diameter of 28 mm. Either 5 g of [BMPL][BF(CN).sub.3], 5 g of [BMIm][BF(CN).sub.3] or 10 g of [BMIm][BF(CN).sub.3] were added. In one reaction vessel, no ionic liquid was added. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 20 mL in each case of a 9 M potassium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The reaction was terminated after 15 minutes. The results are presented in FIGS. 5 and 6 and in Table 2.

TABLE-US-00002 TABLE 2 After 10 minutes of reaction time Flow rate.sub.max ReactionTemp. O.sub.2 volume O.sub.2 volume Ionic liquid [L/h] [° C.] [L] [%] Without 135 49 2.37 95 5 g of [BMIm][BF(CN).sub.3] 38 32 1.55 61 10 g of [BMIm][BF(CN).sub.3] 21 28 1.53 61 5 g of [BMPL][BF(CN).sub.3] 42 31 1.74 70

[0088] It is apparent from this that, without the addition of an ionic liquid, the maximum yield in gas volume of 2.37 L is reached after 10 minutes of reaction time. Addition of 5 g of [BMIm][BF(CN).sub.3] results in a maximum yield in gas volume of 1.55 L being reached after 10 minutes of reaction time. Addition of 10 g of [BMIm][BF(CN).sub.3] results in a maximum yield of 1.55 L being reached after 10 minutes of reaction time. Addition of 5 g of [BMPL][BF(CN).sub.3] results in a maximum yield of 1.82 L being reached. This reaction was terminated after 15 minutes. The maximum gas volume that can theoretically be generated in this reaction is 2.51 L. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course as a result of the addition of the ionic liquid. As a result of the addition of the ionic liquid, the oxygen is released more continuously and more uniformly.

Third Exemplary Embodiment

[0089] 10 g of pulverulent potassium superoxide were initially charged as oxygen source into a cylindrical reaction vessel having an internal diameter of 28 mm. 5 g of [BMPL][BF(CN).sub.3] were added. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 20 mL in each case of a 9 M potassium hydroxide solution. The reaction vessel was sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessel. The oxygen flow rate and the length of the reaction time until complete conversion of the potassium superoxide were additionally measured. The result is presented in FIG. 7. It is apparent from this that, with the addition of [BMPL][BF(CN).sub.3], the maximum yield in gas volume of 2520 mL is reached after 260 minutes. As a result of the addition of the ionic liquid [BMPL][BF(CN).sub.3], the oxygen is released continuously and uniformly over a long reaction time period.

Fourth Exemplary Embodiment

[0090] 1 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into two cylindrical reaction vessels having an internal diameter of 24 mm. 0.5 g of [BMPL][BF(CN).sub.3] were added in each case. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding either 2 mL of a 9 M potassium hydroxide solution or 2 mL of an aqueous 1.5 M tetrabutylammonium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The length of the reaction time was additionally measured. The reaction was terminated after 100 minutes. The results are presented in FIG. 8. It is apparent from this that, without the addition of an aqueous tetrabutylammonium hydroxide solution, the maximum yield in gas volume of 0.21 L is reached after 4 minutes of reaction time. The addition of an aqueous potassium hydroxide solution results in the maximum yield in gas volume of 0.21 L being reached after 93 minutes of reaction time. As a result of the addition of the aqueous potassium hydroxide solution, the oxygen is released over a longer period of time.

Fifth Exemplary Embodiment

[0091] 0.5 g of [BMPL][BF(CN).sub.3] were in each case added to 1 g of pulverulent potassium superoxide as oxygen source in three cylindrical reaction vessels having an internal diameter of 24 mm. At an ambient temperature of +70° C., room temperature or −40° C., the reaction for generating oxygen was initiated by adding 2 mL in each case of an aqueous 9 M potassium hydroxide solution that had been adjusted to the respective ambient temperature. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The results are presented in FIGS. 9 and 10 and in Table 3.

TABLE-US-00003 TABLE 3 Starting temperature Flow rate.sub.max Reaction duration [° C.] [L/h] [min] −40 2 186 RT 13 87 70 33 13

[0092] It is apparent from this that, at an ambient temperature of 70° C., the maximum yield in gas volume of 0.21 L is reached after 13 minutes of reaction time. At an ambient temperature of room temperature, the maximum yield in gas volume of 0.21 L is reached after 87 minutes of reaction time. At an ambient temperature of −40° C., the maximum yield in gas volume of 0.21 L is reached after 186 minutes of reaction time. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course at an ambient temperature of −40° C. As a result of an ambient temperature of −40° C., the oxygen is released more continuously and uniformly.

Sixth Exemplary Embodiment

[0093] 10 g of pulverulent potassium superoxide were initially charged as oxygen source in a cylindrical reaction vessel having an internal diameter of 28 mm. A further cylindrical reaction vessel having an internal diameter of 28 mm was initially charged with 15 g of a paste consisting of 10 g of potassium superoxide as oxygen source and 5 g of [BMIm][BF(CN).sub.3]. A further cylindrical reaction vessel having an internal diameter of 28 mm was initially charged with 20 g of a paste consisting of 10 g of potassium superoxide as oxygen source and 10 g of [BMIm][BF(CN).sub.3]. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 20 mL in each case of a 9 M potassium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The results are presented in FIGS. 11 and 12 and in Table 4.

TABLE-US-00004 TABLE 4 After 10 minutes of reaction Reaction time Flow rate.sub.max temperature O.sub.2 volume O.sub.2 volume IL [L/h] [° C.] [L] [%] Without 135 49 2.37 95 5 g of IL 63 29 1.47 58 10 g of IL 36 26 0.90 35

[0094] It is apparent from this that, with pulverulent potassium superoxide, the maximum yield in gas volume of 2.37 L is reached after 8 minutes of reaction time. With the paste consisting of 10 g of potassium superoxide and 5 g of [BMIm][BF(CN).sub.3], a yield of 1.47 L is reached after 10 minutes of reaction time. With the paste consisting of 10 g of potassium superoxide and 10 g of [BMIm][BF(CN).sub.3], a yield of 0.90 L is reached after 10 minutes of reaction time. The maximum gas volume that can theoretically be generated in this reaction is 2.51 L. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course in the case of the pastes consisting of potassium superoxide and [BMIm][BF(CN).sub.3]. In the case of the pastes consisting of potassium superoxide and [BMIm][BF(CN).sub.3], the oxygen is released more continuously and more uniformly. The oxygen is released more continuously and more uniformly the greater the total weight of the ionic liquid is in relation to the total weight of the oxygen source. As a result of the use of ionic liquids in various concentrations, the flow rates of the oxygen generated can be varied within wide limits and thus the reaction duration can be prolonged as desired from a few minutes up to several hours.

Seventh Exemplary Embodiment

[0095] 4.55 g of potassium superoxide and 0.45 g of [BMPL][BF(CN).sub.3] were pressed into tablets. 5 g of these tablets were initially charged in a cylindrical reaction vessel having an internal diameter of 28 mm. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 10 mL of a 9 M potassium hydroxide solution. The reaction vessel was sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessel. The oxygen flow rate and the length of the reaction time were additionally measured. The reaction was terminated after 225 minutes. The results are presented in FIGS. 13 and 14 and in Table 5.

TABLE-US-00005 TABLE 5 Flow rate.sub.max Reaction temp. O.sub.2 volume O.sub.2 volume Reaction [L/h] [° C.] [L] [%] duration [min] 104 27 1.11 94 219

[0096] It is apparent from this that, in the case of potassium superoxide and [BMPL][BF(CN).sub.3], pressed into tablets, the yield in gas volume of 1.11 L is reached after 219 minutes of reaction time. The maximum gas volume that can theoretically be generated in this reaction is 1.14 L. It is apparent from the flow curve profile ascertained via the measured flow rates that immediately after addition of the aqueous potassium hydroxide solution a maximum flow rate of 104 L per hour is reached. After the maximum flow rate has been reached, the flow rate decreases continuously.

Eighth Exemplary Embodiment

[0097] An open reaction vessel was initially charged with 2 g of pulverulent potassium superoxide and 4 g of a paste consisting of 2 g of potassium superoxide and 2 g of [BMPL][BF(CN).sub.3]. The reaction vessels were each adjusted to an ambient temperature of +70° C. and held at this ambient temperature for 24 hours. No weighable loss of weight was detected in either sample after 24 h at +70° C. ambient temperature.

Ninth Exemplary Embodiment

[0098] 1 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into three cylindrical reaction vessels having an internal diameter of 24 mm. Either 0.5 g of [BMPL]Cl, 0.5 g of [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or 0.5 g of [EMIm][SO.sub.3CF.sub.3] were added. In contrast to the ionic liquid [BMPL]Cl, the ionic liquids [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or [EMIm][SO.sub.3CF.sub.3] contain relatively hydrophobic anions. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 2 mL in each case of a 9 M potassium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 75 minutes. The results are presented in FIGS. 15 and 16 and in Table 6.

TABLE-US-00006 TABLE 6 After 10 minutes of reaction time Flow rate.sub.max O.sub.2 volume O.sub.2 volume Ionic liquid [L/h] [mL] [%] [BMPL]CI 30 220 87 [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] 12 195 78 [EMIm][SO.sub.3CF.sub.3] 11 175 70

[0099] It is apparent from this that, with the addition of [BMPL]Cl, the maximum yield in gas volume of 220 mL is reached after 5 minutes of reaction time. The addition of [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] results in the maximum yield in gas volume of 200 mL being reached after 26 minutes of reaction time. The addition of [EMIm][SO.sub.3CF.sub.3] results in the maximum yield in gas volume of 190 mL being reached after 41 minutes of reaction time. The maximum gas volume that can theoretically be generated in this reaction is 250 mL. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course as a result of addition of the ionic liquids [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] and [EMIm][SO.sub.3CF.sub.3] having hydrophobic anions. As a result of the addition of an ionic liquid having hydrophobic anions, the oxygen is released more continuously and more uniformly.

Tenth Exemplary Embodiment

[0100] 1 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into three cylindrical reaction vessels having an internal diameter of 24 mm. Either 0.5 g of [BMPL]Cl, 0.5 g of [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or 0.5 g of [EMIm][SO.sub.3CF.sub.3] were added. In contrast to the ionic liquid [BMPL]Cl, the ionic liquids [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or [EMIm][SO.sub.3CF.sub.3] contain relatively hydrophobic anions. Next, the reaction for generating oxygen was initiated at an ambient temperature of −20° C. by adding 2 mL in each case of a 40% aqueous propylene glycol mixture that had been adjusted to an ambient temperature of −20° C. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 75 minutes. The volume of the oxygen generated and the flow curve profile ascertained via the measured flow rates are similar to the results shown in exemplary embodiment 9. Here too, as a result of the addition of an ionic liquid having hydrophobic anions, the oxygen is released more continuously and more uniformly.

Eleventh Exemplary Embodiment

[0101] 1 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into three cylindrical reaction vessels having an internal diameter of 24 mm. Either 0.5 g of [BMPL]Cl, 0.5 g of [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or 0.5 g of [EMIm][SO.sub.3CF.sub.3] were added. In contrast to the ionic liquid [BMPL]Cl, the ionic liquids [HMIm][P(C.sub.2F.sub.5).sub.3F.sub.3] or [EMIm][SO.sub.3CF.sub.3] contain relatively hydrophobic anions. Next, the reaction for generating oxygen was initiated at an ambient temperature of −20° C. by adding 2 mL in each case of a 50% aqueous ethylene glycol mixture that had been adjusted to an ambient temperature of −20° C. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided through a drum-type gas meter to measure the volume of the oxygen generated from the reaction vessels. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 75 minutes. The volume of the oxygen generated and the flow curve profile ascertained via the measured flow rates are similar to the results shown in exemplary embodiment 9. Here too, as a result of the addition of an ionic liquid having hydrophobic anions, the oxygen is released more continuously and more uniformly.