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

Abstract

A composition for generating oxygen includes, or is exclusively formed of, the following constituents: an oxygen source, the oxygen source being potassium superoxide, and a water-containing solution or a water-containing mixture. The water-containing solution contains such an amount of a salt or such an amount of a 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. There is also described an oxygen generator and a method of generating oxygen.

Claims

1. A composition for generating oxygen, comprising: an oxygen source, said oxygen source being potassium superoxide; a water-containing solution or a water-containing mixture, said water-containing solution containing a given amount of a salt or a given amount of a salt together with a given amount of an antifreeze, or said water-containing mixture containing a given amount of an antifreeze, to effectively lower a freezing point of said water-containing solution or of said water-containing by at least 10° C. compared to a freezing point of the water; said 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; said antifreeze including an alcohol or consisting of an alcohol.

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

3. 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.

4. The composition according to claim 1, wherein said monohydric alcohol is ethanol or octanol, said dihydric alcohol is propylene glycol or ethylene glycol, and said trihydric alcohol is glycerol.

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

6. The composition according to claim 5, wherein said tetraalkylammonium hydroxide is a tetrabutylammonium hydroxide and said hydrate of a tetraalkylammonium hydroxide is a hydrate of tetrabutylammonium hydroxide.

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

8. The composition according to claim 7, wherein the total weight of said water-containing mixture is at least 40% by weight.

9. The composition according to claim 1, wherein said oxygen source is present in solid form, or wherein said oxygen source is present in suspended form in an ionic liquid, or wherein said oxygen source and an ionic liquid are present in a pressed form with said ionic liquid forming a binder, and wherein said ionic liquid is a salt that is in a liquid state and consists of at least one cation and at most 100 cations and of at least one anion and at most 100 anions.

10. 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.

11. The composition according to claim 10, wherein said additional substance is a phyllosilicate or fumed silica.

12. The composition according to claim 10, wherein said antifoam comprises or consists of octanol, paraffin wax or a polysiloxane.

13. The composition according to claim 1, wherein a total weight of said oxygen source relative to a total weight of the composition amounts to at least 5% by weight and at most 90% by weight, and wherein a remainder of the composition consists of the water-containing solution or the water-containing mixture and, optionally, the ionic liquid and/or a further constituent.

14. 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 being disposed in said first compartment and the water-containing solution or the 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 and said water-containing solution or said water-containing mixture, after overcoming said physical barrier, to come into contact with one another; and said opening or conduit being arranged to allow the oxygen being formed to exit through said opening or through said conduit.

15. The oxygen generator according to claim 14, further comprising an additive selected from the group consisting of sodium dihydrogenphosphate or potassium hydroxide, an additional substance and an antifoam disposed either in said first compartment or in said second compartment,

16. The oxygen generator according to claim 14, further comprising a 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, comes into contact only gradually with a total amount of said oxygen source present in the oxygen generator.

17. The oxygen generator according to claim 16, wherein said delaying means is a perforated, semipermeable membrane or a bulk material, which surrounds or covers said oxygen source or is mixed with said oxygen source and is inert with respect to said oxygen source and said water-containing solution or said water-containing mixture.

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

19. The method according to claim 18, which comprises bringing the components into contact with one another at a temperature in a temperature range from −70° C. to +110° C.

20. The method according to claim 19, which comprises bringing the components into contact with one another at a temperature in a temperature range from −40° C. to −20° C.

Description

BRIEF DESCRIPTION OF THE FIGURES

[0063] FIG. 1 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;

[0064] FIG. 2 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;

[0065] FIG. 3 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the water-containing solution and of the reaction time;

[0066] FIG. 4 shows a graphical representation of the volume of oxygen released by sodium peroxide as oxygen source during the reaction for releasing oxygen, as a function of the reaction time;

[0067] FIG. 5 shows a further graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the water-containing solution and of the reaction time;

[0068] FIG. 6 shows a graphical representation of the oxygen flow rates as a function of the water-containing solution and of the reaction time during reactions for releasing oxygen;

[0069] FIG. 7 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the reactor diameter and of the reaction time;

[0070] FIG. 8 shows a graphical representation of the oxygen flow rates as a function of the reactor diameter and of the reaction time during reactions for releasing oxygen;

[0071] FIG. 9 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the reactor base area and of the reaction time;

[0072] FIG. 10 shows a graphical representation of the oxygen flow rates as a function of the reactor base area and of the reaction time during reactions for releasing oxygen;

[0073] FIG. 11 shows a graphical representation of the linear relationship between reactor base area and oxygen flow rates during reactions for releasing oxygen;

[0074] FIG. 12 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the addition rate for the water-containing solution and of the reaction time;

[0075] FIG. 13 shows a graphical representation of the oxygen flow rates as a function of the addition rate for the water-containing solution and of the reaction time during reactions for releasing oxygen;

[0076] FIG. 14 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the height and nature of a bed and of the reaction time;

[0077] FIG. 15 shows a graphical representation of the oxygen flow rates as a function of the height and nature of a bed and of the reaction time during reactions for releasing oxygen;

[0078] FIG. 16 shows a graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the form of the oxygen source and of the reaction time;

[0079] FIG. 17 shows a graphical representation of the oxygen flow rates as a function of the form of the oxygen source and of the reaction time during reactions for releasing oxygen;

[0080] FIG. 18 shows a further graphical representation of the volume of oxygen released during the reactions for releasing oxygen as a function of the form of the oxygen source and of the reaction time;

[0081] FIG. 19 shows a further graphical representation of the oxygen flow rates as a function of the form of the oxygen source and of the reaction time during reactions for releasing oxygen;

[0082] FIG. 20 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;

[0083] FIG. 21 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;

[0084] FIG. 22 shows a graphical representation of the volume of oxygen released during the reaction for releasing oxygen as a function of the reaction time;

[0085] FIG. 23 shows a graphical representation of the oxygen flow rate as a function of the reaction time during the reaction for releasing oxygen;

[0086] FIG. 24 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;

[0087] FIG. 25 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;

[0088] FIG. 26 shows a further 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; and

[0089] FIG. 27 shows a further graphical representation of the oxygen flow rates as a function of the ambient temperature and of the reaction time during reactions for releasing oxygen.

[0090] The acronym “IL” used in the figures and in the text below stands for “ionic liquid.”

DETAILED DESCRIPTION OF THE INVENTION

First Exemplary Embodiment

[0091] 100 g in each case of pulverulent potassium superoxide was added as oxygen source to three cylindrical reaction vessels having an internal diameter of 55 mm. At an ambient temperature of +70° C., room temperature or −20° C., the reaction for generating oxygen was initiated by adding 100 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The results are presented in FIGS. 1 and 2 and in Table 1.

TABLE-US-00001 TABLE 1 Starting Flow Reaction O.sub.2 O.sub.2 Reaction temperature rate.sub.max temperature volume volume duration [° C.] [L/h] [° C.] [L] [%] [min] −20 371 45 24.9 99 39 RT 287 64 24.9 99 17 +70 564 85 24.9 99 10

[0092] It is apparent from this that, at an ambient temperature of +70° C., the maximum yield in gas volume of 24.9 L is reached after 10 minutes of reaction time. At an ambient temperature of room temperature, the maximum yield in gas volume of 24.9 L is reached after 17 minutes of reaction time. At an ambient temperature of −20° C., the maximum yield in gas volume of 24.9 L is reached after 39 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 −20° C. As a result of an ambient temperature of −20° C., the oxygen is released more continuously and uniformly.

Second Exemplary Embodiment

[0093] 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 an aqueous 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The length of the reaction time was additionally measured. The results are presented in FIG. 3. It is apparent from this that, with 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 92 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.

Third Exemplary Embodiment

[0094] 5 g of pulverulent sodium peroxide was initially charged as oxygen source into a cylindrical reaction vessel. Next, at an ambient temperature of −20° C., 5 mL of an aqueous 6.9 M potassium hydroxide solution comprising 2 mol % of the metal-containing catalyst manganese acetate (abbreviation: Mn(OAc).sub.2), were added, this being adjusted to an ambient temperature of −20° C. The reaction vessel was sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessel through a drum-type gas meter to measure the volume of the oxygen generated. The length of the reaction time was additionally measured. The reaction was terminated after 20 minutes. The result is presented in FIG. 4. It is apparent from this that, with sodium peroxide as oxygen source and at an ambient temperature of −20° C., an increase in the gas volume, measurable via the heating of the composition, is achieved after 8 minutes. However, the reaction for generating oxygen was initiated only after 2 minutes. A maximum yield in gas volume of 725 mL is reached after 18 minutes. In contrast to the results presented in FIGS. 1 and 2 and Table 1, the reaction for generating oxygen proceeds markedly more slowly with sodium peroxide as oxygen source than with potassium superoxide as oxygen source. Moreover, the addition of the metal-containing catalyst Mn(OAc).sub.2 is necessary when generating oxygen with sodium peroxide.

Fourth Exemplary Embodiment

[0095] 10 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into three cylindrical reaction vessels having an internal diameter of 28 mm. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding either 20 mL of water, 20 mL of an aqueous 9 M potassium hydroxide solution or 20 mL of an aqueous 3 M sodium dihydrogenphosphate solution. The pH of the water was 7. The pH of the aqueous 9 M potassium hydroxide solution was 15. The pH of the aqueous 3 M sodium dihydrogenphosphate solution was 3. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurements was halted after 8 minutes since in all cases an oxygen yield of 99% had been achieved. The results are presented in FIGS. 5 and 6 and in Table 2.

TABLE-US-00002 TABLE 2 Aqueous solution Reaction Flow O.sub.2 O.sub.2 (Concentration temperature rate.sub.max volume volume [mol L.sup.−1]) [° C.] [L/h] [L] [%] KOH (9) 49 135 2.5 99 H.sub.2O 63 299 2.5 99 NaH.sub.2PO.sub.4 (3) 81 377 2.5 99

[0096] It is apparent from this that, for all reactions, a maximum yield in gas volume of 2.5 L is reached. Addition of water resulted in the achievement of a maximum reaction temperature of 63° C. and a maximum oxygen flow rate of 299 L/h. Addition of the aqueous potassium hydroxide solution resulted in the achievement of a maximum reaction temperature of 49° C. and a maximum oxygen flow rate of 135 L/h. Addition of aqueous sodium dihydrogenphosphate solution resulted in the achievement of a maximum reaction temperature of 81° C. and a maximum oxygen flow rate of 377 L/h. Depending on whether and in which concentration a salt has been dissolved in the aqueous solution, this has an influence on the maximum reaction temperature and on the maximum oxygen flow rate during the reaction for generating oxygen. Here, a higher maximum reaction temperature results in a higher maximum oxygen flow rate. 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 aqueous potassium hydroxide solution. As a result of the addition of the aqueous potassium hydroxide solution, the oxygen is released more continuously and more uniformly.

Fifth Exemplary Embodiment

[0097] 25 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into four cylindrical reaction vessels having an internal diameter of either 42 mm, 55 mm, 71 mm or 105 mm. Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 50 mL in each case of an aqueous 9 M potassium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 7 minutes since in all cases a yield of 98% of the achievable oxygen volume had been reached. The results are presented in FIGS. 7 and 8 and in Table 3.

TABLE-US-00003 TABLE 3 Internal Flow O.sub.2 O.sub.2 diameter rate.sub.max volume volume [mm] [L/h] [L] [%] 42 148 6.4 98 55 203 6.4 98 71 273 6.4 98 105 316 6.4 98

[0098] It is apparent from this that, for all reactions, a maximum yield in gas volume of 6.4 L is reached. With an internal diameter of the cylindrical reaction vessel of 42 mm, a maximum oxygen flow rate of 148 L/h is reached. With an internal diameter of the cylindrical reaction vessel of 55 mm, a maximum oxygen flow rate of 203 L/h is reached. With an internal diameter of the cylindrical reaction vessel of 71 mm, a maximum oxygen flow rate of 273 L/h is reached. With an internal diameter of the cylindrical reaction vessel of 105 mm, a maximum oxygen flow rate of 316 L/h is reached. The internal diameter of the cylindrical reaction vessel has an influence on the maximum oxygen flow rate during the reaction for generating oxygen. In this case, a greater internal diameter of the cylindrical reaction vessel results in a higher maximum oxygen flow rate. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course in the case of an internal diameter of the cylindrical reaction vessel of 42 mm. With an internal diameter of the cylindrical reaction vessel of 42 mm, the oxygen is released more continuously and more uniformly.

Sixth Exemplary Embodiment

[0099] 25 g in each case of pulverulent potassium superoxide was initially charged into four reaction vessels. The reaction vessels had either a circular base area shape with an internal diameter of 42 mm (1400 mm.sup.2 base area), 71 mm (2400 mm.sup.2 base area) or 105 mm (8700 mm.sup.2 base area) or or a square base area shape with an internal diameter of 80 mm (6400 mm.sup.2 base area). Next, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 50 mL in each case of an aqueous 9 M potassium hydroxide solution. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 8 minutes since in all cases a yield of 98% of the achievable oxygen volume had been reached. The results are presented in FIGS. 9 and 10 and in Table 4.

TABLE-US-00004 TABLE 4 Base area Flow O.sub.2 O.sub.2 [mm.sup.2] rate.sub.max volume volume (shape) [L/h] [L] [%] 1400 (circle) 148 6.4 98 2400 (circle) 203 6.4 98 6400 (square) 277 6.4 98 8700 (circle) 316 6.4 98

[0100] It is apparent from this that, for all reactions, a maximum yield in gas volume of 6.4 L is reached. With a circular base area of 1400 mm.sup.2, a maximum oxygen flow rate of 148 L/h is reached. With a circular base area of 2400 mm.sup.2, a maximum oxygen flow rate of 203 L/h is reached. With a square base area of 6400 mm.sup.2, a maximum oxygen flow rate of 277 L/h is reached. With a circular base area of 8700 mm.sup.2, a maximum oxygen flow rate of 316 L/h is reached. The base area of the reaction vessel has an influence on the maximum oxygen flow rate during the reaction for generating oxygen. A linear relationship between base area of the reaction vessel and maximum oxygen flow rate is presented in FIG. 11. It is apparent from this that a greater base area of the reaction vessel results in a higher maximum oxygen flow rate. It is moreover apparent from this that the base area shape of the reaction vessel does not have any influence on the maximum oxygen flow rate. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course in the case of a base area of the reaction vessel of 1400 mm.sup.2. With a base area of the reaction vessel of 1400 mm.sup.2, the oxygen is released more continuously and more uniformly.

Seventh Exemplary Embodiment

[0101] 25 g in each case of pulverulent potassium superoxide was added as oxygen source to three cylindrical reaction vessels having an internal diameter of 42 mm. At an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 50 mL in each case of aqueous 9 M potassium hydroxide solution. The 50 mL of the aqueous potassium hydroxide solution was added within an addition time of either 11 seconds, 33 seconds or 99 seconds. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 10 minutes. The results are presented in FIGS. 12 and 13. It is apparent from this that, for all reactions, a maximum yield in gas volume of 5.9 L is reached. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course with an addition time of 99 seconds. The addition time for the aqueous potassium hydroxide solution has an influence on the maximum oxygen flow rate during the reaction for generating oxygen. In this case, a longer addition time for the aqueous potassium hydroxide solution results in a lower maximum oxygen flow rate.

Eighth Exemplary Embodiment

[0102] 25 g in each case of pulverulent potassium superoxide was initially charged as oxygen source into four cylindrical reaction vessels having an internal diameter of 42 mm. In the reaction vessels, the initially charged potassium superoxide was overlaid either with a bed of sea sand with a bed height of 15 mm or with a bed of glass beads with a bed height of either 12 mm or 25 mm. In one reaction vessel, the initially charged potassium superoxide was not overlaid with a bed. Next, at an ambient temperature of −20° C., 50 mL in each case of an aqueous 9 M potassium hydroxide solution, adjusted to an ambient temperature of −20° C., were added to the reaction vessels. The reaction vessels were each sealed and the oxygen released by the reaction for generating oxygen was guided out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 70 minutes. The results are presented in FIGS. 14 and 15 and in Table 5.

TABLE-US-00005 TABLE 5 After 15 min of reaction time Flow O.sub.2 O.sub.2 Nature of bed rate.sub.max volume volume (height [mm]) [L/h] [L] [%] Without 94 5.49 84 Sea sand (15) 37 4.58 70 Glass beads (12) 18 2.54 39 Glass beads (25) 8.5 1.50 23

[0103] It is apparent from this that, after 15 minutes of reaction time, a maximum yield in gas volume of 5.49 L and a maximum oxygen flow rate of 94 L/h is made possible with the reaction without bed. For the reaction with a bed of sea sand having a bed height of 15 mm, a maximum yield in gas volume of 4.58 L and a maximum oxygen flow rate of 37 L/h is made possible after 15 minutes of reaction time. For the reaction with a bed of glass beads having a bed height of 12 mm, a maximum yield in gas volume of 2.54 L and a maximum oxygen flow rate of 18 L/h is made possible after 15 minutes of reaction time. For the reaction with a bed of glass beads having a bed height of 25 mm, a maximum yield in gas volume of 1.50 L and a maximum oxygen flow rate of 8.5 L/h is made possible after 15 minutes of reaction time. The nature and height of the bed has an influence on the maximum oxygen flow rate during the reaction for generating oxygen. In this case, a greater bed height results in a lower oxygen flow rate during the reaction for generating oxygen. The flow curve profile ascertained via the measured flow rates has a markedly more plateau-shaped course for the reactions with potassium superoxide overlaid with a bed. In the reactions with potassium superoxide overlaid with a bed, oxygen is released more continuously and more uniformly. This is down to the fact that the bed enables fixing of the potassium superoxide in the reaction vessel. Floating and/or swirling of the potassium superoxide as a result of the addition of the aqueous potassium hydroxide solution is thus prevented. Foaming during the reaction for generating oxygen is also prevented by the bed.

Ninth Exemplary Embodiment

[0104] 10 g in each case of potassium superoxide were initially charged, as powder or pressed in the form of tablets having a fracture resistance of either 60 N, 80 N or 110 N, into four cylindrical reaction vessels having an internal diameter of 28 mm.

[0105] Here and hereinafter, the fracture resistance denotes the mechanical strength of a pressed tablet with respect to a diametrically acting force at the time of fracture (European Pharmacopoeia. 8th ed. 2014; 2.9.8). The fracture resistance of the tablet is determined as the radial fracture resistance or compressive strength of the tablet by crushing the tablet between two jaws.

[0106] 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The potassium superoxide powder was stirred during the addition of the aqueous 9 M potassium hydroxide solution and during the whole reaction time in order to avoid sticking of the surface as a result of reaction products. The reactions were terminated after 10 minutes. The results are presented in FIGS. 16 and 17 and in Table 6.

TABLE-US-00006 TABLE 6 Flow Reaction O.sub.2 O.sub.2 Source (fracture rate.sub.max temperature volume volume resistance) [L/h] [° C.] [L] [%] Powder 456 46 2.2 85 Tablets (60N) 297 48 2.5 96 Tablets (80N) 182 48 2.5 96 Tablets (110N) 189 48 2.5 96

[0107] It is apparent from this that, for the reaction with pulverulent potassium superoxide, a maximum yield in gas volume of 2.2 L is reached. For the reactions of potassium superoxide in tablet form, a maximum yield in gas volume of 2.5 L is reached. With pulverulent potassium superoxide, a maximum oxygen flow rate of 456 L/h is reached. With potassium superoxide pressed into tablets, a maximum oxygen flow rate of 297 L/h is reached with a fracture resistance of 60 N, a maximum oxygen flow rate of 182 L/h is reached with a fracture resistance of 80 N and a maximum oxygen flow rate of 189 L/h is reached with a fracture resistance of 110 N. The fracture resistance of the tablet has an influence on the maximum oxygen flow rate during the reaction for generating oxygen. In this case, a higher fracture resistance of the tablet results in a lower maximum oxygen flow rate.

Tenth Exemplary Embodiment

[0108] 5 g in each case of potassium superoxide were pressed, either with 5 g of potassium hydroxide or with 5 g of sodium dihydrogenphosphate, into tablets having a fracture resistance of 60 N (mass ratio 1:1 in each case). 10 g of these tablets were initially charged in each case into two cylindrical reaction vessels having an internal diameter of 28 mm. 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 15 minutes. The results are presented in FIGS. 18 and 19 and in Table 7.

TABLE-US-00007 TABLE 7 Flow Reaction O.sub.2 O.sub.2 Tablet contents rate.sub.max temperature volume volume (mass ratio) [L/h] [° C.] [L] [%] KO.sub.2, KOH (1:1) 297 44 1.2 96 KO.sub.2, NaH.sub.2PO.sub.4 205 55 1.2 96 (1:1)

[0109] It is apparent from this that, for both reactions, a maximum yield in gas volume of 1.2 L is reached. For tablets consisting of potassium superoxide and potassium hydroxide in a mass ratio of 1:1, a maximum oxygen flow rate of 297 L/h and a maximum reaction temperature of 44° C. are reached. For tablets consisting of potassium superoxide and sodium dihydrogenphosphate in a mass ratio of 1:1, a maximum oxygen flow rate of 297 L/h and a maximum reaction temperature of 55° C. are reached.

Eleventh Exemplary Embodiment

[0110] 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. The reactions were terminated after 40 minutes. The results are presented in FIGS. 20 and 21 and in Table 8.

TABLE-US-00008 TABLE 8 After 10 minutes of reaction time Flow Reaction O.sub.2 O.sub.2 rate.sub.max temperature volume 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

[0111] 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. 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 potassium superoxide in the paste.

Twelfth Exemplary Embodiment

[0112] 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 out of the reaction vessel through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rate and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 225 minutes. The results are presented in FIGS. 22 and 23 and in Table 9.

TABLE-US-00009 TABLE 9 Flow Reaction O.sub.2 O.sub.2 Reaction rate.sub.max temperature volume volume duration [L/h] [° C.] [L] [%] [min] 104 27 1.11 94 219

[0113] It is apparent from this that, in the case of potassium superoxide and [BMPL][BF(CN).sub.3], pressed into tablets, a 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.

Thirteenth Exemplary Embodiment

[0114] 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.

Fourteenth Exemplary Embodiment

[0115] 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 75 minutes since in all reactions the maximum achievable oxygen yield had been reached. The results are presented in FIGS. 24 and 25 and in Table 10.

TABLE-US-00010 TABLE 10 After 10 minutes of reaction time Flow O.sub.2 O.sub.2 rate.sub.max volume volume Ionic liquid [L/h] [mL] [%] [BMPL]Cl 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

[0116] 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 0.25 L. 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.

Fifteenth Exemplary Embodiment

[0117] Pulverulent potassium superoxide and the phyllosilicate mica were intimately mixed in a mass ratio of 10:1 and pressed using a briquetting press into tablets having a mass of 200 mg, a diameter of 6 mm and a fracture resistance of 5 kN.

[0118] Next, for one tablet, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 0.4 mL of a 9 M potassium hydroxide solution. Complete conversion of the potassium superoxide to oxygen, with floating of the tablets, was observed within a reaction time of 2 minutes.

Sixteenth Exemplary Embodiment

[0119] Pulverulent potassium superoxide and the fumed silica Aerosil 200 were intimately mixed in a mass ratio of 10:1 and pressed using a briquetting press into tablets having a mass of 200 mg, a diameter of 6 mm and a fracture resistance of 5 kN.

[0120] Next, for one tablet, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 0.4 mL of a 9 M potassium hydroxide solution. Complete conversion of the potassium superoxide to oxygen, without floating of the tablets, was observed within a reaction time of 2 minutes.

Seventeenth Exemplary Embodiment

[0121] Pulverulent potassium superoxide and the antifoam paraffin were intimately mixed in a mass ratio of 5:1 and pressed using a briquetting press into tablets having a mass of 200 mg, a diameter of 6 mm and a fracture resistance of 5 kN.

[0122] Next, for one tablet, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 0.4 mL of a 9 M potassium hydroxide solution. Complete conversion of the potassium superoxide to oxygen, without floating of the tablets, was observed within a reaction time of 5 minutes.

Eighteenth Exemplary Embodiment

[0123] Pulverulent potassium superoxide and the antifoam silicone oil were intimately mixed in a mass ratio of 2:1 and pressed using a briquetting press into tablets having a mass of 200 mg, a diameter of 6 mm and a fracture resistance of 5 kN.

[0124] Next, for one tablet, at an ambient temperature of room temperature, the reaction for generating oxygen was initiated by adding 0.4 mL of a 9 M potassium hydroxide solution. Complete conversion of the potassium superoxide to oxygen, without floating of the tablets, was observed within a reaction time of 30 minutes.

Nineteenth Exemplary Embodiment

[0125] 10 g in each case of potassium superoxide were pressed in the form of tablets having a fracture resistance of 60 N and initially charged into three cylindrical reaction vessels having an internal diameter of 28 mm. At an ambient temperature of +70° C., room temperature or −40° C., the reaction for generating oxygen was initiated by adding 20 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 70 minutes since the maximum achievable oxygen volume had been reached at every ambient temperature. The results are presented in FIGS. 26 and 27 and in Table 11.

TABLE-US-00011 TABLE 11 Starting Flow Reaction O.sub.2 O.sub.2 Reaction temperature rate.sub.max temperature volume volume duration [° C.] [L/h] [° C.] [L] [%] [min] −40  68 14 2.4 97 62 RT 351 48 2.4 97  7 +70 582 80 2.4 97  3

[0126] It is apparent from this that, at an ambient temperature of +70° C., the maximum yield in gas volume of 2.4 L is reached after 3 minutes of reaction time. At an ambient temperature of room temperature, the maximum yield in gas volume of 2.4 L is reached after 7 minutes of reaction time. At an ambient temperature of −40° C., the maximum yield in gas volume of 2.4 L is reached after 62 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.

Twentieth Exemplary Embodiment

[0127] 10 g in each case of potassium superoxide were pressed in the form of tablets having a fracture resistance of 60 N and initially charged into three cylindrical reaction vessels having an internal diameter of 28 mm. At an ambient temperature of +70° C., room temperature or −20° C., the reaction for generating oxygen was initiated by adding 20 mL in each case of a 50% aqueous ethylene glycol mixture 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 70 minutes since the maximum achievable oxygen volume had been reached at every ambient temperature. 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 19. Here too, at an ambient temperature of −20° C. the oxygen is released more continuously and uniformly.

Twenty-First Exemplary Embodiment

[0128] 10 g in each case of potassium superoxide were pressed in the form of tablets having a fracture resistance of 60 N and initially charged into three cylindrical reaction vessels having an internal diameter of 28 mm. At an ambient temperature of +70° C., room temperature or −20° C., the reaction for generating oxygen was initiated by adding 20 mL in each case of a 40% aqueous propylene glycol mixture 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 out of the reaction vessels through a drum-type gas meter to measure the volume of the oxygen generated. The oxygen flow rates and the length of the reaction time were additionally measured. Recording of the measurement data was halted after 70 minutes since the maximum achievable oxygen volume had been reached at every ambient temperature. 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 19. Here too, at an ambient temperature of −20° C. the oxygen is released more continuously and uniformly.