WO2009006521A2 - Compositions et procédés de chauffage chimique - Google Patents

Compositions et procédés de chauffage chimique Download PDF

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Publication number
WO2009006521A2
WO2009006521A2 PCT/US2008/069014 US2008069014W WO2009006521A2 WO 2009006521 A2 WO2009006521 A2 WO 2009006521A2 US 2008069014 W US2008069014 W US 2008069014W WO 2009006521 A2 WO2009006521 A2 WO 2009006521A2
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WO
WIPO (PCT)
Prior art keywords
heater
water
copper
compartment
halide
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PCT/US2008/069014
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English (en)
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WO2009006521A3 (fr
Inventor
Michael Sheppard Bolmer
Cullen M. Sabin
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Tempra Technology, Inc.
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
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Publication date
Application filed by Tempra Technology, Inc. filed Critical Tempra Technology, Inc.
Priority to EP08781270A priority Critical patent/EP2179229A2/fr
Priority to JP2010515253A priority patent/JP2010532463A/ja
Publication of WO2009006521A2 publication Critical patent/WO2009006521A2/fr
Publication of WO2009006521A3 publication Critical patent/WO2009006521A3/fr

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Classifications

    • F—MECHANICAL ENGINEERING; LIGHTING; HEATING; WEAPONS; BLASTING
    • F24—HEATING; RANGES; VENTILATING
    • F24V—COLLECTION, PRODUCTION OR USE OF HEAT NOT OTHERWISE PROVIDED FOR
    • F24V30/00—Apparatus or devices using heat produced by exothermal chemical reactions other than combustion

Definitions

  • This invention relates to heating compositions for user-activatable, single-use chemical heaters and heating methods employing such compositions.
  • a heater may comprise, for example, a self-heating cup or container for beverages, such as disclosed in published international patent application WO 2005/115872, published international patent application WO 03/096855, United States patent 6,481,214, and United States patent 3,874,557.
  • a heater may be tray-like for heating food, such as disclosed in United States patent 4,809,673.
  • a heater may be in the form of a flexible heat pack adapted to heat body parts or objects, including pouched food such as military meals commonly referred to as meals ready to eat (MRE's), such as shown in United States patent 6,640,801.
  • MRE's meals ready to eat
  • User-activated heating systems for single-use chemical heaters include calcium oxide systems, in which calcium oxide is mixed with, and reacts with, water to generate heat, as described in United States patent 5,809,786; permanganate heating systems, in which an alkali metal permanganate oxidizer is mixed with, and reacts with, a fuel such as glycerol (in aqueous form) to generate heat, as described in United States patents 5,035,230 and 5,984,953.
  • Heating systems described in the literature also include systems in which a powdered active metal such as zinc or magnesium, is mixed with, and reacts with, water to generate heat, as described in international patent application WO 97/06391, and systems in which a combination of powdered copper sulfate, zinc, and magnesium is mixed with, and reacts with, water to generate heat, as disclosed in Russian patent RU 2 271 972.
  • a powdered active metal such as zinc or magnesium
  • This invention includes single-use chemical heaters that include water-activated heating systems that utilize the oxidation-reduction reaction between aluminum metal (Al) and a water- soluble halide salt of copper, either anhydrous or hydrated, such as copper chloride, preferably copper chloride hydrate, CuCl 2 ⁇ H 2 O.
  • the copper halide salt may be included as a starting material, alone or in combination with other copper salts, such as sulfate (CuSO 4 -5H 2 O), that are converted to copper halide during the heating reaction with aluminum metal and water.
  • the soluble copper halide can be generated in the reaction mixture by the reaction between such a nonhalide copper salt, for example copper sulfate, and a non-copper water- soluble halide salt, that reacts with the nonhalide copper salt in water to produce the copper halide, for example copper chloride, that then reacts with aluminum metal in water to generate heat.
  • a non-copper, water- soluble halide salt that is capable of reacting with such a nonhalide copper salt in water to produce a copper halide as a "halide salt catalyst," or, for short, simply as "catalyst".
  • Halide salt catalysts are water-soluble halides.
  • halide salt catalysts include non-copper metal halide, preferably alkali metal halides and alkaline earth metal halides such as sodium chloride (NaCl), potassium chloride (KCl), sodium bromide (NaBr), potassium bromide (KBr), calcium chloride (CaCl 2 ), magnesium chloride (MgCl 2 ), calcium bromide (CaBr 2 ) and magnesium bromide (MgBr 2 ).
  • Hydrogen chloride (HCl) is also a suitable catalyst.
  • Halide salt catalysts also include mixtures of two or more of such halide salts.
  • a nonhalide copper salt such as copper sulfate
  • aluminum metal in water produces no heat. Adding even a small amount of either copper halide salt or halide salt catalyst, or both, to this mixture produces approximately as much heat as if all the copper salt were copper halide. This suggests that the halide ions are catalysts for the reaction of copper ions and aluminum metal.
  • the relative amount of copper halide or catalyst to nonhalide copper salt can be varied to modify the rate of heat generation.
  • a water-soluble acetate salt such as sodium acetate, for example as sodium acetate trihydrate (NaC 2 H 3 O 2 -3H 2 O)
  • sodium acetate trihydrate NaC 2 H 3 O 2 -3H 2 O
  • the form of aluminum metal can be varied to modify its surface area and overall structure so as to modify the rate and completeness of the heat- generating reaction.
  • Suitable nonhalide copper salts for use with copper halide can be tested routinely by substituting them for copper sulfate in the heating composition of Example 3 below.
  • suitable nonhalide copper salts for use with catalyst can be tested routinely by substituting them for copper sulfate in the heating composition of Example 5.
  • Suitability of a particular nonhalide copper salt will be evident from the temperature rise resulting from the heating composition.
  • suitable nonhalide copper salts are those that react with halide salts in water to produce copper halide. The following are expected to be suitable nonhalide copper salts: copper acetate Cu(C 2 H 3 O 2 ) 2 , copper formate Cu(CHO 2 ) 2 and copper lactate Cu(C 3 H 5 O 3 ) 2 .
  • One copper salt that cannot be included in systems of this invention as a nonhalide copper salt reactant in heaters that include either copper halide or catalyst is copper nitrate Cu(NO 3 ) 2 .
  • This and other nitrate salts have been found to be poisons of halide salt catalysts. They can be used to stop the reaction according to the methods described in international patent application WO 2005/108878 A2.
  • Such nitrate compounds can be included in heaters of this invention if normally sequestered but releasable into the catalyst-containing reaction to suppress or terminate the heat-generating reaction, if the temperature rises to a predetermined maximum level.
  • User-activated, single-use chemical heaters include the above- described heating systems.
  • Such heaters include at least one compartment of a first type containing a portion of the heating-system reactants and at least one compartment of a second type containing the remaining heating-system reactants, plus a separator therebetween, such as, for example, a valve or frangible seal or rupturable inner compartment holding liquid reactants, that a user can operate or cause to operate so as to compromise the separation of the two compartment types, otherwise sealed from one another, and allow their contents to mix, thereby initiating the heat-generating reaction.
  • the heater may also include a separate compartment for a product to be heated, for example, a beverage or military meal.
  • Heaters according to this invention may also include a reaction suppressor or killer either in a compartment that can be automatically compromised to release its contents into the reaction or otherwise sequestered in a releasable form, for example, a wax applied to the product compartment.
  • the aluminum and copper halide can be stored as dry reaction ingredients in one compartment, and water can be stored in another compartment.
  • the copper halide can be dissolved in, and stored with, the water. It is less preferred to split the water between the two types of compartments, that is, to store aluminum plus a portion of the water in one compartment and to store the copper halide dissolved in the remaining portion of the water in another compartment.
  • the reactants are aluminum metal, copper sulfate, and copper halide
  • a portion of the water could be included with the metal and sulfate, because the metal and sulfate do not react in the presence of water, but we prefer to place all the water in the other compartment type.
  • the reactants are aluminum metal, copper sulfate, and halide salt catalyst
  • a portion of the water could be included with the metal and sulfate, but we prefer to keep them as dry ingredients.
  • the system includes sodium acetate or another catalyst activator, we prefer to store the activator with the halide salt catalyst in the compartment also containing the water.
  • FIG. 1 is a chart showing temperature as a function of time for the heating composition described in Example 1.
  • FIG. 2 is a chart showing temperature as a function of time for the heating composition described in Example 2.
  • FIG. 3 is a chart showing temperature as a function of time for the heating composition described in Example 3.
  • FIG. 4 is a chart showing temperature as a function of time for the heating composition described in Example 4.
  • FIG. 5 is a chart showing temperature as a function of time for the heating composition described in Example 5.
  • FIG. 6 is a chart showing temperature as a function of time for the heating composition described in Example 6.
  • FIG. 7 is a chart showing temperature as a function of time for the heating composition described in Example 7.
  • FIG. 8 is a chart showing temperature as a function of time for the heating composition described in Example 8.
  • FIG. 9 is a chart showing temperature as a function of time for the heating composition described in Example 9.
  • FIG. 10 is a chart showing temperature as a function of time for the heating composition described in Example 10.
  • FIG. 11 is a chart showing temperature as a function of time for the heating composition described in Example 11.
  • FIG. 12 is a chart showing temperature as a function of time for the heating composition described in Example 12.
  • FIG. 13 is a chart showing temperature as a function of time for the heating composition described in Example 13.
  • FIG. 14 is a chart showing temperature as a function of time for the heating composition described in Example 14.
  • FIG. 15 is a chart showing temperature as a function of time for the heating composition described in Example 15.
  • FIG. 16 is a chart showing temperature as a function of time for the heating composition described in Example 16.
  • FIG. 17 is a simplified, block diagrammatic view of a heater according to this invention.
  • Heater 1 includes compartment 2, a reactant compartment of a first type (only one shown for ease of understanding) and compartment 3, a reactant compartment of a second type (only one shown for ease of understanding).
  • Compartments 2, 3 are generally sealed from one another but their separation includes a user-operable separator, here shown as valve 4.
  • valve 4 To activate the heat-generating reaction, a user operates the separator, here by opening valve 4, which allows mixing of the contents of compartments 2, 3 and the initiation of the heat-generating reaction in one or both compartment types.
  • compartment 2 is shown disposed within compartment 3, but it will be appreciated that it may be outside compartment 3 and separated therefrom by, for example, a frangible seal.
  • compartment 2 is disposed within compartment 3, as shown, we prefer that water be included in compartment 2 so that the contents of compartment 2 flow into compartment 3, which contains dry reactants. Compartment 3 thereupon becomes the reaction compartment.
  • Heater 1 also includes compartment 5, a compartment for a material to be heated. Compartment 5 as shown is disposed largely within compartment 3, such that steam generated in compartment 3 can condense on much of the surface of the wall separating compartment 5 from compartment 3. It will be appreciated that compartment 5 can be thermally connected to compartment 3 otherwise, for example, by being disposed adjacent thereto, separated by a heat- conducting wall, hi embodiments that do not include and are not intended to accommodate a product to be heated, such as a heat pack, compartment 5 will not be included.
  • Heater 1 further includes a sequestered but releasable reaction suppressor or terminator, such as a nitrate catalyst poison, here shown as was ring 6 applied to the outer surface of compartment 5 but releasable into compartment 3 upon melting of the wax when a predetermined temperature is reached at the wall separating compartment 5 from compartment 3.
  • Wax ring 6 contains a suppressor or reaction-killing composition. It will be appreciated that a reaction suppressor or killer could be included in a closed compartment having a release mechanism that activates automatically when a predetermined temperature is reached. It will also be appreciated that a reaction suppressor or killer will not be included in all embodiments.
  • Methods according to this invention comprise the use of a heater according to this invention.
  • a user compromises the separation of reactant compartments of the first and second type, thereby initiating the heat-generating chemical reaction.
  • Methods according to this invention may also include supplying the heater, supplying the product or object to be heated, or both.
  • Heating compositions of this invention utilize the oxidation-reduction reaction in water of aluminum metal (Al) with a copper halide salt, preferably copper chloride (CuCl 2 ).
  • Aluminum is used in a form that provides a high surface area relative to a block of aluminum. We have utilized three such forms: aluminum flakes, aluminum strips, and aluminum wool.
  • the aluminum flakes were aluminum foil 0.05 mm thick chopped into flakes 1 mm square.
  • the aluminum strips were aluminum foil 0.025 mm thick cut into strips about 6 mm wide and about 170 mm long.
  • the aluminum wool was made from aluminum wire 0.04 mm in diameter.
  • Substitution of Al wool for Al flakes increased the surface area available for reaction and also increased the openness of the Al structure for better circulation of the water and soluble reactants, which promotes completeness of the heat-generating reaction.
  • the surface area of the flakes was 40 mmW.
  • the surface area of the wool was 100 mmW.
  • Comparison of Examples 7 and 8 shows that substitution of Al wool (Ex. 8) for Al flakes (Ex 7) increased both the rate and completeness of the reaction.
  • the thinner 0.025 mm aluminum strips (80 mmW) were only used in Example 16. The strips did not pack as tightly as the flakes, and therefore performed more like the wool.
  • Heat-generating reactions of systems according to this invention can be illustrated by a series of equations.
  • copper halide is represented by copper chloride
  • nonhalide copper salt is represented by copper sulfate
  • halide salt catalyst is represented by sodium chloride. Water of hydration is omitted from the equations for the sake of clarity. Persons skilled in the art will understand how to write the equations utilizing alternative ingredients.
  • the oxidation-reduction reactions of this invention utilize a water- soluble copper halide, preferably copper chloride.
  • Copper halide may be included as a starting ingredient, for example in the form of copper chloride hydrate (CuCl 2 -2H 2 O).
  • the reaction is represented by Reaction 1, which is exothermic (water of hydration is omitted from reactions reported below for the sake of clarity, as indicated above):
  • Reaction 2 may also occur to clear any oxide layer off the surface of the aluminum:
  • the copper halide can be the sole source of copper for the reaction.
  • Such a mixture is believed to utilize Reaction 1 , in combination with Reaction 3:
  • copper halide can be generated in the reaction by its reaction in water with a soluble halide salt catalyst, preferably an alkali or alkaline earth metal halide, by means of Reaction 4:
  • halide salt catalyst as a catalyst because it is not consumed in the heat- generating reaction between copper and aluminum, but rather it reacts with the nonhalide copper salt to create a copper halide and is then regenerated.
  • sodium acetate for example as sodium acetate trihydrate (NaC 2 H 3 O 2 -3H 2 O)
  • soluble halide salt such as NaCl
  • a mixture of 17.11 g CuSO 4 SH 2 O and 1.30 g CuCl 2 -2H 2 O and 1.34 g aluminum flakes were placed into 200 ml of water in an insulated flask.
  • the temperature as shown in FIG. 3, heated from 23.4 0 C to 51.9°C.
  • the initial rate of heating was about 1 l°C/minute.
  • This example shows that a combination of copper halide and copper sulfate can be used to generate copper halide in the reaction, and that the copper halide in the combination can be a minor amount relative to the copper sulfate, in this case representing 10 wt. percent of the copper sulfate, and still generate as much heat as if all the Cu salt were CuCl 2 .
  • Substitution of copper nitrate, Cu(NO 3 ) 2 for copper sulfate in a heating composition of this type failed to generate heat.
  • a mixture of 64.42 g CuSO 4 -5H 2 O and 5.57 g aluminum flakes were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 50 ml water was added into the reaction chamber under the steel cup.
  • the temperature of the water in the steel cup remained unchanged at 17 0 C for 8 minutes, showing the nonreactivity of the CuSO 4 -5H 2 O and aluminum flakes.
  • 10 ml water with 0.45g of CuCl 2 -2H 2 O dissolved in it was added to the reaction mixture.
  • a mixture of 57.35 g CuSO 4 -5H 2 O and 0.27 g NaCl and 5.43 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup as an object to be heated.
  • 50 ml water was added into the reaction chamber under the steel cup to activate the reaction. As shown in FIG. 5, the temperature of the water in the steel cup heated from 2O 0 C to 75 0 C.
  • a mixture of 57.35 g CuSO 4 -5H 2 O and 5.43 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup as a liquid to be heated.
  • 50 ml water containing 0.14 g NaCl were added into the reaction chamber under the steel cup to activate the reaction.
  • the temperature of the water in the steel cup heated from 21 0 C to 78°C.
  • the system can include one compartment of dry ingredients (here aluminum and copper sulfate) and one compartment containing water and water-soluble salt, either sodium chloride (as shown) or copper halide (not shown).
  • a mixture of 52.58 g CuSO 4 SH 2 O and 3.99 g CuCl 2 -2H 2 O and 4.21 g aluminum flakes were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups. 265 ml water was placed in the steel cup. 50 ml water was added into the reaction chamber under the steel cup.
  • the temperature of the water in the steel cup heated from 15°C to 49°C. After the heating stopped, the reactants were stirred, and the reaction started again, releasing steam.
  • This example illustrates the use of aluminum flakes and provides a base for comparing the use of aluminum wool in Example 8.
  • a mixture of 52.58 g CuSO 4 -5H 2 O and 3.99 g CuCl 2 -2H 2 O and 4.21 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups. 265 ml water was placed in the steel cup. 50 ml water was added into the reaction chamber under the steel cup. As shown in FIG. 8, the temperature of the water in the steel cup heated from 20 0 C to 64°C. After the heating stopped, the reactants were stirred, and the reaction did not start again.
  • Example 7 Comparing Example 7 with this example, one sees that use of aluminum wool in place of aluminum flakes increased the temperature rise of the water in the steel cup from 34 0 C to 44 0 C and resulted in a complete reaction that did not restart upon subsequent stirring.
  • Aluminum wool thus has advantages over aluminum flakes.
  • the heater can readily be designed such that if the heater is turned upside down, dumping a liquid being heated, the aqueous reaction liquid will drain away from the solid aluminum, stopping the reaction and preventing the temperature from rising excessively due to loss of the heat sink provided by the product being heated.
  • a mixture of 54.00 g CuSO 4 -SH 2 O and 5.55 g aluminum flakes were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 60 ml water containing 0.26 g KBr was added into the reaction chamber under the steel cup.
  • the water in the steel cup heated from 22°C to 57°C in 14.2 minutes. This example shows that chloride is not the only halide ion effective for this invention.
  • a mixture of 54.00 g CuSO 4 -5H 2 O and 5.45 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 50 ml water containing 0.13 g NaCl were added into the reaction chamber under the steel cup.
  • the temperature of the water in the steel cup heated from 2O 0 C to 58 0 C in 4.1 minutes.
  • the temperature of the water in the steel cup heated from 20 0 C to 72 0 C overall.
  • This example illustrates the use of sodium chloride and provides a base case to compare to the further addition of sodium acetate in Example 11.
  • a mixture of 54.00 g CuSO 4 -5H 2 O and 5.46 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 50 ml water containing 0.13 g NaCl and 0.27 g NaC 2 H 3 O 2 -SH 2 O were added into the reaction chamber under the steel cup.
  • the temperature of the water in the steel cup heated from 20 0 C to 58°C in 3.1 minutes.
  • the temperature of the water in the steel cup heated from 20 0 C to 74°C overall.
  • Example 10 illustrates the use of a catalyst activator.
  • a catalyst activator here sodium acetate
  • addition of a catalyst activator, here sodium acetate increased the initial reaction rate to 12 °C/min from 9 0 C /min, and increased the amount of heat transferred to the inner cup to 265 cal/g of CuSO 4 -5H 2 O from 255 cal/g.
  • a mixture of 55.00 g CuSO 4 -5H 2 O and 5.55 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 50 ml water containing 0.30 g NaC 2 H 3 O 2 -3H 2 O were added into the reaction chamber under the steel cup.
  • temperature of the water in the steel cup started at 19.5°C and after 15 minutes it was still at 19.5°C. There was no reaction.
  • This example shows that sodium acetate does not itself act as a catalyst.
  • a mixture of 53.00 g CuSO 4 -5H 2 O and 5.35 g aluminum wool were placed into a 500 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups.
  • 265 ml water was placed in the steel cup.
  • 50 ml water containing 0.12 g CaCl 2 were added into the reaction chamber under the steel cup.
  • the temperature of the water in the steel cup heated from 20 0 C to 58 0 C in 2.8 minutes.
  • the temperature of the water in the steel cup heated from 2O 0 C to 73 0 C overall. This shows that CaCl 2 can be used as a catalyst.
  • a mixture of 17.11 g CuSO 4 -5H 2 O and 1.30 g CuCl 2 -2H 2 O and 1.34 g aluminum flakes were placed into 200 ml of water in an insulated flask. As shown in FIG. 14, the temperature heated from 22 0 C to 35°C, and then 8.00 g Cu(NO 3 ) 2 -2.5H 2 O were added. The dip in the temperature profile in FIG. 14 shows where the thermocouple was removed from the mixture to make room to add the Cu(NO 3 ) 2 -2.5H 2 O. The mixture heated to a maximum temperature of 37°C. The starting mixture is the same as in Example 3, but the total temperature rise was only 15°C, compared to 28.5°C in Example 3. The Cu(NO 3 ) 2 -2.5H 2 O stopped the reaction in the 4-5 seconds that it took to add the powder and mix it into the reaction mixture.
  • a mixture of 56.00 g CuSO 4 -SH 2 O and 5.60 g aluminum wool were placed into a 510 ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 210 ml in the annular space between the two cups.
  • a mixture comprising 9 g Mg(NO 3 ) 2 -6H 2 O and 13 g paraffin wax was applied to the outside of the steel cup.
  • 265 ml water was placed in the steel cup.
  • 60 ml water containing 0.15 g NaCl and 0.35 g NaC 2 H 3 O 2 -SH 2 O were added into the reaction chamber under the steel cup. As shown in FIG.
  • a mixture of 30.00g CuSO 4 -5H 2 0, 12.0Og KMnO 4 , and 4.0Og shredded aluminum foil was placed into a 500ml plastic cup.
  • a 300 ml steel cup was nested into the plastic cup, forming a reaction chamber of about 200 ml in the annular space between the two cups. 275 ml water was placed in the steel cup.
  • 60 ml aqueous solution containing 4.5ml glycerol, 0.2Og HCl, and 0.06ml Surfynol SE-F surfactant from Air Products were added into the reaction chamber under the steel cup. As shown in FIG. 16, the temperature of the water in the steel cup heated from 20 0 C to 58 0 C in 2.8 minutes.
  • the temperature of the water in the steel cup heated from 20 0 C to 72°C overall.
  • This example illustrates: (1) the use of shredded aluminum foil; (2) the use of hydrogen chloride (HCl) as the non-copper water-soluble halide salt; (3) the use of a surfactant in the reactant; and (4) the addition of KMnO 4 and glycerol to the reaction mixture to reduce the overall amount of solid chemicals, compared to Examples 10, 11, and 13, which required about 25% more solids to produce similar heating results. It is believed that the surfactant helped the solution wet the aluminum.
  • HCl hydrogen chloride
  • a mixture of 53.0Og CuSO 4 SH 2 O, and 5.3Og shredded aluminum foil was placed into a 1000ml graduated cylinder.
  • a 55 ml aqueous solution containing 0.18g HCl was added into the graduated cylinder.
  • the reaction mixture produced steam, and foam rose up to 350 ml in the cylinder.
  • the reaction was repeated with 0.01 ml/ml Dow-Corning FG-IO antifoam emulsion added to the solution.
  • the maximum volume of foam was 310 ml.
  • the reaction was repeated with 0.01 ml/ml Air Products Surfynol 504 surfactant.
  • the maximum volume of foam was 250 ml.
  • the reaction was repeated with 0.005 ml/ml Air Products SE-F surfactant.
  • the maximum volume of foam was 220 ml.
  • the heater could include a variety of possible physical configurations.
  • the specific amounts of each ingredient in a heater can differ depending on the specific heating requirements of each application.
  • materials used to manufacture a heater can vary depending on the requirements of a specific application. Accordingly, other embodiments are within the scope of the following claims.

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Abstract

L'invention concerne un élément chauffant chimique à usage unique pouvant être activé par l'utilisateur, qui comprend au moins un compartiment d'un premier type, séparé d'au moins un compartiment d'un deuxième type par un séparateur, lequel peut être retiré par l'utilisateur pour établir une communication entre les compartiments. De l'eau et les ingrédients d'un système de chauffe produisant de la chaleur par une réaction d'oxydation-réduction entre de l'aluminium métallique et un halogénure de cuivre soluble dans l'eau sont stockés dans les compartiments séparés des premier et deuxième type, de sorte que la réaction de production de chaleur ne s'amorce qu'au moment où le contenu desdits compartiments se mélange, après le retrait dudit séparateur.
PCT/US2008/069014 2007-07-03 2008-07-02 Compositions et procédés de chauffage chimique WO2009006521A2 (fr)

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EP08781270A EP2179229A2 (fr) 2007-07-03 2008-07-02 Compositions et procédés de chauffage chimique
JP2010515253A JP2010532463A (ja) 2007-07-03 2008-07-02 化学的加熱組成物および方法

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US8183196B2 (en) 2010-04-23 2012-05-22 The Procter & Gamble Company Detergent composition
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US10036574B2 (en) 2013-06-28 2018-07-31 British American Tobacco (Investments) Limited Devices comprising a heat source material and activation chambers for the same
US10542777B2 (en) 2014-06-27 2020-01-28 British American Tobacco (Investments) Limited Apparatus for heating or cooling a material contained therein
US11064725B2 (en) 2015-08-31 2021-07-20 British American Tobacco (Investments) Limited Material for use with apparatus for heating smokable material
US11241042B2 (en) 2012-09-25 2022-02-08 Nicoventures Trading Limited Heating smokeable material
US11452313B2 (en) 2015-10-30 2022-09-27 Nicoventures Trading Limited Apparatus for heating smokable material
US11659863B2 (en) 2015-08-31 2023-05-30 Nicoventures Trading Limited Article for use with apparatus for heating smokable material
US11672279B2 (en) 2011-09-06 2023-06-13 Nicoventures Trading Limited Heating smokeable material
RU2804552C1 (ru) * 2023-04-18 2023-10-02 Федеральное государственное бюджетное образовательное учреждение высшего образования "Национальный исследовательский Мордовский государственный университет им. Н.П. Огарёва" Неорганическая композиция для использования в беспламенных нагревателях пищи
US11825870B2 (en) 2015-10-30 2023-11-28 Nicoventures Trading Limited Article for use with apparatus for heating smokable material
US11924930B2 (en) 2015-08-31 2024-03-05 Nicoventures Trading Limited Article for use with apparatus for heating smokable material

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WO2010141080A1 (fr) * 2009-06-02 2010-12-09 Deepak Madan Rechauffeurs sans flamme reglables
US8635998B2 (en) 2009-06-02 2014-01-28 Read Manufacturing Company Tunable flameless heaters
US8183196B2 (en) 2010-04-23 2012-05-22 The Procter & Gamble Company Detergent composition
US8357650B2 (en) 2010-04-23 2013-01-22 The Procter & Gamble Company Aminocarboxylic builder particle
US8455422B2 (en) 2010-04-23 2013-06-04 The Procter & Gamble Company Process for making a methyl glycine diacetic acid particle
CN102051612A (zh) * 2010-12-02 2011-05-11 西北工业大学 一种制备轻金属表面超疏水润滑涂层的方法
US11672279B2 (en) 2011-09-06 2023-06-13 Nicoventures Trading Limited Heating smokeable material
US11241042B2 (en) 2012-09-25 2022-02-08 Nicoventures Trading Limited Heating smokeable material
US10036574B2 (en) 2013-06-28 2018-07-31 British American Tobacco (Investments) Limited Devices comprising a heat source material and activation chambers for the same
US10542777B2 (en) 2014-06-27 2020-01-28 British American Tobacco (Investments) Limited Apparatus for heating or cooling a material contained therein
US11064725B2 (en) 2015-08-31 2021-07-20 British American Tobacco (Investments) Limited Material for use with apparatus for heating smokable material
US11659863B2 (en) 2015-08-31 2023-05-30 Nicoventures Trading Limited Article for use with apparatus for heating smokable material
US11924930B2 (en) 2015-08-31 2024-03-05 Nicoventures Trading Limited Article for use with apparatus for heating smokable material
US11452313B2 (en) 2015-10-30 2022-09-27 Nicoventures Trading Limited Apparatus for heating smokable material
US11825870B2 (en) 2015-10-30 2023-11-28 Nicoventures Trading Limited Article for use with apparatus for heating smokable material
RU2804552C1 (ru) * 2023-04-18 2023-10-02 Федеральное государственное бюджетное образовательное учреждение высшего образования "Национальный исследовательский Мордовский государственный университет им. Н.П. Огарёва" Неорганическая композиция для использования в беспламенных нагревателях пищи

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