CREATING HEAT ENERGY WITHOUT COMBUSTION and ELECTRICITY: Sustainability & Climate Tech

 

 

Energy is needed for human activities, especially for activities economy, household, industry, business and transportation. Part The world's large energy supply comes from fossil fuels is a non-renewable resource. Estimated energy requirements continues to increase, while sources of oil and coal reserves the numbers are dwindling. Apart from that, the use of fossil fuels as energy that contributes to excess carbon in the atmosphere thus causing global warming (Jukic & Jerkovic, 2008). Therefore, there is a need for alternative energy supplies other than oil earth and coal. New Renewable Energy (RE) is one of them Alternative sources provide energy, because in addition to having an impact low environmental damage, also guarantees satisfaction energy into the future. 

 

On the other hand, almost every day, in our surrounding environment  we find piles of rubbish, both organic or non-organic. One type of non-organic waste that we often encounter is aluminum foil waste which comes from the remains of packaging wrappers.

 

Meanwhile, on Lombok Island, one of the community business sectors is the center Pottery crafts in Penujak Village, West Praya District Central Lombok Regency, West Nusa Tenggara, lihat web: https://maps.app.goo.gl/RmDXMb55tUoJtkB87 This area is in the surrounding area Lombok International Airport (see map below). Since the beginning In its existence, this craft utilizes biomass from wood and straw as fuel in their production process. The use of firewood and straw as fuel leaves wood ash which has an environmen impact

Conclusion

-          Heavy metal waste in the form of aluminum foil which has an environmental impact

-          On Lombok Island, there is one of the NTB Pottery Craft CentersThis village is located around the Lombok International Airport (BIL) area. Passed by the Bypass road which connects Mataram City with the Mandalika Circuit

-          Burning pottery leaves wood ash which has an impact on the environment

 

 

 

II. The Proposed Solution

Creating heat energy with hydrogen without combustion and electricity 

 

Warming up to the process: 

How the heat is generated by hydrogen through exothermic reactions—reacting aluminum foil with NaOH and converting the hydrogen back into heat using a copper catalyst.

 

Ø  Gathering heat

How the process harnesses heat from exothermic reactions—aluminum with NaOH and hydrogen oxidation with a copper catalyst—rather than relying on a flame to ignite the combustion.

 

Ø  Assessing catalytic potential

whether copper can catalyze hydrogen oxidation at lower temperatures to capture exothermic energy

I’m detailing aluminum foil reacting with NaOH to emit hydrogen and heat, followed by hydrogen oxidation with copper catalyst, capturing the entire exothermic energy without needing flame ignition.   III. Impact and Benefits   •      Reduction in Waste: Reducing aluminium foil and      wood ash waste that pollutes the environment. •     Sustainable Energy Source: Providing more environmentally      friendly energy options for communities in need. •      Community Empowerment: Offering training and economic     opportunities through waste processing, which can increase      community income.   IV. Ongoing Projects   In theory we can harness the heat generated solely from the exothermic chemical processes without igniting an open flame. Let’s break down the two steps we described: 1.       Aluminum and Sodium Hydroxide Reaction When aluminum foil reacts with sodium hydroxide (NaOH) in water, the reaction is exothermic. It produces hydrogen gas along with sodium aluminate and releases a certain amount of heat during the process. The overall reaction is: 2Al (s)+2NaOH (aq)+6H2​O (l)→2NaAlO2​ (aq)+3H2​ (g) n this reaction, some chemical energy is directly converted into thermal energy (heat)   2.       Catalytic Oxidation of Hydrogen: The hydrogen produced can then be oxidized to water in the presence of oxygen. Typically, the oxidation of hydrogen is  a combustion reaction given by: 2H2​(g)+O2​(g)→2H2​O (l)+heat Under normal circumstances,  this reaction is ignited by a spark or flame because it has a high activation energy.  However, if you employ a catalyst (you mentioned copper,  though in many industrial cases catalysts like platinum or palladium are  more common for hydrogen oxidation), the catalyst can lower the activation energy enough  so that the reaction proceeds at a measurable rate without a traditional open flame.  In your proposed system, the idea is to capture the heat generated by the catalytic oxidation of hydrogen.    IV.1. Schematic Diagrams of the System      System Overview: 1. Bottom Chamber: Aluminum and Caustic Soda Reaction ·      Process: In the lower part of the system, aluminum foil reacts with sodium hydroxide (caustic soda)  in the presence of water. ·         Chemical Reaction: 2Al (s)+2NaOH (aq) +6H2​O (l)→2NaAlO2​ (aq) +3H2​ (g) ·  Outcome: This reaction is exothermic and produces hydrogen gas.  Although a part of the energy is released as heat in this step,  a significant portion of the potential energy is stored in the hydrogen gas produced.   2.      Middle Section: Hydrogen Flow and Catalytic Oxidation   ·          Process: The generated hydrogen gas rises from the bottom chamber  into an upper zone that contains a copper catalyst.   ·          Catalytic Oxidation:   Ø  Reaction:: 2H2​(g)+O2​(g) Catalyst (Cu) 2H2​O (l)+Heat   Ø  Role of the Catalyst: The copper catalyst helps lower the activation energy  required for the oxidation of hydrogen. As hydrogen contacts the catalyst  in the presence of oxygen (which must be supplied to the system, possibly  from a controlled inlet or pre-loaded air), the reaction occurs  without the need for an open flame. The reaction is exothermic, releasing  significant heat.   3.       Heat Transfer to the Evaporator Pipes ·       Process: The heat generated by both the exothermic aluminum–NaOH  reaction and the catalytic oxidation of hydrogen is captured within the closed system. ·       Design Feature: Embedded within the system are evaporator pipes  (or a network of pipes) containing water. The generated heat is transferred  to these pipes, heating the water. ·       Outcome: As the water in these pipes absorbs heat, its temperature rises  until it boils, producing steam. This steam can then be harnessed  to drive electric generator or for other thermal applications.   Automatic control of the system.    1.   When the thermos chamber is empty, the pressure {P} and temperature {T}  inside chamber are the same as the pressure and temperature’s room,  at this time solenoid-1 and solenoid-2 are the off condition and the both  valves channels are open, the NaOH solution and aluminum foil grains flow  to the bottom of the chamber.  2. In this condition the tap outlet valve is closed.  3. When the NaOH solution mixes with the aluminum foil grains,  an exothermic reaction occurs to produces hydrogen gas and heat.  4. The flow of hydrogen gas and heat will increase the pressure {P}  and temperature {T) in the chmber.   5. After a certain both pressure {P} and heat {T} condition, it will activate sensor  thereby activating selenoid-1 and 2, then both valves will close  6. the NaOH solution and aluminum foil granules will stop entering  the bottom of the chamber.  7. Oon the other hand, when the aluminum foil has completely oxidized  in the NaOH solution and stops reacting, this condition will be sensed  by the solution sensor and will activate selenoid-3 to open the tap  outlet valve, then all the remaining reaction fluid will flow out.  8. After all the remaining liquid has come out, the tap outlet valve  will automatically close again.  Henceforth, all of these processes from 1 to 8 will repeat again  until the NaOH solution and aluminum foil grains in the reservoir run out.   Under this conditions, pressure {P} and heat {T} will always occur in the chamber.    IV.2. Procurement of raw materials,    Because this program aims for empower community, some raw materials,  especially aluminum foil waste and NaOH production, must be carried out  by the community and the community must also be given training.  NaOH production can be made from wood ash and CaCO₃ .   in this program wood ash comes from ash left over  from burning pottery in Penujak Village,  West Praya District, Central Lombok Regency, West Nusa Tenggara Province.  Steps to Produce NaOH from Wood Ash and CaCO₃    Producing sodium hydroxide (NaOH) from wood ash and calcium carbonate (CaCO₃)  involves several steps, leveraging the basic chemistry of alkalis. Here's a simple guide:   Materials NeededWood: Wood Ash (preferably hardwood ash with high potassium and sodium content) Calcium Carbonate (CaCO₃) (e.g., limestone or chalk) Water  Containers (preferably non-metallic, like plastic or glass) Stirring Rod    Process 1. Leach Potassium and Sodium from Wood Ash Place the wood ash in a container. Add water to the ash in a 2:1 ratio (water:ash). Stir the mixture thoroughly and let it sit for 24–48 hours to allow  the potassium carbonate (K₂CO₃) and sodium carbonate (Na₂CO₃) to leach  into the water. Filter t 2. Prepare Calcium Hydroxide (Slaked Lime) Heat calcium carbonate (CaCO₃) to high temperatures (above 800°C)  in a kiln or furnace. This process produces calcium oxide (CaO)  and releases carbon dioxide The correct chemical reaction for the thermal decomposition  of calcium carbonate (CaCO₃) is: he mixture to separate the liquid (called lye water) from the ash residue.  The filtered liquid contains soluble alkali carbonates.  CaCO3​ heat    CaO+CO2​  This reaction shows that when calcium carbonate is heated,  it decomposes into calcium oxide (CaO) and carbon dioxide (CO₂).  3. React Lye Water with Calcium Hydroxide Mix the lye water (from Step 1) with calcium hydroxide (from Step 2). Stir the mixture well and let it sit for several hours. During this process,  calcium hydroxide reacts with potassium carbonate (K₂CO₃)  and sodium carbonate (Na₂CO₃) to form potassium hydroxide (KOH)  and sodium hydroxide (NaOH), precipitating calcium carbonate (CaCO₃) as a solid: The correct balanced chemical equation for the reaction  between sodium carbonate (Na₂CO₃) and calcium hydroxide (Ca(OH)₂) is: Na2​CO3​+Ca(OH)2          2NaOH+CaCO3​↓ This reaction forms sodium hydroxide (NaOH) and calcium carbonate (CaCO₃),  with calcium carbonate precipitating as a solid (indicated by the downward arrow).   4. Filter the Mixture Separate the liquid (containing NaOH and KOH) from the solid precipitate (CaCO₃)  using a fine cloth or coffee filter.   5. Concentrate the Solution Heat the filtered liquid gently to evaporate excess water, leaving behind a concentrated solution of NaOH and KOH.   6. Storage and Use Store the NaOH solution in a sealed, corrosion-resistant container.  It is now ready for use in various applications, such as producing hydrogen  or cleaning. . Safety Precautions Always wear gloves and eye protection when handling lye or caustic chemicals. Work in a well-ventilated area to avoid inhaling any fumes. Handle calcium oxide and hydroxide carefully as they can cause burns.    IV. 3. Lab. Scale Prototype    To make a lab scale prototype we will use the Gosun device (see Gosun image left), in this case we will try to to modify the Gosun and react NaOH and aluminum foil inside a Gosun cooking tube and will install a catalyst component in it. During the reaction process, the Gosun reflector is closed,. The way this equipment works to be the same as the Gosun works (see: https://gosun.co/blogs/news/how-do-solar-cookers-work,  the difference is that Gosun has to use sunlight as a source of heat energy while this device gain heat energy from the results of exothermic reactions in the tube. To estimate the amount of heat that can be generated from this system (the reaction between aluminum foil and sodium hydroxide to produce hydrogen, and then using copper catalyst to oxidize the hydrogen), we can break it down into two main parts: 1. Heat from the Reaction of Aluminum Foil with Sodium Hydroxide The exothermic reaction between aluminum (Al) and sodium hydroxide (NaOH) in water produces hydrogen (H₂) and heat. The reaction is as follows: 2Al (s)+2NaOH (aq) +6H2​O (l)→2NaAlO2​ (aq)+3H2​ (g) In this reaction, each mole of aluminum contributes to the formation of hydrogen and the release of heat. From thermodynamic data, the energy released from this reaction is approximately 1.6 kJ/mol for each mole of aluminum reacted. For example, if you use 1 gram of aluminum (which is about 0.037 mol), the energy released is:                                 Heat=0.037mol×1.6kJ/mol=0.059kJ(or 59 joules) 2. Heat from Hydrogen Combustion with Copper Catalyst Once hydrogen is produced, it is passed over a copper catalyst to oxidize it (burn it) to form water (H₂O), releasing heat. The reaction is as follows: 2H2​(g)+O2​(g)→2H2​O (l)+heat This exothermic reaction releases approximately 286 kJ/mol of energy for every mole of hydrogen burned. So, for the hydrogen produced from 1 gram of aluminum, which produces approximately 0.037 mol of hydrogen, the heat released is:                         Heat=0.037mol×286kJ/mol=10.6kJ   Total Heat Produced If we combine the heat from both reactions (aluminum and NaOH reaction, and hydrogen oxidation), the total heat generated is: Total Heat=59joules+10,600joules=10,659joules   Adjustment for a Closed System In a closed system, such as a thermos, we can assume that nearly all of this heat can be used to warm the water in the evaporator pipes. The system would have a high efficiency in terms of utilizing the heat, although some heat losses would occur due to insufficient insulation. Conclusion By using 1 gram of aluminum, we can generate approximately 10,659 joules (or 10.66 kJ) of heat from both exothermic reactions. This heat is enough to slightly warm water in a closed system. However, if we want to generate steam or increase the temperature significantly, we would need to use more aluminum or increase the system’s efficiency to generate more heat.    IV.4. Residual Product Pollution  The liquid released from the tap outlet is sodium aluminate (NaAlO₂) where is indeed formed in the reaction between aluminum and sodium hydroxide, and while it does have some industrial applications, its environmental impact largely depends on how it is managed. Environmental Impact of Sodium Aluminate: In its pure form, sodium aluminate is not inherently harmful, but its environmental impact depends on the concentration and how it is handled: Disposal Issues: If sodium aluminate is not disposed of properly, it can have negative environmental effects. For example, it could potentially lead to the contamination of water sources if it leaches into the environment. High pH levels associated with sodium hydroxide (the reagent used to produce sodium aluminate) can make water highly alkaline, which can harm aquatic life and ecosystems. Alkaline Nature: Sodium aluminate is alkaline in nature, so if it is released into natural water bodies in high concentrations, it can raise the pH of the water, which can be harmful to aquatic organisms and disrupt ecosystems. The pH level needs to be carefully controlled to avoid these effects. However, if sodium aluminate is used in controlled industrial processes and disposed of properly, it can have minimal environmental impact. As with any chemical, the key to preventing harm is in how it is handled and managed, especially in regard to waste treatment and disposal. Industrial Uses of Sodium Aluminate: Sodium aluminate has several useful applications in different industries, where it is not considered harmful when used correctly. Some notable applications include: Water Treatment: Sodium aluminate is often used as a coagulant in water and wastewater treatment plants. It helps remove impurities, such as suspended solids and organic matter, by promoting the aggregation of these particles into larger clumps (flocs), which can then be removed more easily. Paper Industry: In the paper industry, sodium aluminate is used in the production of sodium-based paper sizing agents. It can also help in bleaching processes, contributing to the strength and quality of the paper produced. Production of Alumina: Sodium aluminate is a key intermediate in the Bayer process for refining bauxite to produce alumina (Al₂O₃), the precursor to aluminum. This is one of its most important industrial applications, as alumina is the primary raw material used in aluminum production. Ceramics and Glass: Sodium aluminate is sometimes used in the production of ceramics and glass, where it serves as a flux to lower the melting point of certain materials and improve the properties of the final product. Cleaning and Descaling Agents: In some cases, sodium aluminate is used as a cleaning agent or descaling agent in industrial applications, such as removing scale deposits from metal surfaces and pipes. Conclusion: Sodium aluminate itself is not inherently harmful to the environment if handled and disposed of properly, though its alkaline nature does require caution to avoid damage to ecosystems. In fact, sodium aluminate has several industrial applications that are beneficial to industries like water treatment, paper production, and alumina refining. The key to mitigating any negative environmental impact lies in responsible use, waste treatment, and disposal practices.   IV.5. Key Considerations and Challenges Closed System Dynamics: In a thermos-like sealed system, heat loss to the environment is minimized, which improves the efficiency of heat transfer to the water. However, managing the internal pressure is critical, especially as steam forms and the temperature rises. Oxygen Supply for Oxidation: For the hydrogen oxidation to occur, oxygen must be present in the catalytic region. In a sealed system, this requires careful design—either by including a controlled oxygen reservoir or by managing the initial gas composition—so that sufficient oxygen is available without compromising the system's pressure or safety. Catalyst Efficiency and Safety: While copper can act as a catalyst, it might not be the most efficient for hydrogen oxidation compared to other catalysts (such as palladium). The catalyst must be maintained in optimal conditions to ensure the reaction occurs at a controlled rate without causing runaway reactions or overheating. Pressure Management: As the water in the evaporator pipes is heated to boiling, the generation of steam will increase the internal pressure. The system must be designed with robust pressure relief mechanisms or pressure-rated components (similar to a pressure cooker) to ensure safe operation. Heat Distribution: Uniform distribution of heat is essential to ensure consistent boiling of the water in the evaporator pipes. The system should be designed to maximize the transfer of heat from the reaction zones to the evaporator pipes, possibly through conductive materials or fluid circulation. Conclusion In summary, theoretically create a closed system (similar to a thermos) where: The aluminum and caustic soda reaction at the bottom generates hydrogen and some initial heat. The hydrogen rises and reacts in the presence of a copper catalyst (with supplied oxygen), releasing additional exothermic heat. This heat is then transferred to water in evaporator pipes to boil the water and produce steam for a mini steam engine or for other thermal applications. While the concept is feasible in theory, practical implementation requires careful engineering to manage oxygen supply, pressure, catalyst efficiency, and overall system safety.