Monday, 21/08/2023, 08:09.

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Edit¹:

Well, this is me from the future, if I remember correctly, almost all of this project log is useless.

But hey, I found this video here:

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It is about catalytic condensers.

Basically, if you apply a current through certain materials, you will change the amount of electrons on its surface, just like in a capacitor.

This change in electrons makes certains materials act as catalytic materials, just like platinum, palladium and others.

Maybe one could use cheap materials for catalytic condensers for hydrogen fuel cells, the problem is: which ones and how?

The video talks about more or less how these work and its use to produce hydrogen from ammonia, but I don't know how one could make a useful catalytic condenser in a DIY setup.

I'm trying to find more on the subject, but with no success.´

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I can only find articles about veeeery specific catalytic condensers, some for acid groups, others for processors (that use platinum for some reason).

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I also don't know for the life of me how much energy would these things need to act as catalysts, meaning it will inevitably affect the overall efficiency of the fuel cell.

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Well, my apologies, but I think I found something interesting. Basically, you can store hydrogen gas in solid Naphthalene.

(I feel like someone told me about this before and I stupidly ignored them, but I don't quite remember)

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As you may remember, I kinda gave up on the idea of using hydrogen as a fuel because hydrogen is pretty difficult to store, you either need carbon fiber 700 bar (70 MPa) pressure hydrogen gas tanks (which are expensive) or metal hydrides (which are triple expensive), but I think I found something interesting.

ChatGPT is kinda annoying to work with, because you really need to make the right questions in the right order to get the information that you need.

And it never cared to explain that there are other ways of storing hydrogen on solid compounds besides metal hydrides.

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Let's also remember that ChatGPT can be strongly incorrect about a subject.

Although it told me a lot, every time I try to get a useful information, it keeps saying that his knowledge was cut in 2021 and tells me to update to the premium version.

Basically telling me to screw off unless I have money.

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For example, it first told me that you could store 66kg of hydrogen gas in 1kg of naphthalene, then I asked if he was correct and then changed to 6% of hydrogen per kg of Naphthalene.

You could also store it on activated carbon and/or titanium powder, but it would be around 1 to 2% per kg.

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"Yes, there are liquids that can dissolve and store hydrogen gas. One example is organic liquids that are highly hydrogenated and have a high solubility for hydrogen gas. These liquids are often referred to as "liquid organic hydrogen carriers" (LOHCs). LOHCs are typically organic compounds that can reversibly bind and release hydrogen gas through chemical reactions.

Here's how the process generally works:

1. Absorption: The LOHC molecule reacts with hydrogen gas to form a hydrogenated version of the molecule.
2. Storage: The hydrogenated LOHC is stable and can be stored at room temperature and atmospheric pressure.
3. Desorption: When needed, the hydrogen gas can be released from the hydrogenated LOHC by reversing the reaction, which typically requires adding energy (e.g., heat).

The advantage of using LOHCs is that they offer a way to store and transport hydrogen gas without the need for high-pressure tanks, which are often required for storing gaseous hydrogen. This can enhance the safety and practicality of hydrogen storage and transportation.

Another example is using certain ionic liquids, which are salts that are liquid at relatively low temperatures, as solvents for hydrogen gas. These ionic liquids can interact with hydrogen molecules and store them within their structure. However, research in this area is still ongoing, and there are challenges to be addressed, including finding suitable ionic liquids that exhibit high hydrogen solubility and stability.

It's worth noting that while hydrogen gas can be dissolved in these liquids, the storage capacity may be limited compared to other storage methods like metal hydrides or compressed gas storage. The field of hydrogen storage is an active area of research, and scientists are exploring various materials and methods to make hydrogen storage more efficient, safe, and practical."

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"Certainly, here's a list of some common Liquid Organic Hydrogen Carriers (LOHCs) that have been researched for hydrogen storage:

1. Dibenzyltoluene (H12-DBT): This is one of the earliest and most well-known LOHCs. It can react with hydrogen to form hydrogenated dibenzyltoluene, and the hydrogen can be released by applying heat.
2. Methylcyclohexane (MCH): Methylcyclohexane can undergo reversible hydrogenation to form methylcyclohexane with hydrogen. The process is facilitated by catalysts, and the hydrogen can be released by dehydrogenation.
3. Tetrahydroquinoline (THQ): THQ can react with hydrogen to form hydrogenated tetrahydroquinoline, and the hydrogen can be released thermally or by using catalysts.
4. N-Ethylcarbazole (NEC): NEC can form hydrogenated N-ethylcarbazole upon hydrogenation. It is also studied as a potential LOHC.
5. Perhydrocarbazole (PHC): This LOHC can be hydrogenated to form perhydrogenated carbazole. PHC is under investigation as a hydrogen storage medium.
6. Dibenzylmethane (DBM): Dibenzylmethane can react with hydrogen to form a hydrogenated version, and the hydrogen can be released under appropriate conditions.
7. Decalin: Decalin, a bicyclic hydrocarbon, can be hydrogenated to form hydrogenated decalin. It has been explored as a potential LOHC for hydrogen storage.
8. Indoline: Indoline can react with hydrogen to form hydrogenated indoline, and the hydrogen release can be triggered through different methods, such as using catalysts.
9. Cyclohexylbenzene: Cyclohexylbenzene can be hydrogenated to form cyclohexylcyclohexane. It is being investigated for its potential as a LOHC.
10. Naphthalene: Naphthalene is another molecule that can reversibly react with hydrogen to form hydrogenated naphthalene, releasing hydrogen through thermal or catalytic processes."

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"Creating liquid organic hydrogen carriers (LOHCs) in a DIY way can be complex and potentially hazardous due to the handling of flammable materials and the need for specialized equipment. LOHCs are typically synthesized using various chemical reactions that require careful consideration of safety measures and appropriate facilities. However, I can provide you with a simplified overview of the types of LOHCs and their components. Please note that attempting to create these substances without proper expertise and equipment can be dangerous.

1. Toluene-Toluene Dihydrogen Carrier:
   • Components: Toluene, hydrogen gas, catalysts (e.g., noble metals like ruthenium or iridium).
   • Reaction: Hydrogenation of toluene to produce methylcyclohexane under hydrogen gas pressure. Releasing hydrogen involves the dehydrogenation process.
2. Naphthalene-Decalin Hydrogen Carrier:
   • Components: Naphthalene, hydrogen gas, catalysts.
   • Reaction: Hydrogenation of naphthalene to produce partially hydrogenated naphthalene (decalin) as the hydrogen carrier. Releasing hydrogen involves the dehydrogenation process.

It's important to note that while LOHCs offer advantages in terms of hydrogen storage and transport, their hydrogen storage capacities are generally lower compared to other hydrogen storage methods like compressed hydrogen gas or liquid hydrogen. However, LOHCs are advantageous because they allow for safer storage and transport of hydrogen under ambient conditions, avoiding the need for extreme pressures or low temperatures.

Keep in mind that the exact hydrogen capacity can vary based on factors such as the LOHC formulation, temperature, pressure, and the specific catalysts used in the hydrogenation and dehydrogenation processes."

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"The amount of hydrogen that a liquid organic hydrogen carrier (LOHC) can carry is typically expressed as the weight percentage of hydrogen per kilogram (wt% H2/kg) of the carrier substance. The exact capacity depends on the specific LOHC and its chemical structure. For reference, here are the approximate hydrogen storage capacities for toluene and a common toluene-based LOHC, methylcyclohexane:

1. Toluene (C7H8):
   • Hydrogen Capacity: Toluene itself does not have a high hydrogen storage capacity. It is not considered a practical hydrogen carrier due to its low hydrogen solubility and capacity. The hydrogen storage capacity of pure toluene is negligible.
2. Toluene-Dihydrogen Carrier (Methylcyclohexane):
   • Hydrogen Capacity: Methylcyclohexane (C7H14) is a hydrogenated form of toluene and is commonly used as a LOHC.
   • Hydrogen Capacity: Approximately 6-7 wt% H2/kg.
   • Note: This means that around 60 to 70 grams of hydrogen can be stored in one kilogram of methylcyclohexane.
3. The hydrogen storage capacity of a Naphthalene-Decalin hydrogen carrier, also known as a Napthalene-Decalin LOHC, is typically in the range of 5-6 wt% (weight percentage) hydrogen per kilogram of the carrier substance. This means that around 50 to 60 grams of hydrogen can be stored in one kilogram of the Naphthalene-Decalin LOHC.

Keep in mind that the exact hydrogen storage capacity can vary based on factors such as the specific formulation of the LOHC, temperature, pressure, and the specific catalysts used in the hydrogenation and dehydrogenation processes. Hydrogen storage in LOHCs offers advantages in terms of safety and ease of transport, even though their hydrogen storage capacities are lower compared to other methods like compressed hydrogen gas or liquid hydrogen."

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"To calculate the power in watts that can be generated from the combustion of 6 kg of hydrogen at room temperature and pressure (assuming standard conditions), you need to consider the energy content of hydrogen and the rate at which it is consumed. Hydrogen has an energy content of approximately 141.9 megajoules (MJ) per kilogram.

So, for 6 kg of hydrogen:

Energy (Joules) = Mass (kg) × Energy Content (MJ/kg) Energy = 6 kg × 141.9 MJ/kg = 851.4 MJ

To convert megajoules (MJ) to watts (W), you need to consider the time over which this energy is being released. Watts are calculated as joules per second (1 watt = 1 joule/second).

If you want to know the power generated over a certain period of time (e.g., one hour), you can calculate it as follows:

Power (Watts) = Energy (Joules) / Time (seconds)

Let's assume you want to know the power generated over the course of one hour (3600 seconds):

Power (Watts) = 851.4 MJ × 10^6 J/MJ / 3600 s = 236,500 watts

So, 6 kg of hydrogen at room temperature and pressure could potentially generate approximately 236,500 watts of power for one hour if all the hydrogen were to be combusted completely. Please note that in practice, the actual power output may vary depending on the efficiency of the combustion process and any energy losses."

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This means that in 100kg of Naphthalene there is space to more or less 200,000 watts of power.

Of course, it is not as light as Ethanol or gasoline, but it still is more or less 2000 watt hour per kilogram.

Obviously, you need to take into consideration the efficiency of release and adsorbption, the efficiency of the fuel cell and so on. Which would diminish the efficiency way bellow that.

The problem is that I couldn't find many DIY videos about how to do it, and you may need to remember that no energy conversion method is 100% efficient, a DIY hydrogen fuel cell may be in the 40% or bellow that while commercial ones are around 60%

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"Hydrogen storage in naphthalene involves a chemical reaction in which hydrogen gas is absorbed by the naphthalene molecule, resulting in the formation of a hydrogenated compound. This process is typically reversible, allowing for the release of hydrogen gas when needed. The mechanism by which hydrogen is stored in naphthalene is through a reversible hydrogenation-dehydrogenation reaction.

Here's a simplified overview of how hydrogen is stored in naphthalene:

1. Hydrogenation: During hydrogenation, naphthalene (C10H8) reacts with hydrogen gas (H2) in the presence of a suitable catalyst under controlled conditions. The hydrogen molecules break apart, and the resulting hydrogen atoms bond with the carbon atoms in the naphthalene molecule. This leads to the formation of a hydrogenated naphthalene compound.

   Naphthalene + Hydrogen → Hydrogenated Naphthalene

   This hydrogenation process allows naphthalene to act as a storage medium for hydrogen. The hydrogenated naphthalene compound is more stable and can store hydrogen in a chemically bound form.

2. Dehydrogenation: When hydrogen is needed, the hydrogenated naphthalene compound undergoes a dehydrogenation process. This involves breaking the chemical bonds between the hydrogen atoms and the carbon atoms in the naphthalene molecule. The released hydrogen atoms then recombine to form hydrogen gas.

   Hydrogenated Naphthalene → Naphthalene + Hydrogen

The reversibility of this reaction allows for a cycle of hydrogen storage and release. The process involves controlling temperature, pressure, and the use of catalysts to facilitate both hydrogenation and dehydrogenation reactions. By managing these factors, scientists aim to optimize the efficiency of the storage and release processes.

It's important to note that while naphthalene-based hydrogen storage has been explored in research settings, there are practical challenges to be addressed. These challenges include achieving high storage capacity, rapid reaction kinetics, and efficient release of hydrogen gas while maintaining the stability and recyclability of the storage medium. Researchers continue to work on improving the performance of naphthalene and similar compounds as hydrogen storage materials."

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"Hydrogenation and dehydrogenation reactions in hydrogen storage materials like naphthalene are typically facilitated by the use of catalysts and controlled reaction conditions. Catalysts are substances that accelerate chemical reactions without being consumed themselves. The process involves carefully controlling temperature, pressure, and the presence of the catalyst to promote the desired reactions.

Here's a general overview of how hydrogenation and dehydrogenation are carried out for hydrogen storage in naphthalene:

Hydrogenation:

1. Catalyst: A suitable catalyst is chosen to promote the hydrogenation reaction. The catalyst helps break the strong bonds between hydrogen molecules (H2) and naphthalene (C10H8) and allows hydrogen atoms to bond with the carbon atoms in the naphthalene molecule.
2. Reaction Conditions: The hydrogenation reaction is typically performed at elevated temperatures and pressures. The specific conditions may vary based on the chosen catalyst and the desired reaction rate. Common temperatures can range from around 100 to 300°C, and pressures can vary from moderate to high.
3. Hydrogen Supply: Hydrogen gas is introduced into the system at the desired pressure. The hydrogen gas will react with naphthalene in the presence of the catalyst, leading to the formation of hydrogenated naphthalene.

Dehydrogenation:

1. Catalyst: A different catalyst might be used for the dehydrogenation reaction, as the conditions required for hydrogenation and dehydrogenation might not be exactly the same. The dehydrogenation catalyst promotes the breaking of the carbon-hydrogen bonds in the hydrogenated naphthalene compound.
2. Reaction Conditions: Dehydrogenation is typically carried out at higher temperatures than hydrogenation. The temperature range can vary but often falls between 250 to 400°C. The pressure may also be adjusted based on the catalyst and desired reaction rate.
3. Heating: The hydrogenated naphthalene is heated to the appropriate temperature. This heat energy provides the activation energy needed to break the carbon-hydrogen bonds and release hydrogen gas.

In both cases, the key is to carefully manage the reaction conditions to achieve the desired reaction rates and maximize the efficiency of the storage and release processes. Catalysts play a crucial role in enabling the reactions to occur at manageable temperatures and pressures, making the process more practical for real-world applications.

It's important to note that the specific catalysts, conditions, and mechanisms used can vary based on ongoing research and development efforts in the field of hydrogen storage. Scientists continually work to discover new and improved catalysts and methods to enhance the efficiency and feasibility of hydrogen storage technologies."

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"The choice of catalysts for the hydrogenation and dehydrogenation of hydrogen storage materials like naphthalene depends on several factors, including reaction kinetics, stability, selectivity, and compatibility with the specific compounds involved. Over the years, various catalysts have been explored for these processes, and ongoing research aims to identify catalysts that offer better performance and efficiency.

For hydrogenation and dehydrogenation reactions involving naphthalene, different catalysts can be used:

Hydrogenation Catalysts:

1. Transition Metal Catalysts: Catalysts based on transition metals, such as palladium (Pd), platinum (Pt), and nickel (Ni), are commonly used for hydrogenation reactions. These metals can facilitate the dissociation of hydrogen molecules and promote the addition of hydrogen to the carbon-carbon double bonds in naphthalene.
2. Supported Catalysts: Catalysts can be supported on various materials to enhance their stability and dispersion. For example, palladium on carbon (Pd/C) or platinum on alumina (Pt/Al2O3) are frequently used hydrogenation catalysts.
3. Ruthenium Catalysts: Ruthenium (Ru) catalysts have also been studied for hydrogenation reactions due to their high activity and selectivity.

Dehydrogenation Catalysts:

1. Metal Oxides: Metal oxides like chromium oxide (Cr2O3), iron oxide (Fe2O3), and manganese oxide (MnO2) are often used as dehydrogenation catalysts. These catalysts can help break the carbon-hydrogen bonds in hydrogenated compounds during the dehydrogenation process.
2. Supported Catalysts: Similar to hydrogenation, supported catalysts can also be used for dehydrogenation. For example, supported metal catalysts like Pt/C or Pd/C can facilitate the release of hydrogen from hydrogenated naphthalene.
3. Complex Metal Hydrides: Certain complex metal hydrides can act as both hydrogenation and dehydrogenation catalysts. These materials can reversibly release and uptake hydrogen and are of interest for hydrogen storage applications.

It's important to note that the selection of catalysts and their optimization can greatly impact the efficiency and effectiveness of the hydrogenation and dehydrogenation processes. The goal is to find catalysts that allow for fast and controllable reactions while minimizing side reactions and energy losses. Researchers continue to explore new catalysts and catalyst systems to improve the performance of hydrogen storage materials for practical applications."

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"Enhancing the performance of liquid organic hydrogen carriers (LOHCs) like Toluene-Dihydrogen Carrier and Naphthalene-Decalin Hydrogen Carrier can involve the use of various additives. These additives can improve aspects such as hydrogen storage capacity, reaction kinetics, stability, and safety. Here's a list of potential enhancers, along with examples of each type:

Catalysts: Catalysts accelerate chemical reactions and can enhance the efficiency of hydrogenation and dehydrogenation processes.

• Noble metal catalysts: Ruthenium (Ru), Rhodium (Rh), Iridium (Ir).
• Transition metal catalysts: Nickel (Ni), Cobalt (Co).

Co-solvents: Co-solvents can modify the solvent properties of the LOHC, affecting solubility and reaction kinetics.

• Toluene-based LOHC: Adding small amounts of specific solvents like cyclohexane or heptane.
• Naphthalene-based LOHC: Mixing with other aliphatic hydrocarbons.

Chemical Modifiers: Modifiers can alter the chemical structure of the LOHC to improve hydrogenation and dehydrogenation properties.

• Adding alkyl or alkenyl substituents to the aromatic ring of the LOHC molecules.

Stabilizers: Stabilizers prevent unwanted side reactions or decomposition of the LOHC.

• Hindered phenols: Antioxidants like butylated hydroxytoluene (BHT).
• Radical scavengers: Hindered amine light stabilizers (HALS).

Hydrogenation Promoters: These substances enhance the rate or efficiency of hydrogenation reactions.

• Metal hydrides: Sodium borohydride (NaBH4), lithium aluminum hydride (LiAlH4).
• Molecular hydrogenation catalysts: Wilkinson's catalyst (RhCl(PPh3)3).

Dehydrogenation Promoters: Additives that facilitate the dehydrogenation process.

• Metal oxide promoters: Magnesium oxide (MgO), zinc oxide (ZnO).

Thermal Enhancers: Substances that improve heat transfer or thermal stability.

• Thermal conductivity enhancers: Graphene, carbon nanotubes.
• Heat-resistant materials: Silicon carbide (SiC) nanoparticles.

Surfactants and Emulsifiers: These can help disperse or stabilize immiscible components.

• Surfactants: Sodium dodecyl sulfate (SDS), cetyltrimethylammonium bromide (CTAB).
• Emulsifiers: Polyethylene glycol (PEG).

It's important to note that the selection and use of these enhancers require careful consideration of their effects, compatibility with the LOHC, potential for side reactions, and safety. Working with these additives might involve complex chemical processes and may require expertise in the field of organic chemistry. If you're interested in enhancing LOHCs, consulting experts and conducting thorough research is recommended."

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This video talks about a supposedly hydrogen breakthrough that allows the use of hydrogen storage on borous nitride powder.

Basically, you "just" put the boron nitride in a tumbling chamber and let it roll for days or weeks, which will build defects on the boron nitride that allows for hydrogen storage.

You could mix both in a single storage, perhaps.

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Also, it just came to me that you would could simply make a self-contained hydrogen fuel cell using this naphthalene, just like a battery.

Basically, carrying your own hydrogen and your own oxygen, react both to generate electricity, then when recharging, you would take the water that was made and make an electrolysis reaction, separating the oxygen from hydrogen and containing both gases in their structural storage.
A reversible hydrogen fuel cell, basically.

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In an hydroge-oxygen reaction you would need a ratio of 2:1 to oxygen gas, so 1.5kg for the 3kg of hydrogen in naphtalene/titanium/tuolene/boron nitride.

Then you would need a oxide to store the oxygen gas, in this case, pure iron powder.

And you would need a 4:3 ratio of iron to oxygen, so you would need around 3kg to 6kg of pure iron in order to store the oxygen gas in solid form.

Then, once the hydride structure is fully saturated with hydrogen and the oxide structure is fully saturated with oxygen gas, you can start the release of both gases that go into the fuel cell in order to generate electricity.

So, 100kg of naphthalene (without the catalysts) + 3kg of hydrogen + 1.5kg of oxygen + 6kg iron powder (without the catalysts) = 110.5kg in total.

And since the 3kg of hydrogen would have more or less 360 megajoules of energy, or 100,000 Watt-hour, this battery would have around 905 watt-hour per kg.

Of course, not counting the inneficiency of the fuel cell, which in a DIY setup would be around 40%.

Plus, if you count the weight of the catalyst, the weight of the fuel cell itself and the weight of the enclosure (because 3kg of hydrogen gas inside a container is no joke), you would get less than 300 wh/kg of energy density. Which is comparable to lithium-ion batteries (250 wh/kg).

... Which is kinda disappointing... Compared to hydrocarbons/fossil fuels.

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But it also shows how hard it is to actually achieve high energy density.

If you can find a material that can absorb twice the amount of hydrogen gas (6% per weight), then you would have 1400 wh/kg of energy density.

But like I said: with the inneficiencies, less than half of that, around 600 to 500 wh/kg.

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"Certainly, here are some examples of materials from the categories I mentioned, along with their potential hydrogen adsorption capacities (as of my last update in September 2021). Please note that the numbers provided are approximate and may have changed due to ongoing research and advancements.

1. Metal-Organic Frameworks (MOFs):
   • MOF-177: ~6.0 wt% hydrogen adsorption.
   • IRMOF-20: ~5.5 wt% hydrogen adsorption.
2. Porous Organic Polymers (POPs):
   • COP-150: ~5.6 wt% hydrogen adsorption.
   • PAF-1: ~6.0 wt% hydrogen adsorption.
3. Hydrides:
   • MgH2 (Magnesium Hydride): ~7.6 wt% hydrogen adsorption.
   • LiAlH4 (Lithium Aluminum Hydride): ~10.5 wt% hydrogen adsorption.
4. Nanoporous Materials:
   • MCM-41 (Mesoporous Silica): ~2.5 wt% hydrogen adsorption.
   • SBA-15 (Ordered Mesoporous Silica): ~2.8 wt% hydrogen adsorption.
5. Carbon-Based Materials:
   • Activated Carbon: Varies widely, often less than 2 wt% hydrogen adsorption.
   • Carbon Nanotubes: Varies, typically less than 2 wt% hydrogen adsorption.
6. Complex Hydrides:
   • NaBH4 (Sodium Borohydride): ~10.5 wt% hydrogen adsorption.
   • LiBH4 (Lithium Borohydride): ~18.5 wt% hydrogen adsorption.
7. Chemical Hybrids:
   • LiNH2-BH3 (Lithium Amidoborane-Borane): ~11.5 wt% hydrogen adsorption.
   • NaNH2-LiH (Sodium Amide-Lithium Hydride): ~10.5 wt% hydrogen adsorption.

It's important to emphasize that these values are approximate and can vary depending on factors such as temperature, pressure, material modification, and storage conditions. Research in this field is ongoing, and new materials or improved variations may have emerged since my last update. For the most up-to-date information, I recommend consulting recent scientific literature or research publications in the field of hydrogen storage."

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Well, magnesium seems interesting.

Only because it is cheaper and easier to find than the other options.

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"Hydrogen adsorption and release in magnesium-based materials, such as magnesium hydride (MgH2), involve complex chemical reactions and physical processes. Magnesium hydride is a solid-state hydrogen storage material that can reversibly absorb and release hydrogen gas under suitable conditions.

Hydrogen Adsorption in Magnesium Hydride (MgH2):

1. Adsorption Mechanism: Hydrogen adsorption occurs through a process called physisorption, where hydrogen molecules are weakly bound to the surface of the magnesium atoms. This is mainly a physical process that involves van der Waals forces between hydrogen molecules and the magnesium surface.
2. Activation Energy: While the physisorption process is relatively simple, the activation energy required for hydrogen molecules to overcome the energy barrier and adsorb onto the magnesium surface can be relatively high. This can result in slow kinetics for both adsorption and desorption processes.

Hydrogen Release (Desorption) in Magnesium Hydride (MgH2):

1. Desorption Mechanism: The release of hydrogen from magnesium hydride involves breaking the chemical bonds between hydrogen and magnesium. This process is more complex and can occur through various mechanisms, including thermal desorption, reaction with a catalyst, or combination with another chemical compound.
2. Thermal Desorption: One common method for releasing hydrogen from magnesium hydride is by raising the temperature. This provides the energy required to break the bonds between hydrogen and magnesium. However, high temperatures are often needed, and this can lead to issues with material degradation and slow kinetics.
3. Catalytic Dehydrogenation: Adding a catalyst can significantly lower the desorption temperature and improve the kinetics of hydrogen release. Catalysts can create pathways for hydrogen atoms to migrate within the material, facilitating the breaking of chemical bonds. Common catalysts include transition metals and their alloys, as well as additives like TiCl3.
4. Mechanical Activation: Mechanical grinding or milling of the material can also enhance hydrogen release kinetics. This physically breaks down the material into smaller particles, increases the surface area, and can create defects that promote hydrogen release.
5. Nanostructuring: Creating nanostructured versions of magnesium hydride can further improve its hydrogen storage properties. Nanostructuring increases the surface area, reduces diffusion distances, and can lead to faster hydrogen adsorption and release kinetics.

It's worth noting that the practical application of magnesium hydride and similar materials for hydrogen storage faces challenges such as slow kinetics, high operating temperatures, and the need for efficient catalysts. Researchers are continuously working on improving these aspects to make magnesium-based hydrides more viable for real-world hydrogen storage applications."

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Now let's see how do I get those other types of hydrides that would allow me to reach even 1000 watts-hour per kg.

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Synthesizing chemicals like Ammonia Borane (NH3BH3), Sodium Borohydride (NaBH4), Lithium Borohydride (LiBH4), Lithium Amidoborane-Borane (LiNH2-BH3), and Sodium Amide-Lithium Hydride (NaNH2-LiH) in a DIY setup can be challenging due to the need for precise control over reaction conditions, the use of hazardous materials, and the potential for safety risks. These compounds often involve reactive and potentially dangerous chemicals. Additionally, some of these reactions may require specialized equipment and expertise in handling chemicals safely. Therefore, it's crucial to prioritize safety and consider the legality and regulations regarding the production and handling of these substances in your area.

That said, I can provide a very high-level overview of the synthesis of these chemicals:

1. Ammonia Borane (NH3BH3):
   • Ammonia borane can be synthesized by reacting borane (BH3) with ammonia (NH3) in an aprotic solvent under controlled conditions. This reaction is typically carried out in a laboratory setting due to the sensitivity of borane compounds to air and moisture.
2. Sodium Borohydride (NaBH4):
   • Sodium borohydride is often commercially available but can be synthesized by reacting sodium hydride (NaH) with boron trifluoride etherate (BF3·OEt2) in diethyl ether followed by the addition of sodium borohydride.
3. Lithium Borohydride (LiBH4):
   • Lithium borohydride can be prepared by the reaction of lithium hydride (LiH) with boron trifluoride etherate (BF3·OEt2) in diethyl ether followed by the addition of lithium borohydride.
4. Lithium Amidoborane-Borane (LiNH2-BH3):
   • This compound is often prepared by the reaction of lithium amide (LiNH2) with borane-tetrahydrofuran (BH3·THF) in anhydrous conditions.
5. Sodium Amide-Lithium Hydride (NaNH2-LiH):
   • Sodium amide-lithium hydride is typically prepared by mixing sodium amide (NaNH2) and lithium hydride (LiH) in an inert atmosphere.

Please note that the above descriptions are simplified and do not provide detailed step-by-step instructions. The synthesis of these chemicals involves the use of hazardous and reactive materials, and it should only be attempted by individuals with the necessary knowledge, skills, and access to proper laboratory equipment and safety protocols.

Additionally, the production and handling of certain chemicals may be subject to local, state, or federal regulations, so it's essential to be aware of and comply with any legal requirements in your area. If you are interested in working with these chemicals, I strongly recommend seeking guidance from a qualified chemist or researcher and conducting any work in a safe and controlled laboratory environment.

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Among the chemicals you've listed, Sodium Borohydride (NaBH4) is generally considered to be the easiest and safest to work with in a DIY setup, although it's still important to exercise caution and adhere to proper safety practices.

Here's why Sodium Borohydride (NaBH4) is often considered relatively easier and safer:

1. Availability: Sodium borohydride is commercially available as a reagent, making it easier to obtain compared to some other chemicals on your list.
2. Stability: While it is sensitive to moisture and should be stored in a dry environment, sodium borohydride is generally more stable compared to some other boron-containing hydrides.
3. Reaction Conditions: The synthesis of sodium borohydride involves relatively milder reaction conditions compared to some of the other compounds, and the reactions typically occur at or around room temperature.
4. Handling: Sodium borohydride is less reactive and less prone to spontaneous reactions than other boron hydrides, such as borane compounds.

However, even with sodium borohydride, it's important to follow proper safety guidelines:

• Always wear appropriate personal protective equipment, including gloves and safety goggles.
• Work in a well-ventilated area to minimize inhalation exposure to any potential fumes.
• Handle the chemical in a dry atmosphere to prevent moisture exposure.
• Be cautious when working with chemicals and reactions, and be aware of the potential hazards associated with sodium borohydride, which can release hydrogen gas upon contact with water or acids.

Remember that working with any chemicals involves inherent risks, and if you're not experienced in handling chemicals or if you're not equipped with a proper laboratory setup, it's best to avoid attempting these syntheses at home. Instead, consider reaching out to educational institutions or research facilities where you might be able to access appropriate resources and guidance for safe experimentation. Always prioritize safety and adhere to local regulations and laws regarding chemical handling and experimentation.

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Synthesizing Sodium Borohydride (NaBH4) involves the reaction of boron trifluoride etherate (BF3·OEt2) with sodium hydride (NaH) in a suitable solvent. The process requires careful handling and should be conducted in a well-ventilated laboratory environment, as it involves potentially hazardous chemicals. Here's a high-level overview of the synthesis:

Materials Needed:

• Boron trifluoride etherate (BF3·OEt2)
• Sodium hydride (NaH)
• Suitable solvent (diethyl ether is commonly used)
• Apparatus for reaction, such as a round-bottom flask, condenser, and drying tube
• Safety equipment, including gloves, safety goggles, and a lab coat
• Proper ventilation and fume hood

Procedure:

1. Set up the reaction apparatus, including a round-bottom flask fitted with a condenser and drying tube. The drying tube is used to prevent moisture from entering the system.
2. In the round-bottom flask, add an appropriate amount of boron trifluoride etherate (BF3·OEt2). The molar ratio of boron trifluoride to sodium hydride will determine the yield of sodium borohydride.
3. Carefully add sodium hydride (NaH) to the round-bottom flask containing boron trifluoride etherate. Sodium hydride is moisture-sensitive, so it's crucial to handle it in a dry atmosphere.
4. Add a suitable solvent, such as diethyl ether, to the mixture to facilitate the reaction. The solvent should be dry to avoid introducing moisture.
5. Fit the round-bottom flask with a condenser to prevent the loss of volatile components and to ensure that the reaction takes place under reflux conditions.
6. Heat the mixture gently to initiate the reaction. The reaction will produce sodium borohydride and other byproducts.
7. Allow the reaction to proceed for a specified period while maintaining reflux conditions. The reaction time may vary based on reaction conditions.
8. After the reaction is complete, allow the mixture to cool.
9. Carefully work up the reaction mixture by filtering off any solid impurities that may have formed.
10. The filtrate should contain sodium borohydride dissolved in the solvent. This solution can be concentrated or further purified if desired.
11. Sodium borohydride is highly reactive and can release hydrogen gas when it comes into contact with water or acids. Therefore, it's essential to handle and store the product properly to prevent any unintended reactions.

Please note that this is a simplified overview of the synthesis process, and the actual procedure may require adjustments based on specific reaction conditions, equipment availability, and safety considerations. Additionally, working with sodium hydride and boron trifluoride requires careful planning, knowledge of safe laboratory practices, and appropriate protective equipment. If you're not experienced in handling these chemicals, it's best to seek guidance from a qualified chemist or researcher before attempting the synthesis.

---

"The synthesis of Lithium Borohydride (LiBH4) is a bit more complex than some other hydrides and involves multiple steps. It typically requires the reaction of lithium hydride (LiH) with boron trifluoride etherate (BF3·OEt2) in an aprotic solvent. Here's a general overview of the synthesis:

Materials Needed:

• Lithium hydride (LiH)
• Boron trifluoride etherate (BF3·OEt2)
• Aprotic solvent (such as diethyl ether or tetrahydrofuran)
• Apparatus for reaction, such as a round-bottom flask, condenser, and drying tube
• Safety equipment, including gloves, safety goggles, and a lab coat
• Proper ventilation and fume hood

Procedure:

1. Set up the reaction apparatus, including a round-bottom flask fitted with a condenser and drying tube. The drying tube is used to prevent moisture from entering the system.
2. In the round-bottom flask, add an appropriate amount of lithium hydride (LiH). Handle lithium hydride with care, as it reacts violently with water.
3. Carefully add boron trifluoride etherate (BF3·OEt2) to the round-bottom flask containing lithium hydride. Boron trifluoride is often used as a complex with diethyl ether to improve its reactivity.
4. Add a suitable aprotic solvent, such as diethyl ether or tetrahydrofuran, to the mixture. The solvent should be dry to avoid introducing moisture.
5. Fit the round-bottom flask with a condenser to prevent the loss of volatile components and to ensure that the reaction takes place under reflux conditions.
6. Heat the mixture gently to initiate the reaction. The reaction will produce lithium borohydride (LiBH4) and other byproducts.
7. Allow the reaction to proceed for a specified period while maintaining reflux conditions. The reaction time may vary based on reaction conditions.
8. After the reaction is complete, allow the mixture to cool.
9. Carefully work up the reaction mixture by filtering off any solid impurities that may have formed.
10. The filtrate should contain lithium borohydride dissolved in the solvent. This solution can be concentrated or further purified if desired.
11. Lithium borohydride is moisture-sensitive and reactive, so it's important to handle and store the product properly to prevent any unintended reactions.

Please note that the synthesis of lithium borohydride involves working with reactive and potentially hazardous chemicals. It requires careful planning, proper safety practices, and knowledge of handling air-sensitive compounds. If you're not experienced in working with these chemicals, it's best to seek guidance from a qualified chemist or researcher before attempting the synthesis."

---

Well, as it seems, this is a really dangerous and complex procedure that I really, really wouldn't advise doing at home.

And even if you could, why even bother?

You would so much lithium for this that it would be better to simply buy lithium-ion batteries.

---

Also, I was looking at sodium borohydride reaction and got me wondering:

If the metal hydride, in this case sodium borohydride, releases hydrogen gas, water and sodium metaborate in the presence of oxygen gas, doesn't it mean that I can simply take sodium metaborate and react it with hydrogen gas in the presence of a catalyst in order to get sodium borohydride?

Well, ChatGPT says that it wouldn't be that simple and it probably wouldn't work.

---

But you can imagine that I was trying to think in a way of making a solid state metal-hydrogen fuel cell, where the oxygen and hydrogen would be contained in solid metals instead of gas.

So the hydrogen on metal hydrides would react with the oxygen in metal oxides, making a battery more powerful than lithium-ion batteries and somewhat cheaper.

But you would need a metal hydride that can easily be hydrogenated and de-hydrogenated (releasing hydrogen) in a easy way...

Well, I'm asking around, but I doubt someone will be in the mood to answer me. Or else I wouldn't be messing with ChatGPT in the first place.

---

I asked a similar thing and I got this answer from Poe (a ChatGPT based AI of quora):

---

"Storing hydrogen gas can be challenging due to its low density and high reactivity. However, there are materials that can be used to store hydrogen by reacting with it and releasing it later by reacting it with oxygen gas.

One example of a material commonly used for this purpose is metal hydrides. Metal hydrides are compounds formed by the reaction of hydrogen with certain metals. They can absorb and store hydrogen gas and release it upon heating or by reacting with an oxidizing agent like oxygen gas.

One specific metal hydride that has been extensively studied for hydrogen storage is called sodium borohydride (NaBH4). NaBH4 can react with hydrogen gas to form sodium borohydride dihydrate (NaBH4·2H2O), which is a stable compound capable of storing hydrogen. When heated or exposed to a catalyst, NaBH4·2H2O can release hydrogen gas by reacting with oxygen:

2NaBH4·2H2O + O2 → 2NaBO2 + 4H2 + 2H2O

This reaction liberates hydrogen gas and forms sodium metaborate (NaBO2) and water as byproducts. The released hydrogen gas can then be utilized for various applications.

It's worth noting that the development of efficient and practical hydrogen storage materials is an active area of research, and there are ongoing efforts to discover and optimize new materials with improved storage capacities, release kinetics, and safety characteristics."

---

"One material that can be easily hydrogenated in the presence of hydrogen and dehydrogenated in the presence of oxygen is a class of compounds called organic hydrides or liquid organic hydrogen carriers (LOHCs).

LOHCs are organic compounds that can reversibly react with hydrogen to form stable hydride compounds and release hydrogen upon exposure to an oxidizing agent like oxygen. They act as carriers for hydrogen, allowing for its storage and transportation in a safe and efficient manner.

One example of an LOHC is toluene, which can be hydrogenated to form methylcyclohexane (MCH) in the presence of a catalyst and hydrogen:

Toluene + H2 → Methylcyclohexane

MCH can be easily stored and transported, and when desired, it can be dehydrogenated by reacting it with oxygen in the presence of a catalyst:

Methylcyclohexane + O2 → Toluene + H2O

This reaction liberates hydrogen gas and regenerates toluene, allowing for the release of hydrogen when needed.

LOHCs offer advantages such as high hydrogen storage capacity, ease of handling, and the ability to use existing infrastructure for storage and transportation. They are being actively researched for their potential applications in hydrogen storage and energy systems."

---

"The molar mass of hydrogen (H2) is approximately 2 grams/mol, and the molar mass of methylcyclohexane (C7H14) is approximately 98 grams/mol.

To determine the percentage of hydrogen in 1 kg of methylcyclohexane, we need to calculate the number of moles of hydrogen and methylcyclohexane.

Number of moles of hydrogen: 1 kg = 1000 grams Number of moles of H2 = (1000 grams) / (2 grams/mol) = 500 moles

Number of moles of methylcyclohexane: 1 kg = 1000 grams Number of moles of C7H14 = (1000 grams) / (98 grams/mol) ≈ 10.204 moles

Now, we can calculate the percentage of hydrogen in 1 kg of methylcyclohexane:

Percentage of hydrogen = (moles of hydrogen / total moles) × 100 = (500 moles / (500 moles + 10.204 moles)) × 100 ≈ 97.98>#/p###

Therefore, approximately 97.98% of the weight of 1 kg of methylcyclohexane is hydrogen."

I was quite skeptical of this result, so I asked ChatGPT in a new tab and it gave me around 20 grams per kg, which is inside the 2% of hydrogen per kg of weight threshold.

---

"There are several other types of materials that can be easily hydrogenated and dehydrogenated in the presence of hydrogen. Here is a list of some commonly studied materials along with the approximate percentage of extractable hydrogen by weight:

1. Liquid Organic Hydrogen Carriers (LOHCs):
   • Methylcyclohexane (MCH): Approximately 13.3% hydrogen by weight.
   • Decalin: Approximately 14.5% hydrogen by weight.
   • Tetrahydroquinoline (THQ): Approximately 12.2% hydrogen by weight.
   • N-Ethylcarbazole (NEC): Approximately 11.8% hydrogen by weight.
2. Metal Hydrides:
   • Sodium Borohydride (NaBH4): Approximately 10.6% hydrogen by weight.
   • Lithium Aluminum Hydride (LiAlH4): Approximately 10.1% hydrogen by weight.
   • Ammonia Borane (NH3BH3): Approximately 19.6% hydrogen by weight.
3. Complex Hydrides:
   • Sodium Alanate (NaAlH4): Approximately 5.6% hydrogen by weight.
   • Lithium Borohydride (LiBH4): Approximately 18.5% hydrogen by weight.
   • Magnesium Hydride (MgH2): Approximately 7.6% hydrogen by weight.

It's important to note that these percentages can vary depending on the specific material, conditions of hydrogenation/dehydrogenation, and any additional compounds involved in the system. The numbers provided are rough estimates to give you an idea of the hydrogen content in these materials."

---

"Obtaining ammonia borane (NH3BH3) in a DIY setup can be challenging and potentially hazardous. Ammonia borane is a complex hydride that requires careful handling and specific conditions for synthesis. It is typically produced on an industrial scale using specialized equipment and processes.

The synthesis of ammonia borane involves the reaction between ammonia (NH3) and borane (BH3) in a controlled environment. Borane is a highly reactive and toxic gas, and ammonia itself can be hazardous if not handled properly. Additionally, the synthesis process may require the use of specific catalysts and careful control of temperature and pressure.

Due to the complexity and potential hazards involved, it is not recommended to attempt synthesizing ammonia borane in a DIY setup unless you have the necessary expertise, safety knowledge, and access to appropriate facilities and equipment. It is advisable to obtain ammonia borane from commercial sources that specialize in supplying such chemicals."

---

"After releasing hydrogen, ammonia borane (NH3BH3) undergoes a decomposition reaction, resulting in the formation of solid boron nitride (BN) and gaseous ammonia (NH3) as the main products. The reaction can be represented as follows:

2NH3BH3 → BN + 6H2 + 2NH3

The solid boron nitride (BN) formed is a ceramic compound composed of boron and nitrogen atoms arranged in a crystalline lattice structure. Boron nitride has various properties, including high thermal stability, excellent electrical insulation, and chemical inertness. It is often used as a lubricant, a heat-resistant material, and in electronic applications due to its unique properties.

The gaseous ammonia (NH3) released during the decomposition of ammonia borane is a colorless gas with a pungent odor. Ammonia has several industrial applications, including its use as a fertilizer, a refrigerant, and in the production of various chemicals. It is also used in cleaning agents and as a precursor in the synthesis of numerous compounds."

---

"The process of converting boron nitride (BN) and ammonia (NH3) back into ammonia borane (NH3BH3) is not as straightforward as simply exposing them to hydrogen gas. The reverse reaction requires specific conditions and often involves a multi-step synthetic process.

One common method to regenerate ammonia borane from boron nitride and ammonia is through a reaction called rehydrogenation. This process typically involves the use of additional reagents and catalysts. One approach is to react boron nitride with hydrogen gas in the presence of a suitable catalyst to convert it back to ammonia borane. The reaction may proceed as follows:

BN + xH2 → NH3BH3

The exact conditions, catalysts, and stoichiometry required for this rehydrogenation reaction may vary depending on the specific process and desired outcome. It is worth noting that the rehydrogenation of boron nitride is an active area of research, and various methods and catalysts are being investigated to optimize the efficiency of this conversion.

It is important to consider that these reactions can be complex and may require specialized knowledge, handling, and equipment. Attempting these processes without proper expertise and safety precautions is not recommended. If you require ammonia borane, it is generally more practical to obtain it from commercial sources rather than attempting its synthesis in a DIY setup."

>the process of converting back to ammonia borane is not as straightforward
>add hydrogen gas to the mix

bruh

---

"To "store" ammonia gas by reacting it with another material and easily releasing ammonia, one option is to use an amine-based solid sorbent. These sorbents can react with ammonia gas to form an ammonium salt or a solid complex, which can then be heated or subjected to specific conditions to release the stored ammonia.

One example of an amine-based solid sorbent is Ammonia Borane (NH3BH3), which we discussed earlier. Ammonia borane can react with ammonia gas to form a solid complex, and upon heating or under certain conditions, it can release the stored ammonia. However, it is worth noting that ammonia borane itself is not commonly used for this purpose due to its higher cost and other considerations.

Other amine-based solid sorbents, such as metal-organic frameworks (MOFs) or porous materials like zeolites, can also be used to store and release ammonia. These materials have a high affinity for ammonia and can form stable complexes with it. By adjusting the temperature or other parameters, the stored ammonia can be released from the sorbent.

The specific choice of sorbent will depend on factors such as the desired storage capacity, release kinetics, stability, and safety considerations. It is an active area of research, and scientists are exploring various materials and formulations to develop efficient and practical ammonia storage systems."

---

"The amount of ammonia that each of these materials can adsorb or react with per kilogram (kg) can vary significantly depending on several factors, including the specific material, its surface area, pore size, temperature, pressure, and the concentration of ammonia in the environment. It's also worth noting that the adsorption or reaction capacity of these materials may not always be expressed as a fixed percentage by weight but rather in terms of adsorption capacity per unit weight (e.g., mg of ammonia adsorbed per gram of material).

Here are some approximate values for the adsorption or reaction capacities of a few of the materials mentioned earlier:

1. Zeolites: Zeolites can adsorb a significant amount of ammonia, often in the range of 5-15% or more by weight. However, the exact capacity can vary depending on the specific type of zeolite and the conditions.
2. Activated Carbon: Activated carbon can adsorb a wide range of gases, including ammonia. The adsorption capacity for ammonia can vary widely, but it's typically in the range of 5-10% or more by weight.
3. Metal Oxides: The adsorption or reaction capacity of metal oxides like zinc oxide can also vary depending on the specific material and conditions. Capacities are often expressed in terms of milligrams of ammonia adsorbed per gram of material (e.g., several hundred milligrams per gram).
4. Porous Coordination Polymers (Metal-Organic Frameworks): The adsorption capacity of MOFs for ammonia can vary significantly depending on the particular MOF structure. Some MOFs have been shown to adsorb substantial amounts of ammonia, with capacities reported in the range of 5-20% by weight.
5. Silica Gel: Silica gel can adsorb moisture and ammonia. The adsorption capacity for ammonia can vary but is generally lower than some other materials, often in the range of 2-5% by weight for ammonia.
6. Copper-based Materials: The capacity of copper-based materials to react with ammonia and form stable complexes can vary, but it's often expressed in terms of moles of ammonia reacted per mole of copper or another reactive site on the material.
7. Sulfuric Acid: Sulfuric acid can react with ammonia to form ammonium sulfate. The reaction capacity is typically expressed in terms of moles of ammonia reacted per mole of sulfuric acid.
8. Alumina: The adsorption capacity of alumina for ammonia can vary depending on the specific type and conditions. Capacities are often expressed in terms of milligrams of ammonia adsorbed per gram of material.

It's important to consult specific studies, manufacturer specifications, or conduct laboratory tests to determine the precise adsorption or reaction capacity of a material for ammonia in a given application, as these values can vary widely based on the factors mentioned above. Additionally, real-world performance may differ from idealized laboratory conditions."

---

Sorry for the super copy-paste project log, but I really want to make sure I show every information so you can see/point out where the chat made a mistake and/or if the presented information is actually concrete or not.

So, In order to get 6kg of hydrogen gas, you would need 30kg of ammonia borane.

And since you need boron nitride and ammonia gas, you would need around (accordingly to ChatGPT) 16kg of ammonia and 13kg of boron nitride. And in turn, you would need around 160kg of zeolite (if you assume the absorption is 10% per kg).

So, in total 6kg of hydrogen + 16kg of ammonia + 13kg of boron nitride + 160kg of zeolite + 3kg of oxygen + 6kg of iron powder = 204kg in total.

So, you would have around 980 wh/kg.

Well, again, the bottle neck here is the zeolite/adsorbtion material.

---

Well, the project log got so long it actually deleted the new text (that was actually a few exchanges with ChatGPT)

I wish I could explain little by little, but the new energy efficiency reached a 3333.33 wh/kg and a realistically number of 1400 to 1000wh/kg of energy density (maybe if you used Nafion as the membrane, the efficiency could be increased to 2000wh/kg, but this little piece of plastic is more expensive than gold).

You would need to have:

6kg of hydrogen + 16kg of ammonia + 13kg of boron nitride + 16kg of copper metal ammine compelex  + 3kg of oxygen + 6kg of iron powder = 60kg in total.

Of course, this is assuming nothing improperly reacts with other materials.

And if you actually were to have competent people taking a look at this, maybe you could reach an energy density comparable to fossil fuels (which are around 5400 wh/kg dense, since these can't reach pass 40% of efficiency in combustion engines).

---

By the way, a way of making copper metal ammine complex:

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Well, I got an answer, and it seems like everything ChatGPT told is just bullcrap:

https://chemistry.stackexchange.com/questions/175832/is-it-possible-to-make-a-reversible-solid-state-hydrogen-fuel-cell-using-ammon/175844#175844

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I found this blog from an actual chemist that was able to make a nafion-comparable DIY Ion exchange membrane:

https://chemisting.com/2022/12/15/nafion-equivalent-permselectivity-values-using-a-diy-pva-cellulose-cation-exchange-membrane/

https://chemisting.com/2023/06/03/an-improved-diy-cation-exchange-membrane-with-less-degradation-using-a-daramic-pe-microporous-separator-as-base/

And the better part is that it doesn't need to be in an alkaline fluid, meaning that I don't really need a Co2 scrubber neither to carry around caustic soda and caustic potassium in a bag. :)

(unfortunately, I can't find the goddamn daramic separator anywhere)