Turning Fruits Into Ethylene And Ethane Refrigerant

August 2, 2026 by Maya Posch 5 Comments

One of the best parts about DIY chemistry and physics projects is that you get to decide how early in the supply chain you want to begin, such as with [Hyperspace Pirate]’s adventures in ethanol production from sugar fermentation. Although you can certainly just buy packs of sugar and yeast from the store and pretend that this will be helpful once the world embraces its Mad Max era, you may as well start with the stuff that actually grows on trees, like fruit.

While you could use the ethanol produced this way as ethanol fuel in combustion engines and the like, you can also turn the ethanol into ethylene and ethane. That way you can fill up your refrigerator, freezer, and air conditioner to keep your perishable foods and yourself fresh as the outside world descends into highly questionable fashion choices.

Even outside such a scenario it makes sense to generate your own ethane and ethylene, due to how much these refrigerants cost. Once you have the ethanol, some aluminium oxide catalyst at 350°C is enough to produce ethylene and water. Producing ethane is admittedly a bit more involved, requiring acetobacter bacteria to produce acetic acid, along with baking soda, a platinum anode and a few more odds and ends.

Producing butene and even longer chains from ethylene is also possible as a next step, but this gets even hairier than producing ethane from ethanol, so we’re likely to see this in a future update after all the low-hanging fruit has been harvested.

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How To Rebuild An 1800s Victorian Leclanché Cell

July 6, 2026 by Maya Posch 20 Comments

The 19th century was an absolutely electrifying era, including in a literal sense. Although the phenomenon of electricity had been known by that time for centuries, actually making it do useful work was a much taller order. Aside from big, coal-powered generators, there also was a need for a more compact electrochemical solution, such as in the form of a wet or dry cell. One of the first major commercial successes here came in the form of the Leclanché cell, such as the genuine version that [Big Clive] found in an old UK building’s attic and has now revived.

Invented in 1866 by French scientist Georges Leclanché, the Leclanché cell features an ammonium chloride electrolyte solution, carbon cathode and zinc anode. There’s also a manganese dioxide depolarizer for preventing hydrogen build-up. Here water is the solvent for the ammonium chloride (also known as sal ammoniac).

The version that [Clive] got his grubby mitts on features a glass container, an already partially consumed zinc electrode and a slightly cracked porous ceramic tub that contains the carbon electrode and the manganese dioxide. After placing the components inside the specially shaped glass jar and filling it with an electrolyte mixture of one part ammonium chloride and four parts water by weight, the cell starts generating its approximate 1.4 VDC.

This type of wet cell was very popular, being essentially ‘rechargeable’ by topping up the water and replacing the zinc electrode consumable. They did suffer from a voltage drop-off during use due to increasing internal resistance, something that got improved upon with the zinc-carbon dry cell. Itself effectively an evolution of the Leclanché wet cell.

From there zinc-carbon dry cells got replaced with alkalines, which itself got mostly replaced by NiMH and Li-ion cells. Despite more than a hundred years between the electrochemical cell that [Clive] featured in his video and today’s batteries, it’s clear that this wet cell was quite literally just the Victorian-era equivalent of an alkaline AA cell.

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Microdistillery For Microchemistry

July 3, 2026 by Bryan Cockfield 21 Comments

Much like radio operators being encouraged to use the least possible amount of power to make a contact, chemists have a similar rule encouraging using the least amount of materials in experiments. Not only is this rooted in economics, but in safety as well; if something goes wrong it’s generally good if there’s not excess amounts of reactants. With modern techniques, though, it’s possible to bring experimental chemistry down to incredibly small scales, and [Marb’s lab] found that they needed a custom built still for these new, diminutive experiments.

The first step is to build the heating component of the still. This is provided with a few custom aluminum parts for the base and a pair of heaters originally meant for 3D printers, with the assembled unit wrapped in insulation. The heater accomodates a 25 mL round-bottom flask. Temperature control of the heating mantle is provided by a controller mounted to a DIN rail which receives power from a 24V power supply, and an additional temperature probe is added to measure the temperature of the distillate. A test run with water shows the small still quickly and efficiently evaporating the water up to a condenser.

Although building a still doesn’t have to be technically difficult, building something this small that’s effective and safe is a bit more challenging than a backyard moonshining operation. Scaling chemical reactions down can often be a challenge but is possible with the right mindset and equipment. We’ve seen miniaturization of many things that we might not have expected including hydrogen production, aluminum smelting, and even the construction of a microscope.

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Solid-State Batteries Take To The Sky

June 17, 2026 by Bryan Cockfield 13 Comments

There always seem to be a handful of revolutionary technologies perpetually out of reach: fusion energy, quantum computers, and full self-driving cars are always in this list, and it seems like there’s also some battery technology which will finally let us fully decouple from fossil fuels in there as well. Although lithium batteries have allowed some ground-based electric transportation, the energy density is still not enough to enable full electrification, especially for things like aircraft. Solid state batteries may be on the verge of changing some of this, though, and a team has recently put them to work in a test aircraft to help make some headway with this novel battery chemistry.

The main contributing factor of these batteries’ improved energy densities is the ability to use a solid lithium anode, which has much higher energy density than the graphite-based anodes in modern liquid electrolyte batteries. Solid state batteries also have improved safety, since the solid electrolyte is generally not flammable and the battery itself is less prone to thermal runaway. The tests in this aircraft, a modified motorized glider, bear this out as well. With a standard lithium ion pack the team was able to harness 250 Wh/kg and with their new solid state battery they managed 410 Wh/kg, which let them fly the craft up to 24,000 feet (7,315 m) with the help of some wing-mounted solar panels.

Of course, a motorized glider is a long way away from battery-powered commercial flights, but tests like this are an important step on the way to de-carbonizing one of the more impactful industries on the planet, as well as hopefully making it less expensive to operate aircraft in the way EVs are generally much cheaper to operate than their internal combustion equivalents. But the limiting factor to adopting solid state batteries isn’t going to be implementation but rather the discovery of a cost effective way to manufacture them at scale. It’s the same reason we haven’t seen mass adoption of things like algae-based biodiesel or economic carbon capture yet.

Building An Organic Flow Battery Based On Green Tea

June 17, 2026 by Maya Posch 9 Comments

As simple of a concept flow batteries are, the used chemicals can still be somewhat problematic in the context of a school experiment. To this end [Markus Bindhammer] decided to implement a flow battery version that uses compounds from green tea for its electrolyte, based on a German research paper from 2016.

These organic flow batteries can use gallic acid, pyrogallol as well as the polyphenols in green tea, making them rather safe even in the hands of more careless students. The demonstrated flow battery uses a carbon electrode with activated carbon around it to increase surface area, a platinum wire electrode, and a graphite foil as third electrode.

In the paper a silver electrode is also used, along with the additional electrodes, and a terracotta flower pot as the barrier between the carbon and graphite electrodes, with [Markus] further explaining that there are fortunately cheaper options than what he is using, especially with the flower pot instead of a special ceramic vessel.

The electrolyte solution has epigallocatechin gallate (EGCG) dissolved in it, which here comes in the form of finely ground green tea powder (commonly known as matcha), which so happens to be pretty rich in this substance. In the below graphic by [Markus] you can see the complete set of solutions and other relevant details.

Of course, the performance of this type of flow cell isn’t amazing, with a cell voltage of less than a volt and a few mA of current, but it’s enough to spin a small fan, and to light up a few LEDs. This would be more than enough to demonstrate the reaction and flow cells in general, as long as you don’t mind donating some tasty matcha to science.

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The Problem Of Making A Good Metal-To-Glass Seal

June 16, 2026 by Jenny List 22 Comments

If you’ve ever taken a close look at a vacuum tube, you’ll have seen the seals around the pins that keep everything air-tight while providing the the device’s electrical contacts. As [maurycyz] finds out, it’s not an easy process to get right.

The problem is one of both chemistry and thermal expansion, as while a good seal can be made between glass and red copper oxide, it remains very difficult indeed to stop the glass cracking on cooldown due to differing thermal expansion properties. We’re led through a variety of experiments including surface treatments and flattening the metal to a sheet, with varying pros and cons. The most successful seal on the page comes from very thin tungsten wire, though hardly the most practical conductor for a vacuum tube.

It’s a fascinating investigation for the casual reader, taking them into the properties of metal-glass bonds and the difficulties involved in making them. We have even more respect for the people who make their own tubes after reading it.

A boiling flask is mounted in a heating manted, with a tube leading from it to a U-shaped tube. From here, the tube continues to a bottle of yellow fluid, from which another tube emerges. A flame is emitted from this last tube.

Building A Desktop Catalytic Cracker

June 11, 2026 by Aaron Beckendorf 7 Comments

Although crude oil contains a vast diversity of hydrocarbons, a comparatively small number of these make up the bulk of demand for oil. Cracking solves this mismatch: most of the demand is for light, short-carbon-chain molecules, so a cracker breaks down long-chain hydrocarbons into lighter, more commercially-valuable chemicals. This is usually done in massive industrial plants, but as [Markus Bindhammer] showed, it’s possible even in a tabletop apparatus.

There are several methods of cracking, but [Markus] used catalytic fluid cracking: a feedstock high in alkanes (hydrocarbons containing fully saturated carbon-carbon bonds) is heated in the presence of a catalyst, whereupon its long alkane chains split to form alkenes (hydrocarbons with a carbon-carbon double bond) with the loss of a hydrogen molecule. In [Markus]’s setup, a heating mantle heated a boiling flask containing paraffin oil and an amorphous silica-alumina catalyst. Vapors from this flask passed through a condenser tube and a bottle of bromine water, then escaped through a flashback arrestor. Bromine reacts far more readily with alkenes than with alkanes, so the disappearance of its characteristic yellow color would visually indicate the production of alkenes.

To avoid unwanted oxidation, [Markus] purged the cracker with argon before using it. While running the cracker, a flammable mixture of light hydrocarbons and hydrogen escaped from the flask of bromine water. The yellow color of bromine disappeared, and two phases formed: one aqueous, and a lighter phase of hydrocarbons and brominated hydrocarbons. The hot side of the reactor did not survive well; the catalyst turned black with coke, and the heating mantel’s cover fused to the boiling flask. However, the reaction undoubtedly succeeded: while a pool of normal paraffin oil wouldn’t ignite, the cracked oil lit easily.

To go the other way, from small molecules to larger hydrocarbon chains, [Markus] has also used the Fischer-Tropsch process.

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