No. Never. It takes whole teams of people to get it right. (Even then, they sometimes get it wrong.)

That’s a false dichotomy if I’ve ever heard one, dude.

No, just follow the money. It’s all going into marketing. Ban marketing (like the rest of the world!) and prices drop overnight.

There is exactly one easiest option: be like the rest of the civilized world and ban consumer marketing of medicine. HUGE amounts of the prices of drugs are just down to TV ads. “Ask your doctor about…” is horse shit, let your doctor decide what prescription drugs you need. And fire the cocaine-riddled, law-breaking marketing departments that soak up so much money.

“Our recipes are consistent, like a good espresso maker.”

“Okay cool, how do you know that?”

“So many questions! We’re hackers! We are very smart.”

That’s the thing. They have no way of even knowing if they messed up! I’m not even sure the way they could be messing up is a thing they know they should be worried about.

I’m not disputing the reasoning behind why this is important. But “it is important” does not imply that their solution is the right one.

People make illicit drugs chock full of impurities all the time too, and it fucks people up.

There are standards for purity on pharmaceuticals. Impurities have to be ridiculously low. Lower than you can measure in your garage.

These dudes either don’t know you need to even measure purity or have decided that it’s inconvenient and are ignoring it.

I’m a process chemist. I do this sort of thing for a living.

These guys don’t even know why what they’re suggesting is so dangerous. Do not do any of this.

I sort of feel bad about raining on the parade of the person distilling isopropanol in his garage earlier, but it really is dangerous.

But most of us chemists also need to be reminded of it. To the point that someone had to write a paper whose entire point is “don’t distill isopropanol”.

Please, don’t do this thing.

The issue with isopropanol peroxide formation is that exposing it to air – even when just using it, like when you’re cleaning parts – starts the process. The air in the head space of your containers is also enough to form them over time. You don’t necessarily need to see solids in the containers for it to be dangerous, since they’ll crystallize out as you concentrate the solution during distillation.

It’s also a numbers game. It probably won’t explode the first time you do it. But there’s a chance each time. Do it enough, and you’ll have an incident.

There are chemical reductants that can clear peroxides. For industrial scale isopropanol distillation, I’m not sure what they use. It may be that they just never distill down to the point that peroxides concentrate to a dangerous level.

I love EnF. But I assure you, organic peroxide formers are scarier.

No no no no no.

I’m a chemist. Organic chemistry PhD, now a process chemist in the industry. I do this for a living. Do not distill isopropanol that’s been exposed to air for any meaningful length of time.

Isopropanol slowly reacts with oxygen in the air to generate peroxides that, when you concentrate them down, EXPLODE. Source. Sorry, not an open access journal. But please take my word for it.

Unless you have a way of confirming the peroxide levels in your isopropanol are near zero, do not concentrate it down by distillation. You’ll blow up your glassware, which will probably expose what you’re distilling to your heat source, which will generate a secondary fireball.

PLEASE do not do this.

Admission: I stole it.

qntm’s cool science fiction stories are my favorite.

Worse: your sleeper ship arrives at what should be a pristine planet. But FTL capable ships beat you there. And they ruined the planet over a few thousand years. And now they’re sending out refugee ships of their own.

Drawbacks are mostly the economics of it. You have to convince people to put time and energy into turning waste into monomers. If the monomers you get from crude oil are cheaper, you’ve got an uphill battle.

The catalysts can be complex, but the good ones are really simple. The zinc one in this article is pretty easy to understand. Ours was an organic molecule, but a really abundant and cheap one. (We could easily recover and re-use the catalyst, too, which I also doubt most of the metal salt catalysts are capable of). Part of the project was optimizing that catalyst. We found ones that worked a little better, but were like 10x as expensive. So we just used a little more of the simple one and figured out how to use it over and over.

I worked on a similar (but competing) technology to this one for a few years. Depolymerization is absolutely the way forward for most polymer recycling.

For most uses, manufacturers want plastic that’s colorless and has good physical properties. Melting down clear plastic can work, but it degrades the polymers in hard-to-control ways. And if there’s any pigment in the plastic, forget about it.

If you break down polymers into their constituent monomers, you’ve turned a polymer process into a chemical process. Polymers are hard to work with. Chemicals are, comparatively, pretty easy. You can do a step or two to extract all the color and impurities, then re-polymerize the cleaned up material and get plastic that’s indistinguishable from brand new.

If your depoly process is good, it can distinguish between different polymers, so you can recycle mixed waste streams. Ours was even pretty good at distinguishing nylon from PET, which I sorta doubt the zinc process will be. But hey, more competition in this space is gonna be good for the world.

The small beings are being brought to the slender building of magic!

1. Hack together a proof of concept
2. Works well enough that management slaps a “done” sticker on it
3. Pile of hacks becomes load bearing
4. One or two dependencies change, the whole thing falls over
5. Set evenings and weekends on fire to fix it
6. Management brags about moving fast and breaking things, engineers quit and become cabbage farmers and woodworkers
7. New graduates are hired, GOTO 1