sixfold

That's a super interesting project. For anyone else, the project overview has some great system level diagrams:

https://github.com/opentraffic/otv2-platform

time for some kind of anonymizing location data sharing service, peer to peer or federated protocol? that might be interesting, or sketchy, not sure which.

Pretty sure you can download the maps ahead of time, GPS doesn't require data, then upload the fixes when you get home.

Go map keeps crashing for me, does it for you?

I've been using Go Map! but it keeps crashing... Maybe I'll try Streetcomplete if it's on apple.

Crawling and indexing lemmy inter-instance would be an incredible boon to discoverability on the platform.

Do it! it is easy to do at home! Just wear some gloves and safety glasses, those jars can easily shatter during the heating process if you use too hot of a heat source. I recommend a glass top electric stove, or put some kind of metal plate between your jar and the burner to help spread out the heat. Once you seal the jar, take it off the heat right away, so it doesn't build pressure. I boiled mine for a few minutes before sealing to try and get some of the devolved gasses out, and lightly set the lid on top to help the steam push out all the air.

It does. And Firefox is my default browser app.

Yes definitely. The pressure will drop along the vapor pressure curve all the way to the triple point, gently boiling all the way if you remove the heat from the vapor and not directly from the water.

Looks great! Nice work! What mount do you use?

Anything for posterity

Exactly. it was bottled at atmospheric pressure while it was boiling, so 1 atm and 100 degrees C. Check this graph to see the relationship between the water's temperature and it's pressure in the jar (since there is no air, only water vapor). If the vapor is condensed, then the pressure drops below the curve on the graph, that is, the pressure in the jar is lowered below the vapor pressure of the water. Any time the pressure is below the vapor pressure, the water will boil, releasing vapor, until the pressure is equal to the vapor pressure. The pressure does not become negative, it is still positive, just lower than the vapor pressure at the given temperature. You can get below the vapor pressure curve by changing the temperature too, which is what we usually do when boiling water at a pressure near 1 atm (760mmHg)

http://hyperphysics.phy-astr.gsu.edu/hbase/Kinetic/watvap.html#c2

(1 atmosphere is ~760mmHg)

a slight aside, there is an important difference between the total pressure of the air, and the partial pressure of water vapor in the air. Inside the jar, the two are equal, but in a dry location (not humid) the partial pressure of water vapor is usually less than the vapor pressure of water at that temperature, but since the total large pressure of the atmosphere would not allow a pocket/bubble of very low pressure water vapor to form inside the bulk water, the water cannot boil, but it will evaporate at the surface anyway until the partial pressure of water is equal to the vapor pressure (very humid).