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About Justonium

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  • Location
    Roswell, Georgia
  • Interests
    experiments in chemistry and electromagnetism
  • Favorite Area of Science
    Inorganic Chemistry
  • Biography
    I dunno, I like chemistry and physics, and I've re-invented several things patented years ago. I do a lot of electrochemistry, and also have a lot of experience with: hydrochloric acid, sodium hydroxide, hydrogen, and magnesium.
  • Occupation
    Junior in High School
  1. For one thing, potassium sulfate is pretty soluble in water so your procedure would not work. As for the stability of copper chlorate, I believe it should be stable at room temperature, but I've never read anything about that compound in particular so I guess anything is possible. If you were to try to make it via a precipitation reaction, you would need to find out how soluble copper chlorate is, and then work from there to create a situation in which when a chlorate solution and a copper solution mix, the copper chlorate's solubility differs significantly from that of the other salt, so that
  2. I believe it's silver chloride. I have a little experience in photography, and I remember hearing silver chloride mentioned. Silver chloride slowly, very slowly, decomposes when exposed to light, ultraviolet in particular, into chlorine gas as well as silver metal that is seen as black/dark gray because its crystals are so small. I once made some rudimentary photosensitive paper myself, and all I did was coat ordinary printer paper with silver chloride. It worked brilliantly, although it did require a lengthy exposure time to pick up a good image. EDIT: Cripes, this thread is old!
  3. I'm not sure how to intergrate that; when I try 'u' substitution, representing the (x^2) as 'u', I can't get the 'du' in there: du = (d/dx)u = (d/dx)(x^2) = 2xdx There is no 'x' term in the expression, however, so that is where I get stuck.
  4. I made a little over gram of relatively pure sodium by lighting a mixture of powdered sodium hydroxide and powdered magnesium in a well cooled crucible with poor ventilation. I also ended up ruining the crucible with this method, as the extreme temperature changes that it was subjected to caused it to crack apart. Not a safe experiment to do at home, but I'm just pointing out that it's completely possible for sodium to be synthesized at home. I will not give the equation or the formula for this reaction, lest I encourage people who think they have enough experience to perform this. This is VE
  5. All of the responses in the main post seemed to me to be completely focused around the question: "How does this affect me?" This seemed to me to be looking for selfish excuses to do the right thing (not that that's a bad idea). But the way I see it, there's no greater importance of one person's happiness over any other person's, and so one of the motivators for me to help others is to remember that self is just an illusion, and that really, everything is all about just benefiting everybody's existences as much as possible, without regard to who it is, as long as the most people possible are be
  6. To help it dry faster, you can put it in a sealed bag along with some calcium chloride pellets (in another container) which can be bought from Home Depot for absorbing moisture from inside kitchen cabinets. This works best if you added close to equimolar proportions of ammonia and hydrochloric acid, but might be more difficult if you added too much ammonia. What i would do would be to add hydrochloric acid again after I passed the equivalence point, so that there is excess acid, and then dry it using solid sodium hydroxide as a dessicant. This stuff is horrible to get on you're skin though, so
  7. Sodium metal is very useful for making sodium amide, which can then be used to make azides. Lead azide is one of the most practical primary explosives. Also, the reason people love throwing sodium metal into water so much is because it's fascinating that something will actually react with water, which is normally considered somewhat inert, so vigorously that it explodes. =) When I thew a bunch of sodium beads into water on my driveway, i got lots of cheers from my audience lol.
  8. I'm still watching for responses. (Just clarifying that this thread is not old.)
  9. It's the electrode. It's getting oxidized instead of the chloride ions in the solution. To oxidize these, you will need a non reactive electrode. Try graphite. Also, as you're cell runs, chlorine production will soon stop, as the solution becomes more basic. You will then be making hypochlorite ions instead. To prevent this, you need to separate the solutions by the anode and by the cathode. You can complete the circuit easily enough with a salt bridge--a sliced hotdog or a cloth soaked in electrolyte will work OK.
  10. No, I'm afraid that wouldn't work lol.
  11. I suppose I should have been more descriptive. The cathode would sit in cupric nitrate solution, and the silver would hang in sodium nitrate solution. The solutions would be connected by a salt bridge also containing sodium nitrate. As the cell runs, sodium ions in the anode solution should be replaced by silver ions, and the copper ions in the cathode solution should be replaced by sodium ions as they plate out. The reason I would use copper nitrate is that I don't want hydrogen to get reduced, lest a small amount of hydroxide ions find their way through the salt bridge and coat the silver an
  12. OK, instead of using hot nitric acid to dissolve old fine silver jewelry, would it work to just hang the cleaned jewelry in a solution of copper nitrate and use it as an anode? The copper would plate out on the cathode, and the silver would go into solution, right? What I'm worried about is that an oxide layer might coat the silver and stop the process. Is this method feasable, or do I need pure nitric acid? Mine's contaminated with hydrochloric that I'm too lazy to remove.
  13. The regenerator should be as small as possible to maximize efficiency, but you will have to compromise size with functionality. Personally, I never bothered to make one, I never needed efficiency in my Stirling engine; I was only making it rotate a CD and look nice on my shelf, not perform a task.
  14. The higher the temperature difference, the higher the efficiency, I'd say. The only limit to this trend is that you start losing a lot of efficiency if its so hot that the heat leaks out, but in a simple home made Stirling engine, you should not have to worry about that kind of limit. You just don't want to have so much heat that part of you're engine melts. I've made one before, and 2 cylinders of the same size works fine, the real deciding factor is the cycle you design for you're pistons. I use a sinusoidal cycle in which the hot side is one fourth of a period ahead of the cold side, just b
  15. The user NurdRage has a pretty good video on the procedure you are trying, UC.
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