jdurg

No. The tube was in the open atmosphere, but it was heated to a fairly high temperature in order for the ampoule to get sealed. That is why I'm making the assumption that all the gas inside the tube is bromine vapor.

Okay. I think I figured it out. I just made an assumption that all the space in the tube not occupied by the liquid bromine was occupied by bromine vapor. I then was able to use the density of bromine vapor to calculate how much bromine was in the gaseous state. With that information I calculated the pressure at room temperature to be about 1.06 atmospheres. Not too bad. I then did the calculation at a temperature of 313.7 Kelvin and figured out that the pressure would rise to ~1.22 atmospheres. Again, that's not terribly high but it didn't take into acount that at the elevated temperature more bromine would be vaporized. However, I don't believe that the amount of extra bromine in a gaseous state would be all that much in terms of the overall pressure. I also remembered that as the pressure inside the tube increases, the amount of bromine that would be in the vapor state would decrease as well. The boiling point of the bromine is also elevated at a higher pressure since it's harder for the bromine molecules to separate from each other. So really, I have nothing to worry about unless I throw this ampoule in a fire. Especially since the ampoule was formed at an elevated temperature. (We had to melt the borosilicate glass in order to seal it, so the bromine was at a pretty high temperature while the glass melting was occurring.)

Hey guys. I'm hoping someone here can help me out. I've been looking at my halogens and have been paying close attention to my bromine ampoule. I did some calculations and figured out that if all of the bromine vaporized, the pressure in the tube would be 99 atmospheres. heh. It would go boom pretty violently. However, what I can't seem to figure out is how to calculate the pressure present inside a tube when there is still liquid present. I.E. at about 105 degrees Fahrenheit, what would the pressure inside the bromine ampoule be? (That would be about 313.7 K). The cylinder has a total volume of about 24.333 mL, and there is about 4.5 mL of liquid bromine inside the cylinder. The one thing I don't know is the total mass of the bromine that was added, so I really don't know what the pressure is inside the tube right now. Is there any way that a rough estimate could be made. Arrggh. It's late and I'm having a brain fart. lol

Here's digging up an old thread. I've been a smoker for about six years now, and it's a habit I wish I never picked up. I started smoking on a bet. My roommates in college were all smokers, and I was the only one who wasn't. So one day they bet me a six pack of REALLY good beer that I couldn't smoke a cigarette without coughing. I won the bet, but got hooked. I just loved the lightheadedness and the social aspect of it. Whenever I drank, I'd have a cigarette. I'd get out of a long lab and have a cigarette. Finish a meal; have a cigarette. Perhaps the most intense craving came after having sex. lol. Finish-up, clean up, light up. I've tried quitting dozens of times, but I just couldn't do it. Working with dozens of people who also smoke doesn't help things either. I smoked pot for a solid four years, and I was able to quit that easily without any withdrawal. But if I go one day without a cigarette, I feel ultra edgy and just "odd". It's definitely not something someone should EVER do.

Now as for why the craving seems to be stronger with alcohol consumption, I really don't know. I'm guessing it's more psychological than it is physical, but I honestly have no idea why.

Bismuth is really nice because the crystals it makes are so beautiful looking. Also, if you hold it near a pure white metal like silver, palladium, or rhodium, you can see a nice pink tinge to it which is a bit different. Indium is another fun one because it's about as soft as lithium or sodium, but it won't blow up in water or burn your hands. It also maintains its shine indefinitely. Having a collection of elements is neat, but it's also pretty expensive and requires a lot of responsibility. For instance, you CANNOT have your halogens anywhere near your alkali/alkaline-earth metals unless the halogens are completely sealed up in an ampoule. My chlorine, bromine, and iodine are now permanently sealed in borosilicate glass ampoules, so I can finally have them in the same area as my other metals. But there's still the risk that if they break, bad things can happen. That's also why you don't want too much of the really nasty ones. If there was a flood, there would be quite the BOOM coming out of my storage cabinet. That is also why I don't have a few ounces of each of the metals. lol. I also have them stored inside a cabinet and not out in the open so that sunlight won't cause any damage. It took a lot of planning, but the few thousand dollars I've spent has been well worth it. (And having quite a few good nights playing poker with my buddies and at casinos helped fund nearly all of it).

Take a look at this link here. It's a picture of my element collection that I took a while ago. Since then, a few of the samples have been upgraded. The Strontium, Bromine, Chlorine, Iodine, Iron, and a few others have all been upgraded. (The fluorine, technetium, and promethium are pictures I found online. I don't own those elements). But I have that periodic table up on the walls of my cubicle at work, and every single day I get people stopping by in awe of the elements. I have all my elements in labelled jars or ampoules and just like to admire them. My favorites are Osmium because of it's blue color and incredible density; Bromine because of the deep red-brown vapor it gives off and the fact that it's a liquid; Cesium because of its gold color and the fact that it liquifies if I hold the vial; Potassium because of the purple oxide color; Chlorine because of the green color of the gas; and Iodine because of the purple vapor and fun you can have with it. I got nearly all of my elements from E-Bay, or from a very good dealer named Dave Hamric. He has a website at www.elementsales.com where you can get almost everything.

I also have multiple allotropes of each element. I have large samples of graphite and diamond for carbon, and samples of Red, White, and Black Phosphorus. (You can get man-made diamonds fairly cheaply, and uncut diamonds for a steal as well).

to the element collectors!

 

what do you do with your elements? if you start blowing em up then you wouldnt have them anymore' date=' but if you just keep em on a shelf, whats the point?[/quote']

 

 

What's the point in having a coin collection if you are just going to keep them sealed away in books and never spend them? What's the point in having a toy collection if you're never going to play with them and you just keep them in their box? What's the point in having a comic book collection if you're never going to read them and never take them out of their sealed baggies? What's the point in collecting anything if you're never going to use them? Ya see, the point of collecting anything is because you like what you are collecting and you like being able to see them any time you feel like it. It's just something people do.

Well I do have uranium ore. I bought a pretty active piece while browsing E-Bay under the influence a few years ago. But I like having actual large samples of the pure elements. That's why I have to avoid many radioactives. If I had a large sample like I would like, I'd probably die. lol. The only radioactive element I have in a pure form is a small sample of tritium gas inside a key chain. I got that because I wanted some tritium to go with my protium and deuterium samples. But my favorite samples are my osmium pellet, bromine ampoule, chlorine ampoule, and iodine ampoule.

And the nitrogen triiodide you make will cause all the effort to be well worth it. NI3 is the whole reason why I got into chemistry, and it's the whole reason why I have a complete collection of the elements. (Minus fluorine and the radioactives). And they say you never learn things from watching tv. HA! (I found out about nitrogen triiodide by watching the movie 'The Manhattan Project'. It looked cool, and when my chem teacher said that I wasn't allowed to make it, it clinched the notion that I HAD to make it).

You don't even need a lit match. Just take a small piece of platinum and put it into the mixture and BOOM; catalysis city.

Actually, when making nitrogen triiodide it's a good thing to have some KI mixed in with the Iodine since that will allow it to dissolve in water a whole lot better, which will allow it to react with the ammonia a lot easier. Trust me on this. I've garnered much better yields of NI3 by having some iodide salts thrown into the mixture while it's reacting. The aqueous iodine is able to become more "intimate" with the ammonia thus resulting in a better reaction.

Every single electron shell exists for every single atom out there. Even Helium has a 9s shell. However, those shells just aren't in use. An electron "shell" isn't a physical object. It's a mathematic probability that an electron with a certain level of energy will exist in that area. This is where you get into the quantum mechanics junk that can make grown men cry. All of the noble gasses can be reduced, it just takes a good deal of energy to do that. Helium is virtually inert since the amount of energy required to either add an electron, or remove an electron from it and place it into a bond is obscenely high.

The problem with gallium is that you'll have to keep the cylinder somewhat warm so that it doesn't solidify on you, plus gallium will "wet" glass so once you shake it up you'll just have a cylindrical mirror. Mercury, though kind of toxic, would be the best thing to use.

Yeah, cesium is most definitely not a radioactive element. As has been mentioned numerous times, all elements below Bismuth on the periodic table have at least one stable isotope except Technetium and Promethium. The danger with cesium is that it's so incredibly reactive and has such a low melting point. As a result of the low melting point, it will liquify almost immediately which will increase its surface area thus allowing it to react even faster. Upon exposure to air, there's a good chance that it will catch fire due to its reaction with oxygen, nitrogen, and moisture in the air. Then you have to deal with the cleanup of any CsOH which is the strongest base known to man. That stuff will eat glass and make HF look like child's play. Now rubidium is kind of interesting because one of the naturally occuring isotopes of Rb that makes up a good percentage of all naturally occuring Rb is nice and radioactive. I have a small one gram ampoule of it and I left it next to some unexposed, sealed film to see what it could do, and the film has been nice and exposed by the radiation it took in over the past couple months.

I think you have that backwards. Hydrogen doesn't explode - it burns very fast.

 

Burning hydrogen uses 3 moles of reactants to produce 1 mole of products' date=' so the result is a 3:1 reduction in volume of gas. All expansion comes from the energy release, as opposed to products that go solid or liquid -> gas, that expand as a result.[/quote']

 

Actually, it's 3 moles of reactants producing 2 moles of products. So while it is a reduction in moles, it's not a 3:1 reduction. It's only a 3:2 reduction. But when you have the perfect mixture of hydrogen and oxygen, that reduction is a very loud reduction. hehe.