ars3n

And, so do many other transition metals and noble metals, starting from iron, cobalt, mercury, platinum, and so on.

Ditto the two postings above, although from my experience even when it's kept in a dry, well sealed container, it still slowly crumbles into calcium oxide over time.

LOl, that's very interesting indeed.

the falsk would boil off (provided that conc. H2O2 used) because MnO2 catalyse the decomposition of H2O2 to H2O and O2. The reaction also releases heat which further accelerates the reaction. At the end, you are left with MnO2 (no change to this guy as it is catalyst) and water.

A little bit confused about your question... 80%?, 90-95%? Are u talking about ether purity? I believe diethyl ether in the market almost always goes about 99+%. ACS grade usually about >99.8% with minuscule amount of stabilizing agent such as BHT. *** And, no people did NOT DRINK ether in the past. They use it via inhalation. There was time when ether was populary used as an anesthetic of choice. Today, in some parts of the world, where more novel anesthetic agents are unavailable, people sometimes still use diethyl ether.

Very likely it wont work.

Usually it's done to remove any dissolved gas (e.g. CO2) that might affect the pH.

I would doubt you would have to deal with HBr in this case. The greatest danger here is still Bromine and maybe H2O2 if someone foolish enough to use highly concentrtaed H2O2 for this purpose. However such mixture wouldnt give a good yield of Br2 beacuse a significant amount of O2 will also be generated.

Hmm I think oxidation of ammonia with oxygen is possible via catalyst.

First of all, why the heck would you even do this, start with aluminum, oxidize it with chlorine then reduce it back to aluminum, OMG... At any rate, electrolysis of AlCl3 has to be done at molten state (you CANNOT electrolyse aqueous AlCl3). AlCl3 is hard to melt without evaporating it at the same time, so you prolly need either to control the temperature acrefully, adding some flux, or doing it under pressure or a comination of those. On and alstly when you mix HCl (aq) with Al, even after evaporating it CAREFULLY, you'll still get AlCl3.xH2O and if you keep heating it up you'll end up with hydrolisi reaction so you get a mix of Al(OH)xCly.zH2O (still!). One way to make anhydrous AlCl3 is by reacting Al with DRY HCl.

Ditto above, H2O2 is pretty dangerous at high concentration. You can get easily get H2O2 at concentration of up to 50% (usually stabilized). 70% H2O2 is usually more troublesome to get as it doesnt have much laboratory use, unless you are making a rocket or smtg along that line.

That's why you should never work with open fire for this operation, have a very efficienct condenser to cool down the products and transfer them away from the main reactor (where you heat up H2SO4) or use it directly (e.g. for the case of alkene). At any rate, ether is cheap and easy to get, why bother doing this cumbersome method?

Essentially there are two methods of making KClO4 from KClO3. 1. Electrolysis of KClO3 soln.,(rather similar to the production of KClO3 from KOH). A small amount of KClO4 would form at the anode. 2. Careful thermal decomposition of KClO3. The yield is much better but the procedure is a bit risky. KClO3 must be pure FREE from organic material! KClO3 is then slowly heated until it almost liqufies and hold constant at about that temperature. 4 KClO3 -> 3 KClO4 + KCl When the temp. gets too high KClO3 will start to decompose into KCl and O2. CAUTION! Presence of organic material in the crucible or in KClO3 can cause explosion during heating.

Dehydration of alcohol to either alkyl-hydrogen sulfate or ether or alkene all come sdown to the reaction temperature as well as the amount of sulfuric acid. Provided you use conc. H2SO4, then the reaction is controlled by temperature. Below 80ish oC you would only get equlibrium mix. of alkyl hydrogen sulfate. When you increase the T to ca. 120ish oC, you will start distill of some ether and to actually get alkene, you need to go to as high as 180ish oC. Check my temperature again, too lazy to cross check them with the lit. =) Oh, also, it is better to add alcohol slowly throughout the process to sulfuric acid, esp. if you aim for ether and alkene.

More than 1000oC and has to be in inert atmosphere. BaO reverts to BaO2 requires heating to about 600oC (check the value again). When the temperature gets too high (ca. 800oC, I think), BaO2 reverts back to BaO.

How can you be sure that the solution is supersaturated? Even starting with solid Na-acetate, making supersaturated solution isnt that easy, all reagents have to be pure, dissolved at high temperature then slowly cooled down. no dust should get into the mixture, heck even, no disturbance (sometime shaking supersaturated solution a little innitiates the crystalization right away). So my guess, is that your solution is not supersaturated.