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.

"And, no people did NOT DRINK ether in the past."

Sure about that?

http://www.worldwidewords.org/weirdwords/ww-eth1.htm

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.

Does anybody know where an individual can buy diethyl ether (60-29-7), in quantities that are reasonably unlarge (not more than $50)?

 

I know about how most vendors will only ship it out to "educational institutions" and businesses, but if you can but 80% ether as starting fluid, it seems ridiculous that nowhere is there any 90% or 95 or... you get the idea!

 

Thanks for helping!

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.

Mixing NaBr, H2O2 and H2SO4 is one of the dumbest things you could ever do, and most scientists are quite smart enough to know that you should never do that. NEVER mix hydrogen peroxide and sulfuric acid. When you do that, you will lose a good deal of bromine in the form of HBr gas which will bubble out, and the extremely high temperature of the reaction vessel will cause any bromine you have to instantly vaporize away. In addition, the sulfuric acid will form a very nasty and dangerous compound with the hydrogen peroxide, and may itself be reduced into choking, toxic sulfur oxides. There is absolutely no benefit in producing elemental bromine in that manner. In fact, if you try it that way you'll most likely wind up wasting a lot of time, money, and your health.

 

A better method of producing bromine is to oxidize the bromide ion via chlorine gas production. In fact, one trip to a pool supply store will get you everything you need. You can either generate the chlorine gas separately, or you can just generate it in-situ which is probably the easier thing to do. Just get some powdered super shock (Caldium hypochlorite), sodium bromide tablets, and hydrochloric (muriatic) acid. Mix the hypochlorite and sodium bromide in some water so that everything will be nicely dissolved. Then slowly add the hydrochloric acid. You will notice that the solution will start turning a reddish color as free bromine is liberated. You want to add the HCl slowly so that the solution doesn't overheat and you don't generate too much chlorine gas at one time. You will also want to have an excess of acid so that the bromine will remain as the free element. Then all you have to do is cool off the solution and suck out the bromine from the bottom of the beaker with a pipette. Just make absolutely sure you do this outside.

you`d need to "Inject" some energy into the system to make this work!

 

Electrolysis would likely give you A yield of these products, certainly, and you wouldn`t need to use the O2 either.

 

 

 

if it were Singlet Oxygen yes perhaps, or even Ozone, but not O2.

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?

Ah-hah! Well that also means I purified the sulphuric acid, sort of.

 

Well, what are other dehydrating agents for ethanol? All the sources I've seen say that there are others, but they won't tell me which. Any searches I do for that sort of thing returns all sorts of funky patents, but nothing useful!

 

 

 

If you are heating it over 120C, what keeps the ether from exploding?

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.