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paulll
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Good to know, ty.
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S.C. Wack
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My NaBr is slightly halogeny...perhaps from the original crystallization or reaction with the container at some point. Our noses are very sensitive
analytical instruments sometimes...e.g. a super low concentration of IPA smells pleasant and is unrecognizable as such.
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j_sum1
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Hypotherical hydrogen cyanide synthesis
I just composed a problem for my students – calculation of enthalpy of reaction from tables of average bond energies.
Seemed like an ok example of the concept. But is there a feasible reaction schema that produces HCN from ammonia and carbon monoxide?
Just curious.
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DraconicAcid
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I don't think so, but that's a good example.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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njl
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Carbon monoxide is a better reducing agent than it is an oxidizing agent, and ammonia needs to be oxidized to give cyanide.
Reflux condenser?? I barely know her!
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j_sum1
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Quote: Originally posted by njl  | | Carbon monoxide is a better reducing agent than it is an oxidizing agent, and ammonia needs to be oxidized to give cyanide. |
Should have thought of that.
(Shhh. I won't tell the students. It will ruin the illustration.)
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paulll
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Too late to offer bonus marks for balancing the equation?
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j_sum1
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It is an exercise to introduce a concept and not an assessment. So, no marks. What is required is clarity, and a situation that is non-trivial to
give purpose to the exercise and so that the required concepts are repeated a few times. This meets those criteria.
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scienceboi
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Question
Can metals become plasmas? And how easy or useful is it to make them plasma?
I was just looking up sputter deposition for silicon wafers and it got me thinking.
"Read not to contradict and confute; nor to believe and take for granted; nor to find talk and discourse; but to weigh and consider." -Francis Bacon
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Hoffit
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Applied science has some nice videos about sputtering like this one https://www.youtube.com/watch?v=9OEz_e9C4KM
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pneumatician
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What is the ideal acid nitric concentration for dissolving Iron? 30%? 20%? 10%?...
Pure of around 99,9x% and "normal" Iron filing?
[Edited on 30-5-2021 by pneumatician]
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Fulmen
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I would say it depends on what you're after. If it's reaction speed it would probably be strong acid, but that tends to produce lots of NO and NO2.
For a clean reaction with little loss I would keep the concentration below 20%.
We're not banging rocks together here. We know how to put a man back together.
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B(a)P
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Concentrated nitric acid will passivate iron.
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clearly_not_atara
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| Quote: Originally posted by j_sum1 | I just composed a problem for my students – calculation of enthalpy of reaction from tables of average bond energies.
Seemed like an ok example of the concept. But is there a feasible reaction schema that produces HCN from ammonia and carbon monoxide?
|
If you factor entropy into your calculations I'm betting you'll find that delta-G is always positive for the forward reaction (forbidden). But IIRC
you can do it in two steps, by making formamide first and using a selective catalyst second.
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pneumatician
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what is the Pepy's apparatus???
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Belowzero
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Will acrylate or plexiglass resist ~30% nitric acid for long periods of time at room temperature?
Or PVC?
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CharlieA
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https://en.wikipedia.org/wiki/William_Haseldine_Pepys
May be this will help? You didn't mention in what activity the apparatus might be used in.
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njl
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Carboxylic acids can be activated by formation of mixed anhydrides. Could the acid instead be reacted with isocyanate to yield a carbamate (mixed
carbamate anhydride)?
Reflux condenser?? I barely know her!
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pneumatician
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someine use one of this? ocerall qlty?? leaks in joint???
https://www.ebay.de/itm/152510588408?ssPageName=STRK%3AMEBID...
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pneumatician
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near 0 info in archive and gbooks! :-?
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SHADYCHASE54
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Hello fellow S.M'ers,
I am wondering if I were to make hypophosphorus acid with it's Na salt and 32% HCl; then flash distill the resulting solution under strong vacuum to
remove H2O, precipitate most of the NaCl while keeping the acid's boiling point below its d-comp. What would be, after diluting the acid to 10-15
percent of course, the most suitable exchange resin(s') to remove the Na and Cl impurities? Would reacting the diluted solution first with H+ strong
acid cation exchange resin convert the remaining NaCl to HCl? Furthermore I am wondering if I were then to react the resulting solution with a strong
anion exchange resin in the Cl- form would this remove the Cl from the HCl impurity thus liberating the hydrogen (g)?
I have no idea if this would work past making the acid solution. Anyone with experience or knowledge with or about exchange resins, who is willing to
point me in the right direction, I would really appreciate it.
2 side notes: 1 yes I am aware of the danger of this acid's decomp. products. 2 the hypo is not for any illicit use, truthfully I haven't even decided
what I intend to reduce yet? As the real experiment is in reaction conditions and comparing those to similar reducing agents. I am also interested in
comparing it's reducing capacity under various reaction conditions. Such as simple reflux, microwave irradiation and under pressure. (In an actual
pressure bomb). There I'm done.
Any help would be appreciated.
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Sulaiman
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TCCA + EtOH = Chloroform?
I have performed the classic acetone + hypochlorite haloform reaction a couple of times,
I would like to try TCCA instead of hypochlorite,
will it make much difference if I use EtOH (85% or more) instead of acetone.
(I have lots of (pool grade, 90%)TCCA and diy EtOH)
CAUTION : Hobby Chemist, not Professional or even Amateur
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BauArf56
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is it possible to isolate any chlorinated compound by burning propane in chlorine?
Once i wanted to see how does propane (or butane) burn in chlorine gas, so i lighted up the blowtorch inside a bottle filled with chlorine. It burned
with a bigger flame and it was quite luminous too. After a few seconds of burning inside the bottle there was no smell of chlorine at all, just the
typical sweet smell of chlorinated compounds. Can anyone explain which compounds form and if is it possible to isolate them as liquids? Thanks
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macckone
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I have not bought that particular one, but they are commonly used in labs. For large quantities they have significant advantages in filling and
cleaning. The top portion generally uses a standard 100mm opening, you can buy various sealing rings but the ground glass joints should meet as well
as a standard vacuum desiccator.
You can buy various tops for the flask:
https://www.ebay.com/sch/i.html?_from=R40&_trksid=p23220...
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macckone
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| Quote: Originally posted by Sulaiman | I have performed the classic acetone + hypochlorite haloform reaction a couple of times,
I would like to try TCCA instead of hypochlorite,
will it make much difference if I use EtOH (85% or more) instead of acetone.
(I have lots of (pool grade, 90%)TCCA and diy EtOH) |
TCCA will not work by itself. You will have to add a soluble hydroxide base. And you will need extra as the cyanuric acid will need to be
neutralized to form the final product.
There is actually a thread on TCCA.
http://www.sciencemadness.org/talk/viewthread.php?tid=5686
Ethanol will work, It has an alpha carbon.
Ethanol was used in the first haloform reaction.
Since you normally add water in the form of bleach or to dissolve the calcium hypochlorite, the water content won't matter much.
However, ethanol and chloroform give an azetrope so you need to be sure your ethanol totally reacts. Acetone has a similar issue with separation.
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