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plante1999
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Does anyone have a book that details the classic chemistry experiments/demonstration such as coal distillation, lead chamber demo, etc?
I have look for a book about theses early 1900 experiments for a while now.
Thanks
I never asked for this.
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DraconicAcid
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I have a book that does destructive distillation of coal and wood, IIRC, but it doesn't have anything about the lead chamber process.
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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elementcollector1
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Seems like most of them are organic sugars and such. Thanks!
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plante1999
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Quote: Originally posted by DraconicAcid  | | I have a book that does destructive distillation of coal and wood, IIRC, but it doesn't have anything about the lead chamber process.
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It was just to give an idea of the type of book I was talking, it is not obligated to have the three.
Thanks
I never asked for this.
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DraconicAcid
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I have "New Laboratory Experiments in Practical Chemistry" by Newton, Henry, and Black (1949), which has the destructive distillation of coal (but not
of wood).
I also have "Elements of Chemistry" by Shepard (1885), which includes an experiment where the student makes a solution of prussic acid, and feeds a
teaspoon of it to a cat.
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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plante1999
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"(...)which includes an experiment where the student makes a solution of prussic acid, and feeds a teaspoon of it to a cat"
Look exactly like what I want.
Thanks!
I never asked for this.
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confused
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Question
Hi, i was wondering if this platinum electrode could be used for the eletrolysis of copper sulfate solution into sulfuric acid
2 Cu2SO4 + 2 H2O = 4 Cu + 2 H2SO4 + O2
http://www.aliexpress.com/item/1-0-micron-50x50mm-Platinum-C...
would the platinum coating be too thin? 1 micron seems really thin for an electrode.
Also, how thin can the coating be before it is no longer practically usable for this application?
would a 0.5 micron thick coating work, as the prices for the diffrent thicknesses of coating differ somewhat substantialy
0.5 micron, 1.0 micron and 2.5 micron
Price is USD 18, USD 33 and USD 83
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Metacelsus
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I hope this question qualifies as "short":
I am studying the kinetics of a certain reaction in which a two starting materials react to form an isolable intermediate, which then reacts with
another equivalent of one of the original starting materials to form the final product. Both of the reactions are second order. In my case the first
reaction happens significantly faster than the second one, but not so fast that it can be assumed to always be at equilibrium.
1) A + B -> C
2) A + C -> D
I have written these differential equations to describe the system:
d[A]/dt=-k1[A][B]-k2[A][C]
d[B]/dt=-k1[A][B]
d[C]/dt=k1[A][B]-k2[A][C]
d[D]/dt=k2[A][C]
I assumed this type of reaction was a common one, but have not been able to find the general solution, or even a simplified form, of this type of
system. (Experimentally, both [A] and [B] decrease with time, [C] increases and then decreases, and [D] increases.) Does anyone here have experience
and/or knowledge with this type of reaction?
If it matters, I can tell you what compounds A, B, C, and D are.
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DubaiAmateurRocketry
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I wanted to repeat a nitration process a paper stated, they used HCl/HNO3/Ac2O, however I have only pure HNO3 and P2O5.
I also dont have sulfuric acid. Can I do HNO3/ P2O5 ?
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confused
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what exectly do you want to nitrate?
also, do you have the paper u mentioned?
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Galinstan
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No, HNO3 and P2O5 in ether will not nitrate anything as it won't create the nitronium ion ( the nitrating specie in most cases)
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DubaiAmateurRocketry
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Thanks for both of you answering,
I have > 95% HNO3 and so adding more P2O5 to take water out, will generate Nitronium Nitrate, NO2 NO3, a good nitration performer,
The nitration I wanted to perform on is a triazole compound, I fear the P2O5/HNO3 will be too powerful and the N2O5 generated might cause ring opening
and destroy my experiment, something N2O5 can do.
I've only half a liter of HNO3 left and I dont want to waste one gram of it 
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Galinstan
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Ah i stand corrected i din't realise P4O10 had the power to dehydtate HNO3.
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DubaiAmateurRocketry
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whats the most common material that can stand cold temperature, sulfuric acid, and nitric acid at same time?
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elementcollector1
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Glass.
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Zyklon-A
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Very true.
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DubaiAmateurRocketry
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anything other than glass ?
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bismuthate
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I'm not sure, but how about porcelain? Or do you have anything Si plated?
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Zyklon-A
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Gold.
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bismuthate
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He (or she) said common. Also would that etch gold like aqua regia?
Maybe PTFE.
[Edited on 22-12-2013 by bismuthate]
[Edited on 22-12-2013 by bismuthate]
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plante1999
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iron
I never asked for this.
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elementcollector1
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Uh, no? Iron wouldn't hold up to that. At least not the sulfuric acid.
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plante1999
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I bet anything you want, iron WILL hold that.
Seriously, industrial nitrator are made of iron...
It passivate.
I never asked for this.
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DubaiAmateurRocketry
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Yup, i was thinking on the same line.
Alright ahha, ill try that in small ammounts and tell u the results
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Mailinmypocket
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I just aquired a bottle of "animal bone charcoal", can this be used as decolorising charcoal? Not sure what it's purpose is otherwise besides being
incredibly messy
[Edited on 22-12-2013 by Mailinmypocket]
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