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Author: Subject: Cesium production from new method
ChemichaelRXN
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[*] posted on 5-1-2023 at 16:06
Cesium production from new method


Experimental method I discovered.

The boiling point of the following:
670.8C Cesium BP
315C FeCl3 BP

ok the method:

Fe + 3CsCl = FeCl3 + 3Cs

The iron (iii) chloride will sublimate/ distill over first and under this argon atmosphere, the cesium comes over unoxidized next at 670.8C to be collected and ampuled. There can be a copper powder separation to react the iron(iii) chloride possibly and the cesium appropriately collected....interesting experiment anyway...

I am going to be conducting this one and any input, let me know. This one should be pretty interesting.


Mike



[Edited on 6-1-2023 by ChemichaelRXN]




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[*] posted on 5-1-2023 at 17:20


I don't think there's any chance that iron will reduce cesium ions, or that cesium metal would not react vigorously with iron(III) chloride.



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ChemichaelRXN
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[*] posted on 5-1-2023 at 17:29


it is an experiment, but I was thinking they may separate early due to low boiling point of FeCl3 and leave behind the cesium if this works to then be distilled. I know that lithium is used with CsCl to form LiCl and Cs to collect...maybe this way works and I have to test it. There may be a lot of initial heat required then complicating things...

any other data to know?

[Edited on 6-1-2023 by ChemichaelRXN]




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[*] posted on 5-1-2023 at 17:59


I'm certain that you could heat a mixture of CsCl and iron filings until the latter melts and you still wouldn't see any reaction. Unless the CsCl itself boils, of course.

Reductions of alkali metals with divalent metals only work because the alkali oxides are not very stable compounds, since the lattice has to accommodate two positive ions for each negative ion, while the MgO lattice is "balanced". But alkali metal halides are balanced and hence very stable, so no reaction occurs.




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[*] posted on 5-1-2023 at 18:14


Have you checked the thermodynamics of your scheme? I would be very surprised if iron could reduce caesium at the temperatures you suggest. That said, you have come up with a scheme that would push the equilibrium in the right direction.
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[*] posted on 6-1-2023 at 07:02


You don’t get to claim discovery of a new experimental method if you haven’t even tried it yet (in other words, this belongs firmly in Beginnings).



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Texium
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[*] posted on 6-1-2023 at 07:47


Quote: Originally posted by ChemichaelRXN  

any other data to know?
[Edited on 6-1-2023 by ChemichaelRXN]

Code:
ΔH 909.6727 kJ/mol ΔS 86.1067 J mol/K temp 293.15 Kelvin  20 Celsius  ΔG = ΔH - TΔS ΔG 884.43 kJ/mol ΔG=0   T= 10564.48 K 10291.33 C




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ChemichaelRXN
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[*] posted on 6-1-2023 at 09:23


well the Delta G is negative...it would work with some heat and hopefully atomized.

I was thinking this because is you add iron wool to sodium chloride, then a single displacement reaction occurs, but in a solution.

At minimum you can make sodium metal this way, in the method I described ;)

[Edited on 6-1-2023 by ChemichaelRXN]




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[*] posted on 6-1-2023 at 14:16


Quote: Originally posted by Texium  
You don’t get to claim discovery of a new experimental method if you haven’t even tried it yet (in other words, this belongs firmly in Beginnings).


Hear, hear!




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ChemichaelRXN
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[*] posted on 14-1-2023 at 17:43


Awful method. Doesnt work after all lol

Anyone know the best way to make the cesium hydroxide or oxide, so i can use carbon to reduce it and get cesium metal under argon atmosphere?




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[*] posted on 14-1-2023 at 17:56


Look up Cody's lab for a very user friendly apperatus. Essentially a retort using Li as a reductant. Liquid tin is used as a seal. Minimal waste and few problems with blockage, backflow, air intrusion and other things that commonly beset this synthesis



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