ChemichaelRXN
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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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DraconicAcid
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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.
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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ChemichaelRXN
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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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clearly_not_atara
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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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j_sum1
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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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Texium
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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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Thread Moved
6-1-2023 at 07:02 |
Rainwater
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| 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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"You can't do that" - challenge accepted
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ChemichaelRXN
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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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blogfast25
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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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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?
You are the same perception looking out, from the same elements around the universe.
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j_sum1
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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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