symboom
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Non Electrolyic Chlorate Production
chlorate produced without electricity. this is a long process that would take a lot of time and is easier done the electrolytic way as this is
inefficient (i forgot to add before i knew this already when going in to this)
calcium hydroxide (i used calcium hydroxide)
or magnesium hydroxide chlorine is lead into one
the chlorine is produced from
i do not think the hydroxide has to be above room temperature
first starting with making chlorine gas
sulfuric acid react with NaCl to form HCl gas lead into water
to form hydrochloric acid react HCl with MnO2
forming chlorine gas lead gas in to hydroxide solution
----
preparation of calcium hydroxide from calcium carbonate
or to get magnesium hydroxide react magnesium sulfate with calcium hydroxide
of topic chlorine gas from making chlorate through a chlorate cell lead into calcium or magnesium hydroxide
excerpt http://www.dtic.mil/cgi-bin/GetTRDoc?AD=AD016814&Locatio...
be treated with chlorine until
calcium chlorate had formed- The latter, when treated with potassium
chloride, would produce crystals of potassium chlorate while calcium
chloride remained in the discarded mother liquor. With minor modifications
this method was adopted and has maintained its basic
superiority over a number of rivals. It was surpassed only by the
electrolytic process, beginning about 1900.
Tnere are now two major processes for the chemical production of
chloiates in which lime is the initially chlorinated base. The
first process (Liebig) produces potassium chlorate; the second process
(Pechiney) produces sodium chlorate. Pechiney modified both
processes, but was particularly credited with using sodium sulfate
to form sodium chlorate from the calcium chlorate - calcium chloride
liquor.
The Liebig process is described further in this report in connection
with the cost estimate (See Section B). Complete details for operating
both lime-chlorate processes are described by Lunge (28,29>30),
Juiisch (25). and Partington (39)- These descriptions cover the
better techniques at the turn of the century. Important recent
works are those of Dorph (12), Robson (^2), Shah (U3), Fhcherbakov
(kk), Shraibman (46), and Thumm (U9).
The chlorination reaction appears to follow the course indicated
in the equations below (87,88,89). The mechanism may be different
in acid and basic media (90)-
1. 2Ca(0H)2 + 2C12 -» Ca(C10)2 + CaCl2 + 2H20
2. UHsO + 4Cl2-> UH0C1 + UHC1
3. Ca(C10)2 + UH0C1 -» Ca(C103)2 + UHC1
k. UCa(0H)2 + 8HC1-* UCaCl2 + &E^)
5- 6ca(0H)2 + 6Cl2-» Ca(C103)2 + 5CaCl2 + 6Hj>0
6. Ca(C103)2 + 2KC1 -» CaCl2 + 2KC103
For a detailed comparison of the actual cobts of the Liebig process
Dr. Hunter of cur engineering department made the cost estimate reported
in the supplement to this report.
[Edited on 21-4-2011 by symboom]
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woelen
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This process is not efficient at all. Of all chlorine, only 1/6 part goes into the chlorate, the rest becomes chloride. Besides that, you have the
task of separating that small amount of chlorate from the large amount of chloride. Even for potassium, where the solubilities of chlorate and
chloride are quite different at room temperature, this is not such an easy process, because of the low amount of chlorate in the total solution.
Electrolysis is the way to go for making chlorates.
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ScienceSquirrel
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If you want a small amount of potassium chlorate to demonstrate its properties it can be made from bleach.
If you want hundreds of grams then build an electrolysis cell as Woelen suggests.
I would not try and make the bleach myself as it can be bought cheaply from pool supply shops etc.
The process has been described on this website, see here;
http://www.sciencemadness.org/talk/viewthread.php?tid=10727
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symboom
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this was more for a interesting challenge for me as i got the materials from starting materials seashells(calcium carbonate), burning sulfur to get
sulfuric acid and salt, sulfur and manganese dioxide, lantern battery source of manganese dioxide sulfur i had to ordered though
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symboom
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as i cant edit the one above or i would add it there
i found this
Calcium hypochlorite is manufactured commercially by passing chlorine through an aqueous solution of sodium hydroxide containing suspended particles
of calcium hydroxide. In this process, the calcium hydroxide is chlorinated according to the following well known reactions: 2Ca(OH) 2 +2Cl 2
➝Ca(OCl) 2 +2CaCl 2 +2H 2 O 4NaOH+2Cl 2 ➝2NaOCl+2NaCl+2H 2 O CaCl 2 +2NaOCl➝Ca(OCl) 2 +2NaCl
as http://www.freepatentsonline.com/4374115.html
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ScienceSquirrel
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You are going to have to run this on a fairly big scale and it will consume a lot of chemicals. It is also a fairly nasty process
Calcium hypochlorite is readily available from pool suppliers etc in kilo qauntities so buying it is the best idea.
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blogfast25
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Learn at least to distinguish between 0 and O and 1 and l on your keyboard. And what on earth are UH0C1, UCa(0H)2, UCaCl2, E^ and the even more
quizzical “6Hj>0”?
I know this forum isn’t great for writing chemical equations but you’re turning them into incomprehensible gobbledygook. I’m not impressed.
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symboom
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sorry cut and paste must have screwed it up
but yeah i am going to abandon this idea to much problems
[Edited on 27-4-2011 by symboom]
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