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#Post#: 1394--------------------------------------------------
Re: Problem of the week-19/11/12
DIR By: Michel
Date: December 3, 2012, 3:47 pm
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Hopefully, next week's problem will be better
#Post#: 1397--------------------------------------------------
Re: Problem of the week-19/11/12
DIR By: Shiva
Date: December 4, 2012, 12:59 am
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I'm not sure about that reaction either Mich. All I know is it
will react violently for sure. But, I do not think when it
reacts violently, it will give you simply chloride and sulfate.
I know a reaction when bromic acid (HBro3) reacts with hydrogen
sulfide and it precipitates sulfur in that reaction also
liberates elemental Bromine. But, this one is metallic sulfide
and it could react differently. We all know chlorates are very
powerful oxidizing agents and incompatible with almost all
chemicals. One who knows very well about chlorates can only work
with them. Also, we need fumehood for such chemicals as they
produce explosive mixtures with many chemicals. You know
ammonium chlorate explodes even in the presence of sunlight
haha. Salts of Chloric acid are very aggressive oxidizing agents
and slightly unstable. But surprisingly, perchlorates are more
stable with an extra oxygen. Also, I can remember when I studied
in school, books suggested to use Potassium chlorate for oxygen
preparation. I would say that is an Idiotic way especially for
students. Molten potassium chlorate is extremely dangerous and
it will react violently with so many chemicals. We have many
easy and cheap routes for preparing oxygen. I do not understand
why should we go with Potassium chlorate. Really a bad idea.
Shiva
#Post#: 1399--------------------------------------------------
Re: Problem of the week-19/11/12
DIR By: Michel
Date: December 4, 2012, 4:04 am
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I remember reading somewhere where it was recommended to add
MnO2 to catalyse the KClO3 decomposition.
Now imagine if there's some (major?) impurity in your
MnO2...such as powdered graphite..:-/
#Post#: 1400--------------------------------------------------
Re: Problem of the week-19/11/12
DIR By: Shiva
Date: December 4, 2012, 5:27 am
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Yep, that's why we should avoid using Mno2 taken from batteries
for this sort of reaction. For preparing manganese salts or
oxygen, it should be fine. I love to study about properties of
different chemicals. If you see, any compounds contain chlorine
and oxygen, they are not very stable (of course, there are some
exceptions) and a strong oxidant even they contain one atom of
oxygen (salts of hypochlorous acid) and react violently whereas
oxides of other halogens not aggressive this way albeit they are
good oxidizing agents. Very interesting.
Shiva
#Post#: 1408--------------------------------------------------
Re: Problem of the week-19/11/12
DIR By: Michel
Date: December 4, 2012, 10:13 pm
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Perchlorates should be highly stable due to electron
delocalization in the perchlorate ion. That they are very stable
isn't very surprising, but it's quite remarkable and starkly
different from other oxychlorides...I think they are highly
soluble than other oxychloride salts
hope I'm not wrong :P
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