I need a little help here in confirming and replicating an experiment.
you`ll need:
1 part KClO3
1 part water
1 part Cu(NO3)2
1 part H2SO4 (I used 50% conc)
add these into a flask in the order that I presented them, and at room temp, mixing at each stage.
there will be no Apparent! gas evolved, then temp can be taken to 40c also when it`s all mixed.
there will be a Very Distinct Ozone smell, and the "Ozone headache" at greater concentrations.
the mechanics of the synth can be worked out later (or even refined) but for now, I`de just like reproducability.
and please don`t ask what I was trying to make that lead to me to this, lets just say I was having a Blonde moment!12AX7 - 8-11-2006 at 12:24
Most oxidizing gasses (Cl2, NO2, ClO2, O3, probably O2 if it weren't double bonded, OsO4, etc.) smell about the same, due to the similar effect on the
smell receptors.
I think ClO2 smells like Cl2 with an extra hint of something really nasty and choking. NO2 and HNO3 (what I've experienced) smell similar, but are
accompanied by yellow to brown gas.
Timguy - 8-11-2006 at 12:51
I don't think you need Cu(NO3)2 in there, its just ClO2 gas from chlorate and acid. ClO2 probably caused trace amounts of ozone. Ozone can be tested
using iodide paper.
[Edited on 11/8/2006 by guy]woelen - 8-11-2006 at 14:37
Quote:
Ozone can be tested using iodide paper.
This test is not very useful in the presence of ClO2 and/or Cl2. These also give a dark color on the paper.
ClO2 has not the same smell of chlorine. I also once thought it had, but finally, when I made ClO2 without Cl2 traces in it, I found it to have a
rather weak smell and also not being so severely irritating as Cl2 is.
I also did tests with ClO2, dissolved in water, and I was really surprises to see how sluggish it reacts and how stable it seems to be in its
solutions. For this reason, its use also is preferred over the use of Cl2. It is much less reactive and does not chlorinate all kinds of organics.
Only in the gaseous state and in very high concentrations, the compound ClO2 is extremely reactive and explosive.
I did the experiment with the four chemicals, and it indeed does not show any visible reaction at room temperature. The smell I obtained is weak. I
could retry with concentrated H2SO4 instead and leaving out the water, but I do not dare that in glass apparatus. I'm quite sure that results in
formation of dry gaseous ClO2 and that is a serious explosion hazard.
YT2095, why did you add the copper nitrate to the mix? Has this a special reason? Why not KNO3 or NaNO3? I also do not see any reason why this copper
compound should be there.12AX7 - 8-11-2006 at 16:50
Ah, interesting. Wouldn't have suspected of having impure ClO2 as a result of sulfuric and KClO3 or whatever.
TimYT2095 - 9-11-2006 at 03:08
Quote:
Originally posted by woelen
YT2095, why did you add the copper nitrate to the mix? Has this a special reason? Why not KNO3 or NaNO3? I also do not see any reason why this copper
compound should be there.
as I said, I was having a blonde moment, I wasn`t Thinking at all, I was Trying to make Copper Chlorate, I figured that KClO3 + Cu(NO3)2 would make
KNO3 and my copper chlorate.
it didn`t, so rather than just dump it, I poured in some sulphuric acid (excess that wouldn`t fit in the propper bottle), when I remembered that the
reaction uses copper Sulphate not nitrate, so I just dumped it in there to see what would happen if any part of it was Salvagable.
the only Noticable effect to see what the soln went a little clearer blue.
