Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: tryteklitu on July 12, 2020, 06:45:15 AM
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what reaction CuSO4 * 5H2O + 2NaNO2?
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Probably nothing. What could react? What do you know of reduction power of nitrite and oxidation power of copper2+?
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copper will not change its valence. nitrogen will disproportionate with the release of nitric oxide
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there is no copper nitrite so I ask
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If nitrite will disproportionate, which compounds would develop. Note oxidation number of nitrogen is + 3 in this case. Can that work?
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When sodium nitrite is added to the copper salt solutions, the solution turns green. This indicates the formation of a complex compound. Copper(II) nitrite alone could not be isolated, because it will quickly oxidize with air oxygen to nitrate(V).
In more basic solutions, poorly soluble copper basic nitrite Cu(NO2)2·xCu(OH)2 (where x may be from 1 to 3) is formed.
With a large excess of KNO2, K3Cu(NO2)5 was obtained with a complex structure.
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But the question what asked was only to add coppersulfate and sodium nitrite. No alkaline envirement.
The only post I found the catalytical reaction of copper metal to nitrite in a german article from 1919. It describes the formimg of N2O , NO and nitrate.
https://onlinelibrary.wiley.com/doi/abs/10.1002/zaac.19191070108
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copper Has a coordination number of 4 instead of 5 or 6
there are not so many free orbits
since sodium nitrite can be crystallized by the presence of oxygen, I see no reason why this cannot be done with copper nitrate
if it exists
And you can always do that
isolate the inert gas atmosphere
or evaporate
under reduced pressure
the problem with copper nitrate is rather that copper has weak basic properties
and nitrite
would fall apart
nitrous acid
and copper hydroxide and next
9CuSO4*5H2O + 18NaNO2 = 4Cu2(OH)3NO3 + Cu(NO3)2 + 12NO + 9Na2SO4 + 39H2O
for now it is a theory but soon after I get the reagents They will react. it may come down hot
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copper Has a coordination number of 4 instead of 5 or 6
there are not so many free orbits
since sodium nitrite can be crystallized by the presence of oxygen, I see no reason why this cannot be done with copper nitrate
You forget about the catalytic properties of many metals.
It is very difficult to answer inaccurate questions or containing insufficient information (which is very common in this Forum). There is a lack of information on concentrations, proportions of reagents, or the order of adding reagents and the environment. Many reactions do not require such details, but in this case, it may be relevant.
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copper Has a coordination number of 4 instead of 5 or 6
there are not so many free orbits
since sodium nitrite can be crystallized by the presence of oxygen, I see no reason why this cannot be done with copper nitrate
if it exists
And you can always do that
isolate the inert gas atmosphere
or evaporate
under reduced pressure
the problem with copper nitrate is rather that copper has weak basic properties
and nitrite
would fall apart
nitrous acid
and copper hydroxide and next
9CuSO4*5H2O + 18NaNO2 = 4Cu2(OH)3NO3 + Cu(NO3)2 + 12NO + 9Na2SO4 + 39H2O
for now it is a theory but soon after I get the reagents They will react. it may come down hot
Your equation make no sense .
CuSO4* 5 H2O is only existing as a solid.
In aquaeous solution you have [Cu(H2O)42+
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Your equation make no sense .
CuSO4* 5 H2O is only existing as a solid.
In aquaeous solution you have [Cu(H2O)42+
Why?
The copper (II) nitrite that is being formed during solid reaction should be thermally decomposed starting from about 80°C.
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thanks for the attention and especially that copper can catalyze reductions to N2O. what to do I plan to pour concentrated substrate solutions in stoichiometric amounts. Then it may happen
2 [Cu (NO2) 2 (H2O) 2] <-> [Cu (NO2) 4] 2- + [Cu (H2O) 4] 2+
on one copper ion
[Cu (NO2) 4] 2- + H2O -> Cu (OH) 2 + 2NO3- + N2O
globally
2 [Cu (H2O) 4] 2+ 4NO2- -> Cu (OH) 2 + [Cu (H2O) 4] 2+ N2O + 2NO3- + 3H2O
or I wrote it earlier with NO
maybe, any suggestions on how to choose the parameters to create N2O and not NO?
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This reaction can be very sensitive to temperature. You still haven't specified the conditions under which you want to react. Giving copper sulfate pentahydrate as a reagent suggests a reaction in the solid, and this involves heating. In this case, your overall reaction is false because an attempt to dehydrate copper(II) nitrate (which is a product of your reaction) by heating also leads to basic copper nitrate.
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Your equation make no sense .
CuSO4* 5 H2O is only existing as a solid.
In aquaeous solution you have [Cu(H2O)42+
Why?
The copper (II) nitrite that is being formed during solid reaction should be thermally decomposed starting from about 80°C.
You didnt told in the beginning. I thought you dissolve both in water.
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Jak najbardziej będę rozpuszczał w wodzie najpierw przygotuje stężone roztwory które następnie będę wlewał do wody.
Mod edit using google translate
As much as possible I will dissolve in water, first I will prepare concentrated solutions which I will then pour into water.
You should post in English
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http://www.chemicalforums.com/index.php?topic=65859.0
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OK solutions - but then do not write copper sulfate pentahydrate in the reactions. The temperature, mixing order, or two dropping funnels are also important. Closed or open system - it can all be important. I advise you to use deoxygenated solutions and argon as an inert gas. And watch the reaction carefully.
I don't believe in N2O - rather NO, or the mixture with NO2. Higher reagent concentrations can be obtained from Cu(NO3)2 and KNO2.
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Jak najbardziej będę rozpuszczał w wodzie najpierw przygotuje stężone roztwory które następnie będę wlewał do wody.
English please.
Basically OP claims he will prepare concentrated water solutions which will be then added to water.
Why adding them to water instead of just mixing?