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Sciencemadness Discussion Board » Fundamentals » Beginnings » Nitric Acid / Copper: different oxides from different concentration

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RU_KLO

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Registered: 12-10-2022
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posted on 21-12-2024 at 15:32

Nitric Acid / Copper: different oxides from different concentration

Reading "Chemistry a textbook for college" found:

If diluted:

3 Cu + 8(H + , NO3-) —> 3(Cu++, 2 NO3-) + 2 NO + 4 H2O

and if concentrated HNO3:

Cu + 4(H+, NO3-) —> (Cu++, 2 NO3-) + 2 NO2 + 2 H2O

So the difference between NO an NO2 is the concentration of the acid.

8/3 = 2,6 M HNO3 per mol of Cu. -> NO

4/1 = 4M HNO3 per mol of Cu -> NO2

Is this true?

because I think (little experience) that always I see "red smoke" when pouring nitric acid on copper.

Is this because NO oxidizes to NO2 in air?

Or this could be used to produce NO gas? (by using HNO3 of concentration less than 2,6M)

Go SAFE, because stupidity and bad Luck exist.

igxlabs

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posted on 21-12-2024 at 18:04

Nitric oxide very quickly oxidizes in air or an O2 atmosphere - pretty much instantly in any condition I've ever created over a beaker or in a flask.

I can't speak to the HNO3 concentrations - but if you're expecting NO and see NO2 - I'm virtually certain it's the oxidation.

As for generating NO: I think it would work but I don't know if there's another method that would be more efficient.

Edit: The wiki says that what you suggested is indeed the way one might do it in a lab setting. Nitric Oxide

[Edited on 22-12-2024 by igxlabs]

Sciencemadness Discussion Board » Fundamentals » Beginnings » Nitric Acid / Copper: different oxides from different concentration