Aluminum nitrate (Al(NO3)3) and aluminum powder (Al) reaction

[killerpikem]

purple lights aluminium in excited state?

[MrNammle]

Microsoft sam... -.- and you created the very first hand teleportation device.

[Agentoxedo07]

Holy-Terrorist:>*=*

[AKAtheA]

A thermometer is not what I would use to mix pretty much anything...

[MrTechGuy1995]

@AKAtheA XD I was WTF'n when I saw that!

[Peterditaa]

did you burn your hand?

[ChBullz5]

OMG! Your hand blew right off so fast you couldn't even see it!

[ExothermicVideos]

That's an interesting reaction.

[GingyPno123]

Whats happen with your hand at 2:10?

[MagicMussh]

Hahaha. I like how your hand disappeared in like half a second. xD

[MagicMussh]

What's the gram weight for aluminum? The video cuts off right before it is shown.

[MagicMussh]

disregard that comment, my speakers weren't working and i just fixed them and re-watched the video.

[hotje2]

Gaar man,aluminlfum alimumuilm zo praat die gast hij stottert man alumimfm

[adriiPortillo]

german dark is not only produced in germany... also in colombia :b It's atomized and mixed with elemental carbon at about 5%, giving de "dark" name.

[JaycubL]

And also at random people's houses.

[CarbonScience]

Yes, but it probably isn't as fine as the "original" one.

[adriiPortillo]

i cant imagine someone having a molten metal atomizer in their houses.

[bla287]

Did you use anhydrous Al(NO3)3 or it's nonahydrate?

[CarbonScience]

It probably don't matter, the reaction should work in both cases. The only thing different are ratios. See what ratio (there are 2 in the describtion) works best with your aluminum nitrate.

[bla287]

Theoretically yes, but wouldn't the crystal water slow down the combustion reaction? I'm just wondering if the energy of the reaction of one mole of Al(NO3)3 (with equivalent Al) would be enough to completely evaporate 9 moles of H2O...

[CarbonScience]

Yes, I think the reaction would be slower but it should probably work.

I don't quite get what you wondering, I'm not so good at english so can you be more specific?

Thanks.

[bla287]

Oh, I'm not a native English speaker either ;)

See, if you want to make water into vapour (>100°C), you need a whole lot of energy, that's why you use water to extinguish most fires, because it somehow absorbs the heat and cools down the reaction mixture so far that it cannot react any further. Now if you have the nonahydrate, it's just like if you'd add water to a KNO3/Al mixture => it will not ignite anymore (or only slowly).

(cont)

[bla287]

(cont)

That's why I think there's a big difference whether you use the nonahydrate or the anhydrous form. So my question remains: Which one did you use?

[CarbonScience]

Well, I think it was anhydrous because it was heated to 120°C before storing...

[bla287]

Oh, and it didn't decompose? Interesting, I should try that, it's way faster and cheaper than the exsiccator method :)

[CarbonScience]

Boiling point

135 °C (nonahyrdate, decomp.)

Mine never went liquid so the temperature was a little lower... Measure the temperature if you will attempt to do this.

[NurdRage]

interesting, not practical as aluminum nitrate is more expensive to make than buying potassium nitrate, but still very interesting.

Did you grind your stuff using a thermometer? i advise against that cause if the thermometer breaks you'll get crap in your stuff, and if it's mercury then you'll get neurotoxic crap in your stuff.

[CarbonScience]

I only had a alcohol thermometer at hand. I went to the chemistry supply shop today to buy more glassware and it was closed (the fifth time) so I can't get any glass rods to mix wit them. I'll try the same thing with calcium and magnesium nitrate. It's very amazing that a fuel's compound can be an oxidizer, too.