Can Hydrated Fe2o3 React With Aluminium Powder

Because unloyalty of oxide in Fe2O3 “couple” when metal Al is near. When suitable condition is available (high temperature), the oxygen from Fe2O3 will jump into Al’s arm. As a compensation Al will offer Fe3+ its electrons and make it back to bachelor Fe.Ok, be serious! It is because metal Al is a strong reducing agent at high T. It can reduce Fe2O3 to Fe, and capture the left over O2- forming Al2O3.

You’ll get a big dark spot on the ceiling of your lab, at best.( this is just one of the many Utube vids, chose this one because its short; mind you they use alu foil + cold NaOH solution, now imagine fine powder and a hot solution, its reaction speed x 20 or more.):NaOH + Al + H2O => NaAlO2 + 2 H2(g) ( turns later to NaAl(OH)4 ).

Aluminum corrodes but it does not rust. Rust refers only to iron and steel corrosion.Aluminum is actually very prone to corrosion. However, aluminum corrosion is aluminum oxide, a very hard material that actually protects the aluminum from further corrosion. Aluminum oxide corrosion also looks a lot more like aluminum (dull gray to powdery white in color), so it isn't as easy to notice as rusted iron.When iron corrodes the color changes and it actually expands. This expanding and color change can produce large red flakes that we all know as rust. Unlike aluminum oxide, the expanding and flaking off of rust exposes new metal to further rusting. This is why it is so important to provide a barrier so rust doesn't start.While aluminium doesn't rust, it often becomes dull from corrosion, and is often encrusted with brake dust, calcium, lime, tarnish, grease, oil and hard water stains. Simply washing it off will not work, you need something stronger and more effective to do the job.Does Aluminum Rust?

Its not a thermite reaction and its not a galvanic one either. Its simply the reaction of acid with metals.Thermite uses iron oxide not iron metal anyway. And thermite won't start without a magnesium fuse to expose the aluminium, and certainly not in solution. The reaction has nothing to do with thermite chemistry.  Aluminium is highly energetic. The reason it does not react under normal conditions is the very rapid formation of a layer of tough surface oxide. (Anodising is used to thicken the layer even more). In solution the trick is to get water into the oxide layer.Boaties know that aluminium is prone to chloride  corrosion, so the formation of hydroxy-chloride complexes is involved in breaking down the oxide layer in hydrochloric acid. (At a guess this could possibly implicate the iron as a catalytic agent, but its not actually necessary, and I doubt it is involved at all). Aluminium will however react with hot dilute hydrochloric acid. Most likely you got separate reactions:This rather lame reaction is used to de-scale rust.Fe2O3(s) + 6HCl( aq) —> 2FeCl3(aq) + 3H2O(l) A bit better is:2Fe(s) + 6HCl(aq)  --->  2FeCl3(aq) + 3H2(g)These reactions give off hydrogen gas, do not do this anywhere near a lighted flame or enclosed area.  Iron powder will react with the hydrochloric more vigorously than when etching iron objects,  due to the increased surface area:But this one is a different beast, especially as the temperature rises:2Al(s) + 6HCl(aq) —> 2AlCl3(aq) + 3H2(g) Temperature has a lot to do with it, assisting the break down of and the oxide layer (via chloride complexes) which is hydrolysed by the acid. The rate of reaction therefore increases exponentially, and steams. You would have noticed the hydrogen evolution.(Incidentally commercial aluminium already contains an appreciable amount of dissolved hydrogen gas, about 14cc of gas per 100 g of metal and contributes to brittleness.)

This is cool! There are actually two reactions involved in reacting aluminum metal in sodium hydroxide.  You see, aluminum is a VERY reactive metal.  It forms a thin oxide coating (Al2O3) almost instantly on exposure to air and that coating prevents further reaction with the metal, thus making the world safe for soda and beer cans (not to mention beer kegs!).   So if you want to react aluminum with sodium hydroxide, the first reaction you will need is one to get rid of that pesky aluminum oxide coating! This is how:   Al2O3 + 2 NaOH --> 2Na+ + 2[Al(OH)4]- The species, [Al(OH)4]- is the tetrahydroxoaluminate complex ion.  It only appears at high pH.  At low pH you cannot get it to form and thus, you will get no further reaction because you cannot dissolve the aluminum oxide coating on the metal.  Fortunately, we are using sodium hydroxide and low pH is not even a remote possibility! Now that you have pure aluminum metal, you can react that with more sodium hydroxide: 2 Al + 2 NaOH + 6 H2O → 2 Na+ + 2[Al(OH)4]- + 3 H2 (gas) So there you have it.

The thermite process is a chemical reaction in which a metal oxide (preferrably molten) are displaced by another molten metal which is more reactive than the metal in the metal oxide, releasing a lot of heat. Example -2Al + Fe2O3→ Al2O3 + 2Fe2Al + Cr2O3 → Al2O3 + 2CrHere, Al (Aluminium) is more reactive than Fe (Iron) or Cr (Chromium), and displaces it from their oxides.This reaction is used commercially to weld broken metallic parts(due to the molten metal and high temperature at which the reaction occurs). railway lines are joined in the same manner.