Aluminum oxide is on the surface of any aluminum metal, however you probably want more than that. There are three ways to produce the aluminum-oxide.
1. You can melt the aluminum in a furnace. There will be a thin film on top of the molten metal, that is the aluninum-oxide. You can skim this off with anything of a melting point higher than aluminum. This method leaves you with messy gobs of aluminum oxide mixed with small amounts of aluminum.
2. You can mix up a batch of thermite and light it. Aluminum oxide is a by-product of the reaction. However, this is very dangerous and I don't know how you could collect the aluminum-oxide(it is probably mixed with the iron).
3. (My favorite)You grind the aluminum into powder, probably with a bench grinder, and burn it! You get a container that won't burn and set the container with the aluminum in it in a fire(big fire)! The aluminum will burn/oxidize and you are left with a container of aluminum-oxide!
Have fun be safe, oh and make some rubies while you're at it!!!
OR
#4. use some red devel drain cleaner (* 99% Lye *) and mix in a small cup of hot water than place an aluminum bar into it.. it will produce ALLOT of heat, as the reaction is endothermic, as well as lots of hydrogen and FOAM. use a little WD40 in the water to reduce foam.. after the reaction has finished, the aluminum will be converted to Aluminum OXIDE and lye.
allow the mix of water/lye/aluminum oxide to evaporate in a tin. then add a little cutting oil to turn it into a paste.
when adding oil to lye, it turns it into SOAP.. so you'll end up with a polishing compound that will also cleaning agent.. be carefull LYE will cause burns from both the chemical and heat produced while the aluminum is converted to aluminum oxide. so use protective gear, face shield, gloves, and aprin.
enjoy.
Alumin(i)um Oxide Al2O3 is first of all dissolved in molten cryolite Na3AlF6 with calcium fluoride CaF2 and then electrolytically reduced to alumin(i)um at a temperature of approximately 965 °C .
An alternative process which converts the oxide to the carbide is in the process of being developed.
There is more information at the related link.
scrub it with bakeing soda, then use a metal polish on it,
This would be done by just heating it. Has to be hot enough to decompose though.
Example
Sn(OH)2 + Heat --> SnO + H2O
Aluminium oxide can be obtained by the calcination of aluminium hydroxide.
The reduction reaction is with aluminium and a typical example is:
Fe2O3 + 2 Al = 2 Fe + Al2O3
Aluminium oxide is Al2O3. +3 for each Al and -2 for each O.
This is a mole stoichiometry problem. Start with the balanced equation for the synthesis of aluminum oxide: 4Al + 3O2 --> 2Al2O3. The ratio of aluminum to aluminum oxide in this equation is 4:2, or 2:1, so 5.23 moles Al means half that number for Al2O3, so about 2.62 moles of aluminum oxide will be produced.
This is called oxidation, i.e. when iron reacts with oxygen iron oxide is formed. Also, combustion could be included: methane + oxygen -> carbon dioxide + water
The reaction is not possible.
CH=CH + 5N2O -----> 5N2 + 2CO2 + H2O
Aluminium oxide is Al2O3. +3 for each Al and -2 for each O.
Aluminium + Oxygen = Aluminium Oxide 2 Al + O2 = 2AlO2
This is a mole stoichiometry problem. Start with the balanced equation for the synthesis of aluminum oxide: 4Al + 3O2 --> 2Al2O3. The ratio of aluminum to aluminum oxide in this equation is 4:2, or 2:1, so 5.23 moles Al means half that number for Al2O3, so about 2.62 moles of aluminum oxide will be produced.
2Al2O3 --> 4Al + 3O2
This is called oxidation, i.e. when iron reacts with oxygen iron oxide is formed. Also, combustion could be included: methane + oxygen -> carbon dioxide + water
The reaction is not possible.
From '0' to '3'. Elemental aluminium is in oxidation state zero (0). When it combines with oxygen to form aluminium oxide , it 'looses' its three outermost electrons to oxygen. Hence aluminium metal becomes the aluminium cation (Al^3+), which is oxidation state '3'.
aluminium oxide --------------> aluminium and oxygen electrolysis
It means that there are two molecules of Aluminum Oxide, Al2O3.
Oxidation or rust
CH=CH + 5N2O -----> 5N2 + 2CO2 + H2O
Al is the symbol for Aluminum and O is the symbol for oxygen. When oxygen is paired in a compound, it is changed to oxide. The name then is aluminum oxide.