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quote:Originally posted by pyromaster222there are many different thermites such as CaSO4/Al. this is a very high temperature thermite, more so than iron oxide i believe. it's also castable but is extremely hard to light. There are also thermites with copper oxide which burn very fast (like medium grade gunpowder)
quote:Originally posted by DrDickquote:Originally posted by pyromaster222there are many different thermites such as CaSO4/Al. this is a very high temperature thermite, more so than iron oxide i believe. it's also castable but is extremely hard to light. There are also thermites with copper oxide which burn very fast (like medium grade gunpowder)Are you sure you don't mean CuSO4/Al? To convert a metal cation to the elemental metal, you need a more active metal (one that wants to be in the cationic state even more) to perform the conversion. Al is more active than Fe, so Al metal will react with oxidized Fe but Fe metal won't react with oxidized Al. Likewise, Ca is more active than Al, so oxidized Ca won't react with Al metal. However, Cu is a pretty inactive metal, so oxidized Cu will react with Al metal.
How is the Fe oxidized to combine with the sulphur(which must be reduced again to combine with the Fe)? I don't think the Fe really does anything but then again the heat of the reaction could be enough for the reaction to form FeS to occur.Does anyone know the standard enthalpy of formation of S from S6+? What about Al3+ from Al metal? Those figures would help in determining how much material to use to make sure it doesn't kill somebody.
quote:Originally posted by Mr AndrewI think I get it. Just to make sure, if you take S and Fe (that is the elements) and heat them together do you get FeS? If you do then I think it makes sense.
quote: I've thought about this and come up with the following equation:2Al + 3[Ca]2+ + 3[SO4]2- --> 2[Al]3+ 3SO2 + 3[Ca]2+ + 62-I can't see why the S might go all the way from 6+ to 2- (the ox-state needed to make FeS) when it could stop at 4+ and make the molecule SO2 which is not extremely active and smells oh-so-wonderful.
quote:Originally posted by Xare9-11 was a False Flag Shadow Government Operation. It was an Inside Job to set a Pretext for War.
quote:Originally posted by XareThey add the sulfer because it helps lower the melting point of steel.
quote:Originally posted by simpsonsmanso even thou we didnt use any water in the mix, we can still save it by putting it in water now?
quote:Originally posted by simpsonsmanI Know but to make the rust we didnt use any water. We stuck steel wool in blech/vinger mix. So can we make this rust usable by putting it in water?
quote:Originally posted by simpsonsmanWell we have never used this rust before, i my friend thought that It wouldnt work becuase it was pure enough. So I just want to know can this rust be saved or should I just throw It out. And what do you mean by oxygenated water, Sorry i dont know much about chemestry
Im just asking, is rust usable for thermite?
Yay!!! , What did I win?!?
When you said reactions of iron in water are affected by pH, am I right in saying that if the pH is too high, Fe(OH)3 would precipitate? It shouldn't matter if it has a low pH, right...unless the conjugate base of the acid is insoluble when combined with Fe3+ ions.
But then again, if it was generally insoluble, it wouldn't be a strong acid and wouldn't lower the pH much.
I believe acetates are genereally soluble so it wouldn't really matter too much if vinegar was used.
is it true that batery acid mixed with sugar makes a thermite like reaction?