I was doing some Reaserch about various compounds and according to Wikipedia magnesium chloride decomposes if you slowly heat it to about 300 degrees.i was just wondering what it decomposes to because it does not say?

Well, seeing as that the composition of magnesium chloride is [ce]MgCl2[/ce] and that we're told it decomposes (i.e., breaks down), the most probable reaction would be [ce]MgCl2 -> Mg_{(s)} + Cl2_{(g)}[/ce].

Well, seeing as that the composition of magnesium chloride is [ce]MgCl2[/ce] and that we're told it decomposes (i.e., breaks down), the most probable reaction would be [ce]MgCl2 -> Mg_{(s)} + Cl2_{(g)}[/ce].

 

So would it make a sintered magnesium powder?

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Well, seeing as that the composition of magnesium chloride is [ce]MgCl2[/ce] and that we're told it decomposes (i.e., breaks down), the most probable reaction would be [ce]MgCl2 -> Mg_{(s)} + Cl2_{(g)}[/ce].

 

Would it make magnesium metal or would it react with the oxygen to make magnesium oxide?

I would assume magnesium, but I may be mistaken.

magnesium is not stable as an element of its own, chances are that it is reactive and would react to form magnesium oxide, oxidized by oxygen. As temperatures so high are still present, it would certainly be magnesium oxide, a brittle compound. magnesium strips react with oxygen just with a flame burning, much less 300 degress of heating... -.-

The decomposition must refer to the hydrate.

magnesium is not stable as an element of its own, chances are that it is reactive and would react to form magnesium oxide, oxidized by oxygen. As temperatures so high are still present, it would certainly be magnesium oxide, a brittle compound. magnesium strips react with oxygen just with a flame burning, much less 300 degress of heating... -.-

 

I would add that it is probably difficult to avoid some sort of post-reaction to occur. In many cases, a decomp (or similar reaction) may be carried out in an environment (e.g. nitrogen) that is inert towards the target metal. However, magnesium makes the nitride and oxide when heated in air, so it may be difficult in practice to get pure Mg this way. Electrolysis of the molten compound is a better bet I suppose.

Edited November 24, 201114 yr by mrteverett

The real problem will be that you simply don't get magnesium this way.

I think it would create Magnesium flakes under heat. When Mg was first discovered, it was reacted with K vapors to produce pure Mg.

But considering the heat, it will probably form MgO (magnesium is highly reactive w/ O2)...but I'm not sure, haven't tried this experiment.

 

Have you considered heating under vacuum, is that even a possibility does anyone know?

 

 

 

Would it make magnesium metal or would it react with the oxygen to make magnesium oxide?

Er... argon?

If it does create Mg, then I'll be doing this particular experiment a lot.

I think it would create Magnesium flakes under heat.

I don't.