So I want to write the reaction for this. I originally wrote the following equation: 2AlCl3 (l) ---> 2Al(s) + 3Cl2(g)
My teacher said that this was wrong and I'm guessing that there is something wrong with one of the physical states because I'm not really sure what happens when something is electrolyzed. Please oh please help!!
2006-12-17 15:49:26 · 7 answers · asked by danit89 1 in Science & Mathematics ➔ Chemistry
What your teacher is getting at is that AlCl3 and its dimer, Al2Cl6, are essentially covalent. So electrolysing them is not going to produce any aluminium!
To get aluminium by electrolysis, you have to dissolve bauxite into molten cryolite at about 900 degrees Celcius - not something that you could easily do in the laboratory!
2006-12-18 05:04:14 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
Molten Aluminum Chloride Is Electrolyzed
2016-10-18 07:04:30 · answer #2 · answered by ? 4 · 0⤊ 0⤋
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Molten aluminum chloride is electrolyzed?
So I want to write the reaction for this. I originally wrote the following equation: 2AlCl3 (l) ---> 2Al(s) + 3Cl2(g)
My teacher said that this was wrong and I'm guessing that there is something wrong with one of the physical states because I'm not really sure what happens when...
2015-08-07 18:52:21 · answer #3 · answered by ? 1 · 0⤊ 0⤋
I say your teacher is wrong. AlCl3 doesn't have a liquid phase under standard conditions -- it sublimes straight to gas phase Al2Cl6 molecules at 180ºC. So "molten aluminum chloride" doesn't exist, unless you put it under a fair amount of pressure.
Maybe s/he wants liquid aluminum as a product? But mp Al isn't until 660ºC. That is how you isolate Al when you make it, actually, as a liquid, but AlCl3 isn't the starting material in the industrial process. Or maybe you're meant to write out the half reactions separately? Dunno. As written, your equation looks fine to me, except for the fact that it's really unfeasible to make "molten AlCl3" under any practical conditions, which isn't your fault, because it's what the question is asking.
2006-12-17 16:12:50 · answer #4 · answered by Stephen McNeil 4 · 0⤊ 0⤋
this is in effect a redox problem. However, electrolysis involves the breaking down into ions, Al 3+ and Cl 1-
2006-12-17 16:56:58 · answer #5 · answered by Anonymous · 0⤊ 0⤋
Is your teacher looking for a redox reaction? cause it doesn't look like your answer would carry that. Because from what I can tell both are being reduced...so something needs to get oxidized...I don't know...sorry
2006-12-17 16:20:23 · answer #6 · answered by dizzy 2 · 0⤊ 0⤋
K+ + e- --------> K (reduction at cathode) 2 Cl- -------> Cl2(g) + 2 e- (oxidation at anode)
2016-03-20 05:53:47 · answer #7 · answered by Anonymous · 0⤊ 0⤋