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Topic: Aluminium Metal Electrolysis  (Read 212 times)

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Offline iop388

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Aluminium Metal Electrolysis
« on: March 28, 2020, 07:24:45 PM »
How many seconds are required to produce 12.00 g of aluminum metal from the electrolysis of molten Al2(SO4)3 with an electrical current of 4.50 A?

Offline billnotgatez

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Re: Aluminium Metal Electrolysis
« Reply #1 on: March 28, 2020, 08:14:08 PM »
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Offline AWK

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Re: Aluminium Metal Electrolysis
« Reply #2 on: March 29, 2020, 03:35:58 AM »
The problem could be calculated if aluminum sulfate were stable at the melting point, but this is not the case.
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Offline Borek

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Re: Aluminium Metal Electrolysis
« Reply #3 on: March 29, 2020, 04:08:30 AM »
The problem could be calculated if aluminum sulfate were stable at the melting point, but this is not the case.

I don't see how the decomposition changes amount of Al produced in the electrode process?
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Offline AWK

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Re: Aluminium Metal Electrolysis
« Reply #4 on: March 29, 2020, 04:18:49 AM »
The problem could be calculated if aluminum sulfate were stable at the melting point, but this is not the case.

I don't see how the decomposition changes amount of Al produced in the electrode process?
Melting point of Al2O3 is much, much higher
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Offline Borek

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Re: Aluminium Metal Electrolysis
« Reply #5 on: March 29, 2020, 04:58:20 AM »
It makes the process unrealistic, still doesn't change the applicability of the Faraday's law.
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Offline AWK

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Re: Aluminium Metal Electrolysis
« Reply #6 on: March 29, 2020, 05:11:12 AM »
It makes the process unrealistic, still doesn't change the applicability of the Faraday's law.

I formally agree with your statement but it should be clearly stated in the task, as for example in gas tasks it is advisable to treat real gas as an ideal gas.

Students remember all the nonsense best.
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