How long (in hours) will a current of 2.00 A need to be applied to produce 50.0 grams of aluminum metal from molten Al2O3

Explanation:

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In this case, given the mass of aluminum metal which can undergo the following reduction from aluminum oxide:

We can see three moles of electrons are transferred per mole of aluminum, thus, we obtain:

Next, we compute the charge carried by those electrons via the faraday's constant:

Finally, considering the applied current, we compute the elapsed time in hours to achieve such electrolysis:

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