What average current is required to form 5.7 grams of aluminum per hour by the electrolytic reaction? A)1.9 A B)5.7 A C)17 A D)0.024 A E)7.9 × 10^-3 A

Question

Quizplus · Accepted Answer

The amount of aluminum formed in one hour can be calculated using Faraday's law:
moles of Al = (current * time) / (96500 * Molar mass of Al)
where Molar mass of Al = 27 g/mol
Thus, moles of Al = (current * 3600s) / (96500 * 27 g/mol) = 0.0021 * current
To form 5.7 g of Al per hour, we need 5.7 g / 27 g/mol = 0.211 moles of Al
0.211 moles of Al = 0.0021 * current
Therefore, current = 0.211 moles of Al / 0.0021 = 100 A
Therefore, the average current required to form 5.7 g of aluminum per hour is 17 A (Option C).

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