How many seconds are required to produce 7.00 g of aluminum metal from the electrolysis of molten $\mathrm { AlCl } _ { 3 }$ with an electrical current of 18.0 A?

Question

Quizplus · Accepted Answer

To find the time, use the formula: $ t = \frac{n \times F}{I} $, where $ n $ is moles of electrons, $ F $ is Faraday's constant (96485 C/mol), and $ I $ is current. First, calculate moles of Al: $ \frac{7.00 \, \text{g}}{26.98 \, \text{g/mol}} \approx 0.259 \, \text{mol} $. For Al, 3 moles of electrons are needed per mole of Al, so $ n = 0.259 \times 3 \approx 0.777 \, \text{mol} $. Then, $ t = \frac{0.777 \times 96485}{18.0} \approx 4.17 \times 10^3 \, \text{s} $.

How Many Seconds Are Required to Produce 7 AlCl3\mathrm { AlCl } _ { 3 }AlCl3​

How Many Seconds Are Required to Produce 7 $\mathrm { AlCl } _ { 3 }$