If an electrolysis plant operates its electrolytic cells at a total current of 1.8 $\times$10⁶amp,how long will it take to produce one metric ton (one million grams)of Mg(s)from seawater containing Mg²⁺? (1 faraday = 96,485 coulombs)

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The correct answer is A because 1.8 F1F1F1S1F1F1F10 10⁶amp = 1.8 × 96,485 C/s = 1.73 × 10⁸ C/s. To produce 1 metric ton of Mg(s), we need to pass 1 × 10⁶ g of Mg²⁺ through the electrolytic cells. The molar mass of Mg is 24 g/mol, so we need to pass 1 × 10⁶ g / 24 g/mol = 4.17 × 10⁴ mol of Mg²⁺. Each mole of Mg²⁺ requires 2 electrons, so we need to pass 2 × 4.17 × 10⁴ mol × 96,485 C/mol = 8.02 × 10⁸ C of charge. At a current of 1.73 × 10⁸ C/s, it will take 8.02 × 10⁸ C / 1.73 × 10⁸ C/s = 4.64 h to produce 1 metric ton of Mg(s).

If an Electrolysis Plant Operates Its Electrolytic Cells at a Total