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An electric current of 1.00 ampere is passed through an aqueous solution of FeCl3. Assuming 100 percent efficiency, how long will it take to electroplate exactly 1.00 mole of iron metal?(1 faraday = 96,500 coulombs = 6.02 × 1023 electrons)

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An electric current of 1.00 ampere is passed through an aqueous solution of FeCl3. Assuming 100 percent efficiency, how long will it take to electroplate exactly 1.00 mole of iron metal?(1 faraday = 96,500 coulombs = 6.02 × 1023 electrons)






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