Aluminum is produced commercially by the electrolysis of al2o3 in the presence of a molten salt. if a plant has a continuous capacity of 1.10 million amp, what mass of aluminum can be produced in 2.80 h?
Al₂O₃ + 6 e⁻ + 6 H⁺ → 2 Al(s) + 3 H₂O Q = i * t = (1.10 x 10⁶ Amp)*(2.80 x 60 x 60) = 1.11 x 10¹⁰ C number of moles = 1.11 x 10¹⁰ C / 96485 C / mol = 1.15 x 10⁵ mole of e⁻ 6 : 2 (ratio of e and Al) 1.15 x 10⁵ : ?? mole of Al = 1.15 x 10⁵ x [tex] \frac{2}{6} [/tex] = 3.83 x 10⁴ mole of Al Molar mass of Al = 27 g / mole Mass of Al produced = 3.83 x 10⁴ mol x 27 g/mole = 1.03 x 10⁶ g
