The Hall process for the production of aluminum involves the reaction of aluminum oxide with elemental carbon to give aluminum metal and carbon monoxide. If the yield of this reaction is 75%, what mass of aluminum metal can be produced from the reaction of 1.65 * 10⁶ g of aluminum oxide with 1.50 * 10⁶ g of carbon

Question

Quizplus · Accepted Answer

The balanced equation for the Hall process is: 2 Al2O3 + 3 C → 4 Al + 3 CO. First, calculate the moles of Al2O3: (1.65 * 10^6 g) / (101.96 g/mol) = 16189.5 mol. From the stoichiometry, 2 moles of Al2O3 produce 4 moles of Al, so 16189.5 mol of Al2O3 produce 32379 mol of Al. Convert moles of Al to grams: 32379 mol * 26.98 g/mol = 873,000 g. Considering the 75% yield: 873,000 g * 0.75 = 654,750 g, which is approximately 6.6 * 10^5 g.

The Hall Process for the Production of Aluminum Involves the Reaction