To determine the mass of pure aluminum that can be extracted from 655g of aluminum oxide, we need to use the balanced chemical equation for the reaction of aluminum oxide and carbon:
Al2O3 + 3C → 2Al + 3CO
This equation tells us that for every 1 mole of aluminum oxide that reacts with 3 moles of carbon, we will produce 2 moles of aluminum. We can use this information to convert the mass of aluminum oxide to moles of aluminum:
1. Calculate the molar mass of aluminum oxide (Al2O3):
2(Al) + 3(O) = 2(26.98 g/mol) + 3(16.00 g/mol) = 101.96 g/mol
2. Calculate the number of moles of aluminum oxide in 655g:
655 g / 101.96 g/mol = 6.42 mol
3. Use the mole ratio from the balanced equation to calculate the number of moles of aluminum that can be produced:
2 moles Al / 1 mole Al2O3 = 2 * 6.42 mol = 12.84 mol Al
4. Calculate the mass of aluminum produced:
12.84 mol Al x 26.98 g/mol = 346.2 g Al
Therefore, the mass of pure aluminum that can be extracted from 655g of aluminum oxide is 346.2 grams.