Final answer:
The maximum mass of aluminum oxide produced along with 64.39 g of iron is 58.78 g, calculated by using stoichiometry and the molar masses of iron (Fe) and aluminum oxide (Al2O3) from the balanced thermite reaction.
Step-by-step explanation:
Calculating the Mass of Aluminum Oxide Produced
To calculate the maximum mass of aluminum oxide that can be produced along with 64.39 g of iron (Fe), we need to consider the stoichiometry of the thermite reaction, which involves aluminum (Al) reacting with iron(III) oxide (Fe2O3). The reaction can be represented as:
2Al + Fe2O3 → Al2O3 + 2Fe
From the balanced equation, we can see that 1 mole of Fe2O3 produces 2 moles of Fe. Using the molar mass of Fe (55.85 g/mol), we can convert the given mass of iron (64.39 g) to moles:
Moles of Fe = 64.39 g Fe × (1 mol Fe / 55.85 g Fe) = 1.153 moles of Fe
According to the stoichiometry of the reaction, 1.153 moles of iron comes from 0.5765 moles of Fe2O3 (as every 2 moles of Fe come from 1 mole of Fe2O3). Now, we can find how much Al2O3 can be produced from 0.5765 moles of Fe2O3, as the molar ratio of Fe2O3 to Al2O3 is 1:1:
Moles of Al2O3 = 0.5765 moles of Fe2O3 (1 mole of Al2O3 / 1 mole of Fe2O3) = 0.5765 moles of Al2O3
Using the molar mass of Al2O3 (101.96 g/mol), we can convert the moles of Al2O3 to mass:
Mass of Al2O3 = 0.5765 moles Al2O3 × (101.96 g Al2O3 / 1 mol Al2O3) = 58.78 g of Al2O3 (to three significant figures)
Therefore, the maximum mass of aluminum oxide produced along with 64.39 g of iron is 58.78 g.