Final answer:
To calculate the mass of aluminum that reacts to give 1.00 g of iron, you can use the stoichiometry of the reaction. The stoichiometric ratio between Fe2O3 and Al is 1:2, meaning 2 moles of Al are needed for 1 mole of Fe2O3. You can calculate the mass of Al using the molar mass of Al and the stoichiometric ratio.
Step-by-step explanation:
In the given chemical reaction:
Fe2O3(s) + 2Al(s) → 2Fe(s) + Al2O3(s)
The stoichiometric ratio between Fe2O3 and Al is 1:2. This means that for every 1 mole of Fe2O3, we need 2 moles of Al to react completely.
Since we are given that 1.00 g of Fe is produced, we can calculate the mass of Al used using the molar mass of Al and the stoichiometric ratio.
First, calculate the moles of Fe using its molar mass:
1.00 g Fe × (1 mol Fe / molar mass of Fe) = X moles of Fe
Then, use the stoichiometric ratio to calculate the moles of Al:
X moles of Fe × (2 moles Al / 1 mole Fe2O3) = Y moles of Al
Finally, calculate the mass of Al using its molar mass:
Y moles of Al × (molar mass of Al / 1 mol Al) = Mass of Al