grams of Fe are produced if the reaction begins with 3.0 grams of Al and 3.0 grams of F 2Al+3FeOarrow 1Al_(2)O_(3)+3Fe 1.03 g 0.69 g 27.938 2.33g Multiple Choice 10 points

To determine the amount of Fe produced in the reaction, we need to use stoichiometry.<br /><br />Given information:<br />- The balanced chemical equation is: 2Al + 3FeO → 1Al2O3 + 3Fe<br />- The reaction begins with 3.0 grams of Al and 3.0 grams of FeO.<br /><br />Step 1: Calculate the molar mass of the reactants and products.<br />- Molar mass of Al = 26.98 g/mol<br />- Molar mass of FeO = 55.85 g/mol (Fe) + 16.00 g/mol (O) = 71.85 g/mol<br />- Molar mass of Fe = 55.85 g/mol<br /><br />Step 2: Calculate the moles of the reactants.<br />- Moles of Al = 3.0 g / 26.98 g/mol = 0.111 mol<br />- Moles of FeO = 3.0 g / 71.85 g/mol = 0.042 mol<br /><br />Step 3: Determine the limiting reactant.<br />- According to the balanced equation, 2 moles of Al react with 3 moles of FeO.<br />- The ratio of moles of Al to FeO is 0.111 mol / 0.042 mol = 2.64.<br />- Since the ratio is greater than 2, Al is the limiting reactant.<br /><br />Step 4: Calculate the moles of Fe produced.<br />- According to the balanced equation, 2 moles of Al produce 3 moles of Fe.<br />- Moles of Fe produced = (3.0 g Al / 26.98 g/mol) × (3 mol Fe / 2 mol Al) = 0.111 mol<br /><br />Step 5: Calculate the mass of Fe produced.<br />- Mass of Fe produced = 0.111 mol × 55.85 g/mol = 6.21 g<br /><br />Therefore, the correct answer is 6.21 g of Fe are produced if the reaction begins with 3.0 grams of Al and 3.0 grams of FeO.