Problemas
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
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Camila
veterano · Tutor durante 12 años
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Respuesta
To determine the amount of Fe produced in the reaction, we need to use stoichiometry.Given information:- The balanced chemical equation is: 2Al + 3FeO → 1Al2O3 + 3Fe- The reaction begins with 3.0 grams of Al and 3.0 grams of FeO.Step 1: Calculate the molar mass of the reactants and products.- Molar mass of Al = 26.98 g/mol- Molar mass of FeO = 55.85 g/mol (Fe) + 16.00 g/mol (O) = 71.85 g/mol- Molar mass of Fe = 55.85 g/molStep 2: Calculate the moles of the reactants.- Moles of Al = 3.0 g / 26.98 g/mol = 0.111 mol- Moles of FeO = 3.0 g / 71.85 g/mol = 0.042 molStep 3: Determine the limiting reactant.- According to the balanced equation, 2 moles of Al react with 3 moles of FeO.- The ratio of moles of Al to FeO is 0.111 mol / 0.042 mol = 2.64.- Since the ratio is greater than 2, Al is the limiting reactant.Step 4: Calculate the moles of Fe produced.- According to the balanced equation, 2 moles of Al produce 3 moles of Fe.- Moles of Fe produced = (3.0 g Al / 26.98 g/mol) × (3 mol Fe / 2 mol Al) = 0.111 molStep 5: Calculate the mass of Fe produced.- Mass of Fe produced = 0.111 mol × 55.85 g/mol = 6.21 gTherefore, 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.