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Iron(III) oxide reacts with carbon monoxide to produce iron metal and carbon dioxide. If 80 g of Fe ₂ O ₃ is reacted with 84 g of CO and the percentage yield of the reaction is 75 % , the actual mass of iron produced is ________ g . (Given: Atomic masses of Fe = 56 amu , C = 12 amu , and O = 16 amu )

Correct answer

42

Step-by-step solution

The balanced chemical equation for the reduction of iron(III) oxide is: Fe ₂ O ₃ + 3 CO 2 Fe + 3 CO ₂ Calculate the initial number of moles of each reactant: Molar mass of Fe ₂ O ₃ = (2 56) + (3 16) = 112 + 48 = 160 g/mol Moles of Fe ₂ O ₃ = 80 160 = 0.5 mol Molar mass of CO = 12 + 16 = 28 g/mol Moles of CO = 84 28 = 3 mol Identify the limiting reagent: For Fe ₂ O ₃: 0.5 1 = 0.5 For CO : 3 3 = 1 Since 0.5 Calculate the theoretical moles of Fe produced: From the balanced equation, 1 mole of Fe ₂ O ₃ produces 2 moles

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