This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1: Calculate the actual mass and moles of reactants. The balanced chemical equation is: Fe_2O_3 + 3CO 2Fe + 3CO_2 Given: 20 g of 50% pure Fe_2O_3 and 9 g of CO. First, calculate the actual mass of pure Fe_2O_3: Mass of pure Fe_2O_3 = 20 g × 0.50 = 10 g Next, calculate the molar masses of the reactants: Molar mass of Fe_2O_3 = (2 × 55.845) + (3 × 15.999) = 159.687 g/mol Molar mass of CO = 12.011 + 15.999 = 28.010 g/mol Now, calculate the moles of each reactant: Moles of Fe_2O_3 = 10 g159.687 g/mol ≈ 0.06262 mol Moles of CO = 9 g28.010 g/mol ≈ 0.32131 mol Step 2: Determine the limiting reactant. From the balanced equation, 1 mole of Fe_2O_3 reacts with 3 moles of CO. To react completely with 0.06262 mol of Fe_2O_3, the moles of CO required would be: Moles of CO required = 0.06262 mol Fe_2O_3 × 3 mol CO1 mol Fe_2O_3 = 0.18786 mol CO Since we have 0.32131 mol of CO (which is more than 0.18786 mol required), Fe_2O_3 is the limiting reactant. a) i) The limiting reactant is: Fe_2O_3 Step 3: Calculate the moles of unreacted reactant left over. The excess reactant is CO. Moles of CO consumed in the reaction: Moles of CO consumed = 0.18786 mol Moles of CO left over: Moles of CO left over = Initial moles of CO - Moles of CO consumed Moles of CO left over = 0.32131 mol - 0.18786 mol = 0.13345 mol a) ii) Moles of unreacted reactant left over: 0.133 mol CO Step 4: Calculate the number of moles of CO consumed in the reaction. This was calculated in Step 3. a) iii) Number of moles of CO consumed: 0.188 mol CO Step 5: Calculate the mass of NaOH required to absorb all CO_2 produced. First, calculate the moles of CO_2 produced. Since Fe_2O_3 is the limiting reactant: Moles of CO_2 produced = 0.06262 mol Fe_2O_3 × 3 mol CO_21 mol Fe_2O_3 = 0.18786 mol CO_2 The reaction between CO_2 and NaOH is: CO_