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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Hey Trinity🦋💓, good to see you again. a) To construct the chemical equation, we identify the reactants as copper (II) oxide (CuO) and sulfuric acid (H₂SO₄). They react to form copper (II) sulfate (CuSO₄) and water (H₂O). Step 1: Write the unbalanced equation. CuO(s) + H_2SO_4(aq) CuSO_4(aq) + H_2O(l) Step 2: Balance the equation. The equation is already balanced with one copper, one sulfur, and four oxygen atoms (excluding the oxygen in water) on both sides, and two hydrogen atoms on both sides. CuO(s) + H_2SO_4(aq) CuSO_4(aq) + H_2O(l) b) To determine the limiting reactant, we first calculate the moles of each reactant using their given masses and molar masses. Step 1: Calculate the molar masses of the reactants. Molar mass of CuO: Cu = 63.55 g/mol O = 16.00 g/mol Molar mass of CuO = 63.55 + 16.00 = 79.55 g/mol Molar mass of H₂SO₄: H = 1.01 g/mol S = 32.07 g/mol O = 16.00 g/mol Molar mass of H_2SO_4 = (2 × 1.01) + 32.07 + (4 × 16.00) = 2.02 + 32.07 + 64.00 = 98.09 g/mol Step 2: Calculate the moles of each reactant. Moles of CuO: Moles of CuO = 7.95 g79.55 g/mol = 0.1000 mol Moles of H₂SO₄: Moles of H_2SO_4 = 7.35 g98.09 g/mol = 0.07493 mol Step 3: Identify the limiting reactant. From the balanced equation, 1 mole of CuO reacts with 1 mole of H₂SO₄. Since we have fewer moles of H₂SO₄ (0.07493 mol) than CuO (0.1000 mol), sulfuric acid is the limiting reactant. The limiting reactant is H_2SO_4 (sulfuric acid). c) To calculate the mass of copper (II) sulfate crystals (CuSO₄·5H₂O) expected, we use the moles of the limiting reactant. Step 1: Determine the moles of CuSO₄ produced. Based on the stoichiometry of the balanced equation, 1 mole of H₂SO₄ produces 1 mole of CuSO₄. Moles of CuSO_4 = Moles of H_2SO_4 = 0.07493 mol Step 2: Calculate the molar mass of copper (II) sulfate pentahydrate (CuSO₄·5H₂O). Molar mass of CuSO₄: Cu = 63.55 g/mol S = 32.07 g/mol O = 16.00 g/mol Molar mass of CuSO_4 = 63.55 + 32.07 + (4 × 16.00) = 159.62 g/mol Molar mass of 5H₂O: H_2O = (2 × 1.01) + 16.00 = 18.02 g/mol Molar mass of 5H_2O = 5 × 18.02 = 90.10 g/mol Molar mass of CuSO₄·5H₂O: Molar mass of CuSO_4·5H_2O = 159.62 + 90.10 = 249.72 g/mol Step 3: Calculate the theoretical mass of CuSO₄·5H₂O. Theoretical mass = Moles of CuSO_4 × Molar mass of CuSO_4·5H_2O Theoretical mass = 0.07493 mol × 249.72 g/mol = 18.71 g The theoretical mass of copper (II) sulfate crystals is 18.7 g. d) To calculate the percentage yield, we use the actual yield obtained and the theoretical yield calculated in part (c). Step 1: State the actual and theoretical yields. Actual yield = 16.3 g Theoretical yield = 18.71 g Step 2: Calculate the percentage yield. Percentage yield = Actual yieldTheoretical yield × 100\% Percentage yield = 16.3 g18.71 g × 100\% = 87.1\% The percentage yield is 87.1\%. Send me the next one 📸