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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You're on a roll — Here are the solutions to your chemistry problem: 1. Write a balanced chemical equation for the reaction. Copper reacts with sulfuric acid, where sulfuric acid acts as an oxidizing agent, to produce copper(II) sulfate, sulfur dioxide gas, and water. Cu(s) + 2H_2SO_4(aq) → CuSO_4(aq) + SO_2(g) + 2H_2O(l) 2. Calculate the molar mass of the copper metal. Step 1: Convert the volume of sulfuric acid to dm³. V_H_2SO_4 = 25 cm^3 × 1 dm^31000 cm^3 = 0.025 dm^3 Step 2: Calculate the moles of sulfuric acid. Moles of H_2SO_4 = Concentration × Volume Moles of H_2SO_4 = 0.5 mol dm^-3 × 0.025 dm^3 Moles of H_2SO_4 = 0.0125 mol Step 3: Use the stoichiometry from the balanced equation to find the moles of copper. From the balanced equation, the mole ratio of Cu : H₂SO₄ is 1 : 2. Moles of Cu = (1)/(2) × Moles of H_2SO_4 Moles of Cu = (1)/(2) × 0.0125 mol Moles of Cu = 0.00625 mol Step 4: