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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36 g of H2O are produced. Here are the steps: 1. Write the balanced chemical equation: 2H₂(g) + O₂(g) → 2H₂O(l) 2. Calculate the moles of H₂: Molar mass of H₂ = 2 * 1.008 g/mol = 2.016 g/mol Moles of H₂ = Given mass / Molar mass = 4.0 g / 2.016 g/mol = 1.984 mol H₂ 3. Use the mole ratio to find moles of H₂O: From the balanced equation, 2 moles of H₂ react to produce 2 moles of H₂O. The mole ratio is 1:1. Moles of H₂O = Moles of H₂ = 1.984 mol H₂O 4. Calculate the mass of H₂O produced: Molar mass of H₂O = (2 * 1.008 g/mol) + 15.999 g/mol = 18.015 g/mol Mass of H₂O = Moles of H₂O Molar mass of H₂O = 1.984 mol 18.015 g/mol = 35.744 g 5. Round to appropriate significant figures: Since the given mass (4.0 g) has two significant figures, the final answer should also have two significant figures. Mass of H₂O ≈ 36 g