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 is produced. Steps: 1. Write the balanced chemical equation: 2H₂(g) + O₂(g) → 2H₂O(l) 2. Calculate the molar mass of H₂: Molar mass of H₂ = 2 × 1.008 g/mol = 2.016 g/mol 3. Convert the mass of H₂ to moles: Moles of H₂ = Given mass / Molar mass Moles of H₂ = 4.0 g / 2.016 g/mol = 1.984 mol H₂ 4. Use the mole ratio from the balanced equation to find moles of H₂O: From the balanced equation, 2 moles of H₂ react to produce 2 moles of H₂O. Therefore, Moles of H₂O = Moles of H₂ = 1.984 mol H₂O 5. Calculate the molar mass of H₂O: Molar mass of H₂O = (2 × 1.008 g/mol) + 16.00 g/mol = 18.016 g/mol 6. Convert moles of H₂O to mass: Mass of H₂O = Moles of H₂O × Molar mass of H₂O Mass of H₂O = 1.984 mol × 18.016 g/mol = 35.746 g 7. Round to the correct number of significant figures: The given mass (4.0 g) has two significant figures. Therefore, the final answer should also have two significant figures. Mass of H₂O = 36 g