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.
ScanSolve AI Answer
multipleQuestions newQuestion How many grams of water (H2O) are produced when 4.0 g of hydrogen gas (H2) reacts completely with excess oxygen? Show the balanced equation and the final mass. newAnswer 36 g of H2O are produced. Balanced Chemical Equation: 2H₂(g) + O₂(g) → 2H₂O(l) Calculations: 1. Molar masses: H₂: 2 1.008 g/mol = 2.016 g/mol H₂O: (2 1.008 g/mol) + 15.999 g/mol = 18.015 g/mol 2. Moles of H₂: Moles H₂ = 4.0 g H₂ / 2.016 g/mol H₂ = 1.984 mol H₂ 3. Moles of H₂O produced (from mole ratio): From the balanced equation, 2 moles of H₂ produce 2 moles of H₂O. Moles H₂O = 1.984 mol H₂ (2 mol H₂O / 2 mol H₂) = 1.984 mol H₂O 4. Mass of H₂O produced: Mass H₂O = 1.984 mol H₂O 18.015 g/mol H₂O = 35.744 g H₂O 5. Rounding to significant figures: The given mass (4.0 g) has two significant figures. Therefore, the final mass should be rounded to two significant figures: 36 g H₂O.