4.0 g of H2 reacts completely with excess O2 to form H2O. How many grams of H2O are produced? Give the final mass on the first line.
Chemistry
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Answer
36 g H2O are produced.
Step-by-step solution
6 stepsSteps:
Write the balanced chemical equation
2H₂(g) + O₂(g) → 2H₂O(l)
Calculate the molar mass of H₂
Molar mass of H₂ = 2 × 1.008 g/mol = 2.016 g/mol
Convert the mass of H₂ to moles of H₂
Moles of H₂ = Mass / Molar mass = 4.0 g / 2.016 g/mol ≈ 1.984 mol H₂
Use the mole ratio from the balanced equation to find moles of H₂O
From the equation, 2 moles of H₂ produce 2 moles of H₂O.
Moles of H₂O = Moles of H₂ = 1.984 mol H₂OCalculate the molar mass of H₂O
Molar mass of H₂O = (2 × 1.008 g/mol) + (1 × 15.999 g/mol) = 2.016 + 15.999 = 18.015 g/mol
Convert moles of H₂O to grams of H₂O
Mass of H₂O = Moles × Molar mass = 1.984 mol × 18.015 g/mol ≈ 35.74 g H₂O
Rounding to two significant figures (due to 4.0 g H₂), the mass of H₂O produced is 36 g.
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