When 4.0 g of H2 reacts with excess O2 (2H2 + O2 -> 2H2O), how many grams of water are produced? Show the steps.
Chemistry
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Answer
When 4.0 g of H2 reacts with excess O2, 36 grams of water are produced.
Step-by-step solution
5 stepsHere are the steps:
Calculate the molar mass of H2 and H2O
- Molar mass of H2 = 2 * 1.008 g/mol = 2.016 g/mol
- Molar mass of H2O = (2 * 1.008 g/mol) + 16.00 g/mol = 18.016 g/mol
Convert the given mass of H2 to moles
- Moles of H2 = Mass of H2 / Molar mass of H2
- Moles of H2 = 4.0 g / 2.016 g/mol = 1.984 mol H2
Use the mole ratio from the balanced equation to find moles of H2O
- The balanced equation is 2H2 + O2 -> 2H2O.
- From the equation, 2 moles of H2 produce 2 moles of H2O. This is a 1:1 mole ratio.
- Moles of H2O = Moles of H2 = 1.984 mol H2O
Convert moles of H2O to grams
- Mass of H2O = Moles of H2O * Molar mass of H2O
- Mass of H2O = 1.984 mol * 18.016 g/mol = 35.746 g
Round to appropriate significant figures
- The given mass (4.0 g) has two significant figures, so the answer should also be rounded to two significant figures.
- Mass of H2O = 36 g
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