A reaction: 4.0 g of H2 reacts completely with excess O2 to form H2O (2H2 + O2 -> 2H2O). What mass of water is produced? Give the final answer.
Chemistry
ScanSolve AI Answer
Answer
The mass of water produced is 35.7 g.
Step-by-step solution
6 stepsSteps:
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
Moles of H₂ = Mass / Molar mass = 4.0 g / 2.016 g/mol = 1.9841 mol H₂
Use the stoichiometry from the balanced equation (2H₂ + O₂ → 2H₂O) to find moles of H₂O
From the equation, 2 moles of H₂ produce 2 moles of H₂O.
Therefore, Moles of H₂O = Moles of H₂ = 1.9841 mol H₂OCalculate the molar mass of H₂O
Molar mass of H₂O = (2 * 1.008 g/mol) + (1 * 15.999 g/mol) = 18.015 g/mol
Convert moles of H₂O to mass
Mass of H₂O = Moles * Molar mass = 1.9841 mol * 18.015 g/mol = 35.744 g
Round to appropriate significant figures
The given mass (4.0 g) has two significant figures.
Mass of H₂O = 35.7 g
Was this helpful?
Try one yourself
A new problem that tests the same skill.
Still stuck on this one?
Ask a follow-up, and the answer starts from this question.
Got a different question?Ask your own question