If 5.00 g of H2 reacts with excess O2 to form water, what mass of H2O is produced?

Study for the Chemistry 1LD Test with comprehensive flashcards and multiple choice questions. Each question is accompanied by hints and detailed explanations to ensure your success. Prepare thoroughly for your exam!

Multiple Choice

If 5.00 g of H2 reacts with excess O2 to form water, what mass of H2O is produced?

Explanation:
Stoichiometry and molar masses connect the mass of a reactant to the mass of product through a balanced equation. For hydrogen gas reacting with oxygen, the balanced equation is 2 H2 + O2 → 2 H2O, so hydrogen and water are in a 1:1 mole ratio. First convert the given hydrogen mass to moles: 5.00 g H2 ÷ 2.016 g/mol ≈ 2.48 mol H2. With a 1:1 mole ratio to water, this produces about 2.48 mol H2O. Convert to mass using the molar mass of water: 2.48 mol × 18.015 g/mol ≈ 44.7 g. Since oxygen is in excess, all the hydrogen becomes water, giving approximately 44.7 g of H2O.

Stoichiometry and molar masses connect the mass of a reactant to the mass of product through a balanced equation. For hydrogen gas reacting with oxygen, the balanced equation is 2 H2 + O2 → 2 H2O, so hydrogen and water are in a 1:1 mole ratio.

First convert the given hydrogen mass to moles: 5.00 g H2 ÷ 2.016 g/mol ≈ 2.48 mol H2. With a 1:1 mole ratio to water, this produces about 2.48 mol H2O. Convert to mass using the molar mass of water: 2.48 mol × 18.015 g/mol ≈ 44.7 g. Since oxygen is in excess, all the hydrogen becomes water, giving approximately 44.7 g of H2O.

More Multiple Choice Questions
Subscribe

Get the latest from Passetra

You can unsubscribe at any time. Read our privacy policy