Based on the mole ratio you determined in part c, how many moles of H2O are produced when 2 moles of H2 react completely with excess O2 according to the equation: 2 H2 + O2 → 2 H2O?

• A. 4 moles
• B. 0.5 mole
• C. 1 mole
• D. 2 moles

Answer: (D)

Verified step by step guidance

1. Identify the balanced chemical equation: \$2\ \mathrm{H_2} + \mathrm{O_2} \rightarrow 2\ \mathrm{H_2O}$.
2. Determine the mole ratio between \(\mathrm{H_2}\) and \(\mathrm{H_2O}\) from the balanced equation. Here, 2 moles of \(\mathrm{H_2}\) produce 2 moles of \(\mathrm{H_2O}\), so the ratio is \(\frac{2\ \mathrm{mol}\ \mathrm{H_2O}}{2\ \mathrm{mol}\ \mathrm{H_2}} = 1\).
3. Use the mole ratio to calculate the moles of \(\mathrm{H_2O}\) produced from 2 moles of \(\mathrm{H_2}\). Multiply the given moles of \(\mathrm{H_2}\) by the mole ratio: \$2\ \mathrm{mol}\ \mathrm{H_2} \times 1 = 2\ \mathrm{mol}\ \mathrm{H_2O}$.
4. Confirm that oxygen (\(\mathrm{O_2}\)) is in excess, so it does not limit the reaction and all \(\mathrm{H_2}\) reacts completely.
5. Conclude that 2 moles of \(\mathrm{H_2}\) produce 2 moles of \(\mathrm{H_2O}\) according to the balanced equation and mole ratio.