In the reaction 2 H_2 + O_2 → 2 H_2O, how many moles of water (H_2O) are produced from 13.35 mol of oxygen (O_2)?

• A. 53.40 mol
• B. 6.675 mol
• C. 26.70 mol
• D. 13.35 mol

Answer: (C)

Verified step by step guidance

1. Identify the balanced chemical equation: \$2\ H_2 + O_2 \rightarrow 2\ H_2O$.
2. Determine the mole ratio between oxygen (\(O_2\)) and water (\(H_2O\)) from the balanced equation. For every 1 mole of \(O_2\), 2 moles of \(H_2O\) are produced.
3. Set up a conversion using the mole ratio: multiply the given moles of \(O_2\) by the ratio \(\frac{2\ \text{mol } H_2O}{1\ \text{mol } O_2}\).
4. Calculate the moles of water produced by applying the mole ratio to the given moles of oxygen: \$13.35\ \text{mol } O_2 \times \frac{2\ \text{mol } H_2O}{1\ \text{mol } O_2}$.
5. Interpret the result as the number of moles of water produced from 13.35 moles of oxygen.