In the reaction 2 H_2 + O_2 ightarrow 2 H_2O, how many moles of O_2 are required to react completely with 1.67 mol H_2?

• A. 1.67 mol O_2
• B. 2.00 mol O_2
• C. 3.34 mol O_2
• D. 0.835 mol O_2

Answer: (D)

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 \(H_2\) and \(O_2\) from the balanced equation. For every 2 moles of \(H_2\), 1 mole of \(O_2\) is required. This ratio can be written as \(\frac{2\ \text{mol } H_2}{1\ \text{mol } O_2}\).
3. Set up a proportion to find the moles of \(O_2\) needed for 1.67 moles of \(H_2\): \(\text{moles of } O_2 = \frac{1.67\ \text{mol } H_2}{2}\).
4. Calculate the moles of \(O_2\) by dividing the given moles of \(H_2\) by 2, based on the mole ratio.
5. Interpret the result as the amount of \(O_2\) required to completely react with 1.67 moles of \(H_2\) according to the balanced equation.