Which of the following statements about the reaction of one mole of methane (CH_4) with oxygen at standard temperature and pressure (STP) is NOT correct?

• A. The reaction of one mole of CH_4 with oxygen at STP produces one mole of CO_2.
• B. The total volume of gaseous products at STP is 22.4 L.
• C. The complete combustion of one mole of CH_4 produces two moles of H_2O.
• D. The reaction requires two moles of O_2 for complete combustion.

Answer: (B)

Verified step by step guidance

1. Write the balanced chemical equation for the complete combustion of methane (CH_4): \(\mathrm{CH_4 + 2\ O_2 \rightarrow CO_2 + 2\ H_2O}\).
2. Identify the mole ratios from the balanced equation: 1 mole of CH_4 reacts with 2 moles of O_2 to produce 1 mole of CO_2 and 2 moles of H_2O.
3. Recall that at STP (standard temperature and pressure), 1 mole of any ideal gas occupies 22.4 L. Use this to analyze the volumes of gaseous reactants and products.
4. Determine the total volume of gaseous products at STP: CO_2 is a gas, but H_2O produced in combustion is typically in the liquid phase under standard conditions, so only CO_2 contributes to the gaseous volume.
5. Compare the total volume of gaseous products to the volume of gaseous reactants to verify which statement about volume is NOT correct.