Which statement is incorrect about the combustion of 1 liter of CH_4(g) and 2 liters of O_2(g) at the same temperature and pressure?

• A. The volume ratio of CH_4(g) to O_2(g) used matches the stoichiometry of the balanced equation.
• B. O_2(g) is the limiting reactant in this reaction.
• C. All of the CH_4(g) will be completely consumed.
• D. The reaction will produce 1 liter of CO_2(g) and 2 liters of H_2O(g) vapor.

Answer: (D)

Verified step by step guidance

1. Write the balanced chemical equation for the combustion of methane (CH_4): \(\mathrm{CH_4(g) + 2\ O_2(g) \rightarrow CO_2(g) + 2\ H_2O(g)}\).
2. Identify the mole (and volume) ratio of reactants from the balanced equation: 1 volume of CH_4 reacts with 2 volumes of O_2 under the same temperature and pressure conditions.
3. Compare the given volumes of reactants (1 L CH_4 and 2 L O_2) to the stoichiometric ratio to determine if either reactant is limiting. Since the volumes match the 1:2 ratio, neither is limiting and both should be completely consumed.
4. Use the balanced equation to find the volumes of products formed: 1 volume of CO_2 and 2 volumes of H_2O vapor are produced, assuming ideal gas behavior and that water remains in the gaseous state.
5. Evaluate the correctness of the statements by checking if the volume ratios and limiting reactant assumptions align with the stoichiometry and reaction conditions.