Final answer:
The mass of water produced by burning 246.4 g of methane can be calculated through stoichiometry and the balanced chemical equation of methane's combustion. However, the calculation result is not matching any of the provided options, indicating a potential typo or error in the question's data setup.
Step-by-step explanation:
The mass of water produced when a car burns 246.4 g of methane can be calculated through the balanced chemical equation for the combustion of methane:
CH4 + 2O2 → CO2 + 2H2O
For every mole of methane (CH4), two moles of water (H2O) are produced. The molar mass of methane is approximately 16.04 g/mol, and the molar mass of water is approximately 18.02 g/mol. Using stoichiometry, we can find the mass of water produced by the combustion of 246.4 g of methane:
Mass of CH4 Mol of CH4 Mol of H2O Mass of H2O
246.4 g CH4 x 1 mol CH4/16.04 g x 2 mol H2O/1 mol CH4 x 18.02 g H2O/1 mol H2O
This calculation results in 276.48 grams of water; however, this is not one of the options provided in the question, which might mean a typo in the question or an error in the initial mass of methane given. Since none of the options (A: 18.02 g, B: 36.04 g, C: 72.08 g, D: 144.16 g) is correct based on the provided data, we cannot determine the correct answer from the given options.