Final answer:
The calculated mass of water produced from the combustion of 246.4 g of methane is approximately 553.57 g, which doesn't match any of the answer choices provided, suggesting an error in the question or options.
Step-by-step explanation:
To determine the mass of water produced from the combustion of methane (CH4), we need to use the balanced chemical equation for the reaction:
CH₄ + 2O₂ → CO₂ + 2H₂O
According to the stoichiometry of the reaction, one mole of methane (16.04 g/mol) produces two moles of water. First, we need to find the number of moles of methane combusted:
Number of moles of CH4 = 246.4 g / 16.04 g/mol ≈ 15.36 mol
Since 2 moles of H2O are produced per mole of CH4, the total moles of water produced will be:
Total moles of H2O = 15.36 mol CH4 × 2 mol H2O/mol CH4 ≈ 30.72 mol
Next, we calculate the mass of water produced, knowing that the molar mass of water (H2O) is approximately 18.02 g/mol:
Mass of water = 30.72 mol × 18.02 g/mol ≈ 553.57 g
However, none of the given options matches this calculation, suggesting there might be a mistake in the question or answer choices provided. If the intent was to ask about a different reactant being burnt or if there are more details to the problem, please provide them to receive accurate assistance.