Final answer:
The accuracy of the statement about combustion analysis and the molar mass of a compound cannot be confirmed without further calculations. The process involves using the masses of CO₂ and H₂O formed during combustion to determine the molecular formula and then comparing that formula with the given molar mass.
Step-by-step explanation:
The question asks whether a statement regarding the combustion analysis of an organic compound and its molar mass is true or false. However, to verify this claim, additional calculations are needed to determine the compound's empirical formula and molecular mass.
From the combustion analysis, the amount of carbon can be deduced from the mass of CO₂ and the amount of hydrogen from the mass of H₂O produced. The molar mass of CO₂ (44.01 g/mol) and H₂O (18.015 g/mol) would be used to find the moles of carbon and hydrogen, which are used to calculate their mass in the original compound. To confirm whether the molar mass of the compound is indeed 324.38 g/mol as given, the empirical formula would be determined from the mass ratios, then compared with the molecular mass provided.
Without those calculations, there's no way to verify the accuracy of the statement, so we cannot answer true or false without more information. The concept of combustion analysis in chemical stoichiometry is the key aspect here. It involves the burning of a substance to determine its composition based on the products formed (CO₂ and H₂O).