Final answer:
To determine the empirical formula of the organic compound, one must consider the mass percent ratios of C to H, the atomic masses, and the completeness of the combustion reaction. The correct empirical formula must satisfy the given mass percent ratio and the requirement about the oxygen content in relation to combustion.
Step-by-step explanation:
Given the ratio of mass percent of carbon (C) to hydrogen (H) in an organic compound (CxHyO) is 6:1, and considering that one molecule of this compound contains half as much oxygen as needed to burn one molecule of CxHy completely to CO2 and H2O, we can approach the problem by first determining the empirical formula based on the provided mass percentages. Since the empirical formula represents the simplest whole-number ratio of elements in a compound, to find it, we need to balance the mass percentage ratio with the atomic masses of C and H.
Let us denote the number of moles of C in the empirical formula as 'x' and H as 'y'. For oxygen, since the compound has half as much O atom per molecule as required for complete combustion, we can infer that the ratio of C:O should be 1:1 if we assume that in the complete combustion, we get one CO2 for each C atom. Therefore, the oxygen in the empirical formula should be the same as the number of C atoms, which is 'x'.
Given the percentage composition, we can find the moles of C and H and hence their ratio. If this ratio is not 6:1, then we need to adjust 'x' and 'y' to meet this criterion. The number of O atoms will be deduced from the combustion information provided. We can then determine the empirical formula by aligning these ratios to the lowest whole numbers, which represent the atoms' stoichiometry in the compound.
From the answer choices provided, only C2H4O2 and C2H4O3 fit the criteria mentioned above, as they are the only ones with a ratio of 1:1 for carbon to oxygen. The correct choice would then be the one which also honors the C:H mass percent ratio of 6:1.