Final answer:
The data presented for compounds X and Y show different mass ratios of carbon to hydrogen, suggesting they could be different compounds or isomers and do not exemplify either the law of definite proportions or the law of multiple proportions.
Step-by-step explanation:
Understanding carbon and its compounds requires familiarity with basic chemical principles. One such principle is the law of definite proportions, which states that a chemical compound always contains its component elements in a fixed ratio by mass. Conversely, the law of multiple proportions states that when two elements form more than one compound, the ratios of the masses of the second element that combine with a fixed mass of the first element are simple whole numbers.
Considering the compounds X and Y, with masses of carbon and hydrogen given, we can compare the mass ratios to see which law applies. For compound X, the mass ratio of carbon to hydrogen is 14.13g C to 2.96g H, which simplifies to approximately 4.78:1. For compound Y, the mass ratio is 19.91g C to 3.34g H, simplifying to approximately 5.96:1. These are not simple whole numbers related to each other, indicating that we're not looking at an example of the law of multiple proportions.
Therefore, if compound X and Y had the same empirical formula, they would represent the law of definite proportions. However, their differing ratios suggest that they may be different compounds with possibly different empirical formulas, or that they could be isomers (compounds with the same molecular formula but different structural formulas). This information suggests that while they share similarities, such as being clear, colorless, and combustible liquids, they are not the same substance and do not follow either of the specific chemical laws mentioned.