Question

3.50 g of a certain compound x, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar of 192 g/mol, is burned completely in excess oxygen, and the mass of the products carefully measure: product dioxide mass 4.81 g product water mass 1.31 g

Answer 1

The mass ratios of carbon to hydrogen in compound X (14.13 g C to 2.96 g H) and compound Y (19.91 g C to 3.34 g H) indicate that the data is an example of the law of multiple proportions, revealing that X and Y are different compounds.

Step-by-step explanation:

The question concerns the comparison of the compositions of two substances, compounds X and Y, to determine if they follow the law of definite proportions or the law of multiple proportions. In compound X, the ratio of carbon to hydrogen by mass is 14.13 g C to 2.96 g H, while in compound Y, this ratio is 19.91 g C to 3.34 g H. To see if these compounds follow a specific law, we need to consider the mass ratios of the respective elements. When we compare these ratios, we find a simple whole-number ratio, which supports the law of multiple proportions. This means that compounds X and Y, despite being composed of the same elements, are indeed different compounds with different ratios of carbon to hydrogen.