Question

Illustrate the law of multiple proportion using the formation of Sulphur four oxide and sulphur six oxide by sulphur and oxygen.

A. S₄O and S₆O demonstrate the law of multiple proportions by having varying sulfur-to-oxygen ratios.
B. The law of multiple proportions is not applicable to the formation of sulfur oxides.
C. S₄O and S₆O violate the law of multiple proportions due to inconsistent compositions.
D. S₄O and S₆O have the same sulfur-to-oxygen ratio, supporting the law of definite proportions.

Answer 1

The Law of Multiple Proportions illustrates that when two elements form multiple compounds, the masses of one element that combine with a fixed mass of the other are in small whole number ratios. Hypothetical sulfur oxides S₄O and S₆O would exemplify this law if they existed, with oxygen combining with sulfur in a simple whole-number ratio, similar to the ratios observed in real compounds like carbon dioxide and carbon monoxide.

Step-by-step explanation:

The Law of Multiple Proportions states that when two elements (like sulfur and oxygen) form more than one compound, the proportions of the masses of one element that combine with a fixed mass of the second element can be expressed in ratios of small whole numbers. To illustrate this with the formation of sulfur oxides, let's consider hypothetical compounds Sulfur four oxide (S₄O) and Sulfur six oxide (S₆O), although the correct chemical formulas for sulfur oxides are SO₂ and SO₃.

Assuming we keep the sulfur mass constant, the ratio of the masses of oxygen in the two sulfur oxides would be in a simple whole-number ratio, as stated by the law. This law can be compared with the example of carbon oxides. When carbon and oxygen combine to form carbon dioxide (CO₂) and carbon monoxide (CO), the mass ratio of oxygen to carbon for CO₂ is 2.66 to 1, and for CO it is 1.33 to 1, revealing a whole number ratio of 2:1 between the oxygen in the two compounds.