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Answer :
Final answer:
The situation described corresponds to B. The law of multiple proportions. This law indicates that when two elements form multiple compounds, the weights of one element that combine with a fixed weight of the other are in the ratio of small whole numbers.
Explanation:
The situation described can be explained by B. The law of multiple proportions. This law states that when two elements form more than one compound, the ratios of the weights of the second element that combine with a fixed weight of the first element will be ratios of small whole numbers. In the given scenario, the same amount of sulfur (16.0 g) combines with two different quantities of fluorine (37.9 g and 56.9 g) to form two different compounds. If we take the ratio of these two weights of fluorine (56.9:37.9), we get approximately 1.5, a ratio of a small whole number, supporting the law of multiple proportions.
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The answer is B. The law of multiple proportions.
The law of definite proportions states that a given compound always contains the same elements in the same proportion by mass.
The law of multiple proportions states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.
The law of conservation of mass states that matter cannot be created or destroyed, but only transformed from one form to another.
The law of conservation of energy states that energy cannot be created or destroyed, but only transformed from one form to another.
In this case, the two chemical reactions involve the same element (sulfur) combining with different masses of another element (fluorine) to form two different compounds. This is an example of the law of multiple proportions (option B), because the masses of fluorine that combine with a fixed mass of sulfur (16.0 grams) are in the ratio of 37.9:56.9, which simplifies to 1:1.5. This means that the two compounds contain sulfur and fluorine in the ratio of 1:1.5 and 1:2.5, respectively.
