How Does the Law of Multiple Proportions Apply to Sulfur and Fluorine Compounds?

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The discussion focuses on demonstrating the law of multiple proportions using the mass data of sulfur and fluorine compounds. Two compounds are analyzed: one with 0.447 g of sulfur and 1.06 g of fluorine, and another with 0.438 g of sulfur and 1.56 g of fluorine. The key point is to evaluate the ratio of the masses of fluorine that combine with a fixed mass of sulfur. The suggested calculation, (0.447/1.06)/(0.438/1.56), is intended to show how these ratios relate to the law of multiple proportions. However, it is emphasized that simply calculating this number is insufficient; the result must be interpreted to illustrate that the different ratios of fluorine in relation to a constant amount of sulfur confirm the law. The discussion suggests that rewriting the ratio in a clearer format would help in demonstrating the principle effectively.
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Sulfur forms two compounds with fluorine. In one of them it is observed that 0.447 g of sulfur is combined with 1.06 g of fluorine while in the other, 0.438 g of sulfur is combined with 1.56 g of fluorine. Show that these data illustrate the law of multiple proportions.

would (0.447/1.06)/(0.438/1.56) work, why or why not?
 
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Victor Frankenstein said:
Sulfur forms two compounds with fluorine. In one of them it is observed that 0.447 g of sulfur is combined with 1.06 g of fluorine while in the other, 0.438 g of sulfur is combined with 1.56 g of fluorine. Show that these data illustrate the law of multiple proportions.

would (0.447/1.06)/(0.438/1.56) work, why or why not?
All you've done there is write out a number. How would you now show that this number illustrates that the Law of MP is at work in these compounds ?

PS : The illlustration follows directly from evaluating and rewriting that number in a more friendly form.
 

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