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(A) 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

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$N_2O_3, N_2O_4, N_2O_5$

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(A) 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.In $N_2O_3, N_2O_4$,and $N_2O_5$,the element nitrogen $(N)$ combines with oxygen $(O)$ to form different compounds.For a fixed mass of nitrogen $(28 \ g)$,the masses of oxygen are $48 \ g, 64 \ g$,and $80 \ g$ respectively.The ratio of these masses is $48:64:80$,which simplifies to $3:4:5$,a ratio of small whole numbers.Thus,$N_2O_3, N_2O_4, N_2O_5$ illustrates the Law of Multiple Proportions.

Which of the following examples illustrates the Law of Multiple Proportions?

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Which of the following pairs of substances illustrates the Law of Multiple Proportions?

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