Answer
See explanation
Work Step by Step
The law of multiple proportions states that when two elements form more than one compound, the ratio of the masses of one element that combine with a fixed mass of the other element is always a ratio of small whole numbers.
In this case, the two compounds are composed of only carbon and oxygen. By using the data given, we can calculate the mass of oxygen in each sample:
First compound = 100g - 27.2g = 72.8g
Second compound = 100g - 42.9g = 57.1g
The ratio of the mass of carbon to the mass of oxygen in the first compound is 27.2/72.8 = 0.375.
The ratio of the mass of carbon to the mass of oxygen in the second compound is 42.9/57.1 = 0.754.
We can see that these ratios are not small whole numbers, but we can simplify them by dividing them by their greatest common denominator, which is 0.375 and 0.754 respectively.
This will give us:
0.375/0.375 = 1 and 0.754/0.375 = 2
The ratio of the mass of carbon to the mass of oxygen in the first compound is 1:2 which is a ratio of small whole numbers. This supports the law of multiple proportions which states that when two elements form more than one compound, the ratio of the masses of one element that combine with a fixed mass of the other element is always a ratio of small whole numbers.
