Question

Samples of compounds containing nitrogen and oxygen were broken down into their component gases. The volume of each gas was measured. Based on the results shown, do nitrogen and oxygen obey the Law of Definite Proportions or the Law of Multiple Proportions? Support your answer with evidence from the table below.

Answer 1

The results suggest that nitrogen and oxygen in these samples obey the Law of Definite Proportions

Here is why:

The Law of Multiple Proportions states that when two elements 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.

To determine if nitrogen and oxygen in these samples obey the Law of Multiple Proportions, we need to examine the ratios of the volumes of oxygen (O) to nitrogen (N) for each sample.

• Sample 1:
  `\((3.02)/(2.0) = 1.51\)`

• Sample 2:
  `\((1.99)/(1.01) = 1.97\)`

• Sample 3:
  `\((4.99)/(1.98) = 2.52\)`

The ratios are not close to simple whole numbers, indicating that the Law of Multiple Proportions is not followed.

Instead, the results suggest that nitrogen and oxygen in these samples obey the Law of Definite Proportions, as the ratios are not variable and are consistent within each sample.