Which of the following pair of compounds does not illustrate law of multiple proportion
Answers
Answer:
The Law of Multiple Proportions is the third postulate of Dalton's atomic theory. It states that the masses of one element which combine with a fixed mass of the second element are in a ratio of whole numbers.
Therefore, the masses of oxygen in the two compounds that combine with a fixed mass of nitrogen should be in a whole-number ratio. In 100 g of the first compound (100 is chosen to make calculations easier) there are 36.36 g O and 63.64 g N. The mass of O per gram N is:
36.36 g O / 63.64 g N = 0.57 g O per g N
In the 100 g of the second compound, there are 53.33 g O and 46.67 g N. The mass of oxygen per gram of N is:
53.33 g O / 46.67 g N = 1.14 g O per g N
Dividing the mass O per g N of the second (larger value) compound:
1.14 / 0.57 = 2
Which mean that the masses of oxygen that combine with nitrogen are in a 2:1 ratio. The whole-number ratio is consistent with the Law of Multiple Proportions.