What is the law of multiple proportions?

The law of multiple proportions is a fundamental principle in chemistry that states when two elements combine to form more than one compound, the ratio of the masses of one element that combines with a fixed mass of the other element can be expressed in small whole number ratios. This law was first formulated by the English chemist John Dalton in the early 19th century.

In simpler terms, the law of multiple proportions states that if two elements can combine to form more than one compound, the masses of one element that combine with a given mass of the other element will always be in the ratio of small whole numbers.

An example of the law of multiple proportions can be seen in the compounds formed by carbon and oxygen. When carbon combines with oxygen to form carbon monoxide (CO) and carbon dioxide (CO2), the ratio of oxygen in each compound is 1:2. This follows the law of multiple proportions as the ratios are small whole numbers (1:2).

Overall, the law of multiple proportions helps to explain the consistent and predictable ways in which elements combine to form compounds, providing valuable insights into the composition and behavior of chemical substances.