Law of Multiple Proportions
According to Dalton's Law, or the law of multiple proportions, the mass ratios of one element that combine with a fixed mass of the other element can be stated in small whole numbers when two elements combine to form various compounds.
In other words, if two elements may combine to make many compounds, the masses of those compounds will be arranged in simple integer ratios.
Law of Multiple Proportions with Example
Carbon and oxygen can combine to generate two distinct molecules carbon monoxide (CO) and carbon dioxide (CO2). The masses of carbon to oxygen in these compounds will be arranged in simple integer ratios in accordance with the law of multiple proportions.
- In carbon monoxide (CO), the carbon to oxygen mass ratio is 1:1, meaning that the mass of carbon and oxygen are identical.
- Carbon dioxide (CO2) has a carbon to oxygen content of 1:2, meaning that the mass of carbon is twice that of oxygen.
This observation complies with the law of multiple proportions since the mass ratios (1:1 and 1:2) are straightforward whole numbers.
State the Law of Multiple Proportions with Example.
The Law of Multiple Proportions states that “When two elements combine to form two or more compounds, the ratios of the masses of the combining element to the fixed element's mass are simple whole numbers.” It supports the idea that elements have distinct atomic masses and combine in predictable ways to form compounds with different properties.
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