Law of Multiple Proportions
According to the Law of Multiple Proportions, If two elements combined to form more than one compound under different circumstances, then the ratio of the masses for one element when second mass is fixed for all different compounds is always a small whole number.
The Law of Multiple Proportions is also known as Dalton’s Law, as it was first proposed by Dalton in the year 1804. This law doesn’t hold for non-stoichiometric compounds as well as heavy molecules such as polymers and oligomers.
Example of Law of Multiple Proportions
Carbon and oxygen combine to form two distinct compounds (under different circumstances). The first is the most common gas, CO2 (Carbon dioxide), and the second is CO (Carbon monoxide).
Lets take 12 grams of carbon, and by the calculation of moles we can find that it reacts with 16 grams of Oxygen to make Carbon Monoxide and with 32 grams of oxygen to form Carbon dioxide.
As a result, the ratio of mass of oxygen in the first and second compounds is 2:1 = 32/16 = 2, (whole number).
Laws of Chemical Combination
Laws of Chemical Combination are one of the most fundamental building blocks of the subject of chemistry. As in our surrounding different matter reacts with each other and form various kind of different substances. Laws of Chemical Combination are the collection of laws that explains how these substances combine together to form anything at all. When matter reacts with another matter, a chemical reaction happens which changes the form, properties, or characteristics of the matter drastically. This interaction of matter with each other is governed by the Laws of Chemical Combination.
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