Laws of chemical combination
The number of chemical reactions takes place according to certain laws, termed as the Laws of chemical combination.
(1) Law of conservation of mass: This law was proposed by Lavoisier and verified by Landolt. In accordance to this law, Matter can neither be created nor be destroyed in the course of chemical reaction though it might change from one form to other. The total mass of the materials after a chemical reaction is same as the total mass before reaction.
(2) Law of constant or definite proportion: This law was proposed by Proust. According to this law, the pure chemical compound always contains the same elements combined together in the fixed ratio of their weights whatever its process of preparation may be.
(3) Law of multiple proportion : This law was proposed by Dalton and verified by Berzelius. In accordance to this law, When two elements A and B combine with each other to form more than one chemical compounds then different weights of A, which combine with the fixed weight of B, are in proportion of the simple whole numbers.
(4) Law of equivalent proportion or law of reciprocal proportion: This law was proposed by Ritcher. In accordance to this law, the weights of the two or more elements which separately react with the same weight of a third element are also the weights of these elements which react with each other or in simple multiple of them.
(5) Gay-Lussac's law: This law was proposed by Gay-Lussac and it is applicable only for the gases. In accordance to this law, when the gases combine with each other, they do so in volumes, which bear the simple ratio to each other and also to the product formed provided all gases are measured under the similar conditions. The Gay-Lussac's law, was based on the experimental observation.
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