The law of definite proportions states that the samples of a compound will always contain the same proportion of elements by mass. The Law of Definite Proportions vs. The Law of Multiple Proportions The Law of Definite Proportions (or Proust's Law) states that in a single chemical compound (such as H 2 O or CO) the ratio of it's component elements is a fixed whole number ratio. It is different from the Law of Multiple Proportions although both stem from Lavoisier's Law of Conservation of Mass. This law, together with the law of multiple proportions, is the basis for stoichiometry in chemistry. For example, in water (H 2 O) the ratio of hydrogen to oxygen is 2:1 (sometimes written 2/1). The Law of Constant Composition, discovered by Joseph Proust, is also known as the Law of Definite Proportions. On the contrary, the law of multiple proportions states that if two elements combine to form more than one chemical … The law of definite proportions and law of multiple proportions are used to explain the stoichiometry of compounds in chemical reactions. This implies that any pure sample of a compound, no matter the source, will always consist of the same elements that are present in the same ratio by mass.
The law of constant proportions states that chemical compounds are made up of elements that are present in a fixed ratio by mass. In chemistry, the law of constant composition (also known as the law of definite proportions) states that samples of a pure compound always contain the same elements in the same mass proportion.
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