Law of Constant Composition - Chemistry Definition

Understand the Law of Constant Composition (Law of Definite Proportions)

scientist holding model of chemical structure
According to the Law of Constant Composition, all samples of a compound contain the same mass ratios of atoms of the elements. Rafe Swan / Getty Images

Law of Constant Composition Definition

The law of constant composition is a chemistry law which states samples of a pure compound always contain the same elements in the same mass proportion. This law, together with the law of multiple proportions, is the basis for stoichiometry in chemistry.

In other words, no matter how a compound is obtained or prepared, it will always contain the same elements in the same mass proportion.

For example, carbon dioxide (CO2) always contains carbon and oxygen in a 3:8 mass ratio. Water (H2O) always consists of hydrogen and oxygen in a 1:9 mass ratio.

Also Known As: Law of Definite Proportions, Law of Definite Composition, or Proust's Law

Law of Constant Composition History

Discovery of this law is credited to the French chemist Joseph Proust. He conducted a series of experiments from 1798 to 1804 that led him to believe chemical compounds consisted of a specific composition. Keep in mind, at this time most scientists thought elements could combine in any proportion, plus Dalton's atomic theory was just beginning to explain each element consisted of one type of atom.

Law of Constant Composition Example

When you work chemistry problems using this law, your goal is to look for the closest mass ratio between the elements. It's okay if the percentage is few hundredths off! If you're using experimental data, the variation might be even larger.

For example, let's say you want to demonstrate, using the law of constant composition that two samples of cupric oxide abide by the law. The first sample was 1.375 g cupric oxide, which was heated with hydrogen to yield 1.098 g of copper. For the second sample, 1.179 g of copper was dissolved in nitric acid to produce copper nitrate, which was then burned to produce 1.476 g of cupric oxide.

To work the problem, you need to find the mass percent of each element in each sample. It doesn't matter whether you choose to find the percent of copper or of oxygen. You would just subtract one value from 100 to get the percent of the other element.

Write down what you know:

In the first sample:

copper oxide = 1.375 g
copper = 1.098 g
oxygen = 1.375 - 1.098 = 0.277 g

percent oxygen in CuO = (0.277)(100%)/1.375 = 20.15%

For the second sample:

copper = 1.179 g
copper oxide = 1.476 g
oxygen = 1.476 - 1.179 = 0.297 g

percent oxygen in CuO = (0.297)(100%)/1.476 = 20.12%

The samples follow the law of constant composition, allowing for significant figures and experimental error.

Exceptions to the Law of Constant Composition

As it turns out, there are exceptions to this rule. Non-stoichiometric compounds exist which exhibit a variable composition from one sample to another. An example is wustite, a type of iron oxide that may contain 0.83 to 0.95 iron per each oxygen.

Also, because there are different isotopes of atoms, even a normal stoichiometric compound may display variations in mass composition, depending which isotope of the atoms is present. Typically, this difference is relatively small, yet it does exist and can be important.

The mass proportion of heavy water compared with regular water is an example.

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Helmenstine, Anne Marie, Ph.D. "Law of Constant Composition - Chemistry Definition." ThoughtCo, Sep. 3, 2017, thoughtco.com/law-of-constant-composition-chemistry-605850. Helmenstine, Anne Marie, Ph.D. (2017, September 3). Law of Constant Composition - Chemistry Definition. Retrieved from https://www.thoughtco.com/law-of-constant-composition-chemistry-605850 Helmenstine, Anne Marie, Ph.D. "Law of Constant Composition - Chemistry Definition." ThoughtCo. https://www.thoughtco.com/law-of-constant-composition-chemistry-605850 (accessed November 19, 2017).