Laws of Chemical Combination

Introduction to Law of Chemical Combination

Chemistry is the study of matter, the composition of matter, and the various forms in which matter can be found. Because of chemical reactions, matter can take on a variety of shapes and forms. Each of these chemical combinations of different elements and compounds is governed by a set of laws. For this reason, we always strive to achieve equilibrium in chemical equations.

In this article, we will provide you with the five fundamental rules of chemical combination that govern the chemical combinations of elements on the periodic table.

The Fundamental Laws of Chemical Combinations

The following are the five fundamental rules of chemical combination that apply to both elements and compounds.

1.The Law of Conservation of Mass (sometimes known as the Law of Conservation of Mass and Energy)

As stated in the Law of Conservation of Mass, “Mass in an isolated system can neither be created nor destroyed, but it can be converted from one form to another.” Antoine Lavoisier, a French chemist, was the first to use the term in 1789. In a chemical reaction, the mass of the reactants and the mass of the products will always be equal. According to this law, neither mass nor its destruction may be created or destroyed. This is the reason why we must always keep a chemical equation in equilibrium.

This means that the mass of the reactants and products generated are equivalent in mass for each chemical reaction or chemical change that takes place. Dalton’s atomic theory can provide an explanation for this law. To paraphrase Dalton’s atomic theory: “Atoms are indivisible particles that cannot be generated or destroyed during a chemical reaction.”

For Example  consider the formation of water.

2H2 + O2 →2H2O 

Mass of reactants = 4 + 32 = 36g

Mass of products = 2(2+16) = 2(18) = 36g

It is clear from the above Example  that the mass of the reactants and the mass of the product are identical in the reaction. As a result, the law of conservation of mass is demonstrated.

2.The Law of Definite Proportions 

Joseph Proust proposed the law of definite proportions in 1799, and it has been in use ever since. It is referred to as the law of constant proportions in some circles. According to this law, the constituents of a chemical substance are always present in specific proportions to one another in terms of mass. The law of constant proportions was also explained by John Dalton’s hypothesis, which was developed in the 18th century. According to John Dalton’s theory, the relative number and types of atoms in a given molecule remain constant over the course of time. As a result of this assertion, the law of constant proportions is supported.

Consider the following example: In a water molecule, the mass of hydrogen to the mass of oxygen is always the same, which is 1:8. Even though water molecules can be obtained from a variety of sources, the mass ratio of hydrogen to oxygen in a water molecule will always be one to eight.

3.The Law of Multiple Proportions

It was John Dalton who first proposed the law of multiple proportions in 1804. It is stated in this law that if elements combine to form two or more than two different kinds of compounds, then the masses of these elements included within these compounds are in a ratio of tiny whole numbers. Dalton’s atomic theory holds that compounds are formed when atoms join in a proportional ratio of small whole numbers.

Example:-Carbon, when combined with oxygen, generates two oxides: carbon monoxide (CO) and carbon dioxide (CO2) . The mass of carbon in each of these compounds (one molecule) is 12g (fixed), while the mass ratio of oxygen in both compounds CO and CO2 is 16:32 or 1:2, depending on the component.

4.Gay Lussac’s  Law of Gaseous Volumes

In 1808, Joseph Louis Gay-Lussac proposed the Law of Gaseous Volumes, which is still in use today. In accordance with this law, the ratio of the volumes of reacting gases is tiny whole numbers when measured at the same temperature and pressure as the reacting gases. This might be thought of as a variant of the law of definite proportions in a different context. This law applies in relation to volume, whereas the law of definite proportion applies in relation to mass.

5.The Law of Avogadro

Amedeo Avogadro established Avogadro’s law in 1811, . Equivalent quantities of gases at the same temperature and pressure, according to this law, contain identical amounts of moles of gas in each volume. It indicates that if two litres of oxygen and two litres of nitrogen are measured at the same temperature and pressure, they will have the same amount of moles.

CONCLUSION

In most cases, chemistry entails chemical reactions in which two or more components combine to form a single product. The 5 rules of chemical combination control reactions involving the combination of several components to generate a single molecule. The following are the five laws of chemical combination:

1.The law of mass conservation

2.Law of definite proportions law

3.Law of Multiple proportions law

4.The law of gaseous volumes of Gay Lussac

5.Avogadro’s law of chemical combination