5 Basic Chemical Laws That Become Foundations For Various Experiments

Illustration of chemical experiments in school laboratories (Freepic)

YOGYAKARTA - Chemical basic law is an important concept that must be understood by every student who studies Chemical science. In the kima, various calculations involve very small substances or materials. Chemical basic law serves as a guideline so that calculations and analysis are carried out appropriately.

The following will be discussed 5 basic Chemical laws that became the foundation in various modern Kimia experiments and theories. The five laws include mass jurisprudence law, fixed comparison law, double comparison law, volume comparison law, and Avogadro hypothesis. Here's the explanation.

Chemical fundamental law helps determine the chemical formula of substances and explains the inter-element relation in Chemical reactions. Through these laws, scientists are able to understand how atoms interact and form compounds.

The mass hukum was first described by Russian scientist Mikhail Lomonosov in 1748. In his experiment, he showed that tin plates heated in closed containers did not experience mass changes.

The theory was then refined by Antoine Lavoisier in 1765. Lavoisier considered the mass of the substance before and after the Chemical reaction. He found that in a closed system, the mass of the substance before and after the reaction was the same.

This law was put forward by Joseph Proust in 1797 after conducting a series of experiments on various compounds. Proust found that each compound is always composed of elements with a fixed mass comparison.

For example, hydrogen and oxygen always form water with a ratio of 1:8 masses, no matter how much gas is used. These findings prove that each compound has a constant chemical composition.

John Dalton, a British scientist, developed this law based on the results of the Proust experiment. He found that if two elements form more than one compound, then the comparison of the mass of one of the elements that joins the mass remains another element is a simple integer.

For example, in nitrogen dioxide and nitrogen monoxide, the mass comparison is 2:1. This law strengthens Dalton's atomic theory which states that elements consist of small particles are not divided.

This law was discovered by Joseph Louis Gay-Lussac in 1808. It states that at the same temperature and pressure, the volume of the reaction gas and the gas the reaction results are compared as integers and simple ones.

For example, two volumes of hydrogen gas react with one volume of oxygen gas forming two volumes of water vapor. This law is an important basis in understanding gas reactions and strengthening the concept that gas particles have a proportional nature to their volume.

Amedeo Avogadro in 1811 stated that at the same temperature and pressure, the same volume of gas contains the same number of molecules. He also emphasized that elemental particles are not always in the form of single atoms, but can be in the form of molecules with two atoms or more.

For example, two hydrogen molecules react with one oxygen molecule producing two water molecules. This hypothesis then becomes the basis for calculating the number of particles in one mol of a substance known as the Avogadro number.

Those are the 5 basic laws of Chemistry and their explanations. By understanding the basic chemical law, students can understand the concept of calculation and chemical reactions more easily.