Which law states that mass cannot be created or destroyed during a chemical reaction?

The statement about mass not being able to be created or destroyed during a chemical reaction is known as the Law of Conservation of Mass. This fundamental principle, established by Antoine Lavoisier in the late 18th century, asserts that in a closed system, the total mass of the reactants equals the total mass of the products. During a chemical reaction, atoms are rearranged, but the total number of atoms remains constant, meaning that the mass is preserved throughout the process.

This law is crucial for understanding chemical reactions, as it helps predict the quantities of reactants and products involved. It also reinforces the idea that matter is neither created nor obliterated, but merely transformed from one form to another. Other options refer to different principles; for instance, the Law of Energy Conservation concerns the balance of energy, while the Law of Mass Action relates to the rates of chemical reactions based on concentrations of reactants and products. Understanding the Law of Conservation of Mass is essential for mastering concepts in chemistry and for balancing chemical equations correctly.