Chemistry - Principles of Modern Chemistry - Chemical Laws

Chemical Laws

Main article: Chemical law

Chemical reactions are governed by certain laws, which have become fundamental concepts in chemistry. Some of them are:

  • Avogadro's law
  • Beer-Lambert law
  • Boyle's law (1662, relating pressure and volume)
  • Charles's law (1787, relating volume and temperature)
  • Fick's law of diffusion
  • Gay-Lussac's law (1809, relating pressure and temperature)
  • Le Chatelier's Principle
  • Henry's law
  • Hess's Law
  • Law of conservation of energy leads to the important concepts of equilibrium, thermodynamics, and kinetics.
  • Law of conservation of mass continues to be conserved in isolated systems, even in modern physics. However, special relativity shows that due to mass-energy equivalence, whenever non-material "energy" (heat, light, kinetic energy) is removed from a non-isolated system, some mass will be lost with it. High energy losses result in loss of weighable amounts of mass, an important topic in nuclear chemistry.
  • Law of definite composition, although in many systems (notably biomacromolecules and minerals) the ratios tend to require large numbers, and are frequently represented as a fraction.
  • Law of multiple proportions
  • Raoult's Law

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