Laws of Thermodynamics

What is the Third Law of Thermodynamics? The third law of thermodynamics states that the entropy of a perfect crystal at a temperature of zero Kelvin (absolute zero) is equal to zero. Entropy, denoted by ‘S’, is a measure of the disorder/randomness in a closed system. It is directly related to the number of microstates (a fixed microscopic state that can be occupied by a system) accessible by the system, i.e. the greater the number of microstates the closed system can occupy, the greater its entropy. The microstate in which the energy of the system is at its minimum is called the ground state of the system. At a temperature of zero Kelvin, the following phenomena can be observed in a closed system: The system does not contain any heat. All the atoms and molecules in the system are at their lowest energy points. Therefore, a system at absolute zero has only one accessible microstate – it’s ground state. As per the third law of thermodynamics, the entropy of such a system is exactly zero

Conclusion With this we’ve summarized the basics behind the Laws of Thermodynamics. This blog has but just scratched the surface, and there’s a lot of exciting science both to be learned and discovered in this field.  Thermodynamics is a very important field of study as it has implications from the machines we use to the internal machines that run in our bodies. It can be used to build more efficient engines and other stuff in the domains of physics. It can be used to discover new spontaneous reactions, create better chemicals, and improve methods of production of various industrial chemicals, by increasing energy efficiency.  Thermodynamic topics such as Gibbs Free Energy and Enthalpy, become important in biochemistry, especially in understanding the importance of enzymes, and why certain biochemical pathways and various catabolic and anabolic reactions take place in living systems. Thermodynamics is truly a robust and important field of study, with implications and applications every