With the exception of non-crystalline solids ( glasses) the entropy of a system at absolute zero is typically close to zero. The third law of thermodynamics states that a system's entropy approaches a constant value as the temperature approaches absolute zero. Another form of the statement is that heat does not spontaneously pass from a colder body to a warmer body. The second law of thermodynamics states that in a natural thermodynamic process, the sum of the entropies of the interacting thermodynamic systems never decreases. The first law of thermodynamics states that, when energy passes into or out of a system (as work, heat, or matter), the system's internal energy changes in accord with the law of conservation of energy. The zeroth law of thermodynamics defines thermal equilibrium and forms a basis for the definition of temperature: If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other. A more fundamental statement was later labelled as the zeroth law, after the first three laws had been established. Traditionally, thermodynamics has recognized three fundamental laws, simply named by an ordinal identification, the first law, the second law, and the third law. In addition to their use in thermodynamics, they are important fundamental laws of physics in general, and are applicable in other natural sciences.

They state empirical facts that form a basis of precluding the possibility of certain phenomena, such as perpetual motion.

The laws also use various parameters for thermodynamic processes, such as thermodynamic work and heat, and establish relationships between them. The laws of thermodynamics define a group of physical quantities, such as temperature, energy, and entropy, that characterize thermodynamic systems in thermodynamic equilibrium.

Second law of thermodynamics definition