
The second law of thermodynamics asserts that the total entropy of an isolated system can never decrease over time.The second law of thermodynamics says that in nature everything tends to disorder. Imagine a room: you can tidy it up, but without effort it will become messy again. This law states: entropy (a measure of chaos) in a closed system never decreases. Heat always flows from hot to cold, and it is impossible to completely convert heat into useful work without losses.
In 1824, Sadi Carnot, in his work 'Reflections on the Motive Power of Fire', laid the foundations of thermodynamics by introducing the concept of an ideal cycle. In 1850, Rudolf Clausius gave the first formulation and introduced the concept of entropy. In 1851, Lord Kelvin (William Thomson) proposed an alternative formulation. Later, Max Planck and others generalized the law, linking it to molecular statistics.
Applied everywhere: from designing heat engines to climate prediction and cosmology. Limits: fluctuations in small systems can temporarily violate the increase in entropy, but statistically it holds. For open systems, entropy can decrease locally at the expense of the environment.
Precisely because of this law, a perpetual motion machine of the second kind is impossible: part of the energy always dissipates as heat that cannot be recovered.






























