Which concept explains the conservation of energy in thermodynamic processes?

The conservation of energy in thermodynamic processes is explained by the First Law of Thermodynamics. This law states that energy cannot be created or destroyed, only transformed from one form to another. In the context of thermodynamics, this means that the total amount of energy in a closed system remains constant, although it may change forms, such as from kinetic energy to thermal energy or vice versa.

When examining energy exchanges during thermodynamic processes, the First Law provides a foundational understanding of how energy flows and is conserved. For instance, when heat is added to a system, it can increase the internal energy of that system, perform work, or both. The principle assures that any energy entering or leaving the system can be accounted for, reinforcing the concept of energy conservation.

While the Second Law of Thermodynamics deals with the direction of energy transfers and the concept of entropy, and the Third Law relates to the behavior of systems as they approach absolute zero, it is the First Law that fundamentally encapsulates the idea of energy conservation in all thermodynamic contexts. The distinctions among these laws clarify various aspects of thermodynamic processes but do not negate the core principle of energy conservation highlighted by the First Law.