The first law of thermodynamics, also known as the law of energy conservation, is a fundamental principle in the field of thermodynamics. It states that energy cannot be created or destroyed in an isolated system. Instead, energy can only be transferred or transformed from one form to another.
Mathematically, the first law of thermodynamics can be expressed as:
ΔU = Q - W
where:
- ΔU represents the change in the internal energy of the system,
- Q represents the heat transferred to the system, and
- W represents the work done by the system.
According to this equation, the change in the internal energy of a system is equal to the heat added to the system minus the work done by the system. In other words, any increase in the internal energy of a system can be accounted for by the heat supplied to the system and the work performed by the system.
The first law of thermodynamics essentially states that energy is conserved within a closed system, and it provides a fundamental understanding of the relationship between heat, work, and the internal energy of a system. It serves as a cornerstone in the study and application of thermodynamics, helping to analyze and understand various energy-related processes and phenomena.