The first law of thermodynamics, also known as the law of conservation of energy, states that energy cannot be created or destroyed in an isolated system; it can only change forms. Mathematically, it can be expressed as:
Where:
- ΔU represents the change in internal energy of the system.
- Q represents the heat added to the system.
- W represents the work done by the system.
The units for these quantities are as follows:
- ΔU (change in internal energy): joules (J) or calories (Cal)
- Q (heat): joules (J) or calories (Cal)
- W (work): joules (J) or calories (Cal)