Introduction:
The first law of thermodynamics is a fundamental principle in physics that describes the conservation of energy in a closed system. It states that the total energy of an isolated system remains constant, i.e., energy cannot be created or destroyed; it can only be transformed or transferred from one form to another.
Let's break down this law and understand it in more detail
- Internal Energy: The internal energy of a system is the sum of all the kinetic and potential energies of its molecules. According to the first law of thermodynamics, 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
Where, ΔU: change in internal energy Q: heat added to the system W: work done by the system
- 2.Heat: Heat is a form of energy that flows from hotter to cooler objects. When heat is added to a system, it increases the internal energy of the system.
3.Work: Work is the energy transferred to or from a system through the application of a force over a distance. When work is done by a system, it decreases the internal energy of the system.
4.Law of conservation of energy: The first law of thermodynamics is based on the law of conservation of energy, which states that energy cannot be created or destroyed, only transformed from one form to another. Therefore, the total energy of an isolated system remains constant.
5.Applications: The first law of thermodynamics has many applications in our daily lives. For example, it is used in the design of engines, refrigerators, air conditioners, and power plants.
In conclusion, the first law of thermodynamics is a fundamental principle that describes the conservation of energy in a closed system. It states that the total energy of an isolated system remains constant, and 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.
First Law Of Thermodynamics Notes
By aswin aryal
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