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First Law of Thermodynamics
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The First Law of Thermodynamics, also known as the Law of Energy Conservation, states that:
Energy cannot be created or destroyed; it can only be transformed from one form to another or transferred from one system to another.
In the context of thermodynamics, the First Law can be mathematically expressed as:
ΔQ = ΔU + ΔW

Where:
ΔQ = Heat added to the system
ΔU = Change in the internal energy of a system
ΔW = Work done by the system on its surroundings

Key Points:
1. Internal Energy U: Refers to the total energy contained within a system, including kinetic and potential energy at the molecular level.
2. Heat Q: Energy transferred between the system and its surroundings due to a temperature difference.
3. Work W: Energy transferred when the system exerts force on its surroundings (e.g., expansion of a gas).

This law emphasizes that the total energy of an isolated system remains constant, ensuring that all energy exchanges are accounted for in physical and chemical processes.

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