Internal energy changes relate to heat and work from "summary" of Thermodynamics and an Introduction to Thermostatistics by Herbert B. Callen
The concept of internal energy changes in a system is intimately connected to the concepts of heat and work. When a system undergoes a process, its internal energy changes as a result of the transfer of energy into or out of the system in the form of heat and/or work. Heat is the transfer of energy between a system and its surroundings due to a temperature difference. When heat flows into a system, it increases the internal energy of the system, causing its temperature to rise. On the other hand, when heat flows out of a system, its internal energy decreases, leading to a decrease in temperature. Work, on the other hand, is the transfer of energy between a system and its surroundings due to a non-temperature-related mechanism, such as compression or expansion. When work is done on a system, its internal energy increases, while when work is done by a system, its internal energy decreases. The first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system, encapsulates the relationship between internal energy changes, heat, and work. This law allows us to quantify the internal energy changes in a system based on the heat and work interactions it undergoes. By understanding how internal energy changes relate to heat and work, we can gain valuable insights into the behavior of thermodynamic systems and predict how they will respond to various processes and interactions. This knowledge forms the foundation of thermodynamics and allows us to analyze and manipulate energy transfers in a wide range of practical applications.
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