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Definition of a system in thermodynamics
A system is the part of the universe being observed, while the surroundings include everything outside the system.
The universe= The system + The surroundings
What is a system?
A thermodynamic system is a specific portion of matter or space chosen for analysis, which can exchange energy or matter with its surroundings.
Types of system
Open System: An open system allows for the transfer of both energy and matter between the system and its surroundings. This type of system is common in natural processes, such as a boiling pot of water or a car engine, where heat energy and matter (e.g., steam or exhaust) are exchanged with the environment.
Closed System: A closed system can exchange energy but not matter with its surroundings. In a closed system, the total mass remains constant, but energy can flow in or out. An example of a closed system is a sealed container of gas, where heat can be added or removed, but the gas itself cannot escape or enter.
Isolated System: An isolated system does not exchange either matter or energy with the surroundings. This type of system is idealized in thermodynamics since it assumes perfect insulation. An example of an isolated system is a thermos bottle in a perfect environment, where neither heat nor substances enter or leave.
What is a state functions in thermodynamics?
1) A state function is a property whose value depends only on the state of the system, not on the path taken to reach that state. Examples include temperature, pressure, and volume.
on what factors does the state function depend on?
2) State functions depend only on the current state of the system, whereas path functions depend on the specific pathway taken to reach a certain state. For example, work and heat are path functions because their values can change based on the process used.
Examples of state functions
1) Temperature 2) Pressure 3) Volume 4) Internal Energy 5) Enthalpy 6) Gibbs Free Energy
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