What are three thermodynamic quantities that are not state functions and three that are?
See here for examples of state functions.
http://en.wikipedia.org/wiki/Thermodynamic_state#State_functions
See here where you note "processes" are non-state functions first reference).
http://www.google.com/search?q=thermodynamic+non-state+functions&ie=utf-8&oe=utf-8&aq=t&rls=org.mozilla:en-US:official&client=firefox-a
Thanks.
Three thermodynamic quantities that are not state functions are work (W), heat (Q), and path-dependent functions (e.g., heat transfer coefficient, friction coefficient, etc.).
Three thermodynamic quantities that are state functions are internal energy (U), enthalpy (H), and entropy (S).
To answer this question, let's first understand the concept of state functions in thermodynamics. State functions are properties that only depend on the current state of a system and are independent of the path taken to reach that state. On the other hand, non-state functions (also called path functions) depend on the path taken to reach a particular state.
Three examples of thermodynamic quantities that are not state functions include:
1. Heat (q): Heat is the transfer of energy between a system and its surroundings. It depends on the specific process or path taken to transfer the heat. For example, the amount of heat required to raise the temperature of a substance from A to B may differ depending on whether the heat is supplied slowly or quickly.
2. Work (w): Work is the energy transfer that occurs due to a mechanical process such as expansion or compression. Like heat, it is path-dependent and varies based on the specific process followed.
3. Enthalpy (H): Enthalpy is a thermodynamic quantity commonly used to represent the heat content of a system under constant pressure conditions. However, it is not a state function since it is influenced by both heat and work, which are path functions.
Now, let's consider three examples of thermodynamic quantities that are state functions:
1. Temperature (T): Temperature is a measure of the average kinetic energy of the particles in a system. It is a state function since it is solely determined by the state of the system and is independent of the path taken to reach that state.
2. Pressure (P): Pressure is a measure of the force exerted per unit area by a gas or a fluid. It is a state function because it only depends on the current state of the system, such as the number of molecules and their kinetic energies, regardless of how the system reached that state.
3. Internal Energy (U): Internal energy is the total energy of a system, including both its kinetic and potential energies. It is also a state function as it depends only on the current state of the system and not on the path taken to reach that state.
By understanding the concept of state functions and path functions, we can identify and differentiate between various thermodynamic quantities accordingly.