State Function Vs Path Function
The key differences between State Function and Path Function are given as follows:
Difference Between State Function and Path Function | ||
|---|---|---|
Aspect | State Function | Path Function |
Definition | A state function is a property that depends only the current state and not on the path taken to reach that state. | A path function is a property that depends on the path taken to reach a particular state. |
| Different paths give the same value of the system. | Different paths give different values of the system. |
Integration | State function can be integrated using the initial and final values of the thermodynamic property of the system. | Path function requires multiple integrals and limits of integration to integrate the property. |
Mathematical Representation | ΔU, ΔH, ΔS etc. | δW , δQ etc. |
Expressions | Basically represented by equations or mathematical relations. | Depends on the specific process or path. |
Example | Temperature, Pressure, Volume, Internal energy, enthalpy, entropy etc. | Work, Heat and other energy transfer forms. |
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State Functions
State Functions are the functions that are independent of the path of the function i.e. they are concerned about the final state and not how the state is achieved. State Functions are most used in thermodynamics. In this article, we will learn the definition of state function, what are the state functions in Thermodynamics, and how they differ from path function.
Table of Content
- What are State Functions?
- Examples of State Functions in Thermodynamics
- Equation of State Function
- State Function Vs Path Function
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