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# State Function

A state function is a thermodynamic quantity that depends only on the present state of a system and not on how the system arrived at that state. It describes the system’s equilibrium state. In contrast, a path function depends on how it arrived at the present state from a former state [1-4].

List of State Functions

• Pressure
• Temperature
• Volume
• Mass
• Internal Energy
• Gibbs Free Energy
• Entropy
• Enthalpy

## Equation

Consider a state function φ whose initial value is φ1 and the final value is φ2. Then, the change in the state function is given by [1-7]

Δφ = φ2 – φ1

Thus, the change in state function is the difference between its final value and initial value.

### Example

Suppose we have 1 M of helium gas that occupies a volume of 10 L at 300 K, which is the initial state. The gas is allowed to expand adiabatically to 20 L while its temperature changes to 500 K, which is the final state. Let us again go back to the initial state and allow the gas to expand isothermally at 300 K to 20 L. Note that the volume changed from 10 L to 20 L in both adiabatic and isothermal processes. Mathematically, this can be written as

ΔV = 20 L – 10 L = 10 L

Irrespective of how the gas expanded from its initial to the final value, the final volume is always 20 L. It implies that volume is a state function.

### Integral Form

The change in state function can also be expressed in integral notation. To evaluate the integral, one needs to know three things – the function, the lower limit, and the upper limit. In other words, integral highlights that state function depends on the initial and final values. Based on this concept, let us look at the expression for enthalpy (H) change in integral form.

∫H(t)dt = H(t2) – H(t1)

This equation is similar to the enthalpy change that we are familiar with.

ΔH = Hfinal – Hinitial

## State Function and Path Function [1-7]

### Similarities

• Both are thermodynamic quantities
• Both define the properties of a thermodynamic system

References