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.

What are State Functions?

State function is a property that only depends on the current state and not on the path taken to reach that state.

In other words, it doesn’t matter how you got there, just where you are. It provides valuable information about the state without requiring knowledge of the previous changes that led to the current state.

Examples of State Functions in Thermodynamics

State functions are crucial in thermodynamics as they provide a way to describe and analyze systems without having to consider the specific process that occurred. Here are some important state function examples commonly considered in thermodynamics:

• Temperature
• Pressure
• Volume
• Internal Energy
• Gibb’s Free Energy
• Entropy
• Enthalpy

Temperature (T)

Temperature is a measure of the average kinetic energy of the particles in a system. It is a state function because it describes the current state of the system, irrespective of the path taken to reach that state.

Pressure (P)

Pressure is the force applied per unit area on a surface. It is a state function as it only depends on the current state of the system. Pressure is an essential parameter to determine the behavior of gases and fluids in various thermodynamic processes.

Volume (V)

Volume refers to the amount of space occupied by a substance or system. In thermodynamics, volume is an essential parameter in determining the behaviors of gases and fluids, especially in processes involving expansion or compression.

Internal Energy(U)

Internal energy represents the total energy stored within a system, surrounding the kinetic and potential energies of its particles. Internal energy is crucial in understanding the energy transfers and changes within a system during various thermodynamic processes.

The Internal Energy is given by the following equation:

ΔU=Q-W

where ΔU represents the change in internal energy, Q is the heat added to the system, and W is the work done by the system.

Enthalpy(H)

Enthalpy is the total heat content of a system at constant pressure. It includes the internal energy of the system and the work required to move the system’s surroundings.

Enthalpy is a state function as it depends only on the current state of the system, regardless of the path taken to achieve that state. It is particularly useful in studying heat transfer processes and chemical reactions.

The Enthalpy is given by the following equation:

ΔH = ΔU + PΔV

where ΔV represents the change in volume and P is the pressure.

Entropy(S)

Entropy is a measure of the disorder or haphazardness within a system. It is a state function as it depends only on the current state of the system, irrespective of the path taken to achieve that state.

Entropy provides valuable information about the direction and extent of spontaneous processes and is a fundamental concept in understanding thermodynamic equilibrium.

Gibbs Free Energy(G)

The Gibbs free energy, denoted by the symbol “G,” predicts whether a chemical or physical process will occur spontaneously at constant temperature and pressure. It combines enthalpy, entropy, and temperature into a single equation. If the Gibbs free energy is negative, the process is spontaneous, indicating that the system tends to move towards a lower energy state.

Gibbs free energy is a state function as it depends only on the current state of the system, regardless of the path taken to achieve that state.

It is commonly used in chemical reactions and phase transitions to predict the possibility and direction of such processes.
The Gibb’s Free Energy is given by the following equation:

ΔG = ΔH – TΔS

where ΔS refer to the change in entropy and T is the temperature.

Equation of State Function

State functions can be measured as integrals because integrals depend on only the function, its lower limit and upper limit. In the same way, state functions also depend on the property, its initial value and final value.

Consider a state function integral of enthalpy H, and t₀ represents the initial state and t₁ represents the final state is given by the following equation:

This equation is similar to the equation of enthalpy:

ΔH = H _final − H _initial

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

State Function Vs Path Function

The key differences between State Function and Path Function are given as follows:

Read More,

• Thermodynamics
• Thermodynamic Processes
• Thermodynamic Cycles

State Function – Solved Examples

Problem 1: The entropy of a system increase from 69 j/k to 96 j/k during system process. Now find the entropy change for this process.

Solution:

Entropy change ( ΔS)=S _final – S _initial

ΔS= 96 – 69 j/k = 27 j/k

Problem 2: The initial internal energy of a system is 200 J, and the final internal energy is 350 J. Calculate the change in internal energy (ΔU) .

Solution:

Internal energy (ΔU) = U_final -U_initial

ΔU=350J−200J=150J

Problem 3: Given that the enthalpy of a system changes from 450 kJ to 700 kJ during a certain process, Calculate the enthalpy change (ΔH) .

Solution:

Enthalpy (ΔH) = H_final -H_initial

ΔH=700kJ−450kJ=250kJ

State Function – FAQs

1. What is State Function?

A state function is a property that depends only the current state and not on the path taken to reach that state.

2. What is Path Function?

A path function is a property that depends on the path taken to reach a particular state.

3. What is the Difference Between a State and a Path of Function?

A state function depends only on the current state of the system ,while path functions describe the changes that occur during a specific process and depend on the path taken.

4. What is Gibbs Free Energy?

Gibbs free energy is a measure of the maximum work that can be obtained from a system at constant temperature and pressure. It combines enthalpy and entropy to determine the spontaneity of a process.

5. What are State Functions in Thermodynamics?

State Functions in Thermodynamics are Temperature, Enthalpy, Entropy, Pressure, Volume, Internal Energy, Gibbs Free Energy

6. Give an Example of Path Function.

An example of a path function is Heat. It depends on the path taken to reach a particular state.