Thermodynamic Properties
Thermodynamic Properties :
- Thermodynamic Properties Are Measurable Characteristics That
Describe The State And Behavior Of A System Thermodynamics.
- These Properties Help In Understanding And Predicting The
Energy Transfers, Equilibrium Conditions, And Transformations
That Occur Within A System.
- Thermodynamic Properties May Be Extensive Or Intensive.
- Intensive Properties Are Properties That Do Not Depend On The
Quantity Of Matter. Pressure And Temperature Are Intensive
Properties.
- In The Case Of Extensive Properties, Their Values Depends On
The Mass Of The System. Volume, Energy, And Enthalpy Are
Extensive Properties.
Enthalpy :
- Definition:
Enthalpy, Represented By The Symbol H, Is A Thermodynamic
Property That Measures The Total Heat Content Of A System. It
Includes The Internal Energy Of The System And The Work
Done By Or On The System.
- Hess's Law:
Enthalpy Follows Hess's Law, Which States That The Enthalpy
Change Of A Reaction Is Independent Of The Pathway Taken.
This Principle Allows For The Determination Of Enthalpy
Changes By Combining Known Enthalpy Changes Of
Intermediate Steps Or Reactions.
- Endothermic And Exothermic Processes:
Enthalpy Change Allows Us To Classify Processes Or Reactions
As Endothermic Or Exothermic. An Endothermic Process
Absorbs Heat From The Surroundings, Resulting In A Positive
∆H Value.Conversely, An Exothermic Process Releases Heat To
The Surroundings, Resulting In A Negative ∆H Value.
- Mathematically, The Enthalpy, H, Equals The Sum Of The
Internal Energy, E, And The Product Of The Pressure, P, And
Volume, V, Of The System.
H = E + Pv
- The Equation H = E + Pv Is Widely Used In Various Applications
Of Thermodynamics, Such As Analyzing Chemical Reactions,
Energy Transfer In Systems, And Heat Exchange Processes.
Entropy :
- Definition:
Entropy, Typically Represented By The Symbol S, Is A
Thermodynamic Property That Quantifies The Degree Of
Disorder Or Randomness In A System. It Is A Measure Of The
Distribution Of Energy Within A System.
- Microscopic Disorder:
Entropy Is Associated With The Number Of Microstates Or
Arrangements That Are Available To A System At A Given
Macroscopic State. It Represents The Uncertainty Or Lack Of
Knowledge About The Exact Arrangement Of Particles Within
The System.
- Second Law Of Thermodynamics:
Entropy Is Central To The Second Law Of Thermodynamics,
Which States That The Entropy Of An Isolated System Tends To
Increase Over Time. This Is Often Expressed As The Statement
That The Total Entropy Of The Universe Always Increases In A
Spontaneous Process.
- Example: The Entropy Of A Solid, Where The Particles Are Not
Free To Move, Is Less Than The Entropy Of A Gas, Where The
Particles Will Fill The Container.
Thermodynamic Potentials :
- Thermodynamic Potentials Are Mathematical Functions That
Provide A Convenient Way To Describe And Analyze The
Behavior Of Thermodynamic Systems.
- They Are Derived From The Fundamental Thermodynamic
Properties And Are Used To Determine The Equilibrium
Conditions, Energy Transfers, And Other Important Aspects Of A
System.
- Four Primary Thermodynamic Potentials
( 1 ) Internal Energy (U):
- The Internal Energy Represents The Total Energy Of A System
Due To The Microscopic Motions And Interactions Of Its
Particles.
- It Includes The Kinetic And Potential Energies Of The Particles.
- The Internal Energy Is A Fundamental Thermodynamic
Potential That Describes The System's Energy Content.
( 2 ) Enthalpy (H):
- Enthalpy Is Defined As The Sum Of The Internal Energy (U) And
The Product Of The Pressure (P) And Volume (V) Of The
System.
- It Is Particularly Useful For Constant-Pressure Processes And
Accounts For The Work Done By Or On The System.
- Enthalpy Helps Analyze Heat Transfer And Energy Changes
During Processes.
- Enthalpy [H = U + Pv]
( 3 ) Helmholtz Free Energy (F):
- The Helmholtz Free Energy Is Denoted By The Symbol F And Is
Defined As The Difference Between The Internal Energy (U) And
The Product Of The Temperature (T) And Entropy (S) Of The
System.
- It Is A Thermodynamic Potential That Describes The Maximum
Useful Work That Can Be Obtained From A System At Constant
Temperature And Volume.
- The Helmholtz Free Energy Is Often Used To Analyze Systems
In Equilibrium And Determine The Conditions For Stability.
- Helmholtz Free Energy [F = U – Ts]
( 4 ) Gibbs Free Energy (G):
- The Gibbs Free Energy, Represented By The Symbol G, Is
Defined As The Difference Between The Enthalpy (H) And The
Product Of The Temperature (T) And Entropy (S) Of The System.
- It Is A Thermodynamic Potential That Determines Whether A
Process Or Reaction Is Thermodynamically Favorable Or
Spontaneous.
- The Gibbs Free Energy Is Particularly Useful In Constant-
Pressure And Constant-Temperature Conditions And Is Used To
Predict The Direction And Feasibility Of Chemical Reactions.
- Gibbs Free Energy [G = U + Pv – Ts]
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