What Is Entropy Change Definition Formula Units and Example Calculations
Thermodynamics is the study of the changes in energy associated with the change in temperature and heat. It also deals with the work done for the conversion of energy from one form to another. Three laws govern the science of thermodynamics and here we will discuss the second law of thermodynamics. The second law of thermodynamics talks about the concept of entropy and tells that the entropy of the universe is always increasing. By this law, the entropy of the universe can never be negative. So, let's understand this concept of entropy and the change in entropy.
Entropy
Entropy is the measure of disorder or randomness. This randomness could be in regards to the entire universe or a simple chemical reaction or something as simple as the heat exchange and heat transfer. The term disorder denotes the irregularity or lack of uniformity of a thermodynamic system.
The entropy is denoted by ‘S’ and it is an extensive property because the value of entropy or Entropy Change is dependent on the substance present in a thermodynamic system. Entropy is an interesting concept as it challenges the belief of complete heat transfer. It helps redefine the second law of thermodynamics.
Entropy relates to spontaneity i.e.; the more is the spontaneity in a thermodynamic process, the higher is its entropy or the degree of disorder. In simpler words, entropy gives us an idea about that portion of energy that does not convert into work done and adds to the disorder of the system instead. Since energy gives the ability to get work done, it is practically impossible for all the energy to be used in doing work. Entropy gives us a measure of that.
As is clear from the law of thermodynamics that energy can neither be created nor destroyed but can be converted from one form to another, it is not possible to signify entropy at a single point, and hence, it can be measured as a change. That is why we calculate the Entropy Change.
Entropy Change
Entropy Change can be defined as the change in the state of disorder of a thermodynamic system that is associated with the conversion of heat or enthalpy into work. A system with a great degree of disorderliness has more entropy.
Entropy is a factor of state function i.e., its value does not dependent on the pathway of the thermodynamic process and it acts as the determinant of only the initial and final state of the system. In the rule of chemical reactions, the changes in entropy occur as a result of the rearrangement of atoms and molecules that change the initial order of the system. This may either lead to an increase or a decrease in the randomness of the system and hence, will lead to an increase or a decrease in the entropy respectively.
Change in Entropy Formula Thermodynamics
The Entropy Change of a thermodynamic system is represented as ΔS. We can calculate the Entropy Change of a chemical reaction or a system by using the change in entropy formula:
ΔS = (Q/T)rev
Where,
Q is the heat transfer to or from the thermodynamic system
T is the absolute temperature.
The SI unit of Entropy Change is J/Kmol
Example:
The entropy of vaporization of water can be calculated by dividing the heat of vaporization with the boiling point i.e., 1000C or 373 K.
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Did You Know?
The physicist Clausius discovered the concept of entropy with the help of a steam engine and he coined the term entropy because it sounded similar to the word energy.
The formula for Entropy Changes of the universe can be denoted through the following change in the entropy equation:
ΔSuniverse = ΔSsystem+ ΔSsurrounding
This change in entropy formula provides an idea about the spontaneity of a process or a chemical reaction.
For a spontaneous process, there is an increase in entropy leading to ΔStotal being greater than zero.
Now let’s discuss further how does the change in entropy varies with different processes and conditions:
Entropy Change with Temperature:
Considering the formula for Entropy Change it is clear to conclude that the change in entropy is increased when heat transfer occurs at a lower temperature and the Entropy Change is more for the same at a higher temperature.
Entropy Change in a Reversible Process:
In conceptual terms, the Entropy Change definition applies to a reversible process. Thus, the change in entropy of the reversible process is the same as described above.
Entropy Change in an Irreversible Process:
From a practical point of view, no process can be an irreversible process is considered. As discussed above, the entropy is dependent only on the initial and final state of the system irrespective of the pathway of the thermodynamic process.
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Thus, the change in entropy is the same for an irreversible and a reversible process as it is independent of the pathway. This concept is also used in determining the Entropy Change for an ideal gas as it is an irreversible non-quasi static process.
Characteristics of Entropy
The important characteristics of the entropy of a thermodynamic system are as follows:
Entropy denotes the tendency of the universe to move towards disorder or randomness.
Entropy can be denoted as a function of the enthalpy or heat that can be converted into work.
Entropy depends on the mass of a thermodynamic system. It does not depend on the path of heat exchange or heat conversion and that is why it is an extensive property.
The entropy of the universe keeps increasing
The change in entropy for the adiabatic process is zero hence, it has constant entropy.
It is denoted by ‘S’ and has been formulated using the second law of thermodynamics. When spontaneous processes occur then this causes an increase in disorderness or randomness of the molecules present in the system. Thus, the entropy can be said to increase in all the processes that occur spontaneously. In simple terms, entropy is the measure of randomness or disorderness of the molecules that occur in a system.
More about Entropy
Entropy can be defined as the disorder or randomness that occurs in a system present in nature. It was first explained by scientist Clausius in the year of 1850 and has been used widely in the field of Chemistry. We’ll learn more about the concept of entropy and Entropy Changes on Vedantu and also learn problems related to this.
When we talk about entropy in thermodynamics, we look into its behavior instead of other details. It is related to other thermodynamic properties like pressure, temperature and heat. All the other factors are taken into consideration for the system’s equilibrium state. The phenomenon of entropy is also explained in statistics. It is used to define the molecular motions that occur in a system. Thus, in statistical definition, it is a molecular disorder measure.
When there is a presence of an isolated system then the entropy is also present at a higher rate thus, there is an increase in randomness or disorderness in the system. An isolated system is a closed system where there is no transfer of energy around its boundaries. Thus, there are no interactions of the system with the surroundings. One must remember that when there is a high temperature in the system then there is more randomness i.e. entropy as compared to the system where there is low temperature. This means that the entropy increases with a decrease in regularity. In addition, when a reaction occurs then we observe that there is a breakdown of these reactants into products and this causes an increase in entropy. The entropy order is: entropy is highest in gasses, followed by liquid and then lastly solids.
FAQs on Entropy Change in Thermodynamics Explained Clearly
1. What is entropy change in chemistry?
The entropy change (ΔS) is the measure of the change in disorder or randomness of a system during a chemical or physical process. It indicates how the distribution of energy and particles changes.
- If ΔS > 0, disorder increases (more randomness).
- If ΔS < 0, disorder decreases (more order).
- Entropy is a thermodynamic state function measured in J mol-1 K-1.
Entropy change is a key concept in thermodynamics and spontaneity of reactions.
2. What is the formula for entropy change?
The formula for entropy change at constant temperature is ΔS = qrev / T, where qrev is reversible heat and T is temperature in Kelvin.
- ΔS = entropy change (J K-1)
- qrev = heat absorbed reversibly (J)
- T = absolute temperature (K)
For reactions under standard conditions, the entropy change is calculated using ΔS° = ΣS°(products) − ΣS°(reactants).
3. How do you calculate entropy change for a chemical reaction?
The entropy change of a reaction is calculated using ΔS° = ΣS°(products) − ΣS°(reactants) with standard molar entropies.
- Step 1: Multiply each substance’s standard entropy (S°) by its stoichiometric coefficient.
- Step 2: Add values for all products.
- Step 3: Add values for all reactants.
- Step 4: Subtract reactants from products.
All values must be in J mol-1 K-1 and equations must be balanced before calculation.
4. Why does entropy increase when a solid turns into a gas?
Entropy increases when a solid turns into a gas because gas particles have much greater freedom of motion and randomness than solid particles.
- Solids have fixed positions and low disorder.
- Liquids have moderate movement.
- Gases move freely with maximum disorder.
For example, during vaporization of water: H2O(l) → H2O(g), the entropy change (ΔS) is positive because randomness increases.
5. What is the unit of entropy change?
The SI unit of entropy change is joules per kelvin (J K-1), and for molar entropy it is J mol-1 K-1.
- ΔS for a system: J K-1
- Standard molar entropy (S°): J mol-1 K-1
Temperature must always be expressed in Kelvin when calculating entropy change.
6. What is the relationship between entropy change and spontaneity?
Entropy change influences spontaneity through the Gibbs free energy equation: ΔG = ΔH − TΔS.
- If ΔG < 0, the process is spontaneous.
- A positive ΔS favors spontaneity.
- Higher temperature increases the effect of TΔS.
Thus, an increase in entropy often makes a reaction more thermodynamically favorable.
7. What happens to entropy when the number of gas molecules increases?
Entropy increases when the number of gas molecules increases because more particles create greater disorder.
- More moles of gas → more possible arrangements.
- Fewer moles of gas → lower entropy.
For example: CaCO3(s) → CaO(s) + CO2(g) shows a positive ΔS because gas is produced from solids.
8. What is standard entropy change (ΔS°)?
The standard entropy change (ΔS°) is the entropy change of a reaction when all substances are in their standard states at 1 bar pressure and a specified temperature (usually 298 K).
- Calculated using standard molar entropy values (S°).
- Uses the formula ΔS° = ΣS°(products) − ΣS°(reactants).
- Units: J mol-1 K-1.
Standard entropy values are obtained from thermodynamic data tables.
9. How does temperature affect entropy change?
Entropy increases with temperature because particles gain kinetic energy and move more randomly.
- Higher temperature → greater molecular motion.
- Lower temperature → reduced randomness.
- In ΔG = ΔH − TΔS, increasing T magnifies the effect of ΔS.
At higher temperatures, processes with positive ΔS become more favorable.
10. Can you give an example of entropy change in a chemical reaction?
An example of entropy change is the decomposition of ammonium nitrate: NH4NO3(s) → N2O(g) + 2H2O(g), where ΔS is positive.
- A solid decomposes into gaseous products.
- The number of gas molecules increases.
- Disorder increases significantly.
Because gases are more random than solids, this reaction shows a large positive entropy change.
