Students should understand the importance of entropy law as it is very helpful for studying physics. Entropy can be explained in numerous ways. The applications of entropy are useful in thermodynamic stages.
In 1850, Rudolf, a German physicist, named its entropy. Entropy is a measurement of disorder or randomness found in a system. Many definitions are associated with entropy. In this article, we will know about two definitions of entropy, such as thermodynamic definition as well as statistical definition.
We will now understand the three laws associated with thermodynamics.
The first law of thermodynamics relating to entropy
The second law of thermodynamics in terms of entropy
The third law of thermodynamics in terms of entropy
This law states that heat is one type of energy that cannot be produced or neither be ruined. Well, thermodynamic processes are there that always consider a state i.e., conservation of energy.
However, heat can be transferred from one place to another, and this sort of energy is only convertible from one form to another.
Some miscellaneous facts on the first law of thermodynamics
We notice a surge of entropy when there is a change of state of the mater.
Also, we encounter the rise of entropy when the number of moles of gaseous products rises more than reactants.
Some specific points are there that can illustrate the entropy and second law of thermodynamics.
Natural or spontaneous processes are irreversible in terms of thermodynamics.
Entropy second law of thermodynamics states that the transfer of heat into work is not possible without wasting a certain amount of energy.
The entropy level for the universe is surging continuously.
2nd law of thermodynamics entropy: ∆Stotal =∆Ssurroundings+∆Ssystem >0
The overall sum of the entropy of the system and the surrounding will be above zero.
When the temperature of any solid crystalline has an absolute temperature, then the entropy will appear towards zero. This happens only due to a perfect order that exists in a crystal at absolute zero.
This law has a limitation that it is only applicable for the solid substances which do not have zero entropy at absolute zero such as glassy solid, solid containing a mixture of isotopes.
When you talk about the entropy of vaporization, the definition for it can be given as the upsurge of entropy due to the change of a liquid into vapours.
This phenomenon is happening only due to the rise of molecular movement. This behaviour manifests randomness of motion.
The entropy of vaporization can be stated as the ratio of the enthalpy of vaporization and its boiling point.
It can be represented as ∆vap S = ∆vap H / Tb
Chemical reactions that have Exothermic behaviour possess Spontaneity because ∆Ssurr is positive. This allows the value ∆Stotal to remain positive.
Some of the Endothermic reactions are spontaneous.
It happens due to ∆Ssystem is positive only. Though ∆Ssurroundings is negative but complete ∆Stotal is positive.
The standards for the change in Free energy are always there for forecasting spontaneity. This concept is superior to entropy change criteria.
This is due to some important requirements that stand only for the free energy change of the system. However, some of the free energy also needs entropy change of both system and surroundings.
Entropy evolves numerous ideas when it comes to nature tending from order to disorder states. It means, the right-hand-side box of molecules existed before the left-side molecules
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Entropy is one of the thermodynamic properties that help us to measure the disorder of a system in detail. We can conclude that when we notice any heat transfer from higher to the lower temperature, the magnitude of entropy decreases. However, in the opposite case, the entropy value increases.
Q1. What is the Reason Behind the Entropy Constant at the Triple Point of Water?
Ans: Do you know what the triple point is? This is a point where the simultaneous equilibrium between the solid, liquid, and gas phases exist. The entropy of the liquid phase is lower than the entropy of the gas phase and is the reason why entropy is constant at the triple point of water.
Q2. Is there Any Chance of an Increase in Entropy at a Freezing Point?
Ans: Yes, entropy will increase. Water has a greater entropy than ice. We know that entropy is in favour of melting, and freezing works as an exothermic process.
So, the amount of energy that is lost from the water will move away to the surroundings. Therefore, it promotes a higher entropy value.
Q3. When Can Entropy Decrease?
Ans: It is impossible for entropy to decrease as the total entropy of the universe can never decline from a certain value. It may be possible somewhere.
Q4. What is the Possibility for Infinite Entropy Value?
Ans: This is impossible as the entropy of the system can’t be infinite. This is because there is no finite system that can have an infinite number of microstates. Entropy always promotes along with the finite maximum values for a system that approaches equilibrium.