Entropy Study Guide
Entropy in everyday life is a crucial concept that you would come across while studying chemistry and physics. It is defined in various ways and serves various purposes.
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INTRODUCTION
Have you ever spent a day organizing your room only to find it back in the same state of disarray a few days or weeks later? Nature has the tendency to decline gradually from order to disorder and randomness, a concept known as entropy. Entropy is utilized in many fields, including cosmology, thermodynamics, economics, and chemistry. It exists not only in concept, but also as a measurable physical property that is always related to uncertainty in one way or another.
WHAT IS ENTROPY IN CHEMISTRY?
Entropy is the measurement of systemic disorder. It is considered an extensive property of a thermodynamic system, and its value changes depending on the amount of matter the system contains. The entropy of a system is the sum of all entropies within said system, and any change in entropy results from interactions between the system and its surroundings. In equations, entropy is represented by the letter “S” with the unit joules per kelvin (J/K). A system that is highly ordered has very low entropy.
REVERSIBLE PROCESS ENTROPY
In thermodynamics, a reversible process is a process that occurs between a system and its surroundings that can be reversed by a change in the properties of the surroundings, such as temperature or pressure. In a reversible process, the system remains in physical and chemical equilibrium, meaning its entropy value is always zero.
When it comes to calculating the entropy of a reversible process, there are quite a few assumptions to keep in mind (the assumption that each configuration within the process is equally probable for example). Considering the outcomes having equal probability, entropy equals Boltzmann’s constant multiplied by the natural logarithm of all possible numbers of states (W). In equation form, this is written as:
S = kB ln W
Where kB = 1.38065 × 10⁻²³ J/K.
ISOTHERMAL PROCESS ENTROPY
An isothermal process is a reversible process in which the temperature of the system remains constant as its pressure is increased. The change in entropy of an isothermal process is calculated by dividing the change in energy by the temperature of a system. In simpler terms, the change in entropy equals the change in heat. In equation form, this is written as:
ΔS = ΔQ / T
Where ΔQ = the change in the heat energy of the system (J), T = the absolute temperature of the system (K), and ΔS = the entropy of an isothermal process (J/K).
INTERNAL ENERGY AND ENTROPY
Internal energy is the energy contained within a thermodynamic system. It is an extensive property and thus cannot be measured directly. To find the value of a system’s internal energy, we can use the following equation:
ΔU = q + w
Where, ΔU = the change in the internal energy of a system, q = the heat energy exchanged between a system and its surroundings, and w = the work done by the system.
SECOND LAW OF THERMODYNAMICS AND ENTROPY
The second law of thermodynamics states that the total entropy within a closed system does not decrease. However, in a system, the entropy of one system could decrease while raising the entropy of another system.
EXAMPLES OF ENTROPY IN EVERYDAY LIFE
Melting ice is an excellent example of entropy. In the form of ice, water molecules exist in a fixed, highly-organized crystalline lattice structure. As ice melts, the water molecules become free to move and break away from their lattice structure into a state of relative disorder. In this scenario, the entropy of the ice increases.
CONCLUSION
- Entropy is regarded as the measurement of systemic disorder.
- An example of entropy is melting ice.
- Entropy is an extensive property.
- The SI unit of entropy is J/Kmol.
- To calculate the entropy of a reversible process, use the following equation: S = kB ln W
- To calculate the entropy of an isothermal process, use the following equation: ΔS = ΔQ / T
- To calculate internal energy, use the following equation: ΔU = q + w
FAQs
1. What is an example of entropy in everyday life?
Melting ice is an example of entropy in everyday life.
2. What are some examples of entropy?
Some examples of entropy would be the melting of ice, sugar dissolving, and a campfire.
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SOURCES:
- Example of Entropy: https://socratic.org/questions/what-is-an-example-of-entropy-from-everyday-life#:~:text=A%20campfire%20is%20an%20example,increasing%20entropy%20in%20your%20kitchen.Accessed 10th March 2022.
- Entropy in Chemistry: https://study.com/academy/lesson/entropy-in-chemistry-definition-lesson.html.Accessed 10th March 2022.
- What Is Entropy? https://www.thoughtco.com/definition-of-entropy-604458.Accessed 10th March 2022.
- Entropy: https://byjus.com/jee/entropy/.Accessed 10th March 2022.