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Brian Curtis
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Why does there tend to be disagreement on an irreversible adiabat entropy determination? Doesn't an irreversible adiabatic expansion increase the entropy of a system by the Clausius inequality?
That's what I've thought. It can be proved by determining entropy through a reversible cycle. However, in class, it was mentioned on an assignment that the delta S is negative and not spontaneous. Which again, does not make senseLet'sthink said:Total entropy of an isolated system or of Universe increases when the isolated system or universe undergoes irreversible adiabatic process.
An adiabatic irreversible process is a thermodynamic process that occurs without any heat exchange with the surroundings, and is not reversible. This means that the system's entropy increases during the process, and it cannot return to its initial state without external intervention.
In an adiabatic reversible process, the system is able to return to its initial state without any change in entropy. This is because the process is carried out slowly, allowing the system to maintain thermodynamic equilibrium at all times. In contrast, an adiabatic irreversible process occurs quickly and does not allow the system to reach equilibrium, resulting in an increase in entropy.
Some common examples of adiabatic irreversible processes include free expansion of a gas into a vacuum, sudden compression of a gas, and mixing of two gases without thermal contact. These processes occur quickly and do not allow the system to reach equilibrium, resulting in an increase in entropy.
During an adiabatic irreversible process, the internal energy of a system may change due to work being done on or by the system. However, there is no heat transfer involved, so the change in internal energy is solely due to work. The change in internal energy can be calculated using the first law of thermodynamics, which states that the change in internal energy is equal to the work done on or by the system.
No, an adiabatic irreversible process cannot be reversed. This is because the process occurs quickly and does not allow the system to reach equilibrium, resulting in an increase in entropy. In order to reverse the process, external intervention would be required to decrease the system's entropy, which goes against the second law of thermodynamics.