A Free expansion of an ideal gas and changes in entropy

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For a freely expanding ideal gas undergoing an irreversible transformation, the change in entropy is equivalent to that of a reversible transformation between the same initial and final states. This is due to the definition of entropy, which is based on the integral of heat transfer divided by temperature over a reversible process. In free expansion, there is no work done or heat flow, so the internal energy remains constant, and the temperature does not change. The reversible path involves a quasi-static expansion with heat flow to maintain constant temperature, leading to a positive change in entropy. Thus, the change in entropy for an irreversible process can still be calculated using the same principles as for a reversible process.
Ahmed1029
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For a freely expanding ideal gas(irreversible transformation), the change in entropy is the same as in a reversible transformation with the same initial and final states. I don't quite understand why this is true, since Clausius' theorm only has this corrolary when the two transformations are reversible. Anyone can help?
Edit : the transformations are also isothermal, no change in temperature during any of the transformations
 
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Do you think that the change in entropy for a gas experiencing an irreversible transformation should be Q/T? What is your understanding of how to determine the change of entropy for a gas that has experienced an irreversible transformation? Is entropy a property of the gas or a feature of the applied process?
 
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Ahmed1029 said:
For a freely expanding ideal gas(irreversible transformation), the change in entropy is the same as in a reversible transformation with the same initial and final states. I don't quite understand why this is true, since Clausius' theorem only has this corollary when the two transformations are reversible. Anyone can help?
The reason it is true is because that is how entropy is defined. Change in entropy is the integral of dQ/T over a reversible process from the initial to final states:

##\Delta S = \int_i^f\frac{dQ_{rev}}{T}##

In a free expansion of an ideal gas, there is no work done and no heat flow in getting from the initial to final states. So internal energy (T) is unchanged (first law). The reversible path between the initial and final states consists of:
1. a quasi-static expansion doing work against an external pressure. The external pressure is kept an arbitrarily small amount less than the internal gas pressure
2. positive heat flow into the gas during expansion to maintain constant temperature.

Since the process does not change internal energy, Q-W=0 where Q is the heat flow into the gas and W is the work done BY the gas: ie. Q = W

Therefore: ##\Delta S = \frac{Q_{rev}}{T}=\frac{W_{rev}}{T}>0##

AM
 
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