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Silviu
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Poster has been reminded to post schoolwork-related questions in the HH forums and use the Template
Hello! I have this GRE question:
In process 1, a monoatomic ideal gas is heated from temperature T to temperature 2T reversibly and at constant temperature. In process 2, a monoatomic ideal gas freely expands from V to 2V. Which is the correct relationship between the change in entropy ##\Delta S_1## in process 1 and the change in entropy ##\Delta S_2## in process 2?
So, I am not sure in the first process what do they mean by, at constant temperature, if the temperature goes from T to 2T, but leaving that aside the correct answer is: ##0 < \Delta S_2 < \Delta S_1 ##. However, another option is ##0 =\Delta S_1 < \Delta S_2##. My main question is: isn't the change in entropy always 0 in a reversible process? So, shouldn't be this answer the right answer (being also the only one with ##0 =\Delta S_1##)?
Thank you!
In process 1, a monoatomic ideal gas is heated from temperature T to temperature 2T reversibly and at constant temperature. In process 2, a monoatomic ideal gas freely expands from V to 2V. Which is the correct relationship between the change in entropy ##\Delta S_1## in process 1 and the change in entropy ##\Delta S_2## in process 2?
So, I am not sure in the first process what do they mean by, at constant temperature, if the temperature goes from T to 2T, but leaving that aside the correct answer is: ##0 < \Delta S_2 < \Delta S_1 ##. However, another option is ##0 =\Delta S_1 < \Delta S_2##. My main question is: isn't the change in entropy always 0 in a reversible process? So, shouldn't be this answer the right answer (being also the only one with ##0 =\Delta S_1##)?
Thank you!