Unformatted text preview: process. The entropy of the gas decreases. Does this violate the 2nd law? Briefly (in no more than 10 words) justify your answer below. √ You could imagine removing heat from an ideal gas, while simultaneously doing reversible configuration work on the gas, so that the change in internal energy is zero. In this situation, the temperature of the gas would remain unchanged, but its entropy decreased because heat flowed out. The entropy increase of the surroundings would then be equal and opposite to the entropy decrease of the gas. Another example would be if the gas condensed at constant temperature....
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This note was uploaded on 12/15/2011 for the course PHY 3513 taught by Professor Staff during the Fall '08 term at University of Florida.
- Fall '08