## entropy of steam and water

1. The problem statement, all variables and given/known data

Why does the entropy of the water increase with increasing temperature, while the entropy of steam decreases, while the entropy of steam decreases with increasing temperature?
3. The attempt at a solution

I think the reason why the entropy increases with water is because it takes an extra amount of heat to convert water to steam when it reaches a temperature of 100 degrees celsius more than increasng the temperature of water while since when increasing the temperature of steam , its not gong through a phase transition and so as the temperature goes up, the entropy goes down since S=Q/T
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 Recognitions: Gold Member Homework Help Science Advisor I'm stuck at the premise of the question. Who says that the entropy of steam decreases with increasing temperature? That would mean that the specific heat of steam is negative, which is untrue.
 Recognitions: Gold Member If you look at the steam tables, you will find that the entropy of steam in the saturated vapor (steam) condition does decrease as the temperature and pressure both increase. At a pressure of 0.6113 kPa and a saturation temperature of 0.01 C the entropy is 9.1562 kJ/kg-K. At the critical point of 22.09 MPa and a saturation temperature of 374.14 C the entropy is 4.4298 kJ/kg-k Now, a saturated liquid (water) has an increase in entropy as the temperature and pressure both increase. So the original question is justified as long as one indicates that the pressure is increasing also. Thanks Matt

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Homework Help
Ah, got it. I was thinking $(\partial S/\partial T)_P$ or $(\partial S/\partial T)_V$. This would be more like $(\partial S/\partial T)_{\mu=\mu(H_2O(l),\,T,\,P)}$