Hi! I have a practical problem that causes me to wonder. It seems like I have to choose from gaining energy from nothing, or to get a reduction in entropy from a spontaneous process. Imagine a small enclosed chamber filled with dry H2O gas. The properties are: 0.5 Bar 8.0 kJ/(kg*K) 200C 2850kJ/kg An infinitely large reservoir of H2O gas has the following properties: 1.0 Bar 8.0kJ/(kg*K) 240C 2950kJ/kg Here is a reference chart: http://www.steamtablesonline.com/images/steam tables p-h diagram (large).png A valve between the large reservoir and the small chamber is opened and the two gasses are mixed until they reach equilibrium inside the chamber and the pressure is stabilized at 1 bar. Am I correct in assuming that no work has been done and that the properties will be as follows?: 1.0 Bar 7.9kJ/(kg*K) 220C 2900kJ/kg This seems to be correct as far as temperature and pressure goes. It also seems to add up with the enthalpy as the process is thought to be adiabatic. However, the entropy is lowered, and the process seems to be a so called spontaneous process. The question is if this goes along with the second law of thermodynamics. (It can be read here if you need it refreshed: http://en.wikipedia.org/wiki/Second_law_of_thermodynamics) Also, I see no room for different results. The pressure is given by the infinite source. This means we can not leave the 1 bar line. There is no way we can get any condensation, so we have the following options: 1: The entropy is actually reduced 2: Enthalpy is lost or gained, and so is temperature ...or am I overlooking something here? Thanks for any response!