Calculate the increase in entropy when 1.00 mol of a monoatomic ideal gas with Cv,m = 2.5 R, is heated from 300 K to 600 K and simultaneously expanded from 30.0 dm3 to 50.0 dm3.

A system consisting of 0.20 mol of supercooled gaseous water (95°C, 1 bar) partially condenses to liquid water; the process is done adiabatically at constant pressure.         At equilibrium, what is the temperature of the system? How many moles of gaseous water have condensed? Calculate the entropy change for the process.

choose the correct answer

The following equation of state is found to describes the behavior of a particular gas with reasonable accuracy. Z = 1 + (a - b/T)P/RT where a=15x10-6 m3/mol and b= 0.06 (m3.K)/mol. Show that the residual enthalpy and residual entropy take the form: (H^r)/RT =(A-2B) and (S^r)/R = -B where A =(aP)/RT and B = (bP)/(RT^2)