Two moles of an ideal gas undergo an irreversible isothermal expansion from Va=100 liters to Vb=300 liters at T=300K. (a) What is the entropy change for this process? (b)  What is the Gibbs free energy change? (c)  Is this process spontaneous or not? Explain your answer.

Refrigerant 134a (R134a) is at vapor/liquid equilibrium at 300 K. The saturation pressure is 7.0282 bar, the entropy of the saturated liquid is 1.1287 J/(g K) and the entropy of the saturated vapor is 1.7156 J/(g K). If the system has a an entropy of 1.38 J/(g K), what is the quality? (That is, what fraction of the system is vapor?) Report your answer to three decimal places.

One mole of an ideal monatomic gas, initially at a pressure of 1.29 atm and a volumeof 0.0152 m3, , is heated to a final state wherethe pressure is 6.29 atm and the volume is0.0552 m3.The gas constant is 8.31447 J/mol · K .Determine the change in entropy for this

A 2.00 - mol sample of an ideal diatomic gas at a pressure of 1.00 atm and temperature of 440 K undergoes a process in which its pressure increases linearly with temperature, use P = Po + aT .  The final temperature and pressure are 720 K and 1.60 atm.  Determine (e) the change in internal energy, (b) the work done by the gas, and (c) the heat added to the gas.  (Assume five active degrees of freedom . )