a) An ideal gas occupying a volume of 10.8L at a pressure of 1bar and a temperature of 300 K, is compressed reversibly and adiabatically to a volume of 6.45L. What is its final pressure and temperature? (Note: for thisideal gas, you may assume thatR/Cv= 0.4, or γ=5/3; these represent the same thing.) (b) The heat capacity ratio, γ= 1.20, for a certain ideal gas. By what factor does the pressure changeif the volume is doubled in a reversible adiabatic expansion?

Krypton is contained in a closed cylinder fitted with a weightless piston at 63 K and 1 bar. Heat is added under constant pressure until the volume has doubled in size. What is the change in the molar internal energy (Δ�)? Assume krypton is an ideal gas. From Appendix B in the text, we can assume the heat capacity of krypton is independent of temperature and ��=2.5� , where R is the molar gas constant �=8.314 J/(mol K). For an ideal gas, recall ��=��−�=1.5�. Report your answer in units of kJ/mol using three decimal places.

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.

Current Attempt in Progress * Your answer is incorrect. A rigid tank whose volume is 4 m³, initially containing air at 1 bar, 295 K, is connected by a valve to a large vessel holding air at 6 bar, 295 K. The valve is opened only as long as required to fill the tank with air to a pressure of 6 bar and a temperature of 350 K. Assuming the ideal gas model for the air, determine the heat transfer between the tank contents and the surroundings, in kJ. Qcy F i 879.84 eTextbook and Media kJ