Three moles of an ideal gas at 1 atm pressure and 20 °C are heated at  constant pressure until the final temperature is 80 °C. For the gas Cv = 7.50  + 3.2×10–3 T cal mol–1 deg–1. Calculate w, ∆E, ∆H, and q for the process.

Consider an ideal gas for which Cv= 20.88 and Cp= 29.2 J/mol K. The initial state is 100 kPa and 295 K. Calculate OS when 1 kmol is heated at constant volume to 355 K b. 1 kmol is heated at constant pressure to 355 K

Complete the property table for water below. Use only the Thermodynamic Property Table for Water referring to the Smith, Van Ness and Abbot Thermodynamics textbook. P [kPa] V [m³/kg] H[ kJ/kg] T[°C] Phase Description X 500 Saturated liquid 171 2044.5 300 0.8 Note that x refers to the "quality" or the mass fraction of the water in vapor phase. If the system is composed of pure liquid water, x = 0. If the system is composed of pure gaseous steam, x = 1. The volume of a liquid/vapor system can be determined using the following equation. V = Vj + x(Vg-Vj) V - volume of saturated liquid water Va - volume of saturated gaseous steam Similar calculation can be done for other properties such as internal energy, entropy, and enthalpy. H = HỊ + x(Hg-H) Under phase description, indicate whether the system is composed of saturated liquid, saturated vapor, superheated vapor, or liquid-vapor mixture. Also note that when pressure is given, it is more advisable to use the Superheated Steam Table than…

13 An ideal solution of 5.25 moles of benzene and 3.0 moles of toluene is placed in a piston and cylinder assembly. At 298 K, the vapor pressure of pure substances are P°(benzene) = 96.4 torr & P°(toluene) = 28.9 torr. The vapor pressure of the solution is; 69.81 torr O 71.83 torr 53.47 torr O 66.61 torr 67.50 torr