1.) A sample consisting of 1.0 mol of monotonic perfect gas, for which Cv,m= 3/2R, initially at p1 = 1.00 atm and T1 = 300 K, is heated reversibly to 400 K at constant volume. Calculate the final pressure, DU, q and w.
2.) A certain liquid has DvapH? = 260 kJ mol-1. Calculate q, w, DH, DU when 0.5 mol is vaporized at 250 K and 750 Torr.
3.) Use standard enthalpies of formation to calculate the standard enthalpy of the reaction:
2NO2(g), N2O4(g).
4.) Write down the exact differential for dU and dH and define Cv, the heat capacity at constant volume and Cp the heat capacity at constant pressure.
5.) By direct differentiation of H = U + pV, obtain a relation between (δH/δU)p and (δU/δV)p.
6.) Draw a diagram that depicts the how U changes as a function of the pressure and volume of a system under and adiabatic path and a non-adiabatic path. Describe what variables are state functions vs. path functions.