1.) A sample consisting of 1.0 mol of monotonic perfect gas, for which C_v,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 D_vapH^? = 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 C_v, the heat capacity at constant volume and C_p 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.