Initially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabatically against a constant pressure of 4 atm until equilibrium is achieved. Assume the gas to be ideal with Cp,m = 28.58 + 1.76 x 10^-2 T (The units of T are K and the units of Cp,m are J K-1 mol-1.) Compute DU, DH, q and w.

Silver, Water and Aluminum

Derive an expression for (∂S/∂P)T of an ideal gas. Then determine (∂S/∂P)T o for a sample containing 2.00 mol Ne (ideal gas) at 1.50 atm and 298 K. (answers: (∂S/∂P)T = -nR/P; -11.1 J/atmK)

Part A: 10 moles of ideal gas initially at 10 atm and 250 K is expanded isothermally and reversibly to a final pressure of 2 atm. Calculate W; U; and Q in Joules. Part B: The same gas in part A, starting in the same initial state, is expanded isothermally against a constant external pressure of 2 atm, to a final pressure of 2 atm. Calculate W; U; and Q in Joules for this irreversible process. Part C: The same gas in part B, starting in the same initial state, is expanded isothermally to a nal pressure of 2 atm. The process is carried out in 4 stages. First the gas is expanded against a constant pressure of 8 atm, to 8 atm. Then the gas is expanded against a constant pressure of 6 atm, to 6 atm. Then the gas is expanded against a constant pressure of 4 atm, to 4 atm. Finally, the gas is expanded against a constant pressure of 2 þtm, to 2 atm. Calculate W; U; and Q in Joules for the 4-step process.

Calculate 4G in two different ways for the dimerization of NO₂. The first method uses the Gibbs free energies of formation and the second method uses the equation 4G = AH-TAS. 2NO₂(g) → N₂O4(g) Starting with the natural variable equation of dH = TdS+Vdp, show that OH др T = V(1-aT)