0.64 moles of an ideal gas undergoes a couple of change processes that move the system from (P₁, V₁) to (P2, V₂) as shown on the diagram below. Both points share the same temperature, T = 451 K, and P₁ = 1.36 bars, P₂ = 0.63 bars. The two pathways are defined as Pathway 1 + 2- isochoric cooling to (P2, V₁), then isobaric expansion to (P2, V₂). Pathway 3- isothermal expansion directly to (P2, V₂). 3 For the purposes of this problem, you may assume that C₁ = ³R and Cp = R. 2 P↑ (P₁,V₁) To (P₂, V₁) T (3) (2) (P₂, V₂) V a) Find the volumes V₁ and V₂ and compute AV (in L) for the net process. (b) For each of the three paths drawn, calculate AU, AH, and AS. Report the first two in units of kJ, and the last in units of J/K. (c) Since Gibbs energy is a state function, AG is the same for both pathways. Evaluate it for the net process and report it in units of kJ. Note: The temperature at the point (P2, V₁) is different from that of the isotherm, and has been labeled To. You may need to define this temperature in your calculations. Also, for part (c) the absolute entropy content at that same point can be assumed to be 200 J/K.

A 10.0 mL sample of CO2 is collected by the downward displacement of water at 23.0°C and a room pressure of 100.5 kPa. What is the volume of dry CO2 at 0.00°C and 90.0 kPa?

Ratio of specific heats of CO2 at 825K?

3.

At low pressures, the compressibility factor of a van der Waals gas is given by the equation: Z = 1+ (b-a/RT) P/RT Calculate ΔG (in units J/mol) associated with the isothermal compression of nitrogen gas at 298 K from 10 bar to 25 bar. The van der Waals constants of nitrogen gas are a = 1.408 L^2-bar-mol and b = 0.03913 L-mol^-1