Consider the catalytic cracking reaction of propane, C3Hg: C3H3(g) = C2H4(g) + CH4 (9) C3H3(g) C2H4@) CH4(E) 9R 5R 4R DATA: Standard-state constant-pressure heat capacity (approximately constant at all T, P), c Standard-state Gibbs free energy of formation at 298.15 K, A, G Standard-state enthalpy of formation at 298.15 K, A,H -24 kJ/mol 68 kJ/mol -50 kJ/mol -105 kJ/mol 53 kJ/mol -75 kJ/mol (a) We perform this reaction in an isothermal and isobaric reactor, initially loaded with pure C3Hg and maintained at 1 bar. Express the equilibrium conversion of C3H8, Xeq, as a function of the equilibrium constant, K, only. State all assumptions you need. (Note: The equilibrium conversion is the amount of C3Hg that has reacted when the reaction reaches equilibrium, divided by the initial amount of C3Hg loaded.) (b) For the reactor in Part (a), determine the equilibrium conversion of CzHg at 700 K. (c) Calculate the heat per mole of input C3Hg required to keep the reactor in Part (a) at constant temperature throughout the reaction (i.e., from the initial state of pure C3Hg at 700 K to the equilibrium state at 700 K). (d) If we instead perform this reaction in an isothermal and isochoric reactor of volume 1 m3, initially loaded with 10 moles of pure CzHg at 700 K, calculate the equilibrium conversion and the equilibrium pressure