Consider the following reaction at T = 298 K and at constant pressure: = C2H,OH (g) = C2H4 (g) + H2O (8) Assume that all species can be modeled as ideal gases. c. Assuming that the initial partial pressure of each gas is Pi = 1.0 bar and that the reaction is performed against a constant external pressure Pext 3.0 bar and at T = 298 K. P cl. Given these initial conditions, determine the reaction quotient, lp, and the Gibb's potential of reaction, A.G. c2. In which direction will the reaction proceed? d. Assuming that the initial partial pressure of each gas is Pethanol 0.5 bar , Pethene 1.0 bar, and Pwater = 1.5 bar against a constant external pressure Pext 3.0 bar and at T 298 K. = dl. Given these initial conditions, determine the reaction quotient, the entropy, enthalpy, and Gibbs potential of reaction, i.e., determine Qp, A, S, A,H, and ArG. d2. In which direction will the reaction proceed? d3. Determine the mole fraction equilibrium constant, Kx. d4. Assuming that the gas mixture was initially contained in a volume of V = 0.02478 m3, determine the mole fraction and partial pressure of each species at equilibrium. = e. Suppose that the external pressure were doubled such that the reaction was performed against a constant external pressure Pext 6.0 bar at T - 298 K. What will be the new mole fraction equilibrium constant, Kz? Did increasing the pressure drive the equilibrium towards the reactants or products side? Why