Answer:
a) Xac = 0.39
b) Xac = 0.58
c) There would be a difference in the two values of the equilibrium conversion because in constant pressure condition it would take longer time to reach the same conversion rate ( higher conversion equilibrium ) and this because the volume increase with the reaction at constant pressure
Explanation:
From elementary gas phase reaction
Cao = Po / RT
Po = 10
R = 82.06
T = 400 K
Cao = 3.05 * 10^-4 mol/cm^3 ≈ 0.305 mol/dm^3
Kc = 0.25 (mol/dm^3 )^2
Calculate the equilibrium conversion for each of the following situations
a) The gas-phase reaction is carried out in a constant-volume batch reactor
Xac = 0.39
b) The gas-phase reaction is carried out in a constant-pressure batch reactor
Xac = 0.58
c) There would be a difference in the two values of the equilibrium conversion because in constant pressure condition it would take longer time to reach the same conversion rate ( higher conversion equilibrium ) and this because the volume increase with the reaction at constant pressure
Attached below is a detailed solution as regards the question above
