Consider the elementary gas-phase reversible reaction A 3C Pure A enters at a temperature of 400 K and a pressure of 10 atm. At this temperature, KC 0.25(mol/dm3)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. (b) The gas-phase reaction is carried out in a constant-pressure batch reactor. (c) Can you explain the reason why there would be a difference in the two values of the equilibrium conversion

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

am i too late?

explanation: