Ammonia is synthesized industrially via the gas–phase equilibrium
N2(g)+3H2(g)⇌2NH3(g)
At 450\,°C the equilibrium constant expressed in terms of partial pressures is Kp=4.0×10−2. A rigid 5.00\,L reaction vessel at this temperature is charged with 1.20\,mol N2, 3.60\,mol H2, and 0.80\,mol NH3 and sealed. The total pressure at the moment the vessel is sealed is 120\,atm.
(a) Calculate the partial pressure of each gas in the vessel immediately after sealing, assuming ideal–gas behavior.
(b) Compute the value of the reaction quotient, Qp, for the system at that instant.
(c) Using your result from part (b), predict whether the net reaction will proceed toward reactants or toward products as equilibrium is established.
(d) Based on the magnitude of the difference between Qp and Kp, discuss whether the shift you predicted in part (c) will be extensive or limited, and justify your reasoning.