Ammonia is manufactured industrially by the reaction
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
At 298 K the equilibrium constant Kp for this reaction is 6.0×105. A chemist is asked to evaluate whether the reaction mixture will deliver a practically complete conversion of nitrogen under laboratory conditions in which the gases are initially mixed in stoichiometric proportions at a total pressure of 1.0 atm and allowed to reach equilibrium at 298 K.
Answer the following questions.
(a) Describe qualitatively the composition of the equilibrium mixture with respect to reactants and product under the stated conditions.
(b) Explain, with reference to the magnitude of Kp, whether the reaction can be considered to proceed essentially to completion in this situation.
(c) Discuss one operational factor other than temperature that industrial plants typically adjust to further increase the yield of NH3 despite the already large value of Kp. Justify your choice based on principles of chemical equilibrium.