Final answer:
The chemical equation N2(g) + 3H2(g) ⇒ 2NH3(g) describes the formation of ammonia in the Haber process, and the equilibrium constant expression is derived from the partial pressures of the reactants and products. At equilibrium, changes in the formation of ammonia can affect the total pressure and the position of the equilibrium.
Step-by-step explanation:
The reaction N2(g) + 3H2(g) ⇒ 2NH3(g) represents the synthesis of ammonia from nitrogen and hydrogen gases, commonly known as the Haber process. The number in front of the chemical formula represents the stoichiometric coefficients and the (g) indicates that the substances are in gaseous state. This balanced chemical equation conveys that one mole of nitrogen reacts with three moles of hydrogen to produce two moles of ammonia.
The equilibrium constant expression for this reaction, based on partial pressures, is K = (PNH3)² / (PN2 ⋅ (PH2)³), where PNH3 represents the partial pressure of ammonia, PN2 is the partial pressure of nitrogen, and PH2 is the partial pressure of hydrogen. This equation emphasizes the relationship between the concentrations of reactants and products in an equilibrium state at a specific temperature.
As the system reaches equilibrium, the formation of ammonia can impact the total pressure of the system and thus influence the dynamics of the equilibrium according to Le Chatelier's principle.