Final answer:
The production of ammonia from nitrogen and hydrogen is described by the exothermic reaction N2(g) + 3H2(g) → 2NH3(g), with a ΔH of -92 kJ/mol. In stoichiometry, this reaction's stoichiometric factors help determine the amount of reactants needed for a certain amount of product. Ammonia production is efficiently scaled up in industries through the Haber process, which adjusts conditions to improve yield despite the challenge of a small equilibrium constant at room temperature.
Step-by-step explanation:
Understanding the Reaction to Produce Ammonia
The balanced chemical equation N₂(g) + 3H₂(g) → 2NH₃(g) represents the production of ammonia from nitrogen and hydrogen in a chemical reaction. This particular reaction has a negative enthalpy change (ΔH) of -92 kJ/mol, indicating that it is an exothermic process. In the context of stoichiometry, stoichiometric factors can be calculated based on the ratio of consumed reactants to produced products, which for this reaction is N₂:H₂:NH₃ in a 1:3:2 ratio.
The industrial synthesis of ammonia, known as the Haber process, poses certain challenges due to the small equilibrium constant at room temperature and the slow rate of reaction at low temperatures. However, by adjusting conditions such as pressure and temperature, industries can increase the yield of ammonia. The equilibrium constant (K) varies with temperature, affecting the amount of ammonia produced at different temperatures.