Describe the Haber process and why it is both an exothermic and endothermic reaction (reversible)
Answers
Answer:
Explanation:
On a large scale, ammonia is manufactured by Haber’s process. N2 (g) + 3H2 (g) = 2NH3 (g); ∆H0 = – 46.1 kJ mol–1 In accordance with Le Chatelier’s principle, high pressure would favour the formation of ammonia. The optimum conditions for the production of ammonia are a pressure of 200 × 105 Pa (about 200 atm), a temperature of ~ 700 K and the use of a catalyst such as iron oxide with small amounts of K2O and Al2O3 to increase the rate of attainment of equilibrium. Earlier, iron was used as a catalyst with molybdenum as a promoter.
A system that releases heat to the surroundings, an exothermic reaction, has a negative ΔH by convention, because the enthalpy of the products is lower than the enthalpy of the reactants of the system. The enthalpies of these reactions are less than zero, and are therefore exothermic reactions.
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