Question

The Haber process for the production of ammonia is the main industrial process of producing ammonia today. Prior to developing this process, ammonia was difficult to produce on an industrial scale. The reaction for the Haber process is: N2(g) + 3 H2(g) ⇌ 2 NH3(g). Using the following values, determine the equilibrium constant for this reaction at 25oC. Substance ΔGfo(kJ/mol) N2 0 H2 0 NH3 -16.4

Answer 1

Answer:

Equilibrium constant for the reaction at 25⁰C = 1.81 x 10⁻⁶

Explanation:

                            Reaction for the Haber's process

                              N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Free energy change of reaction

                    ΔGr° = ∑products free energy - ∑reactants free energy

                             = 2 x (- 16.4) - 0

                             = - 32.8 KJ / mole

Equilibrium constant for this reaction at 25⁰C

                           ΔGr° = - 2.303 RT log K

                      ⇒  log K = $\frac{-32.8}{2.303 X8.314X10^{-3}X 298 }$

                      ⇒        K = Anti log( -5.74) = 1.81 x 10⁻⁶