The Haber process for the production of ammonia relies on a heterogeneous catalyst.How does the use of this catalyst effect the yield of the reaction at equilibrium? $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}) \quad\quad\quad\quad\quad\quad \Delta H^{\circ}=-92.2 \mathrm{~kJ}$

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The use of a catalyst, including a heterogeneous catalyst like in the Haber process, speeds up both the forward and reverse reactions equally without affecting the position of equilibrium or the yield of the product. Catalysts only affect the rate at which equilibrium is reached.

The Haber Process for the Production of Ammonia Relies on a Heterogeneous