For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier's principle.

N2 (g) + 3 H2 (g) 2 NH3 (g) H = -92 kJ/mol

Question

For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier's principle.

N2 (g) + 3 H2 (g)  2 NH3 (g) H = -92 kJ/mol

anonymous · Answer

the reaction is exothermic, so heat is being released. so to produce an even higher yield, you would decrease the heat that is being added via decrease in the temperature. This would drive the reaction further toward the products.

in terms of pressure, there is 1 mol of N2 and 3 mols of H2 for a total of 4 mols of reactant whereas the products side has 2 mols of NH3. this means that you would increase the pressure so that the reaction is driven to the products. This happens because the products side of the equation has a lower number of mols.

anonymous · Answer

Thank you so much!