The synthesis of ammonia from nitrogen and hydrogen gas is an exothermic reaction, which can be represented by the following equation:N2 g + 3H2 g 2NH3 g The relationship between the reaction rate and reaction yield is governed by the principles of chemical equilibrium and kinetics. The reaction rate determines how fast the reaction proceeds, while the reaction yield refers to the amount of product ammonia formed at equilibrium.Le Chatelier's principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract the change and restore a new equilibrium. In the case of ammonia synthesis, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the product side ammonia . This results in a higher reaction yield. However, increasing the temperature for an exothermic reaction will shift the equilibrium towards the reactants nitrogen and hydrogen , resulting in a lower reaction yield.The reaction rate is influenced by the temperature and pressure as well. Higher temperatures increase the kinetic energy of the molecules, leading to more frequent and energetic collisions, which in turn increases the reaction rate. Similarly, increasing the pressure also increases the reaction rate, as it brings the molecules closer together, leading to more frequent collisions.In summary, increasing the pressure in the synthesis of ammonia from nitrogen and hydrogen gas will generally lead to a higher reaction yield and faster reaction rate. However, increasing the temperature will increase the reaction rate but decrease the reaction yield. Therefore, optimizing the temperature and pressure conditions is crucial for maximizing both the reaction rate and yield in ammonia synthesis. In industrial processes, such as the Haber-Bosch process, a compromise is made by using moderately high pressures and temperatures to achieve a balance between reaction rate and yield.