The reaction between nitrogen gas N2 and hydrogen gas H2 to form ammonia NH3 is known as the Haber-Bosch process, which can be represented by the following balanced equation:N2 g + 3H2 g 2NH3 g This reaction is an example of a reversible reaction, and its rate is influenced by various factors, including pressure and temperature. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in pressure, temperature, or concentration of reactants and products, the system will adjust itself to counteract the change and restore a new equilibrium.Effect of pressure:The Haber-Bosch process involves a decrease in the number of moles of gas as the reaction proceeds from reactants to products 4 moles of reactants to 2 moles of products . Therefore, increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas, which in this case is the side of the products NH3 . As a result, the rate of the reaction will increase with increasing pressure.Effect of temperature:The Haber-Bosch process is an exothermic reaction, meaning it releases heat as it proceeds. According to Le Chatelier's principle, increasing the temperature will shift the equilibrium position towards the endothermic side the side that absorbs heat , which in this case is the side of the reactants N2 and H2 . Therefore, increasing the temperature will decrease the rate of the reaction. However, it is important to note that increasing the temperature also increases the kinetic energy of the molecules, which can lead to a higher collision frequency and, consequently, a higher reaction rate. In the case of the Haber-Bosch process, the optimal temperature is typically around 400-500C to balance these competing effects.In summary, the rate of the reaction between nitrogen gas and hydrogen gas is positively affected by increasing pressure and can be influenced by temperature, with an optimal temperature range for the Haber-Bosch process being around 400-500C.