The Haber process is very important for agriculture because it converts N₂(g) from the atmosphere into bound nitrogen, which can be taken up and used by plants. The Haber process reaction is N₂(g) + 3 H₂(g) → 2 NH₃(g). The reaction is exothermic but is carried out at relatively high temperatures. Why?

Verified step by step guidance

1. <Understand the Haber process: The Haber process synthesizes ammonia (NH3) from nitrogen (N2) and hydrogen (H2) gases. The balanced chemical equation is N2(g) + 3 H2(g) → 2 NH3(g).>
2. <Recognize the nature of the reaction: The reaction is exothermic, meaning it releases heat.>
3. <Consider the effect of temperature on reaction rate: Higher temperatures increase the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the reaction rate.>
4. <Apply Le Chatelier's Principle: Although the reaction is exothermic, increasing the temperature shifts the equilibrium position to favor the reactants (N2 and H2). However, high temperatures are used to achieve a reasonable reaction rate despite this shift.>
5. <Balance between rate and yield: The process is carried out at high temperatures to ensure a faster reaction rate, even though it slightly reduces the yield of ammonia due to the equilibrium shift.>