Controlling Equilibrium: The Haber Process
Temperature changes have predictable effects on equilibrium position. For exothermic reactions (which release heat), increasing temperature shifts the equilibrium left, whilst decreasing temperature shifts it right. Endothermic reactions do the opposite - they favour the forward direction when heated.
Pressure changes only affect reactions involving gases. Increasing pressure pushes the equilibrium towards the side with fewer gas molecules, whilst decreasing pressure favours the side with more molecules. Concentration changes work intuitively - add more reactant and you get more product.
The Haber Process perfectly demonstrates these principles in action. This industrial process makes ammonia (NH₃) from nitrogen and hydrogen gases, and it's essential for producing fertilizers that feed billions of people.
Real-World Application: The Haber Process feeds about half the world's population through nitrogen fertilizers - that's the power of understanding equilibrium!
Industries use compromise conditions because perfect equilibrium conditions might be too slow or expensive. At 450°C and 200 atmospheres pressure with an iron catalyst, the Haber Process balances maximum yield with reasonable costs and reaction speed. It's not the theoretical optimum, but it's the most profitable approach.