Hello future chemists! 🧪🌟 Today, we are going to dive into the awesome world of Le Châtelier’s principle. It's like a superhero for chemical reactions!

• Definition: If a dynamic equilibrium is disturbed by a change in reaction conditions (temperature, pressure, concentration), the equilibrium will shift to counteract the change!
• Example: Think of a seesaw. When you add weight to one side, the other side goes up to balance it out. That’s what reactions do!

• Concentration: Changing concentration is like adding or removing players in a tug-of-war!
  • Example: For N₂ + 3H₂ ⇌ 2NH₃, if you add more H₂, the equilibrium will shift to the right to make more NH₃. It’s like helping your team in tug-of-war!
  • 🌟 Real-world Example: Our body uses this principle to maintain balance in blood gas levels!
• Pressure: It affects reactions with gases. Increasing pressure will favor the side with fewer gas molecules!
  • Example: For N₂ + 3H₂ ⇌ 2NH₃, increasing pressure shifts equilibrium to the right. It’s like squeezing into a crowded room; it’s easier if fewer people are inside!
  • 🌟 Tip: It doesn’t affect solids and liquids as they are nearly incompressible!
• Temperature: The cool and hot member of the reaction party! It affects both equilibrium position and the equilibrium constant (K).
  • Example: For exothermic reactions like the synthesis of ammonia (N₂ + 3H₂ ⇌ 2NH₃), increasing temperature shifts the equilibrium to the left, reducing ammonia. It’s like turning up the heat and everyone moving to the cooler side of the room!
  • 🌟 Fun Fact: For reactions with ΔH⦵ r = 0, temperature has no effect on equilibrium!