Reversible reactions and le chateliers principle

• What is the general form of a reversible reaction?

  A + B ⇌ C + D
• What does it mean for a reversible reaction to reach equilibrium?

  It means the rates of forward and reverse reactions are equal
• Can reversible reactions be endothermic and exothermic?

  Yes, they can be both types of reactions
• What happens when you heat blue hydrated copper(II) sulfate crystals?

  It becomes white anhydrous copper(II) sulfate
• What occurs when you add water to white anhydrous copper(II) sulfate?

  It forms blue hydrated copper(II) sulfate
• What is Le Chatelier's Principle?

  It states systems will counteract changes to restore equilibrium
• How does a decrease in temperature affect a reversible reaction at equilibrium?

  It shifts equilibrium towards the exothermic direction
• What happens to equilibrium when the temperature is raised?

  It shifts towards the endothermic direction
• What effect does changing pressure have on gaseous equilibria?

  It affects the direction of equilibrium based on gas molecules
• What happens if you increase the pressure in a gaseous equilibrium?

  It shifts towards the side with fewer gas molecules
• What occurs if you decrease the pressure in a gaseous equilibrium?

  It shifts towards the side with more gas molecules
• How does changing concentration affect equilibrium?

  It causes the system to adjust back to equilibrium
• What happens if you increase the concentration of reactants?

  The system produces more products
• What occurs if you decrease the concentration of products?

  The system reduces reactants to increase products
• How does pressure affect the equilibrium of the reaction N₂ + 3H₂ ⇌ 2NH₃?

  • There are 4 moles on the left (1 N₂ and 3 H₂)
  • There are 2 moles on the right (2 NH₃)
  • Increasing pressure shifts equilibrium to the right (more NH₃)
• What happens if more N₂ or H₂ is added to the reaction N₂ + 3H₂ ⇌ 2NH₃?

  The forward reaction produces more NH₃