Le Chatelier's Principle

• What principle is covered in this video?

  Le Chatelier's principle
• What does Le Chatelier's principle describe?

  How equilibrium shifts during reversible reactions
• What factors affect the position of equilibrium?

  Temperature, pressure, and concentration
• What does the position of equilibrium refer to?

  Ratio of reactant to product particles
• How do we describe the equilibrium position if there are more reactants?

  The equilibrium lies to the left
• How do we describe the equilibrium position if there are more products?

  The equilibrium lies to the right
• What happens to equilibrium when conditions change?

  It shifts to counteract the change
• What is the reaction for the production of ammonia?

  Nitrogen and hydrogen react to form ammonia
• What is the overall energy change of the forward reaction for ammonia production?

  -92 kilojoules per mole
• What does a negative energy change indicate about the forward reaction?

  It is exothermic and releases energy
• What type of reaction is the backward reaction if the forward reaction is exothermic?

  Endothermic
• What happens to equilibrium if the temperature is decreased?

  It shifts to the exothermic direction
• What happens to equilibrium if the temperature is increased?

  It shifts to the endothermic direction
• How does pressure affect the position of equilibrium?

  It shifts to reduce pressure
• What side does equilibrium shift to if pressure is increased?

  To the side with fewer molecules
• How many molecules are on the left side of the ammonia reaction?

  Four molecules
• How many molecules are on the right side of the ammonia reaction?

  Two molecules
• What happens to equilibrium if pressure is decreased?

  It shifts to the side with more molecules
• What happens to equilibrium if more nitrogen is added?

  It shifts to the right to form more ammonia
• What are the effects of changing temperature, pressure, and concentration on equilibrium?

  • Decreasing temperature shifts equilibrium to exothermic direction
  • Increasing temperature shifts equilibrium to endothermic direction
  • Increasing pressure shifts equilibrium to side with fewer molecules
  • Decreasing pressure shifts equilibrium to side with more molecules
  • Adding reactants shifts equilibrium to product side