C5.3 Equilibria

• What is a dynamic equilibrium?

  A dynamic equilibrium is a state where the rates of the forward and backward reactions are equal.
• What happens to a dynamic equilibrium if the conditions are changed?

  The equilibrium will shift to counteract the change in conditions.
• What happens to anhydrous copper sulfate when water is added?

  It turns blue and becomes hydrated copper sulfate.
• How does heating affect the equilibrium position?

  Heating can shift the equilibrium position depending on whether the reaction is exothermic or endothermic.
• What are the steps to analyze the concentrations of liquid and gas states at equilibrium?

  1. Identify the concentrations of reactants and products.
  2. Determine the state of each component (liquid or gas).
  3. Analyze how changes in conditions affect these concentrations.
• What is the balanced equation for the reaction of sodium with hydrogen to form ammonia?

  Na + 2H₂ → 2NaH
• How can you tell that a reaction is reversible?

  You can tell a reaction is reversible if the products can react to form the original reactants again.
• What is the principle of Le Chatelier?

  Le Chatelier's principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
• What happens to the equilibrium position if the concentration of a substance is decreased?

  The equilibrium will shift to increase the concentration of that substance again.
• How does increasing the pressure affect the equilibrium position?

  Increasing the pressure shifts the equilibrium towards the side with fewer gas molecules.
• Why are catalysts used in reversible reactions?

  Catalysts speed up the rate of reaction without changing the equilibrium position.
• What is the effect of increasing temperature on the equilibrium position of an endothermic reaction?

  Increasing temperature shifts the equilibrium position to the right, favoring the formation of products.
• How is methanol produced from carbon monoxide and hydrogen?

  Methanol is produced by reacting carbon monoxide with hydrogen under specific conditions.
• What are the factors that affect the position of equilibrium?

  • Concentration of reactants and products
  • Temperature
  • Pressure (for gaseous reactions)
  • Presence of catalysts
• What is the typical temperature used in industrial reactions for equilibrium?

  Typically around 300°C.
• Why is it important to choose suitable reaction conditions in industrial processes?

  Choosing suitable conditions maximizes yield and minimizes costs.
• How does the concentration of reactants affect the yield of products in a reversible reaction?

  Higher concentrations of reactants generally lead to higher yields of products.
• What is the role of temperature in the equilibrium position of a reaction?

  Temperature affects the rate of reaction and can shift the equilibrium position depending on whether the reaction is exothermic or endothermic.
• What is the effect of adding more reactants to a system at equilibrium?

  Adding more reactants shifts the equilibrium position to the right, favoring the formation of products.
• Why do catalysts not change the equilibrium position?

  Catalysts speed up both the forward and backward reactions equally, thus not affecting the position of equilibrium.