rates of reactions & equilibrium

• What is the definition of reaction rate?

  Reaction rate refers to the speed at which reactants are converted into products in a chemical reaction.
• How could the reaction rate of 2H₂ + O₂ → 2H₂O be measured?

  By measuring how quickly the concentration of H₂ decreases over time.
• What factors affect reaction rates?

  1. Temperature: Higher temperatures increase reaction rates.
  2. Concentration: Higher concentrations of reactants speed up reactions.
  3. Surface area: Increasing surface area of solid reactants speeds up reactions.
  4. Catalysts: Substances that increase reaction rates without being consumed.
  5. Nature of reactants: Some substances react faster than others.
• What is chemical equilibrium?

  Chemical equilibrium is a state in a reversible reaction where the forward and reverse reaction rates are equal.
• What does it mean when a reaction is at equilibrium?


  It means there is no net change in the concentrations of reactants and products over time.
• What characterizes a dynamic process in chemical equilibrium?


  Reactions continue, but at equal rates.
• What is the equilibrium constant (K)?


  The equilibrium constant expresses the ratio of products to reactants at equilibrium.
• In the reaction N₂ + 3H₂ ⇌ 2NH₃, what happens at equilibrium?

  The rate of ammonia formation equals the rate of its decomposition back into nitrogen and hydrogen.
• What does Le Chatelier's Principle state?


  When a system at equilibrium is disturbed, it will shift to counteract the change.
• What are the effects of disturbances on a system at equilibrium according to Le Chatelier's Principle?


  • Changes in concentration: The system shifts to use up added reactants or products.
  • Changes in pressure: The system shifts towards the side with fewer gas molecules.
  • Changes in temperature: The system shifts in the direction that absorbs or releases heat.
• How do catalytic converters work in relation to reaction rates?

  Catalytic converters use catalysts to increase the rate of reactions that convert harmful emissions to less harmful substances.
• How does the concept of equilibrium apply to blood pH regulation?

  The bicarbonate buffer system uses equilibrium shifts to maintain a constant pH in blood.
• How does the Haber process contribute to agriculture?


  It provides a method to produce nitrogen fertilizers on an industrial scale.
• What is the role of the iron catalyst in the Haber process?


  The iron catalyst increases the reaction rate without being consumed.
• Who developed the Haber process?


  Fritz Haber and Carl Bosch.
• If you add more reactants to a system at equilibrium, what will happen?


  The system will shift to use up some of the added reactants, producing more products.
• What are some real-world applications of rates and equilibrium concepts?

  1. Industrial processes: Haber process for ammonia production.
  2. Carbonated drinks: Equilibrium between dissolved CO₂ and carbonic acid.
  3. Blood pH regulation: Bicarbonate buffer system.
  4. Catalytic converters: Increase reaction rates for emissions.
  5. Cooking: Pressure cookers raise boiling point to cook faster.
• In which type of chemical change do elements combine with other elements or compounds to form one product?  Combination reactions
• In which type of chemical change do two or more substances break down into simpler substances?  Decomposition reactions