reaction rates

• What does the rate of reaction refer to?

  The change in concentration or amount of a reactant or product per unit time.
• How is the rate of reaction calculated?

  By dividing the amount of reactant used or product made by time.
• What must happen for a reaction to occur according to collision theory?

  Particles must collide in the right direction and have sufficient kinetic energy.
• What is activation energy?

  The minimum amount of energy required for a reaction to occur.
• What does an energy profile diagram show?

  Changes in energy during a reaction, including activation energy.
• How does the shape of the energy profile relate to activation energy?

  A flatter dome indicates lower activation energy is needed for the reaction.
• What does the Maxwell-Boltzmann distribution illustrate?

  The distribution of kinetic energy among gas particles.
• What does the area under the Maxwell-Boltzmann curve represent?

  The total number of molecules in the sample.
• What is the difference between the most likely energy and the mean energy of particles?

  The most likely energy is the peak of the distribution, while the mean energy is the average energy of all particles.
• How does temperature affect the rate of reaction?

  Higher temperatures increase the average kinetic energy of particles, leading to more frequent and energetic collisions.
• What happens to the Maxwell-Boltzmann distribution when temperature is increased?

  The curve shifts to the right, and the area beyond the activation energy increases.
• What occurs when the temperature is decreased in a reaction?

  A smaller proportion of molecules will have energy greater than the activation energy.
• Why do reactions occur faster at higher temperatures?

  Particles move more quickly, collide more often, and have more energetic collisions.
• How does pressure affect the rate of reaction?

  Increasing pressure brings particles closer together, leading to more frequent collisions.
• How does concentration affect the rate of reaction?

  Higher concentration increases the likelihood of collisions between particles.
• What is a catalyst?

  A substance that increases the rate of reaction without being consumed in the process.
• How do catalysts lower activation energy?

  By providing an alternative pathway for the reaction.
• What is a heterogeneous catalyst?

  A catalyst that is in a different phase from the reactants.
• What is the Haber process used for?

  Manufacturing ammonia from nitrogen and hydrogen gases.
• Why is the use of catalysts important in industrial processes?

  They speed up reactions, saving time and reducing costs.
• What is the role of zeolite as a catalyst?

  It increases the surface area for reactions to occur more quickly.
• What are the key factors affecting the rate of reaction?

  • Temperature
  • Pressure
  • Concentration
  • Presence of catalysts
• What are the types of catalysts?

  • Homogeneous catalysts: same phase as reactants
  • Heterogeneous catalysts: different phase from reactants
• What is the significance of activation energy in chemical reactions?

  • Minimum energy required for a reaction to occur
  • Determines the rate of reaction
• How does the Maxwell-Boltzmann distribution relate to reaction rates?

  • Shows the distribution of kinetic energy among particles
  • Indicates the proportion of particles with energy greater than activation energy
• How does increasing temperature affect the Maxwell-Boltzmann distribution?

  • Shifts the curve to the right
  • Increases the area beyond activation energy
• How does increasing concentration affect reaction rates?

  • Increases the likelihood of collisions
  • Leads to a higher chance of reaction
• How does increasing pressure affect reaction rates?

  • Brings particles closer together
  • Increases frequency of collisions
• What is the relationship between catalysts and activation energy?

  • Catalysts lower activation energy
  • Provide an alternative pathway for reactions
• What is the importance of catalysts in industrial chemistry?

  • Speed up reactions
  • Reduce costs and energy consumption
• What is the role of zeolite in catalysis?

  • Solid catalyst with microscopic pores
  • Increases surface area for reactions
• What are the tiny microscopic pores in catalysts called?

  Micropores
• How do micropores affect the surface area of a catalyst?

  They increase the surface area, allowing reactions to happen quicker.
• What is a zeolite?

  A type of catalyst with a large surface area due to micropores.
• What are the two types of catalysts?

  • Homogeneous catalysts: same phase as reactants.
  • Heterogeneous catalysts: different phase from reactants.
• What does "heterogeneous" mean in the context of catalysts?

  It means the catalyst is in a different phase from the reactants.
• What is the Haber process used for?

  It is used for the manufacturing of ammonia.
• What type of catalyst is used in the Haber process?

  An iron catalyst.
• How does a heterogeneous catalyst speed up a reaction?

  It provides an alternative pathway for the reaction.
• How can the surface area of a solid catalyst be increased?

  By grinding it into a powder.