Kinetics

• What is the fundamental requirement for a reaction to take place according to collision theory?

  Particles need to collide.
• How does temperature affect the rate of reactions?

  Higher temperature increases particle energy and speed, leading to more successful collisions.
• What happens to the frequency of successful collisions when concentration or pressure is increased?

  Particles are closer together, resulting in more frequent successful collisions.
• How does surface area affect reaction rates?

  • High surface area increases the amount of solid exposed to reactants.
  • This leads to faster reactions and more successful collisions.
• What is the role of a catalyst in a chemical reaction?

  A catalyst speeds up the rate of reactions while remaining chemically unchanged.
• How does a catalyst affect activation energy?

  A catalyst provides an alternative pathway with lower activation energy, leading to more successful collisions.
• What is activation energy (Ea)?

  It is the minimum amount of energy needed for a successful collision to allow a reaction to occur.
• What happens if the collision energy is less than the required activation energy?

  The particles will collide and drift away without reacting.
• Why is the orientation of particles important in collision theory?

  Particles need to be in the correct alignment for a successful reaction.
• What does the Maxwell-Boltzmann distribution plot represent?

  • It shows the number of particles versus the energy they have at a fixed temperature.
  • The area under the curve represents the total number of molecules present.
• What does the curve of the Maxwell-Boltzmann distribution plot indicate about particles with energy greater than Ea?

  Particles with energy ≥ Ea lead to successful collisions.
• What does the area under the Maxwell-Boltzmann distribution curve represent?

  The total number of molecules present.
• Why does the Maxwell-Boltzmann distribution curve not touch the axis?

  There is no limit to the energy that particles can have.
• What happens to the Maxwell-Boltzmann distribution curve when temperature increases?

  More molecules have energy greater than Ea, leading to more successful collisions.
• How does increasing temperature affect the most probable energy (Emp) in the Maxwell-Boltzmann distribution?

  Emp decreases as the curve moves down and right.
• What are the benefits of using catalysts in industrial processes?

  • Saves money by lowering Ea and reducing energy requirements.
  • Better for the environment as they are not consumed.
  • Improves efficiency and saves time due to faster reactions.
• How does increasing concentration or pressure affect the Maxwell-Boltzmann distribution curve?

  It increases the average number of molecules per unit volume, leading to more successful collisions.
• What is the effect of lower concentration on the rate of reaction?

  Lower concentration results in fewer successful collisions.
• What is the effect of higher concentration on the rate of reaction?

  Higher concentration increases the rate of reaction.