Chemistry Kinetics-Physical

• What must happen for a reaction to occur?

  Particles must collide
• How is the rate of reaction defined?

  Change in concentration per unit time
• What is the formula for rate of reaction?

  Rate = amount of reactant used / time
• Why do most collisions not lead to a reaction?

  Particles often bounce off each other
• What is required for a reaction to occur after a collision?

  Correct orientation and sufficient energy
• What is activation energy?

  Minimum energy required for a reaction
• How is activation energy represented in an energy profile diagram?

  As the difference between reactants and peak energy
• What happens to bonds during a reaction?

  Bonds stretch and break as energy increases
• What does the Maxwell-Boltzmann distribution illustrate?

  Energy distribution of gas particles
• What does the area under the Maxwell-Boltzmann curve represent?

  Total number of molecules
• How does the mean energy of particles compare to the most likely energy?

  Mean energy is slightly to the right
• What does the activation energy line indicate on the Maxwell-Boltzmann plot?

  Energy required for particles to react
• How does temperature affect the rate of reaction?

  Higher temperature increases kinetic energy
• What happens to the area beyond activation energy when temperature increases?

  It increases due to more energetic particles
• What occurs when temperature decreases in a reaction?

  Fewer particles exceed activation energy
• Why do reactions occur faster at higher temperatures?

  More frequent and energetic collisions happen
• How does concentration affect the rate of reaction?

  Higher concentration increases collision frequency
• What is the role of a catalyst in a reaction?

  It lowers activation energy and speeds up reactions
• What is zeolite?

  A catalyst with a honeycomb structure
• How does a catalyst affect the Maxwell-Boltzmann distribution?

  It shifts activation energy to the left
• What is measured when a precipitate forms in an experiment?

  Time taken for the precipitate to form
• What is a common method to measure gas production?

  Using a gas syringe
• What is a potential issue with measuring precipitate formation?

  Difficulty in determining when it disappears
• What must be used when measuring toxic gas production?

  A fume cupboard for safety
• What is the significance of the area under both Maxwell-Boltzmann curves?

  It remains the same regardless of temperature
• What happens to the activation energy with a catalyst?

  It decreases, allowing reactions to occur easier
• How can the rate of reaction be affected by pressure?

  Higher pressure increases collision frequency
• What is the relationship between temperature and reaction rate?

  Higher temperature leads to faster reactions
• What are the key factors affecting the rate of reaction?

  • Temperature
  • Concentration
  • Pressure
  • Catalysts
• What are the methods to measure the rate of reaction?

  1. Timing precipitate formation
  2. Measuring mass loss
  3. Measuring gas volume produced
• What is the significance of activation energy in reactions?

  • Minimum energy required for a reaction
  • Determines the rate of reaction
  • Affects the choice of catalysts
• How does a catalyst function in a chemical reaction?

  • Provides an alternative pathway
  • Lowers activation energy
  • Remains unchanged after the reaction
• What is the Maxwell-Boltzmann distribution used for?

  • Illustrates energy distribution of particles
  • Shows the effect of temperature on energy
  • Helps understand reaction rates