Kinetics

• What is required for a chemical reaction to occur?

  Particles must collide with sufficient energy
• What is activation energy in a chemical reaction?

  Minimum energy needed for a reaction
• How does particle orientation affect chemical reactions?

  Correct orientation is necessary for successful collisions
• What are the reaction conditions that can be altered to increase reaction rates?

  • Temperature
  • Concentration
  • Pressure
• How do reaction conditions impact particle collisions?

  They can provide particles with more energy
• What is the Maxwell-Boltzmann distribution?

  Energy distribution pattern of molecules
• What happens to the Maxwell-Boltzmann distribution when reaction conditions change?

  Its shape alters, affecting energy distribution

  
• What does the area under the Maxwell-Boltzmann curve represent?

  Total number of molecules in the sample

  
• What occurs when a substance is heated?

  Thermal energy converts to kinetic energy
• How does increased molecular movement affect reaction rates?

  More collisions occur with greater energy

  
• What is the effect of increasing temperature on reaction rates?

  It increases the rate of reaction
• How does the Maxwell-Boltzmann distribution shift with increased temperature?

  It shifts to the right
• What happens when the concentration of a sample is increased?

  More molecules are packed closer together
• How does increased concentration affect collision likelihood?

  It makes collisions more likely
• What is the effect of increasing pressure on molecules?

  Molecules are packed closer together
• How does increasing pressure affect the Maxwell-Boltzmann distribution?

  It shifts to the right
• What is a catalyst?

  A substance that increases reaction rate
• How does a catalyst affect activation energy?

  It provides an alternative path with lower energy
• What happens to the Maxwell-Boltzmann distribution curve when a catalyst is used?

  Its shape remains unchanged, but activation energy shifts

  
• How does the position of activation energy change with a catalyst?

  It shifts to the left
• What are the effects of temperature, concentration, pressure, and catalysts on reaction rates?

  • Temperature: Increases kinetic energy and collision frequency
  • Concentration: Increases likelihood of collisions
  • Pressure: Packs molecules closer, increasing collisions
  • Catalysts: Lower activation energy, increase reaction rate