kinetics

• What is required for a chemical reaction to occur according to collision theory?


  Particles must collide with energy greater than or equal to the activation energy and correct orientation.
• How do reaction conditions affect the likelihood of a collision occurring?


  They can be altered to provide particles with more energy, increasing the likelihood of effective collisions.
• What is the Maxwell-Boltzmann distribution?


  • It describes the distribution of energies among molecules in a substance.
  • Not all molecules have the same energy.
  • The shape of the curve changes with reaction conditions.
• What happens to the Maxwell-Boltzmann distribution when reaction conditions are changed?


  The shape of the curve alters, affecting the number of particles with energy greater than the activation energy.
• What does the total area under the Maxwell-Boltzmann curve represent?


  It represents the total number of molecules in the sample.
• What effect does heating a substance have on its molecules?


  It increases their kinetic energy, causing them to move faster and further.
• How does increased temperature affect the rate of reaction?


  It increases the rate of reaction by causing more frequent and energetic collisions.
• What happens to the Maxwell-Boltzmann distribution at increased temperatures?


  It shifts to the right, increasing the proportion of molecules with energy greater than or equal to the activation energy.
• What occurs when the concentration of a sample is increased?


  More molecules are present in the same volume, making collisions more likely.
• How does increasing pressure affect molecular collisions?


  It packs molecules closer together, increasing the likelihood of collisions.
• What is the effect of increased concentration or pressure on the Maxwell-Boltzmann distribution?


  It shifts to the right, indicating more molecules have energy greater than the activation energy.
• What is a catalyst?


  A catalyst is a substance that increases the rate of reaction without being used up.
• How does a catalyst affect the activation energy of a reaction?


  It provides an alternative reaction path that requires lower activation energy.
• What happens to the Maxwell-Boltzmann distribution curve when a catalyst is used?


  The shape remains unchanged, but the position of the activation energy shifts to the left.
• What is the significance of the position of the activation energy in the Maxwell-Boltzmann distribution?


  A leftward shift means a greater proportion of molecules have sufficient energy to react.
• What are the effects of temperature, concentration, pressure, and catalysts on reaction rates?


  • **Temperature**: Increases kinetic energy, leading to more frequent and energetic collisions.
  • Concentration: More molecules in the same volume increase collision likelihood.
  • Pressure: Similar to concentration, it packs molecules closer together.
  • **Catalysts**: Lower activation energy and provide alternative reaction paths.