the maxwell-boltzmann distribution curve

• What do gas molecules have that causes them to move at different speeds?

  Varying kinetic energies
• What does the Maxwell-Boltzmann distribution curve represent?

  Variation of molecular kinetic energies in gases
• What happens to some gas molecules due to low kinetic energy?

  They move slowly
• What is true about molecules with high kinetic energy?

  They move very fast
• What describes the majority of gas molecules in terms of kinetic energy?

  They have moderate kinetic energies and speeds
• What is the significance of kinetic energy being greater than or equal to activation energy?

  It allows molecules to react upon collision
• What are the key features of the Maxwell-Boltzmann distribution curve?

  • Originates at the origin (no zero kinetic energy)
  • Peaks at the most common kinetic energy level
  • Total area equals total number of molecules
  • Peak shows most probable kinetic energy
  • Average kinetic energy is higher than peak energy
• What happens to the Maxwell-Boltzmann distribution curve when temperature increases?

  The curve shifts to the right
• What effect does increasing temperature have on the number of molecules surpassing activation energy?

  More molecules attain necessary kinetic energy
• What remains constant despite the shift in the distribution curve due to temperature increase?

  Total number of molecules
• What happens to the peak height of the Maxwell-Boltzmann distribution curve at higher temperatures?

  It decreases
• What does the broadening of the kinetic energy distribution at higher temperatures indicate?

  Increased frequency of collisions
• How does a modest rise in temperature affect the rate of reaction?

  It significantly increases the rate of reaction
• What is the relationship between temperature and effective collisions in gas reactions?

  • Higher temperature increases frequency of collisions
  • More molecules exceed activation energy
  • Leads to a higher proportion of effective collisions