kinetics

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

  Collisions must have energy greater than or equal to the activation energy and correct particle orientation.
• How do reaction conditions impact the likelihood of a collision occurring?

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

  • A pattern that describes how the energies of molecules in a substance are distributed.
  • Not all molecules have the same amount of energy.

  
• 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?

  The total number of molecules in the sample.
• What occurs to the kinetic energy of molecules when a substance is heated?

  Thermal energy is converted to kinetic energy, causing molecules to move faster and further.

  
• How does increased molecular movement affect the rate of reaction?

  It leads to more frequent collisions with greater energy, increasing the rate of reaction.

  
• What happens to the Maxwell-Boltzmann distribution at increased temperature?

  It shifts to the right, resulting in a greater proportion of molecules having energy greater than or equal to the activation energy.

  
• What effect does increasing the concentration of a sample have on molecular collisions?

  It makes collisions more likely as molecules are packed closer together.
• How does increasing pressure affect molecular collisions?

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

  It shifts the distribution to the right.

  
• What is a catalyst?

  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.

  
• Total area under the Maxwell-Boltzmann curve


  The total number of particles in the sample.