Kinetics

    Cards (6)

    • Collision Theory:
      • Chemical reactions occur when particles of substances collide
      • Collisions must have energy greater than or equal to the activation energy of the reaction
      • Particle orientation must be correct for a successful reaction
    • Reaction Conditions:
      • Impact the collisions of particles
      • Conditions can be altered to provide particles with more energy
      • Changing conditions can increase the likelihood of a collision occurring with sufficient energy to react and increase the rate of reaction
    • Maxwell-Boltzmann Distribution:
      • Not all molecules in a substance have the same amount of energy
      • Energies are distributed in a pattern called the Maxwell-Boltzmann distribution
      • Changing reaction conditions alters the shape of the curve, affecting the number of particles with energy greater than the activation energy
      • The total area under the curve represents the total number of molecules in the sample, which must remain constant
    • Effect of Temperature:
      • Heating a substance transfers thermal energy, converted to kinetic energy
      • Molecules move faster and further with increased temperature
      • Increased movement leads to more frequent collisions with greater energy
      • Increasing temperature increases the rate of reaction as more collisions of greater energy occur
    • Effect of Concentration and Pressure:
      • Increasing concentration leads to molecules being packed closer together, increasing the likelihood of collisions with greater energy
      • Increasing pressure has a similar effect by packing molecules closer together in a smaller volume
      • Both concentration and pressure increase the rate of reaction
    • Effect of Catalysts:
      • Catalysts increase the rate of reaction without being used up
      • Provide an alternative reaction path with a lower activation energy
      • The Maxwell-Boltzmann distribution curve remains unchanged in shape, but the position of the activation energy is shifted to the left, allowing a greater proportion of molecules to have sufficient energy to react
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