Chapter 17 - Reaction Kineticsexternal image puzzle1.gif
  • How chemical reactions occur
  • Needs to be an effective collision, to have an effective collision two molecules must have:
    • Proper orientation - The two molecules must be faced the correct way which would allow for an effective collision such as the puzzle pieces pictured above.
    • Adequate kinetic energy - The two molecules must have enough kinetic energy therefore allowing the collision to occur.
  • How can you maximize the chances of getting an effective collision?
    • Adding a catalyst will decrease the activation energy (Ea) because the catalyst puts the molecules in the correct position faster which saves energy.
      • ex: Enzymes ------> "ase"
        • Enzymes are located in the human body and they are catalysts. One may identify an enzyme by finding the letters "ase" at the end of the name. (Sucrase, Lactase, and Glucase)
    • Increasing temperature causes the molecules to move faster which produces an effective collision quicker because it increases the chances of an effective collision.
    • Increasing concentration of x ( [x] ) increases the chances of an effective collision because the molecules are in a more compact area with less room to move.
ALL ABOVE POINTS AFFECT THE REACTION RATE which increases the surface area during the reaction.

What are two things that molecules need to have before an effective collision?What three things can you do to a system to increase the chances of an effective collision?
What is the enzyme for lactose?
What reaction would occur the fastest, 6 mol of gaseous HCl, 3 mol of gaseous HCL, 8 mol of gaseous HCl, or 4 mol of gaseous HCl, if they are all in the same size container?

Proper orientation, adequate kinetic energy

Add a catalyst, increase temperature, and increase the concentration of x


8 mol of H2O
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