Collision Theory and Reaction Rates

Introduction

• Experiment: Comparison of sugar dissolution in hot vs. cold water.
• Observation: Sugar dissolves faster in hot water than in cold water.

Collision Theory

• Developed by: Max Trotz and William Lewis in the early 1900s.
• Purpose: Explain different rates of chemical reactions.

Key Assumptions of Collision Theory

1. Particle Collisions

   • Particles must collide to react.
   • Collisions likened to billiard balls in a pool game.

2. Activation Energy

   • Not all collisions lead to a reaction.
   • Particles must have enough energy (speed) to break and form new bonds.
   • Activation Energy: Minimum energy required for a reaction.
   • Reactions vary in the amount of activation energy required.

3. Temperature and Kinetic Energy

   • Increase in temperature raises the average kinetic energy of particles.
   • Higher kinetic energy increases the likelihood of having enough activation energy.

4. Orientation of Particles

   • Correct orientation is necessary for reactions, even if speed and energy are sufficient.
   • Example: Reaction between nitrogen monoxide and ozone depends on correct molecular alignment.

Conclusion

• Summary of Collision Theory:
  • Particles must collide.
  • Sufficient energy is needed.
  • Correct orientation is essential.

Conclusion

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