Module 3, Chapter 2: Physical Chemistry (REACTION AND EQUILIBRIUM)

STUDY
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Collision Theory
- collide in the right direction (facing the right way)

- collide with a certain minimum amount of kinetic energy
Activation Energy
the minimum amount of kinetic energy particles need to react
Why do particle need Ea?
the particles need this much energy to break the bonds to start the reaction
Increasing Temperature of Rate of Reaction
- particles have more kinetic energy

- particles will move faster

- greater proportion of molecules will have at least the activation energy and be able to react
Increasing Temperature on Botzmann Distribution
- pushes Boltzmann Distribution Curve to the right

- the total number of molecules is still the same, which means the area under each curve must be the same
How does Concentration Affect Rate
- closer together

- collide more frequently

- more chances to react

- more successful collisions
How does increasing Pressure Speeds up Reactions?
- closer together

- collide more frequently

- more chances to react

- more successful collisions
How do Catalysts Increase Rate of Reaction?
- lower activation energy

- different reaction pathway

- particles will have enough energy
Catalysts at the end of the reaction
catalyst
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