What must happen in order for a reaction to occur?
Reactant peroxides must collide with sufficient energy.
What is it called when reactant particles exceed the activation energy as collisions
Successful collision
What happens if there are more frequent collisions
The more likely successfully collisions occur in a given time
Factors that increase collision frequency
Increase in concentration of reactants (for solution)
Increase in pressure (for gaseous reactants)
Increase in surface area (for solids)
Increase in temperature
How does a catalyst increase rate of reaction
By providing an alternative reaction pathway with a lower activation energy
So a greater proportion of reactant particles exceed the Ea in a given time
When drawing boltzman distribution curves why should the line always touch the origin
There are no particles with zero energy
What does the total area under the curve =
Total number of particles (fixed)
What does the area under the curve and above the activation energy =
Total number of particles that exceed
Why should the line never touch the x axis after the origin
There are always some particles with very high energy
