The document discusses collision theory and factors that affect chemical reaction rates, stating that reaction rates increase with higher temperatures, larger surface areas, higher concentrations of reactants, and the presence of catalysts as these factors all lead to more frequent collisions between reactant molecules that have sufficient kinetic energy to reach the transition state.

2. The collision theory states
that gas-phase chemical
reaction occurs when
molecules colliding have
sufficient kinetic energy.

3. What is activation energy?
Activation energy is
the energy required to
proceed and reach the
transition state.

4. Reaction rate
Reaction rate is
intuitively defines as
how quickly or slowly a
reaction takes place.

5. Factors affecting reaction
rate
Temperature
Surface area
Concentration of
reactants
Catalyst

6. Temperature
If the temperature is increased:
* the reactant particles move more
quickly
* the reactant particles have more
kinetic energy
* the reaction rate increases

8. Surface area
Larger surface area
would have a larger
space of collision
between particles of a
reaction.

10. Concentration of reactants
If the concentration is increased:
* the reactant particles become more
crowded
* there is a greater chance of the
particles colliding;
* the rate of reaction increases

12. Catalyst
Catalyst is a
substance that
makes a chemical
reaction faster.