The collision theory states that chemical reactions occur when reactant molecules collide with sufficient kinetic energy to reach the transition state. The reaction rate is affected by factors like temperature, surface area, concentration of reactants, and catalysts - an increase in temperature or concentration raises the kinetic energy and number of collisions of reactants, speeding the reaction rate, while more surface area or a catalyst provide more opportunities for collisions without being consumed in the reaction.

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.