1. Unit 1 Kinetics and Equilibrium U1 S1 L1 Collision Theory
Unit 1
Kinetics and Equilibrium
U1 S1 L1
Collision Theory

2. Upon completion of this lesson, you will be able to:
state the Kinetic Molecular Theory.
describe two pieces of evidence that support the Kinetic Molecular Theory;
pressure
diffusion.
state the Collision Theory.
relate the rate of reaction to the number of successful collisions between reacting particles.
list ways of quantifying reaction rates such as the measurement of changes in  mass, colour, volume, pH, and other macroproperties.  

3. Kinetic Molecular Theory
All matter is composed of either atoms, ions, or molecules.
This is the basic premise of chemistry – you must believe this!
These particles are in a state of constant, random motion.
The particles are always moving, and because of this, they are always colliding with other particles of matter. The energy associated with each collision is conserved.
Ie: pressure inside a balloon
An increase in energy of the particles causes an increase in the motion of the particles.
as the particles move faster they require more space
Ie: expansion of solids and liquids, increased pressure of liquids

4. Collision Theory
In order for a chemical reaction to occur the collision theory states:
reacting particles must collide with one another in order for a reaction to occur.
the particles must collide with proper orientation and
The particles must collide with sufficient intensity (energy) to allow for old bonds to break and/or new bonds to form.
All three conditions must be met, at the same time, in order for a reaction to occur!

5. Rates of Chemical reactions
The rate of a chemical reaction is the rate at which reactants are consumed (or products produced) for a given unit of time.
In terms of the collision theory, reaction rate is a measure of the number of successful collisions over time.
In order to measure reaction rate we measure observable properties of the reaction:
Change in mass of solids over time.
Change in pH over time.
Change in electrical conductivity over time.
Change in gas Pressure over time.
Change in color (colorimeter) over time.
Change in gas volume over time.

6. Fe(s) + 2 HCl(aq) → H2 (g) + FeCl2 (aq)

7. You have a brand new bottle of dill pickles
You have a brand new bottle of dill pickles. Your mouth is watering at the thought of crunching into one. The only problem is that the lid is stuck! How do you safely remove the lid?
Hit the lid with a sharp knife.
Run hot water over the lid.
Run ice cold water over the lid.
Smash the bottle, pick the pickles up off the floor.

8. 2. How do the motion of molecules in a glass of water at 15°C compare with another glass of water 80°C?
The molecules are moving faster at 15 C than at 80 C
The molecules are moving slower 15 C than at 80 C
The molecules are moving at the same speed at both temperatures
Temperature has no effect on the speed of molecules.

9. Posting:
Use the collision theory to explain why a container of gasoline does not ignite when left out in the open on a hot summer day.
Textbook Readings
page 462: Reaction Rates of Chemicals
page 463: Expressing Reaction Rates
page 466: Methods for Measuring Reaction Rates
page : Theories of Reaction Rates
page 472: Reactions and orientation of Reactants
Textbook Practice Items
page 486: item 7
page 538: item 4