Kinetics Lesson 3 Collision Theory

The Collision Theory   Link to Simulation of Molecular Motion 1. Matter consists of moving particles. 2. As the temperature increases the particles move faster and collide more often and with more energy. 3. In chemical reactions bonds must be broken and new ones formed. 4. The energy for this comes from particle collisions. 5. The collisions have a variety of energy, as some are harder than others. 6. A collision energy diagram is a graph of the number of the collisions versus the energy of each collision.

Collision Energy Diagram Simulation 100 % Percent of Collisions With Energy 0 % Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- to break the bonds! Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! This area represents the fraction of collisions that do not have the Ea- not successful. Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! This area represents the fraction of collisions with the Ea -successful. Low Collision energy High

What happens to the number of successful collisions if we add a catalyst, which lowers the activation energy Ea? Watch!

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! This area represents the fraction of collisions with the Ea -successful. Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! Lowering the Ea increases successful collisions! Low Collision energy High

What happens to the number of successful collisions if we increase the temperature- so that the average collision energy is greater? Watch!

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! Low Collision energy High

Collision Energy Diagram 100 % Percent of Collisions With Energy 0 % Activation Energy Ea- minimum energy required for a successful collision- too break the bonds! Push the graph down and right! Increasing the temperature increases successful collisions- increases rate! Low Collision energy High

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires:

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires:

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products no products

Collision Theory   You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 1. Favourable Geometry versus Poor Geometry products no products

Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2. Sufficient Energy to break the chemical bonds  

Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2. Sufficient Energy to break the chemical bonds  

Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2. Sufficient Energy to break the chemical bonds  

Collision Theory You need a collision to have a reaction. Collisions provide the energy required to break bonds. Most collisions are not successful A successful collision requires: 2. Sufficient Energy to break the chemical bonds   Activation energy is the minimum amount of energy required for a successful collision.

The Collision Theory can be used to explain how the rate of a reaction can be changed. Reaction rates can increase due to 1. More collisions 2. Harder collisions- greater collision energy 3. Lower activation energy or Ea, which allows low energy collisions to be more effective. And that’s it!

The Collision Theory can be used to explain how the rate of a reaction can be changed. 1. Increasing the temperature increases the rate because there are:  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 1. Increasing the temperature increases the rate because there are:   More frequent collisions

The Collision Theory can be used to explain how the rate of a reaction can be changed. 1. Increasing the temperature increases the rate because there are:   More frequent collisions Harder collisions

The Collision Theory can be used to explain how the rate of a reaction can be changed. 2. Increasing the reactant concentration increases the rate because there are:  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 2. Increasing the reactant concentration increases the rate because there are:   More frequent collisions

The Collision Theory can be used to explain how the rate of a reaction can be changed. 3. Adding a catalyst increases the rate because:  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 3. Adding a catalyst increases the rate because   Lower activation energy or Ea, which allows low energy collisions to be successful Movie- The catalyst KI is added to H2O2, food colouring, and dishwashing detergent. The O2 produced makes foam.  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 4. Changing the nature of the reactant for a more reactive chemical changes the rate because  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 4. Changing the nature of the reactant for a more reactive chemical changes the rate because   Lower activation energy or Ea, which allows low energy collisions to be more effective

The Collision Theory can be used to explain how the rate of a reaction can be changed. 5. Increasing the surface area of a solid reactant increases the rate because:  

The Collision Theory can be used to explain how the rate of a reaction can be changed. 5. Increasing the surface area of a solid reactant increases the rate because:   More frequent collisions

Explain each Scenario Using the Collision Theory   1. A balloon full of H2 and O2 do not react at room temperature. A small spark ignites causes an explosion.

Explain each Scenario Using the Collision Theory   1. A balloon full of H2 and O2 do not react at room temperature. Ea is too high for the room temperature collisions A small spark ignites causes an explosion.

Explain each Scenario Using the Collision Theory   1. A balloon full of H2 and O2 do not react at room temperature. Ea is too high for the room temperature collisions A small spark ignites causes an explosion. The spark provides the Ea and it explodes because it is exothermic

Explain each Scenario Using the Collision Theory   2. A candle does not burn at room temperature A match causes the candle to burn. The candle continues to burn

Explain each Scenario Using the Collision Theory   2. A candle does not burn at room temperature   Ea is too high for the room temperature collisions A match causes the candle to burn. The candle continues to burn

Explain each Scenario Using the Collision Theory   2. A candle does not burn at room temperature   Ea is too high for the room temperature collisions A match causes the candle to burn.   The match provides the Ea The candle continues to burn

Explain each Scenario Using the Collision Theory   2. A candle does not burn at room temperature   Ea is too high for the room temperature collisions A match causes the candle to burn.   The match provides the Ea The candle continues to burn It burns because it is exothermic

Explain each Scenario Using the Collision Theory   3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically.

Explain each Scenario Using the Collision Theory   3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically.

Explain each Scenario Using the Collision Theory   3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically. KI is a catalyst as it is not a reactant and it speeds up the rate.

Explain each Scenario Using the Collision Theory   3. H2O2 decomposes very slowly at room temperature. 2H2O2(aq) → O2(g) + 2H2O(l) KI increases the reaction rate dramatically. KI is a catalyst as it is not a reactant and it speeds up the rate. Lowers the activation energy or Ea, which allows low energy collisions to be more effective

Describe and Graph the Relationship between the Following    Ea and the rate Rate Ea

Describe and Graph the Relationship between the Following    Ea and the rate Decreasing the Ea increases the rate- inverse. Rate Ea

Describe and Graph the Relationship between the Following    Ea and the rate Decreasing the Ea increases the rate- inverse. Ea Rate

Describe and Graph the Relationship between the Following   Temperature and the rate Rate Temp

Describe and Graph the Relationship between the Following   Temperature and the rate Increasing the temperature increases the rate- direct. Rate Temp

Describe and Graph the Relationship between the Following   Temperature and the rate Increasing the temperature increases the rate- direct. Rate Temp

Describe and Graph the Relationship between the Following   Concentration and the rate Rate Conc

Describe and Graph the Relationship between the Following   Concentration and the rate Increasing the concentration increases the rate- direct. Rate Conc

Describe and Graph the Relationship between the Following   Concentration and the rate Increasing the concentration increases the rate- direct. Rate Conc

Describe and Graph the Relationship between the Following   Ea and the temperature Temp Ea

Describe and Graph the Relationship between the Following   Ea and the temperature The only way to change the Ea is by adding a catalyst! No relationship! Temp Ea

Describe and Graph the Relationship between the Following   Ea and the temperature The only way to change the Ea is by adding a catalyst! No relationship! Temp Ea