1. Factors Affecting the Rate of a Chemical Reaction
1. temperature
2. concentration
3. pressure (gases)
4. surface area
5. orientation (molecules must collide in a specific manner to form a chemical bond)
6. nature of the reactants (polar, non-polar, electronegativity, heterogeneous, homogeneous)
7. catalyst

2. The following events must occur before a reaction can proceed:
The reactant particles must collide with each other.
The collisions must be of enough energy to overcome the ‘energy barrier’, called the activation energy (more about this on the next slide).
The reactants must form new bonds to produce products.

3. Activation Energy Defined as:
The minimum energy required to bring about a chemical reaction.
If there were no such thing as ‘activation energy’ life would be very difficult:
Gasoline for your car would ignite as soon as it came into contact with air.
You would burst into flames.
Activation energy is why these things do not happen, there is an energy barrier so most reactions need to be ‘started off’ by putting in some energy.

4. Activation Energy 2 Activation energy for a reaction is
shown on reaction profile diagrams
Reactants
Products
Activated intermediate
Activation energy H
energy

5. 1. Temperature Higher temperature = faster reaction
According to kinetic theory (do you remember this?) as the temperature increases the particles in a substance move about more quickly.
Reaction at 300C
Reaction at 500C
As the temperature increases the number of collisions increases as well as the energy of the collisions. So temperature has a big effect on the rate of reaction. For every 100C increase the rate approximately doubles.
Higher temperature = faster reaction

6. 2. Concentration Zn + 2HCl  H2 + ZnCl2
Consider the reaction between zinc and hydrochloric acid:
Zn + 2HCl  H2 + ZnCl2
Acid Particles
Zinc
1M hydrochloric acid
2M hydrochloric acid
There are more particles of acid per unit volume in the 2M acid than there are in the 1M acid. So, there will more collisions between the acid and zinc particles in the stronger acid, giving a faster reaction.
Higher concentration = faster reaction

7. 3. Pressure:Gas Reactions
The rate of reaction between gases is increased by increased pressure.
In effect pressure is the gas equivalent of concentration.
Low pressure, particles far apart.
These two gas jars contain the same number of gas particles.
The higher pressure jar has more particles per unit volume which means a higher concentration, hence faster reaction.
Higher pressure, particles closer together.
Higher pressure = faster reaction

8. 4. Surface Area
When solids take part in chemical reactions only the surface particles are exposed so they are the only ones that can collide with particles of other reactants.
‘Inner’ particles are protected and cannot collide with other particles until they become ‘exposed’.
The surface particles are ‘exposed’ and can react.

9. 4. More on Surface Area Larger surface area = faster reaction.
If we break up this ‘lump’ into smaller pieces the number of particles has not changed but the there are now more ‘surface’ particles.
There is now a greater surface area with more exposed particles so more collisions can occur, hence faster reaction.
Larger surface area = faster reaction.

10. 3. Orientation and Efficiency of Molecular Collisions
A2 + B2 → 2AB

11. 7. Effect of a Catalyst .
A catalyst is a substance that increases the speed of a reaction, without being used up. A catalyst can be recovered at the end of a reaction and used again.
An enzyme is a catalyst
A catalyst reduces the activation energy of a reaction .

12. 7. Effect of a Catalyst 2 Catalyst = faster reaction.
Activation energy without catalyst.
The lower activation energy in the presence of a catalyst means the reaction will be faster. More of the collisions have enough energy to react. There is a lower ‘energy barrier’.
energy
Activation energy with catalyst.
Catalyst = faster reaction.

13. Changing the Rate of a Chemical Reaction
To change the rate of a reaction one or more of the following things must happen:
Increase the number of collisions between the reactant particles
Increase the energy of the collisions.
Decrease the activation energy.
Increase the speed of the rate determining step
This is all very well but how can we follow the progress of a chemical reaction?

14. Following a Chemical Reaction
To find the rate of a chemical reaction we must be able to follow its progress with time.
We have two choices:
Record the increase in product concentration as the reaction progresses.
Record the decrease in reactant concentration as the reaction progresses.

15. Following a Chemical Reaction 2
As an example consider the reaction between calcium carbonate and hydrochloric acid.
CaCO3 + 2HCl  CaCl2 + H2O + CO2
We can follow this reaction by measuring the volume of carbon dioxide produced as the reaction proceeds.
Gas being collected
Measure the amount of CO2 collected
Dilute acid
Marble chips

16. Following a Chemical Reaction 3
If you collect data for the total amount of gas produced as the reaction progresses then plot this data on a graph you should get a curve similar to that shown below.
Volume of gas/cm3
Time/sec.
Reaction fastest at the beginning.
Slowing down.
Reaction finished.
All very well, but what does the graph tell you?
The gradient or slope of the graph shows the rate of the reaction.
Steeper slope = faster reaction.

17. More About Rate Graphs Why is the reaction fastest at the beginning?
Volume of gas/cm3
Time/sec.
Reaction fastest at the beginning.
Slowing down.
Reaction finished.
Why is the reaction fastest at the beginning?
Why does the reaction slow down?
Why does the reaction eventually stop?
This is where the concentration of the reactants is highest, therefore fastest reaction.
As the reactants are used their concentration decreases so the rate of reaction decreases.
One of the reactants is used up, so there can be no further reaction.

18. Summary
Increasing the surface area gives a faster reaction because more particles are ‘exposed’ to the other reactant.
Increasing the concentration increases the rate of reaction because there are more collisions between the reactant particles.
Increasing the temperature increases the rate of reaction because the particles move faster and collide more often with greater energy.
If the reactants are both of the same nature, ex. All gases, the reaction will proceed at a faster rate. (homogeneous)
A catalyst increases the rate of a reaction because it reduces the activation energy so more of the collisions have enough energy to react.

19. Result of effective collisions